Statement I: \(\Lambda _m\) for weak electrolytes shows a sharp increase when the electrolytic solution is diluted

Statement II: For weak electrolytes degree of dissociation increases with a dilution of the solution

Both Statement I and Statement II are correct and Statement II is the correct explanation of Statement I

The correct answer is option 1. Both Statement I and Statement II are correct, and Statement II is the correct explanation of Statement I.

Statement I: \(\Lambda_m\) for weak electrolytes shows a sharp increase when the electrolytic solution is diluted.

This statement is correct. \(\Lambda_m\) (molar conductivity) is a measure of the conductivity of a solution containing one mole of an electrolyte. For weak electrolytes, as the solution is diluted (more solvent is added), the number of ions per unit volume decreases, and the average distance between ions increases. This results in a decrease in the effective collision frequency between ions, leading to a decrease in the conductivity of the solution. However, for weak electrolytes, as the solution is further diluted, the degree of dissociation of the electrolyte increases significantly. More ions are released, and their mobility improves. Consequently, the molar conductivity (\(\Lambda_m\)) shows a sharp increase upon further dilution of the solution.

Statement II:  For weak electrolytes, the degree of dissociation increases with the dilution of the solution.

This statement is also correct and provides the correct explanation for Statement I. The degree of dissociation (\(\alpha\)) of an electrolyte is a measure of the extent to which it dissociates into ions in solution. For weak electrolytes, \(\alpha\) is usually small at higher concentrations, indicating a lower extent of ionization. However, when the solution is diluted, the concentration of the electrolyte decreases, leading to a decrease in the ion-ion interactions. As a result, more molecules of the weak electrolyte dissociate into ions, and the degree of dissociation increases significantly with dilution.

The increase in the degree of dissociation directly contributes to the increase in the molar conductivity (\(\Lambda_m\)) observed in Statement I when the solution is diluted. More ions are available in the solution, and their mobility improves, resulting in higher conductivity.

In conclusion, both statements are correct. Statement I correctly states that the molar conductivity for weak electrolytes shows a sharp increase when the solution is diluted, and Statement II provides the correct explanation for this phenomenon, stating that the degree of dissociation of weak electrolytes increases with a dilution of the solution.