Sodium iodate

From Wikipedia, the free encyclopedia

This is an old revision of this page, as edited by Berberisb (talk | contribs) at 01:10, 24 May 2013 (fix a punctuation error). The present address (URL) is a permanent link to this revision, which may differ significantly from the current revision.

Jump to navigation Jump to search
Sodium iodate
The sodium cation
The iodate anion (space-filling model)
Other names
iodic acid, sodium salt
3D model (JSmol)
ECHA InfoCard 100.028.793
RTECS number
  • NN1400000
Molar mass 197.8924 g/mol
Appearance white orthorhombic crystals
Density 4.28 g/cm³, solid
Melting point 425 °C (decomp)

[1] (anhydrous)
19.85 °C (pentahydrate)

9.47 g/100 mL (25 °C)
34 g/100 mL (100 °C)
Solubility soluble in acetic acid
insoluble in alcohol
not listed
NFPA 704 (fire diamond)
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. ^ Lide, David R. (1998), Handbook of Chemistry and Physics (87 ed.), Boca Raton, FL: CRC Press, pp. 4–85, ISBN 0-8493-0594-2