Sodium bromate
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| Names | |||
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| IUPAC name
Sodium bromate | |||
| Other names
Sodium bromate(V) Bromic acid, sodium salt | |||
| Identifiers | |||
7789-38-0  | |||
| ChEBI | CHEBI:75229  | ||
| ChemSpider | 23009 | ||
| EC number | 232-160-4 | ||
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| Jmol-3D images | Image | ||
| PubChem | 23668195 | ||
| RTECS number | EF8750000 | ||
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| 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 | ||
| Refractive index (nD) |
1.594 | ||
| Structure | |||
| Crystal structure | cubic | ||
| Thermochemistry | |||
| Std molar entropy (S |
130.5 J/mol K | ||
| Std enthalpy of formation (ΔfH |
-342.5 kJ/mol | ||
| Gibbs free energy (ΔfG˚) |
-252.6 kJ/mol | ||
| Hazards | |||
| MSDS | ICSC 0196 | ||
| Main hazards | Oxidizing agent | ||
| EU Index | Not listed | ||
| R-phrases | R8, R36, R37, R38 | ||
| S-phrases | S26, S27, S36, S37, S39 | ||
| NFPA 704 | |||
| 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 noted otherwise, data is given for materials in their standard state (at 25 °C (77 °F), 100 kPa) | |||
| verify (what is: /?) | |||
| 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
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 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
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