Question

Does mass play a role in freezing point? For example, will Ba(NO₃)₂ or Mg(ClO₄)₂ have the highest freezing point:?

Answer 1

decrease in freezing point is given by,
delta Tf = i*Kf*m
here m is molality of olution
i is van't hoff factor which is defined as:
i = Normal molar mass / Abnormal molar mass
Or i is relative number of particle in solution
If number of particles in solution is more, delta Tf will be more and freezing point will be less

I can't say exactly which will ahve more in this case
Since both Ba(NO3)2 and Mg(ClO4)2 have i nearly equal to 3 as they give 3 ions when dissolved