Sodium iodate

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Sodium iodate
The sodium cation The iodate anion (space-filling model)
Identifiers
CAS number 7681-55-2 N
PubChem 23675764
ChemSpider 22760 YesY
RTECS number NN1400000
Jmol-3D images Image 1
Properties
Molecular formula 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)

Solubility in water 9.47 g/100 mL (25 °C)
34 g/100 mL (100 °C)
Solubility soluble in acetic acid
insoluble in alcohol
Hazards
EU classification not listed
NFPA 704
Flammability (red): no hazard code 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
Related compounds
Other anions sodium iodide
sodium periodate
sodium bromate
sodium chlorate
Other cations potassium iodate
silver iodate
Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
 N (verify) (what is: YesY/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.

Preparation[edit]

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[edit]

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

NaIO3 + NaOClNaIO4 + NaCl

Safety[edit]

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

References[edit]

  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