Iodic acid
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| Names | |||
|---|---|---|---|
| Other names
Iodic(V) acid | |||
| Identifiers | |||
7782-68-5  | |||
| ChEBI | CHEBI:24857 | ||
| ChEMBL | ChEMBL1161636 | ||
| ChemSpider | 22761 | ||
| Jmol interactive 3D | Image | ||
| PubChem | 24345 | ||
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| Properties | |||
| HIO3 | |||
| Molar mass | 175.91 g/mol | ||
| Appearance | White solid | ||
| Density | 4.62 g/cm3, solid | ||
| Melting point | 110 °C (230 °F; 383 K) | ||
| 269 g/100 mL (20 °C) | |||
| Acidity (pKa) | 0.75 | ||
| Hazards | |||
| Flash point | Non-flammable | ||
| Related compounds | |||
| Other cations |
Lithium iodate Potassium iodate | ||
| Chloric acid Bromic acid | |||
| Related compounds |
Hydroiodic acid Iodine pentoxide Periodic acid | ||
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |||
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| Infobox references | |||
Iodic acid, HIO3, can be obtained as a white or off-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.
Preparation
Iodic acid can be produced by oxidizing I2 with strong oxidizers such as Nitric acid HNO
3, Chlorine Cl
2, Chloric acid HClO
3 or Hydrogen peroxide H
2O
2,[1] for example :
Properties
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.
Uses
Iodic acid is used as a strong acid in analytical chemistry. It may be used to standardize solutions of both weak and strong bases, with methyl red or methyl orange as the indicator.
Use in salt industry
Iodic acid can be used to synthesize sodium or potassium iodate for increasing iodine content of salt.
References
- ↑ (German) Arnold F. Holleman, Nils Wiberg, « Lehrbuch der Anorganischen Chemie », 102. Auflage, Berlin, 2007. ISBN 978-3-11-017770-1