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Colligative properties of the solution depend upon:
A ) nature of the solution
B ) nature of the solvent
C ) number of solute particles
D ) number of moles of solvent

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Last updated date: 20th Jun 2024
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Answer
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Hint: Equimolar solutions of two different solutes have same osmotic pressure. Colligative properties of a solution do not depend on the nature of solution.

Complete step by step answer:
The following are the examples of some colligative properties
( i ) Relative lowering of the vapour pressure of the solvent.
( ii ) Elevation of the boiling point of the solvent.
( iii ) Depression of the freezing point of the solvent.
( iv ) Osmotic pressure of the solution.
Solute particles can be molecules, atoms or ions.
Colligative properties are independent of nature of solute, nature of the solution, nature of the solvent and number of moles of solvent.

Thus, if we dissolve one mole of glucose in one liter of water, its colligative properties such as osmotic pressure will be the same as when we dissolve one mole of urea in one liter of water. But the osmotic pressure of a solution containing one mole of urea in one liter of water will be different from the osmotic pressure of a solution containing two moles of urea in one liter of water.

Hence, the option C ) is the correct answer.

Note:
Do not mix up the concept of colligative properties with that of some physical properties such as density which depends on the nature of solute and solvent. Colligative properties depend on the number of solute particles but are independent of the nature of solute and solution. However physical properties such as density are independent of the number of solute particles and depend on the nature of solute and solvent.