Henry's law

Henry's law states that, at constant temperature, the concentration of a dissolved gas is proportional to its partial pressure above the liquid. Its proportionality constant depends on the gas, solvent, and temperature.

Henry's law constant: A proportionality constant relating a gas’s partial pressure to its concentration or mole fraction in a liquid. Its value sets the numerical relationship between pressure and dissolved-gas concentration.
Carbon dioxide in seawater: The dissolution and chemical transformation of atmospheric carbon dioxide in ocean water. Air–sea carbon dioxide exchange uses pressure-dependent dissolution as its starting point.
Chemical potential: A thermodynamic measure of how a system’s energy changes when the amount of a component changes. Gas–liquid equilibrium occurs when the gas component has equal chemical potential in both phases.
Dalton's law of partial pressures: A rule that the total pressure of an ideal gas mixture equals the sum of its component partial pressures. It provides the component pressure used when applying Henry’s law to a gas mixture.
William Henry: An English chemist who studied gases and liquids and formulated the relation now known as Henry’s law. His experiments on gas absorption established the pressure–solubility relation.
Partial pressure: The pressure contributed by one gas in a mixture, equal to its mole fraction times total pressure for an ideal gas. The law uses the gas’s pressure contribution, not the mixture’s total pressure.
Oxygen in blood: The transport of oxygen in blood, chiefly bound to hemoglobin and partly dissolved in plasma. Henry’s law relates oxygen partial pressure to the small fraction dissolved in plasma.
Mole fraction: The number of moles of a mixture component divided by the total moles in the mixture. Some forms of Henry’s law relate gas pressure to its mole fraction in solution.
Non-ideal solution: A solution whose components do not obey ideal-mixture relations because intermolecular interactions affect their behavior. Non-ideal interactions can make dissolved concentration depart from a simple pressure proportionality.
Gas absorption experiments: Measurements of how much gas a liquid absorbs under controlled pressure and temperature. Henry’s relation arose from comparing absorbed gas amounts across pressures.

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