Q. No.The variation of molar conductivity with the concentration of an electrolyte (X) in an aqueous solution is shown in the given figure.
The electrolyte X is:
| 1. | CH3COOH | 2. | KNO3 |
| 3. | HCl | 4. | NaCl |
The value of for NH4Cl, NaOH and NaCl are respectively 149.74, 248.1 and 126.4 The value of of NH4OH is -
1. 317.44
2. 271.44
3. 71.44
4. It cannot be calculated from the data given
1. \(14~S~m^2mole^{-2}\)
2. \(16~S~m^2mole^{-2}\)
3. \(48~S~m^2mole^{-2}\)
4. \(12.6~S~m^2mole^{-2}\)
Which of the following expressions gives the limiting molar conductivity \(\lambda_m^0\) of MgCl₂ in terms of the given values:
[Given: \(\small{\lambda_m^o(CaCl_2)=x~S~\text{cm}^2\text{mol}^{-1}},\) \(\small{\lambda^o(MgSO_4)=y~S~\text{cm}^2\text{mol}^{-1}}\) and \(\small{\lambda^o(CaSO_4)=z~S~\text{cm}^2\text{mol}^{-1}}.\)]1. \(2x+y-z\)
2. \(x-\frac{y}{2}-\frac z2\)
3. \(x+y-z\)
4. \(x-\frac y2-z\)
| 1. | 215 \(Scm^2mol^{-1}\) | 2. | 340 \(Scm^2mol^{-1}\) |
| 3. | 126 \(Scm^2mol^{-1}\) | 4. | 261 \(Scm^2mol^{-1}\) |
| 1. | 128.5 | 2. | 138.3 |
| 3. | 161.5 | 4. | 283.3 |
|
Electrolyte |
KCl |
KNO3 |
HCl |
NaOAc |
NaCl |
|
(Scm2mol-1) |
149.9 |
145.0 |
426.2 |
91.0 |
126.5 |
Calculate using appropriate molar conductances of the electrolytes listed
above at infinite dilution in H2O at 25°C
1. 517.2
2. 552.7
3. 390.7
4. 217.5
| 1. | |
| 2. | An electrolyte is 100% dissociated |
| 3. | All interionic effects disappear |
| 4. | All of the above |
What is the cell constant of a conductance cell in which the distance between the electrodes is 1.5 cm and the area of cross-section of each electrode is 0.75 cm²?
1. 1.0125 cm
2. 0.5 cm
3. 2.0 cm-1
4. 0.2cm-1
1. 20.800%
2. 4.008%
3. 40.800%
4. 2.080%
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