Chemical elements
    Physical Properties
    Chemical Properties
      Barium Hydride
      Barium Subfluoride
      Barium Fluoride
      Acid Barium Fluoride
      Barium Subchloride
      Barium Chloride
      Barium Bromide
      Barium Perbromides
      Barium Iodide
      Barium Periodides
      Barium Mixed Halides
      Barium Mixed Perhalides
      Barium Oxychloride
      Barium Hypochlorite
      Barium Chlorite
      Barium Chlorate
      Barium Perchlorate
      Barium Oxybromide
      Barium Hypobromite
      Barium Bromate
      Barium Perbromate
      Barium Oxyiodide
      Barium Iodate
      Barium Periodate
      Barium Manganites
      Barium Manganate
      Barium Permanganate
      Barium Suboxide
      Barium Oxide
      Barium Hydroxide
      Barium Peroxide
      Barium Peroxyhydrate
      Barium Tetroxide
      Barium Sulphide
      Barium Hydrosulphide
      Barium Polysulphides
      Barium Hydroxyhydrosulphide
      Barium Oxysulphides
      Barium Sulphite
      Barium Thiosulphate
      Barium Dithionate
      Barium Trithionate
      Barium Tetrathionate
      Barium Pentathionate
      Barium Sulphate
      Acid Barium Sulphates
      Barium Pyrosulphate
      Barium Persulphate
      Barium Selenide
      Barium Selenite
      Barium Selenate
      Acid Barium Selenate
      Barium Telluride
      Barium Tellurite
      Barium Tellurate
      Barium Chromite
      Barium Chromate
      Barium Dichromate
      Barium Potassium Trichromate
      Barium Chlorochromate
      Barium Perchromate
      Barium Molybdate
      Barium Permolybdate
      Barium Tungstate
      Barium Uranate
      Barium Diuranate
      Barium Peruranate
      Barium Nitride
      Barium Azide
      Barium Hexammoniate
      Barium Ammonium
      Barium Amide
      Barium Amidosulphonate
      Barium Imide
      Barium Imidosulphonate
      Barium Hyponitrite
      Barium Nitroxysulphite
      Barium Nitrososulphate
      Barium Nitrohydroxylaminate
      Barium Nitrite
      Barium Nitrate
      Barium Phosphide
      Barium Dihydrohypophosphite
      Barium Hydrophosphite
      Barium Hypophosphate
      Barium Orthophosphates
      Barium Pyrophosphate
      Barium Metaphosphate
      Basic Barium Phosphates
      Barium Thiophosphites
      Barium Thiophosphates
      Barium Selenophosphates
      Barium Azophosphates
      Barium Phosphimates
      Barium Arsenide
      Barium Orthoarsenite
      Barium Pyroarsenite
      Barium Orthoarsenates
      Barium Pyroarsenate
      Barium Thioarsenites
      Barium Thioarsenates
      Barium Sodium Selenoxyarsenate
      Barium Metantimonate
      Barium Thioantimonites
      Barium Chloroantimonite
      Barium Orthothioantimonate
      Barium Hypovanadate
      Barium Vanadates
      Barium Metapervanadate
      Barium Niobate
      Barium Tantalate
      Barium Pertantalate
      Barium Carbide
      Barium Carbonyl
      Barium Formate
      Barium Acetate
      Barium Oxalate
      Barium Carbonate
      Barium Thiocarbonate
      Barium Percarbonate
      Barium Cyanide
      Barium Cyanamide
      Barium Cyanate
      Barium Cyanurate
      Barium Thiocyanate
      Barium Selenocyanate
      Barium Silicide
      Barium Silicates
      Barium Fluosilicate
      Barium Stannate
      Barium Orthoplumbate
      Barium Titanate
      Barium Peroxide Pertitanate
      Barium Pertitanate
      Barium Fluoroxytitanate
      Barium Zirconate
      Barium Boride
      Barium Borates
      Barium Fluorborate
      Barium Perborate
      Barium Aluminates
      Barium Ferrite
      Barium Ferrate
      Barium Gobaltite
      Barium Dinickelite
      Barium Platinate
    Detection of Barrium
    PDB 1djh-3iqp
    PDB 3iqr-4e7y

Barium Bromide, BaBr2

Barium Bromide, BaBr2, may be formed by the action of hydro-bromic acid on barium carbonate, by the precipitation of ferrous bromide with barium hydroxide or carbonate, by the action of a solution of bromine on barium sulphide, by the action of bromine on barium hydroxide and extraction by alcohol of the bromide from admixture with bromate, or, finally, by calcination of barium bromate. To obtain the anhydrous salt the solution formed by most of these methods is evaporated to dryness and heated to a little above 130° C. It is a white deliquescent substance of density 4.79 at 24° C. It melts at 880° C., and sublimes at 820° C. The heat of formation is 179.82 Cal., and the heat of solution 4.98 Cal.

The following values have been found for the solubility at different temperatures: -

Temperature, °C-20-97161940717677104145160175
Grams BaBr2 per 100 grams solution.45.746.548.548.849.350.955.155.555.656.660.559.460.3

Milikan determined the concentration of solutions in contact with ice at different temperatures.

Temperature, °C-3.9-14.1–21.1
Grams BaBr2 per 100 grams solution17.838.244.6

The cryohydric temperature is – 22.6° C., the concentration of the solution being 46.6 per cent, of barium bromide.

The solubility is diminished by the presence of the barium or bromine ion. The effect of barium iodide has been studied by Etard.

The properties of barium bromide solutions have been investigated from the point of view of density, vapour pressure, electrical conductivity, freezing-point, and refractive index.

An aqueous solution of barium bromide is decomposed by carbon dioxide with the formation of bromine and barium carbonate.

Barium bromide is soluble in both ethyl and methyl alcohol, but more so in the latter than the former.

Hydrates of Barium Bromide

From saturated solutions at ordinary temperatures the dihydrate separates out in rhombic or monoclinic crystals, which are rather hygroscopic, but do not liquefy under ordinary atmospheric conditions, and which have a density of 3.852 at 24° C. At red heat the hydrated salt is slightly decomposed with loss of bromine. It is isomorphous with barium chloride dihydrate. The solubility in methyl alcohol, which is considerable, decreases with the addition of water, reaching a minimum at about 50 per cent, of alcohol.

The heat of solution of the dihydrate is –4.130 Cal., and, therefore, since the heat of solution of the anhydrous salt is 4.98 Cal., the heat of hydration is 9.11 Cal.

The dihydrate is in equilibrium with the monohydrate, BaBr2.H2O, at about 70° C. In dry air the dihydrate may be reduced to the monohydrate at ordinary temperatures. By heating to 100°-130° C. the anhydrous salt is obtained.

Addition Compounds of Barium Bromide

By the action of pure dry ammonia on dry barium bromide the compound BaBr2.8NH3 is formed. Its dissociation pressure is 760 mm. at 35-4° C. An addition compound with glycine is also formed, of composition BaBr2.2NH3CH2COOH.H2O.

Double Salts of Barium Bromide

The following double salts have been mentioned: BaRhBr5, BaBr2.HgBr2, BaBr2.2Hg(CN)2.6H2O or 7H2O, and BaBr2.2KBr.
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