Match List-I with List-II.List-IList-II(A) Azeotropes(p) Molality(B)…

The correct answer is Option (3) → A-s, B-q, C-r, D-p

Each List-II entry is the definition or the cause of one solution term in List-I.

(A) Azeotropes — This matches (s) Solutions with the same composition in the vapour and liquid phases. An azeotrope is a binary mixture whose vapour has the same composition as the liquid, so it boils at a constant temperature and cannot be separated by fractional distillation.

(B) A mixture of chloroform and acetone shows negative deviation from Raoult’s law — This matches (q) Stronger intermolecular attraction between the components. The H of \( \ce{CHCl3} \) forms a hydrogen bond with the O of acetone. The A–B attraction is stronger than the A–A and B–B attractions, so fewer molecules escape and the vapour pressure is lower than Raoult’s law predicts.

(C) The ratio of the normal molar mass to the abnormal (experimentally determined) molar mass — This matches (r) van’t Hoff factor. It measures how far a solute dissociates or associates in solution:

    \( \displaystyle i=\frac{\text{Normal molar mass}}{\text{Abnormal molar mass}} \)

(D) The number of moles of solute dissolved in 1 kg of solvent — This matches (p) Molality. It is the definition of molality:

    \( \displaystyle m=\frac{\text{Moles of solute}}{\text{Mass of solvent in kg}} \)

NCERT (2026-27 edition):
1.5.2 Non-ideal Solutions – “Some liquids on mixing, form azeotropes which are binary mixtures having the same composition in liquid and vapour phase and boil at a constant temperature.”

1.5.2 Non-ideal Solutions – “… In case of negative deviations from Raoult’s law, the intermolecular attractive forces between A-A and B-B are weaker than those between A-B and leads to decrease in vapour pressure resulting in negative deviations. … Similarly, a mixture of chloroform and acetone forms a solution with negative deviation from Raoult’s law.”

1.7 Abnormal Molar Masses – “In 1880 van’t Hoff introduced a factor i, known as the van’t Hoff factor, to account for the extent of dissociation or association. This factor i is defined as:

    \( \displaystyle i=\frac{\text{Normal molar mass}}{\text{Abnormal molar mass}} \)

… Here abnormal molar mass is the experimentally determined molar mass and calculated colligative properties are obtained by assuming that the non-volatile solute is neither associated nor dissociated.”

1.2 Expressing Concentration of Solutions – “(vii) Molality: Molality (m) is defined as the number of moles of the solute per kilogram (kg) of the solvent and is expressed as:

    \( \displaystyle \text{Molality (m)}=\frac{\text{Moles of solute}}{\text{Mass of solvent in kg}} \)”