Sodium iodate

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Sodium iodate
The sodium cation
The iodate anion (space-filling model)
Names
Other names
iodic acid, sodium salt
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.028.793
RTECS number
  • NN1400000
Properties
NaIO3
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
Hazards
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).
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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 + NaOClNaIO4 + 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