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Depression in Freezing Point is considered one of the most asked concept.
15 Questions around this concept.
Kf for water is 1.86K kg mol -1 If your automobile radiator holds 1.0 kg of water, how many grams of ethylene glycol (C2H6O2) must you add to get the freezing point of the solution lowered to –2.8o C?
Depression in Freezing Point:
Freezing Point: It is the temperature at which the liquid and the solid form of the same substance are in equilibrium and have the same vapour pressure. A solution freezes when its vapour pressure is equal to the vapor pressure of pure solid solvent. Due to lower vapour pressure of the solution, solid form of a solution separates out a lower temperature.
On adding a non-volatile solute to the solvent, the vapor pressure of the solution is lesser than the solvent and the vapor pressure of the solution becomes equal to the vapor pressure of solid solvent at a lower temperature when compared to the pure solvent and hence the freezing point of decreases.
Suppose are the freezing point of pure solvent and solution respectively. Decrease in freezing point is given as:
Hence
If molality of the solution is one, then
and M can be found out by using these relations.
Here w = weight of solute
W = weight of solvent
Kf = molal depression constant or cryoscopic constant.
M = molar mass of solute
M1 = molar mass of solvent
The value of Kf or Cryoscopic constant is a property of the solvent only and does not depend on the type of solute. The value of Kf can be calculated as:
Here,
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