Chlorous acid
 |
|
 |
|
| Names | |
|---|---|
| IUPAC name
Chlorous acid
|
|
| Identifiers | |
13898-47-0  |
|
| ChEBI | CHEBI:29219  |
| ChemSpider | 22861 |
| Jmol 3D model | Interactive image |
| KEGG | C01486 |
| PubChem | 24453 |
|
|
|
|
| Properties | |
| HClO2 | |
| Molar mass | 68.46 g/mol |
| Acidity (pKa) | 1.96 |
|
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 | |
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):
- 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 chlorite and dilute sulfuric acid:
- Ba(ClO2)2 + H2SO4 → BaSO4 + 2HClO2
Stability
Chlorous acid is a powerful oxidizing agent, although its tendency to disproportionation counteracts its oxidizing potential.
Chlorine is the only halogen to form an isolable acid of formula HXO2.[1] Neither bromous acid nor iodous acid has ever been isolated. A few salts of bromous acid, bromites, are known, but no iodites.[1]
References
Media related to Lua error in package.lua at line 80: module 'strict' not found. at Wikimedia Commons
- ↑ 1.0 1.1 Egon Wiberg, Arnold Frederick Holleman (2001) Inorganic Chemistry, Elsevier ISBN 0-12-352651-5
<templatestyles src="Asbox/styles.css"></templatestyles>
 |
This inorganic compound–related article is a stub. You can help Wikipedia by expanding it. |
