Sodium bromide
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| Names | |
|---|---|
| IUPAC name
Sodium bromide | |
| Identifiers | |
7647-15-6  13466-08-5 (dihydrate)  | |
| 3D model (Jmol) | Interactive image |
| ChEMBL | ChEMBL1644694 |
| ChemSpider | 22712 |
| ECHA InfoCard | 100.028.727 |
| PubChem | 253881 |
| RTECS number | VZ3150000 |
| UNII | LC1V549NOM |
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| Properties | |
| BrNa | |
| Molar mass | 102.89 g·mol−1 |
| Appearance | White powder, hygroscopic |
| Density | 3.21 g/cm3 (anhydrous) 2.18 g/cm3 (dihydrate) |
| Melting point | 747 °C (1,377 °F; 1,020 K) (anhydrous) 36 °C (97 °F; 309 K) (dihydrate) decomposes[1] |
| Boiling point | 1,390 °C (2,530 °F; 1,660 K) [1] |
| 71.35 g/100 mL (−20 °C) 79.52 g/100 mL (0 °C) 94.32 g/100 mL (25 °C)[2] 104.9 g/100 mL (40 °C) 116.2 g/100 mL (100 °C)[3] | |
| Solubility | Soluble in alcohol, liquid ammonia, pyridine, hydrazine, SO2, amine Insoluble in acetone, acetonitrile[2] |
| Solubility in methanol | 17.3 g/100 g (0 °C) 16.8 g/100 g (20 °C) 16.1 g/100 g (40 °C) 15.3 g/100 g (60 °C)[2] |
| Solubility in ethanol | 2.45 g/100 g (0 °C) 2.32 g/100 g (20 °C) 2.29 g/100 g (30 °C) 2.35 g/100 g (70 °C)[2] |
| Solubility in formic acid | 19.3 g/100 g (18 °C) 19.4 g/100 g (25 °C)[2] |
| Solubility in glycerol | 38.7 g/100 g (20 °C)[2] |
| Solubility in dimethylformamide | 3.2 g/100 g (10.3 °C)[2] |
| Vapor pressure | 1 torr (806 °C) 5 torr (903 °C)[1] |
| Thermal conductivity | 5.6 W/m·K (150 K)[4] |
| Refractive index (nD) |
1.6428 (24 °C) nKrF = 1.8467 (24 °C) nHe–Ne = 1.6389 (24 °C)[5] |
| Viscosity | 1.42 cP (762 °C) 1.08 cP (857 °C) 0.96 cP (937 °C)[2] |
| Structure | |
| Cubic | |
| Thermochemistry | |
| 51.4 J/mol·K[2] | |
| Std molar entropy (S |
86.82 J/mol·K[2] |
| Std enthalpy of formation (ΔfH |
−361.41 kJ/mol[2] |
| Gibbs free energy (ΔfG˚) |
−349.3 kJ/mol[2] |
| Hazards | |
| Safety data sheet | External MSDS |
| R-phrases | R36 |
| S-phrases | (S2), S24/25, S46 |
| NFPA 704 | |
| Flash point | 800 °C (1,470 °F; 1,070 K) |
| Lethal dose or concentration (LD, LC): | |
| LD50 (median dose) |
3500 mg/kg (rats, oral) |
| Related compounds | |
| Other anions |
Sodium fluoride Sodium chloride Sodium iodide Sodium astatide |
| Other cations |
Lithium bromide Potassium bromide Rubidium bromide Caesium bromide Francium bromide |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| verify (what is ?) | |
| Infobox references | |
Sodium bromide is an inorganic compound with the formula NaBr. It is a high-melting white, crystalline solid that resembles sodium chloride. It is a widely used source of the bromide ion and has many applications.[7]
Synthesis, structure, reactions
NaBr crystallizes in the same cubic motif as NaCl, NaF and NaI. The anhydrous salt crystallizes above 50.7 °C.[7] Dihydrate salts (NaBr·2H2O) crystallize out of water solution below 50.7 °C.[8]
NaBr is produced by treating sodium hydroxide with hydrogen bromide.
Sodium bromide can be used as a source of the chemical element bromine. This can be accomplished by treating an aqueous solution of NaBr with chlorine gas:
- 2 NaBr + Cl2 → Br2 + 2 NaCl
Applications
Sodium bromide is the most useful inorganic bromide in industry.[7] It is also used as a catalyst in TEMPO-mediated oxidation reactions.[9]
Medicine
Also known as Sedoneural, sodium bromide has been used as a hypnotic, anticonvulsant, and sedative in medicine, widely used as an anticonvulsant and a sedative in the late 19th and early 20th centuries. Its action is due to the bromide ion, and for this reason potassium bromide is equally effective. In 1975, bromides were removed from drugs in the U.S. such as Bromo-Seltzer due to toxicity.[10]
Preparation of other bromine compounds
Sodium bromide is widely used for the preparation of other bromides in organic synthesis and other areas. It is a source of the bromide nucleophile to convert alkyl chlorides to more reactive alkyl bromides by the Finkelstein reaction:
- NaBr + RCl → RBr + NaCl (R = alkyl)
Once a large need in photography, but now shrinking, the photosensitive salt silver bromide is prepared using NaBr.
Disinfectant
Sodium bromide is used in conjunction with chlorine as a disinfectant for hot tubs and swimming pools.
Petroleum industry
Sodium bromide is used to prepare dense fluids used in oil wells.
Safety
NaBr has a very low toxicity with an oral LD50 estimated at 3.5 g/kg for rats.[6] However, this is a single-dose value. Bromide ion is a cumulative toxin with a relatively long half life (in excess of a week in humans): see potassium bromide.
References
- 1 2 3 Pradyot, Patnaik (2003). Handbook of Inorganic Chemicals. The McGraw-Hill Companies, Inc. ISBN 0-07-049439-8.
- 1 2 3 4 5 6 7 8 9 10 11 12 http://chemister.ru/Database/properties-en.php?dbid=1&id=714
- ↑ Seidell, Atherton; Linke, William F. (1919). Solubilities of Inorganic and Organic Compounds (2nd ed.). D. Van Nostrand Company.
- 1 2 "Sodium Bromide (NaBr)". korth.de. Korth Kristalle GmbH. Retrieved 2014-06-11.
- ↑ Polyanskiy, Mikhail. "Refractive index of NaBr (Sodium bromide) - Li". refractiveindex.info. Retrieved 2014-06-11.
- 1 2 "Sodium bromide MSDS" (PDF). sciencelab.com. Sciencelab.com, Inc. 2013-05-21. Retrieved 2014-06-11.
- 1 2 3 Michael J. Dagani, Henry J. Barda, Theodore J. Benya, David C. Sanders "Bromine Compounds" in Ullmann's Encyclopedia of Industrial Chemistry Wiley-VCH, Weinheim, 2000. doi:10.1002/14356007.a04_405
- ↑ Eagleson, Mary (translated by) (1994). Concise Encyclopedia Chemistry (Illustrated, revised, English language ed.). Berlin [u.a.]: Walter De Gruyter. p. 996. ISBN 9783110114515.
- ↑ "Water dispersion of cellulose II nanocrystals prepared by TEMPO-mediated oxidation of mercerized cellulose at pH 4.8". Cellulose. 17: 279–288. doi:10.1007/s10570-009-9381-2.
- ↑ "Bromide: Potassium & Sodium". canine-epilepsy.com. Canine-Epilepsy Resources. 2011-05-31. Retrieved 2014-06-11.
External links
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