Hypoiodous acid
(Redirected from Hydroxidoiodine)
| Hypoiodous acid | |
|---|---|
| IUPAC name | Hypoiodous acid[note 1] |
| Other names | Iodic(I) acid Iodanol Hydroxidoiodine |
| Identifiers | |
| InChI | InChI=1/HIO/c1-2/h2H |
| InChIKey | GEOVEUCEIQCBKH-UHFFFAOYAY |
| Standard InChI | InChI=1S/HIO/c1-2/h2H |
| Standard InChIKey | GEOVEUCEIQCBKH-UHFFFAOYSA-N |
| CAS number | [] |
| ChemSpider | |
| Properties[2] | |
| Chemical formula | HOI |
| Molar mass | 143.91 g mol−1 |
| Acidity (pKa) | 10.70 |
| Related compounds | |
| Other hypohalous acids | Hypofluorous acid Hypochlorous acid Hypobromous acid |
| Other compounds | Iodous acid Iodic acid Periodic acid |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) | |
Hypoiodous acid, HOI, is an oxoacid of iodine. It is often considered to be only stable in aqueous solution.[2][3]
Contents
Preparation
Hypoiodous acid can be prepared in solution by the reaction of iodine with a well-stirred suspension of mercury(II) oxide.[2]
- 2 I2 + 2 HgO + H2O → 2 HOI + HgO·HgI2
It is also formed by the disproportionation of iodine in water, although the equilibrium concentration is only 6.4 × 10−6 mol dm−3 in a saturated iodine solution (1.3 mmol dm−3) at 25 °C.[2]
- I2 + H2O ⇌ HOI + H+ + I−
A convenient method to prepare HOI for use in organic synthesis is the reaction of sodium hypochlorite with sodium iodide:[4]
- ClO− + I− + H2O → HOI + Cl− + OH−
Hypoiodous acid is prepared in the gas phase or in matrix isolation studies by the reaction of hydroxyl radicals or atomic oxygen with iodine or iodoalkanes.[5][6][7]
Reactivity
Notes and references
Notes
- ↑ Hypoiodous acid is a retained name in IUPAC nomenclature.[1]
References
- ↑ Nomenclature of Inorganic Chemistry; IUPAC Recommendations 2005; Royal Society of Chemistry: Cambridge, 2005; p 299. ISBN 0-85404-438-8, <http://www.iupac.org/publications/books/rbook/Red_Book_2005.pdf>.
- ↑ 2.0 2.1 2.2 2.3 Cotton, F. Albert; Wilkinson, Geoffrey Advanced Inorganic Chemistry, 5th ed.; Wiley-Interscience: New York, 1988; pp 563–67. ISBN 0-471-84997-9.
- ↑ Greenwood, Norman N.; Earnshaw, A. Chemistry of the Elements; Pergamon: Oxford, 1984; pp 999–1007. ISBN 0-08-022057-6.
- ↑ LeBlond, Carl R.; Rossen, Kai; Gortsema, Frank P.; Zavialov, Ilia A.; Cianciosi, Steven J.; Andrews, Arthur T.; Sun, Yongkui Harvesting short-lived hypoiodous acid for efficient diastereoselective iodohydroxylation in Crixivan® synthesis. Tetrahedron Lett. 2001, 42 (49), 8603–6. DOI: 10.1016/S0040-4039(01)01863-9.
- ↑ Walker, N.; Tevault, D. E.; Smardzewski, R. R. Matrix reactions of ozone and oxygen atoms with hydrogen iodide. HOI formation. J. Chem. Phys. 1978, 69 (2), 564–68. DOI: 10.1063/1.436647.
- ↑ Barnes, I.; Becker, K. H.; Starcke, J. FTIR spectroscopic observation of gaseous HOI. Chem. Phys. Lett. 1992, 196 (6), 578–82. DOI: 10.1016/0009-2614(92)85997-O.
- ↑ Klaassen, Jody J.; Lindner, Jörg; Leone, Stephen R. Observation of the ν1 OH(OD) stretch of HOI and DOI by Fourier transform infrared emission spectroscopy. J. Chem. Phys. 1996, 104 (19), 7403–11. DOI: 10.1063/1.471456.
Further reading
- Thomas, T. R.; Pence, D. T.; Hasty, R. A. The disproportionation of hypoiodous acid. J. Inorg. Nucl. Chem. 1980, 42 (2), 183–86. DOI: 10.1016/0022-1902(80)80237-5.
External links
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