Bromous acid

Bromous acid
Names
	IUPAC names hydroxy-λ3-bromanone; hydroxidooxidobromine; bromous acid
Identifiers
3D model (JSmol)	Interactive image;
ChemSpider	145144 ;
PubChem CID	165616;
CompTox Dashboard (EPA)	DTXSID80276549 ;
	InChI InChI=1S/BrHO2/c2-1-3/h(H,2,3) Key: DKSMCEUSSQTGBK-UHFFFAOYSA-N ; InChI=1/BrHO2/c2-1-3/h(H,2,3) Key: DKSMCEUSSQTGBK-UHFFFAOYAC;
	SMILES O=BrO;
Properties
Chemical formula	HBrO2
Molar mass	112.911 g/mol
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). verify (what is ?) Infobox references

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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.^[1]

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.^[1]

Use

Bromites can be used for the reduction of permanganates to manganates.^[1]

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

References

^ ^a ^b ^c Egon Wiberg, Arnold Frederick Holleman (2001) Inorganic Chemistry, Elsevier ISBN 0-12-352651-5

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[Wiberg&Holleman-1] Egon Wiberg, Arnold Frederick Holleman (2001) Inorganic Chemistry, Elsevier ISBN 0-12-352651-5

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