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I'm fairly certain that, based on the formula Na2H3CO6, and based on the caption for the crystal structure in the article, the formula should be Na2CO3 1.5H2O2 instead of Na2CO3 3H2O2.
Tag: Reverted
Template changed to chem2, simpler code.
 
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{{Other uses|Sodium peroxycarbonate}}
{{Other uses|Sodium peroxycarbonate}}
{{chembox
{{chembox
| Verifiedfields = changed
| Watchedfields = changed
| verifiedrevid = 464402772
| Name =
| Name =
| ImageFile =
| ImageFile = Sodium-percarbonate-xtal-100K-2x2x2-3D-bs-17.png
| ImageCaption = Crystal structure at 100 K <ref name="prit1"/>
| ImageFile1 =
| ImageFile1 =
| ImageSize1 = 250px
| ImageSize1 =
| ImageFile2 = Sodium-percarbonate-xtal-100K-2003-CM-3D-balls.png
| ImageFile2 =
| ImageSize2 = 300px
| ImageSize2 = 300px
| IUPACName = sodium carbonate—hydrogen peroxide (2/3)
| IUPACName = sodium carbonate—hydrogen peroxide (2/3)
| SystematicName =
| SystematicName =
| OtherNames = sodium carbonate sesquiperhydrate, PCS, SPC, solid hydrogen peroxide, Sodium carbonate hydrogen peroxide, sodium carbonate peroxyhydrate
| OtherNames = Sodium carbonate peroxide,<ref>{{cite web|title=Substance Name: Sodium carbonate peroxide|url=https://chem.nlm.nih.gov/chemidplus/rn/15630-89-4|access-date=2021-09-09}}</ref> sodium carbonate sesquiperhydrate, PCS, SPC, solid hydrogen peroxide, Sodium carbonate hydrogen peroxide, sodium carbonate peroxyhydrate
| Section1 = {{Chembox Identifiers
| Section1 = {{Chembox Identifiers
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
Line 27: Line 25:
| CASNo_Ref = {{cascite|correct|CAS}}
| CASNo_Ref = {{cascite|correct|CAS}}
| EINECS = 239-707-6
| EINECS = 239-707-6
| UNII_Ref = {{fdacite|changed|FDA}}
| UNII_Ref = {{fdacite|correct|FDA}}
| UNII = Z7G82NV92P
| UNII = Z7G82NV92P
| UNNumber = 3378
| PubChem = 159762
| PubChem = 159762
| RTECS = FG0750000
| RTECS = FG0750000
}}
}}
| Section2 = {{Chembox Properties
| Section2 = {{Chembox Properties
| Formula = Na<sub>2</sub>CO<sub>3</sub><nowiki>&middot;</nowiki>1.5 H<sub>2</sub>O<sub>2</sub>
| Formula = Na<sub>2</sub>CO<sub>3</sub><nowiki>·</nowiki>1.5 H<sub>2</sub>O<sub>2</sub>
| MolarMass = 156.982 g/mol
| MolarMass = 156.982 g/mol
| Appearance = white solid
| Appearance = White solid
| Density =
| Density =
| MeltingPt =
| MeltingPt =
| BoilingPt =
| BoilingPt =
| Solubility = 150 g/l
| Solubility = 150 g/l
| SolubleOther =
| SolubleOther =
| Solvent =
| Solvent =
| pKb =
| pKb =
}}
}}
| Section3 =
| Section3 =
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| Section7 = {{Chembox Hazards
| Section7 = {{Chembox Hazards
| ExternalSDS =
| ExternalSDS =
⚫
| MainHazards = Irritant, oxidizer
| EUClass =
| NFPA-H =
⚫
| MainHazards = Irritant, Oxidizer
| NFPA-H =
| NFPA-F =
| NFPA-F =
| NFPA-R =
| NFPA-R =
| NFPA-S =
| NFPA-S =
| HPhrases =
| RPhrases =
| PPhrases =
| SPhrases =
| GHS_ref =
| FlashPt = Non-flammable
| FlashPt = Non-flammable
| PEL =
| PEL =
}}
}}
| Section8 = {{Chembox Related
| Section8 = {{Chembox Related
| OtherAnions = [[Sodium carbonate]]<br/>[[Sodium bicarbonate]]
| OtherAnions = [[Sodium carbonate]]<br />[[Sodium bicarbonate]]
| OtherCations = [[Calcium percarbonate]]<br/>[[Magnesium percarbonate]]
| OtherCations = [[Calcium percarbonate]]<br />[[Magnesium percarbonate]]
| OtherFunction =
| OtherFunction =
| OtherFunction_label =
| OtherFunction_label =
| OtherCompounds = [[Sodium perborate]]<br/>[[Sodium persulfate]]<br/>[[Sodium perphosphate]]
| OtherCompounds = [[Sodium perborate]]<br />[[Sodium persulfate]]<br />[[Sodium perphosphate]]
}}
}}
}}
}}


