A solution comprises a solute and a solvent. It is defined as a homogeneous mixture of two or more than two substances. They can be classified into three types:
- Solid solutions
- Gaseous solutions
- Liquid solutions
Molarity, mole fraction, percentages, and molality are the terms used to express the concentration of a solution.
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CBSE Class 12 Chemistry Chapter 2 Solutions – Related Links
In liquids, the dissociation of gas is controlled by Henry’s law. The states that, the solubility of a gas in a liquid, at a given temperature, is directly proportional to the partial pressure of the gas. Due to the presence of a non-volatile solute, the vapour pressure of the solvent is lowered.
The lowering of the vapour pressure of the solvent is ruled by Raoult’s law. The law states that the relative lowering of the vapour pressure of the solvent over a solution and the mole fraction of a non-volatile solute present in the solution is equal. It is expressed as:
When a solution obeys Raoult’s law over the entire range of concentrations it is called an ideal solution. Types of deviations from Raoult’s law:
- Positive deviations
- Negative deviations
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Few Important Questions
- What is mole fraction?
- Explain the role of molecular interaction in a solution of water and alcohol?
- Give the statement of Henry’s law. List some applications.
- What is a solution? Explain the different types of solution.
- What is molarity?
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Frequently asked Questions on CBSE Class 12 Chemistry Notes Chapter 2: Solutions
What are the different types of solutions?
The 3 main types of solutions are: 1. Solid 2. Liquid 3. Gas
What are ‘Ideal solutions’?
When a solution obeys Raoult’s law over the entire range of concentrations it is called an ideal solution.
What is ‘Molarity’?
Molarity or molar concentration, is the concentration of a solution measured as the number of moles of solute per liter of solution.