Molar Conductivities and their Variation with Concentration NEET Questions

Physical Chemistry - Redox Reactions and Electrochemistry

Molar Conductivities and their Variation with Concentration MCQ Questions


13.
Kohlrausch's law is particularly useful for determining Λm° of:
A.
Strong electrolytes only
B.
Weak electrolytes
C.
Non-electrolytes
D.
Molten salts
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ANSWER :
B. Weak electrolytes
14.
Λm°(CH₃COOH) can be calculated using:
A.
Λm°(CH₃COONa) - Λm°(HCl) - Λm°(NaCl)
B.
Λm°(CH₃COONa) - Λm°(HCl) + Λm°(NaCl)
C.
Λm°(CH₃COONa) + Λm°(HCl) - Λm°(NaCl)
D.
Λm°(CH₃COONa) + Λm°(HCl) + Λm°(NaCl)
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ANSWER :
C. Λm°(CH₃COONa) + Λm°(HCl) - Λm°(NaCl)
15.
For strong electrolytes, the variation of Λm with concentration is given by Debye-Hückel-Onsager equation:
A.
Λm = Λm° - Ac
B.
Λm = Λm° + A√c
C.
Λm = Λm° - A√c
D.
Λm = Λm° × √c
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ANSWER :
C. Λm = Λm° - A√c
16.
A plot of Λm versus √c for a strong electrolyte gives:
A.
A straight line with negative slope and intercept = Λm°
B.
A straight line with positive slope
C.
A horizontal line
D.
A curve passing through origin
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ANSWER :
A. A straight line with negative slope and intercept = Λm°
17.
For a strong electrolyte, the limiting molar conductivity is obtained by:
A.
Multiplying conductivity by concentration
B.
Taking value at c = 1 M
C.
Extrapolating Λm vs √c plot to c = 0
D.
Direct measurement at infinite concentration
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ANSWER :
C. Extrapolating Λm vs √c plot to c = 0
18.
The decrease in Λm of strong electrolytes with increasing concentration is mainly due to:
A.
Decrease in degree of dissociation
B.
Increase in viscosity
C.
Decrease in number of ions
D.
Inter-ionic attractions (relaxation and electrophoretic effects)
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ANSWER :
D. Inter-ionic attractions (relaxation and electrophoretic effects)