Sodium bromate

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Sodium bromate
Sodium bromate
The sodium cation
The bromate anion (space-filling model)
Names
IUPAC name
Sodium bromate
Other names
Sodium bromate(V)
Bromic acid, sodium salt
Identifiers
3D model (Jmol)
ChEBI
ChemSpider
ECHA InfoCard 100.029.237
EC Number 232-160-4
RTECS number EF8750000
UN number 1494
Properties
NaBrO3
Molar mass 150.892 g/mol
Appearance colorless or white solid
Odor odorless
Density 3.339 g/cm3
Melting point 381 °C (718 °F; 654 K)
Boiling point 1,390 °C (2,530 °F; 1,660 K)
27.5 g/100 mL (0 °C)
36.4 g/100 mL (20 °C)
48.8 g/100 mL (40 °C)
90.8 g/100 mL (100 °C)
Solubility soluble in ammonia
insoluble in ethanol
−44.2·10−6 cm3/mol
1.594
Structure
cubic
Thermochemistry
130.5 J/mol K
-342.5 kJ/mol
-252.6 kJ/mol
Hazards
Main hazards Oxidizing agent
Safety data sheet ICSC 0196
R-phrases R8, R36, R37, R38
S-phrases S26, S27, S36, S37, S39
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 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogen Special hazard OX: Oxidizer. E.g., potassium perchlorateNFPA 704 four-colored diamond
Flash point 381 °C (718 °F; 654 K)
Related compounds
Other anions
Sodium chlorate
Sodium iodate
Other cations
Potassium bromate
Calcium bromate
Related compounds
Sodium bromide
Sodium hypobromite
Sodium bromite
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 bromate, the inorganic compound with the chemical formula of NaBrO3, is the sodium salt of bromic acid. It is a strong oxidant.

Uses[edit]

Sodium bromate is mainly used in continuous or batch dyeing processes involving sulfur or vat dyes and as a hair-permagent, chemical agent, or gold solvent in gold mines when used with sodium bromide.

Production[edit]

Sodium bromate is produced by passing bromine into a solution of sodium carbonate. It may also be produced by the electrolytic oxidation of sodium bromide. Alternatively, it can also be created by the oxidation of bromine with chlorine to sodium hydroxide at 80 °C.

External links[edit]