- 1(current)
Q. No.| 1. | \( 0.225 \) | 2. | \( 0.215 \) |
| 3. | \(0.115 \) | 4. | \(0.125\) |
| 1. | 3.34 cm–1 | 2. | 1.34 cm–1 |
| 3. | 3.28 cm–1 | 4. | 1.26 cm–1 |
\(\Lambda_{\mathrm{m}}=\Lambda_{\mathrm{m}}^{\circ}-\mathrm{A} \sqrt{\mathrm{c}} \)
Consider the following four statements:
| 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 |
| 1. | 0.124 S cm2 mol–1 | 2. | 1.24 S m2 mol–1 |
| 3. | 124 S cm2 mol–1 | 4. | 124 S m2 mol–1 |
\(\land^o_m\) 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:
\(\lambda_{m}^{0} \left(\right. H_{2} S O_{4} \left.\right) = x\) \(S c m^{2}\) \(m o l^{- 1}\)
\(\lambda_{m}^{0} \left(\right. K_{2} S O_{4} \left.\right) = y\) \(S c m^{2}\) \(m o l^{- 1}\)
\(\lambda_{m}^{0} \left(\right. C H_{3} C O O K \left.\right) = z\) \(S c m^{2}\) \(m o l^{- 1}\)
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. | \(\mathrm{{(x-y) \over 2}+z}\) |
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