- 1(current)
Q. No.Molar conductivities at infinite dilution of
NaCl, HCl, and are 126.4, 425.9, and 91.0 S cm2 mol–1 respectively.
for will be:
| 1. | \(180.5~S~cm^2~mol^{-1}\) | 2. | \(290.8~S~cm^2~mol^{-1}\) |
| 3. | \(390.5~S~cm^2~mol^{-1}\) | 4. | \(425.5~S~cm^2~mol^{-1}\) |
\(\Lambda _{m(NH_{4}OH)}^{o}\) is equal to -
1. \(\Lambda _{m(NH_{4}OH)}^{o} \ + \ \Lambda _{m(NH_{4}Cl)}^{o} \ - \ \Lambda _{m(HCl)}^{o}\)
2. \(\Lambda _{m(NH_{4}Cl)}^{o} \ + \ \Lambda _{m(NaOH)}^{o} \ - \ \Lambda _{m(NaCl)}^{o}\)
3. \(\Lambda _{m(NH_{4}Cl)}^{o} \ + \ \Lambda _{m(NaCl)}^{o} \ - \ \Lambda _{m(NaOH)}^{o}\)
4. \(\ \Lambda _{m(NaOH)}^{o} \ + \ \Lambda _{m(NaCl)}^{o}\ - \ \Lambda _{m(NH_{4}Cl)}^{o}\)
The resistance of a conductivity cell containing 0.001M KCl solution at 298 K is 1500 Ω. The cell constant if conductivity of 0.001 M KCl solution at 298 K is 0.146 ×10-3 S cm-1 will be:
1. 0.32 cm-1
2. 0.47 cm
3. 0.22 cm-1
4. 0.23 cm
The resistance of a cell containing 0.001 M KCl solution at 298 K is 1500 Ω. The conductivity is 0.146 × 10–3 S cm–1. The cell constant would be-
| 1. | 2. | ||
| 3. | 4. |
The molar conductance of solution of a weak monobasic acid is 8.0 ohm-1 cm2 and at infinite dilution is 400 ohm-1 cm2. The dissociation constant of this acid is:
| 1. | \(1.25 \times10^{-5}\) | 2. | \(1.25 \times10^{-6}\) |
| 3. | \(6.25 \times10^{-4}\) | 4. | \(1.25 \times10^{-4}\) |
Kohlrausch's law states that at:
| 1. | Finite dilution, each ion makes definite contribution to equivalent conductance of an electrolyte, whatever be the nature of the other ion of the electrolyte. |
| 2. | Infinite dilution, each molecule makes definite contribution to equivalent conductance of an electrolyte depending on the nature of the other ion of the electrolyte. |
| 3. | Finite dilution, each molecule makes definite contribution to conductance of an electrolyte whatever be the nature of the other ion of the electrolyte. |
| 4. | Infinite dilution, each ion makes definite contribution to equivalent conductance of an electrolyte, whatever be the nature of the other ion of the electrolyte. |
Value of for (strong electrolyte) in water at from the data below is:
| Conc. (mol/litre) | 0.25 | 1 |
| 260 | 250 |
1. 270 Ω-1 cm2 mol-1
2. 260 Ω-1 cm2 mol-1
3. 250 Ω-1 cm2 mol-1
4. 255 Ω-1 cm2 mol-1
Consider the following graph of molar conductivity of KCl solution at different concentrations.
The value of limiting molar conductivity for KCl is 150.0 S cm2 mol-1. The value of the slope at point A will be :
| 1. | 120 | 2. | 100 |
| 3. | 110 | 4. | None of the above |
- 1(current)
Q. No.
© 2025 GoodEd Technologies Pvt. Ltd.