By B. Trémillon
Arising without doubt from its pre-eminence as a common liquid, water has continuously been thought of by means of chemists because the unique solvent within which very various chemical reactions can happen, either for preparational and for analytical reasons. This explains the very long-standing curiosity proven within the research of aqueous options. during this con nection, it has to be under pressure that the idea of Arrhenius and Ostwald (1887-1894) on electrolytic dissociation, used to be initially devised completely for ideas in water and that the 1st actual proposal of acidity due to this can be associated with using this solvent. The more moderen improvement of diverse physico-chemical dimension tools has made attainable a rise of information during this sector as much as a really complex measure of systematization. hence at the present time we have now to be had either a truly great amount of experimental info, including very sophisticated tools of deduction and of quantitative therapy of chemical reactions in answer which permit us to make the fullest use of this information. however, . it sounds as if really glaring at this time that there are various chemical tactics which can't occur in water, and that its use as a solvent imposes 2 advent barriers. with a purpose to triumph over those barriers, it was once usual that curiosity could be interested in solvents except water and that the hot chances hence unfolded can be explored.
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Additional info for Chemistry in Non-Aqueous Solvents
Lonophoric substances behave - at least in not too concentrated solution - like strong electrolytes. But it is found that an ionophoric substance, which behaves like a strong electrolyte in water, can, in another molecular solvent of lower dielectric constant, exhibit divergences from the conductivity law (1-1) similar to those observed for weak electrolytes. There can be no * In aqueous solution the concentration is generally expressed in mol 1-1 (molarity, M); in the case of solvents other than water this unit is often replaced by that of molality: the number of moles of solute per kilogram of solvent (mol kg-1).
A quantitative treatment of the reactions between acids and bases - leading to the combination of the hydrogen ions of the acid with the hydroxide anions of the base, to form molecules of water - based on the laws of chemical equilibria, then became possible. The idea of 'neutrality', the result of 'neutralization' of an acid by a base or vice versa was introduced. As far as aqueous solutions are concerned, this theory of Arrhenius showed itself to be satisfactory and completely acceptable. But it appeared inadequate when interest started to be taken in solvents other than water, and when attempts were made to rationalize the properties of acids and bases in all solvents.
When miscibility is not total, two immiscible liquid phases molten salt saturated with metal and metal saturated with molten salt - can appear. Bredig has shown that two categories of solution can be distinguished, depending on the state of the metal dissolved in the molten salt. The first category is that where the solutions retain the metallic character of the solute. Solutions of alkali metals in their halides are a typical example of this; they recall solutions of these metals in liquid ammonia.