1. | 3.34 cm–1 | 2. | 1.34 cm–1 |
3. | 3.28 cm–1 | 4. | 1.26 cm–1 |
A: | This equation applies to both strong and weak electrolytes. |
B: | The value of the constant A depends upon the nature of the solvent. |
C: | The value of constant A is the same for both \(BaCl_2\) and \(MgSO_4\) |
D: | The value of constant A is the same for both \(BaCl_2\) and \(Mg(OH)_2\) |
1. | (A) and (B) only | 2. | (A), (B), and (C) only |
3. | (B) and (C) only | 4. | (B) and (D) only |
\(\land^o_m\) for NaCl, HCl and \(\mathrm{CH_3COONa }\) are 126.4, 425.9, and 91.05 S cm2 mol–1 respectively. If the conductivity of 0.001028 mol L–1 acetic acid solution is \(4.95 \times 10^{-5} S ~cm^{-1} \), the degree of dissociation of the acetic acid solution is:
1. | 0.01233 | 2. | 1.00 |
3. | 0.1233 | 4. | 1.233 |
Limiting molar conductivities, for the given solutions, are :
From the data given above, it can be concluded that \(\lambda_m^0 \) in (\(S\ cm^2\ mol^{-1}\)) for CH3COOH will be :
1. \(\mathrm{x-y+2z}\)
2. \(\mathrm{x+y+z}\)
3. \(\mathrm{x-y+z}\)
4. \(\mathrm{{(x-y) \over 2}+z}\)