Sodium iodate

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Sodium iodate
Sodium iodate
Identifiers
CAS number 7681-55-2 N
PubChem 23675764
ChemSpider 22760 YesY
EC number 231-672-5
RTECS number NN1400000
Jmol-3D images Image 1
Properties
Molecular formula INaO3
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)
(pentahydrate)
Solubility in water 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]
Structure
Crystal structure Orthorhombic
Thermochemistry
Specific
heat capacity
C
125.5 J/mol·K[1]
Std molar
entropy
So298
135 J/mol·K[1]
Std enthalpy of
formation
ΔfHo298
−490.4 kJ/mol[1]
Gibbs free energy ΔG 35.1 kJ/mol[1]
Hazards
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
GHS hazard statements H272, H302, H317, H334[4]
GHS precautionary statements P220, P261, P280, P342+311[4]
EU classification Oxidizing Agent O Harmful Xn
R-phrases R8, R22, R42/43
S-phrases S17, S22, S36/37, S45
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
LD50 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 noted otherwise, 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[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. ^ a b c d e f g http://chemister.ru/Database/properties-en.php?dbid=1&id=759
  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, FL: CRC Press. pp. 4–85. ISBN 0-8493-0594-2. 
  4. ^ a b c Sigma-Aldrich Co., Sodium iodate. Retrieved on 2014-05-25.