Calculate the theoretical elevation in boiling point () of an aqueous solution containing of dissolv — Solutions and Colligative Properties Chemistry Question
Question
Calculate the theoretical elevation in boiling point ($\Delta T_b$) of an aqueous solution containing $13.44\text{ g}$ of $CuCl_2$ dissolved in $1\text{ kg}$ of water. (Molecular weight of $CuCl_2 = 134.4\text{ g mol}^{-1}$, $K_b$ for water $= 0.52\text{ K kg mol}^{-1}$, assume $100\%$ ionization).
Answer: B
💡 Solution & Explanation
Molality $m = \frac{13.44 / 134.4}{1\text{ kg}} = 0.1\text{ m}$. $CuCl_2$ is a strong electrolyte that dissociates into 3 ions ($Cu^{2+} + 2Cl^-$), so $i=3$. $\Delta T_b = i \times K_b \times m = 3 \times 0.52 \times 0.1 = 0.156^\circ\text{C} \approx 0.16^\circ\text{C}$.
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