'''Sodium percarbonate''' is a [[chemical substance]] with formula {{chem|Na|2|H|3|CO|6}}. It is an [[adduct]] of [[sodium carbonate]] ("soda ash" or "washing soda") and [[hydrogen peroxide]] (that is, a [[wikt:perhydrate|perhydrate]]) whose formula is more properly written as 2&nbsp;{{chem|Na|2|CO|3}}&nbsp;·&nbsp;1.5&nbsp;{{chem|H|2|O|2}}. It is a colorless, crystalline, [[hygroscopic]] and water-soluble solid.<ref name = "Jones">{{cite book | author = Craig W. Jones | title = Applications of hydrogen peroxide and its derivatives | year = 1999 | publisher = [[Royal Society of Chemistry]] | isbn = 0-85404-536-8}}</ref> It is sometimes abbreviated as '''SPC'''. It contains 32.5% by weight of hydrogen peroxide.
'''Sodium percarbonate''' or '''sodium carbonate peroxide''' is a [[chemical substance]] with formula {{chem2|Na2H3CO6}}. It is an [[adduct]] of [[sodium carbonate]] ("soda ash" or "washing soda") and [[hydrogen peroxide]] (that is, a [[wikt:perhydrate|perhydrate]]) whose formula is more properly written as {{chem2|2 Na2CO3 * 3 H2O2}}. It is a colorless, crystalline, [[hygroscopic]] and water-soluble solid.<ref name = "Jones">{{cite book | author = Craig W. Jones | title = Applications of hydrogen peroxide and derivatives | year = 1999 | publisher = [[Royal Society of Chemistry]] | isbn = 0-85404-536-8}}</ref> It is sometimes abbreviated as '''SPC'''. It contains 32.5% by weight of hydrogen peroxide.


The product is used in some [[eco-friendly]] [[bleach]]es and other [[cleaning product]]s.
The product is used in some [[eco-friendly]] [[bleach]]es and other [[cleaning product]]s.<ref name = "Jones"/>


==History==
==History==
Sodium percarbonate was first prepared in 1899 by [[Russian Empire|Russian]] chemist [[Sebastian Moiseevich Tanatar]] (7 October 1849 – 30 November 1917).<ref>S. Tanatar (1899) [http://gallica.bnf.fr/ark:/12148/bpt6k90753b/f193.image.langEN "Percarbonate"], ''Berichte der Deutschen chemischen Gesellschaft zu Berlin'', '''32''' : 1544–1546.</ref>
Sodium percarbonate was first prepared in 1899 by [[Russian Empire|Ukrainian]] chemist [[Sebastian Moiseevich Tanatar]] (7 October 1849 – 30 November 1917).<ref>{{cite journal |last1=Tanatar |first1=S. |title=Percarbonate |journal=Berichte der Deutschen Chemischen Gesellschaft zu Berlin |date=1899 |volume=32 |issue=2 |pages=1544–1546 |doi=10.1002/cber.18990320233 |url=https://babel.hathitrust.org/cgi/pt?id=hvd.cl1i1w&view=1up&seq=198&skin=2021 |language=German}}</ref>


