Sodium percarbonate: Difference between revisions
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==History== |
==History== |
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Sodium percarbonate was first prepared in 1899 by [[Russian Empire|Russian]] chemist [[Sebastian Moiseevich Tanatar]] (7 October 1849 – 30 November 1917).<ref>{{cite journal |last1=Tanatar |first1=S. |title=Percarbonate |journal=Berichte der Deutschen |
Sodium percarbonate was first prepared in 1899 by [[Russian Empire|Russian]] 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> |
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==Structure== |
==Structure== |
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Revision as of 08:03, 12 December 2021
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| Names | |
|---|---|
| IUPAC name
sodium carbonate—hydrogen peroxide (2/3)
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| Other names
sodium carbonate sesquiperhydrate, PCS, SPC, solid hydrogen peroxide, Sodium carbonate hydrogen peroxide, sodium carbonate peroxyhydrate, sodium carbonate peroxide[1]
| |
| Identifiers | |
3D model (JSmol)
|
|
| ChemSpider | |
| ECHA InfoCard | 100.036.082 |
| EC Number |
|
PubChem CID
|
|
| RTECS number |
|
| UNII | |
CompTox Dashboard (EPA)
|
|
| |
| |
| 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
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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).
| |
Sodium percarbonate is a chemical substance with formula Na
2H
3CO
6. 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 Na
2CO
3 · 3 H
2O
2. It is a colorless, crystalline, hygroscopic and water-soluble solid.[2] 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.
History
Sodium percarbonate was first prepared in 1899 by Russian chemist Sebastian Moiseevich Tanatar (7 October 1849 – 30 November 1917).[3]
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 °C.[4]
Chemistry
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.[2][5]
Production
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][4][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]
- C
2H
5OH + Na
2O
2 → O:NaOH + C
2H
5ONa.
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
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,[2] and Vanish.[5]
Many commercial products mix a percentage of sodium percarbonate with sodium carbonate. The average percentage of an "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. [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
- ^ "Substance Name: Sodium carbonate peroxide". Retrieved 2021-09-09.
{{cite web}}: CS1 maint: url-status (link) - ^ a b c Craig W. Jones (1999). Applications of hydrogen peroxide and its 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 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.
- ^ 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.