Chemical elements
    Physical Properties
    Chemical Properties
      Iridium Monochloride
      Iridium Dichloride
      Iridium Trichloride
      Potassium Chloriridite
      Sodium Chloriridite
      Ammonium Chloriridite
      Aquo Chloriridites
      Iridium Tetrachloride
      Potassium Chloriridate
      Sodium Chloriridate
      Ammonium Chloriridate
      Silver Chloriridate
      Thallium Chloriridate
      Iridium Tribromide
      Iridium Tetrabromide
      Potassium Bromiridate
      Sodium Bromiridate
      Ammonium Bromiridate
      Iridium Oxybromide
      Iridium Tri-iodide
      Potassium Iodiridite
      Iridium Tetra-iodide
      Potassium Iodiridate
      Iridium Monoxide
      Iridium Sesquioxide
      Iridium Dioxide
      Iridium Trioxide
      Iridium Monosulphide
      Iridium Sesquisulphide
      Iridium Disulphide
      Iridium Sesquisulphite
      Potassium Iridium Sulphite
      Iridium Sesquisulphate
      Potassium Iridium Alum
      Ammonium Iridium Alum
      Caesium Iridium Alum
      Rubidium Iridium Alum
      Iridium Disulphate
      Iridium Sesquiselenide
      Hydrogen Iridi-nitrite
      Potassium Iridi-nitrite
      Sodium Iridi-nitrite
      Ammonium Iridi-nitrite
      Hydrogen Iridicyanide
      Potassium Iridicyanide
      Barium Iridicyanide
    PDB 1c1k-4enb

Iridium Disulphate, Ir(SO4)2

Iridium Disulphate, Ir(SO4)2, is obtained as a yellowish brown, amorphous mass on oxidising iridium sulphide with concentrated nitric acid.3 On gently warming, the reaction takes place with vigour, and, when complete, the nitrous fumes are expelled by repeated evaporation and re-solution in water.

It does not appear to yield double salts, and on warming with, concentrated sulphuric acid yields iridium sesquisulphate.

Complex Iridium Disulphates

Two series of salts known as disulphates have been prepared, namely:
  1. Green salts of the type M2[Ir(SO4)2.OH.H2O], and
  2. Reddish brown salts of the type M3[Ir(SO4)2.(OH)2], where M stands for a monovalent metal.

Of these the former salts are usually acidic, whilst the latter are basic. They are readily converted, the one into the other, by addition of acid or base, as occasion requires. Several such salts have been prepared.
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