Question

An aqueous solution of an electrolyte \( A_3B \) is prepared by dissolving \( 0.5625 \) g in \( 750 \) ml of water and is found to be \( 80\% \) ionised. If \( K_b \) for water is \( 0.52 \, \text{K kg mol}^{-1} \), calculate the boiling point of the solution at \( 1.0 \) atm pressure.

• A. \( 374.33 \, \text{K} \)
• B. \( 371.68 \, \text{K} \)
• C. \( 373.18 \, \text{K} \)
• D. \( 377.2 \, \text{K} \)

Hint:

For electrolytes, always calculate Van't Hoff factor using \( i = 1+\alpha(n-1) \), then apply \( \Delta T_b = iK_bm \).

Answer 1

The Correct Option is A