Depression in Freezing Point (ΔTf)
Freezing point of the liquid is the temperature at which the vapour pressure of the substance in its liquid phase is equal to its vapour pressure in the solid phase. If we add any solute to the solvent the freezing point of the solution is lower than the freezing point of the solvent.
Depression of frezzing point is the difference between the frezzing point of the solution and the freezing point of the solvent. If Tf is the frezzing point of pure solvent and TIf is the frezzing point of the pure solvent. Then deprezzion in freezing point is given as,
ΔTf = TIf – Tf
Experimentally it is proven that, ΔTf is proportional to morality of the solute, then
ΔTf ∝ m
ΔTf = kfm
Where, kf is molal elevation constant.
ΔTf = 1000kb(m2)/(M2m1)
where,
- m2 is the mass of solvent in g
- m1 is the mass of solvent in kg
- M2 is the molar mass of solute
Colligative Properties
Colligative Properties of any solution is the property of the solution that depends on the ratio of the total number of solute particles and the total number of solvent particles. Changing the moles or number of particles of solute or solvent changes the colligative properties of the solution. These colligative properties are not dependent on the chemical nature of the solute or solvent but are rather dependent on the number of solutes and solvent particles in the solution. These colligative properties depend on the number of particles in the solution rather than the nature of the solute and the solvent. These properties can be easily linked with the concentration of the solution, i.e. Molarity, Normality, and Molality.
In this article, we will learn about, various types of Colligative properties of the solution, their examples, and others in detail.
Table of Content
- What are Colligative Properties?
- Colligative Properties Examples
- Types of Colligative Properties
- Lowering Of Vapour Pressure
- Elevation in Boiling Point (ΔTb)
- Depression in Freezing Point (ΔTf)
- Osmotic Pressure (π)
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