Molal depression constant $(K_{f})$ is dependent on

When an aqueous solution freezes at its freezing point,which components are in equilibrium?

Which of the following has the lowest freezing point?

What is the molar mass (in $g \ mol^{-1}$) of a substance,which forms a $7 \%$ by mass solution in water,which freezes at $-0.93^{\circ} C$? ($K_{f}$ of $H_2O = 1.86 \ K \ kg \ mol^{-1}$)

When a solute is dissolved in a solvent,the freezing point decreases by $0.184 \ ^oC$. What will be the molality of the solution? (Given $K_f = 18.4 \ K \ kg \ mol^{-1}$)

Identify the correct relation between depression in freezing point and the freezing point of a pure solvent.