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Sodium percarbonate

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Sodium percarbonate
Identifiers
CAS number 15630-89-4 YesY
PubChem 159762
EC number 239-707-6
Properties
Molecular formula Na2CO3·1.5H2O2
Molar mass 157.01 g/mol
Appearance white solid
Solubility in water 150 g/l
Hazards
EU Index Not listed
Main hazards Irritant, Oxidizer
Flash point Non-flammable
Related compounds
Other anions Sodium carbonate
Sodium bicarbonate
Related compounds Sodium perborate
Sodium persulfate
Sodium perphosphate
 YesY (what is this?)  (verify)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Infobox references

Sodium percarbonate is a white crystalline water-soluble adduct of sodium carbonate and hydrogen peroxide, with formula Na2CO3·1.5H2O2.[1] Despite the name, it is, in fact, a carbonate perhydrate.[1]; it should not be confused with sodium peroxocarbonate Na2CO4 or peroxodicarbonate Na2C2O6.

Sodium percarbonate is an oxidizing agent and ingredient in a number of home and laundry cleaning products, including eco-friendly bleach products such as OxiClean. [1] Dissolved in water, it releases hydrogen peroxide and soda ash (sodium carbonate):[1]

2(Na2CO3·1.5H2O2) → 2 Na2CO3 + 3 H2O2

Sodium percarbonate can be used in organic synthesis as a convenient source of anhydrous H2O2, particularly in solvents that cannot dissolve the carbonate but can leach the H2O2 out of it.[2]

Contents

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[edit] Structure

Solid sodium percarbonate is a colorless, hygroscopic, crystalline solid with the orthorhombic crystal structure. The crystallographic point group is Cmca at room temperature, but changes to Pbca as the crystals are cooled below about -30 °C. [3]

[edit] Synthesis

Since sodium percarbonate is easily decomposed by water, it is produced commercially by reacting powdered anhydrous Na2CO3 with H2O2 dissolved in carbon tetrachloride CCl4.[4] It can be obtained in the laboratory by reacting the two substances in aqueous solution with proper control of the pH[4] or concentrations.[3]

[edit] References

  1. ^ a b c d Craig W. Jones Applications of hydrogen peroxide and its derivatives (1999) Royal Society of Chemistry ISBN 0854045368
  2. ^ A. McKillop, W. R. Sanderson (2000) Sodium perborate and sodium percarbonate: further applications in organic synthesis (survey article). Journal of the Chemical Society, Perkin Transactions 1, pages 471-476. doi:10.1016/0040-4020(95)00304-Q
  3. ^ a b R. G. Pritchard and E. Islam (2003). “Sodium percarbonate between 293 and 100 K”. Acta Crystallographica Section B B59: 596–605. doi:10.1107/S0108768103012291. 
  4. ^ a b J. M. Adams and R. G. Pritchard (1977). “The crystal structure of sodium percarbonate: an unusual layered solid”. Acta Crystallographica Section B B33: 3650–3653. doi:10.1107/S0567740877011790. 

[edit] External links