Chlorous acid
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| Names | |
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| IUPAC name
Chlorous acid, Chloric (III) acid
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| Identifiers | |
3D model (
JSmol ) |
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| ChEBI | |
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| KEGG | |
PubChem CID
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| UNII | |
CompTox Dashboard (EPA)
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| Properties | |
| H Cl O2 | |
| Molar mass | 68.46 g/mol |
| Acidity (pKa) | 1.96 |
Conjugate base
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Chlorite |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Chlorous acid is an
weak acid. Chlorine has oxidation state +3 in this acid. The pure substance is unstable, disproportionating to hypochlorous acid (Cl oxidation state +1) and chloric acid
(Cl oxidation state +5):
- 2 HClO2 → HClO + HClO3
Although the acid is difficult to obtain in pure substance, the conjugate base, chlorite, derived from this acid is stable. One example of a salt of this anion is the well-known sodium chlorite. This and related salts are sometimes used in the production of chlorine dioxide.
Preparation
HClO2 can be prepared through reaction of barium or lead chlorite and dilute sulfuric acid:
- Ba(ClO2)2 + H2SO4 → BaSO4 + 2 HClO2
- Pb(ClO2)2 + H2SO4 → PbSO4 + 2 HClO2
Stability
Chlorous acid is a powerful oxidizing agent, although its tendency to undergo disproportionation counteracts its oxidizing potential.[citation needed]
Chlorine is the only
iodous acid has ever been isolated. A few salts of bromous acid, bromites, are known, but no iodites.[1]
References
Media related to Chlorous acid at Wikimedia Commons
- ^ ISBN 0-12-352651-5
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