Chemical elements
  Cerium
    Isotopes
    Energy
    Production
    Application
    Physical Properties
    Chemical Properties
      Cerous hydride
      Cerous fluoride
      Cerous chloride
      Cerous oxychloride
      Cerous bromide
      Cerous iodide
      Cerous perchlorate
      Cerous bromate
      Cerous iodate
      Cerous oxide
      Cerous sesquioxide
      Cerous hydroxide
      Cerous sulphide
      Cerous persulphide
      Cerous oxysulphide
      Cerous sulphite
      Cerous sulphate
      Cerous dithionate
      Cerous selenite
      Cerous selenate
      Cerous chromate
      Cerous molybdate
      Cerous tungstate
      Cerous nitride
      Cerous nitrite
      Cerous nitrate
      Cerous hypophosphite
      Cerous orthophosphate
      Cerous vanadate
      Cerous carbide
      Cerous silicide
      Cerous carbonate
      Cerous thiocyanate
      Cerous platinocyanide
      Cerous oxalate
      Cerous silicate
      Ceric fluoride
      Ceric chloride
      Ceric iodate
      Ceroceric oxide
      Ceroceric hydroxide
      Ceric oxide
      Cerium dioxide
      Ceria
      Ceric hydroxide
      Perceric hydroxide
      Ceric hydrosulphate
      Ceric sulphate
      Ceric selenite
      Ceric chromate
      Ceric molybdate
      Ceric nitrate
      Ceric ammonium nitrate
      Ceric orthophosphate
      Ceric dihydrogen arsenate
      Ceric carbonate
      Perceric carbonate
      Ceric acetate
      Ceric oxalate
      Ceric acetylacetonate
      Ceric borate
    PDB 1ak8-1n65

Ceric sulphate, Ce(SO4)2






Ceria is quantitatively converted into ceric sulphate when heated on a sand-bath with concentrated sulphuric acid. The salt, which is insoluble in the excess of acid, may be washed with glacial acetic acid and dried over potash, when it is obtained as a deep yellow, crystalline powder. When heated in the air, slight loss of weight is observed at 155°, and when heated to constant weight at 195° the basic sulphate 3CeO2.4SO3 is produced. On raising the temperature, further loss of sulphur trioxide occurs at 250°, and at 300° the loss in weight is continuous until cerium dioxide is left.

Ceric sulphate is very soluble in water, in which it forms a yellowish-brown, unstable solution. A concentrated solution of the salt in dilute sulphuric acid may be prepared either by dissolving the anhydrous salt in dilute sulphuric acid or by carefully dissolving ceric hydroxide in the same medium. When concentrated over sulphuric acid, sulphur-yellow, orthorhombic crystals of the tetrahydrate, Ce(SO4)2.4H2O, are obtained (bipyramidal; a:b:c = 0.717:1:0.471).

Ceric sulphate in solution readily hydrolyses, and, according to Wyrouboff and Verneuil, when diluted largely or warmed, a crystalline basic salt of the composition 2CeO2.2SO3.5H2O is obtained; from a dilute ice-cold solution the compound 4CeO2.3SO3.12H2O has been prepared, and from a saturated solution at 0° C. the compound 2CeO2.3SO3.4H2O. A physicochemical study of the hydrolysis has been made by Spencer, who could only prepare and characterise one basic salt at 25° C., viz. CeO2.SO3.2H2O.

Ceric potassium sulphate, Ce(SO4)2.2K2SO4.2H2O, is obtained in orange-yellow, monoclinic crystals (a:b:c = 1.216:1:2.093; β = 100°40'), scarcely soluble in water, by adding a solution of potassium sulphate to an acid solution of ceric sulphate.

Ceric ammonium sulphate, Ce(SO4)2.2(NH4)2SO4.2H2O, separates in yellow crystals when an acid solution of the mixed sulphates is evaporated: it is followed by orange-red crystals of the monoclinic (a:b:c = 0.6638:1:0.7838; β = 96°44') double salt Ce(SO4)2.3(NH4)2SO4.2H2O.

Ceric silver sulphate, 5Ce(SO4)2.3Ag2SO4, is obtained as an orange-yellow, crystalline precipitate by adding silver nitrate to a strongly acid solution of ceric sulphate. The salt slowly combines with 2H2O, and is decomposed by boiling water.


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