Chlorous acid is an inorganic compound with the formula HClO2. It is a 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):
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| IUPAC name
Chlorous acid, Chloric (III) acid
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CompTox Dashboard (EPA)
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| Properties | |
| H Cl O2 | |
| Molar mass | 68.46 g/mol |
| Acidity (pKa) | 1.96 |
| Conjugate base | 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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- 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
editHClO2 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
editChlorous acid is a powerful oxidizing agent, although its tendency to undergo disproportionation counteracts its oxidizing potential.[citation needed]
Chlorine is the only halogen to form an isolable acid of formula HXO2.[1] Fluorine is resistant to oxidation, having a -1 oxidation state even in hypofluorous acid, and is thus unable to form any higher oxoacids; despite the name, fluorite minerals are chemically fluoride compounds. Neither bromous acid nor iodous acid has ever been isolated. A few salts of bromous acid, bromites, are known, but no iodites.[1]
References
edit- ^ a b Egon Wiberg, Arnold Frederick Holleman (2001) Inorganic Chemistry, Elsevier ISBN 0-12-352651-5
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