Calculate van't Hoff factor of 0.2 m aquesous solution of an electrolyte if it freezes at -0.7 K $\left[\mathrm{K}_{\mathrm{f}}=1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\right]$

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Aicharya · Accepted Answer

$\begin{array}{ll} & \Delta \mathrm{T}_{\mathrm{f}}=\mathrm{i} \mathrm{m} \mathrm{K}_{\mathrm{f}} \ 	herefore \quad & 0.7=\mathrm{i} 	imes 0.2 \mathrm{~mol} \mathrm{~kg}^{-1} 	imes 1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1} \ 	herefore \quad & \mathrm{i}=\frac{0.7}{0.2 	imes 1.86}=\frac{0.7}{0.372}=1.882\end{array}$

Calculate van't Hoff factor of 0.2 m aquesous solution of an electrolyte if it freezes at -0.7 K…

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