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
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Plumbic Sulphate

Plumbic Sulphate, lead disulphate, Pb(SO4)2, is formed by the electrolytic oxidation of lead in presence of sulphuric acid. It was prepared by Elbs and Fischer by the electrolysis of sulphuric acid of density 1.7 to 1.8 with a lead anode. The temperature did not exceed 30° C., the current density was 0.02 to 0.06 ampere per sq. cm., and the anode was separated from the cathode by immersion in a porous pot containing a considerable volume of the acid. The anode mud contained 60 to 85 per cent, of plumbic sulphate; a purer product subsequently crystallised from the anode liquid. The crystals of plumbic sulphate were of a faintly greenish yellow tint, but yielded a practically white powder when dried on a porous plate. They could not, however, be completely freed from sulphuric acid.

One hundred c.c. of sulphuric acid dissolve about 0.345 gram of plumbic sulphate at 30° C. This salt is hydrolysed by water into sulphuric acid and lead dioxide; the same effect is produced more slowly by the action of sulphuric acid of density less than 1.65. Hydrolysis, however, takes place in two stages, the basic sulphate PbOSO4.H2O being an intermediate product.

Concentrated hydrochloric acid dissolves plumbic sulphate forming a yellow solution containing lead tetrachloride or chloroplumbic acid; glacial acetic acid also dissolves the salt at 40°-50° C., and white needles of the tetra-acetate crystallise from the solution on cooling. Sodium acetate solution likewise dissolves plumbic sulphate, forming sodium plumbi-acetate; double salts, such as K2Pb(SO4)3 and (NH4)2Pb(SO4)3, are also formed with sulphates of the alkali metals, ammonia, and amines. Cold concentrated sodium hydroxide solution forms sodium plumbate.

Plumbic sulphate resembles, but is more energetic than, lead dioxide as an oxidising agent; ferrous salts are oxidised to ferric, alcohol to aldehyde, and oxalic acid to carbon dioxide by this compound. These oxidations are accompanied by the separation of lead sulphate, without the appearance of the dioxide.

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