|Jmol-3D images||Image 1|
|Molar mass||112.911 g/mol|
|Other anions||Hydrobromic acid; hypobromous acid; bromic acid; perbromic acid|
|Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)|
|(what is: / ?)|
Bromous acid is an acid with the formula HBrO2. It has bromine in the +3 oxidation state. The salts of bromous acid are called bromites. The acid is not stable and only occurs as an intermediate; for example, in the oxidation of hypobromites.
- HBrO + HClO → HBrO2 + HCl
- 2 HBrO → HBrO2 + HBr
Lastly, a synproportion reaction of bromic acid and hydrobromic acid gives bromous acid.
- 2 HBrO3 + HBr → 3 HBrO2
Several bromites are stable and have been isolated. For example NaBrO2· 3H2O and Ba(BrO2)2·H2O.
4 + BrO−
2 + OH− → 2MnO2−
4 + BrO−
3 + H2O
- Egon Wiberg, Arnold Frederick Holleman (2001) Inorganic Chemistry, Elsevier ISBN 0-12-352651-5
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