The k of water is 1.86 kg °C/mol, approximately 4x the value of k,. If you attempted to freeze your 1.3m solution, how do you think the freezing point of water would be impacted?
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- Freezing point depression is a colligative property and it is noticed in solution when solute molecules are introduced into a solvent.
- The freezing point of solutions is all lower than that of a pure solvent and it is directly proportional to the molality of a solute.
- For example, when salt is added to the water, the water gets frozen before its freezing point and thus it gets depressed.
- Salt water has a lower vapor pressure than water.
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