==Structure==
==Structure==
At room temperature, solid sodium percarbonate has the [[orthorhombic]] [[crystal structure]], with the ''Cmca'' crystallographic [[space group]]. The structure changes to ''Pbca'' as the crystals are cooled below about −30&nbsp;°C.<ref name="prit1">
At room temperature, solid sodium percarbonate has the [[orthorhombic]] [[crystal structure]], with the ''Cmca'' crystallographic [[space group]]. The structure changes to ''Pbca'' as the crystals are cooled below about −30&nbsp;°C.<ref name="prit1">
{{cite journal
{{cite journal
| title = Sodium percarbonate between 293 and 100 K
| title = Sodium percarbonate between 293 and 100 K
|author1=R. G. Pritchard |author2=E. Islam
| author1=R. G. Pritchard
| author2=E. Islam
|name-list-style=amp | journal = [[Acta Crystallographica Section B]]
| name-list-style=amp
| journal = [[Acta Crystallographica Section B]]
| volume = B59
| volume = B59
| issue = 5
| issue = 5
| pages = 596–605
| pages = 596–605
| year = 2003
| year = 2003
| url =
| url =
| doi = 10.1107/S0108768103012291 |pmid=14586079 }}
| doi = 10.1107/S0108768103012291
| pmid=14586079
</ref>
}}</ref>


==Chemistry==
==Chemistry==
Dissolved in water, sodium percarbonate yields a mixture of hydrogen peroxide (which eventually decomposes to water and [[oxygen]]), [[sodium]] [[cation]]s {{chem|Na|+}}, and [[carbonate]] {{chem|CO|3|2-}}.<ref name = "Jones"/><ref name="rscvanish" />
Dissolved in water, sodium percarbonate yields a mixture of hydrogen peroxide (which eventually decomposes to water and [[oxygen]]), [[sodium]] [[cation]]s ({{chem|Na|+}}), and [[carbonate]] ({{chem|CO|3|2-}}).<ref name = "Jones"/><ref name="rscvanish" />


: <chem> 2Na2CO3*3H2O2 -> 3H2O2 + 4Na+ + 2CO3^2- </chem>
:{{chem2|2 Na2CO3 * 3 H2O2 -> 3 H2O2 + 4 Na+ + 2 CO3(2-)}}
:{{chem2|2 H2O2 -> 2 H2O + O2}}

: <chem> 2H2O2 -> 2H2O + O2 </chem>


==Production==
==Production==
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Alternatively, dry sodium carbonate may be treated directly with concentrated hydrogen peroxide solution.<ref name=kimpat>Sang Ryul Kim, Chong Yun Kwag, Hwan Kee Heo, Jong-Pill Lee (1996): "[https://patents.google.com/patent/US5851420 Process for manufacturing granular sodium percarbonate]". US Patent US5851420A, priority date 1996-02-29</ref>
Alternatively, dry sodium carbonate may be treated directly with concentrated hydrogen peroxide solution.<ref name=kimpat>Sang Ryul Kim, Chong Yun Kwag, Hwan Kee Heo, Jong-Pill Lee (1996): "[https://patents.google.com/patent/US5851420 Process for manufacturing granular sodium percarbonate]". US Patent US5851420A, priority date 1996-02-29</ref>


It may also be formed from a process starting from sodium peroxide When absolute ethyl alcohol reacts with sodium peroxide at 0° C. a perhydroxide is produced.
It may also be formed from a process starting from sodium peroxide; when absolute ethyl alcohol reacts with sodium peroxide at 0{{nbsp}}°C, a perhydroxide is produced.{{citation needed|date=September 2021}}


