What does Henry's law state about the solubility of gases in liquids?

Henry's law specifically addresses the relationship between the solubility of a gas in a liquid and the partial pressure of that gas above the liquid. It states that the amount of gas that will dissolve in a liquid at a given temperature is directly proportional to the partial pressure of that gas in equilibrium with the liquid. Therefore, when the partial pressure of a gas increases, more of the gas will dissolve in the liquid, and conversely, if the partial pressure decreases, less gas will be present in the solution. This principle is crucial in understanding gas exchange processes in biological systems and various applications in fields like chemistry and environmental science.

In contrast, other options do not accurately reflect the interactions dictated by Henry's law. Option A incorrectly states that gas solubility is independent of partial pressure; this contradicts the core premise of the law. Option C mentions the temperature effect, which is a separate consideration—the relationship described by Henry's law holds true only at a constant temperature. Lastly, option D misinterprets the influence of the volume of liquid; while the volume can affect the absolute amount of gas that can dissolve, Henry's law focuses on the concentration of gas in terms of partial pressure.