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Hypoiodous acid






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From Wikipedia, the free encyclopedia
  
(Redirected from Hypoiodite)
Hypoiodous acid
  Hydrogen, H
  Oxygen, O
  Iodine, I
Names
IUPAC name

Hypoiodous acid

Identifiers

CAS Number

3D model (JSmol)
ChEBI
ChemSpider

PubChem CID
UNII

CompTox Dashboard (EPA)

  • InChI=1S/HIO/c1-2/h2H checkY

    Key: GEOVEUCEIQCBKH-UHFFFAOYSA-N checkY

  • IO

Properties

Chemical formula

 HOI
Molar mass 143.911 g·mol−1
Acidity (pKa) 10.5 (in water, estimate)[1]
Conjugate base Hypoiodite
Related compounds

Related compounds
  • Hypochlorous acid
  • Hypobromous 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 checkY☒N ?)

    Infobox references

    Hypoiodous acid is an inorganic compound with the chemical formula HOI. It forms when an aqueous solutionofiodine is treated with mercuricorsilver 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]

    1. ^ 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.


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    • Retrieved from "https://en.wikipedia.org/w/index.php?title=Hypoiodous_acid&oldid=1228472075"
    Categories: 
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