A) \[-{{0.69}^{o}}C\]
B) \[{{0.34}^{o}}C\]
C) \[{{0.0}^{o}}C\]
D) \[{{0.24}^{o}}C\]
Correct Answer: A
Solution :
Depression in freezing point \[(\Delta {{T}_{f}})\] \[=\frac{1000\times {{k}_{f}}\times w}{m\times W}\] where, \[{{k}_{f}}\] is molar depression constant, w and W are the weights of solute and solvent, m is the molecular weight of solute. \[\Delta {{T}_{f}}=\frac{1000\times 1.86\times 17}{46\times 1000}\] \[={{0.69}^{o}}C\] Freezing point of solution, \[{{T}_{f}}=0-0.69=-{{0.69}^{o}}C\]
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