Given below are two statements:
Statement-I: \( K_H \) is constant with change in concentration of gas till solution is dilute at a given temperature.
Statement-II: According to Henry’s Law, partial pressure of gas in vapor phase is inversely proportional to mole fraction of gas in solution.

Question

Which one of the following is not correct for an ideal solution?

Answer 1

Let's analyze each statement individually to determine their correctness in the context of Henry's Law:

Statement-I: \( K_H \) is constant with change in concentration of gas till solution is dilute at a given temperature.
- Henry's Law states that at a constant temperature, the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas over the liquid. This relationship is mathematically expressed as \( P = K_H \times x \), where \( P \) is the partial pressure, \( K_H \) is Henry's Law constant, and \( x \) is the mole fraction of the gas.
- The constant \( K_H \) is specific for a particular gas-solvent pair and remains constant as long as the temperature is constant and the solution is diluted. Thus, Statement-I is correct.
Statement-II: According to Henry’s Law, the partial pressure of gas in vapor phase is inversely proportional to mole fraction of gas in solution.
- As mentioned, Henry's Law indicates a direct proportionality between the partial pressure of a gas and its mole fraction in a solution: \( P = K_H \times x \).
- Since this relationship is direct, not inverse, Statement-II is incorrect because it incorrectly states an inverse relationship.

Based on the above analysis, the correct choice is: Statement-I is correct, Statement-II is incorrect.

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