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Question
Assertion (A): The enthalpy of mixing Δmix H is equal to zero for an ideal solution.
Reason (R): For an ideal solution the interaction between solute and solvent molecules is stronger than the interactions between solute-solute or solvent-solvent molecules.
Options
Both (A) and (R) are true and (R) is the correct explanation of (A).
Both (A) and (R) are true, but (R) is not the correct explanation of (A).
(A) is true, but (R) is false.
(A) is false, but (R) is true.
Solution
Both (A) and (R) are true and (R) is the correct explanation of (A).
Explanation:
For an ideal solution, the enthalpy of mixing and the volume of mixing are both zero. This is because the intermolecular forces of attraction between two solute particles and two solvent particles are the same as the forces of attraction between a solute particle and a solvent particle.
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Vapour pressure of pure acetone and chloroform at 328 K are 741.8 mm Hg and 632.8 mm Hg respectively. Assuming that they form ideal solution over the entire range of composition, plot `"P"_"total"`, `"P"_"chloroform"` and `"P"_"acetone"` as a function of `"x"_"acetone"`. The experimental data observed for different compositions of mixtures is:
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