Class 12 Exam > Class 12 Videos > L31 : Colligative Properties: Numerical -2 - Solutions, Chemistry, Class 12
L31 : Colligative Properties: Numerical -2 - Solutions, Chemistry, Class 12 Video Lecture
FAQs on L31 : Colligative Properties: Numerical -2 - Solutions, Chemistry, Class 12 Video Lecture
| 1. What are colligative properties? |  |
Ans. Colligative properties are properties of a solution that depend on the number of solute particles present, rather than the nature of the solute itself. These properties include boiling point elevation, freezing point depression, vapor pressure lowering, and osmotic pressure.
| 2. How do solute particles affect colligative properties? | |
Ans. Solute particles affect colligative properties because they disrupt the normal behavior of the solvent molecules. This disruption leads to changes in the boiling point, freezing point, vapor pressure, and osmotic pressure of the solution. The more solute particles present, the greater the effect on these properties.
| 3. Why does adding a solute lower the freezing point of a solvent? | |
Ans. Adding a solute lowers the freezing point of a solvent because the solute particles disrupt the formation of a regular crystal lattice structure in the solvent. This disruption requires a lower temperature for the solvent to solidify, resulting in a lower freezing point.
| 4. How does boiling point elevation occur in a solution? | |
Ans. Boiling point elevation occurs in a solution because the presence of solute particles raises the boiling point of the solvent. This happens because the solute particles increase the vapor pressure of the solution, requiring a higher temperature to reach the boiling point compared to the pure solvent.
| 5. What is osmotic pressure and how is it related to colligative properties? | |
Ans. Osmotic pressure is the pressure required to prevent the flow of solvent through a semipermeable membrane due to the presence of solute particles. It is directly related to colligative properties because osmotic pressure depends on the number of solute particles in a solution. The greater the number of solute particles, the higher the osmotic pressure. Osmotic pressure is an important factor in processes such as osmosis and can be used to determine the molar mass of a solute.
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