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Colligative properties of a solution dep...

Colligative properties of a 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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To answer the question regarding what the colligative properties of a solution depend upon, we can follow these steps: ### Step-by-Step Solution: 1. **Understanding Colligative Properties**: - Colligative properties are properties of solutions that depend on the number of solute particles in a given amount of solvent, rather than the identity of the solute. 2. **Identifying the Four Main Colligative Properties**: - The four main colligative properties are: - Relative lowering of vapor pressure - Elevation of boiling point - Depression of freezing point - Osmotic pressure 3. **Effect of Non-volatile Solute**: - When a non-volatile solute is added to a pure solvent, it affects these properties: - It lowers the vapor pressure of the solvent. - It raises the boiling point of the solvent. - It lowers the freezing point of the solvent. - It creates osmotic pressure. 4. **Dependence on Number of Solute Particles**: - The key point is that colligative properties depend on the number of solute particles in the solution, not on their nature or identity. This means that whether the solute is a salt, sugar, or any other non-volatile solute, the effect on the colligative properties will be determined by how many particles are present. 5. **Conclusion**: - Therefore, the colligative properties depend on the number of solute particles in the solution, irrespective of their nature. ### Final Answer: The colligative properties of a solution depend upon the number of solute particles.
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Colligative properties of solution depend upon the number of particles present in solution. Experimental values colligative properties for electrolytes are always higher than these obtained theoretically because electrolyte dissociates to furnish more ions in solution. The ration of experimental values to theoretical values is called as van't Hoff factor (i) . For 1M solution of a weak acid HA , the dissociation constant K in terms of van't Hoff factor:

Colligative properties of solution depend upon the number of particles present in solution. Experimental values colligative properties for electrolytes are always higher than these obtained theoretically because electrolyte dissociates to furnish more ions in solution. The ration of experimental values to theoretical values is called as van't Hoff factor (i) . The correct order of freezing point for the following, each are 1 molal solutions in water and take alpha = 1 : (i) Urea , (ii) NaCl (iii) Na_(3)PO_(4) , (iv) Na_(2)SO_(4)

Colligative properties of solution depend upon the number of particles present in solution. Experimental values colligative properties for electrolytes are always higher than these obtained theoretically because electrolyte dissociates to furnish more ions in solution. The ration of experimental values to theoretical values is called as van't Hoff factor (i) . van't Hoff factor for dimerisation of benzoic acid in water, assuming 70% degree of association: