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{{Chembox
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|ImageFile = Bariumsulfatpulver.png
|ImageFile1 = Barium-sulfate-2D.png
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|ImageName1 = Chemical structure of barium sulfate
|ImageFileL2 = Barite-unit-cell-3D-vdW.png
|ImageNameL2 = 3D model of barium sulfate
|Section1={{Chembox Identifiers
|UNII_Ref = {{fdacite|correct|FDA}}
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|InChIKey = TZCXTZWJZNENPQ-NUQVWONBAD
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|SMILES = [Ba+2].[O-]S([O-])(=O)=O
|InChI = 1/Ba.H2O4S/c;1-5(2,3)4/h;(H2,1,2,3,4)/q+2;/p-2
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|Section2={{Chembox Properties
|Formula = BaSO<sub>4</sub>
|MolarMass = 233.39 g/mol
|Appearance = white crystalline
|Odor = odorless
|Density = 4.49 g/cm<sup>3</sup>
|MeltingPtC = 1580
|BoilingPtC = 1600
|BoilingPt_notes = (decomposes)
|Solubility = 0.2448 mg/100 mL (20 °C) <br> 0.285 mg/100 mL (30 °C)
|SolubilityProduct = 1.0842 × 10<sup>−10</sup> (25 °C)
|SolubleOther = insoluble in [[ethanol|alcohol]],<ref>{{cite book |title=CRC Handbook of Chemistry and Physics |publisher=CRC Press |year=2004 |edition=85th |pages=[https://archive.org/details/crchandbookofche81lide/page/4 4–45] |isbn=0-8493-0485-7 |url=https://archive.org/details/crchandbookofche81lide/page/4 |url-access=registration}}</ref> soluble in concentrated, hot [[sulfuric acid]]
|RefractIndex = 1.636 (alpha)
|MagSus = −71.3·10<sup>−6</sup> cm<sup>3</sup>/mol
}}
|Section3={{Chembox Structure
|CrystalStruct = orthorhombic
}}
|Section4={{Chembox Thermochemistry
|DeltaHf = −1465 kJ/mol<ref name="Zumdahl, Steven S. 2009">{{cite book |author=Zumdahl, Steven S. |title=Chemical Principles |edition=6th |publisher=Houghton Mifflin Company |year=2009 |isbn=978-0-618-94690-7}}</ref>
|Entropy = 132 J/(mol·K)<ref name="Zumdahl, Steven S. 2009"/>
|HeatCapacity = 101.7 J/(mol K)
}}
|Section5={{Chembox Pharmacology
|ATCCode_prefix = V08
|ATCCode_suffix = BA01
|AdminRoutes = by mouth, rectal
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|Excretion = rectal
|Legal_US = Rx only
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'''Barium sulfate''' (or '''sulphate''') is the [[inorganic compound]] with the chemical formula [[barium|Ba]][[sulfate|SO<sub>4</sub>]]. It is a white crystalline solid that is odorless and [[solubility|insoluble]] in [[water]]. It occurs in nature as the mineral [[barite]], which is the main commercial source of [[barium]] and materials prepared from it. Its opaque white appearance and its high density are exploited in its main applications.<ref name=Holleman>Holleman, A. F. and Wiberg, E. (2001) ''Inorganic Chemistry'', San Diego, CA. Academic Press, {{ISBN|0-12-352651-5}}.</ref>
==Uses==
===Drilling fluids===
About 80% of the world's barium sulfate production, mostly purified mineral, is consumed as a component of [[oil well]] [[drilling fluid]]. It increases the density of the fluid,<ref name="Ullmann">{{cite book |chapter=Barium and Barium Compounds |title=Ullmann's Encyclopedia of Industrial Chemistry |year=2007 |last1=Kresse |first1=Robert |last2=Baudis |first2=Ulrich |last3=Jäger |first3=Paul |last4=Riechers |first4=H. Hermann |last5=Wagner |first5=Heinz |last6=Winkler |first6=Jochen |last7=Wolf |first7=Hans Uwe |isbn=978-3-527-30673-2 |doi=10.1002/14356007.a03_325.pub2}}</ref> increasing the hydrostatic pressure in the well and reducing the chance of a [[blowout (well drilling)|blowout]].
===Radiocontrast agent===
{{Main|Barium sulfate suspension}}
[[Barium sulfate suspension|Barium sulfate in suspension]] is often used medically as a [[radiocontrast]] agent for [[X-ray]] [[medical imaging|imaging]] and other diagnostic procedures. It is most often used in imaging of the [[gastrointestinal tract|GI tract]] during what is colloquially known as a "[[barium meal]]". It is administered orally, or by [[enema]], as a [[barium sulfate suspension|suspension]] of fine particles in a thick milk-like solution (often with sweetening and flavoring agents added). Although barium is a [[heavy metals|heavy metal]], and its water-soluble compounds are often highly toxic, the low solubility of barium sulfate protects the patient from absorbing harmful amounts of the metal. Barium sulfate is also readily removed from the body, unlike [[Thorotrast]], which it replaced. Due to the relatively high [[atomic number]] (''Z'' = 56) of barium, its compounds absorb X-rays more strongly than compounds derived from lighter nuclei.
===Pigment===
The majority of synthetic barium sulfate is used as a component of white pigment for paints. In oil paint, barium sulfate is almost transparent{{citation needed|date=December 2020}}, and is used as a filler or to modify consistency. One major manufacturer of artists' oil paint sells "permanent white" that contains a mixture of titanium white pigment ([[titanium dioxide|TiO<sub>2</sub>]]) and barium sulfate. The combination of barium sulfate and [[zinc sulfide]] (ZnS) is the inorganic pigment called [[lithopone]]. In photography it is used as a coating for certain photographic papers.<ref name=Ullmann/>
It is also used as a coating to diffuse light evenly.
===Light-reflecting paint for cooling===
Barium sulfate is highly reflective, of both visible and ultraviolet light.<ref name=":0">{{cite web |last=Puiu |first=Tibi |date=2022-10-04 |title=World's whitest paint is now thin enough to coat and cool down cars, trains and planes |website=ZME Science |language=en-US |url=https://www.zmescience.com/science/news-science/worlds-whitest-paint-usable-04102022/ |access-date=2022-10-12}}</ref> Researchers used it as an ingredient in paint that reflects 98.1% of [[solar radiation]], allowing surfaces to which it has been applied to stay cooler in sunlit conditions. Commercially available white paints only reflect 80 - 90% of solar radiation.<ref name="PurduePaint">{{cite web |last=Wiles |first=Kayla |date=September 16, 2021 |title=Purdue record for the whitest paint appears in latest edition of 'Guinness World Records' |website=purdue.edu |language=en |url=https://www.purdue.edu/newsroom/releases/2021/Q3/purdue-record-for-the-whitest-paint-appears-in-latest-edition-of-guinness-world-records.html |access-date=2022-10-12}}</ref> By using hexagonal nanoplatelet [[boron nitride]], the thickness of a coat of this type of paint was reduced to 0.15 mm.<ref name=":0"/>
===Paper brightener===
A thin layer of barium sulfate called baryta is first coated on the base surface of most [[photographic paper]] to increase the [[reflectiveness]] of the image, with the first such paper introduced in 1884 in [[Germany]].<ref name='getty-sg'>The Getty Conservation Institute, ''Silver Gelatin. The Atlas of Analytical Signatures of Photographic Processes''. J. Paul Getty Trust, 2013.</ref> The light-sensitive [[silver halide]] emulsion is then coated over the baryta layer. The baryta coating limits the penetration of the emulsion into the fibers of the paper and makes the emulsion more even, resulting in more uniform blacks.<ref>Salvaggio, ''Nanette L. Basic Photographic Materials and Processes.'' Taylor & Francis US, Oct 27, 2008. p. 362.</ref> Further coatings may then be present for fixing and protection of the image. Baryta has also been used to brighten papers intended for [[ink-jet printing]].<ref>Nikitas, Theano. "Inkjet papers that will give your photos pizzazz: are you and your clients bored with your photo prints? check out our favorite fine-art and specialty inkjet papers that are sure to make your images stand out." Photo District News July 2012: 36+. General Reference Center GOLD. Web. 3 November 2012</ref>
===Plastics filler===
Barium sulfate is commonly used as a [[filler (materials)|filler]] for plastics to increase the density of the polymer in vibrational mass damping applications. In [[polypropylene]] and [[polystyrene]] plastics, it is used as a filler in proportions up to 70%. It has an effect of increasing acid and alkali resistance and opacity. Such composites are also used as X-ray shielding materials due to their enhanced radio-opacity.<ref>{{cite journal |last1=Lopresti |first1=Mattia |last2=Alberto |first2=Gabriele |last3=Cantamessa |first3=Simone |last4=Cantino |first4=Giorgio |last5=Conterosito |first5=Eleonora |last6=Palin |first6=Luca |last7=Milanesio |first7=Marco |title=Light Weight, Easy Formable and Non-Toxic Polymer-Based Composites for Hard X-ray Shielding: A Theoretical and Experimental Study |journal=International Journal of Molecular Sciences |date=28 January 2020 |volume=21 |issue=3 |pages=833 |pmc=7037949 |doi=10.3390/ijms21030833 |doi-access=free |pmid=32012889}}</ref> In cases where machinability and weight are a concern, composites with high mass fraction (70–80%) of barium sulfate may be preferred to the more commonly used steel shields.<ref>{{cite journal |last1=Lopresti |first1=Mattia |last2=Alberto |first2=Gabriele |last3=Cantamessa |first3=Simone |last4=Cantino |first4=Giorgio |last5=Conterosito |first5=Eleonora |last6=Palin |first6=Luca |last7=Milanesio |first7=Marco |date=2020-01-28 |title=Light Weight, Easy Formable and Non-Toxic Polymer-Based Composites for Hard X-ray Shielding: A Theoretical and Experimental Study |journal=International Journal of Molecular Sciences |volume=21 |issue=3 |pages=833 |issn=1422-0067 |pmc=7037949 |doi=10.3390/ijms21030833 |doi-access=free |pmid=32012889}}</ref>
===Niche uses===
Barium sulfate is used in soil testing. Tests for [[soil pH]] and other qualities of soil use colored indicators, and small particles (usually clay) from the soil can cloud the test mixture and make it hard to see the color of the indicator. Barium sulfate added to the mixture binds with these particles, making them heavier so they fall to the bottom, leaving a clearer solution.
In [[colorimetry]], barium sulfate is used as a near-perfect [[diffuser (optics)|diffuser]] when measuring light sources.
In metal casting, the moulds used are often coated with barium sulfate in order to prevent the molten metal from bonding with the mould.
It is also used in [[brake lining]]s, [[anechoic|anacoustic]] foams, [[powder coating]]s, and [[root canal]] filling.
Barium sulfate is an ingredient in the [[rubber bullet|"rubber" pellets]] used by [[Carabineros de Chile|Chilean police]].<ref name=UChile>{{cite news |title=Investigación U. de Chile comprueba que perdigones usados por Carabineros contienen solo 20 por ciento de goma |date=November 18, 2019 |work=Universidad de Chile |url=https://www.uchile.cl/noticias/159315/perdigones-usados-por-carabineros-contienen-solo-20-por-ciento-de-goma |access-date=June 29, 2020}}</ref> This together with silica helps the pellet attain a 96.5 [[Shore durometer|Shore A]] hardness.<ref name=UChile/>
====Catalyst support====
Barium sulfate is used as a [[catalyst support]] when selectively [[hydrogenation|hydrogenating]] functional groups that are sensitive to [[redox|overreduction]]. With a low surface area, the contact time of the substrate with the catalyst is shorter and thus selectivity is achieved. Palladium on barium sulfate is also used as a catalyst in the [[Rosenmund reduction]].
====Pyrotechnics====
As barium compounds emit a characteristic green light when heated at high temperature, barium salts are often used in green pyrotechnic formulas, although [[nitrate]] and [[chlorate]] salts are more common. Barium sulfate is commonly used as a component of "strobe" pyrotechnic compositions.
====Copper industry====
As barium sulfate has a high [[melting point]] and is [[solubility|insoluble]] in water, it is used as a release material in casting of [[copper extraction#Refining|copper anode plates]]. The [[anode]] plates are cast in copper molds, so to avoid the direct contact of the liquid copper with the solid copper mold, a suspension of fine barium sulfate powder in water is used as a coating on the mold surface. Thus, when the molten copper solidifies in form of an anode plate it can be easily released from its mold.
====Radiometric measurements====
Barium sulfate is sometimes used (or else PTFE) to coat the interior of integrating spheres due to the high reflectance of the material and near [[Lambertian reflectance|Lambertian characteristics]].
====3D printing of firearms====
Barium sulfate is listed among the materials acceptable to the [[BATFE]] for the manufacturing of firearms and/or components that are made of plastic, to achieve compliance with the U.S. federal requirement that an X-ray machine must be able to accurately depict the shape of the plastic firearm or component.<ref name=BATF>{{cite news |title=Is a firearm illegal if it is made out of plastic? |date=September 23, 2016 |url=https://www.atf.gov/firearms/qa/firearm-illegal-if-it-made-plastic |access-date=March 4, 2023}}</ref>
==Production==
Almost all of the barium consumed commercially is obtained from [[barite]], which is often highly impure. Barite is processed by thermo-chemical sulfate reduction (TSR), also known as carbothermal reduction (heating with [[coke (fuel)|coke]]) to give [[barium sulfide]]:
: BaSO<sub>4</sub> + 4 C → BaS + 4 CO
In contrast to barium sulfate, barium sulfide is soluble in water and readily converted to the oxide, carbonate, and halides. To produce highly pure barium sulfate, the sulfide or chloride is treated with [[sulfuric acid]] or sulfate salts:
: BaS + H<sub>2</sub>SO<sub>4</sub> → BaSO<sub>4</sub> + H<sub>2</sub>S
Barium sulfate produced in this way is often called {{lang|fr|blanc fixe}}, which is French for "permanent white". Blanc fixe is the form of barium encountered in consumer products, such as paints.<ref name=Ullmann/>
In the laboratory barium sulfate is generated by combining solutions of barium ions and sulfate salts. Because barium sulfate is the least toxic salt of barium due to its insolubility, wastes containing barium salts are sometimes treated with [[sodium sulfate]] to immobilize (detoxify) the barium. Barium sulfate is one of the most insoluble salts of sulfate. Its low solubility is exploited in [[qualitative inorganic analysis]] as a test for Ba<sup>2+</sup> ions, as well as for sulfate.
Untreated raw materials such as natural [[baryte]] formed under [[hydrothermal mineral deposit|hydrothermal conditions]] may contain many impurities, a.o., [[quartz]], or even amorphous [[silica]].<ref name="Fedele_2003">{{cite journal |last1=Fedele |first1=L. |last2=Todesca |first2=R. |last3=Boni |first3=M. |title=Barite-silica mineralization at the inter-Ordovician unconformity in southwestern Sardinia (Italy): a fluid inclusion study |journal=Mineralogy and Petrology |date=1 February 2003 |volume=77 |issue=3–4 |pages=197–213 |bibcode=2003MinPe..77..197F |doi=10.1007/s00710-002-0200-9 |s2cid=129874363}}</ref>
==History==
Barium sulfate is reduced to [[barium sulfide]] by carbon. The accidental discovery of this conversion many centuries ago led to the discovery of the first synthetic [[phosphor]].<ref name=Holleman/> The sulfide, unlike the sulfate, is water-soluble.
During the early part of the 20th century, during the Japanese colonization period, '''hokutolite''' was found to exist naturally in the Beitou hot-springs area near Taipei City, Taiwan. Hokutolite is a radioactive mineral composed mostly of [[lead(II) sulfate|PbSO<sub>4</sub>]] and BaSO<sub>4</sub>, but also containing traces of uranium, thorium and radium. The Japanese harvested these elements for industrial uses, and also developed dozens of “[[Radioactive quackery|therapeutic hot-spring baths]]” in the area.<ref>{{cite journal |last1=Chu |first1=Tieh-Chi |last2=Wang |first2=Jeng-long |title=Radioactive Disequilihrium of Uranium and Thorium Nuclide Series in Hot Spring and River Water from Peitou Hot Spring Basin in Taipei |journal=Journal of Nuclear and Radiochemical Sciences |date=2000 |volume=1 |issue=1 |pages=5–10 |doi=10.14494/jnrs2000.1.5 |doi-access=free}}</ref>
==Safety aspects==
Although soluble salts of barium are moderately toxic to humans, barium sulfate is nontoxic due to its insolubility. The most common means of inadvertent barium poisoning arises from the consumption of soluble barium salts mislabeled as BaSO<sub>4</sub>. In the [[Celobar incident]] (Brazil, 2003), nine patients died from improperly prepared radiocontrast agent. In regards to occupational exposures, the [[Occupational Safety and Health Administration]] set a [[permissible exposure limit]] at 15 mg/m<sup>3</sup>, while the [[National Institute for Occupational Safety and Health]] has a [[recommended exposure limit]] at 10 mg/m<sup>3</sup>. For respiratory exposures, both agencies have set an occupational exposure limit at 5 mg/m<sup>3</sup>.<ref>{{cite web |title=Barium Sulfate |work=NIOSH Pocket Guide to Chemical Hazards |publisher=Centers for Disease Control and Prevention |date=April 4, 2011 |url=https://www.cdc.gov/niosh/npg/npgd0047.html |access-date=November 18, 2013}}</ref>
==See also==
* [[Baryte]]
* [[List of inorganic pigments]]
==References==
{{Reflist}}
{{Barium compounds}}
{{Contrast media}}
{{Sulfates}}
{{Authority control}}
[[Category:Barium compounds]]
[[Category:Sulfates]]
[[Category:Inorganic pigments]]
[[Category:Radiocontrast agents]]' |
New page wikitext, after the edit (new_wikitext) | '{{Short description|Inorganic chemical compound}}
{{Chembox
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|Watchedfields = changed
|verifiedrevid = 476997146
|ImageFile = Bariumsulfatpulver.png
|ImageFile1 = Barium-sulfate-2D.png kys
|ImageSize1 = 225px
|ImageName1 = Chemical structure of barium sulfate
|ImageFileL2 = Barite-unit-cell-3D-vdW.png
|ImageNameL2 = 3D model of barium sulfate
|Section1={{Chembox Identifiers
|UNII_Ref = {{fdacite|correct|FDA}}
|UNII = 25BB7EKE2E
|ChEMBL_Ref = {{ebicite|changed|EBI}}
|ChEMBL = 2105897
|InChIKey = TZCXTZWJZNENPQ-NUQVWONBAD
|StdInChI_Ref = {{stdinchicite|correct|chemspider}}
|StdInChI = 1S/Ba.H2O4S/c;1-5(2,3)4/h;(H2,1,2,3,4)/q+2;/p-2
|StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
|StdInChIKey = TZCXTZWJZNENPQ-UHFFFAOYSA-L
|CASNo = 7727-43-7
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|ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
|ChemSpiderID =22823
|EINECS = 231-784-4
|PubChem = 24414
|SMILES = [Ba+2].[O-]S([O-])(=O)=O
|InChI = 1/Ba.H2O4S/c;1-5(2,3)4/h;(H2,1,2,3,4)/q+2;/p-2
|RTECS = CR060000
|ChEBI_Ref = {{ebicite|changed|EBI}}
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|KEGG_Ref = {{keggcite|correct|kegg}}
|KEGG = D02052
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|UNNumber = 1564
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|Section2={{Chembox Properties
|Formula = BaSO<sub>4</sub>
|MolarMass = 233.39 g/mol
|Appearance = white crystalline
|Odor = odorless
|Density = 4.49 g/cm<sup>3</sup>
|MeltingPtC = 1580
|BoilingPtC = 1600
|BoilingPt_notes = (decomposes)
|Solubility = 0.2448 mg/100 mL (20 °C) <br> 0.285 mg/100 mL (30 °C)
|SolubilityProduct = 1.0842 × 10<sup>−10</sup> (25 °C)
|SolubleOther = insoluble in [[ethanol|alcohol]],<ref>{{cite book |title=CRC Handbook of Chemistry and Physics |publisher=CRC Press |year=2004 |edition=85th |pages=[https://archive.org/details/crchandbookofche81lide/page/4 4–45] |isbn=0-8493-0485-7 |url=https://archive.org/details/crchandbookofche81lide/page/4 |url-access=registration}}</ref> soluble in concentrated, hot [[sulfuric acid]]
|RefractIndex = 1.636 (alpha)
|MagSus = −71.3·10<sup>−6</sup> cm<sup>3</sup>/mol
}}
|Section3={{Chembox Structure
|CrystalStruct = orthorhombic
}}
|Section4={{Chembox Thermochemistry
|DeltaHf = −1465 kJ/mol<ref name="Zumdahl, Steven S. 2009">{{cite book |author=Zumdahl, Steven S. |title=Chemical Principles |edition=6th |publisher=Houghton Mifflin Company |year=2009 |isbn=978-0-618-94690-7}}</ref>
|Entropy = 132 J/(mol·K)<ref name="Zumdahl, Steven S. 2009"/>
|HeatCapacity = 101.7 J/(mol K)
}}
|Section5={{Chembox Pharmacology
|ATCCode_prefix = V08
|ATCCode_suffix = BA01
|AdminRoutes = by mouth, rectal
|Bioavail = negligible by mouth
|Excretion = rectal
|Legal_US = Rx only
}}
|Section6={{Chembox Hazards
|PPhrases = {{P-phrases|260|264|270|273|314|501}}
|NFPA-H = 0
|NFPA-F = 0
|NFPA-R = 0
|FlashPt = noncombustible
|FlashPt_ref=<ref name=PGCH/>
|PEL = TWA 15 mg/m<sup>3</sup> (total) TWA 5 mg/m<sup>3</sup> (resp)<ref name=PGCH>{{PGCH|0047}}</ref>
|REL = TWA 10 mg/m<sup>3</sup> (total) TWA 5 mg/m<sup>3</sup> (resp)<ref name=PGCH/>
|IDLH = N.D.<ref name=PGCH/>
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}}
'''Barium sulfate''' (or '''sulphate''') is the [[inorganic compound]] with the chemical formula [[barium|Ba]][[sulfate|SO<sub>4</sub>]]. It is a white crystalline solid that is odorless and [[solubility|insoluble]] in [[water]]. It occurs in nature as the mineral [[barite]], which is the main commercial source of [[barium]] and materials prepared from it. Its opaque white appearance and its high density are exploited in its main applications.<ref name=Holleman>Holleman, A. F. and Wiberg, E. (2001) ''Inorganic Chemistry'', San Diego, CA. Academic Press, {{ISBN|0-12-352651-5}}.</ref>
==Uses==
===Drilling fluids===
About 80% of the world's barium sulfate production, mostly purified mineral, is consumed as a component of [[oil well]] [[drilling fluid]]. It increases the density of the fluid,<ref name="Ullmann">{{cite book |chapter=Barium and Barium Compounds |title=Ullmann's Encyclopedia of Industrial Chemistry |year=2007 |last1=Kresse |first1=Robert |last2=Baudis |first2=Ulrich |last3=Jäger |first3=Paul |last4=Riechers |first4=H. Hermann |last5=Wagner |first5=Heinz |last6=Winkler |first6=Jochen |last7=Wolf |first7=Hans Uwe |isbn=978-3-527-30673-2 |doi=10.1002/14356007.a03_325.pub2}}</ref> increasing the hydrostatic pressure in the well and reducing the chance of a [[blowout (well drilling)|blowout]].
