Bromous acid

Bromous acid
IUPAC name hydroxy-λ3-bromanone hydroxidooxidobromine bromous acid
Identifiers
PubChem	165616
ChemSpider	145144 Y
ChEBI	CHEBI:29247 Y
Jmol-3D images	Image 1
SMILES O=BrO
InChI InChI=1S/BrHO2/c2-1-3/h(H,2,3) Y Key: DKSMCEUSSQTGBK-UHFFFAOYSA-N Y InChI=1/BrHO2/c2-1-3/h(H,2,3) Key: DKSMCEUSSQTGBK-UHFFFAOYAC
Properties
Molecular formula	HBrO2
Molar mass	112.911 g/mol
Related compounds
Other anions	Hydrobromic acid; hypobromous acid; bromic acid; perbromic acid
Y (verify) (what is: Y/N?) Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Infobox references

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.

Chemistry

Bromous acid can be produced by classical chemical or electrochemicals method via anodic oxidation.^{[citation needed]}

HBrO + HClO → HBrO₂ + HCl

Also disproportioning of hypobromous acid will give bromous acid and hydrobromic acid.^{[citation needed]}

2 HBrO → HBrO₂ + HBr

Lastly, a synproportion reaction of bromic acid and hydrobromic acid gives bromous acid.^{[citation needed]}

2 HBrO₃ + HBr → 3 HBrO₂

Compounds

Several bromites are stable and have been isolated. For example NaBrO₂· 3H₂O and Ba(BrO₂)₂·H₂O.

Use

Bromites can be used for the reduction of permanganates to manganates.

2MnO−
4 + BrO−
2 + OH⁻ → 2MnO2−
4 + BrO−
3 + H₂O