C2H5OH + Na2O2 - O:NaOH + C2H5ONa.
:{{chem2|C2H5OH + Na2O2 -> O:NaOH + C2H5ONa}}


Carbon dioxide converts it into sodium hydrogen percarbonate.
Carbon dioxide converts it into sodium hydrogen percarbonate.
Line 112: Line 113:


==Uses==
==Uses==
As an [[oxidizing agent]], sodium percarbonate is an ingredient in a number of home and [[laundry detergent|laundry cleaning]] products, including non-chlorine [[bleach]] products such as [[Oxyper]], [[OxiClean]], [[Tide (detergent)|Tide laundry detergent]],<ref name = "Jones"/> and [[Vanish (stain remover)|Vanish]].<ref name="rscvanish">"[http://www.chemistryinyourcupboard.org/vanish/4 Oxygen-based bleaches] {{webarchive|url=https://web.archive.org/web/20120124185550/http://www.chemistryinyourcupboard.org/vanish/4 |date=2012-01-24 }}", The [[Royal Society of Chemistry]], and [[Reckitt Benckiser]] (the manufacturers of Vanish).</ref>
As an [[oxidizing agent]], sodium percarbonate is an ingredient in a number of home and [[laundry detergent|laundry cleaning]] products, including non-chlorine [[bleach]] products such as [[Oxyper]], [[OxiClean]], [[Tide (detergent)|Tide laundry detergent]],<ref name = "Jones"/> and [[Vanish (stain remover)|Vanish]].<ref name="rscvanish">"[http://www.chemistryinyourcupboard.org/vanish/4 Oxygen-based bleaches] {{webarchive|url=https://web.archive.org/web/20120124185550/http://www.chemistryinyourcupboard.org/vanish/4 |date=2012-01-24 }}", The [[Royal Society of Chemistry]], and [[Reckitt Benckiser]] (the manufacturers of Vanish).</ref>


Many commercial products mix a percentage of sodium percarbonate with sodium carbonate. The average percentage of an "Oxy" product in the supermarket is 65% sodium percarbonate and 35% sodium carbonate. The "ultra boosters" seen on infomercials may contain as much as 80% sodium percarbonate. However, sodium percarbonate is less expensive in its pure form {{citation needed|date=May 2017}} and can be adjusted to any percentage the user desires.
Many commercial products mix a percentage of sodium percarbonate with sodium carbonate. The average "Oxy" product in the supermarket contains 35–40% sodium percarbonate with about 5% active oxygen when titrated.


Sodium percarbonate is also used as a cleaning agent by many home brewers. <ref name="Sodium Percarbonate | MoreBeer">{{cite web |title=Sodium Percarbonate |url=https://www.morebeer.com/products/sodium-percarbonate.html |website=MoreBeer.com |accessdate=26 June 2020}}</ref>
Sodium percarbonate is also used as a cleaning agent in [[homebrewing]].<ref name="Sodium Percarbonate | MoreBeer">{{cite web |title=Sodium Percarbonate |url=https://www.morebeer.com/products/sodium-percarbonate.html |website=MoreBeer.com |accessdate=26 June 2020}}</ref>


