- 1(current)
Q. No.1. \(0.01 \mathrm{M} ~\mathrm{Na}_2 \mathrm{SO}_4 \)
2. \(0.015 \text M~\mathrm{C}_6 \mathrm{H}_{12} \mathrm{O}_6 \)
3. \(0.01 \text {M Urea} \)
4. \(0.01 \mathrm{M} ~\mathrm{KNO}_3\)
| 1. | 0.05 M NaCl | 2. | 0.1 M KCl |
| 3. | 0.1 M MgSO4 | 4. | 0.1 M NaCl |
The van’t Hoff factor (i) for a dilute aqueous solution of a strong electrolyte barium hydroxide is:
1. 0
2. 1
3. 2
4. 3
The electrolyte having the same value of Van't Hoff factor (i) as that of Al2(SO4)3 (if all are 100% ionized) is:
| 1. | K2SO4 | 2. | K3[Fe(CN)6] |
| 3. | Al(NO3)3 | 4. | K4[Fe(CN)6] |
The van’t Hoff factor, i, for a compound that undergoes
dissociation and association in a solvent is, respectively:
1. Less than one and less than one.
2. Greater than one and less than one.
3. Greater than one and greater than one.
4. Less than one and greater than one.
A 0.0020 m aqueous solution of an ionic compound Co(NH3)5(NO2)Cl freezes at -0.0073 oC. The number of moles of ions that 1 mol of ionic compound produces on being dissolved in water will be:
(Kf = -1.86 oC/m)
| 1. | 2 | 2. | 3 |
| 3. | 4 | 4. | 1 |
0.5 molal aqueous solution of a weak acid (HX) is 20 % ionised. The lowering in the freezing point of the solution will be:
[Kf for water = 1.86 K kg mol-1]
1. -1.12 K
2. 0.56 K
3. 1.12 K
4. -0.56 K
- 1(current)
Q. No.
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