Sodium iodate

From Wikipedia the free encyclopedia

Sodium iodate
Sodium iodate
Names
Other names
Iodic acid, sodium salt
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
ECHA InfoCard 100.028.793 Edit this at Wikidata
EC Number
  • 231-672-5
KEGG
RTECS number
  • NN1400000
UNII
  • InChI=1S/HIO3.Na/c2-1(3)4;/h(H,2,3,4);/q;+1/p-1 checkY
    Key: WTCBONOLBHEDIL-UHFFFAOYSA-M checkY
  • InChI=1/HIO3.Na/c2-1(3)4;/h(H,2,3,4);/q;+1/p-1
    Key: WTCBONOLBHEDIL-REWHXWOFAB
  • [Na+].[O-]I(=O)=O
Properties
INaO3
Molar mass 197.891 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)
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
Structure
Orthorhombic
Thermochemistry
125.5 J/mol·K[1]
135 J/mol·K[1]
−490.4 kJ/mol[1]
35.1 kJ/mol[1]
Hazards
GHS labelling:
GHS03: OxidizingGHS07: Exclamation markGHS08: Health hazard[4]
Danger
H272, H302, H317, H334[4]
P220, P261, P280, P342+P311[4]
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 1: Exposure would cause irritation but only minor residual injury. E.g. turpentineFlammability 0: Will not burn. E.g. waterInstability 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g. calciumSpecial hazard OX: Oxidizer. E.g. potassium perchlorate
1
0
1
OX
Lethal dose or concentration (LD, LC):
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 checkY☒N ?)

Sodium iodate (NaIO3) is the sodium salt of iodic acid. Sodium iodate is an oxidizing agent. It has several uses.

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 sodium 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 + NaOCl → NaIO4 + NaCl

Uses[edit]

The main use of sodium iodate in everyday life is in iodised salt. The other compounds which are used in iodised table salt are potassium iodate, potassium iodide, and sodium iodide. Sodium iodate comprises 15 to 50 mg per kilogram of applicable salt.

Sodium iodate is also used as a dough conditioner to strengthen the dough.

Safety[edit]

Iodates combined with organic compounds form an explosive mixture.[citation needed]

References[edit]

  1. ^ a b c d e f g "Sodium iodate".
  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 "https://en.wikipedia.org/w/index.php?title=Sodium_iodate&oldid=1198587886"