Sodium percarbonate can be used in [[organic synthesis]] as a convenient source of anhydrous H<sub>2</sub>O<sub>2</sub>, in particular in solvents that cannot dissolve the carbonate but can leach the H<sub>2</sub>O<sub>2</sub> out of it.<ref name="mckill">{{cite journal | last1 = McKillop | first1 = A | title = Sodium perborate and sodium percarbonate: Cheap, safe and versatile oxidising agents for organic synthesis | journal = Tetrahedron | volume = 51 | pages = 6145–6166 | year = 1995 | doi = 10.1016/0040-4020(95)00304-Q | issue = 22}}</ref> A method for generating [[trifluoroperacetic acid]] ''in situ'' for use in [[Baeyer–Villiger oxidation]]s from sodium percarbonate and [[trifluoroacetic anhydride]] has been reported; it provides a convenient and cheap approach to this reagent without the need to obtain highly concentrated hydrogen peroxide.<ref>{{cite journal|title = New Method of Generating Trifluoroperoxyacetic acid for the Baeyer-Villiger Reaction|first1 = Ho-Jung|last1 = Kang|first2 = Hee-Sun|last2 = Jeong|journal = [[Bull. Korean Chem. Soc.]]|volume = 17|issue = 1|year = 1996|pages = 5–6|url = http://journal.kcsnet.or.kr/main/j_search/j_download.htm?code=B960104}}</ref><ref>{{cite encyclopedia|doi = 10.1002/047084289X.rt254.pub2|encyclopedia = [[Encyclopedia of Reagents for Organic Synthesis|e-EROS Encyclopedia of Reagents for Organic Synthesis]]|chapter = Trifluoroperacetic Acid|first1 = Kenneth C.|title = Encyclopedia of Reagents for Organic Synthesis|last1 = Caster|first2 = A. Somasekar|last2 = Rao|first3 = H. Rama|last3 = Mohan|first4 = Nicholas A.|last4 = McGrath|first5 = Matthew|last5 = Brichacek|year = 2012|isbn = 978-0471936237}}</ref>
Sodium percarbonate can be used in [[organic synthesis]] as a convenient source of anhydrous H<sub>2</sub>O<sub>2</sub>, in particular in solvents that cannot dissolve the carbonate but can leach the H<sub>2</sub>O<sub>2</sub> out of it.<ref name="mckill">{{cite journal | last1 = McKillop | first1 = A | title = Sodium perborate and sodium percarbonate: Cheap, safe and versatile oxidising agents for organic synthesis | journal = Tetrahedron | volume = 51 | pages = 6145–6166 | year = 1995 | doi = 10.1016/0040-4020(95)00304-Q | issue = 22}}</ref> A method for generating [[trifluoroperacetic acid]] ''in situ'' for use in [[Baeyer–Villiger oxidation]]s from sodium percarbonate and [[trifluoroacetic anhydride]] has been reported; it provides a convenient and cheap approach to this reagent without the need to obtain highly concentrated hydrogen peroxide.<ref>{{cite journal|title = New Method of Generating Trifluoroperoxyacetic acid for the Baeyer-Villiger Reaction|first1 = Ho-Jung|last1 = Kang|first2 = Hee-Sun|last2 = Jeong|journal = [[Bull. Korean Chem. Soc.]]|volume = 17|issue = 1|year = 1996|pages = 5–6|url = http://journal.kcsnet.or.kr/main/j_search/j_abstract_view.htm?code=B960104&cpage=3&qpage=j_search&spage=j_search&journal=B&vol=17&no=1&page=&year1=1990&year2=1999&view=10&qpage=j_search&abstract=}}</ref><ref>{{cite encyclopedia|doi = 10.1002/047084289X.rt254.pub2|encyclopedia = [[Encyclopedia of Reagents for Organic Synthesis|e-EROS Encyclopedia of Reagents for Organic Synthesis]]|chapter = Trifluoroperacetic Acid|first1 = Kenneth C.|title = Encyclopedia of Reagents for Organic Synthesis|last1 = Caster|first2 = A. Somasekar|last2 = Rao|first3 = H. Rama|last3 = Mohan|first4 = Nicholas A.|last4 = McGrath|first5 = Matthew|last5 = Brichacek|year = 2012|isbn = 978-0471936237}}</ref>


==References==
==References==
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* [https://www.organic-chemistry.org/chemicals/oxidations/sodiumpercarbonate.shtm Organic Chemistry Portal: Sodium percarbonate]
* [https://www.organic-chemistry.org/chemicals/oxidations/sodiumpercarbonate.shtm Organic Chemistry Portal: Sodium percarbonate]
* [https://www.whatsinproducts.com/chemicals/view/1/3259/003313-92-6/Sodium%20percarbonate Consumer Product Information Database: Sodium percarbonate]
* [https://www.whatsinproducts.com/chemicals/view/1/3259/003313-92-6/Sodium%20percarbonate Consumer Product Information Database: Sodium percarbonate]
* [https://belchem.com/Sodium-Percarbonate.php Sodium percarbonate]
{{sodium compounds}}
{{sodium compounds}}


