Freezing point depression in terms of intermolecular forces

  • Thread starter BrianC12
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  • #1
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Sorry if this is an obvious question...I understand how the justification via the pressure v temp graph works, but I'm not quite understanding freezing point depression in terms of intermolecular forces and temperature. I was taught that due to attractive IMF between solute and solvent particles in solution, vapor pressure will be lowered, and therefore higher temperature is needed to boil. But if that's the case, then doesn't that mean the same attractive IMF will overcome the kinetic energy of the molecules at a higher temperature than pure solvent, resulting in an increase of freezing point?

Thanks for any help!
 

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  • #2
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Freezing point depression relies on the fact that the IMFs between the solvent and solute are strong enough to disrupt the freezing process. The solvent more readily associates with the solute molecules instead of forming its solid structure.
 

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