===Radiocontrast agent===
{{Main|Barium sulfate suspension}}
[[Barium sulfate suspension|Barium sulfate in suspension]] is often used medically as a [[radiocontrast]] agent for [[X-ray]] [[medical imaging|imaging]] and other diagnostic procedures. It is most often used in imaging of the [[gastrointestinal tract|GI tract]] during what is colloquially known as a "[[barium meal]]". It is administered orally, or by [[enema]], as a [[barium sulfate suspension|suspension]] of fine particles in a thick milk-like solution (often with sweetening and flavoring agents added). Although barium is a [[heavy metals|heavy metal]], and its water-soluble compounds are often highly toxic, the low solubility of barium sulfate protects the patient from absorbing harmful amounts of the metal. Barium sulfate is also readily removed from the body, unlike [[Thorotrast]], which it replaced. Due to the relatively high [[atomic number]] (''Z'' = 56) of barium, its compounds absorb X-rays more strongly than compounds derived from lighter nuclei.
===Pigment===
The majority of synthetic barium sulfate is used as a component of white pigment for paints. In oil paint, barium sulfate is almost transparent{{citation needed|date=December 2020}}, and is used as a filler or to modify consistency. One major manufacturer of artists' oil paint sells "permanent white" that contains a mixture of titanium white pigment ([[titanium dioxide|TiO<sub>2</sub>]]) and barium sulfate. The combination of barium sulfate and [[zinc sulfide]] (ZnS) is the inorganic pigment called [[lithopone]]. In photography it is used as a coating for certain photographic papers.<ref name=Ullmann/>
It is also used as a coating to diffuse light evenly.
===Light-reflecting paint for cooling===
Barium sulfate is highly reflective, of both visible and ultraviolet light.<ref name=":0">{{cite web |last=Puiu |first=Tibi |date=2022-10-04 |title=World's whitest paint is now thin enough to coat and cool down cars, trains and planes |website=ZME Science |language=en-US |url=https://www.zmescience.com/science/news-science/worlds-whitest-paint-usable-04102022/ |access-date=2022-10-12}}</ref> Researchers used it as an ingredient in paint that reflects 98.1% of [[solar radiation]], allowing surfaces to which it has been applied to stay cooler in sunlit conditions. Commercially available white paints only reflect 80 - 90% of solar radiation.<ref name="PurduePaint">{{cite web |last=Wiles |first=Kayla |date=September 16, 2021 |title=Purdue record for the whitest paint appears in latest edition of 'Guinness World Records' |website=purdue.edu |language=en |url=https://www.purdue.edu/newsroom/releases/2021/Q3/purdue-record-for-the-whitest-paint-appears-in-latest-edition-of-guinness-world-records.html |access-date=2022-10-12}}</ref> By using hexagonal nanoplatelet [[boron nitride]], the thickness of a coat of this type of paint was reduced to 0.15 mm.<ref name=":0"/>
===Paper brightener===
A thin layer of barium sulfate called baryta is first coated on the base surface of most [[photographic paper]] to increase the [[reflectiveness]] of the image, with the first such paper introduced in 1884 in [[Germany]].<ref name='getty-sg'>The Getty Conservation Institute, ''Silver Gelatin. The Atlas of Analytical Signatures of Photographic Processes''. J. Paul Getty Trust, 2013.</ref> The light-sensitive [[silver halide]] emulsion is then coated over the baryta layer. The baryta coating limits the penetration of the emulsion into the fibers of the paper and makes the emulsion more even, resulting in more uniform blacks.<ref>Salvaggio, ''Nanette L. Basic Photographic Materials and Processes.'' Taylor & Francis US, Oct 27, 2008. p. 362.</ref> Further coatings may then be present for fixing and protection of the image. Baryta has also been used to brighten papers intended for [[ink-jet printing]].<ref>Nikitas, Theano. "Inkjet papers that will give your photos pizzazz: are you and your clients bored with your photo prints? check out our favorite fine-art and specialty inkjet papers that are sure to make your images stand out." Photo District News July 2012: 36+. General Reference Center GOLD. Web. 3 November 2012</ref>
===Plastics filler===
Barium sulfate is commonly used as a [[filler (materials)|filler]] for plastics to increase the density of the polymer in vibrational mass damping applications. In [[polypropylene]] and [[polystyrene]] plastics, it is used as a filler in proportions up to 70%. It has an effect of increasing acid and alkali resistance and opacity. Such composites are also used as X-ray shielding materials due to their enhanced radio-opacity.<ref>{{cite journal |last1=Lopresti |first1=Mattia |last2=Alberto |first2=Gabriele |last3=Cantamessa |first3=Simone |last4=Cantino |first4=Giorgio |last5=Conterosito |first5=Eleonora |last6=Palin |first6=Luca |last7=Milanesio |first7=Marco |title=Light Weight, Easy Formable and Non-Toxic Polymer-Based Composites for Hard X-ray Shielding: A Theoretical and Experimental Study |journal=International Journal of Molecular Sciences |date=28 January 2020 |volume=21 |issue=3 |pages=833 |pmc=7037949 |doi=10.3390/ijms21030833 |doi-access=free |pmid=32012889}}</ref> In cases where machinability and weight are a concern, composites with high mass fraction (70–80%) of barium sulfate may be preferred to the more commonly used steel shields.<ref>{{cite journal |last1=Lopresti |first1=Mattia |last2=Alberto |first2=Gabriele |last3=Cantamessa |first3=Simone |last4=Cantino |first4=Giorgio |last5=Conterosito |first5=Eleonora |last6=Palin |first6=Luca |last7=Milanesio |first7=Marco |date=2020-01-28 |title=Light Weight, Easy Formable and Non-Toxic Polymer-Based Composites for Hard X-ray Shielding: A Theoretical and Experimental Study |journal=International Journal of Molecular Sciences |volume=21 |issue=3 |pages=833 |issn=1422-0067 |pmc=7037949 |doi=10.3390/ijms21030833 |doi-access=free |pmid=32012889}}</ref>
===Niche uses===
Barium sulfate is used in soil testing. Tests for [[soil pH]] and other qualities of soil use colored indicators, and small particles (usually clay) from the soil can cloud the test mixture and make it hard to see the color of the indicator. Barium sulfate added to the mixture binds with these particles, making them heavier so they fall to the bottom, leaving a clearer solution.
In [[colorimetry]], barium sulfate is used as a near-perfect [[diffuser (optics)|diffuser]] when measuring light sources.
In metal casting, the moulds used are often coated with barium sulfate in order to prevent the molten metal from bonding with the mould.
It is also used in [[brake lining]]s, [[anechoic|anacoustic]] foams, [[powder coating]]s, and [[root canal]] filling.
Barium sulfate is an ingredient in the [[rubber bullet|"rubber" pellets]] used by [[Carabineros de Chile|Chilean police]].<ref name=UChile>{{cite news |title=Investigación U. de Chile comprueba que perdigones usados por Carabineros contienen solo 20 por ciento de goma |date=November 18, 2019 |work=Universidad de Chile |url=https://www.uchile.cl/noticias/159315/perdigones-usados-por-carabineros-contienen-solo-20-por-ciento-de-goma |access-date=June 29, 2020}}</ref> This together with silica helps the pellet attain a 96.5 [[Shore durometer|Shore A]] hardness.<ref name=UChile/>
====Catalyst support====
Barium sulfate is used as a [[catalyst support]] when selectively [[hydrogenation|hydrogenating]] functional groups that are sensitive to [[redox|overreduction]]. With a low surface area, the contact time of the substrate with the catalyst is shorter and thus selectivity is achieved. Palladium on barium sulfate is also used as a catalyst in the [[Rosenmund reduction]].
====Pyrotechnics====
As barium compounds emit a characteristic green light when heated at high temperature, barium salts are often used in green pyrotechnic formulas, although [[nitrate]] and [[chlorate]] salts are more common. Barium sulfate is commonly used as a component of "strobe" pyrotechnic compositions.
====Copper industry====
As barium sulfate has a high [[melting point]] and is [[solubility|insoluble]] in water, it is used as a release material in casting of [[copper extraction#Refining|copper anode plates]]. The [[anode]] plates are cast in copper molds, so to avoid the direct contact of the liquid copper with the solid copper mold, a suspension of fine barium sulfate powder in water is used as a coating on the mold surface. Thus, when the molten copper solidifies in form of an anode plate it can be easily released from its mold.
====Radiometric measurements====
Barium sulfate is sometimes used (or else PTFE) to coat the interior of integrating spheres due to the high reflectance of the material and near [[Lambertian reflectance|Lambertian characteristics]].
====3D printing of firearms====
Barium sulfate is listed among the materials acceptable to the [[BATFE]] for the manufacturing of firearms and/or components that are made of plastic, to achieve compliance with the U.S. federal requirement that an X-ray machine must be able to accurately depict the shape of the plastic firearm or component.<ref name=BATF>{{cite news |title=Is a firearm illegal if it is made out of plastic? |date=September 23, 2016 |url=https://www.atf.gov/firearms/qa/firearm-illegal-if-it-made-plastic |access-date=March 4, 2023}}</ref>
==Production==
Almost all of the barium consumed commercially is obtained from [[barite]], which is often highly impure. Barite is processed by thermo-chemical sulfate reduction (TSR), also known as carbothermal reduction (heating with [[coke (fuel)|coke]]) to give [[barium sulfide]]:
: BaSO<sub>4</sub> + 4 C → BaS + 4 CO
In contrast to barium sulfate, barium sulfide is soluble in water and readily converted to the oxide, carbonate, and halides. To produce highly pure barium sulfate, the sulfide or chloride is treated with [[sulfuric acid]] or sulfate salts:
: BaS + H<sub>2</sub>SO<sub>4</sub> → BaSO<sub>4</sub> + H<sub>2</sub>S
Barium sulfate produced in this way is often called {{lang|fr|blanc fixe}}, which is French for "permanent white". Blanc fixe is the form of barium encountered in consumer products, such as paints.<ref name=Ullmann/>
In the laboratory barium sulfate is generated by combining solutions of barium ions and sulfate salts. Because barium sulfate is the least toxic salt of barium due to its insolubility, wastes containing barium salts are sometimes treated with [[sodium sulfate]] to immobilize (detoxify) the barium. Barium sulfate is one of the most insoluble salts of sulfate. Its low solubility is exploited in [[qualitative inorganic analysis]] as a test for Ba<sup>2+</sup> ions, as well as for sulfate.
Untreated raw materials such as natural [[baryte]] formed under [[hydrothermal mineral deposit|hydrothermal conditions]] may contain many impurities, a.o., [[quartz]], or even amorphous [[silica]].<ref name="Fedele_2003">{{cite journal |last1=Fedele |first1=L. |last2=Todesca |first2=R. |last3=Boni |first3=M. |title=Barite-silica mineralization at the inter-Ordovician unconformity in southwestern Sardinia (Italy): a fluid inclusion study |journal=Mineralogy and Petrology |date=1 February 2003 |volume=77 |issue=3–4 |pages=197–213 |bibcode=2003MinPe..77..197F |doi=10.1007/s00710-002-0200-9 |s2cid=129874363}}</ref>
==History==
Barium sulfate is reduced to [[barium sulfide]] by carbon. The accidental discovery of this conversion many centuries ago led to the discovery of the first synthetic [[phosphor]].<ref name=Holleman/> The sulfide, unlike the sulfate, is water-soluble.
