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Bromous acid with the formula HBrO2 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.
Bromous acid can be produced by classical chemical or electrochemicals method via anodic oxidation.[citation needed]
Also disproportioning of hypobromous acid will give bromous acid and hydrobromic acid.[citation needed]
Lastly, a synproportion reaction of bromic acid and hydrobromic acid gives bromous acid.[citation needed]
Several bromites are stable and have been isolated. For example NaBrO2· 3H2O and Ba(BrO2)2·H2O.
Bromites can be used for the reduction of permanganates to manganates.
This page contains text from Wikipedia, the Free Encyclopedia -
http://en.wikipedia.org/wiki/Bromous_acid
This article is licensed under the Creative Commons Attribution-ShareAlike 3.0 Unported License, which means that you can copy and modify it as long as the entire work (including additions) remains under this license.
This article is licensed under the Creative Commons Attribution-ShareAlike 3.0 Unported License, which means that you can copy and modify it as long as the entire work (including additions) remains under this license.
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