The molar conductance of NaCl, HCI, and CH3COONa at infinite dilution are 126.45, 426.16, and 91.0 S cm mol-1 respectively. The molar conductance of CH3COOH at infinite dilution will be:

1. 698.28 S cm2 mol-1

2. 540.48 S cm2 mol-1

3. 201.28 S cm2 mol-1

4. 390.71 S cm2 mol-1

Subtopic:   Kohlrausch Law & Cell Constant |
 81%
From NCERT
NEET - 2021
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The molar conductivity of 0.007 M acetic acid is 20 S cm2 mol-1. The dissociation constant of acetic acid is :

(\(\mathrm{\Lambda_{H^{+}}^{o} \ = \ 350 \ S \ cm^{2} \ mol^{-1} }\))
(\(\mathrm{\mathrm{\Lambda_{CH_{3}COO^{-}}^{o} \ = \ 50 \ S \ cm^{2} \ mol^{-1} }}\))

1. 1.75×10-5 mol L-1 

2. 2.50×10-5 mol L-1 

3. 1.75×10-4 mol L-1 

4. 2.50×10-4 mol L-1 

Subtopic:   Kohlrausch Law & Cell Constant |
 55%
From NCERT
NEET - 2021
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The EMF of a Daniel cell at 298 K is E Zn|ZnSO4(0.01 M) || CuSO4(1.0 M)|Cu.
When the concentration of ZnSO4 is 1.0 M and that of CuSO4 is 0.01 M, the EMF is changed to E2. The correct relationship between E1 and E2 is:

1. E1 > E2 2. E1 < E2
3. E1 = E2 4. E2 = 0 ≠ E1
Subtopic:  Electrode & Electrode Potential |
 78%
From NCERT
AIPMT - 2003
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On the basis of the information available from the reaction:

43Al+O223Al2O3, G=-827 KJ mol-1

The minimum e.m.f. required to carry out the electrolysis of Al2O3 is:
(F = 96500 C mol–1)

1. 2.14 V

2. 4.28 V

3. 6.42 V

4. 8.56 V

Subtopic:  Electrode & Electrode Potential |
 65%
From NCERT
AIPMT - 2003
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In electrolysis of NaCl when Pt electrode is taken then H2 is liberated at the cathode while with Hg cathode it forms sodium amalgam because:

1. Hg is more inert than Pt
2. More voltage is required to reduce H+ at Hg than at Pt
3. Na is dissolved in Hg while it does not dissolve in Pt
4. The concentration of H+ ions is larger when the Pt electrode is taken
Subtopic:  Electrode & Electrode Potential |
From NCERT
AIPMT - 2002
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The standard Emf of a galvanic cell involving cell reaction with n = 2 is found to be 0.295 V at 25 ºC. The equilibrium constant of the reaction would be:

(Given F = 96500 C mol–1; R = 8.314 J K–1 mol–1

1. 4.0 × 1012

2. 1.0 × 102

3. 1.0 × 1010

4. 2.0 × 1011

Subtopic:  Relation between Emf, G, Kc & pH |
 75%
From NCERT
AIPMT - 2004
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The value of E0 cell for the following reaction is:
\(Cu^{2+}+ Sn^{2+}\to Cu +Sn^{4+ } \)

(Given, equilibrium constant is 106)

1. 0.17 2. 0.01
3. 0.05 4. 1.77
Subtopic:  Electrode & Electrode Potential |
 73%
From NCERT
AIPMT - 1999
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A cell reaction become spontaneous when:

1. ∆Gº is negative

2. ∆Gº is positive

3. ERed° is positive

4. ERed° is negative

Subtopic:  Relation between Emf, G, Kc & pH |
 88%
From NCERT
AIPMT - 2000
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For the disproportionation of copper:

2Cu+ → C u2+ + C u, E° is:
(Given E° for Cu+2/Cu is 0.34 V & Eº for Cu+2/Cuis 0.15 V )

1. 0.49 V

2. – 0.19 V

3. 0.38 V

4. – 0.38 V

Subtopic:  Electrode & Electrode Potential |
From NCERT
AIPMT - 2000
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4.5 g of aluminium (at. mass = 27 amu) is deposited at cathode from Al3+ solution by a certain quantity of electric charge. The volume of hydrogen produced at STP from H+ ions in solution by the same quantity of electric charge will be:

1. 44.8 L 2. 11.2 L
3. 22.4 L 4. 5.6 L
Subtopic:  Faraday’s Law of Electrolysis |
 52%
From NCERT
AIPMT - 2005
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