During the early part of the 20th century, during the Japanese colonization period, '''hokutolite''' was found to exist naturally in the Beitou hot-springs area near Taipei City, Taiwan. Hokutolite is a radioactive mineral composed mostly of [[lead(II) sulfate|PbSO<sub>4</sub>]] and BaSO<sub>4</sub>, but also containing traces of uranium, thorium and radium. The Japanese harvested these elements for industrial uses, and also developed dozens of “[[Radioactive quackery|therapeutic hot-spring baths]]” in the area.<ref>{{cite journal |last1=Chu |first1=Tieh-Chi |last2=Wang |first2=Jeng-long |title=Radioactive Disequilihrium of Uranium and Thorium Nuclide Series in Hot Spring and River Water from Peitou Hot Spring Basin in Taipei |journal=Journal of Nuclear and Radiochemical Sciences |date=2000 |volume=1 |issue=1 |pages=5–10 |doi=10.14494/jnrs2000.1.5 |doi-access=free}}</ref>
==Safety aspects==
Although soluble salts of barium are moderately toxic to humans, barium sulfate is nontoxic due to its insolubility. The most common means of inadvertent barium poisoning arises from the consumption of soluble barium salts mislabeled as BaSO<sub>4</sub>. In the [[Celobar incident]] (Brazil, 2003), nine patients died from improperly prepared radiocontrast agent. In regards to occupational exposures, the [[Occupational Safety and Health Administration]] set a [[permissible exposure limit]] at 15 mg/m<sup>3</sup>, while the [[National Institute for Occupational Safety and Health]] has a [[recommended exposure limit]] at 10 mg/m<sup>3</sup>. For respiratory exposures, both agencies have set an occupational exposure limit at 5 mg/m<sup>3</sup>.<ref>{{cite web |title=Barium Sulfate |work=NIOSH Pocket Guide to Chemical Hazards |publisher=Centers for Disease Control and Prevention |date=April 4, 2011 |url=https://www.cdc.gov/niosh/npg/npgd0047.html |access-date=November 18, 2013}}</ref>
==See also==
* [[Baryte]]
* [[List of inorganic pigments]]
==References==
{{Reflist}}
{{Barium compounds}}
{{Contrast media}}
{{Sulfates}}
{{Authority control}}
[[Category:Barium compounds]]
[[Category:Sulfates]]
[[Category:Inorganic pigments]]
[[Category:Radiocontrast agents]]' |
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Parsed HTML source of the new revision (new_html) | '<div class="mw-content-ltr mw-parser-output" lang="en" dir="ltr"><div class="shortdescription nomobile noexcerpt noprint searchaux" style="display:none">Inorganic chemical compound</div>
<style data-mw-deduplicate="TemplateStyles:r1084375498">.mw-parser-output .ib-chembox{border-collapse:collapse;text-align:left}.mw-parser-output .ib-chembox td,.mw-parser-output .ib-chembox th{border:1px solid #a2a9b1;width:40%}.mw-parser-output .ib-chembox td+td{width:60%}</style>
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<caption>Barium sulfate
</caption>
<tbody><tr>
<td colspan="2" style="text-align:center; padding:2px;"><span typeof="mw:File"><a href="/enwiki/wiki/File:Bariumsulfatpulver.png" class="mw-file-description"><img src="/upwiki/wikipedia/commons/thumb/7/74/Bariumsulfatpulver.png/220px-Bariumsulfatpulver.png" decoding="async" width="220" height="249" class="mw-file-element" srcset="/upwiki/wikipedia/commons/thumb/7/74/Bariumsulfatpulver.png/330px-Bariumsulfatpulver.png 1.5x, /upwiki/wikipedia/commons/thumb/7/74/Bariumsulfatpulver.png/440px-Bariumsulfatpulver.png 2x" data-file-width="1198" data-file-height="1355" /></a></span>
</td></tr>
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<td colspan="2" style="text-align:center; padding:2px;"><span typeof="mw:Error mw:File"><a href="/enwiki//en.wikipedia.org/wiki/Special:Upload?wpDestFile=Barium-sulfate-2D.png_kys" class="new" title="File:Barium-sulfate-2D.png kys"><span class="mw-file-element mw-broken-media" data-width="225">Chemical structure of barium sulfate</span></a></span>
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<td style="border-right:1px solid #aaa; width:50%;"><figure class="mw-halign-center" typeof="mw:File"><a href="/enwiki/wiki/File:Barite-unit-cell-3D-vdW.png" class="mw-file-description" title="3D model of barium sulfate"><img alt="3D model of barium sulfate" src="/upwiki/wikipedia/commons/thumb/0/08/Barite-unit-cell-3D-vdW.png/110px-Barite-unit-cell-3D-vdW.png" decoding="async" width="110" height="89" class="mw-file-element" srcset="/upwiki/wikipedia/commons/thumb/0/08/Barite-unit-cell-3D-vdW.png/165px-Barite-unit-cell-3D-vdW.png 1.5x, /upwiki/wikipedia/commons/thumb/0/08/Barite-unit-cell-3D-vdW.png/220px-Barite-unit-cell-3D-vdW.png 2x" data-file-width="1100" data-file-height="891" /></a><figcaption>3D model of barium sulfate</figcaption></figure>
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<th colspan="2" style="background: #f8eaba; text-align: center;">Identifiers
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<td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/enwiki/wiki/CAS_Registry_Number" title="CAS Registry Number">CAS Number</a></div>
</td>
<td><style data-mw-deduplicate="TemplateStyles:r1126788409">.mw-parser-output .plainlist ol,.mw-parser-output .plainlist ul{line-height:inherit;list-style:none;margin:0;padding:0}.mw-parser-output .plainlist ol li,.mw-parser-output .plainlist ul li{margin-bottom:0}</style><div class="plainlist"><ul><li><span title="commonchemistry.cas.org"><a rel="nofollow" class="external text" href="https://commonchemistry.cas.org/detail?cas_rn=7727-43-7">7727-43-7</a></span><sup> <span typeof="mw:File"><span><img alt="check" src="/upwiki/wikipedia/en/thumb/f/fb/Yes_check.svg/7px-Yes_check.svg.png" decoding="async" width="7" height="7" class="mw-file-element" srcset="/upwiki/wikipedia/en/thumb/f/fb/Yes_check.svg/11px-Yes_check.svg.png 1.5x, /upwiki/wikipedia/en/thumb/f/fb/Yes_check.svg/14px-Yes_check.svg.png 2x" data-file-width="600" data-file-height="600" /></span></span><span style="display:none">Y</span></sup></li></ul></div>
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<td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;">3D model (<a href="/enwiki/wiki/JSmol" class="mw-redirect" title="JSmol">JSmol</a>)</div>
</td>
<td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li><span title="chemapps.stolaf.edu (3D interactive model)"><a rel="nofollow" class="external text" href="https://chemapps.stolaf.edu/jmol/jmol.php?model=%5BBa%2B2%5D.%5BO-%5DS%28%5BO-%5D%29%28%3DO%29%3DO">Interactive image</a></span></li></ul></div>
</td></tr>
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<td><a href="/enwiki/wiki/ChEBI" title="ChEBI">ChEBI</a>
</td>
<td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li><span title="www.ebi.ac.uk"><a rel="nofollow" class="external text" href="https://www.ebi.ac.uk/chebi/searchId.do?chebiId=133326">CHEBI:133326</a></span><sup> <span typeof="mw:File"><span><img alt="☒" src="/upwiki/wikipedia/commons/thumb/a/a2/X_mark.svg/7px-X_mark.svg.png" decoding="async" width="7" height="8" class="mw-file-element" srcset="/upwiki/wikipedia/commons/thumb/a/a2/X_mark.svg/11px-X_mark.svg.png 1.5x, /upwiki/wikipedia/commons/thumb/a/a2/X_mark.svg/14px-X_mark.svg.png 2x" data-file-width="525" data-file-height="600" /></span></span><span style="display:none">N</span></sup></li></ul></div>
</td></tr>
<tr>
<td><a href="/enwiki/wiki/ChEMBL" title="ChEMBL">ChEMBL</a>
</td>
<td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li><span title="www.ebi.ac.uk"><a rel="nofollow" class="external text" href="https://www.ebi.ac.uk/chembldb/index.php/compound/inspect/ChEMBL2105897">ChEMBL2105897</a></span><sup> <span typeof="mw:File"><span><img alt="☒" src="/upwiki/wikipedia/commons/thumb/a/a2/X_mark.svg/7px-X_mark.svg.png" decoding="async" width="7" height="8" class="mw-file-element" srcset="/upwiki/wikipedia/commons/thumb/a/a2/X_mark.svg/11px-X_mark.svg.png 1.5x, /upwiki/wikipedia/commons/thumb/a/a2/X_mark.svg/14px-X_mark.svg.png 2x" data-file-width="525" data-file-height="600" /></span></span><span style="display:none">N</span></sup></li></ul></div>
</td></tr>
<tr>
<td><a href="/enwiki/wiki/ChemSpider" title="ChemSpider">ChemSpider</a>
</td>
<td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li><span title="www.chemspider.com"><a rel="nofollow" class="external text" href="https://www.chemspider.com/Chemical-Structure.22823.html">22823</a></span><sup> <span typeof="mw:File"><span><img alt="check" src="/upwiki/wikipedia/en/thumb/f/fb/Yes_check.svg/7px-Yes_check.svg.png" decoding="async" width="7" height="7" class="mw-file-element" srcset="/upwiki/wikipedia/en/thumb/f/fb/Yes_check.svg/11px-Yes_check.svg.png 1.5x, /upwiki/wikipedia/en/thumb/f/fb/Yes_check.svg/14px-Yes_check.svg.png 2x" data-file-width="600" data-file-height="600" /></span></span><span style="display:none">Y</span></sup></li></ul></div>
</td></tr>
<tr>
<td><a href="/enwiki/wiki/DrugBank" title="DrugBank">DrugBank</a>
</td>
<td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li><span title="www.drugbank.ca"><a rel="nofollow" class="external text" href="https://www.drugbank.ca/drugs/DB11150">DB11150</a></span></li></ul></div>
</td></tr>
<tr>
<td><a href="/enwiki/wiki/ECHA_InfoCard" class="mw-redirect" title="ECHA InfoCard"><span title="echa.europa.eu">ECHA InfoCard</span></a>
</td>
<td><a rel="nofollow" class="external text" href="https://echa.europa.eu/substance-information/-/substanceinfo/100.028.896">100.028.896</a> <span class="mw-valign-text-top noprint" typeof="mw:File/Frameless"><a href="https://www.wikidata.org/wiki/Q309038#P2566" title="Edit this at Wikidata"><img alt="Edit this at Wikidata" src="/upwiki/wikipedia/en/thumb/8/8a/OOjs_UI_icon_edit-ltr-progressive.svg/10px-OOjs_UI_icon_edit-ltr-progressive.svg.png" decoding="async" width="10" height="10" class="mw-file-element" srcset="/upwiki/wikipedia/en/thumb/8/8a/OOjs_UI_icon_edit-ltr-progressive.svg/15px-OOjs_UI_icon_edit-ltr-progressive.svg.png 1.5x, /upwiki/wikipedia/en/thumb/8/8a/OOjs_UI_icon_edit-ltr-progressive.svg/20px-OOjs_UI_icon_edit-ltr-progressive.svg.png 2x" data-file-width="20" data-file-height="20" /></a></span>
</td></tr>
<tr>
<td><a href="/enwiki/wiki/European_Community_number" title="European Community number"><span title="European Community number (chemical identifier)">EC Number</span></a>
</td>
<td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li>231-784-4</li></ul></div>
</td></tr>
<tr>
<td><a href="/enwiki/wiki/KEGG" title="KEGG">KEGG</a>
</td>
<td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li><span title="www.kegg.jp"><a rel="nofollow" class="external text" href="https://www.kegg.jp/entry/D02052">D02052</a></span><sup> <span typeof="mw:File"><span><img alt="check" src="/upwiki/wikipedia/en/thumb/f/fb/Yes_check.svg/7px-Yes_check.svg.png" decoding="async" width="7" height="7" class="mw-file-element" srcset="/upwiki/wikipedia/en/thumb/f/fb/Yes_check.svg/11px-Yes_check.svg.png 1.5x, /upwiki/wikipedia/en/thumb/f/fb/Yes_check.svg/14px-Yes_check.svg.png 2x" data-file-width="600" data-file-height="600" /></span></span><span style="display:none">Y</span></sup></li></ul></div>
</td></tr>
<tr>
<td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/enwiki/wiki/PubChem" title="PubChem">PubChem</a> <abbr title="Compound ID">CID</abbr></div>
</td>
<td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li><span title="pubchem.ncbi.nlm.nih.gov"><a rel="nofollow" class="external text" href="https://pubchem.ncbi.nlm.nih.gov/compound/24414">24414</a></span></li></ul></div>
</td></tr>
<tr>
<td><a href="/enwiki/wiki/RTECS" class="mw-redirect" title="RTECS">RTECS number</a>
</td>
<td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li>CR060000</li></ul></div>
</td></tr>
<tr>
<td><a href="/enwiki/wiki/Unique_Ingredient_Identifier" title="Unique Ingredient Identifier">UNII</a>
</td>
<td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li><span title="precision.fda.gov"><a rel="nofollow" class="external text" href="https://precision.fda.gov/uniisearch/srs/unii/25BB7EKE2E">25BB7EKE2E</a></span><sup> <span typeof="mw:File"><span><img alt="check" src="/upwiki/wikipedia/en/thumb/f/fb/Yes_check.svg/7px-Yes_check.svg.png" decoding="async" width="7" height="7" class="mw-file-element" srcset="/upwiki/wikipedia/en/thumb/f/fb/Yes_check.svg/11px-Yes_check.svg.png 1.5x, /upwiki/wikipedia/en/thumb/f/fb/Yes_check.svg/14px-Yes_check.svg.png 2x" data-file-width="600" data-file-height="600" /></span></span><span style="display:none">Y</span></sup></li></ul></div>
</td></tr>
<tr>
<td><a href="/enwiki/wiki/UN_number" title="UN number">UN number</a>
</td>
<td>1564
</td></tr>
<tr>
<td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/enwiki/wiki/CompTox_Chemicals_Dashboard" title="CompTox Chemicals Dashboard">CompTox Dashboard</a> <span style="font-weight:normal">(<abbr title="U.S. Environmental Protection Agency">EPA</abbr>)</span></div>
</td>
<td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li><span title="comptox.epa.gov"><a rel="nofollow" class="external text" href="https://comptox.epa.gov/dashboard/chemical/details/DTXSID0050471">DTXSID0050471</a> <span class="mw-valign-text-top noprint" typeof="mw:File/Frameless"><a href="https://www.wikidata.org/wiki/Q309038#P3117" title="Edit this at Wikidata"><img alt="Edit this at Wikidata" src="/upwiki/wikipedia/en/thumb/8/8a/OOjs_UI_icon_edit-ltr-progressive.svg/10px-OOjs_UI_icon_edit-ltr-progressive.svg.png" decoding="async" width="10" height="10" class="mw-file-element" srcset="/upwiki/wikipedia/en/thumb/8/8a/OOjs_UI_icon_edit-ltr-progressive.svg/15px-OOjs_UI_icon_edit-ltr-progressive.svg.png 1.5x, /upwiki/wikipedia/en/thumb/8/8a/OOjs_UI_icon_edit-ltr-progressive.svg/20px-OOjs_UI_icon_edit-ltr-progressive.svg.png 2x" data-file-width="20" data-file-height="20" /></a></span></span></li></ul></div>
</td></tr>
<tr>
<td colspan="2"><div class="collapsible-list mw-collapsible mw-collapsed" style="text-align: left;">
<div style="line-height: 1.6em; font-weight: bold; text-align:left; font-weight:normal; background:transparent;"><div><a href="/enwiki/wiki/International_Chemical_Identifier" title="International Chemical Identifier">InChI</a></div></div>
<ul class="mw-collapsible-content" style="margin-top: 0; margin-bottom: 0; line-height: inherit; list-style: none; margin-left: 0; word-break:break-all;"><li style="line-height: inherit; margin: 0"><div style="border-top:1px solid #ccc; padding:0.2em 0 0.2em 1.5em; text-align:left;"><div style="word-wrap:break-word; text-indent:-1.5em; font-size:97%; line-height:120%;">InChI=1S/Ba.H2O4S/c;1-5(2,3)4/h;(H2,1,2,3,4)/q+2;/p-2<sup> <span typeof="mw:File"><span><img alt="check" src="/upwiki/wikipedia/en/thumb/f/fb/Yes_check.svg/7px-Yes_check.svg.png" decoding="async" width="7" height="7" class="mw-file-element" srcset="/upwiki/wikipedia/en/thumb/f/fb/Yes_check.svg/11px-Yes_check.svg.png 1.5x, /upwiki/wikipedia/en/thumb/f/fb/Yes_check.svg/14px-Yes_check.svg.png 2x" data-file-width="600" data-file-height="600" /></span></span><span style="display:none">Y</span></sup></div><div style="word-wrap:break-word; text-indent:-1.5em; font-size:97%; line-height:120%;">Key: TZCXTZWJZNENPQ-UHFFFAOYSA-L<sup> <span typeof="mw:File"><span><img alt="check" src="/upwiki/wikipedia/en/thumb/f/fb/Yes_check.svg/7px-Yes_check.svg.png" decoding="async" width="7" height="7" class="mw-file-element" srcset="/upwiki/wikipedia/en/thumb/f/fb/Yes_check.svg/11px-Yes_check.svg.png 1.5x, /upwiki/wikipedia/en/thumb/f/fb/Yes_check.svg/14px-Yes_check.svg.png 2x" data-file-width="600" data-file-height="600" /></span></span><span style="display:none">Y</span></sup></div></div></li><li style="line-height: inherit; margin: 0"><div style="border-top:1px solid #ccc; padding:0.2em 0 0.2em 1.5em; text-align:left;"><div style="word-wrap:break-word; text-indent:-1.5em; font-size:97%; line-height:120%;">InChI=1/Ba.H2O4S/c;1-5(2,3)4/h;(H2,1,2,3,4)/q+2;/p-2</div><div style="word-wrap:break-word; text-indent:-1.5em; font-size:97%; line-height:120%;">Key: TZCXTZWJZNENPQ-NUQVWONBAD</div></div></li></ul>
</div>
</td></tr>
<tr>
<td colspan="2"><div class="collapsible-list mw-collapsible mw-collapsed" style="text-align: left;">
<div style="line-height: 1.6em; font-weight: bold; text-align:left; font-weight:normal; background:transparent;"><div><a href="/enwiki/wiki/Simplified_molecular-input_line-entry_system" title="Simplified molecular-input line-entry system">SMILES</a></div></div>
<ul class="mw-collapsible-content" style="margin-top: 0; margin-bottom: 0; line-height: inherit; list-style: none; margin-left: 0; word-break:break-all;"><li style="line-height: inherit; margin: 0"><div style="border-top:1px solid #ccc; padding:0.2em 0 0.2em 1.6em; word-wrap:break-word; text-indent:-1.5em; text-align:left; font-size:97%; line-height:120%;">[Ba+2].[O-]S([O-])(=O)=O</div></li></ul>
</div>
</td></tr>
<tr>
<th colspan="2" style="background: #f8eaba; text-align: center;">Properties
</th></tr>
<tr>
<td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/enwiki/wiki/Chemical_formula" title="Chemical formula">Chemical formula</a></div>
</td>
<td>BaSO<sub>4</sub> 
</td></tr>
<tr>
<td><a href="/enwiki/wiki/Molar_mass" title="Molar mass">Molar mass</a>
</td>
<td>233.39 g/mol   
</td></tr>
<tr>
<td>Appearance
</td>
<td>white crystalline
</td></tr>
<tr>
<td><a href="/enwiki/wiki/Odor" title="Odor">Odor</a>
</td>
<td>odorless
</td></tr>
<tr>
<td><a href="/enwiki/wiki/Density" title="Density">Density</a>
</td>
<td>4.49 g/cm<sup>3</sup>
</td></tr>
<tr>
<td><a href="/enwiki/wiki/Melting_point" title="Melting point">Melting point</a>
</td>
<td>1,580 °C (2,880 °F; 1,850 K)
</td></tr>
<tr>
<td><a href="/enwiki/wiki/Boiling_point" title="Boiling point">Boiling point</a>
</td>
<td>1,600 °C (2,910 °F; 1,870 K) (decomposes)
</td></tr>
<tr>
<td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/enwiki/wiki/Aqueous_solution" title="Aqueous solution">Solubility in water</a></div>
</td>
<td>0.2448 mg/100 mL (20 °C) <br /> 0.285 mg/100 mL (30 °C)
</td></tr>
<tr>
<td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/enwiki/wiki/Solubility_equilibrium" title="Solubility equilibrium">Solubility product</a> (<i>K</i><sub>sp</sub>) </div>
</td>
<td>1.0842 × 10<sup>−10</sup> (25 °C)
</td></tr>
<tr>
<td><a href="/enwiki/wiki/Solubility" title="Solubility">Solubility</a>
</td>
<td>insoluble in <a href="/enwiki/wiki/Ethanol" title="Ethanol">alcohol</a>,<sup id="cite_ref-1" class="reference"><a href="#cite_note-1">[1]</a></sup> soluble in concentrated, hot <a href="/enwiki/wiki/Sulfuric_acid" title="Sulfuric acid">sulfuric acid</a>
</td></tr>
<tr>
<td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/enwiki/wiki/Magnetic_susceptibility" title="Magnetic susceptibility">Magnetic susceptibility</a> (χ)</div>
</td>
<td>−71.3·10<sup>−6</sup> cm<sup>3</sup>/mol
</td></tr>
<tr>
<td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/enwiki/wiki/Refractive_index" title="Refractive index">Refractive index</a> (<i>n</i><sub>D</sub>)</div>
</td>
<td>1.636 (alpha)
</td></tr>
<tr>
<th colspan="2" style="background: #f8eaba; text-align: center;">Structure
</th></tr>
<tr>
<td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/enwiki/wiki/Crystal_structure" title="Crystal structure">Crystal structure</a></div>
</td>
<td>orthorhombic
</td></tr>
<tr>
<th colspan="2" style="background: #f8eaba; text-align: center;">Thermochemistry
</th></tr>
<tr>
<td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/enwiki/wiki/Heat_capacity" title="Heat capacity">Heat capacity</a> <span style="font-family:sans-serif;font-size:112%;color:black;background-color:transparent;;">(<i>C</i>)</span></div>
</td>
<td>101.7 J/(mol K)
</td></tr>
<tr>
<td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/enwiki/wiki/Standard_molar_entropy" title="Standard molar entropy">Std molar<br />entropy</a> <span style="font-family:sans-serif;font-size:112%;color:black;background-color:transparent;;">(<i>S</i><sup>⦵</sup><sub>298</sub>)</span></div>
</td>
<td>132 J/(mol·K)<sup id="cite_ref-Zumdahl,_Steven_S._2009_2-0" class="reference"><a href="#cite_note-Zumdahl,_Steven_S._2009-2">[2]</a></sup>
</td></tr>
<tr>
<td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/enwiki/wiki/Standard_enthalpy_change_of_formation" class="mw-redirect" title="Standard enthalpy change of formation">Std enthalpy of<br />formation</a> <span style="font-family:sans-serif;font-size:112%;color:black;background-color:transparent;;">(Δ<sub>f</sub><i>H</i><sup>⦵</sup><sub>298</sub>)</span></div>
