What is the primary factor that influences gas solubility as described by Henry's Law?

Henry's Law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of that gas above the liquid. This means that as the pressure of the gas increases, its solubility in the liquid also increases. The relationship can be represented mathematically as ( C = k_H \cdot P ), where ( C ) is the concentration of the dissolved gas, ( k_H ) is Henry's law constant (specific to each gas at a given temperature), and ( P ) is the partial pressure of the gas.

In essence, the driving force for gas solubility lies in the tendency of the gas molecules to escape from the liquid into the gaseous phase. When the pressure on the gas is increased, more gas molecules collide with the surface of the liquid, leading to a greater number dissolving into the liquid until a new equilibrium is reached.

While temperature does influence gas solubility—generally, higher temperatures reduce the solubility of gases—Henry’s Law specifically emphasizes pressure as the primary factor for gas solubility in a liquid under equilibrated conditions. Concentration of solute and volume of solvent are relevant in many aspects of solutions but are not the primary factors