# Why is freezing point depression greater than boiling point elevation for equimolar substances?

I know that the freezing point depression and boiling point elevation are given by the formulas $$\Delta\mathrm{T}_{b}=ib\mathrm{K}_{eb}$$ and $$\Delta\mathrm{T}_{f}=ib\mathrm{K}_{F}.$$ It seems that when this formula is applied for equimolar concentrations, the magnitude of freezing point depression is greater than boiling point elevation. Is there a qualitative reason for this? If so, what is it?