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Henry's law for the solubility of a gas in a liquid is best stated as:
AThe solubility of a gas is independent of its partial pressure
BThe partial pressure of the gas in the vapour phase is proportional to its mole fraction in the solution, $p = K_H x$
CThe solubility of a gas equals its mole fraction at all pressures
DThe solubility of a gas increases with rise in temperature
Answer & Solution
Correct answer: B. The partial pressure of the gas in the vapour phase is proportional to its mole fraction in the solution, $p = K_H x$
Henry's law: $p = K_H x$, where $p$ is the partial pressure of the gas above the solution, $x$ is the mole fraction of the dissolved gas, and $K_H$ is the Henry's law constant. A larger $K_H$ for a given $p$ means a smaller $x$, so a larger $K_H$ corresponds to *lower* solubility — the OCR's mention of 'greater $K_H$ greater solubility' is misleading. Solubility of a gas decreases with rising temperature.
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