Sodium iodate
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Other names Iodic acid, sodium salt | |
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ECHA InfoCard | 100.028.793 |
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Properties | |
Chemical formula | INaO3 |
Molar mass | 197.891 g·mol−1 |
Appearance | White orthorhombic crystals |
Odor | Odorless |
Density | 4.28 g/cm3 |
Melting point | 425 °C (797 °F; 698 K) (anhydrous) decomposes[3] 19.85 °C (67.73 °F; 293.00 K) (pentahydrate) |
Solubility in water | 2.5 g/100 mL (0 °C) 8.98 g/100 mL (20 °C) 9.47 g/100 mL (25 °C)[1] 32.59 g/100 mL (100 °C)[2] |
Solubility | Soluble in acetic acid Insoluble in alcohol |
Solubility in dimethylformamide | 0.5 g/kg[1] |
−53.0·10−6 cm3/mol | |
Structure | |
Orthorhombic | |
Thermochemistry | |
Heat capacity (C) | 125.5 J/mol·K[1] |
Std molar entropy (S⦵298) | 135 J/mol·K[1] |
Std enthalpy of formation (ΔfH⦵298) | −490.4 kJ/mol[1] |
Gibbs free energy (ΔfG⦵) | 35.1 kJ/mol[1] |
Hazards | |
GHS labelling: | |
[4] | |
Danger | |
H272, H302, H317, H334[4] | |
P220, P261, P280, P342+P311[4] | |
NFPA 704 (fire diamond) | 1 0 1 OX |
Lethal dose or concentration (LD, LC): | |
LD50 (median dose) | 108 mg/kg (mice, intravenous)[1] |
Related compounds | |
Other anions | Sodium iodide Sodium periodate Sodium bromate Sodium chlorate |
Other cations | Potassium iodate Silver iodate |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). N verify (what is YN ?) Infobox references |
Sodium iodate (NaIO3) is the sodium salt of iodic acid. Sodium iodate is an oxidizing agent. It has several uses.
Preparation
It can be prepared by reacting a sodium-containing base such as sodium hydroxide with iodic acid, for example:
- HIO3 + NaOH → NaIO3 + H2O
It can also be prepared by adding iodine to a hot, concentrated solution of sodium hydroxide or sodium carbonate:
Reactions
Sodium iodate can be oxidized to sodium periodate in water solutions by hypochlorites or other strong oxidizing agents:
Uses
The main use of sodium iodate in everyday life is in iodised salt. The other compounds which are used in iodised table salt are potassium iodate, potassium iodide, and sodium iodide. Sodium iodate comprises 15 to 50 mg per kilogram of applicable salt.
Sodium iodate is also used as a dough conditioner to strengthen the dough.
Safety
Iodates combined with organic compounds form an explosive mixture.[citation needed]
References
- ^ a b c d e f g "Sodium iodate".
- ^ Seidell, Atherton; Linke, William F. (1919). Solubilities of Inorganic and Organic Compounds (2nd ed.). D. Van Nostrand Company.
Results here are multiplied by water's density at temperature of solution for unit conversion. - ^ Lide, David R. (1998). Handbook of Chemistry and Physics (87 ed.). Boca Raton, Florida: CRC Press. pp. 4–85. ISBN 0-8493-0594-2.
- ^ a b c Sigma-Aldrich Co., Sodium iodate. Retrieved on 2014-05-25.
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Chalcogenides | |
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Oxyhalides | |
Oxychalcogenides |
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Oxypnictogenides |
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Others |
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- CH3ONa
- C2H5ONa
- HCOONa
- C2H5COONa
- C3H7COONa
- Na2C4H4O6
- C4H5NaO6
- NaCH3COO
- NaC6H5CO2
- NaC6H4(OH)CO2
- NaC12H23O2
- NaC10H8
- Na2[Fe[CN5]NO]
- C6H16AlNaO4
- NaC6H7O6
- C5H8NO4Na
- C6H5Na
- C4H9Na
- NaC5H5
- C15H31COONa
- C17H33COONa
- C18H35O2Na
- C164H256O68S2Na2