Q. No.For an aqueous solution, freezing point is -0.186oC. Elevation of the boiling point of the same solution is:
(Given: Kf =1.86 K kg mol-1 and Kb = 0.512 K kg mol-1)
1. 0.186
2. 0.0512
3. 1.86
4. 5.12
Find the value of \(x\):
| 1. | Seven (7) | 2. | Three (3) |
| 3. | One (1) | 4. | Two (2) |
The depression in freezing point of 0.01 M aqueous solutions of urea, sodium chloride and sodium sulphate is in the ratio of:
1. 1 : 1 : 1
2. 1 : 2 : 3
3. 1 : 2 : 4
4. 2 : 2 : 3
What is the depression in freezing point of benzene when 1.00 g of a non-electrolyte solute (molar mass = 250 g mol⁻¹) is dissolved in 51.2 g of benzene?
[Given: The molal depression constant (Kf) for benzene is 5.12 K kg mol⁻¹]
| 1. | 0.4 K | 2. | 0.3 K |
| 3. | 0.5 K | 4. | 0.2 K |
If the molality of the dilute solution is doubled, then the value of a molal depression constant (Kf) will be:
1. Halved
2. Tripled
3. Unchanged
4. Doubled
\([\text{K}_f \) of the given solvent \( =1.2 \mathrm{K ~kg}~ \mathrm{mol}^{-1}] \)
| 1. | \(242.8 \mathrm{~g} \mathrm{~mol}^{-1}\) | 2. | \(238.2 \mathrm{~g} \mathrm{~mol}^{-1}\) |
| 3. | \(241.8 \mathrm{~g} \mathrm{~mol}^{-1}\) | 4. | \(240.0 \mathrm{~g} \mathrm{~mol}^{-1}\) |
1. Ionization of benzoic acid
2. Dimerization of benzoic acid
3. Trimerization of benzoic acid
4. Solvation of benzoic acid
A solution of sucrose (molar mass = 342 g mol–1) has been prepared by dissolving 68.5 g of sucrose in 1000 g of water. The freezing point of the solution obtained will be:
(kf for water = 1.86 K kg mol–1)
1. –0.372 oC
2. –0.520 oC
3. +0.372 oC
4. –0.570 oC
| Column-I | Column-II | ||
| A. | Rate constant (k) of a second-order reaction | I. | m3mol-1 |
| B. | Cryoscopic constant (Kf) | II. | mol-1L s-1 |
| C. | Van der Waals constant (b) | III. | No units |
| D. | Compressibility factor (Z) | IV. | kg K mol-1 |
| Options: | (A) | (B) | (C) | (D) |
| 1. | II | IV | I | III |
| 2. | III | IV | II | I |
| 3. | II | III | IV | I |
| 4. | IV | I | II | III |
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