Sodium iodate

Sodium iodate

Names
Other names Iodic acid, sodium salt
Identifiers
CAS Number	7681-55-2
ChemSpider	22760
EC Number	231-672-5
Jmol interactive 3D	Image
PubChem	23675764
RTECS number	NN1400000
InChI InChI=1S/HIO3.Na/c2-1(3)4;/h(H,2,3,4);/q;+1/p-1 Key: WTCBONOLBHEDIL-UHFFFAOYSA-M InChI=1/HIO3.Na/c2-1(3)4;/h(H,2,3,4);/q;+1/p-1 Key: WTCBONOLBHEDIL-REWHXWOFAB
SMILES [Na+].[O-]I(=O)=O
Properties
Chemical formula	INaO3
Molar mass	197.89 g·mol^−1
Appearance	White orthorhombic crystals
Odor	Odorless
Density	4.28 g/cm^3
Melting point	425 °C (797 °F; 698 K) (anhydrous) decomposes[1] 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)[2] 32.59 g/100 mL (100 °C)[3]
Solubility	Soluble in acetic acid Insoluble in alcohol
Solubility in dimethylformamide	0.5 g/kg[2]
Structure
Crystal structure	Orthorhombic
Thermochemistry
Specific heat capacity (C)	125.5 J/mol·K[2]
Std molar entropy (S^o298)	135 J/mol·K[2]
Std enthalpy of formation (ΔfH^o298)	−490.4 kJ/mol[2]
Gibbs free energy (ΔfG˚)	35.1 kJ/mol[2]
Hazards
GHS pictograms	[4]
GHS signal word	Danger
GHS hazard statements	H272, H302, H317, H334[4]
GHS precautionary statements	P220, P261, P280, P342+311[4]
EU classification (DSD)	O Xn
R-phrases	R8, R22, R42/43
S-phrases	S17, S22, S36/37, S45
NFPA 704	0 1 1 OX
Lethal dose or concentration (LD, LC):
LD50 (Median dose)	108 mg/kg (mice, intravenous)[2]
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).
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Infobox references

Sodium iodate (NaIO₃) is the sodium salt of iodic acid. Sodium iodate is an oxidizing agent, and as such it can cause fires upon contact with combustible materials or reducing agents.

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 its 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

Safety

Conditions/substances to avoid are: heat, shock, friction, combustible materials, reducing materials, aluminium, organic compounds, carbon, hydrogen peroxide, sulfides.

References

1. Lide, David R. (1998). Handbook of Chemistry and Physics (87 ed.). Boca Raton, FL: CRC Press. pp. 4–85. ISBN 0-8493-0594-2.
2. http://chemister.ru/Database/properties-en.php?dbid=1&id=759
3. 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.
4. Sigma-Aldrich Co., Sodium iodate. Retrieved on 2014-05-25.