Raoult’s law for Non-Volatile Solutes
For solutions having non volatile solutes, vapour pressure is only due to the solvent as non volatile solutes do not exert any pressure. Thus, Raoult’s law for non volatile solutes is defined as
Vapour pressure of the solution is directly propotional to the mole fraction of the solvent.
Mathematically,
pTotal ∝ xs
pTotal = ps0xs
where,
- pTotal is Total Vapour Pressure of Solution
- ps0 is Vapour Pressure of Solvent in Pure Form
- xs is Mole Fraction of Solvent
Raoult’s Law
Raoult’s Law in chemistry relates partial pressures of volatile liquid components to their mole fractions in a liquid solution. It states that the partial pressure of each component in the solution is directly proportional to its mole fraction. Thus, it helps us to calculate the total vapour pressure of the solution. Based on Raoult’s law, liquid solutions are classified as Ideal Solutions and Non-Ideal Solutions.
In this article, we will discuss the definition of Raoult’s law, ideal and non-ideal solutions, Raoult’s law for non-volatile solutes and some solved numerical problems based on Raoult’s law.
Table of Content
- Raoult’s Law Definition
- Raoult’s Law Formula
- Classification of Solutions based on Raoult’s law
- Raoult’s law for Non-Volatile Solutes
- Raoult’s Law with Other Laws
- Significance of Raoult’s Law
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