Question

Solubility of a gas in liquid increases on:
(A) increasing temperature
(B) decreasing pressure
(C) increasing pressure
(D) increasing temperature and pressure

Answer 1

Hint: The solubility of a substance is more than can be dissolved in a specific amount of a solvent at a specified temperature and also depends upon the nature of the solute and solvent. Temperature and pressure also affect a solution of a solid or a gas in a liquid.

Complete step by step solution:
Most of the gases dissolve in water. For example oxygen gas dissolves to a small extent which is known as dissolved oxygen and on the other hand HCl gas is highly soluble in water.
The temperature and pressure are great impacts on the solubility of gases in liquids. Henry explained the relation between pressure and solubility of a gas in a liquid, which is known as Henry’s Law.
This law states that “the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas present above the surface of liquid or solution”. This Henry’s law applies to solutions at constant temperature and expressed as:
$p={{K}_{H}}x$
Where, p =partial pressure of a gas in the vapor phase,
x = mole fraction of the gas,
${{K}_{H}}$ = Henry’s law constant, which is a function of the nature of the gas.
From the above equation, the solubility of gases increases with an increase in pressure.

So, the correct answer is option C.

Note: There are more industrial applications of Henry’s law that to increase the solubility of carbon dioxide in soft drinks sealed under high pressure, the solubility of gases in liquids decreases with an increase in temperature.