</td>
<td>−1465 kJ/mol<sup id="cite_ref-Zumdahl,_Steven_S._2009_2-1" class="reference"><a href="#cite_note-Zumdahl,_Steven_S._2009-2">[2]</a></sup>
</td></tr>
<tr>
<th colspan="2" style="background: #f8eaba; text-align: center;">Pharmacology
</th></tr>
<tr>
<td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/enwiki/wiki/Anatomical_Therapeutic_Chemical_Classification_System" title="Anatomical Therapeutic Chemical Classification System">ATC code</a></div>
</td>
<td><a href="/enwiki/wiki/ATC_code_V08" title="ATC code V08">V08BA01</a> (<span title="www.whocc.no"><a rel="nofollow" class="external text" href="https://www.whocc.no/atc_ddd_index/?code=V08BA01">WHO</a></span>) 
</td></tr>
<tr>
<td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/enwiki/wiki/Route_of_administration" title="Route of administration">Routes of<br />administration</a></div>
</td>
<td>by mouth, rectal
</td></tr>
<tr>
<td colspan="2" style="text-align:left; background-color:#eaeaea;"><a href="/enwiki/wiki/Pharmacokinetics" title="Pharmacokinetics">Pharmacokinetics</a>:
</td></tr>
<tr style="background:#f1f1f1;">
<td style="padding-left:1em;"><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/enwiki/wiki/Bioavailability" title="Bioavailability">Bioavailability</a></div>
</td>
<td>negligible by mouth
</td></tr>
<tr style="background:#f1f1f1;">
<td style="padding-left:1em;"><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/enwiki/wiki/Excretion" title="Excretion">Excretion</a></div>
</td>
<td>rectal
</td></tr>
<tr>
<td><a href="/enwiki/wiki/Regulation_of_therapeutic_goods" title="Regulation of therapeutic goods">Legal status</a>
</td>
<td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist">
<ul><li><small><abbr class="country-name" title="United States">US</abbr>:</small> <a href="/enwiki/wiki/Prescription_drug" title="Prescription drug">℞-only</a></li></ul></div>
</td></tr>
<tr>
<th colspan="2" style="background: #f8eaba; text-align: center;">Hazards
</th></tr>
<tr>
<td colspan="2" style="text-align:left; background-color:#eaeaea;"><a href="/enwiki/wiki/Globally_Harmonized_System_of_Classification_and_Labelling_of_Chemicals" title="Globally Harmonized System of Classification and Labelling of Chemicals"><b>GHS</b> labelling</a>:
</td></tr>
<tr style="background:#f1f1f1;">
<td style="padding-left:1em;"><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/enwiki/wiki/GHS_precautionary_statements" title="GHS precautionary statements">Precautionary statements</a></div>
</td>
<td><abbr class="abbr" title="P260: Do not breathe dust/fume/gas/mist/vapours/spray.">P260</abbr>, <abbr class="abbr" title="P264: Wash ... thoroughly after handling.">P264</abbr>, <abbr class="abbr" title="P270: Do not eat, drink or smoke when using this product.">P270</abbr>, <abbr class="abbr" title="P273: Avoid release to the environment.">P273</abbr>, <abbr class="abbr" title="P314: Get Medical advice/attention if you feel unwell.">P314</abbr>, <abbr class="abbr" title="P501: Dispose of contents/container to ...">P501</abbr>
</td></tr>
<tr>
<td><a href="/enwiki/wiki/NFPA_704" title="NFPA 704"><b>NFPA 704</b></a> (fire diamond)
</td>
<td><style data-mw-deduplicate="TemplateStyles:r1170367383">.mw-parser-output .nfpa-704-diamond-ref{float:right;padding:1px;text-align:right}.mw-parser-output .nfpa-704-diamond-container{width:82px;font-family:sans-serif;margin:0 auto}.mw-parser-output .nfpa-704-diamond-container-ref{float:left;margin-left:1em}.mw-parser-output .nfpa-704-diamond-images{float:left;font-size:20px;text-align:center;position:relative;height:80px;width:80px;padding:1px}.mw-parser-output .nfpa-704-diamond-map{position:absolute;height:80px;width:80px}.mw-parser-output .nfpa-704-diamond .noresize{margin:0 auto}.mw-parser-output .nfpa-704-diamond-code{line-height:1em;text-align:center;position:absolute}.mw-parser-output .nfpa-704-diamond-code>a{color:black}.mw-parser-output .nfpa-704-diamond-blue{width:13px;top:31px;left:15px}.mw-parser-output .nfpa-704-diamond-red{width:12px;top:12px;left:35px}.mw-parser-output .nfpa-704-diamond-yellow{width:13px;top:31px;left:54px}.mw-parser-output .nfpa-704-diamond-white-image{position:relative;top:51px;left:0}.mw-parser-output .nfpa-704-diamond-white-text{vertical-align:middle;text-align:center;line-height:80%;position:absolute;top:52px}.mw-parser-output .nfpa-704-diamond-white-text a>span{position:absolute;color:black}.mw-parser-output .nfpa-704-diamond-white-wors{font-size:15px;width:23px;left:29px}.mw-parser-output .nfpa-704-diamond-white-wox{font-size:15px;font-stretch:condensed;width:21px;line-height:80%;top:-4px;left:29px}.mw-parser-output .nfpa-704-diamond-white-abcp{font-size:13.5px;font-stretch:condensed;width:28px;left:26px}.mw-parser-output .nfpa-704-diamond-white-ac{font-size:10px;width:30px;left:25px}.mw-parser-output .nfpa-704-diamond-white-strike{text-decoration:line-through}</style><div class="nfpa-704-diamond"><div class="nfpa-704-diamond-container"><div class="nfpa-704-diamond-images nounderlines">
<div class="nfpa-704-diamond-map"><figure class="noresize" typeof="mw:File"><span><img alt="NFPA 704 four-colored diamond" src="/upwiki/wikipedia/commons/thumb/6/6f/NFPA_704.svg/80px-NFPA_704.svg.png" decoding="async" width="80" height="80" class="mw-file-element" srcset="/upwiki/wikipedia/commons/thumb/6/6f/NFPA_704.svg/120px-NFPA_704.svg.png 1.5x, /upwiki/wikipedia/commons/thumb/6/6f/NFPA_704.svg/160px-NFPA_704.svg.png 2x" data-file-width="512" data-file-height="512" usemap="#ImageMap_fbee98d65da2341e" /></span><map name="ImageMap_fbee98d65da2341e"><area href="/enwiki/wiki/NFPA_704#Blue" shape="poly" coords="23,23,47,47,23,70,0,47" alt="Health 0: Exposure under fire conditions would offer no hazard beyond that of ordinary combustible material. E.g. sodium chloride" title="Health 0: Exposure under fire conditions would offer no hazard beyond that of ordinary combustible material. E.g. sodium chloride" /><area href="/enwiki/wiki/NFPA_704#Red" shape="poly" coords="47,0,70,23,47,47,23,23" alt="Flammability 0: Will not burn. E.g. water" title="Flammability 0: Will not burn. E.g. water" /><area href="/enwiki/wiki/NFPA_704#Yellow" shape="poly" coords="70,23,94,47,70,70,47,47" alt="Instability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogen" title="Instability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogen" /><area href="/enwiki/wiki/NFPA_704#White" shape="poly" coords="47,47,70,70,47,94,23,70" alt="Special hazards (white): no code" title="Special hazards (white): no code" /></map><figcaption></figcaption></figure></div><div class="nfpa-704-diamond-code nfpa-704-diamond-blue">
<a href="/enwiki/wiki/NFPA_704#Blue" title="NFPA 704"><span title="Health 0: Exposure under fire conditions would offer no hazard beyond that of ordinary combustible material. E.g. sodium chloride">0</span></a></div><div class="nfpa-704-diamond-code nfpa-704-diamond-red">
<a href="/enwiki/wiki/NFPA_704#Red" title="NFPA 704"><span title="Flammability 0: Will not burn. E.g. water">0</span></a></div><div class="nfpa-704-diamond-code nfpa-704-diamond-yellow">
<a href="/enwiki/wiki/NFPA_704#Yellow" title="NFPA 704"><span title="Instability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogen">0</span></a></div></div></div></div>
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<td><a href="/enwiki/wiki/Flash_point" title="Flash point">Flash point</a>
</td>
<td>noncombustible<sup id="cite_ref-PGCH_3-3" class="reference"><a href="#cite_note-PGCH-3">[3]</a></sup>
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<td colspan="2" style="text-align:left; background-color:#eaeaea;"><a href="/enwiki/wiki/National_Institute_for_Occupational_Safety_and_Health" title="National Institute for Occupational Safety and Health"><b>NIOSH</b></a> (US health exposure limits):
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<td style="padding-left:1em;"><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/enwiki/wiki/Permissible_exposure_limit" title="Permissible exposure limit">PEL</a> (Permissible)</div>
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<td>TWA 15 mg/m<sup>3</sup> (total) TWA 5 mg/m<sup>3</sup> (resp)<sup id="cite_ref-PGCH_3-0" class="reference"><a href="#cite_note-PGCH-3">[3]</a></sup>
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<td style="padding-left:1em;"><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/enwiki/wiki/Recommended_exposure_limit" title="Recommended exposure limit">REL</a> (Recommended)</div>
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<td>TWA 10 mg/m<sup>3</sup> (total) TWA 5 mg/m<sup>3</sup> (resp)<sup id="cite_ref-PGCH_3-1" class="reference"><a href="#cite_note-PGCH-3">[3]</a></sup>
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<td style="padding-left:1em;"><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/enwiki/wiki/IDLH" class="mw-redirect" title="IDLH">IDLH</a> (Immediate danger)</div>
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<td>N.D.<sup id="cite_ref-PGCH_3-2" class="reference"><a href="#cite_note-PGCH-3">[3]</a></sup>
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<td colspan="2" style="text-align:left; background:#f8eaba; border:1px solid #a2a9b1;"><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;">Except where otherwise noted, data are given for materials in their <a href="/enwiki/wiki/Standard_state" title="Standard state">standard state</a> (at 25 °C [77 °F], 100 kPa).</div>
<div style="margin-top: 0.3em;"><div style="text-align:center;"><span typeof="mw:File"><span><img alt="☒" src="/upwiki/wikipedia/commons/thumb/a/a2/X_mark.svg/12px-X_mark.svg.png" decoding="async" width="12" height="14" class="mw-file-element" srcset="/upwiki/wikipedia/commons/thumb/a/a2/X_mark.svg/18px-X_mark.svg.png 1.5x, /upwiki/wikipedia/commons/thumb/a/a2/X_mark.svg/24px-X_mark.svg.png 2x" data-file-width="525" data-file-height="600" /></span></span><span style="display:none">N</span> <span class="reflink plainlinks nourlexpansion"><a class="external text" href="https://en.wikipedia.org/enwiki/w/index.php?title=Special:ComparePages&rev1=476997146&page2=Barium+sulfate">verify</a></span> (<a href="/enwiki/wiki/Wikipedia:WikiProject_Chemicals/Chembox_validation" title="Wikipedia:WikiProject Chemicals/Chembox validation">what is</a> <sup><span typeof="mw:File"><span><img alt="check" src="/upwiki/wikipedia/en/thumb/f/fb/Yes_check.svg/7px-Yes_check.svg.png" decoding="async" width="7" height="7" class="mw-file-element" srcset="/upwiki/wikipedia/en/thumb/f/fb/Yes_check.svg/11px-Yes_check.svg.png 1.5x, /upwiki/wikipedia/en/thumb/f/fb/Yes_check.svg/14px-Yes_check.svg.png 2x" data-file-width="600" data-file-height="600" /></span></span><span style="display:none">Y</span><span typeof="mw:File"><span><img alt="☒" src="/upwiki/wikipedia/commons/thumb/a/a2/X_mark.svg/7px-X_mark.svg.png" decoding="async" width="7" height="8" class="mw-file-element" srcset="/upwiki/wikipedia/commons/thumb/a/a2/X_mark.svg/11px-X_mark.svg.png 1.5x, /upwiki/wikipedia/commons/thumb/a/a2/X_mark.svg/14px-X_mark.svg.png 2x" data-file-width="525" data-file-height="600" /></span></span><span style="display:none">N</span></sup> ?)
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<div style="margin-top: 0.3em; text-align: center;"><a href="/enwiki/wiki/Wikipedia:Chemical_infobox#References" title="Wikipedia:Chemical infobox">Infobox references</a></div>
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</tbody></table><div class="shortdescription nomobile noexcerpt noprint searchaux" style="display:none">Chemical compound</div>
<p><b>Barium sulfate</b> (or <b>sulphate</b>) is the <a href="/enwiki/wiki/Inorganic_compound" title="Inorganic compound">inorganic compound</a> with the chemical formula <a href="/enwiki/wiki/Barium" title="Barium">Ba</a><a href="/enwiki/wiki/Sulfate" title="Sulfate">SO<sub>4</sub></a>. It is a white crystalline solid that is odorless and <a href="/enwiki/wiki/Solubility" title="Solubility">insoluble</a> in <a href="/enwiki/wiki/Water" title="Water">water</a>. It occurs in nature as the mineral <a href="/enwiki/wiki/Barite" class="mw-redirect" title="Barite">barite</a>, which is the main commercial source of <a href="/enwiki/wiki/Barium" title="Barium">barium</a> and materials prepared from it. Its opaque white appearance and its high density are exploited in its main applications.<sup id="cite_ref-Holleman_4-0" class="reference"><a href="#cite_note-Holleman-4">[4]</a></sup>
</p>
<div id="toc" class="toc" role="navigation" aria-labelledby="mw-toc-heading"><input type="checkbox" role="button" id="toctogglecheckbox" class="toctogglecheckbox" style="display:none" /><div class="toctitle" lang="en" dir="ltr"><h2 id="mw-toc-heading">Contents</h2><span class="toctogglespan"><label class="toctogglelabel" for="toctogglecheckbox"></label></span></div>
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<li class="toclevel-1 tocsection-1"><a href="#Uses"><span class="tocnumber">1</span> <span class="toctext">Uses</span></a>
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<li class="toclevel-2 tocsection-2"><a href="#Drilling_fluids"><span class="tocnumber">1.1</span> <span class="toctext">Drilling fluids</span></a></li>
<li class="toclevel-2 tocsection-3"><a href="#Radiocontrast_agent"><span class="tocnumber">1.2</span> <span class="toctext">Radiocontrast agent</span></a></li>
<li class="toclevel-2 tocsection-4"><a href="#Pigment"><span class="tocnumber">1.3</span> <span class="toctext">Pigment</span></a></li>
<li class="toclevel-2 tocsection-5"><a href="#Light-reflecting_paint_for_cooling"><span class="tocnumber">1.4</span> <span class="toctext">Light-reflecting paint for cooling</span></a></li>
<li class="toclevel-2 tocsection-6"><a href="#Paper_brightener"><span class="tocnumber">1.5</span> <span class="toctext">Paper brightener</span></a></li>
<li class="toclevel-2 tocsection-7"><a href="#Plastics_filler"><span class="tocnumber">1.6</span> <span class="toctext">Plastics filler</span></a></li>
<li class="toclevel-2 tocsection-8"><a href="#Niche_uses"><span class="tocnumber">1.7</span> <span class="toctext">Niche uses</span></a>
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<li class="toclevel-3 tocsection-9"><a href="#Catalyst_support"><span class="tocnumber">1.7.1</span> <span class="toctext">Catalyst support</span></a></li>
<li class="toclevel-3 tocsection-10"><a href="#Pyrotechnics"><span class="tocnumber">1.7.2</span> <span class="toctext">Pyrotechnics</span></a></li>
<li class="toclevel-3 tocsection-11"><a href="#Copper_industry"><span class="tocnumber">1.7.3</span> <span class="toctext">Copper industry</span></a></li>
<li class="toclevel-3 tocsection-12"><a href="#Radiometric_measurements"><span class="tocnumber">1.7.4</span> <span class="toctext">Radiometric measurements</span></a></li>
<li class="toclevel-3 tocsection-13"><a href="#3D_printing_of_firearms"><span class="tocnumber">1.7.5</span> <span class="toctext">3D printing of firearms</span></a></li>
</ul>
</li>
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<li class="toclevel-1 tocsection-14"><a href="#Production"><span class="tocnumber">2</span> <span class="toctext">Production</span></a></li>
<li class="toclevel-1 tocsection-15"><a href="#History"><span class="tocnumber">3</span> <span class="toctext">History</span></a></li>
<li class="toclevel-1 tocsection-16"><a href="#Safety_aspects"><span class="tocnumber">4</span> <span class="toctext">Safety aspects</span></a></li>
<li class="toclevel-1 tocsection-17"><a href="#See_also"><span class="tocnumber">5</span> <span class="toctext">See also</span></a></li>
<li class="toclevel-1 tocsection-18"><a href="#References"><span class="tocnumber">6</span> <span class="toctext">References</span></a></li>
</ul>
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<h2><span class="mw-headline" id="Uses">Uses</span><span class="mw-editsection">
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<h3><span class="mw-headline" id="Drilling_fluids">Drilling fluids</span><span class="mw-editsection">
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<p>About 80% of the world's barium sulfate production, mostly purified mineral, is consumed as a component of <a href="/enwiki/wiki/Oil_well" title="Oil well">oil well</a> <a href="/enwiki/wiki/Drilling_fluid" title="Drilling fluid">drilling fluid</a>. It increases the density of the fluid,<sup id="cite_ref-Ullmann_5-0" class="reference"><a href="#cite_note-Ullmann-5">[5]</a></sup> increasing the hydrostatic pressure in the well and reducing the chance of a <a href="/enwiki/wiki/Blowout_(well_drilling)" title="Blowout (well drilling)">blowout</a>.
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<h3><span class="mw-headline" id="Radiocontrast_agent">Radiocontrast agent</span><span class="mw-editsection">
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<style data-mw-deduplicate="TemplateStyles:r1033289096">.mw-parser-output .hatnote{font-style:italic}.mw-parser-output div.hatnote{padding-left:1.6em;margin-bottom:0.5em}.mw-parser-output .hatnote i{font-style:normal}.mw-parser-output .hatnote+link+.hatnote{margin-top:-0.5em}</style><div role="note" class="hatnote navigation-not-searchable">Main article: <a href="/enwiki/wiki/Barium_sulfate_suspension" title="Barium sulfate suspension">Barium sulfate suspension</a></div>
<p><a href="/enwiki/wiki/Barium_sulfate_suspension" title="Barium sulfate suspension">Barium sulfate in suspension</a> is often used medically as a <a href="/enwiki/wiki/Radiocontrast" class="mw-redirect" title="Radiocontrast">radiocontrast</a> agent for <a href="/enwiki/wiki/X-ray" title="X-ray">X-ray</a> <a href="/enwiki/wiki/Medical_imaging" title="Medical imaging">imaging</a> and other diagnostic procedures. It is most often used in imaging of the <a href="/enwiki/wiki/Gastrointestinal_tract" title="Gastrointestinal tract">GI tract</a> during what is colloquially known as a "<a href="/enwiki/wiki/Barium_meal" class="mw-redirect" title="Barium meal">barium meal</a>". It is administered orally, or by <a href="/enwiki/wiki/Enema" title="Enema">enema</a>, as a <a href="/enwiki/wiki/Barium_sulfate_suspension" title="Barium sulfate suspension">suspension</a> of fine particles in a thick milk-like solution (often with sweetening and flavoring agents added). Although barium is a <a href="/enwiki/wiki/Heavy_metals" title="Heavy metals">heavy metal</a>, and its water-soluble compounds are often highly toxic, the low solubility of barium sulfate protects the patient from absorbing harmful amounts of the metal. Barium sulfate is also readily removed from the body, unlike <a href="/enwiki/wiki/Thorotrast" title="Thorotrast">Thorotrast</a>, which it replaced. Due to the relatively high <a href="/enwiki/wiki/Atomic_number" title="Atomic number">atomic number</a> (<i>Z</i> = 56) of barium, its compounds absorb X-rays more strongly than compounds derived from lighter nuclei.
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<h3><span class="mw-headline" id="Pigment">Pigment</span><span class="mw-editsection">
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<p>The majority of synthetic barium sulfate is used as a component of white pigment for paints. In oil paint, barium sulfate is almost transparent<sup class="noprint Inline-Template Template-Fact" style="white-space:nowrap;">[<i><a href="/enwiki/wiki/Wikipedia:Citation_needed" title="Wikipedia:Citation needed"><span title="This claim needs references to reliable sources. (December 2020)">citation needed</span></a></i>]</sup>, and is used as a filler or to modify consistency. One major manufacturer of artists' oil paint sells "permanent white" that contains a mixture of titanium white pigment (<a href="/enwiki/wiki/Titanium_dioxide" title="Titanium dioxide">TiO<sub>2</sub></a>) and barium sulfate. The combination of barium sulfate and <a href="/enwiki/wiki/Zinc_sulfide" title="Zinc sulfide">zinc sulfide</a> (ZnS) is the inorganic pigment called <a href="/enwiki/wiki/Lithopone" title="Lithopone">lithopone</a>. In photography it is used as a coating for certain photographic papers.<sup id="cite_ref-Ullmann_5-1" class="reference"><a href="#cite_note-Ullmann-5">[5]</a></sup>
It is also used as a coating to diffuse light evenly.
