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0.48g of a substane was dissolved in 10....

`0.48`g of a substane was dissolved in `10.6g C_(6)H_(6)` . The freezing point of benzene was lowered by `1.8^(@)C` . Calculate m.w.t. of the substance. Molecular depression constant for benzene is `50 K"mol"^(-1) 100 g`.

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To solve the problem, we will use the formula for freezing point depression, which is given by: \[ \Delta T_f = K_f \cdot \frac{m \cdot w}{W} \] Where: - \(\Delta T_f\) = change in freezing point (in °C) ...
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