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Originally appearing in Volume V26, Page 1018 of the 1911 Encyclopedia Britannica.
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SOC . 1907, ii. 557.) See also:

Titanium fluoride, TiF4, is a fuming colourless liquid boiling at 284°, obtained by distilling a mixture of titanium See also:oxide, fluorspar and sulphuric See also:acid; by See also:heating See also:barium titanofluoride, BaTiF5 (Emrich, Monats., 1904, 25, p. 907) ; and by the See also:action of dry hydrofluoric acid on the chloride (See also:Ruff and See also:Plato, Ber., 1904, 37, p. 673). By dissolving the dioxide in hydrofluoric acid a syrupy See also:solution is obtained which probably contains titanofluoric acid, IhTiF6. The salts of this acid are well known; they are isomorphous with the silico-, stanno- and zircono-fluorides. They are obtained by neutralizing the solution of the acid, or by fusing the oxide with See also:potassium carbonate and treating the melt with hydrofluoric acid. Potassium titanofluoride. K2TiFs-See also:H2O, forms See also:white, shining, See also:monoclinic scales. When ignited in a current of See also:hydrogen it yields titanium trifluoride, TiF3, as a See also:violet See also:powder. Titanium chloride, TiC14, is obtained as a colourless fuming liquid of 1.7604 sp. gr. at o° C.. boiling at 116.4° under 753.3 mm. pressure (T.

E. See also:

Thorpe), by heating to dull redness an intimate dry mixture Of the oxide and ignited See also:lamp-See also:black in dry See also:chlorine. In the method of A. Stabler and H. Wirthwein, the titanium See also:mineral is fused withcarbon in the electric See also:furnace, the carbides treated with chlorine, and the titanium chloride condensed. The distillate is freed from See also:vanadium by digestion with See also:sodium See also:amalgam. Other methods are due to E. Vigouroux and G. Arrivaut (Abst. Journ. Chem. Soc., 1907, ii.

97, 270) and See also:

Ellis (ibid., p. 270). By passing See also:chloroform vapour over the heated dioxide the tetra- di- and tri-chlorides are formed, together with the See also:free See also:metal and a gaseous hydride, TiH4 (Renz, Ber., 1906, 39, p. 249). When dropped very cautiously into See also:cold See also:water it dissolves into a clear solution. According to the amount of water used, TiC13OH, TiCl2(OH)2, TiCI(OH)3 or titanic acid is formed. The solution when boiled deposits most of its oxide in the See also:meta-See also:hydrate See also:form. It forms addition compounds similar to those formed by stannic chloride, and combines with See also:ammonia to form TiCI4.8NH3 and TiC14.6NH3, both of which with liquid ammonia give titanamide, Ti(See also:NH2)4. Titanium dichloride, TiCl2, obtained by passing hydrogen over the trichloride at a dull red See also:heat, is a very hygroscopic See also:brown powder which inflames when exposed to See also:air, and energetically decomposes water. Titanium trichloride, TiCla, forms involatile, dark violet scales, and is obtained by passing the vapour of the tetrachloride mixed with hydrogen through a red-hot See also:tube, or by heating the tetrachloride with molecular See also:silver to 200°. It is a powerful reducing See also:agent. Titanium tetrabromide, TiBr4, is an See also:amber-coloured crystalline See also:mass.

The tetraiodide, TiI4, is a reddish brown mass having a metallic lustre. The di-iodide, TiI2, is obtained as black lamella by passing the vapour of the tetraiodide over heated See also:

mercury in an See also:atmosphere of hydrogen (E. Defacqz and H. Copaux, Compt. rend., 1908, 147, p. 65). Sulphides are known corresponding to the best-known oxides. Titanium sesquisulphate, Ti2(SO4)i.8H2O, obtained by concentrating the violet solution formed when the metal is dissolved in sulphuric acid, is interesting since it forms a See also:caesium See also:alum, CsTi(SO4)2.12H2O. It gives the normal sulphate as a yellow, deliquescent, amorphous mass when treated with nitric acid. Acid solutions of titanates are not precipitated by suiphuretted hydrogen ; but ammonium sulphide acts on them as if it were ammonia, the suiphuretted hydrogen being liberated. Titanium oxide when fused with microcosmic See also:salt in the oxidizing See also:flame yields a See also:bead which is yellowish in the heat but colourless after cooling. In the reducing flame the bead becomes violet, more readily on the addition of See also:tin; in the presence of See also:iron it becomes See also:blood-red. Titanic oxides when fused on See also:charcoal, even with potassium See also:cyanide, yield no metal.

See also:

Rose determined the atomic See also:weight to be 47.72 (H = i ). A redetermination in 1885 by T. E. Thorpe gave the value 47.7 (see Journ. Chem. Soc., 1885, p. 108).

End of Article: SOC

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