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<h3><span class="mw-headline" id="Light-reflecting_paint_for_cooling">Light-reflecting paint for cooling</span><span class="mw-editsection">
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<p>Barium sulfate is highly reflective, of both visible and ultraviolet light.<sup id="cite_ref-:0_6-0" class="reference"><a href="#cite_note-:0-6">[6]</a></sup> Researchers used it as an ingredient in paint that reflects 98.1% of <a href="/enwiki/wiki/Solar_radiation" class="mw-redirect" title="Solar radiation">solar radiation</a>, allowing surfaces to which it has been applied to stay cooler in sunlit conditions. Commercially available white paints only reflect 80 - 90% of solar radiation.<sup id="cite_ref-PurduePaint_7-0" class="reference"><a href="#cite_note-PurduePaint-7">[7]</a></sup> By using hexagonal nanoplatelet <a href="/enwiki/wiki/Boron_nitride" title="Boron nitride">boron nitride</a>, the thickness of a coat of this type of paint was reduced to 0.15 mm.<sup id="cite_ref-:0_6-1" class="reference"><a href="#cite_note-:0-6">[6]</a></sup>
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<h3><span class="mw-headline" id="Paper_brightener">Paper brightener</span><span class="mw-editsection">
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<p>A thin layer of barium sulfate called baryta is first coated on the base surface of most <a href="/enwiki/wiki/Photographic_paper" title="Photographic paper">photographic paper</a> to increase the <a href="/enwiki/wiki/Reflectiveness" class="mw-redirect" title="Reflectiveness">reflectiveness</a> of the image, with the first such paper introduced in 1884 in <a href="/enwiki/wiki/Germany" title="Germany">Germany</a>.<sup id="cite_ref-getty-sg_8-0" class="reference"><a href="#cite_note-getty-sg-8">[8]</a></sup> The light-sensitive <a href="/enwiki/wiki/Silver_halide" title="Silver halide">silver halide</a> emulsion is then coated over the baryta layer. The baryta coating limits the penetration of the emulsion into the fibers of the paper and makes the emulsion more even, resulting in more uniform blacks.<sup id="cite_ref-9" class="reference"><a href="#cite_note-9">[9]</a></sup> Further coatings may then be present for fixing and protection of the image. Baryta has also been used to brighten papers intended for <a href="/enwiki/wiki/Ink-jet_printing" class="mw-redirect" title="Ink-jet printing">ink-jet printing</a>.<sup id="cite_ref-10" class="reference"><a href="#cite_note-10">[10]</a></sup>
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<h3><span class="mw-headline" id="Plastics_filler">Plastics filler</span><span class="mw-editsection">
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<p>Barium sulfate is commonly used as a <a href="/enwiki/wiki/Filler_(materials)" title="Filler (materials)">filler</a> for plastics to increase the density of the polymer in vibrational mass damping applications. In <a href="/enwiki/wiki/Polypropylene" title="Polypropylene">polypropylene</a> and <a href="/enwiki/wiki/Polystyrene" title="Polystyrene">polystyrene</a> plastics, it is used as a filler in proportions up to 70%. It has an effect of increasing acid and alkali resistance and opacity. Such composites are also used as X-ray shielding materials due to their enhanced radio-opacity.<sup id="cite_ref-11" class="reference"><a href="#cite_note-11">[11]</a></sup> In cases where machinability and weight are a concern, composites with high mass fraction (70–80%) of barium sulfate may be preferred to the more commonly used steel shields.<sup id="cite_ref-12" class="reference"><a href="#cite_note-12">[12]</a></sup>
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<h3><span class="mw-headline" id="Niche_uses">Niche uses</span><span class="mw-editsection">
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<p>Barium sulfate is used in soil testing. Tests for <a href="/enwiki/wiki/Soil_pH" title="Soil pH">soil pH</a> and other qualities of soil use colored indicators, and small particles (usually clay) from the soil can cloud the test mixture and make it hard to see the color of the indicator. Barium sulfate added to the mixture binds with these particles, making them heavier so they fall to the bottom, leaving a clearer solution.
</p><p>In <a href="/enwiki/wiki/Colorimetry" title="Colorimetry">colorimetry</a>, barium sulfate is used as a near-perfect <a href="/enwiki/wiki/Diffuser_(optics)" title="Diffuser (optics)">diffuser</a> when measuring light sources.
</p><p>In metal casting, the moulds used are often coated with barium sulfate in order to prevent the molten metal from bonding with the mould.
</p><p>It is also used in <a href="/enwiki/wiki/Brake_lining" title="Brake lining">brake linings</a>, <a href="/enwiki/wiki/Anechoic" class="mw-redirect" title="Anechoic">anacoustic</a> foams, <a href="/enwiki/wiki/Powder_coating" title="Powder coating">powder coatings</a>, and <a href="/enwiki/wiki/Root_canal" title="Root canal">root canal</a> filling.
</p><p>Barium sulfate is an ingredient in the <a href="/enwiki/wiki/Rubber_bullet" title="Rubber bullet">"rubber" pellets</a> used by <a href="/enwiki/wiki/Carabineros_de_Chile" title="Carabineros de Chile">Chilean police</a>.<sup id="cite_ref-UChile_13-0" class="reference"><a href="#cite_note-UChile-13">[13]</a></sup> This together with silica helps the pellet attain a 96.5 <a href="/enwiki/wiki/Shore_durometer" title="Shore durometer">Shore A</a> hardness.<sup id="cite_ref-UChile_13-1" class="reference"><a href="#cite_note-UChile-13">[13]</a></sup>
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<h4><span class="mw-headline" id="Catalyst_support">Catalyst support</span><span class="mw-editsection">
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<p>Barium sulfate is used as a <a href="/enwiki/wiki/Catalyst_support" title="Catalyst support">catalyst support</a> when selectively <a href="/enwiki/wiki/Hydrogenation" title="Hydrogenation">hydrogenating</a> functional groups that are sensitive to <a href="/enwiki/wiki/Redox" title="Redox">overreduction</a>. With a low surface area, the contact time of the substrate with the catalyst is shorter and thus selectivity is achieved. Palladium on barium sulfate is also used as a catalyst in the <a href="/enwiki/wiki/Rosenmund_reduction" title="Rosenmund reduction">Rosenmund reduction</a>.
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<h4><span class="mw-headline" id="Pyrotechnics">Pyrotechnics</span><span class="mw-editsection">
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<p>As barium compounds emit a characteristic green light when heated at high temperature, barium salts are often used in green pyrotechnic formulas, although <a href="/enwiki/wiki/Nitrate" title="Nitrate">nitrate</a> and <a href="/enwiki/wiki/Chlorate" title="Chlorate">chlorate</a> salts are more common. Barium sulfate is commonly used as a component of "strobe" pyrotechnic compositions.
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<h4><span class="mw-headline" id="Copper_industry">Copper industry</span><span class="mw-editsection">
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<p>As barium sulfate has a high <a href="/enwiki/wiki/Melting_point" title="Melting point">melting point</a> and is <a href="/enwiki/wiki/Solubility" title="Solubility">insoluble</a> in water, it is used as a release material in casting of <a href="/enwiki/wiki/Copper_extraction#Refining" title="Copper extraction">copper anode plates</a>. The <a href="/enwiki/wiki/Anode" title="Anode">anode</a> plates are cast in copper molds, so to avoid the direct contact of the liquid copper with the solid copper mold, a suspension of fine barium sulfate powder in water is used as a coating on the mold surface. Thus, when the molten copper solidifies in form of an anode plate it can be easily released from its mold.
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<h4><span class="mw-headline" id="Radiometric_measurements">Radiometric measurements</span><span class="mw-editsection">
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<p>Barium sulfate is sometimes used (or else PTFE) to coat the interior of integrating spheres due to the high reflectance of the material and near <a href="/enwiki/wiki/Lambertian_reflectance" title="Lambertian reflectance">Lambertian characteristics</a>.
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<h4><span class="mw-headline" id="3D_printing_of_firearms">3D printing of firearms</span><span class="mw-editsection">
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<p>Barium sulfate is listed among the materials acceptable to the <a href="/enwiki/wiki/BATFE" class="mw-redirect" title="BATFE">BATFE</a> for the manufacturing of firearms and/or components that are made of plastic, to achieve compliance with the U.S. federal requirement that an X-ray machine must be able to accurately depict the shape of the plastic firearm or component.<sup id="cite_ref-BATF_14-0" class="reference"><a href="#cite_note-BATF-14">[14]</a></sup>
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<h2><span class="mw-headline" id="Production">Production</span><span class="mw-editsection">
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<p>Almost all of the barium consumed commercially is obtained from <a href="/enwiki/wiki/Barite" class="mw-redirect" title="Barite">barite</a>, which is often highly impure. Barite is processed by thermo-chemical sulfate reduction (TSR), also known as carbothermal reduction (heating with <a href="/enwiki/wiki/Coke_(fuel)" title="Coke (fuel)">coke</a>) to give <a href="/enwiki/wiki/Barium_sulfide" title="Barium sulfide">barium sulfide</a>:
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<dl><dd>BaSO<sub>4</sub> + 4 C → BaS + 4 CO</dd></dl>
<p>In contrast to barium sulfate, barium sulfide is soluble in water and readily converted to the oxide, carbonate, and halides. To produce highly pure barium sulfate, the sulfide or chloride is treated with <a href="/enwiki/wiki/Sulfuric_acid" title="Sulfuric acid">sulfuric acid</a> or sulfate salts:
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<dl><dd>BaS + H<sub>2</sub>SO<sub>4</sub> → BaSO<sub>4</sub> + H<sub>2</sub>S</dd></dl>
<p>Barium sulfate produced in this way is often called <span title="French-language text"><i lang="fr">blanc fixe</i></span>, which is French for "permanent white". Blanc fixe is the form of barium encountered in consumer products, such as paints.<sup id="cite_ref-Ullmann_5-2" class="reference"><a href="#cite_note-Ullmann-5">[5]</a></sup>
</p><p>In the laboratory barium sulfate is generated by combining solutions of barium ions and sulfate salts. Because barium sulfate is the least toxic salt of barium due to its insolubility, wastes containing barium salts are sometimes treated with <a href="/enwiki/wiki/Sodium_sulfate" title="Sodium sulfate">sodium sulfate</a> to immobilize (detoxify) the barium. Barium sulfate is one of the most insoluble salts of sulfate. Its low solubility is exploited in <a href="/enwiki/wiki/Qualitative_inorganic_analysis" title="Qualitative inorganic analysis">qualitative inorganic analysis</a> as a test for Ba<sup>2+</sup> ions, as well as for sulfate.
</p><p>Untreated raw materials such as natural <a href="/enwiki/wiki/Baryte" title="Baryte">baryte</a> formed under <a href="/enwiki/wiki/Hydrothermal_mineral_deposit" title="Hydrothermal mineral deposit">hydrothermal conditions</a> may contain many impurities, a.o., <a href="/enwiki/wiki/Quartz" title="Quartz">quartz</a>, or even amorphous <a href="/enwiki/wiki/Silica" class="mw-redirect" title="Silica">silica</a>.<sup id="cite_ref-Fedele_2003_15-0" class="reference"><a href="#cite_note-Fedele_2003-15">[15]</a></sup>
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<h2><span class="mw-headline" id="History">History</span><span class="mw-editsection">
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<p>Barium sulfate is reduced to <a href="/enwiki/wiki/Barium_sulfide" title="Barium sulfide">barium sulfide</a> by carbon. The accidental discovery of this conversion many centuries ago led to the discovery of the first synthetic <a href="/enwiki/wiki/Phosphor" title="Phosphor">phosphor</a>.<sup id="cite_ref-Holleman_4-1" class="reference"><a href="#cite_note-Holleman-4">[4]</a></sup> The sulfide, unlike the sulfate, is water-soluble.
</p><p>During the early part of the 20th century, during the Japanese colonization period, <b>hokutolite</b> was found to exist naturally in the Beitou hot-springs area near Taipei City, Taiwan. Hokutolite is a radioactive mineral composed mostly of <a href="/enwiki/wiki/Lead(II)_sulfate" title="Lead(II) sulfate">PbSO<sub>4</sub></a> and BaSO<sub>4</sub>, but also containing traces of uranium, thorium and radium. The Japanese harvested these elements for industrial uses, and also developed dozens of “<a href="/enwiki/wiki/Radioactive_quackery" title="Radioactive quackery">therapeutic hot-spring baths</a>” in the area.<sup id="cite_ref-16" class="reference"><a href="#cite_note-16">[16]</a></sup>
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<h2><span class="mw-headline" id="Safety_aspects">Safety aspects</span><span class="mw-editsection">
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<p>Although soluble salts of barium are moderately toxic to humans, barium sulfate is nontoxic due to its insolubility. The most common means of inadvertent barium poisoning arises from the consumption of soluble barium salts mislabeled as BaSO<sub>4</sub>. In the <a href="/enwiki/wiki/Celobar_incident" title="Celobar incident">Celobar incident</a> (Brazil, 2003), nine patients died from improperly prepared radiocontrast agent. In regards to occupational exposures, the <a href="/enwiki/wiki/Occupational_Safety_and_Health_Administration" title="Occupational Safety and Health Administration">Occupational Safety and Health Administration</a> set a <a href="/enwiki/wiki/Permissible_exposure_limit" title="Permissible exposure limit">permissible exposure limit</a> at 15 mg/m<sup>3</sup>, while the <a href="/enwiki/wiki/National_Institute_for_Occupational_Safety_and_Health" title="National Institute for Occupational Safety and Health">National Institute for Occupational Safety and Health</a> has a <a href="/enwiki/wiki/Recommended_exposure_limit" title="Recommended exposure limit">recommended exposure limit</a> at 10 mg/m<sup>3</sup>. For respiratory exposures, both agencies have set an occupational exposure limit at 5 mg/m<sup>3</sup>.<sup id="cite_ref-17" class="reference"><a href="#cite_note-17">[17]</a></sup>
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<h2><span class="mw-headline" id="See_also">See also</span><span class="mw-editsection">
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<ul><li><a href="/enwiki/wiki/Baryte" title="Baryte">Baryte</a></li>
<li><a href="/enwiki/wiki/List_of_inorganic_pigments" title="List of inorganic pigments">List of inorganic pigments</a></li></ul>
<h2><span class="mw-headline" id="References">References</span><span class="mw-editsection">
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<li id="cite_note-1"><span class="mw-cite-backlink"><b><a href="#cite_ref-1">^</a></b></span> <span class="reference-text"><style data-mw-deduplicate="TemplateStyles:r1215172403">.mw-parser-output cite.citation{font-style:inherit;word-wrap:break-word}.mw-parser-output .citation q{quotes:"\"""\"""'""'"}.mw-parser-output .citation:target{background-color:rgba(0,127,255,0.133)}.mw-parser-output .id-lock-free.id-lock-free a{background:url("/upwiki/wikipedia/commons/6/65/Lock-green.svg")right 0.1em center/9px no-repeat}body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .id-lock-free a{background-size:contain}.mw-parser-output .id-lock-limited.id-lock-limited a,.mw-parser-output .id-lock-registration.id-lock-registration a{background:url("/upwiki/wikipedia/commons/d/d6/Lock-gray-alt-2.svg")right 0.1em center/9px no-repeat}body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .id-lock-limited a,body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .id-lock-registration a{background-size:contain}.mw-parser-output .id-lock-subscription.id-lock-subscription a{background:url("/upwiki/wikipedia/commons/a/aa/Lock-red-alt-2.svg")right 0.1em center/9px no-repeat}body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .id-lock-subscription a{background-size:contain}.mw-parser-output .cs1-ws-icon a{background:url("/upwiki/wikipedia/commons/4/4c/Wikisource-logo.svg")right 0.1em center/12px no-repeat}body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .cs1-ws-icon a{background-size:contain}.mw-parser-output .cs1-code{color:inherit;background:inherit;border:none;padding:inherit}.mw-parser-output .cs1-hidden-error{display:none;color:#d33}.mw-parser-output .cs1-visible-error{color:#d33}.mw-parser-output .cs1-maint{display:none;color:#2C882D;margin-left:0.3em}.mw-parser-output .cs1-format{font-size:95%}.mw-parser-output .cs1-kern-left{padding-left:0.2em}.mw-parser-output .cs1-kern-right{padding-right:0.2em}.mw-parser-output .citation .mw-selflink{font-weight:inherit}html.skin-theme-clientpref-night .mw-parser-output .cs1-maint{color:#18911F}html.skin-theme-clientpref-night .mw-parser-output .cs1-visible-error,html.skin-theme-clientpref-night .mw-parser-output .cs1-hidden-error{color:#f8a397}@media(prefers-color-scheme:dark){html.skin-theme-clientpref-os .mw-parser-output .cs1-visible-error,html.skin-theme-clientpref-os .mw-parser-output .cs1-hidden-error{color:#f8a397}html.skin-theme-clientpref-os .mw-parser-output .cs1-maint{color:#18911F}}</style><cite class="citation book cs1"><span class="id-lock-registration" title="Free registration required"><a rel="nofollow" class="external text" href="https://archive.org/details/crchandbookofche81lide/page/4"><i>CRC Handbook of Chemistry and Physics</i></a></span> (85th ed.). CRC Press. 2004. pp. <a rel="nofollow" class="external text" href="https://archive.org/details/crchandbookofche81lide/page/4">4–45</a>. <a href="/enwiki/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/enwiki/wiki/Special:BookSources/0-8493-0485-7" title="Special:BookSources/0-8493-0485-7"><bdi>0-8493-0485-7</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=CRC+Handbook+of+Chemistry+and+Physics&rft.pages=4-45&rft.edition=85th&rft.pub=CRC+Press&rft.date=2004&rft.isbn=0-8493-0485-7&rft_id=https%3A%2F%2Farchive.org%2Fdetails%2Fcrchandbookofche81lide%2Fpage%2F4&rfr_id=info%3Asid%2Fen.wikipedia.org%3ABarium+sulfate" class="Z3988"></span></span>
