Hypoiodous acid
(Redirected from Hypoiodite)
| |||
Names | |||
---|---|---|---|
IUPAC name
Hypoiodous acid
| |||
Identifiers | |||
3D model (JSmol)
|
|||
ChEBI | |||
ChemSpider | |||
PubChem CID
|
|||
UNII | |||
CompTox Dashboard (EPA)
|
|||
| |||
| |||
Properties | |||
HOI | |||
Molar mass | 143.911 g·mol−1 | ||
Acidity (pKa) | 10.5 (in water, estimate)[1] | ||
Conjugate base | Hypoiodite | ||
Related compounds | |||
Related compounds
|
|||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|
Hypoiodous acid is an inorganic compound with the chemical formula HOI.It forms when an aqueous solution of iodine is treated with mercuric or silver salts. It rapidly decomposes by disproportionation:[2]
- 5 HIO → HIO3 + 2 I2 + 2 H2O
Hypoiodites of alkali and alkaline earth metals can be made in cold dilute solutions if iodine is added to their respective hydroxides. Hypoiodous acid is a weak acid with a pKa of about 11. The conjugate base is hypoiodite (IO−). Salts of this anion can be prepared by treating I2 with alkali hydroxides. They rapidly disproportionate to form iodides and iodates.[2]
References[edit]
- ^ Perrin, D. D., ed. (1982) [1969]. Ionisation Constants of Inorganic Acids and Bases in Aqueous Solution. IUPAC Chemical Data (2nd ed.). Oxford: Pergamon (published 1984). Entry 119. ISBN 0-08-029214-3. LCCN 82-16524.
- ^ a b Holleman, A.F. (2001). Wiberg, Nils (ed.). Inorganic chemistry (1st English ed.). San Diego, Calif. : Berlin: Academic Press, W. de Gruyter. ISBN 0-12-352651-5.