MHTCET 11 Apr 2026 Shift 2 Paper

Concept:Henry's law states that at constant temperature, the concentration of a gas dissolved in a liquid is directly proportional to its partial pressure.Explanation:Since $K_H$ is given in $\mathrm{mol\ dm}^{-3}\ \mathrm{atm}^{-1}$, the concentration is calculated using the direct relation:$C = K_H \times P$Where:$C$ = concentration of the dissolved gas$K_H$ = Henry's law constant $= 0.15\ \mathrm{mol\ dm}^{-3}\ \mathrm{atm}^{-1}$$P$ = partial pressure of the gas $= 0.18\ \mathrm{atm}$Substitute the given values into the formula:$C = 0.15 \times 0.18$$C = 0.027\ \mathrm{mol\ dm}^{-3}$Since $1\ \mathrm{mol\ dm}^{-3} = 1\ \mathrm{M}$ (molarity), the concentration is:$C = 0.027\ \mathrm{M}$Answer:The concentration of the gas dissolved at $25^\circ\mathrm{C}$ is $0.027\ \mathrm{M}$.Hence, the correct option is Option A: 0.027 M.