</li>
<li id="cite_note-Zumdahl,_Steven_S._2009-2"><span class="mw-cite-backlink">^ <a href="#cite_ref-Zumdahl,_Steven_S._2009_2-0"><sup><i><b>a</b></i></sup></a> <a href="#cite_ref-Zumdahl,_Steven_S._2009_2-1"><sup><i><b>b</b></i></sup></a></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1215172403"><cite id="CITEREFZumdahl,_Steven_S.2009" class="citation book cs1">Zumdahl, Steven S. (2009). <i>Chemical Principles</i> (6th ed.). Houghton Mifflin Company. <a href="/enwiki/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/enwiki/wiki/Special:BookSources/978-0-618-94690-7" title="Special:BookSources/978-0-618-94690-7"><bdi>978-0-618-94690-7</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Chemical+Principles&rft.edition=6th&rft.pub=Houghton+Mifflin+Company&rft.date=2009&rft.isbn=978-0-618-94690-7&rft.au=Zumdahl%2C+Steven+S.&rfr_id=info%3Asid%2Fen.wikipedia.org%3ABarium+sulfate" class="Z3988"></span></span>
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<li id="cite_note-PGCH-3"><span class="mw-cite-backlink">^ <a href="#cite_ref-PGCH_3-0"><sup><i><b>a</b></i></sup></a> <a href="#cite_ref-PGCH_3-1"><sup><i><b>b</b></i></sup></a> <a href="#cite_ref-PGCH_3-2"><sup><i><b>c</b></i></sup></a> <a href="#cite_ref-PGCH_3-3"><sup><i><b>d</b></i></sup></a></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1215172403"><cite id="CITEREFNIOSH_Pocket_Guide_to_Chemical_Hazards" class="citation web cs1">NIOSH Pocket Guide to Chemical Hazards. <a rel="nofollow" class="external text" href="https://www.cdc.gov/niosh/npg/npgd0047.html">"#0047"</a>. <a href="/enwiki/wiki/National_Institute_for_Occupational_Safety_and_Health" title="National Institute for Occupational Safety and Health">National Institute for Occupational Safety and Health</a> (NIOSH).</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=unknown&rft.btitle=%230047&rft.pub=National+Institute+for+Occupational+Safety+and+Health+%28NIOSH%29&rft.au=NIOSH+Pocket+Guide+to+Chemical+Hazards&rft_id=https%3A%2F%2Fwww.cdc.gov%2Fniosh%2Fnpg%2Fnpgd0047.html&rfr_id=info%3Asid%2Fen.wikipedia.org%3ABarium+sulfate" class="Z3988"></span></span>
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<li id="cite_note-Holleman-4"><span class="mw-cite-backlink">^ <a href="#cite_ref-Holleman_4-0"><sup><i><b>a</b></i></sup></a> <a href="#cite_ref-Holleman_4-1"><sup><i><b>b</b></i></sup></a></span> <span class="reference-text">Holleman, A. F. and Wiberg, E. (2001) <i>Inorganic Chemistry</i>, San Diego, CA. Academic Press, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1215172403"><a href="/enwiki/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/enwiki/wiki/Special:BookSources/0-12-352651-5" title="Special:BookSources/0-12-352651-5">0-12-352651-5</a>.</span>
</li>
<li id="cite_note-Ullmann-5"><span class="mw-cite-backlink">^ <a href="#cite_ref-Ullmann_5-0"><sup><i><b>a</b></i></sup></a> <a href="#cite_ref-Ullmann_5-1"><sup><i><b>b</b></i></sup></a> <a href="#cite_ref-Ullmann_5-2"><sup><i><b>c</b></i></sup></a></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1215172403"><cite id="CITEREFKresseBaudisJägerRiechers2007" class="citation book cs1">Kresse, Robert; Baudis, Ulrich; Jäger, Paul; Riechers, H. Hermann; Wagner, Heinz; Winkler, Jochen; Wolf, Hans Uwe (2007). "Barium and Barium Compounds". <i>Ullmann's Encyclopedia of Industrial Chemistry</i>. <a href="/enwiki/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<a rel="nofollow" class="external text" href="https://doi.org/10.1002%2F14356007.a03_325.pub2">10.1002/14356007.a03_325.pub2</a>. <a href="/enwiki/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/enwiki/wiki/Special:BookSources/978-3-527-30673-2" title="Special:BookSources/978-3-527-30673-2"><bdi>978-3-527-30673-2</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=bookitem&rft.atitle=Barium+and+Barium+Compounds&rft.btitle=Ullmann%27s+Encyclopedia+of+Industrial+Chemistry&rft.date=2007&rft_id=info%3Adoi%2F10.1002%2F14356007.a03_325.pub2&rft.isbn=978-3-527-30673-2&rft.aulast=Kresse&rft.aufirst=Robert&rft.au=Baudis%2C+Ulrich&rft.au=J%C3%A4ger%2C+Paul&rft.au=Riechers%2C+H.+Hermann&rft.au=Wagner%2C+Heinz&rft.au=Winkler%2C+Jochen&rft.au=Wolf%2C+Hans+Uwe&rfr_id=info%3Asid%2Fen.wikipedia.org%3ABarium+sulfate" class="Z3988"></span></span>
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<li id="cite_note-:0-6"><span class="mw-cite-backlink">^ <a href="#cite_ref-:0_6-0"><sup><i><b>a</b></i></sup></a> <a href="#cite_ref-:0_6-1"><sup><i><b>b</b></i></sup></a></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1215172403"><cite id="CITEREFPuiu2022" class="citation web cs1">Puiu, Tibi (2022-10-04). <a rel="nofollow" class="external text" href="https://www.zmescience.com/science/news-science/worlds-whitest-paint-usable-04102022/">"World's whitest paint is now thin enough to coat and cool down cars, trains and planes"</a>. <i>ZME Science</i><span class="reference-accessdate">. Retrieved <span class="nowrap">2022-10-12</span></span>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=unknown&rft.jtitle=ZME+Science&rft.atitle=World%27s+whitest+paint+is+now+thin+enough+to+coat+and+cool+down+cars%2C+trains+and+planes&rft.date=2022-10-04&rft.aulast=Puiu&rft.aufirst=Tibi&rft_id=https%3A%2F%2Fwww.zmescience.com%2Fscience%2Fnews-science%2Fworlds-whitest-paint-usable-04102022%2F&rfr_id=info%3Asid%2Fen.wikipedia.org%3ABarium+sulfate" class="Z3988"></span></span>
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<li id="cite_note-getty-sg-8"><span class="mw-cite-backlink"><b><a href="#cite_ref-getty-sg_8-0">^</a></b></span> <span class="reference-text">The Getty Conservation Institute, <i>Silver Gelatin. The Atlas of Analytical Signatures of Photographic Processes</i>. J. Paul Getty Trust, 2013.</span>
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<li id="cite_note-9"><span class="mw-cite-backlink"><b><a href="#cite_ref-9">^</a></b></span> <span class="reference-text">Salvaggio, <i>Nanette L. Basic Photographic Materials and Processes.</i> Taylor & Francis US, Oct 27, 2008. p. 362.</span>
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<li id="cite_note-10"><span class="mw-cite-backlink"><b><a href="#cite_ref-10">^</a></b></span> <span class="reference-text">Nikitas, Theano. "Inkjet papers that will give your photos pizzazz: are you and your clients bored with your photo prints? check out our favorite fine-art and specialty inkjet papers that are sure to make your images stand out." Photo District News July 2012: 36+. General Reference Center GOLD. Web. 3 November 2012</span>
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<li id="cite_note-11"><span class="mw-cite-backlink"><b><a href="#cite_ref-11">^</a></b></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1215172403"><cite id="CITEREFLoprestiAlbertoCantamessaCantino2020" class="citation journal cs1">Lopresti, Mattia; Alberto, Gabriele; Cantamessa, Simone; Cantino, Giorgio; Conterosito, Eleonora; Palin, Luca; Milanesio, Marco (28 January 2020). <a rel="nofollow" class="external text" href="https://www.ncbi.nlm.nih.gov/pmc/articles/PMC7037949">"Light Weight, Easy Formable and Non-Toxic Polymer-Based Composites for Hard X-ray Shielding: A Theoretical and Experimental Study"</a>. <i>International Journal of Molecular Sciences</i>. <b>21</b> (3): 833. <a href="/enwiki/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<span class="id-lock-free" title="Freely accessible"><a rel="nofollow" class="external text" href="https://doi.org/10.3390%2Fijms21030833">10.3390/ijms21030833</a></span>. <a href="/enwiki/wiki/PMC_(identifier)" class="mw-redirect" title="PMC (identifier)">PMC</a> <span class="id-lock-free" title="Freely accessible"><a rel="nofollow" class="external text" href="https://www.ncbi.nlm.nih.gov/pmc/articles/PMC7037949">7037949</a></span>. <a href="/enwiki/wiki/PMID_(identifier)" class="mw-redirect" title="PMID (identifier)">PMID</a> <a rel="nofollow" class="external text" href="https://pubmed.ncbi.nlm.nih.gov/32012889">32012889</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=International+Journal+of+Molecular+Sciences&rft.atitle=Light+Weight%2C+Easy+Formable+and+Non-Toxic+Polymer-Based+Composites+for+Hard+X-ray+Shielding%3A+A+Theoretical+and+Experimental+Study&rft.volume=21&rft.issue=3&rft.pages=833&rft.date=2020-01-28&rft_id=https%3A%2F%2Fwww.ncbi.nlm.nih.gov%2Fpmc%2Farticles%2FPMC7037949%23id-name%3DPMC&rft_id=info%3Apmid%2F32012889&rft_id=info%3Adoi%2F10.3390%2Fijms21030833&rft.aulast=Lopresti&rft.aufirst=Mattia&rft.au=Alberto%2C+Gabriele&rft.au=Cantamessa%2C+Simone&rft.au=Cantino%2C+Giorgio&rft.au=Conterosito%2C+Eleonora&rft.au=Palin%2C+Luca&rft.au=Milanesio%2C+Marco&rft_id=https%3A%2F%2Fwww.ncbi.nlm.nih.gov%2Fpmc%2Farticles%2FPMC7037949&rfr_id=info%3Asid%2Fen.wikipedia.org%3ABarium+sulfate" class="Z3988"></span></span>
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<li id="cite_note-12"><span class="mw-cite-backlink"><b><a href="#cite_ref-12">^</a></b></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1215172403"><cite id="CITEREFLoprestiAlbertoCantamessaCantino2020" class="citation journal cs1">Lopresti, Mattia; Alberto, Gabriele; Cantamessa, Simone; Cantino, Giorgio; Conterosito, Eleonora; Palin, Luca; Milanesio, Marco (2020-01-28). <a rel="nofollow" class="external text" href="https://www.ncbi.nlm.nih.gov/pmc/articles/PMC7037949">"Light Weight, Easy Formable and Non-Toxic Polymer-Based Composites for Hard X-ray Shielding: A Theoretical and Experimental Study"</a>. <i>International Journal of Molecular Sciences</i>. <b>21</b> (3): 833. <a href="/enwiki/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<span class="id-lock-free" title="Freely accessible"><a rel="nofollow" class="external text" href="https://doi.org/10.3390%2Fijms21030833">10.3390/ijms21030833</a></span>. <a href="/enwiki/wiki/ISSN_(identifier)" class="mw-redirect" title="ISSN (identifier)">ISSN</a> <a rel="nofollow" class="external text" href="https://www.worldcat.org/issn/1422-0067">1422-0067</a>. <a href="/enwiki/wiki/PMC_(identifier)" class="mw-redirect" title="PMC (identifier)">PMC</a> <span class="id-lock-free" title="Freely accessible"><a rel="nofollow" class="external text" href="https://www.ncbi.nlm.nih.gov/pmc/articles/PMC7037949">7037949</a></span>. <a href="/enwiki/wiki/PMID_(identifier)" class="mw-redirect" title="PMID (identifier)">PMID</a> <a rel="nofollow" class="external text" href="https://pubmed.ncbi.nlm.nih.gov/32012889">32012889</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=International+Journal+of+Molecular+Sciences&rft.atitle=Light+Weight%2C+Easy+Formable+and+Non-Toxic+Polymer-Based+Composites+for+Hard+X-ray+Shielding%3A+A+Theoretical+and+Experimental+Study&rft.volume=21&rft.issue=3&rft.pages=833&rft.date=2020-01-28&rft_id=https%3A%2F%2Fwww.ncbi.nlm.nih.gov%2Fpmc%2Farticles%2FPMC7037949%23id-name%3DPMC&rft.issn=1422-0067&rft_id=info%3Apmid%2F32012889&rft_id=info%3Adoi%2F10.3390%2Fijms21030833&rft.aulast=Lopresti&rft.aufirst=Mattia&rft.au=Alberto%2C+Gabriele&rft.au=Cantamessa%2C+Simone&rft.au=Cantino%2C+Giorgio&rft.au=Conterosito%2C+Eleonora&rft.au=Palin%2C+Luca&rft.au=Milanesio%2C+Marco&rft_id=https%3A%2F%2Fwww.ncbi.nlm.nih.gov%2Fpmc%2Farticles%2FPMC7037949&rfr_id=info%3Asid%2Fen.wikipedia.org%3ABarium+sulfate" class="Z3988"></span></span>
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.navbar-collapse{float:left;text-align:left}.mw-parser-output .navbar-boxtext{word-spacing:0}.mw-parser-output .navbar ul{display:inline-block;white-space:nowrap;line-height:inherit}.mw-parser-output .navbar-brackets::before{margin-right:-0.125em;content:"[ "}.mw-parser-output .navbar-brackets::after{margin-left:-0.125em;content:" ]"}.mw-parser-output .navbar li{word-spacing:-0.125em}.mw-parser-output .navbar a>span,.mw-parser-output .navbar a>abbr{text-decoration:inherit}.mw-parser-output .navbar-mini abbr{font-variant:small-caps;border-bottom:none;text-decoration:none;cursor:inherit}.mw-parser-output .navbar-ct-full{font-size:114%;margin:0 7em}.mw-parser-output .navbar-ct-mini{font-size:114%;margin:0 4em}</style><div class="navbar plainlinks hlist navbar-mini"><ul><li class="nv-view"><a href="/enwiki/wiki/Template:Barium_compounds" title="Template:Barium compounds"><abbr title="View this template" style=";;background:none transparent;border:none;box-shadow:none;padding:0;">v</abbr></a></li><li class="nv-talk"><a href="/enwiki/wiki/Template_talk:Barium_compounds" title="Template talk:Barium compounds"><abbr title="Discuss this template" style=";;background:none transparent;border:none;box-shadow:none;padding:0;">t</abbr></a></li><li class="nv-edit"><a href="/enwiki/wiki/Special:EditPage/Template:Barium_compounds" title="Special:EditPage/Template:Barium compounds"><abbr title="Edit this template" style=";;background:none transparent;border:none;box-shadow:none;padding:0;">e</abbr></a></li></ul></div><div id="Barium_compounds" style="font-size:114%;margin:0 4em"><a href="/enwiki/wiki/Barium_compounds" class="mw-redirect" title="Barium compounds">Barium compounds</a></div></th></tr><tr><td colspan="2" class="navbox-list navbox-odd hlist" style="width:100%;padding:0"><div style="padding:0 0.25em">
<ul><li><a href="/enwiki/wiki/Barium_hexaboride" title="Barium hexaboride">BaB<sub>6</sub></a></li>
<li><a href="/enwiki/wiki/Barium_borate" title="Barium borate">Ba(BO<sub>2</sub>)<sub>2</sub></a></li>
<li><a href="/enwiki/wiki/Barium_bromide" title="Barium bromide">BaBr<sub>2</sub></a></li>
<li><a href="/enwiki/wiki/Barium_bromate" title="Barium bromate">Ba(BrO<sub>3</sub>)<sub>2</sub></a></li>
<li><a href="/enwiki/wiki/Barium_acetate" title="Barium acetate">Ba(CH<sub>3</sub>CO<sub>2</sub>)<sub>2</sub></a></li>
<li><a href="/enwiki/wiki/Barium_acetylacetonate" title="Barium acetylacetonate">Ba(C<sub>5</sub>H<sub>7</sub>O<sub>2</sub>)<sub>2</sub></a></li>
<li><a href="/enwiki/wiki/Barium_hypochlorite" title="Barium hypochlorite">Ba(ClO)<sub>2</sub></a></li>
<li><a href="/enwiki/wiki/Barium_carbide" title="Barium carbide">BaC<sub>2</sub></a></li>
<li><a href="/enwiki/wiki/Barium_carbonate" title="Barium carbonate">BaCO<sub>3</sub></a></li>
<li><a href="/enwiki/wiki/Barium_oxalate" title="Barium oxalate">BaC<sub>2</sub>O<sub>4</sub></a></li>
<li><a href="/enwiki/wiki/Barium_chlorate" title="Barium chlorate">Ba(ClO<sub>3</sub>)<sub>2</sub></a></li>
<li><a href="/enwiki/wiki/Barium_chloride_fluoride" title="Barium chloride fluoride">BaClF</a></li>
<li><a href="/enwiki/wiki/Barium_perchlorate" title="Barium perchlorate">Ba(ClO<sub>4</sub>)<sub>2</sub></a></li>
<li><a href="/enwiki/wiki/Barium_cyanide" title="Barium cyanide">Ba(CN)<sub>2</sub></a></li>
<li><a href="/enwiki/wiki/Barium_chloride" title="Barium chloride">BaCl<sub>2</sub></a></li>
<li><a href="/enwiki/wiki/Barium_chromate" title="Barium chromate">BaCrO<sub>4</sub></a></li>
<li><a href="/enwiki/wiki/Barium_fluoride" title="Barium fluoride">BaF<sub>2</sub></a></li>
<li><a href="/enwiki/wiki/Barium_ferrate" title="Barium ferrate">BaFeO<sub>4</sub></a></li>
<li><a href="/enwiki/wiki/Barium_ferrite" title="Barium ferrite">BaFe<sub>2</sub>O<sub>4</sub></a></li>
<li><a href="/enwiki/wiki/Barium_hydride" title="Barium hydride">BaH<sub>2</sub></a></li>
<li><a href="/enwiki/wiki/Barium_iodide" title="Barium iodide">BaI<sub>2</sub></a></li>
<li><a href="/enwiki/wiki/Barium_iodate" title="Barium iodate">Ba(IO<sub>3</sub>)<sub>2</sub></a></li>
<li><a href="/enwiki/wiki/Barium_manganate" title="Barium manganate">BaMnO<sub>4</sub></a></li>
<li><a href="/enwiki/wiki/Barium_permanganate" title="Barium permanganate">Ba(MnO<sub>4</sub>)<sub>2</sub></a></li>
<li><a href="/enwiki/wiki/Barium_azide" title="Barium azide">Ba(N<sub>3</sub>)<sub>2</sub></a></li>
<li><a href="/enwiki/wiki/Barium_nitrite" title="Barium nitrite">Ba(NO<sub>2</sub>)<sub>2</sub></a></li>
<li><a href="/enwiki/wiki/Barium_nitrate" title="Barium nitrate">Ba(NO<sub>3</sub>)<sub>2</sub></a></li>
<li><a href="/enwiki/wiki/Barium_oxide" title="Barium oxide">BaO</a></li>
<li><a href="/enwiki/wiki/Barium_peroxide" title="Barium peroxide">BaO<sub>2</sub></a></li>
<li><a href="/enwiki/wiki/Barium_hydroxide" title="Barium hydroxide">Ba(OH)<sub>2</sub></a></li>
<li><a href="/enwiki/wiki/Barium_metaphosphate" title="Barium metaphosphate">Ba(PO<sub>3</sub>)<sub>2</sub></a></li>
<li><a href="/enwiki/wiki/Barium_sulfide" title="Barium sulfide">BaS</a></li>
<li><a href="/enwiki/wiki/Barium_selenide" title="Barium selenide">BaSe</a></li>
<li><a href="/enwiki/wiki/Barium_selenate" title="Barium selenate">BaSeO<sub>4</sub></a></li>
<li><a href="/enwiki/wiki/Barium_thiocyanate" title="Barium thiocyanate">Ba(SCN)<sub>2</sub></a></li>
<li><a href="/enwiki/wiki/Barium_sulfite" title="Barium sulfite">BaSO<sub>3</sub></a></li>
<li><a class="mw-selflink selflink">BaSO<sub>4</sub></a></li>
<li><a href="/enwiki/wiki/Barium_ruthenate" title="Barium ruthenate">BaRuO<sub>3</sub></a></li>
<li><a href="/enwiki/wiki/Barium_stannate" title="Barium stannate">BaSnO<sub>3</sub></a></li>
<li><a href="/enwiki/wiki/Barium_titanate" title="Barium titanate">BaTiO<sub>3</sub></a></li>
<li><a href="/enwiki/wiki/Barium_orthotitanate" title="Barium orthotitanate">Ba<sub>2</sub>TiO<sub>4</sub></a></li>
<li><a href="/enwiki/wiki/Barium_tungstate" title="Barium tungstate">BaWO<sub>4</sub></a></li>
<li><a href="/enwiki/wiki/BaZnGa" title="BaZnGa">BaZnGa</a></li>
<li><a href="/enwiki/wiki/Strontium_barium_niobate" title="Strontium barium niobate">Sr<sub>2</sub>Ba<sub>1-x</sub>Nb<sub>2</sub>O<sub>6</sub></a></li>
<li><a href="/enwiki/wiki/Yttrium_barium_copper_oxide" title="Yttrium barium copper oxide">YBa<sub>2</sub>Cu<sub>3</sub>O<sub>7-x</sub></a></li></ul>
</div></td></tr></tbody></table></div>
