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• Physical Properties

  The anhydrous sulfate is a colorless rhombohedral crystalline solid; refractive index 1.658; density 3.54 g/cm3; decomposes at 600°C; soluble in water, methanol, and glycerol.
  The heptahydrate, ZnSO4•7H2O, is a colorless crystalline solid; metallic taste; rhombohedral crystals; effloresces; refractive index 1.457; density 1.957 g/cm3 at 25°C; melts at 100°C; loses all its water molecules at 280°C; decomposes above 500°C; very soluble in water, 96.5 g/100mL at 20°C; soluble in glycerol, 40 g/100 mL; insoluble in alcohol.
  The hexahydrate, ZnSO4•6H2O constitutes colorless monoclinic or tetragonal crystals; density 2.072 g/cm3 at 15°C; loses five water molecules at 70°C; soluble in water. ;

• Occurrence and Uses

  Zinc sulfate occurs in nature as the mineral, zinkosite. The heptahydrate, ZnSO4•7H2O is the mineral, goslarite. The salt is used as a mordant in calicoprinting, in making rayon, in preserving wood, in animal feeds, in electroplating, and in preparing many zinc compounds. ;

• Production

  Zinc sulfate is produced as an intermediate in recovering zinc from mineral zinc blende, ZnS (see Zinc, Recovery). The mineral is roasted at about 1,000°C to form zinc oxide and sulfur dioxide which, on prolonged heating in excess air, converts to zinc sulfate:
  2ZnS + 3O2 → 2ZnO + 2SO2
  2ZnO + 2SO2 + O2 → 2ZnSO4
  In the zinc recovery process, roasted products are leached with sulfuric acid, whereupon zinc oxide is converted to sulfate.
  ZnO + H2SO4 → ZnSO4 + H2O
  Also, zinc sulfate can be prepared by reacting metallic zinc with dilute sulfuric acid followed by evaporation and crystallization:
  Zn + H2SO4 → ZnSO4 + H2 ;

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