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$0.8 \mathrm{~mL}$ of acetic acid of density $1.06 \mathrm{~g} \mathrm{~mL}^{-1}$ when dissolved in $1 \mathrm{~kg}$ of water causes a depression in freezing point by $0.0325^{\circ} \mathrm{C}$. The Van't Hoff factor is:
$\left(\mathrm{K}_{\mathrm{f}} \text { of } \mathrm{H}_2 \mathrm{O}=1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\right)$
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$\left(\mathrm{K}_{\mathrm{f}} \text { of } \mathrm{H}_2 \mathrm{O}=1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\right)$
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The correct answer is:
$1.24$
No solution. Refer to answer key.
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