Which gas law explains the relationship between the amount of gas in a solution and its partial pressure?

Henry's Law describes the relationship between the amount of gas that dissolves in a liquid and the partial pressure of that gas above the liquid. According to this law, the amount of gas that will dissolve in a liquid at a constant temperature is directly proportional to the partial pressure of that gas in the atmosphere above the liquid. This principle is crucial in understanding various biological processes, including how gases are transported in the bloodstream and how they behave under different pressures and conditions, such as in diving or at altitude.

The other laws mentioned pertain to different gas behaviors. For example, Dalton's Law deals with the total pressure of a gas mixture and the contribution of individual gases to that pressure. Charles' Law relates temperature and volume of a gas at constant pressure. The Law of Gaseous Diffusion outlines how gases mix or move from areas of higher concentration to lower concentration. Each of these laws captures different aspects of gas behavior, but it is Henry's Law that specifically addresses the solubility of a gas in relation to its partial pressure.