|3D model (Jmol)||Interactive image|
|Molar mass||112.911 g/mol|
|Hydrobromic acid; hypobromous acid; bromic acid; perbromic acid|
Except where otherwise noted, 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
|This inorganic compound–related article is a stub. You can help Wikipedia by expanding it.|