Iodic acid
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| Other names
Iodic(V) acid
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| Identifiers | |||
3D model (JSmol)
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| ChemSpider | |||
| ECHA InfoCard | 100.029.056 | ||
PubChem CID
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CompTox Dashboard (EPA)
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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[1] | ||
| Conjugate base | Iodate | ||
| −48.0·10−6 cm3/mol | |||
| Hazards | |||
| Occupational safety and health (OHS/OSH): | |||
Main hazards
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acid, corrosive, oxidant | ||
| GHS labelling:[2] | |||
 
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| Danger | |||
| NFPA 704 (fire diamond) | |||
| Flash point | Non-flammable | ||
| Related compounds | |||
Other cations
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Lithium iodate Potassium iodate | ||
| Chloric acid Bromic acid | |||
Related compounds
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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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Iodic acid is a white water-soluble solid with the chemical formula HIO3. Its robustness contrasts with the instability of chloric acid and bromic acid. Iodic acid features iodine in the oxidation state +5 and is one of the most stable oxo-acids of the halogens. When heated, samples dehydrate to give iodine pentoxide. On further heating, the iodine pentoxide further decomposes, giving a mix of iodine, oxygen and lower oxides of iodine.
Preparation
[edit]Iodic acid can be produced by oxidizing iodine with strong oxidizers such as nitric acid, chlorine, chloric acid or hydrogen peroxide,[3] for example:
- I2 + 6H2O + 5Cl2 ⇌ 2HIO3 + 10HCl
Iodic acid is also produced by the reaction of iodine monochloride with water:
- 5ICl + 3H2O → 5HCl + HIO3 + 2I2
Structure
[edit]Iodic acid crystallises from acidic solution as orthorhombic α-HIO
3 in space group P212121. The structure consists of pyramidal molecules linked by hydrogen bonding and intermolecular iodine-oxygen interactions. The I=O bond lengths are 1.81 Å while the I–OH distance is 1.89 Å.[4][5][6] Several other polymorphs have been reported, including an orthorhombic γ form in space group Pbca[7] and an orthorhombic δ form in space group P212121.[8] All of the polymorphs contain pyramidal molecules, hydrogen bonding and I···O interactions, but differ in packing arrangement.
Properties
[edit]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 ions, such as 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.[citation needed]
Uses
[edit]Iodic acid is used as a strong acid in analytical chemistry. It may be used to standardize solutions of both weak and strong bases, using methyl red or methyl orange as the indicator.
Use in salt industry
[edit]Iodic acid can be used to synthesize sodium or potassium iodate for increasing iodine content of salt.[citation needed]
Other oxyacids
[edit]Iodic acid is part of a series of oxyacids in which iodine can assume oxidation states of −1, +1, +3, +5, or +7. A number of neutral iodine oxides are also known.
| Iodine oxidation state | −1 | +1 | +3 | +5 | +7 |
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| Name | Hydrogen iodide | Hypoiodous acid | Iodous acid | Iodic acid | Periodic acid |
| Formula | HI | HIO | HIO2 | HIO3 | HIO4 or H5IO6 |
References
[edit]- ^ 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 127. ISBN 0-08-029214-3. LCCN 82-16524.
- ^ "Iodic acid" (PDF). Archived from the original (PDF) on 2014-09-26. Retrieved 2022-01-30.
- ^ Holleman, Arnold F.; Wiberg, Nils (2007). Lehrbuch der Anorganischen Chemie (in German) (102nd ed.). Berlin. ISBN 978-3-11-017770-1.
{{cite book}}: CS1 maint: location missing publisher (link) - ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 863. ISBN 978-0-08-037941-8.
- ^ Rogers, Max T.; Helmholz, Lindsay (1941). "The Crystal Structure of Iodic Acid". J. Am. Chem. Soc. 63 (1): 278–284. doi:10.1021/ja01846a068.
- ^ Ståhl, Kenny; Szafranski, Marek (1992). "A Single-Crystal Neutron Diffraction Study of HIO3 at 295 and 30 K and of DIO3 at 295 K". Acta Chem. Scand. 46: 1146–1148. doi:10.3891/acta.chem.scand.46-1146.
- ^ Fischer, Andreas; Lindsjö, Martin (2005). "γ-HIO3 – a Metastable, Centrosymmetric Polymorph of Iodic Acid". Z. Anorg. Allg. Chem. 631 (9): 1574–1576. doi:10.1002/zaac.200500099.
- ^ Wu, Tao; Zavalij, Peter Y.; Zachariah, Michael R. (2017). "Crystal structure of a new polymorph of iodic acid, δ-HIO3, from powder diffraction". Powder Diffraction. 32 (4): 261–264. Bibcode:2017PDiff..32..261W. doi:10.1017/S0885715617000859. S2CID 104100313.