Question

The value of Henry’s constant ${K_H}$ is:
A. Greater for gases with higher solubility.
B. Greater for gases with lower solubility.
C. Constant for all gases.
D. Not related to the solubility of gases.

Answer 1

Hint: We need to remember that the pressure will affects the solubility of solids or liquids by little amount whereas which has powerful effect on solubility of gases
If the solubility of gas increases, the partial pressure above the liquid also increases.
 We know Mathematically, Henry’s law is expressed as,
$P = {K_H}x$
Where,
P is the pressure.
X is the solubility of the gas in liquid.
${K_H}$ is Henry’s law constant.

Complete step by step answer:
Let us see Henry’s law statement:
The solubility of gas in liquid is directly proportional to the pressure of the gas which is in equilibrium with that liquid at constant temperature.
Rewrite the equation,
${{\text{K}}_{\text{H}}}{\text{ = }}\dfrac{{\text{P}}}{{\text{x}}}$
From the above equation it is clear, the Henry’s constant and solubility of the gas in liquid (x) are inversely proportional which means Henry’s constant is greater for the gases with lower solubility.

So, the correct answer is Option B.

Additional information:
We must know that Henry's law is applicable only in certain conditions. The conditions are,
It works only if the molecules are at equilibrium.
It does not work for gases at high pressure. For example, Nitrogen at high pressure it becomes soluble and it is harmful in the blood supply.
It does not work if there is a chemical reaction between the solute and solvent. For example, Hydrochloric acid reacts with water by a dissociation reaction to generate hydronium and chloride ions.

Note: Also we must know that the solubility means the maximum quantity of solute dissolved in a certain quantity of a solution.
Variation of the solubility of gas in liquid:
Temperature: The solubility of gas in liquid decreases as the temperature increases.
Pressure: The solubility of gas in liquid increases as the pressure increases.