The correct option is Henry’s law.
Explanation
The question pertains to the quantitative relationship between the solubility of a gas in a liquid solvent and the pressure exerted by that gas. This relationship is fundamental to understanding the behavior of solutions containing volatile solutes or dissolved gases.
Detailed Analysis:
- Henry’s Law (Correct): This law states that at a constant temperature, the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas present above the surface of the liquid or solution. The most common mathematical expression is p = KH · x, where p is the partial pressure of the gas in the vapour phase, x is the mole fraction of the gas in the solution, and KH is the Henry’s law constant.
- Raoult’s Law: This law relates the partial vapour pressure of a volatile component (usually a liquid) in a solution to its mole fraction in the solution. It is expressed as p = p⁰ · x. While mathematically similar to Henry's Law, Raoult's Law is generally applied to liquid-liquid solutions or solid-liquid solutions involving volatile solvents, whereas Henry's Law specifically addresses the solubility of gases in liquids.
- Dalton’s Law: This law relates to a mixture of non-reacting gases. It states that the total pressure exerted by the mixture is equal to the sum of the partial pressures of individual gases. It does not relate gas pressure to its concentration in a liquid solution.
- Boyle’s Law: This law describes the relationship between the pressure and volume of a fixed mass of gas at a constant temperature (PV = constant). It deals exclusively with the gaseous state, not solutions.
Key Takeaway:
Henry’s Law specifically governs the solubility of gases in liquids, establishing that the partial pressure of the gas is proportional to its mole fraction in the solution (p ∝ x).