Chemical elements
    Physical Properties
    Chemical Properties
      Lead Tetramethyl
      Lead Tetraethyl
      Lead Tetraphenyl
      Lead Ethoxide
      Lead Fluoride
      Lead Tetrafluoride
      Hydrofluoplumbic Acid
      Lead Chloride
      Lead Chloride Double Salts
      Basic Lead Chlorides
      Lead Tetrachloride
      Ammonium Plumbichloride
      Lead Chlorite
      Lead Chlorate
      Lead Perchlorate
      Lead Dibromide
      Double Salts of Lead Bromide
      Basic Lead Bromides
      Lead Bromate
      Lead Iodide
      Lead Iodide Complex Salts
      Basic Lead Iodides
      Lead Tetra-iodide
      Lead Iodate
      Lead Periodates
      Lead Suboxide
      Lead Monoxide
      Lead Hydroxides
      Lead Dioxide
      Plumbic Acids
      Hexahydroxyplumbic Acid
      Colloidal Plumbic Acid
      Potassium Plumbate
      Lead Plumbate
      Calcium Orthoplumbate
      Lead Orthoplumbate
      Red Lead
      Metaplumbic Acid
      Calcium Metaplumbate
      Lead Metaplumbate
      Basic Lead Plumbate
      Lead Sulphide
      Lead Sulphohalides
      Lead Polysulphide
      Lead Sulphite
      Lead Sulphates
      Lead Sulphate
      Basic Lead Sulphates
      Lead Hydrogen Sulphate
      Plumbic Sulphate
      Lead Persulphate
      Lead Thiosulphate
      Lead Dithionate
      Lead Selenide
      Lead Selenite
      Lead Selenate
      Lead Telluride
      Lead Tellurite
      Lead Azide
      Lead Azoimide
      Lead Hydrazoate
      Lead Imide
      Lead Hyponitrite
      Lead Nitrites
      Lead Nitrate
      Lead saltpetre
      Basic Lead Nitrates
      Lead Hypophosphite
      Lead Phosphite
      Lead Orthophosphate
      Lead Monohydrogen Phosphate
      Lead Dihydrogen Phosphate
      Lead Pyrophosphate
      Lead Metaphosphate
      Lead Arsenite
      Lead Orthoarsenate
      Lead Hydrogen Arsenate
      Lead Pyroarsenate
      Lead Antimonate
      Lead Carbonate
      White Lead
      Lead Formate
      Lead Acetate
      Sugar of Lead
      Complex Lead Acetates
      Plumbic Acetate
      Lead Tetra-acetate
      Lead Oxalate
      Lead Tartrate
      Lead Silicates
      Lead Borates
      Normal Lead Chromate
      Lead Dichromate
      Basic Lead Chromate
      Lead Molybdate
      Lead Tungstate
      Lead Metatungstate
      Lead Diuranate
      Lead Peruranate
    PDB 1afv-3qjk

Lead Dibromide, PbBr2

Lead Dibromide, PbBr2, resembles the corresponding chloride, and is prepared by dissolving lead oxide in hydrobromic acid and crystallising the solution, or by precipitating a lead salt with potassium bromide solution. It crystallises from hot water in white needles, which belong to the rhombic system, and have a density of 6.63.

If hydrobromic acid solution is added in excess to a 0.5 per cent, solution of lead bromide in hot water, needle-shaped crystals separate on cooling, which have the composition PbBr2.3H2O.

Various observations have been made upon the melting-point of this salt, which lies between 480° C. and 499° C. When fused it is a red liquid, solidifying to a white, horny mass; if, however, it is melted in moist air it emits white fumes and forms an oxybromide. The boiling-point of lead bromide is about 920° C., and its molecular heat of formation from the metal and liquid bromine is 75,000 calories (Berthelot), or 64,450 calories (Thomsen). This salt slowly darkens in the light owing to the separation of metal.

The solubility of lead bromide in water increases rapidly with rising temperature as the following figures show:

Temp. ° C.015253545556580100
Grams PbBr2 in 100 grams H2O0.45540.73050.97441.32201.74572.13762.5743.3434.751

In general, the solubility of lead bromide in hydrochloric, nitric, and acetic acids, as well as in ammonium chloride solution, is greater than in water; but the solubility of this compound in hydrogen bromide solution is analogous to that of lead chloride in hydrochloric acid; that is to say it is less soluble in dilute hydrogen bromide solution than in pure water - 1 litre of 0.5 normal solution of HBr dissolves only 1.25 gram PbBr2 at 11° C., whilst a litre of water at the same temperature dissolves 6 grams - but more soluble in a concentrated solution than in pure water, owing to the formation of complex ions.

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