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The equation is:
Tf = Kf*i*m
If I understand it correctly, the higher the Tf value, the lower the freezing point, meaning compounds with the lowest molecular weight (assuming the amount of solvent and the value of "i" is the same) have the lowest freezing points because their molality will be the highest? Or do I have it backwards?
If that's true, then for boiling point elevation (Tb = Kb*i*m), the lower the molecular weight, the higher the boiling point (once again, assuming the amount of solvent and "i" values are equal). Where I'm confused is that I thought the first thing you look for when distinguishing boiling point was IM forces and after that, molecular weight. Compounds with the highest molecular weights have the highest boiling points, or so I thought. But given this equation, it doesn't work out.
Can anyone explain it to me please?
Tf = Kf*i*m
If I understand it correctly, the higher the Tf value, the lower the freezing point, meaning compounds with the lowest molecular weight (assuming the amount of solvent and the value of "i" is the same) have the lowest freezing points because their molality will be the highest? Or do I have it backwards?
If that's true, then for boiling point elevation (Tb = Kb*i*m), the lower the molecular weight, the higher the boiling point (once again, assuming the amount of solvent and "i" values are equal). Where I'm confused is that I thought the first thing you look for when distinguishing boiling point was IM forces and after that, molecular weight. Compounds with the highest molecular weights have the highest boiling points, or so I thought. But given this equation, it doesn't work out.
Can anyone explain it to me please?