The freezing point of a solution is found to be less than pure solvent. But freezing point is the temperature at which vapour pressure of liquid phase and solid phase become equal . vapour pressure of solution is less than pure solvent . So wouldn't the vapour pressures of liquid phase and vapour phase become equal(freezing point) at a high temperature rather than at a lower temp.?
Asked by Sumayya
20th March 2016,
10:00 PM
Answered by Expert
Answer:
Dear sumukooripparambil@gmail.com
Thanks for asking us a question in Ask the Expert section of TopperLearning.com.
We have not understood the query that you have posted. We would request you to clarify / provide additional details so that we may answer this to the best of the ability.
The query which you have posted depicts the following-
1) Freezing point of a solution is found to be less than pure solvent.
2) The vapour pressure of solution is less than that of a pure solvent.
3) Freezing point is the temperature at which vapour pressure of liquid phase and solid phase become equal.
The statement - "So wouldn't the vapour pressures of liquid phase and vap....lower temp.?" is unclear to us.
However, answer to the query posted from what we could understand is-
Freezing point depression is a colligative property observed in solutions that results from the introduction of solute molecules to a solvent. The freezing points of solutions are all lower than that of the pure solvent and is directly proportional to the molality of the solute.
The vapor pressure of any substance increases non-linearly with temperature according to the Clausius–Clapeyron relation. With any incremental increase in that temperature, the vapor pressure becomes sufficient to overcome atmospheric pressureand lift the liquid to form vapor bubbles inside the bulk of the substance. Bubble formation deeper in the liquid requires a higher pressure, and therefore higher temperature, because the fluid pressure increases above the atmospheric pressure as the depth increases.
Topperlearning Team.
Answered by Expert
21st March 2016,
11:35 AM
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