Sodium iodate

From Wikipedia, the free encyclopedia
Jump to navigation Jump to search
Sodium iodate
Sodium iodate
Other names
Iodic acid, sodium salt
  • 7681-55-2 ☒N
3D model (JSmol)
  • Interactive image
  • 22760 ☑Y
ECHA InfoCard 100.028.793
EC Number 231-672-5
PubChem CID
  • 23675764
RTECS number NN1400000
Molar mass 197.89 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)
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
125.5 J/mol·K[1]
135 J/mol·K[1]
−490.4 kJ/mol[1]
35.1 kJ/mol[1]
GHS pictograms The flame-over-circle pictogram in the Globally Harmonized System of Classification and Labelling of Chemicals (GHS)The exclamation-mark pictogram in the Globally Harmonized System of Classification and Labelling of Chemicals (GHS)The health hazard pictogram in the Globally Harmonized System of Classification and Labelling of Chemicals (GHS)[4]
GHS signal word Danger
H272, H302, H317, H334[4]
P220, P261, P280, P342+311[4]
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 1: Exposure would cause irritation but only minor residual injury. E.g., turpentine Reactivity code 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g., calcium Special hazard OX: Oxidizer. E.g., potassium perchlorateNFPA 704 four-colored diamond
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 ☑Y☒N ?)
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.


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


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

NaIO3 + NaOClNaIO4 + NaCl


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


  1. ^ a b c d e f g
  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. ^ a b c Sigma-Aldrich Co., Sodium iodate. Retrieved on 2014-05-25.
Retrieved from ""
This content was retrieved from Wikipedia :
This page is based on the copyrighted Wikipedia article "Sodium iodate"; it is used under the Creative Commons Attribution-ShareAlike 3.0 Unported License (CC-BY-SA). You may redistribute it, verbatim or modified, providing that you comply with the terms of the CC-BY-SA