Barium bromide

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Barium bromide
10553-31-8 (anhydrous) N
7791-28-8 (dihydrate) N
ChemSpider 59728 YesY
Jmol interactive 3D Image
BaBr2 (anhydrous)

BaBr2·2H2O (dihydrate)

Molar mass 297.14 g/mol
Appearance White solid
Density 4.78 g/cm3 (anhydrous)
3.58 g/cm3 (dihydrate)
Melting point 857 °C (1,575 °F; 1,130 K)
Boiling point 1,835 °C (3,335 °F; 2,108 K)
92.2 g/100 mL (0°C)
orthorhombic, oP12
Pnma, No. 62
−181.1 kcal/mol
Harmful (Xn)
R-phrases R20, R22
S-phrases S28[1]
Related compounds
Other anions
Barium fluoride
Barium chloride
Barium iodide
Other cations
Beryllium bromide
Magnesium bromide
Calcium bromide
Strontium bromide
Radium bromide
Lead bromide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Barium bromide is the chemical compound with the formula BaBr2. Like barium chloride, it dissolves well in water and is toxic in aqueous solution.

Structure and properties[edit]

BaBr2 crystallizes in a lead chloride motif, giving white orthorhombic crystals which are deliquescent.[2] In aqueous solution BaBr2 behaves as a simple salt.

Barium bromide reacts with the sulfate ion from sulfuric acid to produce a precipitate of barium sulfate.

BaBr2(aq) + SO42− → BaSO4(s) + 2 Br(aq)

Similar reactions occur with oxalic acid, hydrofluoric acid, and phosphoric acid.


Barium bromide can be prepared from barium sulfide or barium carbonate via reaction with hydrobromic acid to give hydrated barium bromide. This happens over a short period of time

BaS + HBr → BaBr2 + H2S
BaCO3 + HBr → BaBr2 + CO2 + H2O

Barium bromide can be crystallized out from the solution in its dihydrate form, BaBr2·2H2O, which gives the anhydrous form upon heating to 120 °C.[3]


Barium bromide is a precursor to chemicals used in photography and to other bromides.
Historically, barium bromide was used to purify radium in a process of fractional crystallization devised by Marie Curie. Since radium precipitates preferentially in a solution of barium bromide, the ratio of radium to barium in the precipitate would be higher than the ratio in the solution.[4]


Barium bromide, along with other water-soluble barium salts, is toxic and can cause severe poisoning if ingested.


  1. ^
  2. ^ Brackett, Elizabeth B.; Breackett, Thomas E.; Sass, Ronald L. (December), "The Crystal Structures of Barium Chloride, Barium Bromide, and Barium Iodide.", The Journal of Physical Chemistry (– Scholar search) 67 (published 1963), p. 2132, retrieved 2007-12-03  Check date values in: |date= (help)[dead link]
  3. ^ Patnaik, Pradyot (2003), Handbook of Inorganic Chemical Compounds, McGraw-Hill Professional, pp. 81–82, ISBN 0-07-049439-8, retrieved 2007-12-03 
  4. ^ Sime, Ruth Lewin (1996), Lise Meitner: A Life in Physics, University of California Press, p. 233, ISBN 0-520-20860-9, retrieved 2007-12-03