<div class="navbox-styles"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1129693374"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1061467846"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1129693374"></div><div role="navigation" class="navbox" aria-labelledby="Contrast_media_(V08)" style="padding:3px"><table class="nowraplinks mw-collapsible autocollapse navbox-inner" style="border-spacing:0;background:transparent;color:inherit"><tbody><tr><th scope="col" class="navbox-title" colspan="2"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1129693374"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1063604349"><div class="navbar plainlinks hlist navbar-mini"><ul><li class="nv-view"><a href="/enwiki/wiki/Template:Contrast_media" title="Template:Contrast media"><abbr title="View this template" style=";;background:none transparent;border:none;box-shadow:none;padding:0;">v</abbr></a></li><li class="nv-talk"><a href="/enwiki/wiki/Template_talk:Contrast_media" title="Template talk:Contrast media"><abbr title="Discuss this template" style=";;background:none transparent;border:none;box-shadow:none;padding:0;">t</abbr></a></li><li class="nv-edit"><a href="/enwiki/wiki/Special:EditPage/Template:Contrast_media" title="Special:EditPage/Template:Contrast media"><abbr title="Edit this template" style=";;background:none transparent;border:none;box-shadow:none;padding:0;">e</abbr></a></li></ul></div><div id="Contrast_media_(V08)" style="font-size:114%;margin:0 4em"><a href="/enwiki/wiki/Contrast_medium" class="mw-redirect" title="Contrast medium">Contrast media</a> (<a href="/enwiki/wiki/ATC_code_V08" title="ATC code V08">V08</a>)</div></th></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/enwiki/wiki/Radiocontrast" class="mw-redirect" title="Radiocontrast">X-ray and CT</a></th><td class="navbox-list-with-group navbox-list navbox-odd hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"></div><table class="nowraplinks navbox-subgroup" style="border-spacing:0"><tbody><tr><th scope="row" class="navbox-group" style="width:1%">Iodinated,<br />Water soluble</th><td class="navbox-list-with-group navbox-list navbox-odd" style="width:100%;padding:0"><div style="padding:0 0.25em"></div><table class="nowraplinks navbox-subgroup" style="border-spacing:0"><tbody><tr><th scope="row" class="navbox-group" style="width:1%">Nephrotropic,<br /><a href="/enwiki/wiki/Radiocontrast#High_osmolar_.28ionic.29" class="mw-redirect" title="Radiocontrast">high osmolar</a></th><td class="navbox-list-with-group navbox-list navbox-odd" style="width:100%;padding:0"><div style="padding:0 0.25em">
<ul><li><a href="/enwiki/wiki/Diatrizoic_acid" class="mw-redirect" title="Diatrizoic acid">Diatrizoic acid</a><sup>#</sup></li>
<li><a href="/enwiki/wiki/Metrizoic_acid" title="Metrizoic acid">Metrizoic acid</a></li>
<li><a href="/enwiki/wiki/Iodamide" title="Iodamide">Iodamide</a></li>
<li><a href="/enwiki/wiki/Iotalamic_acid" title="Iotalamic acid">Iotalamic acid</a></li>
<li><a href="/enwiki/wiki/Ioxitalamic_acid" title="Ioxitalamic acid">Ioxitalamic acid</a></li>
<li><a href="/enwiki/wiki/Ioglicic_acid" title="Ioglicic acid">Ioglicic acid</a></li>
<li><a href="/enwiki/wiki/Acetrizoic_acid" title="Acetrizoic acid">Acetrizoic acid</a></li>
<li><a href="/enwiki/wiki/Iocarmic_acid" title="Iocarmic acid">Iocarmic acid</a></li>
<li><a href="/enwiki/wiki/Methiodal" title="Methiodal">Methiodal</a></li>
<li><a href="/enwiki/wiki/Diodone" title="Diodone">Diodone</a></li></ul>
</div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Nephrotropic,<br /><a href="/enwiki/wiki/Radiocontrast#Low_osmolar_.28non-ionic.29" class="mw-redirect" title="Radiocontrast">low osmolar</a></th><td class="navbox-list-with-group navbox-list navbox-even" style="width:100%;padding:0"><div style="padding:0 0.25em">
<ul><li><a href="/enwiki/wiki/Metrizamide" title="Metrizamide">Metrizamide</a></li>
<li><a href="/enwiki/wiki/Iohexol" title="Iohexol">Iohexol</a><sup>#</sup></li>
<li><a href="/enwiki/wiki/Ioxaglic_acid" title="Ioxaglic acid">Ioxaglic acid</a></li>
<li><a href="/enwiki/wiki/Iopamidol" title="Iopamidol">Iopamidol</a></li>
<li><a href="/enwiki/wiki/Iopromide" title="Iopromide">Iopromide</a></li>
<li><a href="/enwiki/wiki/Iotrolan" title="Iotrolan">Iotrolan</a></li>
<li><a href="/enwiki/wiki/Ioversol" title="Ioversol">Ioversol</a></li>
<li><a href="/enwiki/wiki/Iopentol" title="Iopentol">Iopentol</a></li>
<li><a href="/enwiki/wiki/Iodixanol" title="Iodixanol">Iodixanol</a></li>
<li><a href="/enwiki/wiki/Iomeprol" title="Iomeprol">Iomeprol</a></li>
<li><a href="/enwiki/wiki/Iobitridol" title="Iobitridol">Iobitridol</a></li>
<li><a href="/enwiki/wiki/Ioxilan" title="Ioxilan">Ioxilan</a></li></ul>
</div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Hepatotropic</th><td class="navbox-list-with-group navbox-list navbox-odd" style="width:100%;padding:0"><div style="padding:0 0.25em">
<ul><li><a href="/enwiki/wiki/Iodoxamic_acid" title="Iodoxamic acid">Iodoxamic acid</a></li>
<li><a href="/enwiki/wiki/Iotroxic_acid" title="Iotroxic acid">Iotroxic acid</a><sup>#</sup></li>
<li><a href="/enwiki/wiki/Ioglycamic_acid" title="Ioglycamic acid">Ioglycamic acid</a></li>
<li><a href="/enwiki/wiki/Adipiodone" title="Adipiodone">Adipiodone</a></li>
<li><a href="/enwiki/wiki/Iobenzamic_acid" title="Iobenzamic acid">Iobenzamic acid</a></li>
<li><a href="/enwiki/wiki/Iopanoic_acid" title="Iopanoic acid">Iopanoic acid</a></li>
<li><a href="/enwiki/wiki/Iocetamic_acid" title="Iocetamic acid">Iocetamic acid</a></li>
<li><a href="/enwiki/wiki/Sodium_iopodate" class="mw-redirect" title="Sodium iopodate">Sodium iopodate</a></li>
<li><a href="/enwiki/wiki/Tyropanoic_acid" title="Tyropanoic acid">Tyropanoic acid</a></li>
<li><a href="/enwiki/w/index.php?title=Calcium_iopodate&action=edit&redlink=1" class="new" title="Calcium iopodate (page does not exist)">Calcium iopodate</a></li></ul>
</div></td></tr></tbody></table><div></div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Iodinated,<br />Water insoluble</th><td class="navbox-list-with-group navbox-list navbox-even" style="width:100%;padding:0"><div style="padding:0 0.25em">
<ul><li><a href="/enwiki/wiki/Lipiodol" title="Lipiodol">Ethiodized oil</a> (= <a href="/enwiki/wiki/Ethyl_ester" class="mw-redirect" title="Ethyl ester">Ethyl esters</a> of iodised <a href="/enwiki/wiki/Fatty_acid" title="Fatty acid">fatty acids</a>, lipiodol)</li>
<li><a href="/enwiki/wiki/Iopydol" title="Iopydol">Iopydol</a></li>
<li><a href="/enwiki/wiki/Propyliodone" title="Propyliodone">Propyliodone</a></li>
<li><a href="/enwiki/wiki/Iofendylate" title="Iofendylate">Iofendylate</a><sup>‡</sup></li></ul>
</div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Non-iodinated</th><td class="navbox-list-with-group navbox-list navbox-odd" style="width:100%;padding:0"><div style="padding:0 0.25em">
<ul><li><a class="mw-selflink selflink">Barium sulfate</a><sup>#</sup></li></ul>
</div></td></tr></tbody></table><div></div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/enwiki/wiki/MRI_contrast_agent" title="MRI contrast agent">MRI</a></th><td class="navbox-list-with-group navbox-list navbox-odd hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"></div><table class="nowraplinks navbox-subgroup" style="border-spacing:0"><tbody><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/enwiki/wiki/Paramagnetic" class="mw-redirect" title="Paramagnetic">Paramagnetic</a></th><td class="navbox-list-with-group navbox-list navbox-even" style="width:100%;padding:0"><div style="padding:0 0.25em">
<ul><li><b><a href="/enwiki/wiki/Gadolinium-based_MRI_contrast_agent" class="mw-redirect" title="Gadolinium-based MRI contrast agent">Gadolinium-based</a></b>: <a href="/enwiki/wiki/Gadobenic_acid" title="Gadobenic acid">Gadobenic acid</a></li>
<li><a href="/enwiki/wiki/Gadobutrol" title="Gadobutrol">Gadobutrol</a></li>
<li><a href="/enwiki/wiki/Gadodiamide" title="Gadodiamide">Gadodiamide</a></li>
<li><a href="/enwiki/wiki/Gadofosveset" title="Gadofosveset">Gadofosveset</a></li>
<li><a href="/enwiki/wiki/Gadolinium" title="Gadolinium">Gadolinium</a></li>
<li><a href="/enwiki/wiki/Gadopentetic_acid" title="Gadopentetic acid">Gadopentetic acid</a></li>
<li><a href="/enwiki/wiki/Gadopiclenol" title="Gadopiclenol">Gadopiclenol</a></li>
<li><a href="/enwiki/wiki/Gadoteric_acid" title="Gadoteric acid">Gadoteric acid</a></li>
<li><a href="/enwiki/wiki/Gadoteridol" title="Gadoteridol">Gadoteridol</a></li>
<li><a href="/enwiki/wiki/Gadoversetamide" title="Gadoversetamide">Gadoversetamide</a></li>
<li><a href="/enwiki/wiki/Gadoxetic_acid" title="Gadoxetic acid">Gadoxetic acid</a></li></ul>
<ul><li><b>Other</b>: <a href="/enwiki/wiki/Ferric_ammonium_citrate" class="mw-redirect" title="Ferric ammonium citrate">Ferric ammonium citrate</a></li>
<li><a href="/enwiki/wiki/Mangafodipir" title="Mangafodipir">Mangafodipir</a><sup>‡</sup></li></ul>
</div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/enwiki/wiki/Superparamagnetism" title="Superparamagnetism">Superparamagnetic</a></th><td class="navbox-list-with-group navbox-list navbox-odd" style="width:100%;padding:0"><div style="padding:0 0.25em">
<ul><li><a href="/enwiki/w/index.php?title=Ferumoxsil&action=edit&redlink=1" class="new" title="Ferumoxsil (page does not exist)">Ferumoxsil</a></li>
<li><a href="/enwiki/w/index.php?title=Ferristene&action=edit&redlink=1" class="new" title="Ferristene (page does not exist)">Ferristene</a></li>
<li><a href="/enwiki/wiki/Iron_oxide" title="Iron oxide">Iron oxide</a>, <a href="/enwiki/wiki/Nanoparticle" title="Nanoparticle">nanoparticles</a></li></ul>
</div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Other</th><td class="navbox-list-with-group navbox-list navbox-even" style="width:100%;padding:0"><div style="padding:0 0.25em">
<ul><li><a href="/enwiki/wiki/Perflubron" title="Perflubron">Perflubron</a></li></ul>
</div></td></tr></tbody></table><div></div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/enwiki/wiki/Contrast-enhanced_ultrasound" title="Contrast-enhanced ultrasound">Ultrasound</a></th><td class="navbox-list-with-group navbox-list navbox-odd hlist" style="width:100%;padding:0"><div style="padding:0 0.25em">
<ul><li><a href="/enwiki/wiki/Microsphere" class="mw-redirect" title="Microsphere">Microspheres</a> of <a href="/enwiki/wiki/Human_serum_albumin" title="Human serum albumin">human albumin</a></li>
<li><a href="/enwiki/wiki/Microparticle" title="Microparticle">Microparticles</a> of <a href="/enwiki/wiki/Galactose" title="Galactose">galactose</a></li>
<li><a href="/enwiki/wiki/Perflenapent" class="mw-redirect" title="Perflenapent">Perflenapent</a></li>
<li>Microspheres of <a href="/enwiki/wiki/Phospholipid" title="Phospholipid">phospholipids</a></li>
<li><a href="/enwiki/wiki/Sulfur_hexafluoride" title="Sulfur hexafluoride">Sulfur hexafluoride</a></li></ul>
</div></td></tr><tr><td colspan="2" class="navbox-list navbox-even hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"><div class="hlist">
<ul><li><sup>#</sup><a href="/enwiki/wiki/WHO_Model_List_of_Essential_Medicines" title="WHO Model List of Essential Medicines">WHO-EM</a></li>
<li><sup>‡</sup><a href="/enwiki/wiki/List_of_withdrawn_drugs" title="List of withdrawn drugs">Withdrawn</a> from market</li>
<li><a href="/enwiki/wiki/Clinical_trial" title="Clinical trial">Clinical trials</a>:
<ul><li><sup>†</sup><a href="/enwiki/wiki/Phases_of_clinical_research#Phase_III" title="Phases of clinical research">Phase III</a></li>
<li><sup>§</sup>Never to phase III</li></ul></li></ul>
</div></div></td></tr></tbody></table></div>
<div class="navbox-styles"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1129693374"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1061467846"><style data-mw-deduplicate="TemplateStyles:r886047488">.mw-parser-output .nobold{font-weight:normal}</style><style data-mw-deduplicate="TemplateStyles:r1123817410">.mw-parser-output .template-chem2-su{display:inline-block;font-size:80%;line-height:1;vertical-align:-0.35em}.mw-parser-output .template-chem2-su>span{display:block;text-align:left}.mw-parser-output sub.template-chem2-sub{font-size:80%;vertical-align:-0.35em}.mw-parser-output sup.template-chem2-sup{font-size:80%;vertical-align:0.65em}</style></div><div role="navigation" class="navbox" aria-labelledby="Compounds_containing_the_sulfate_group_(SO2−4)" style="display:table;;padding:3px"><table class="nowraplinks mw-collapsible autocollapse navbox-inner" style="border-spacing:0;background:transparent;color:inherit;table-layout:fixed;"><tbody><tr><th scope="col" class="navbox-title" colspan="2"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1129693374"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1063604349"><div class="navbar plainlinks hlist navbar-mini"><ul><li class="nv-view"><a href="/enwiki/wiki/Template:Sulfates" title="Template:Sulfates"><abbr title="View this template" style=";;background:none transparent;border:none;box-shadow:none;padding:0;">v</abbr></a></li><li class="nv-talk"><a href="/enwiki/wiki/Template_talk:Sulfates" title="Template talk:Sulfates"><abbr title="Discuss this template" style=";;background:none transparent;border:none;box-shadow:none;padding:0;">t</abbr></a></li><li class="nv-edit"><a href="/enwiki/wiki/Special:EditPage/Template:Sulfates" title="Special:EditPage/Template:Sulfates"><abbr title="Edit this template" style=";;background:none transparent;border:none;box-shadow:none;padding:0;">e</abbr></a></li></ul></div><div id="Compounds_containing_the_sulfate_group_(SO2−4)" style="font-size:114%;margin:0 4em">Compounds containing the <a href="/enwiki/wiki/Sulfate" title="Sulfate">sulfate</a> group (<span class="nobold"><span class="chemf nowrap">SO<span class="template-chem2-su"><span>2−</span><span>4</span></span></span></span>)</div></th></tr><tr><td colspan="2" class="navbox-list navbox-odd" style="width:100%;padding:0;border-width:0;"><div style="padding:0"><div class="mw-collapsible-content" style="overflow-x:auto">
<table class="center">
<tbody><tr style="background-color:mistyrose">
<td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap"><a href="/enwiki/wiki/Sulfuric_acid" title="Sulfuric acid">H<sub class="template-chem2-sub">2</sub>SO<sub class="template-chem2-sub">4</sub></a></span>
</td>
<td style="background-color:white;border:none">
</td>
<td style="background-color:white;border:none" colspan="11" rowspan="3">
</td>
<td style="background-color:white;border:none" colspan="5">
</td>
<td>He
</td></tr>
<tr style="background-color:mistyrose">
<td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap"><a href="/enwiki/wiki/Lithium_sulfate" title="Lithium sulfate">Li<sub class="template-chem2-sub">2</sub>SO<sub class="template-chem2-sub">4</sub></a></span>
</td>
<td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap"><a href="/enwiki/wiki/Beryllium_sulfate" title="Beryllium sulfate">BeSO<sub class="template-chem2-sub">4</sub></a></span>
</td>
<td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap"><a href="/enwiki/wiki/Boron_sulfate" class="mw-redirect" title="Boron sulfate">B<sub class="template-chem2-sub">2</sub>S<sub class="template-chem2-sub">2</sub>O<sub class="template-chem2-sub">9</sub></a></span><br /><a href="/enwiki/wiki/Borosulfate" title="Borosulfate">-BO<sub>3</sub></a><br /><a href="/enwiki/wiki/Borate_sulfate" title="Borate sulfate">+BO<sub>3</sub></a>
</td>
<td>esters<br /><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap"><a href="/enwiki/wiki/Organosulfate" title="Organosulfate">ROSO<span class="template-chem2-su"><span>−</span><span>3</span></span></a></span><br /><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">(RO)<sub class="template-chem2-sub">2</sub>SO<sub class="template-chem2-sub">2</sub></span><br /><a href="/enwiki/wiki/Sulfate_carbonate" title="Sulfate carbonate">+CO<sub>3</sub></a><br /><a href="/enwiki/wiki/Oxalate_sulfate" title="Oxalate sulfate">+C<sub>2</sub>O<sub>4</sub></a>
</td>
<td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap"><a href="/enwiki/wiki/Ammonium_sulfate" title="Ammonium sulfate">(NH<sub class="template-chem2-sub">4</sub>)<sub class="template-chem2-sub">2</sub>SO<sub class="template-chem2-sub">4</sub></a></span><br /><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap"><a href="/enwiki/wiki/Hydrazine_sulfate" title="Hydrazine sulfate">[N<sub class="template-chem2-sub">2</sub>H<sub class="template-chem2-sub">5</sub>]HSO<sub class="template-chem2-sub">4</sub></a></span><br /><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap"><a href="/enwiki/wiki/Hydroxylammonium_sulfate" title="Hydroxylammonium sulfate">(NH<sub class="template-chem2-sub">3</sub>OH)<sub class="template-chem2-sub">2</sub>SO<sub class="template-chem2-sub">4</sub></a></span><br /><a href="/enwiki/wiki/Nitrosylsulfuric_acid" title="Nitrosylsulfuric acid">NOHSO<sub>4</sub></a><br /><a href="/enwiki/wiki/Sulfate_nitrates" title="Sulfate nitrates">+NO<sub>3</sub></a>
</td>
<td><a href="/enwiki/wiki/Peroxymonosulfuric_acid" title="Peroxymonosulfuric acid">HOSO<sub>4</sub></a>
</td>
<td><a href="/enwiki/wiki/Sulfate_fluoride" title="Sulfate fluoride">+F</a>
</td>
<td>Ne
</td></tr>
<tr style="background-color:mistyrose">
<td><a href="/enwiki/wiki/Sodium_sulfate" title="Sodium sulfate">Na<sub>2</sub>SO<sub>4</sub></a><br /><a href="/enwiki/wiki/Sodium_bisulfate" title="Sodium bisulfate">NaHSO<sub>4</sub></a>
</td>
<td><a href="/enwiki/wiki/Magnesium_sulfate" title="Magnesium sulfate">MgSO<sub>4</sub></a>
</td>
<td><a href="/enwiki/wiki/Aluminium_sulfate" title="Aluminium sulfate">Al<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a><br /><a href="/enwiki/wiki/Aluminium_sulfacetate" title="Aluminium sulfacetate">Al<sub>2</sub>SO<sub>4</sub>(OAc)<sub>4</sub></a>
</td>
<td>Si
</td>
<td><a href="/enwiki/wiki/Phosphate_sulfate" title="Phosphate sulfate">+PO<sub>4</sub></a>
</td>
<td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap"><a href="/enwiki/wiki/Sulfate" title="Sulfate">SO<span class="template-chem2-su"><span>2−</span><span>4</span></span></a></span><br /><a href="/enwiki/wiki/Disulfuric_acid" title="Disulfuric acid">HSO<sub>3</sub>HSO<sub>4</sub></a><br /><a href="/enwiki/wiki/Peroxydisulfuric_acid" title="Peroxydisulfuric acid">(HSO<sub>4</sub>)<sub>2</sub></a><br /><a href="/enwiki/wiki/Sulfite_sulfate" title="Sulfite sulfate">+SO<sub>3</sub></a>
