| |||
| |||
| Names | |||
|---|---|---|---|
| IUPAC name
Sodium bromate
| |||
| Other names
Sodium bromate(V)
Bromic acid, sodium salt | |||
| Identifiers | |||
3D model (JSmol)
|
|||
| ChEBI | |||
| ChemSpider | |||
| ECHA InfoCard | 100.029.237 | ||
| EC Number |
| ||
PubChem CID
|
|||
| RTECS number |
| ||
| UNII | |||
| UN number | 1494 | ||
CompTox Dashboard (EPA)
|
|||
| |||
| |||
| 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)
|
1.594 | ||
| Structure | |||
| cubic | |||
| Thermochemistry | |||
Std molar
entropy (S⦵298) |
130.5 J/mol K | ||
Std enthalpy of
formation (ΔfH⦵298) |
-342.5 kJ/mol | ||
Gibbs free energy (ΔfG⦵)
|
-252.6 kJ/mol | ||
| Hazards | |||
| Occupational safety and health (OHS/OSH): | |||
Main hazards
|
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
|
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).
| |||
Sodium bromate, the inorganic compound with the chemical formula of NaBrO3, is the sodium salt of bromic acid. It is a strong oxidant.
YouTube Encyclopedic
-
1/2Views:8 9092 413
-
Synthesis of sodium bromated and potassium metaperiodate
-
Belousov-Zhabotinsky Oscillating Reaction (bromide to diatomic bromine)
Transcription
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 can be produced from a solution of sodium carbonate and bromine using chlorine gas as the oxidising agent.[1] This reaction proceeds according to the equation 6 Na2CO3 + Br2 + 5 Cl2 → 2 NaBrO3 + 10 NaCl + 6 CO2
It may also be produced by the electrolytic oxidation of aqueous sodium bromide.[2]
Human health issues
Bromate in drinking water is undesirable because it is a suspected human carcinogen.[3][4] Its presence in Coca-Cola's Dasani bottled water forced a recall of that product in the UK.[5]
References
- ^ CN patent 1034653C, Zhao Naizhi; Wu Zongsheng; Sun Guishi, published 1997-04-23, assigned to Daqinghe Saltern Changlu Hebei Prov.
- ^ WO patent 1996030562A1, David B. Blum; Rodney H. Sergent; Vadim Zolotarsky, "Process and apparatus for generating bromine", published 1996-10-03, assigned to Electrocatalytic Inc
- ^ "Potassium Bromate (Group 2B)". International Agency for Research on Cancer: Summaries and Evaluations. Canadian Centre for Occupational Health and Safety. Retrieved 2008-03-09.
- ^ Kurokawa, Yuji; Maekawa, A; Takahashi, M; Hayashi, Y (July 1990). "Toxicity and carcinogenicity of potassium bromate—a new renal carcinogen". Environmental Health Perspectives. 87: 309–35. doi:10.1289/EHP.9087309. JSTOR 3431039. PMC 1567851. PMID 2269236.
- ^ "Coke recalls controversial water". BBC News. 2004-03-19. Retrieved 2008-03-09.
Notes
External links
 | This inorganic compound–related article is a stub. You can help Wikipedia by expanding it. |
This page was last edited on 22 May 2024, at 13:17