Henry’s law statement

Henry’s law can be written as $p = K_H x$ where:

• $p$ = partial pressure of the gas,
• $x$ = mole fraction of the gas in solution,
• $K_H$ = Henry’s law constant.

Interpretation of $K_H$

From $x = \frac{p}{K_H}$ at a given pressure $p$, the solubility of gas in liquid is proportional to $x$ and hence $x \propto \frac{1}{K_H}$ Therefore, larger $K_H$ means lower solubility, not higher solubility.

Check each option

Option A: Higher the value of $K_H$ at a given pressure, higher is the solubility of the gas in the liquids.

• From $x=\frac{p}{K_H}$
• If $K_H$ increases, $x$ decreases.
• So this statement is incorrect.

Option B: Different gases have different $K_H$ values at the same temperature.

• True, because $K_H$ depends on the nature of the gas.
• So correct.

Option C: The partial pressure of the gas in vapour phase is proportional to the mole fraction of the gas in the solution.

• This is exactly Henry’s law: $p \propto x$
• So correct.

Option D: The value of $K_H$ increases with increase of temperature and $K_H$ is function of the nature of the gas.

• Gas solubility usually decreases with increase in temperature, so $K_H$ generally increases.
• Also, $K_H$ depends on the nature of gas.
• So correct.

Conclusion

The statement that is not correct is: $\boxed{A}$

Comparison with stored correct answer

Stored correct answer: A

My derived answer matches the stored answer.