The conductivity of 0.001028 mol L–1 acetic acid is 4.95 ×10–5 S cm–1.  if Λ°m for acetic acid is 390.5 S cm2­­­­ mol–1, Its dissociation constant value is- 1. 1.58 × 10–5 mol L–1 2. 1.78 × 10–5 mol L–1 3. 1.98 × 10–5 mol L–1 4. 2.18 × 10–5 mol L–1

Subtopic:   Kohlrausch Law & Cell Constant |
54%
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What is the mass of copper deposited at the cathode after electrolyzing a solution of CuSO4 for 10 minutes with a current of 1.5 amperes?

1. 0.36 g
2. 0.48 g
3. 0.30 g
4. 0. 22 g

Subtopic:  Faraday’s Law of Electrolysis |
54%
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Λ°m for NaCl, HCl and NaAc are 126.4, 425.9 and 91.0 S cm2­­­­ mol–1 respectively. The value of Λ°m for HAc is-

1. 380.9 S cm
2­­­­ mol–1
2. 390.5 S cm
2­­­­ mol–1
3. 400 S cm
2­­­­ mol–1
4. 410.6 S cm
2­­­­ mol–1

Subtopic:   Kohlrausch Law & Cell Constant |
90%
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Consider the following data:
Λ°m(Ca2+) = 119.0 S cm2mol–1
Λ°m(Cl-) = 76.3 S cm2mol–1
Λ°m(Mg2+) = 106.0 S cm2mol–1
Λ°m($$SO_{4}^{2-}$$) = 160.0 S cm2mol–1

The correct statement among the following is-

 1 For CaCl2 Λ°m is 271.6 S cm2­­­­ mol–1 and for MgSO4 Λ°m is 266 S cm2­­­­ mol–1. 2 For CaCl2 Λ°m is 195.3 S cm2­­­­ mol–1 and for MgSO4 Λ°m is 266 S cm2­­­­ mol–1. 3 For CaCl2 Λ°m is 271.6 S cm2­­­­ mol–1 and for MgSO4 Λ°m is 133 S cm2­­­­ mol–1. 4 For CaCl2 Λ°m is 135.8 S cm2­­­­ mol–1 and for MgSO4 Λ°m is 133 S cm2­­­­ mol–1.

Subtopic:   Kohlrausch Law & Cell Constant |
73%
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The electrical resistance of a column of 0.05 mol L–1 NaOH solution of diameter 1 cm and length 50 cm is 5.55 × 103 ohm.

The molar conductivity of the NaOH solution is-

1. 235.4 S cm
2 mol–1
2. 229.6 S cm2 mol–1
3. 217.8 S cm2 mol–1
4. 232.2 S cm2 mol–1

Subtopic:  Conductance & Conductivity |
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Resistance of a conductivity cell filled with 0.1 mol L–1 KCl solution is 100 . If the resistance of the same cell when filled with 0.02 mol L–1 KCl solution is 520 . The conductivity of 0.1 mol L–1 KCl solution is 1.29 S/m. The molar conductivity of 0.02 mol L–1 KCl solution is-

1.
134 S cm2 mol–1
2. 124 S cm2 mol–1
3. 144 S cm2 mol–1
4. 154 S cm2 mol–1

Subtopic:  Conductance & Conductivity |
74%
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The standard electrode potential for Daniell cell is 1.1V. The standard Gibbs energy for the given reaction is-

Zn(s) + Cu2+(aq)  Zn2+(aq) + Cu(s)

(Given: F = 96487 C
mol1)

1. 312.27 kJ mol–1
2. 212.27 kJ mol–1
3. – 312.27 kJ mol–1
4. – 212.27 kJ mol–1

Subtopic:  Relation between Emf, G, Kc & pH |
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The equilibrium constant value for the given reaction is:

Cu(s) + 2Ag+(aq)  Cu2+(aq) + 2Ag(s)

(Given: EƟ(cell)
= 0.46 V)

1. 3.92 × 1014
2. 3.92 × 1015
3. 3.92 × 1016
4. 3.92 × 1017

Subtopic:  Relation between Emf, G, Kc & pH |
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Mg(s) + 2Ag+(0.0001M)  Mg2+(0.130M) + 2Ag(s)

If  EƟ(cell) for the above mentioned cell is 3.17 V, then E(cell) value will be-

(log 13=1.1)

1. 2.87 V
2. 3.08 V
3. 2.96 V
4. 2.68 V

Subtopic:  Nernst Equation |
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