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L30 : Colligative Properties: Numerical -1 - Solutions, Chemistry, Class 12 Video Lecture

FAQs on L30 : Colligative Properties: Numerical -1 - Solutions, Chemistry, Class 12 Video Lecture

1. What are colligative properties in chemistry?

Ans. Colligative properties in chemistry refer to the properties of a solution that depend only on the number of solute particles present, regardless of their identity. These properties include boiling point elevation, freezing point depression, osmotic pressure, and vapor pressure lowering.

2. How do colligative properties affect the boiling point of a solution?

Ans. Colligative properties, such as boiling point elevation, cause the boiling point of a solution to be higher than that of the pure solvent. This is because the presence of solute particles increases the entropy of the solution, making it harder for the solvent molecules to escape into the vapor phase.

3. What is freezing point depression in colligative properties?

Ans. Freezing point depression is a colligative property that describes the phenomenon of lowering the freezing point of a solvent when a non-volatile solute is added. The solute particles disrupt the regular arrangement of solvent molecules, making it more difficult for them to form a solid structure.

4. How is osmotic pressure related to colligative properties?

Ans. Osmotic pressure is a colligative property that is related to the concentration of solute particles in a solution. It is the pressure required to prevent the flow of solvent molecules across a semipermeable membrane. Osmotic pressure increases with the concentration of solute particles and can be used to determine the molar mass of a solute.

5. How does vapor pressure lowering occur in colligative properties?

Ans. Vapor pressure lowering is a colligative property that occurs when a non-volatile solute is added to a solvent. The presence of solute particles reduces the number of solvent particles at the surface, decreasing the rate of evaporation and lowering the vapor pressure of the solution compared to the pure solvent.

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