Sodium percarbonate
Crystal structure at 100 K [1]
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Names | |
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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
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Identifiers | |
3D model (
JSmol ) |
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ChemSpider | |
ECHA InfoCard
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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
The product is used in some
History
Sodium percarbonate was first prepared in 1899 by
Structure
At room temperature, solid sodium percarbonate has the
Chemistry
Dissolved in water, sodium percarbonate yields a mixture of hydrogen peroxide (which eventually decomposes to water and
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][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]
- 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
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
- ^ a b c
R. G. Pritchard & E. Islam (2003). "Sodium percarbonate between 293 and 100 K". PMID 14586079.
- ^ "Substance Name: Sodium carbonate peroxide". Retrieved 2021-09-09.
- ^ ISBN 0-85404-536-8.
- .
- ^ Reckitt Benckiser(the manufacturers of Vanish).
- ^ 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
- ISBN 978-3527306732.)
{{cite encyclopedia}}
: CS1 maint: multiple names: authors list (link - ^ "Sodium Percarbonate". MoreBeer.com. Retrieved 26 June 2020.
- .
- ^ 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.
- ISBN 978-0471936237.