Question

In fig. (1), identify the nature of electrolyte A & B. In which case it is not possible to obtain value of limiting molar conductivity? Explain giving reason.​

Answer 1

Answer:

the electrolyte A and B in the. nature

Explanation:

Answer 2

Final answer:

Curve A represents strong electrolytes and curve B represents weak electrolytes.

Curve B fails to give a limiting value of $\Lambda_{m}$ in a measurable range of concentration. This is because the plot of $\Lambda_{m}$ against $c^\frac{1}{2}$ rises steeply near lower concentrations and does not approach linearity even in very dilute solutions.

Given that: We are given a figure.

To find: We have to find the nature of electrolytes A & B and in which case it is not possible to obtain the value of limiting molar conductivity.

Explanation:

We are given a graph of $\Lambda_{m}$ versus $c^\frac{1}{2}$.

• Curve A will have a high $\Lambda_{m}$ value even at high concentrations (low dilution) whereas curve B will have a low $\Lambda_{m}$ value under similar conditions.

Hence, curve A represent solution of a strong electrolyte and curve B represents the solution of a weak electrolyte.

It is not possible to determine molar conductivity at infinite dilution of curve B (weak electrolyte).

• The rate of increase in $\Lambda_{m}$ with increasing dilution (that is decrease in concentration) is more rapid for a weak electrolyte, particularly at a higher dilution.

• For a weak electrolyte, the molar conductivity is low at low dilution since the electrolyte is only slightly ionized.

• With increasing dilution, the molar conductivity increases gradually as the number of ions increases due to greater ionization of the electrolyte.

• Further, as dilution increases, the interionic attraction decrease. This causes an increase in the velocity and conducting capacity of the ions and thereby contributes to an increase in molar conductivity.

• Towards higher dilutions, the effects due to greater ionization and reduced interionic attractions become so pronounced that the molar conductivity increases rapidly.

Hence accurate measurements of limiting molar conductivity are not practicable.

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