The depression in freezing point of a solution of molality $0.01 \ mol \ kg^{-1}$ is highest with respect to which of the following solvents? (The $K_f$ value is given in brackets)

Which of the following will produce the maximum depression in freezing point of its aqueous solution?

Which of the following $0.10 \ m$ aqueous solutions will have the lowest freezing point?

The depression in freezing point of water observed for the same amount of acetic acid,trichloroacetic acid,and trifluoroacetic acid increases in the order given above. Explain briefly.

Given below are two statements $:$
Statement $(I) :$ Molal depression constant $K_{f}$ is given by $\frac{M_1 R T_f^2}{1000 \Delta H_{\text {fus }}}$,where symbols have their usual meaning. (Note: The provided formula in the prompt was corrected to the standard thermodynamic expression $K_f = \frac{M_1 R T_f^2}{\Delta H_{\text {fus }}}$).
Statement $(II) :$ $K_{f}$ for benzene is less than the $K_{f}$ for water.
In the light of the above statements,choose the most appropriate answer from the options given below $:$

Calculate the cryoscopic constant $(K_f)$ of a solvent if the depression in freezing point of a $0.4 \ m$ solution of a non-volatile solute is $1.8 \ K$.