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Sodium bromide information


Sodium bromide
3D model of sodium bromide
Sodium bromide powder
Names
IUPAC name
Sodium bromide
Identifiers
CAS Number
  • anhydrous: 7647-15-6 checkY
  • dihydrate: 13466-08-5 ☒N
3D model (JSmol)
  • anhydrous: Interactive image
ChEMBL
  • anhydrous: ChEMBL1644694 checkY
ChemSpider
  • anhydrous: 22712 checkY
ECHA InfoCard 100.028.727 Edit this at Wikidata
PubChem CID
  • anhydrous: 253881
RTECS number
  • anhydrous: VZ3150000
UNII
  • anhydrous: LC1V549NOM checkY
CompTox Dashboard (EPA)
  • anhydrous: DTXSID3034903 Edit this at Wikidata
InChI
  • InChI=1S/BrH.Na/h1H;/q;+1/p-1 checkY
    Key: JHJLBTNAGRQEKS-UHFFFAOYSA-M checkY
  • anhydrous: InChI=1/BrH.Na/h1H;/q;+1/p-1
    Key: JHJLBTNAGRQEKS-REWHXWOFAR
SMILES
  • anhydrous: [Na+].[Br-]
Properties
Chemical formula
 NaBr
Molar mass 102.894 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[3]
Boiling point 1,390 °C (2,530 °F; 1,660 K)[3]
Solubility in water
 71.35 g/100 mL (−20 °C)
79.52 g/100 mL (0 °C)
94.32 g/100 mL (25 °C)[1]
104.9 g/100 mL (40 °C)
116.2 g/100 mL (100 °C)[2]
Solubility Soluble in alcohol, liquid ammonia, pyridine, hydrazine, SO2
Insoluble in acetone, acetonitrile[1]
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)[1]
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)[1]
Solubility in formic acid 19.3 g/100 g (18 °C)
19.4 g/100 g (25 °C)[1]
Solubility in glycerol 38.7 g/100 g (20 °C)[1]
Solubility in dimethylformamide 3.2 g/100 g (10.3 °C)[1]
Vapor pressure 1 torr (806 °C)
5 torr (903 °C)[3]
Magnetic susceptibility (χ)
 −41.0·10−6 cm3/mol
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)[1]
Structure
Crystal structure
 Cubic
Lattice constant
a = 5.97 Å[4]
Thermochemistry
Heat capacity (C)
 51.4 J/(mol·K)[1]
Std molar
entropy (S⦵298)
 86.82 J/(mol·K)[1]
Std enthalpy of
formation (ΔfH⦵298)
 −361.41 kJ/mol[1]
Gibbs free energy (ΔfG⦵)
 −349.3 kJ/mol[1]
Pharmacology
Legal status
  • AU: S4 (Prescription only) /S5
Hazards
NFPA 704 (fire diamond)
[6]
NFPA 704 four-colored diamondHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
2
0
0
Flash point 800 °C (1,470 °F; 1,070 K)
Lethal dose or concentration (LD, LC):
LD50 (median dose)
 3500 mg/kg (rats, oral)
Safety data sheet (SDS) External MSDS
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).
☒N verify (what is checkY☒N ?)
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]

  1. ^ a b c d e f g h i j k l "Sodium bromide".
  2. ^ Seidell, Atherton; Linke, William F. (1919). Solubilities of Inorganic and Organic Compounds (2nd ed.). D. Van Nostrand Company.
  3. ^ a b c Pradyot, Patnaik (2003). Handbook of Inorganic Chemicals. The McGraw-Hill Companies, Inc. ISBN 978-0-07-049439-8.
  4. ^ a b "Sodium Bromide (NaBr)". korth.de. Korth Kristalle GmbH. Archived from the original on 2014-07-14. Retrieved 2014-06-11.
  5. ^ Polyanskiy, Mikhail. "Refractive index of NaBr (Sodium bromide) - Li". refractiveindex.info. Retrieved 2014-06-11.
  6. ^ Cite error: The named reference scl was invoked but never defined (see the help page).
  7. ^ 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

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