Q. No.1 g of a non-volatile non-electrolyte solute is dissolved in 100 g of two different solvents A and B whose ebullioscopic constants are in the ratio of 1 : 5. The ratio of the elevation in their boiling points, , is:
1. 5:1
2. 1:2
3. 10:1
4. 1:5
1. \(1.0~M~NaOH\)
2. \(1.0~M~Na_2SO_4\)
3. \(1.0~M~NH_4NO_3\)
4. \(1.0~M~KNO_3\)
1. 4
2. 6
3. 10
4. 8
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
1.00 g of a non-electrolyte solute dissolved in 50 g of benzene lowered the freezing point of benzene by 0.40 K. The freezing point depression constant of benzene is 5.12 K kg mol–1. The molar mass of the solute is:
| 1. | 245 g mol–1 |
2. | 256 g mol–1 |
| 3. | 264 g mol–1 |
4. | 274 g mol–1 |
| Statement I: | At 20 °C, the molality of KCl solution is 'X' m, and on decreasing temperature to -10 °C molality remains unchanged. |
| Statement II: | On changing temperature mass remains unchanged. |
| 1. | Both Statement I and Statement II are True. |
| 2. | Both Statement I and Statement II are False. |
| 3. | Statement I is True, and Statement II is False. |
| 4. | Statement I is False, and Statement II is True. |
The value of \(X\) is:
| 1. | 7 | 2. | 3 |
| 3. | 1 | 4. | 2 |
18 g of glucose, C6H12O6, is dissolved in 1 kg of water in a saucepan. The temperature at which water boil at 1.013 bar is-
(Kb for water is 0.52 K kg mol-1)
1. 383.202 K
2. 373.202 K
3. 363.202 K
4. 393.202 K
[Given : (\(K_b\)) for water is \(0.5~ K⋅kg/mol\), and the boiling point of pure water is \(100^∘C\).]
| 1. | \(105^\circ \text{C}\) | 2. | \(100.5^\circ \text{C}\) |
| 3. | \(273.5^\circ \text{C}\) | 4. | \(273.5^\circ \text{C}\) |
(Molecular weight of \(\mathrm {C}_3\mathrm{H}_5 \mathrm {(OH)_3}\) = 92.1 g/mol,
\(\mathrm{k}_{\mathrm{b}} \text { of } \mathrm{H}_2 \mathrm{O}=0.52^{\circ} \mathrm{Ckg} / \mathrm{mol}\))
1. 5.65 g
2. 92.0 g
3. 184 g
4. 194 g
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