Sodium iodate

Last updated
Sodium iodate
Sodium iodate Natriumjodaat t.png
Sodium iodate
Names
Other names
Iodic acid, sodium salt
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
ECHA InfoCard 100.028.793 OOjs UI icon edit-ltr-progressive.svg
EC Number
  • 231-672-5
KEGG
PubChem CID
RTECS number
  • NN1400000
UNII
  • InChI=1S/HIO3.Na/c2-1(3)4;/h(H,2,3,4);/q;+1/p-1 Yes check.svgY
    Key: WTCBONOLBHEDIL-UHFFFAOYSA-M Yes check.svgY
  • InChI=1/HIO3.Na/c2-1(3)4;/h(H,2,3,4);/q;+1/p-1
    Key: WTCBONOLBHEDIL-REWHXWOFAB
  • [Na+].[O-]I(=O)=O
Properties
INaO3
Molar mass 197.891 g·mol−1
AppearanceWhite orthorhombic crystals
Odor Odorless
Density 4.28 g/cm3
Melting point 425 °C (797 °F; 698 K)
(anhydrous) decomposes [1]
19.85 °C (67.73 °F; 293.00 K)
(pentahydrate)
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]
−53.0·10−6 cm3/mol
Structure
Orthorhombic
Thermochemistry
125.5 J/mol·K [2]
Std molar
entropy (S⦵298)
135 J/mol·K [2]
−490.4 kJ/mol [2]
35.1 kJ/mol [2]
Hazards
GHS labelling:
GHS-pictogram-rondflam.svg GHS-pictogram-exclam.svg GHS-pictogram-silhouette.svg [4]
Danger
H272, H302, H317, H334 [4]
P220, P261, P280, P342+P311 [4]
NFPA 704 (fire diamond)
NFPA 704.svgHealth 1: Exposure would cause irritation but only minor residual injury. E.g. turpentineFlammability 0: Will not burn. E.g. waterInstability 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g. calciumSpecial hazard OX: Oxidizer. E.g. potassium perchlorate
1
0
1
OX
Lethal dose or concentration (LD, LC):
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).
X mark.svgN  verify  (what is  Yes check.svgYX mark.svgN ?)

Sodium iodate (Na I O3) is the sodium salt of iodic acid. Sodium iodate is an oxidizing agent. It has several uses.

Contents

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.[ citation needed ]

References

  1. ↑ Lide, David R. (1998). Handbook of Chemistry and Physics (87 ed.). Boca Raton, Florida: CRC Press. pp. 4–85. ISBN   0-8493-0594-2.
  2. 1 2 3 4 5 6 7 "Sodium iodate".
  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. 1 2 3 Sigma-Aldrich Co., Sodium iodate. Retrieved on 2014-05-25.
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