Q. No.At a given temperature, osmotic pressure of a concentrated solution of a substance:
1.
Is higher than that of a dilute solution.
2.
Is lower than that of a dilute solution.
3.
Is same as that of a dilute solution.
4.
Cannot be compared with osmotic pressure of dilute solution.
The incorrect statement among the following is:
| 1. | Two different solutions of sucrose of the same molality prepared in different solvents will have the same depression in freezing point. |
| 2. | The osmotic pressure of a solution is given by the equation π = CRT (where C is the molarity of the solution) |
| 3. | Decreasing order of osmotic pressure for 0.01 M aqueous solutions of BaCl2 > KCl > CH3COOH > sucrose |
| 4. | The vapour pressure exerted by a volatile component of a solution is directly proportional to its mole fraction in the solution. |
The incorrect statement among the following is:
| 1. | Units of atmospheric pressure and osmotic pressure are the same. |
| 2. | In reverse osmosis, solvent molecules move through a semipermeable membrane from a region of lower concentration of solute to a region of higher concentration. |
| 3. | The value of molal depression constant depends on nature of solvent. |
| 4. | Relative lowering of vapour pressure, is a dimensionless quantity. |
| 1. | Increases with an increase in temperature. |
| 2. | Decreases with an increase in temperature. |
| 3. | Remains constant. |
| 4. | First increases then decreases. |
Three aqueous solutions of NaCl are labelled as ‘A', ‘B’ and ‘C with concentrations 0.1 M, 0.01 M and 0.001 M, respectively. The value of van’t Hoff factor for these solutions will be in the order of :
1. iA < iB < iC
2. iA > iB > iC
3. iA = iB = iC
4. iA < iB > iC
4 L of 0.02 M aqueous solution of NaCl was diluted by adding 1 L of water. The molarity of the resultant solution is:
| 1. | 0.004 M | 2. | 0.008 M |
| 3. | 0.012 M | 4. | 0.016 M |
For a binary ideal liquid solution, the curve that represents the variation in total vapor pressure versus composition of the solution is:
| a. |  |
b. |  |
| c. |  |
d. |  |
The correct option is:
1. a and b
2. b and c
3. c and d
4. a and d
Match the laws/colligative properties given in Column-I with expressions given in Column-II.
| Column-I | Column-II | ||
| A. | Raoult’s law | I. | \(\mathrm{\pi=C R T}\) |
| B. | Osmotic pressure | II. | \(\Delta \mathrm{T}_{\mathrm{f}}=\mathrm{K}_{\mathrm{f}} \mathrm{~m}\) |
| C. | Elevation of boiling point | III. | \(\mathrm{p=x_1 p_1^0+x_2 p_2^0}\) |
| D. | Depression in freezing point | IV. | \(\Delta \mathrm{T}_{\mathrm{b}}=\mathrm{K}_{\mathrm{b}} \mathrm{~m}\) |
Codes:
| A | B | C | D | |
| 1. | I | III | IV | I |
| 2. | I | II | III | IV |
| 3. | I | IV | III | II |
| 4. | III | I | IV | II |
Match the terms given in Column I with expressions given in Column II.
| Column I (Term) | Column II (Expression) |
| A. Mass percentage | 1. \(\text{Number of moles of the solute component} \over \text{Volume of solution in litres}\) |
| B. Volume percentage | 2. \(\text{Number of moles of the solute component} \over \text{Mass of solvent in kilograms}\) |
| C. Molarity | 3. \(\small{\text{Volume of the solute component in solution} \over \text{Total volume of solution}} \times 100\) |
| D. Molality | 4. \(\small{\text{Mass of the solute component in solution} \over \text{Total Mass of solution}} \times 100\) |
Codes:
| A | B | C | D | |
| 1. | 2 | 3 | 4 | 1 |
| 2. | 1 | 2 | 3 | 4 |
| 3. | 1 | 4 | 3 | 2 |
| 4. | 4 | 3 | 1 | 2 |
Select the correct option based on statements below:
| Assertion (A): | Molarity of a solution in liquid state changes with temperature. |
| Reason (R): | The volume of a solution changes with change in temperature. |
| 1. | Both (A) and (R) are True and (R) is the correct explanation of (A). |
| 2. | Both (A) and (R) are True but (R) is not the correct explanation of (A). |
| 3. | (A) is True but (R) is False. |
| 4. | (A) is False but (R) is True. |
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