Latest revision as of 07:41, 9 September 2024

For other uses, see Sodium peroxycarbonate.
Sodium percarbonate

Crystal structure at 100 K [1]
Names
IUPAC name
sodium carbonate—hydrogen peroxide (2/3)
Other names
Sodium carbonate peroxide,[2] sodium carbonate sesquiperhydrate, PCS, SPC, solid hydrogen peroxide, Sodium carbonate hydrogen peroxide, sodium carbonate peroxyhydrate
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.036.082 Edit this at Wikidata
EC Number
  • 239-707-6
RTECS number
  • FG0750000
UNII
UN number 3378
  • InChI=1S/CH2O4.Na/c2-1(3)5-4;/h4H,(H,2,3);/q;+1/p-1 checkY
    Key: MWNQXXOSWHCCOZ-UHFFFAOYSA-M checkY
  • InChI=1S/CH2O4.Na/c2-1(3)5-4;/h4H,(H,2,3);/q;+1/p-1
    Key: MWNQXXOSWHCCOZ-REWHXWOFAO
  • Key: MWNQXXOSWHCCOZ-UHFFFAOYSA-M
  • [Na+].[O-]C(=O)OO
Properties
Na2CO3·1.5 H2O2
Molar mass 156.982 g/mol
Appearance White solid
150 g/l
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 Irritant, oxidizer
Flash point Non-flammable
Related compounds
Other anions
 Sodium carbonate
Sodium bicarbonate
Other cations
 Calcium percarbonate
Magnesium percarbonate
Related compounds
 Sodium perborate
Sodium persulfate
Sodium perphosphate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Sodium percarbonate or sodium carbonate peroxide is a chemical substance with formula Na2H3CO6. It is an adduct of sodium carbonate ("soda ash" or "washing soda") and hydrogen peroxide (that is, a perhydrate) whose formula is more properly written as 2 Na2CO3 · 3 H2O2. It is a colorless, crystalline, hygroscopic and water-soluble solid.[3] It is sometimes abbreviated as SPC. It contains 32.5% by weight of hydrogen peroxide.

The product is used in some eco-friendly bleaches and other cleaning products.[3]

History

[edit]

Sodium percarbonate was first prepared in 1899 by Ukrainian chemist Sebastian Moiseevich Tanatar (7 October 1849 – 30 November 1917).[4]

Structure

[edit]

At room temperature, solid sodium percarbonate has the orthorhombic crystal structure, with the Cmca crystallographic space group. The structure changes to Pbca as the crystals are cooled below about −30 °C.[1]

Chemistry

[edit]

Dissolved in water, sodium percarbonate yields a mixture of hydrogen peroxide (which eventually decomposes to water and oxygen), sodium cations (Na+
), and carbonate (CO2−
3).[3][5]

2 Na2CO3 · 3 H2O2 → 3 H2O2 + 4 Na+ + 2 CO2−3
2 H2O2 → 2 H2O + O2

Production

[edit]

Sodium percarbonate is produced industrially by crystallization of a solution of sodium carbonate and hydrogen peroxide, with proper control of the pH and concentrations.[6][1][7] This is also a convenient laboratory method.

Alternatively, dry sodium carbonate may be treated directly with concentrated hydrogen peroxide solution.[8]

It may also be formed from a process starting from sodium peroxide; when absolute ethyl alcohol reacts with sodium peroxide at 0 °C, a perhydroxide is produced.[citation needed]

C2H5OH + Na2O2 → O:NaOH + C2H5ONa

Carbon dioxide converts it into sodium hydrogen percarbonate.

