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Sodium iodate

Names
Other names Iodic acid, sodium salt
Identifiers
CAS Number	7681-55-2
3D model (JSmol)	Interactive image
ChEBI	CHEBI:81708
ChemSpider	22760
ECHA InfoCard	100.028.793
EC Number	231-672-5
KEGG	C18366
PubChem CID	23675764
RTECS number	NN1400000
UNII	U558PCS5Z9
CompTox Dashboard (EPA)	DTXSID90858754
InChI InChI=1S/HIO3.Na/c2-1(3)4;/h(H,2,3,4);/q;+1/p-1Key: WTCBONOLBHEDIL-UHFFFAOYSA-M InChI=1/HIO3.Na/c2-1(3)4;/h(H,2,3,4);/q;+1/p-1Key: WTCBONOLBHEDIL-REWHXWOFAB
SMILES .I(=O)=O
Properties
Chemical formula	INaO3
Molar mass	197.891 g·mol
Appearance	White orthorhombic crystals
Odor	Odorless
Density	4.28 g/cm
Melting point	425 °C (797 °F; 698 K) (anhydrous) decomposes 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) 32.59 g/100 mL (100 °C)
Solubility	Soluble in acetic acid Insoluble in alcohol
Solubility in dimethylformamide	0.5 g/kg
Magnetic susceptibility (χ)	−53.0·10 cm/mol
Structure
Crystal structure	Orthorhombic
Thermochemistry
Heat capacity (C)	125.5 J/mol·K
Std molar entropy (S298)	135 J/mol·K
Std enthalpy of formation (ΔfH298)	−490.4 kJ/mol
Gibbs free energy (ΔfG)	35.1 kJ/mol
Hazards
GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H272, H302, H317, H334
Precautionary statements	P220, P261, P280, P342+P311
NFPA 704 (fire diamond)	1 0 1OX
Lethal dose or concentration (LD, LC):
LD50 (median dose)	108 mg/kg (mice, intravenous)
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 , 100 kPa). N verify (what is  ?) 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:

3 I₂ + 6 NaOH → NaIO₃ + 5 NaI + 3 H₂O

Reactions

Sodium iodate can be oxidized to sodium periodate in water solutions by hypochlorites or other strong oxidizing agents:

NaIO₃ + NaOCl → NaIO₄ + NaCl

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.

References

1. ^ "Sodium iodate".
2. 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.
3. Lide, David R. (1998). Handbook of Chemistry and Physics (87 ed.). Boca Raton, Florida: CRC Press. pp. 4–85. ISBN 0-8493-0594-2.
4. ^ Sigma-Aldrich Co., Sodium iodate. Retrieved on 2014-05-25.

• Iodates
• Sodium compounds
• Oxidizing agents