For binary solution of two liquids, A and B

Match List-I with List-II

Choose the correct answer from the options given below:

(A)-(IV), (B)-(III), (C)-(I), (D)-(II)

The correct answer is Option (1) → (A)-(IV), (B)-(III), (C)-(I), (D)-(II)

The behavior of liquid mixtures depends on the relative strength of intermolecular interactions between molecules of components A and B. Raoult's law describes the vapor pressure of ideal solutions.

Case (A): A–A and B–B ≈ A–B

When the interaction between unlike molecules (A–B) is nearly the same as that between like molecules (A–A and B–B), the solution behaves ideally. Thus, the solution follows Raoult's law exactly.

Therefore: (A) → No deviation from Raoult's Law (IV)

Case (B): A–A and B–B stronger than A–B

Here the attraction between unlike molecules is weaker. Molecules escape more easily into vapor phase. This increases vapor pressure compared to ideal behavior. Thus the solution shows positive deviation from Raoult's law.

Therefore: (B) → Positive deviation (III)

Case (C): A–A and B–B weaker than A–B

In this case, unlike molecules attract each other more strongly than like molecules. This reduces the escaping tendency of molecules and lowers vapor pressure. Thus the solution shows negative deviation from Raoult's law.

Therefore: (C) → Negative deviation (I)

Case (D): Very strong A–B interaction

Very strong interactions between components can lead to formation of azeotropes, where the mixture boils at constant composition.

Therefore: (D) → Azeotropes (II)