Hypoiodous acid (original) (raw)
From Wikipedia, the free encyclopedia
Hypoiodous acid
 |
|
|---|---|
 Hydrogen, H Oxygen, O Iodine, I  |
|
| Names | |
| IUPAC name Hypoiodous acid | |
| Identifiers | |
| CAS Number | 14332-21-9  Y |
| 3D model (JSmol) | Interactive image |
| ChEBI | CHEBI:29231 Y |
| ChemSpider | 109942 Y |
| PubChem CID | 123340 |
| UNII | 2PYC923C5W Y |
| CompTox Dashboard (EPA) | DTXSID8042050  |
| InChI InChI=1S/HIO/c1-2/h2H YKey: GEOVEUCEIQCBKH-UHFFFAOYSA-N Y |
|
| SMILES IO | |
| Properties | |
| Chemical formula | HOI |
| Molar mass | 143.911 g·mol−1 |
| Acidity (p_K_a) | 10.5 (in water, estimate)[1] |
| Conjugate base | Hypoiodite |
| Related compounds | |
| Related compounds | Hypofluorous acidHypochlorous acidHypobromous acid |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).  N verify (what is Y N ?) Infobox references |
Chemical compound
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
Hypoiodous acid is a weak acid with a p_K_a 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]
Ammonium hypoiodites can be formed by oxiation of the analogous iodide salts. These and also sodium hypoiodite are useful as oxidizing agents for a various types of organic compounds.
Hypoiodite is one of the active oxidizing agents generated by lactoperoxidase as part of the mamalian innate immune system.[3]
Hypoiodous acid is part of a series of oxyacids in which iodine can assume oxidation states of −1, +1, +3, +5, or +7. A number of neutral iodine oxides are also known.
| Iodine oxidation state | −1 | +1 | +3 | +5 | +7 |
|---|---|---|---|---|---|
| Name | Hydrogen iodide | Hypoiodous acid | Iodous acid | Iodic acid | Periodic acid |
| Formula | HI | HIO | HIO2 | HIO3 | HIO4 or H5IO6 |
- ^ 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.
- ^ Singh, Prashant K.; Ahmad, Nayeem; Yamini, Shavait; Singh, Rashmi P.; Singh, Amit K.; Sharma, Pradeep; Smith, Michael L.; Sharma, Sujata; Singh, Tej P. (2022). "Structural evidence of the oxidation of iodide ion into hyper-reactive hypoiodite ion by mammalian heme lactoperoxidase". Protein Science. 31 (2): 384–395. doi:10.1002/pro.4230. PMC 8819834. PMID 34761444.