A) \[103.3\]
B) \[105.7\]
C) \[107.9\]
D) \[109.3\]
Correct Answer: B
Solution :
The molar mass of solute \[=\frac{1000\times {{K}_{f}}\times W}{\Delta {{T}_{f}}\times \omega }\] Here weight of solute \[(W)=1.25g\] weight of solvent \[(\omega )=20g\] Molar depression constant \[({{K}_{f}})=1.86\] Freezing point of a solution \[(\Delta {{T}_{f}})=(273-271.9)\] \[=1.1K\] Putting the values, the molar mass of the solute \[=\frac{1000\times 1.86\times 1.25}{1.1\times 20}=105.7\]You need to login to perform this action.
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