World production capacity of this compound was estimated at several hundred thousand tons for 2004.[9]

Uses

[edit]

As an oxidizing agent, sodium percarbonate is an ingredient in a number of home and laundry cleaning products, including non-chlorine bleach products such as Oxyper, OxiClean, Tide laundry detergent,[3] and Vanish.[5]

Many commercial products mix a percentage of sodium percarbonate with sodium carbonate. The average "Oxy" product in the supermarket contains 35–40% sodium percarbonate with about 5% active oxygen when titrated.

Sodium percarbonate is also used as a cleaning agent in homebrewing.[10]

Sodium percarbonate can be used in organic synthesis as a convenient source of anhydrous H2O2, in particular in solvents that cannot dissolve the carbonate but can leach the H2O2 out of it.[11] A method for generating trifluoroperacetic acid in situ for use in Baeyer–Villiger oxidations from sodium percarbonate and trifluoroacetic anhydride has been reported; it provides a convenient and cheap approach to this reagent without the need to obtain highly concentrated hydrogen peroxide.[12][13]

References

[edit]
  1. ^ a b c R. G. Pritchard & E. Islam (2003). "Sodium percarbonate between 293 and 100 K". Acta Crystallographica Section B. B59 (5): 596–605. doi:10.1107/S0108768103012291. PMID 14586079.
  2. ^ "Substance Name: Sodium carbonate peroxide". Retrieved 2021-09-09.
  3. ^ a b c d Craig W. Jones (1999). Applications of hydrogen peroxide and derivatives. Royal Society of Chemistry. ISBN 0-85404-536-8.
  4. ^ Tanatar, S. (1899). "Percarbonate". Berichte der Deutschen Chemischen Gesellschaft zu Berlin (in German). 32 (2): 1544–1546. doi:10.1002/cber.18990320233.
  5. ^ a b "Oxygen-based bleaches Archived 2012-01-24 at the Wayback Machine", The Royal Society of Chemistry, and Reckitt Benckiser (the manufacturers of Vanish).
  6. ^ J. M. Adams and R. G. Pritchard (1977): "The crystal structure of sodium percarbonate: an unusual layered solid". Acta Crystallographica Section B, volume B33, issue 12, pages 3650–3653. doi:10.1107/S0567740877011790
  7. ^ Alun P. James, Graham R. Horne, Richard Roesler, and others (1997): "Process for producing sodium percarbonate". US Patent US6231828B1, priority date 1997-03-26.
  8. ^ Sang Ryul Kim, Chong Yun Kwag, Hwan Kee Heo, Jong-Pill Lee (1996): "Process for manufacturing granular sodium percarbonate". US Patent US5851420A, priority date 1996-02-29
  9. ^ Harald Jakob, Stefan Leininger, Thomas Lehmann, Sylvia Jacobi, Sven Gutewort. "Peroxo Compounds, Inorganic". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a19_177.pub2. ISBN 978-3527306732.{{cite encyclopedia}}: CS1 maint: multiple names: authors list (link)
  10. ^ "Sodium Percarbonate". MoreBeer.com. Retrieved 26 June 2020.
  11. ^ McKillop, A (1995). "Sodium perborate and sodium percarbonate: Cheap, safe and versatile oxidising agents for organic synthesis". Tetrahedron. 51 (22): 6145–6166. doi:10.1016/0040-4020(95)00304-Q.
  12. ^ Kang, Ho-Jung; Jeong, Hee-Sun (1996). "New Method of Generating Trifluoroperoxyacetic acid for the Baeyer-Villiger Reaction". Bull. Korean Chem. Soc. 17 (1): 5–6.
  13. ^ Caster, Kenneth C.; Rao, A. Somasekar; Mohan, H. Rama; McGrath, Nicholas A.; Brichacek, Matthew (2012). "Trifluoroperacetic Acid". Encyclopedia of Reagents for Organic Synthesis. e-EROS Encyclopedia of Reagents for Organic Synthesis. doi:10.1002/047084289X.rt254.pub2. ISBN 978-0471936237.
[edit]
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