Elevation in Boiling Point (ΔTb)
Boiling point of the liquid is the temperature at which the vapour pressure of the liquid is equal to the atmospheric pressure. If we add any solute to the solvent the boiling point of the solution is greater than the boiling point of the solvent.
Elevation of the boiling point is the difference between the boiling point of the solution and the boiling point of the solvent. If Tb is the boiling point of pure solvent and TIb is the boiling point of the pure solvent. Then elevation of boiling point is given as,
ΔTb = TIb – Tb
Experimentally it is proven that, ΔTb is proportional to morality of the solute, then
ΔTb ∝ m
ΔTb = kbm
Where, kb is molar elevation constant.
ΔTb = 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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