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Q.
What should be the freezing point of aqueous solution containing $17 \,g$ of $ C_{2}H_{5}OH $ in $1000 \,g$ of water (water $ k_{f}=1.86^{\circ}kg\,mol^{-1} $ ) ?
AMUAMU 2007
Solution:
Depression in freezing point $\left(\Delta T_{f}\right)$
$=\frac{1000 \times k_{f} \times w}{m \times W}$
where, $k_{f}$ is molar depression constant, $w$ and $W$ are the weights of solute and solvent, $m$ is the molecular weight of solute.
$\Delta T_{f} =\frac{1000 \times 1.86 \times 17}{46 \times 1000} $
$=0.69^{\circ} C$
Freezing point of solution,
$T_{f}=0-0.69=-0.69^{\circ} C$