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Question

To one litre of 0.1 M-HCl solution, 0.025 mole of solid NH4Cl is added. Assuming complete dissociation of solutes, the freezing point of solution is (Kf of water = 1.86 K-kg mol−1)

Options

A.−0.465°C
B.−0.93°C
C.−0.372°C
D.−0.279°C

Solution

$\Delta T_{f} = K_{f}.m = 1.86 \times \lbrack 0.1 \times 2 + 0.025 \times 2\rbrack = 0.465^{o}C$

∴ F.P. of solution = – 0.465° C

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