Sodium percarbonate
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Sodium percarbonate or sodium carbonate peroxide is an inorganic compound with the formula Template:Chem2. It is an adduct of sodium carbonate ("soda ash" or "washing soda") and hydrogen peroxide (that is, a perhydrate). It is a colorless, crystalline, hygroscopic, and water-soluble solid.[1] 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.[1]
History
Sodium percarbonate was first prepared in 1899 by Ukrainian chemist Sebastian Moiseevich Tanatar (7 October 1849 – 30 November 1917).[2]
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.[3]
Chemistry
Dissolved in water, sodium percarbonate yields a mixture of hydrogen peroxide, sodium cations (Template:Chem), and carbonate (Template:Chem).[1][4]
Production
Sodium percarbonate is produced industrially by crystallization of a solution of sodium carbonate and hydrogen peroxide, with attention to the pH and concentrations.[5][3][6] This method is also convenient for the laboratory preparation. Alternatively, dry sodium carbonate may be treated directly with concentrated hydrogen peroxide solution.[7]
World production capacity of this compound was estimated at several hundred thousand tons for 2004.[8]
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,[1] and Vanish.[4]
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._MoreBeer-9|[9]
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.[10] 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.[11][12]
References
External links
- Organic Chemistry Portal: Sodium percarbonate
- Consumer Product Information Database: Sodium percarbonate
- ↑ a b c d Script error: No such module "citation/CS1".
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- ↑ a b Script error: No such module "Citation/CS1".
- ↑ a b "Template:Usurped", 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. Script error: No such module "doi".
- ↑ 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
- ↑ Template:Ullmann
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