Calcium bromide

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Calcium bromide
IUPAC name
Calcium bromide
Other names
Calcium dibromide
7789-41-5 YesY
22208-73-7 (dihydrate) N
ChEBI CHEBI:31338 YesY
ChemSpider 23010 YesY
EC number 232-164-6
Jmol-3D images Image
PubChem 24608
RTECS number EV9328000
Molar mass 199.89 g/mol (anhydrous)
235.98 g/mol (dihydrate)
Appearance Odorless, very hygroscopic colorless crystals
sharp saline taste
Density 3.353 g/cm3
Melting point 730 °C (1,350 °F; 1,000 K)
Boiling point 1,935 °C (3,515 °F; 2,208 K) (anhydrous)
810 °C (dihydrate)
125 g/100 mL (0 °C)
143 g/100 ml (20 °C)
312 g/100 mL (100 °C)
Solubility in alcohol, acetone soluble
Acidity (pKa) 9
75 J/mol K
130 J/mol K
-647.9 kJ/mol
-656.1 kJ/mol
Main hazards Decomposes on heating at high temperature producing toxic and corrosive fumes
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g., chloroform Reactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogen Special hazards (white): no codeNFPA 704 four-colored diamond
Lethal dose or concentration (LD, LC):
4100 mg/kg (rat, oral)
1580 mg/kg (mouse, subcutaneous)
Related compounds
Other anions
Calcium fluoride
Calcium chloride
Calcium iodide
Other cations
Beryllium bromide
Magnesium bromide
Strontium bromide
Barium bromide
Radium bromide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
 N verify (what isYesY/N?)
Infobox references

Calcium bromide is the calcium salt of hydrobromic acid with the chemical formula of CaBr2. It is a white powder that reacts with water to form the hexahydrate. CaBr2 is mainly used in drilling fluid.[1]

Synthesis, structure, and reactions[edit]

It is produced by the reaction of calcium oxide, calcium carbonate with hydrobromic acid or the reaction of calcium metal with elemental bromine.[1]

It adopts the rutile structure, featuring octahedral Ca centres bound to six bromide anions, which also bridge to other Ca centres.

When strongly heated in air, calcium bromide will produce calcium oxide and bromine:

2 CaBr2 + O2 → 2 CaO + 2 Br2

In this reaction the oxygen oxidizes the bromide to bromine.


It is mainly used as dense aqueous solutions for drilling fluids.[1] It is also used in neuroses medication, freezing mixtures, food preservatives, photography and fire retardants.[2]


  1. ^ a b c Michael J. Dagani, Henry J. Barda, Theodore J. Benya, David C. Sanders “Bromine Compounds” Ullmann's Encyclopedia of Industrial Chemistry 2002, Wiley-VCH, Weinheim. doi:10.1002/14356007.a04_405
  2. ^ "Chemical Land 21". Retrieved 25 December 2008. 

External links[edit]