Chemical elements
    Physical Properties
    Chemical Properties
      Titanium Trifluoride
      Titanium Tetrafluoride
      Hydrofluotitanic acid
      Potassium Titanifluoride
      Sodium Titanifluoride
      Titanium Dichloride
      Titanium Trichloride
      Titanium Tetrachloride
      Titanic Chloride
      Titanium Oxychlorides
      Hydrochlorotitanic Acid
      Addition Compounds of Titanium Tetrachloride
      Titanium Tribromide Hexahydrate
      Titanium Tetrabromide
      Titanic Bromide
      Hydrobromotitanic Acid
      Titanium Chlorobromides
      Titanium Di-iodide
      Titanium Tri-iodide
      Titanium Tetra-iodide
      Titanic Iodide
      Titanium Monoxide
Titanium Sesquioxide
      Titanium Dioxide
      Titanic Oxide
      Titanic Hydroxides
      Metatitanic Acid
      Titanium Monosulphide
      Titanium Sesquisulphide
      Titanium Disulphide
      Titanium Sulphates
      Titanous Sulphate
      Titanium Sesquisulphate
      Complex Sulphates of Tervalent Titanium
      Normal Titanic Sulphate
      Potassium Titanisulphate
      Potassium and Ammonium Titanylsulphates
      Titanous Nitride
      Titanic Nitride
      Titanium Nitrogen Halides
      Titaninitric Acid
      Titanium Phosphide
      Titaniphosphoric Acid
      Titanium Carbide
      Titanium Cyanonitride
      Titanium Thiocyanates
      Titanium Sesquioxalate
      Titanitartrates and Allied Salts
      Titanium Silicide

Titanic Hydroxides

The ortho- and meta- hydroxides, Ti(OH)4 and TiO(OH)2, are generally believed to exist, and there are probably other hydroxides which are of the nature of condensed acids. There are no natural titanates which reach the degree of complexity shown by the natural silicates, neither is a form of titanic acid known which is definitely analogous to β-stannic acid, Sn5O5(OH)10; nevertheless, as will appear, there is reason to believe that titanic acid may exist in complex molecules.

Orthotitanic acid, Ti(OH)4, is obtained as a voluminous, white precipitate when ammonia or alkali hydroxide or carbonate is added to a cold hydrochloric acid solution of a titanate. Whilst it remains fully hydrated it is soluble in dilute hydrochloric, sulphuric, and strong organic acids, forming the corresponding salts, but on heating it loses water and passes into more complex and less soluble hydrates. Even in contact with water it gradually passes into the meta-acid, and on ignition forms the dioxide with evolution of light.

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