Henry's law about solubility of gases in liquids does not apply to the solubility of which gas due to reaction with water?

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Henry's law describes how a gas dissolves in a liquid when the process is purely physical and there’s no chemical reaction with the solvent. If the gas chemically reacts with water, the amount that dissolves is not determined solely by its partial pressure but also by the chemical equilibria that form ions like carbonic acid, bicarbonate, and carbonate. Carbon dioxide is the gas that reacts with water to form carbonic acid, which then dissociates in solution. This reaction network means the dissolved amount depends on pH and these equilibria, so the simple proportional relationship of Henry's law doesn’t apply in its straightforward form for CO2. In contrast, oxygen, nitrogen, and methane don’t react with water under normal conditions, so their dissolution in water is well described by Henry’s law.