MHTCET 13 Apr 2026 Shift 2 Paper

Concept:Henry's law applies only to gases that dissolve without reacting chemically with the solvent.Explanation:Option A is true: solubility of gases in water usually decreases with rise in temperature.Option B is true: solubility of a gas in a liquid increases with increase in pressure.Option C is true: substances with similar intermolecular forces are generally soluble in each other, i.e., "like dissolves like".Option D is NOT true: gases like $\mathrm{NH}_{3}$ and $\mathrm{CO}_{2}$ do not strictly obey Henry's law because they react chemically with water.$\mathrm{NH}_{3}$ reacts with water as:$$\mathrm{NH}_{3}+\mathrm{H}_{2}\mathrm{O} \rightleftharpoons \mathrm{NH}_{4}\mathrm{OH}$$$\mathrm{CO}_{2}$ reacts with water as:$$\mathrm{CO}_{2}+\mathrm{H}_{2}\mathrm{O} \rightleftharpoons \mathrm{H}_{2}\mathrm{CO}_{3}$$Due to this chemical reaction, their solubility depends not only on pressure but also on reaction with water. Hence they do not follow Henry's law simply.Answer:Option D is the statement that is NOT true.