Henry's Law

States that, at equilibrium and constant temperature, the concentration of a dissolved non-reactive gas in a liquid is proportional to the partial pressure of that gas above the liquid.

At low concentration and equilibrium between a gas and a liquid at fixed temperature, the concentration of a dissolved gaseous species in the liquid phase (c_i or x_i at infinite dilution) is proportional to its partial pressure in the contacting gas phase (p_i) via a proportionality constant known as a Henry’s constant (H_i): c_i = H_i·p_i or, in an alternative form, p_i = k_H·c_i.

Henry’s Law states that, at equilibrium and for relatively dilute gases that do not react with the solvent, the concentration of a dissolved gas in a liquid is proportional to its partial pressure in the contacting gas phase (c = k_H·p), where k_H (the Henry constant) depends on temperature and the specific gas–solvent pair.