|Jmol-3D images||Image 1|
|Molar mass||175.91 g/mol|
|Density||4.62 g/cm3, solid|
|Melting point||110 °C|
|Solubility in water||269 g/100 mL (20 °C)|
|EU Index||Not listed|
|Other cations||Lithium iodate
|Related halogen oxoacids||Chloric acid
|Related compounds||Hydroiodic acid
|Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)|
|(what is: / ?)|
Iodic acid, HIO3, can be obtained as a white solid. It dissolves in water very well, but it also exists in the pure state, as opposed to chloric acid or bromic acid. Iodic acid contains iodine in the oxidation state +5 and it is one of the most stable oxo-acids of the halogens in its pure state. When iodic acid is carefully heated, it dehydrates to iodine pentoxide. On subsequent heating, the iodine pentoxide further decomposes, giving a mix of iodine, oxygen and lower oxides of iodine.
Iodic acid is a relatively strong acid with a pKa of 0.75. It is strongly oxidizing in acidic solution, less so in basic solution. When iodic acid acts as oxidizer, then the product of the reaction is either iodine, or iodide ion. Under some special conditions (very low pH and high concentration of chloride ion, e.g. in concentrated hydrochloric acid), iodic acid is reduced to iodine trichloride, a golden yellow compound in solution and no further reduction occurs. In the absence of chloride ions, when there is an excess amount of reductant, then all iodate is converted to iodide ion. When there is an excess amount of iodate, then part of the iodate is converted to iodine.
Use in salt industry
|This article needs additional citations for verification. (May 2013)|
- (German) Arnold F. Holleman, Nils Wiberg, « Lehrbuch der Anorganischen Chemie », 102. Auflage, Berlin, 2007.
This 978-3-11-017770-1 lacks ISBNs for the books listed in it. (May 2013)