Sodium bromate
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Names | |||
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IUPAC name
Sodium bromate
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Other names
Sodium bromate(V)
Bromic acid, sodium salt | |||
Identifiers | |||
3D model (
JSmol ) |
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ChEBI | |||
ChemSpider | |||
ECHA InfoCard
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100.029.237 | ||
EC Number |
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PubChem CID
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RTECS number
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UNII | |||
UN number | 1494 | ||
CompTox Dashboard (EPA)
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Properties | |||
NaBrO3 | |||
Molar mass | 150.89g/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 | |||
Refractive index (nD)
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1.594 | ||
Structure | |||
cubic | |||
Thermochemistry | |||
Std molar
entropy (S⦵298) |
130.5 J/mol K | ||
Std enthalpy of (ΔfH⦵298)formation |
-342.5 kJ/mol | ||
Gibbs free energy (ΔfG⦵)
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-252.6 kJ/mol | ||
Hazards | |||
Occupational safety and health (OHS/OSH): | |||
Main hazards
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Oxidizing agent | ||
GHS labelling: | |||
Danger | |||
H271, H272, H302, H315, H319, H335, H341, H350 | |||
P201, P202, P210, P220, P221, P261, P264, P270, P271, P280, P281, P283, P301+P312, P302+P352, P304+P340, P305+P351+P338, P306+P360, P308+P313, P312, P321, P330, P332+P313, P337+P313, P362, P370+P378, P371+P380+P375, P403+P233, P405, P501 | |||
NFPA 704 (fire diamond) | |||
Flash point | 381 °C (718 °F; 654 K) | ||
Safety data sheet (SDS) | ICSC 0196 | ||
Related compounds | |||
Other anions
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Sodium chlorate Sodium iodate | ||
Other cations
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Potassium bromate Calcium bromate | ||
Related compounds
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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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This article needs additional citations for verification. (June 2019) |
Sodium bromate, the
oxidant
.
Uses
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
Sodium bromate is produced by passing
oxidation of sodium bromide. Alternatively, it can also be created by the oxidation of bromine with chlorine to sodium hydroxide
at 80 °C.
3 Br2+3 Na2CO3 → 5 NaBr+NaBrO3+3 CO2
Human health issues
Bromate in drinking water is undesirable because it is a suspected human
UK.[4]
References
- ^ "Br2 + Na2CO3 = NaBr + NaBrO3 + CO2 | Chemical reaction and equation".
- ^ "Potassium Bromate (Group 2B)". International Agency for Research on Cancer: Summaries and Evaluations. Canadian Centre for Occupational Health and Safety. Retrieved 2008-03-09.
- PMID 2269236.
- ^ "Coke recalls controversial water". BBC News. 2004-03-19. Retrieved 2008-03-09.
External links