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Chapter 13: Problem 24

What is the effect of pressure on the solubility of a liquid in liquid and of a solid in liquid?

Short Answer

Expert verified
The solubility of a liquid in a liquid is not significantly affected by pressure. Increase in pressure usually increases the solubility of a solid in a liquid, but there can be exceptions.

Step by step solution

01

Pressure and Solubility of a Liquid in Liquid

According to the Le Chatelier's principle, increasing the pressure has no significant effect on the solubility of a liquid in another liquid. This is because liquids are virtually incompressible and a change in pressure does not significantly affect the volume or the structure of a liquid. Therefore, increasing or decreasing the pressure has no significant effect on the distribution of the solute between the two liquids.
02

Pressure and Solubility of a Solid in Liquid

According to Henry's Law, the solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid. Thus, increasing the pressure increases the solubility of a solid in a liquid. However, this rule only applies to gases. Solubility of solids in liquids can vary; in most cases it's increased by high pressure but there are exceptions.

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Most popular questions from this chapter

Acetic acid is a weak acid that ionizes in solution as follows: $$ \mathrm{CH}_{3} \mathrm{COOH}(a q) \rightleftharpoons \mathrm{CH}_{3} \mathrm{COO}^{-}(a q)+\mathrm{H}^{+}(a q) $$ If the freezing point of a \(0.106 \mathrm{~m} \mathrm{CH}_{3} \mathrm{COOH}\) solution is \(-0.203^{\circ} \mathrm{C},\) calculate the percent of the acid that has undergone ionization.

Which of these two aqueous solutions has (a) the higher boiling point, (b) the higher freezing point, and (c) the lower vapor pressure: \(0.35 \mathrm{~m} \mathrm{CaCl}_{2}\) or \(0.90 \mathrm{~m}\) urea? State your reasons.

A 0.86 percent by mass solution of \(\mathrm{NaCl}\) is called "physiological saline" because its osmotic pressure is equal to that of the solution in blood cells. Calculate the osmotic pressure of this solution at normal body temperature \(\left(37^{\circ} \mathrm{C}\right)\). Note that the density of the saline solution is \(1.005 \mathrm{~g} / \mathrm{mL}\).

How do the solubilities of most ionic compounds in water change with temperature?

Liquids A (molar mass \(100 \mathrm{~g} / \mathrm{mol}\) ) and \(\mathrm{B}\) (molar mass \(110 \mathrm{~g} / \mathrm{mol}\) ) form an ideal solution. At \(55^{\circ} \mathrm{C}\), A has a vapor pressure of \(95 \mathrm{mmHg}\) and \(\mathrm{B}\) has a vapor pressure of \(42 \mathrm{mmHg}\). A solution is prepared by mixing equal masses of \(\mathrm{A}\) and \(\mathrm{B}\). (a) Calculate the mole fraction of each component in the solution. (b) Calculate the partial pressures of \(\mathrm{A}\) and \(\mathrm{B}\) over the solution at \(55^{\circ} \mathrm{C}\). (c) Suppose that some of the vapor described in (b) is condensed to a liquid. Calculate the mole fraction of each component in this liquid and the vapor pressure of each component above this liquid at \(55^{\circ} \mathrm{C}\).
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