Question

Assertion :An aqueous solution of HCl is a much better conductor of electricity than an aqueous solution of $C{H}_{3}COOH$ of the same concentration. Reason: The freezing point depression and the boiling point elevation of weak electrolytes are significantly less than for strong electrolytes of the same concentration.

• A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
• B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
• C. Assertion is correct but Reason is incorrect
• D. Both Assertion and Reason are incorrect

Answer 1

The correct option is B Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion

An aqueous solution of $HCl$ is a much better conductor of electricity than an aqueous solution of $C{H}_{3}COOH$ of the same concentration.

$HCl$ is a strong acid. It completely dissociates in aqueous solution.
Acetic acid is a weak acid. It only partially dissociates in aqueous solution.
Hence, the number of ions given by $HCl$ is more than acetic acid.

The freezing point depression and the boiling point elevation of weak electrolytes are significantly less than for strong electrolytes of the same concentration.

Strong electrolytes completely dissociate in aqueous solution whereas weak electrolytes partially dissociate. Hence, the number of ions given by strong electrolytes are higher than the number of ions given by weak electrolytes.

The colligative properties depend on the number of ions/molecules/particles.

Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion.