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Chemical elements
  Tin
    Isotopes
    Energy
    Production
    Application
    Physical Properties
    Chemical Properties
      Tetramethyl Stannane
      Methyl stannic chloride
      Tin Tetra-ethyl
      Tin Tri-ethyl
      Stannous Fluoride
      Stannic Fluoride
      Sodium Stannifluoride
      Potassium Stannifluoride
      Ammonium Stannifluoride
      Stannous Chloride
      Stannic Chloride
      Chlorostannates
      Stannous Bromide
      Stannic Bromide
      Stannous Iodide
      Stannic Iodide
      Mixed Stannic Halides
      Stannous Oxide
      Stannous Hydroxide
      Stannic Oxide
      Potassium Stannate
      Stannic Acid and its Derivatives
      Parastannic Acid
      Stannyl Chloride
      Parastannyl Chloride
      Stannous Sulphide
      Stannic Sulphide
      Stannic Oxysulphide
      Stannic Iodosulphide
      Stannous Sulphate
      Stannic Sulphate
      Stannic Nitrate
      Stannous Nitrate
      Phosphor-tin
      Stannioxalic Acid
      Stannous Tartrate
      Tin and Silicon
      Stannous Tungstate
    PDB 3e94-3kwy

Chlorostannates

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Chlorostannic acid, H₂SnCl₆, exists, and from it are derived a number of salts, the stannichlorides.

Chlorostannic Acid, H₂SnCl₆.6H₂O, is formed when the solid pentahydrate SnCl₄.5H₂O, or a concentrated solution of the chloride is saturated with hydrogen chloride gas. It separates on cooling the liquid to 0° C. in thin plates, which melt at about 20° C. There is a marked similarity between this acid and its salts and chloroplatinic acid, H₂PtCl₆.6H₂O, and its salts, though the latter acid and its salts are the more stable.

Sodium Stannichloride, Na₂SnCl₆.5H₂O, crystallises in prisms when the concentrated solutions of the constituent salts are mixed together, the potassium salt K₂SnCl₆ crystallises in anhydrous regular octahedra, with which the ammonium salt (NH₄)₂SnCl₆ is isomorphous. This latter salt was formerly used by dyers, and was named pink salt, because of its use as a mordant for madder-red colours; it dissolves in 3 parts of water at 14.5° C., and from its dilute solution stannic hydroxide separates on boiling. A large number of stannichlorides have been prepared containing various amounts of water of crystallisation; the chlorides of barium, cadmium, copper, silver, lead, and thallium, however, appear not to combine with stannic chloride.