</td>
<td><a href="/enwiki/wiki/Sulfate_chloride" title="Sulfate chloride">+Cl</a>
</td>
<td>Ar
</td></tr>
<tr style="background-color:mistyrose">
<td><a href="/enwiki/wiki/Potassium_sulfate" title="Potassium sulfate">K<sub>2</sub>SO<sub>4</sub></a><br /><a href="/enwiki/wiki/Potassium_bisulfate" title="Potassium bisulfate">KHSO<sub>4</sub></a>
</td>
<td><a href="/enwiki/wiki/Calcium_sulfate" title="Calcium sulfate">CaSO<sub>4</sub></a>
</td>
<td style="background-color:white;border:none">
</td>
<td><a href="/enwiki/wiki/Scandium_sulfate" title="Scandium sulfate">Sc<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a>
</td>
<td><a href="/enwiki/wiki/Titanyl_sulfate" title="Titanyl sulfate">TiOSO<sub>4</sub></a>
</td>
<td><a href="/enwiki/wiki/Vanadium(II)_sulfate" title="Vanadium(II) sulfate">VSO<sub>4</sub></a><br /><a href="/enwiki/wiki/Vanadium(III)_sulfate" title="Vanadium(III) sulfate">V<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a><br /><a href="/enwiki/wiki/Vanadyl_sulfate" title="Vanadyl sulfate">VOSO<sub>4</sub></a>
</td>
<td><a href="/enwiki/wiki/Chromium(II)_sulfate" title="Chromium(II) sulfate">CrSO<sub>4</sub></a><br /><a href="/enwiki/wiki/Chromium(III)_sulfate" title="Chromium(III) sulfate">Cr<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a>
</td>
<td><a href="/enwiki/wiki/Manganese(II)_sulfate" title="Manganese(II) sulfate">MnSO<sub>4</sub></a>
</td>
<td><a href="/enwiki/wiki/Iron(II)_sulfate" title="Iron(II) sulfate">FeSO<sub>4</sub></a><br /><a href="/enwiki/wiki/Iron(III)_sulfate" title="Iron(III) sulfate">Fe<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a>
</td>
<td><a href="/enwiki/wiki/Cobalt(II)_sulfate" title="Cobalt(II) sulfate">CoSO<sub>4</sub></a><br /><a href="/enwiki/w/index.php?title=Cobalt(III)_sulfate&action=edit&redlink=1" class="new" title="Cobalt(III) sulfate (page does not exist)">Co<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a>
</td>
<td><a href="/enwiki/wiki/Nickel(II)_sulfate" title="Nickel(II) sulfate">NiSO<sub>4</sub></a><br /><a href="/enwiki/w/index.php?title=Nickel(III)_sulfate&action=edit&redlink=1" class="new" title="Nickel(III) sulfate (page does not exist)">Ni<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a>
</td>
<td><a href="/enwiki/wiki/Copper(II)_sulfate" title="Copper(II) sulfate">CuSO<sub>4</sub></a><br /><a href="/enwiki/wiki/Copper(I)_sulfate" title="Copper(I) sulfate">Cu<sub>2</sub>SO<sub>4</sub></a><br /><a href="/enwiki/wiki/Tetraamminecopper(II)_sulfate" title="Tetraamminecopper(II) sulfate">[Cu(NH<sub>3</sub>)<sub>4</sub>(H<sub>2</sub>O)]SO<sub>4</sub></a>
</td>
<td><a href="/enwiki/wiki/Zinc_sulfate" title="Zinc sulfate">ZnSO<sub>4</sub></a>
</td>
<td><a href="/enwiki/wiki/Gallium_sulfate" class="mw-redirect" title="Gallium sulfate">Ga<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a>
</td>
<td>Ge
</td>
<td>As
</td>
<td><a href="/enwiki/wiki/Selenite_sulfate" title="Selenite sulfate">+SeO<sub>3</sub></a>
</td>
<td>Br
</td>
<td>Kr
</td></tr>
<tr style="background-color:mistyrose">
<td><a href="/enwiki/wiki/Rubidium_hydrogen_sulfate" title="Rubidium hydrogen sulfate">RbHSO<sub>4</sub></a><br /><a href="/enwiki/wiki/Rubidium_sulfate" title="Rubidium sulfate">Rb<sub>2</sub>SO<sub>4</sub></a>
</td>
<td><a href="/enwiki/wiki/Strontium_sulfate" title="Strontium sulfate">SrSO<sub>4</sub></a>
</td>
<td style="background-color:white;border:none">
</td>
<td><a href="/enwiki/wiki/Yttrium_sulfate" class="mw-redirect" title="Yttrium sulfate">Y<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a>
</td>
<td><a href="/enwiki/wiki/Zirconium(IV)_sulfate" title="Zirconium(IV) sulfate">Zr(SO<sub>4</sub>)<sub>2</sub></a>
</td>
<td><a href="/enwiki/w/index.php?title=Niobium_dioxide_trisulfate&action=edit&redlink=1" class="new" title="Niobium dioxide trisulfate (page does not exist)">Nb<sub>2</sub>O<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a>
</td>
<td><a href="/enwiki/w/index.php?title=Molybdenum(VI)_oxysulfate&action=edit&redlink=1" class="new" title="Molybdenum(VI) oxysulfate (page does not exist)">MoO(SO<sub>4</sub>)<sub>2</sub></a><br /><a href="/enwiki/w/index.php?title=Molybdenum(VI)_dioxysulfate&action=edit&redlink=1" class="new" title="Molybdenum(VI) dioxysulfate (page does not exist)">MoO<sub>2</sub>(SO<sub>4</sub>)</a>
</td>
<td>Tc
</td>
<td><a href="/enwiki/w/index.php?title=Ruthenium(IV)_sulfate&action=edit&redlink=1" class="new" title="Ruthenium(IV) sulfate (page does not exist)">Ru(SO<sub>4</sub>)<sub>2</sub></a>
</td>
<td><a href="/enwiki/wiki/Rhodium(III)_sulfate" title="Rhodium(III) sulfate">Rh<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a>
</td>
<td><a href="/enwiki/wiki/Palladium(II)_sulfate" title="Palladium(II) sulfate">PdSO<sub>4</sub></a>
</td>
<td><a href="/enwiki/wiki/Silver_sulfate" title="Silver sulfate">Ag<sub>2</sub>SO<sub>4</sub></a><br /><a href="/enwiki/wiki/Silver(II)_sulfate" class="mw-redirect" title="Silver(II) sulfate">AgSO<sub>4</sub></a>
</td>
<td><a href="/enwiki/wiki/Cadmium_sulfate" title="Cadmium sulfate">CdSO<sub>4</sub></a>
</td>
<td><a href="/enwiki/wiki/Indium(III)_sulfate" title="Indium(III) sulfate">In<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a>
</td>
<td><a href="/enwiki/wiki/Tin(II)_sulfate" title="Tin(II) sulfate">SnSO<sub>4</sub></a><br /><a href="/enwiki/w/index.php?title=Tin(IV)_sulfate&action=edit&redlink=1" class="new" title="Tin(IV) sulfate (page does not exist)">Sn(SO<sub>4</sub>)<sub>2</sub></a>
</td>
<td><a href="/enwiki/wiki/Antimony_sulfate" class="mw-redirect" title="Antimony sulfate">Sb<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a>
</td>
<td>Te
</td>
<td><a href="/enwiki/wiki/Iodate_sulfate" title="Iodate sulfate">+IO<sub>3</sub></a>
</td>
<td>Xe
</td></tr>
<tr style="background-color:mistyrose">
<td><a href="/enwiki/wiki/Caesium_sulfate" title="Caesium sulfate">Cs<sub>2</sub>SO<sub>4</sub></a><br /><a href="/enwiki/wiki/Caesium_hydrogen_sulfate" class="mw-redirect" title="Caesium hydrogen sulfate">CsHSO<sub>4</sub></a>
</td>
<td><a class="mw-selflink selflink">BaSO<sub>4</sub></a>
</td>
<td style="background-color:white;border:none">*
</td>
<td><a href="/enwiki/w/index.php?title=Lutetium(III)_sulfate&action=edit&redlink=1" class="new" title="Lutetium(III) sulfate (page does not exist)">Lu<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a>
</td>
<td>Hf
</td>
<td>Ta
</td>
<td><a href="/enwiki/w/index.php?title=Tungsten(VI)_oxysulfate&action=edit&redlink=1" class="new" title="Tungsten(VI) oxysulfate (page does not exist)">WO(SO<sub>4</sub>)<sub>2</sub></a>
</td>
<td><a href="/enwiki/w/index.php?title=Rhenium(VII)_oxysulfate&action=edit&redlink=1" class="new" title="Rhenium(VII) oxysulfate (page does not exist)">Re<sub>2</sub>O<sub>5</sub>(SO<sub>4</sub>)<sub>2</sub></a>
</td>
<td><a href="/enwiki/w/index.php?title=Osmium(II)_sulfate&action=edit&redlink=1" class="new" title="Osmium(II) sulfate (page does not exist)">OsSO<sub>4</sub></a><br /><a href="/enwiki/w/index.php?title=Osmium(III)_sulfate&action=edit&redlink=1" class="new" title="Osmium(III) sulfate (page does not exist)">Os<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a><br /><a href="/enwiki/w/index.php?title=Osmium(IV)_sulfate&action=edit&redlink=1" class="new" title="Osmium(IV) sulfate (page does not exist)">Os(SO<sub>4</sub>)<sub>2</sub></a>
</td>
<td><a href="/enwiki/w/index.php?title=Iridium(II)_sulfate&action=edit&redlink=1" class="new" title="Iridium(II) sulfate (page does not exist)">IrSO<sub>4</sub></a><br /><a href="/enwiki/w/index.php?title=Iridium(III)_sulfate&action=edit&redlink=1" class="new" title="Iridium(III) sulfate (page does not exist)">Ir<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a>
</td>
<td><a href="/enwiki/w/index.php?title=Pentasulfatodiplatinate(III)&action=edit&redlink=1" class="new" title="Pentasulfatodiplatinate(III) (page does not exist)">Pt<sub>2</sub>(SO<sub>4</sub>)<sub>5</sub><sup>4–</sup></a>
</td>
<td><a href="/enwiki/wiki/Gold(II)_sulfate" title="Gold(II) sulfate">AuSO<sub>4</sub></a><br /><a href="/enwiki/w/index.php?title=Gold(III)_sulfate&action=edit&redlink=1" class="new" title="Gold(III) sulfate (page does not exist)">Au<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a>
</td>
<td><a href="/enwiki/wiki/Mercury(I)_sulfate" title="Mercury(I) sulfate">Hg<sub>2</sub>SO<sub>4</sub></a><br /><a href="/enwiki/wiki/Mercury(II)_sulfate" title="Mercury(II) sulfate">HgSO<sub>4</sub></a>
</td>
<td><a href="/enwiki/wiki/Thallium(I)_sulfate" title="Thallium(I) sulfate">Tl<sub>2</sub>SO<sub>4</sub></a><br /><a href="/enwiki/w/index.php?title=Thallium(III)_sulfate&action=edit&redlink=1" class="new" title="Thallium(III) sulfate (page does not exist)">Tl<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a>
</td>
<td><a href="/enwiki/wiki/Lead(II)_sulfate" title="Lead(II) sulfate">PbSO<sub>4</sub></a><br /><a href="/enwiki/w/index.php?title=Lead(IV)_sulfate&action=edit&redlink=1" class="new" title="Lead(IV) sulfate (page does not exist)">Pb(SO<sub>4</sub>)<sub>2</sub></a>
</td>
<td><a href="/enwiki/wiki/Bismuth(III)_sulfate" title="Bismuth(III) sulfate">Bi<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a>
</td>
<td><a href="/enwiki/w/index.php?title=Polonium(II)_sulfate&action=edit&redlink=1" class="new" title="Polonium(II) sulfate (page does not exist)">PoSO<sub>4</sub></a><br /><a href="/enwiki/wiki/Polonium(IV)_sulfate" title="Polonium(IV) sulfate">Po(SO<sub>4</sub>)<sub>2</sub></a>
</td>
<td>At
</td>
<td>Rn
</td></tr>
<tr style="background-color:mistyrose">
<td>Fr
</td>
<td><a href="/enwiki/wiki/Radium_sulfate" title="Radium sulfate">RaSO<sub>4</sub></a>
</td>
<td style="background-color:white;border:none">**
</td>
<td>Lr
</td>
<td>Rf
</td>
<td>Db
</td>
<td>Sg
</td>
<td>Bh
</td>
<td>Hs
</td>
<td>Mt
</td>
<td>Ds
</td>
<td>Rg
</td>
<td>Cn
</td>
<td>Nh
</td>
<td>Fl
</td>
<td>Mc
</td>
<td>Lv
</td>
<td>Ts
</td>
<td>Og
</td></tr>
<tr>
<td style="background-color:white;border:none" colspan="2" rowspan="3">
</td>
<td style="background-color:white;border:none" colspan="20"> 
</td></tr>
<tr style="background-color:mistyrose">
<td style="background-color:white;border:none">*
</td>
<td><a href="/enwiki/w/index.php?title=Lanthanum(III)_sulfate&action=edit&redlink=1" class="new" title="Lanthanum(III) sulfate (page does not exist)">La<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a>
</td>
<td><a href="/enwiki/wiki/Cerium(III)_sulfate" title="Cerium(III) sulfate">Ce<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a><br /><a href="/enwiki/wiki/Cerium(IV)_sulfate" title="Cerium(IV) sulfate">Ce(SO<sub>4</sub>)<sub>2</sub></a>
</td>
<td><a href="/enwiki/wiki/Praseodymium(III)_sulfate" title="Praseodymium(III) sulfate">Pr<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a>
</td>
<td><a href="/enwiki/wiki/Neodymium(III)_sulfate" title="Neodymium(III) sulfate">Nd<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a>
</td>
<td><a href="/enwiki/w/index.php?title=Promethium(III)_sulfate&action=edit&redlink=1" class="new" title="Promethium(III) sulfate (page does not exist)">Pm<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a>
</td>
<td><a href="/enwiki/w/index.php?title=Samarium(III)_sulfate&action=edit&redlink=1" class="new" title="Samarium(III) sulfate (page does not exist)">Sm<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a>
</td>
<td><a href="/enwiki/wiki/Europium(II)_sulfate" title="Europium(II) sulfate">EuSO<sub>4</sub></a><br /><a href="/enwiki/w/index.php?title=Europium(III)_sulfate&action=edit&redlink=1" class="new" title="Europium(III) sulfate (page does not exist)">Eu<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a>
</td>
<td><a href="/enwiki/w/index.php?title=Gadolinium(III)_sulfate&action=edit&redlink=1" class="new" title="Gadolinium(III) sulfate (page does not exist)">Gd<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a>
</td>
<td><a href="/enwiki/w/index.php?title=Terbium(III)_sulfate&action=edit&redlink=1" class="new" title="Terbium(III) sulfate (page does not exist)">Tb<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a>
</td>
<td><a href="/enwiki/w/index.php?title=Dysprosium(III)_sulfate&action=edit&redlink=1" class="new" title="Dysprosium(III) sulfate (page does not exist)">Dy<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a>
</td>
<td><a href="/enwiki/w/index.php?title=Holmium(III)_sulfate&action=edit&redlink=1" class="new" title="Holmium(III) sulfate (page does not exist)">Ho<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a>
</td>
<td><a href="/enwiki/w/index.php?title=Erbium(III)_sulfate&action=edit&redlink=1" class="new" title="Erbium(III) sulfate (page does not exist)">Er<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a>
</td>
<td><a href="/enwiki/w/index.php?title=Thulium(III)_sulfate&action=edit&redlink=1" class="new" title="Thulium(III) sulfate (page does not exist)">Tm<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a>
</td>
<td><a href="/enwiki/wiki/Ytterbium(III)_sulfate" title="Ytterbium(III) sulfate">Yb<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a>
</td></tr>
<tr style="background-color:mistyrose">
<td style="background-color:white;border:none">**
</td>
<td><a href="/enwiki/w/index.php?title=Actinium(III)_sulfate&action=edit&redlink=1" class="new" title="Actinium(III) sulfate (page does not exist)">Ac<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a>
</td>
<td><a href="/enwiki/w/index.php?title=Thorium(IV)_sulfate&action=edit&redlink=1" class="new" title="Thorium(IV) sulfate (page does not exist)">Th(SO<sub>4</sub>)<sub>2</sub></a>
</td>
<td>Pa
</td>
<td><a href="/enwiki/w/index.php?title=Uranium(III)_sulfate&action=edit&redlink=1" class="new" title="Uranium(III) sulfate (page does not exist)">U<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a><br /><a href="/enwiki/wiki/Uranium(IV)_sulfate" title="Uranium(IV) sulfate">U(SO<sub>4</sub>)<sub>2</sub></a><br /><a href="/enwiki/wiki/Uranyl_sulfate" title="Uranyl sulfate">UO<sub>2</sub>SO<sub>4</sub></a>
</td>
<td><a href="/enwiki/w/index.php?title=Neptunium(IV)_sulfate&action=edit&redlink=1" class="new" title="Neptunium(IV) sulfate (page does not exist)">Np(SO<sub>4</sub>)<sub>2</sub></a>
</td>
<td><a href="/enwiki/w/index.php?title=Plutonium(IV)_sulfate&action=edit&redlink=1" class="new" title="Plutonium(IV) sulfate (page does not exist)">Pu(SO<sub>4</sub>)<sub>2</sub></a>
</td>
<td><a href="/enwiki/w/index.php?title=Americium(III)_sulfate&action=edit&redlink=1" class="new" title="Americium(III) sulfate (page does not exist)">Am<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a>
</td>
<td><a href="/enwiki/w/index.php?title=Curium(III)_sulfate&action=edit&redlink=1" class="new" title="Curium(III) sulfate (page does not exist)">Cm<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a>
</td>
<td>Bk
</td>
<td><a href="/enwiki/w/index.php?title=Californium(III)_sulfate&action=edit&redlink=1" class="new" title="Californium(III) sulfate (page does not exist)">Cf<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a>
</td>
<td>Es
</td>
<td>Fm
</td>
<td>Md
</td>
<td>No
</td></tr></tbody></table></div>
</div></td></tr></tbody></table></div>
<div class="navbox-styles"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1129693374"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1061467846"></div><div role="navigation" class="navbox authority-control" aria-labelledby="Authority_control_databases_frameless&#124;text-top&#124;10px&#124;alt=Edit_this_at_Wikidata&#124;link=https&#58;//www.wikidata.org/wiki/Q309038#identifiers&#124;class=noprint&#124;Edit_this_at_Wikidata" style="padding:3px"><table class="nowraplinks hlist mw-collapsible autocollapse navbox-inner" style="border-spacing:0;background:transparent;color:inherit"><tbody><tr><th scope="col" class="navbox-title" colspan="2"><div id="Authority_control_databases_frameless&#124;text-top&#124;10px&#124;alt=Edit_this_at_Wikidata&#124;link=https&#58;//www.wikidata.org/wiki/Q309038#identifiers&#124;class=noprint&#124;Edit_this_at_Wikidata" style="font-size:114%;margin:0 4em"><a href="/enwiki/wiki/Help:Authority_control" title="Help:Authority control">Authority control databases</a> <span class="mw-valign-text-top noprint" typeof="mw:File/Frameless"><a href="https://www.wikidata.org/wiki/Q309038#identifiers" title="Edit this at Wikidata"><img alt="Edit this at Wikidata" src="/upwiki/wikipedia/en/thumb/8/8a/OOjs_UI_icon_edit-ltr-progressive.svg/10px-OOjs_UI_icon_edit-ltr-progressive.svg.png" decoding="async" width="10" height="10" class="mw-file-element" srcset="/upwiki/wikipedia/en/thumb/8/8a/OOjs_UI_icon_edit-ltr-progressive.svg/15px-OOjs_UI_icon_edit-ltr-progressive.svg.png 1.5x, /upwiki/wikipedia/en/thumb/8/8a/OOjs_UI_icon_edit-ltr-progressive.svg/20px-OOjs_UI_icon_edit-ltr-progressive.svg.png 2x" data-file-width="20" data-file-height="20" /></a></span></div></th></tr><tr><th scope="row" class="navbox-group" style="width:1%">International</th><td class="navbox-list-with-group navbox-list navbox-odd" style="width:100%;padding:0"><div style="padding:0 0.25em">
<ul><li><span class="uid"><a rel="nofollow" class="external text" href="http://id.worldcat.org/fast/1721124/">FAST</a></span></li></ul>
</div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">National</th><td class="navbox-list-with-group navbox-list navbox-even" style="width:100%;padding:0"><div style="padding:0 0.25em">
<ul><li><span class="uid"><a rel="nofollow" class="external text" href="https://d-nb.info/gnd/4144045-6">Germany</a></span></li>
<li><span class="uid"><a rel="nofollow" class="external text" href="http://olduli.nli.org.il/F/?func=find-b&local_base=NLX10&find_code=UID&request=987007283147605171">Israel</a></span></li>
<li><span class="uid"><a rel="nofollow" class="external text" href="https://id.loc.gov/authorities/sh85011860">United States</a></span></li></ul>
</div></td></tr></tbody></table></div></div>' |
Whether or not the change was made through a Tor exit node (tor_exit_node) | false |
Unix timestamp of change (timestamp) | '1715120103' |