Hydrogen chloride, in water

If, for a given acid, we wish to increase the acid strength, then we choose a solvent which has a greater affinity for protons than has water. If we add ammonia to a solution of hydrogen chloride in water, the essential equilibrium is... 

Solution of Gases in Liquids Certain gases will dissolve readily in hquids. In some cases in which the quantities are not large, this may be a practical storage procedure. Examples of gases that can be handled in this way are ammonia in water, acetylene in acetone, and hydrogen chloride in water. Whether or not this method is used depends mainly on whether the end use requires the anhydrous or the liquid state. Pressure may be either atmospheric or elevated. The... 

Solubility in water.—The solubility of hydrogen chloride in water at different temp, and press, has been investigated by H. E. Roscoe and W. Dittmar,1 who found results which may be expressed in several different ways (press. 760 mm.). Let C denote the volumes of gas in c.c. per 100 c.c. of water Cx grms. of HC1 per 100 grms. of water and C2 grms. of HC1 per 100 grms. of soln. 

All three hydrates have been isolated in the form of white crystalline solids. With more cone. soln. the liquid separates into two layers on cooling. The lighter liquid is almost pure hydrogen chloride with very little dissolved water. Soln. with between 67 and 99 per cent, hydrogen chloride do not exist at low temp. The solubility of water in liquid hydrogen chloride, LK, is less than 0 1 per cent, at 0°, and at the most 0 2 per cent, at 30°. The lower aq. layer, GH, represents soln. of liquid hydrogen chloride in water, which decreases with rise of temp. ... 

Below —15°, the aq. layer freezes to crystals of the monohydrate. The solubility curves HG and LK do not approach a critical soln. temp, with rising temp. at 54-5°, the HC1 layer vanishes, on account of its proximity to the critical temp, of hydrogen chloride. The curve LM represents the solubility of the monohydrate in liquid hydrogen chloride. The existence of an octohydrate, HC1.8H20, has been inferred from the heat of soln. of hydrogen chloride in water but it is quite an imaginary hydrate, for it has not been isolated. If it does exist, its presence is not... 

What is the solubility of hydrogen chloride in water What is the composition of an azeotropic mixture of hydrochloric acid with water What is called an azeotropic mixture of liquids and how does it differ from the pure liquids ... 

The fogging of the breath is possible because of the extreme solubility of hydrogen chloride in water. The fog then consists of countless minute globules of hydrochloric acid solution. 

B. ABSORPTION OF HYDROGEN CHLORIDE IN WATER 1. Theoretical principles of absorption... 

Absorption of a gas in a liquid for example, ammonia in water, carbon dioxide in water, hydrogen chloride in water. 

Henry s law is obeyed most accurately for dilute solutions of gases that do not dissociate in or react with the solvent. For example, Henry s law is obeyed by oxygen gas in water, but it does not correctly represent the behavior of gaseous hydrogen chloride in water because of the dissociation reaction ... 

Derivation Dissolving hydrogen chloride in water at various concentrations. 

Fig. 2. The Concentration Dependence of the Rational Activity Coefficient, f, of Hydrogen Chloride in Water, Methyl and Ethyl Alcohol.

Figure 9.10-2 Mean molar activity coefficient for hydrogen chloride in water at 25°C as a function of the square root of the ionic strength I = Mna- Points are the experimental data, and the lines are the results of various models.

Evaluate the diffusion coefficient of hydrogen chloride in water at 420 K and 1.2 bar. The data required to use Brokaw s relation (see Problem 1.14) are shown below (Reid, et al., 1987) ... 

The mechanism of the ionization of hydrogen chloride in water may be expressed similarly. The water molecules play the same part as the ammonia forming the hydrate... 

The state of substances in solution will now be taken up briefly. The electrolytic dissociation of a large number of substances is dependent evidently upon the properties of the solvent as well as upon the character of the dissolved substance (solute), because on the one hand all substances do not ionize in a solvent such as water, and on the other hand, a substance may ionize in one solvent, hydrogen chloride in water, and not in a different solvent, hydrogen chloride in benzene. The solvent must, therefore, also be considered in the ionization relationships and the manner in which it may be done follows directly from what has been said. 

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