Question:
Match List I and List IIList II List II A. van't Hoff factor, i I. Cryoscopic constant B. $k_f$ II. Isotonic solutions C. Solution with same with same osmotic pressure III. Normal molar mass /Abnormal molar mass D. Azeotropes IV. Solutions with same composition of vapour above it
Choose the correct answer from the options given below :
Match List I and List II
Choose the correct answer from the options given below :
| List II | List II |
|---|---|
| A. van't Hoff factor, i | I. Cryoscopic constant |
| B. $k_f$ | II. Isotonic solutions |
| C. Solution with same with same osmotic pressure | III. Normal molar mass /Abnormal molar mass |
| D. Azeotropes | IV. Solutions with same composition of vapour above it |
Updated On: Sep 24, 2024
- A-I, B-III, C-II, D-IV
- A-III, B-I, C-IV, D-II
- A-III, B-I, C-II, D-IV
- A-III, B-II, C-I, D-IV
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The Correct Option is C
Solution and Explanation
The correct option is (C): A-III, B-I, C-II, D-IV.
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Concepts Used:
Colligative Properties
Colligative Property of any substance is entirely dependent on the ratio of the number of solute particles to the total number of solvent particles but does not depend on the nature of particles. There are four colligative properties: vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure.
Examples of Colligative Properties
We can notice the colligative properties of arrangements by going through the accompanying examples:
- On the off chance that we add a spot of salt to a glass full of water, its freezing temperature is brought down impressively than its normal temperature. On the other hand, the boiling temperature is likewise increased and the arrangement will have a lower vapor pressure. There are also changes observed in its osmotic pressure.
- In the same way, if we add alcohol to water, the solution’s freezing point goes down below the normal temperature that is usually observed for either pure alcohol or water.
Types of Colligative Properties
- Freezing point depression: ΔTf =1000 x kf x m2 /(M2 x m1)
- Boiling point elevation: ΔTb = kb m
- Osmotic pressure: π = (n2/V) RT
- Relative lowering of vapor pressure: (Po - Ps)/Po