Sodium percarbonate: Difference between revisions
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{{Other uses|Sodium peroxycarbonate}} |
{{Other uses|Sodium peroxycarbonate}} |
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| ImageCaption = Crystal structure at 100 K <ref name="prit1"/> |
| ImageCaption = Crystal structure at 100 K <ref name="prit1"/> |
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| IUPACName = sodium carbonate—hydrogen peroxide (2/3) |
| IUPACName = sodium carbonate—hydrogen peroxide (2/3) |
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| OtherNames = Sodium carbonate peroxide,<ref>{{ |
| 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 |
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| UNII = Z7G82NV92P |
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| UNNumber = 3378 |
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'''Sodium percarbonate |
'''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. |
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The product is used in some [[eco-friendly]] [[bleach]]es and other [[cleaning product]]s.<ref name = "Jones"/> |
The product is used in some [[eco-friendly]] [[bleach]]es and other [[cleaning product]]s.<ref name = "Jones"/> |
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==Chemistry== |
==Chemistry== |
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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" /> |
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:{{chem2|2 Na2CO3 * 3 H2O2 -> 3 H2O2 + 4 Na+ + 2 CO3(2-)}} |
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:{{chem2|2 H2O2 -> 2 H2O + O2}} |
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==Production== |
==Production== |
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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}} |
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}} |
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:{{chem2|C2H5OH + Na2O2 -> O:NaOH + C2H5ONa}} |
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Carbon dioxide converts it into sodium hydrogen percarbonate. |
Carbon dioxide converts it into sodium hydrogen percarbonate. |
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==Uses== |
==Uses== |
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As an [[oxidizing agent]], |
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> |
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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. |
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. |
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Latest revision as of 07:41, 9 September 2024
 Crystal structure at 100 K [1]
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| Names | |
|---|---|
| IUPAC name
sodium carbonate—hydrogen peroxide (2/3)
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| 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)
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| ChemSpider | |
| ECHA InfoCard | 100.036.082 |
| EC Number |
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PubChem CID
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| RTECS number |
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| UNII | |
| UN number | 3378 |
CompTox Dashboard (EPA)
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| 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
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Irritant, oxidizer |
| Flash point | Non-flammable |
| Related compounds | |
Other anions
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Sodium carbonate Sodium bicarbonate |
Other cations
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Calcium percarbonate Magnesium percarbonate |
Related compounds
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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).
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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]- ^ 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.
- ^ "Substance Name: Sodium carbonate peroxide". Retrieved 2021-09-09.
- ^ a b c d Craig W. Jones (1999). Applications of hydrogen peroxide and derivatives. Royal Society of Chemistry. ISBN 0-85404-536-8.
- ^ Tanatar, S. (1899). "Percarbonate". Berichte der Deutschen Chemischen Gesellschaft zu Berlin (in German). 32 (2): 1544–1546. doi:10.1002/cber.18990320233.
- ^ 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).
- ^ 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
- ^ Alun P. James, Graham R. Horne, Richard Roesler, and others (1997): "Process for producing sodium percarbonate". US Patent US6231828B1, priority date 1997-03-26.
- ^ 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
- ^ 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) - ^ "Sodium Percarbonate". MoreBeer.com. Retrieved 26 June 2020.
- ^ 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.
- ^ 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.
- ^ 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.