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Question

Which of the following statement(s) is/are correct for a weak electrolytic solution?
Λm - Molar conductivity
Λ0m - Limiting molar conductivity
C - concentration of electrolyte

A
Λ0m cannot be found by extrapolation of Λm to zero concentration.
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B
On dilution, molar conductivity increases due to decrease in ion-ion forces of attraction.
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C
Plot of Λ0m vsC will give a rectangular hyperbola curve.
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D
Λ0m can be found by extrapolation of Λm to zero concentration.
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Solution

The correct option is C Plot of Λ0m vsC will give a rectangular hyperbola curve.
On dilution, the molar conductivity increases for both strong and weak electrolyte.

On dilution of weak electrolyte, the degree of dissociation increases which results in increase in the number of ions in solution. So, there will be overall increase in molar conductance.

Variation in Λm for weak electrolyte:
Weak electrolytes like acetic acid have lower degree of dissociation.
With dilution of an ionic solution, the degree of dissociation (α) of the electrolyte increases which result in increase in the number of ions in solution. Near lower concentration, there will be a steep increase in molar conductance.

Plot of Λm vs C

From above it is evident that curve for Λm vs C for a weak electrolyte (here acetic acid) is rectangular hyperbola. It does not intercept the y-axis.
Although, the concept of molar conductance at infinite dilution exists for a weak electrolyte.
But graphically, the value cannot be evaluated.

Thus, statements (a) and (c) are correct.

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