Caesium bromide fluoride

More and more, however, other solvents are coming into use in the laboratory and in industry. Aside from organic solvents such as alcohols, acetone, and hydrocarbons, which have been in use for many years, industrial processes use such solvents as sulfuric acid, hydrogen fluoride, ammonia, molten sodium hexafluoroaluminate (cryolite), various other ionic liquids (Welton, 1999), and liqnid metals, lander and Lafrenz (1970) cite the industrial use of bromine to separate caesium bromide (sol y 19.3g/100g bromine) from the much less soluble rubidium salt. The list of solvents available for preparative and analytical purposes in the laboratory now is long and growing, and though water will still be the first solvent that comes to mind, there is no reason to stop there. 

The Equation of State of the Alkali Halides.—The alkali halides, the fluorides, chlorides, bromides, and iodides of lithium, sodium, potassium, rubidium, and caesium have been more extensively studied experimentally than any other group of ionic crystals. For most of these materials, enough data are available to make a fairly satisfactory comparison between experiment and theory. The observations include the compressibility and its change with pressure, at room temperature, from which the quantities ai(T), o2(r) of Eq. (1.1), Chap. XIII, can be found... 

Reaction of a mixture containing hexafluoroacetone and caesium fluoride with allyl bromide or chloride occurs readily [131, 132] (Figure 8.31) but the mixture does not react with trimethylchlorosilane [131]. 

Caesium fluoridejtetra-n-butylammonium bromide or Aliquot 336 Mild, heterogeneous nucleophilic substitution with fluoride ion in the absence of solvent... 

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