Calcium iodate

Calcium iodate is any of two inorganic compounds with the formula Ca(IO3)2(H2O)x, where x = 0 or 1. Both are colourless salts that occur as the minerals lautarite and bruggenite, respectively. A third mineral form of calcium iodate is dietzeite, a salt containing chromate with the formula Ca2(IO3)2CrO4.[1] These minerals are the most common compounds containing iodate.

Calcium iodate
Names
IUPAC name
Calcium diiodate
Other names
Lautarite
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.029.265
EC Number
  • 232-191-3
E number E916 (glazing agents, ...)
UNII
  • InChI=1S/Ca.2HIO3/c;2*2-1(3)4/h;2*(H,2,3,4)/q+2;;/p-2 checkY
    Key: UHWJJLGTKIWIJO-UHFFFAOYSA-L checkY
  • InChI=1/Ca.2HIO3/c;2*2-1(3)4/h;2*(H,2,3,4)/q+2;;/p-2
    Key: UHWJJLGTKIWIJO-NUQVWONBAT
  • [Ca+2].[O-]I(=O)=O.[O-]I(=O)=O
Properties
Ca(IO3)2
Molar mass 389.88 g/mol (anhydrous)
407.90 g/mol (monohydrate)
Appearance white solid
Density 4.519 g/cm3 (monohydrate)
Melting point 540 °C (1,004 °F; 813 K) (monohydrate)
Boiling point decomposes
0.09 g/100 mL (0 °C)
0.24 g/100 mL (20 °C)
0.67 g/100 mL (90 °C)
6.47×10−6
Solubility soluble in nitric acid
insoluble in alcohol
-101.4·10−6 cm3/mol
Structure
monoclinic (anhydrous)
cubic (monohydrate)
orthorhombic (hexahydrate)
Hazards
Flash point non-flammable
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

Production and uses

Lautarite, described as the most important mineral source of iodine, is mined in the Atacama Desert.[1] Processing of the ore entails reduction of its aqueous extracts with sodium bisulfite to give sodium iodide. This comproportionation reaction is a major source of the sodium iodide.[1]

Calcium iodate can be produced by the anodic oxidation of calcium iodide or by passing chlorine into a hot solution of lime in which iodine has been dissolved.

Calcium iodate is used as an iodine supplement in chicken feed.[1] Ethylenediamine dihydroiodide (EDDI) is a more typical source of nutritional iodine.

References
  1. Lyday, Phyllis A.; Kaiho, Tatsuo (2015). "Iodine and Iodine Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. pp. 1–13. doi:10.1002/14356007.a14_381.pub2.
This article is issued from Wikipedia. The text is licensed under Creative Commons - Attribution - Sharealike. Additional terms may apply for the media files.