Statement Type Solution Questions for NEET
In each of the following questions a Statement I is given
followed by a corresponding Statement II just below it.
Mark the correct answer from the following statements.
1. If both Statement I and Statement II are correct and Statement II is the correct explanation of Statement I
2. If both Statement I and Statement II are correct but Statement II is not the correct explanation of Statement I
3. If Statement I is correct but Statement II is false
4. If Statement I is false but Statement II is correct
1. Statement I: The vapour pressure of a liquid deceases if some non-volatile solute is dissolved in it.
Statement II: The relative lowering of vapour pressure of a solution containing a non-volatile solute is equal to the mole fraction of the solute in the solution.
2. Statement II: The vapour pressure of 0.1 M sugar solution is more than that of 0.1 M KCl solution.
Statement II: Lowering of vapour pressure is directly proportional to the number of species present in the solution.
3. Statement I: The solubility of the gas in a liquid increases with increase of pressure at constant temperature.
Statement II: The solubility of the gas in a liquid is directly proportional to the pressure of the gas at constant temperature.
4. Statement I: The freezing point of 0.05 M urea solution is different from that of 0.05 M NaCl solution.
Statement II: The depression in freezing point is directly proportional to the number of particles in the solution.
5. Statement I: Vapour pressure of water is less than 1.013 bar at 373 K.
Statement II: Water boils at 373 K as the vapour pressure of water at this temperature becomes equal to atmospheric pressure.
6. Statement I: The molecular weight of acetic acid in benzene is more than the actual value of the solute.
Statement II: Molecules of acetic acid dimerize in benzene due to hydrogen bonding.
7. Statement I: Addition of ethylene glycol (non volatile) to water lowers the freezing point of water, hence used as antifreeze.
Statement II: Addition of any substance to water lower freezing point of water.
8. Statement I: The freezing point of water is depressed by the addition of glucose.
Statement II: Entropy of solution is less than entropy of pure solvent.
9. Statement I: Mercuric iodide dissolves in potassium iodide solution forming K2HgI4 and the freezing point gets elevated.
Statement II: The number of particles in K2HgI4 is same as those in HgI2.
10. Statement I: In solution different parts show different composition.
Statement II: Solution is homogeneous mixture.
11. Statement I: Stirring a solution leads to high solubility.
Statement II: Due to stirring solvent molecules surrounding solute increases.
12. Statement I: Molarity of a solution is always greater than that of molality.
Statement II: Ratio of molarity and molality depends on density of solvent.
13. Statement I: Raoult’s law is applicable to ideal solutions only.
Statement II: In ideal solutions association or dissociation does not takes place.
14. Statement I: Relative lowering of vapour pressure is independent of temperature.
Statement II: Relative lowering of vapour pressure is nothing but the mole fraction of solution.
15. Statement I: With increase in temperature molarity increases.
Statement II: Molarity consists with volume terms.
16. Statement I: Molarity of 0.02N HNO3 is 0.02M.
Statement II: Molarity and normality of a solution are always same.
17. Statement I: The solution having greater vapour pressure has higher boiling point.
Statement II: More volatile liquids have low boil- ing point.
18. Statement I: If hydration energy is greater than lat- tice energy, the solid dissolves in liquid.
Statement II: The solubility of solid in a liquid depends upon lattice energy and hydration energy.
19. Statement I: Cooking time is reduced in a pressure cooker.
Statement II: Boiling point of water inside is elevated.
20. Statement I: Strength and normality are the different methods of expressing the concentration of the solution.
Statement II: Strength is equal to normality of a solution.
21. Statement I: Normality and molarity can be calculated from each other.
Statement II: Normality is equal to the product of molarity and n.
22. Statement I: If 100 cm3 of 0.1 N HCl is mixed with 100 cm3 of 0.2N HCl, the normality of the final solution will be 0.30N.
Statement II: Normalities of similar solutions like HCl can be added.
23. Statement I: The vapour pressure of 0.1 M sugar solution is less than that of 0.1M KCl solution.
Statement II: Lowering of vapour pressure is directly proportional to the number of species present in solution.
24. Statement I: At the same temperature, water has higher vapour pressure than acetic acid.
Statement II: Hydrogen bonding in water is weaker than in acetic acid.
25. Statement I: Osmotic pressure is a colligative property.
Statement II: Osmotic pressure depends on the number of particles dissolved in solution.
26. Statement I: If a liquid solute is added to a solvent which is more volatile than solvent, then vapour pressure of solution may increase, that is, Ps > Po.
Statement II: In the presence of a more volatile liquid solute, only the solute will form the vapours and solvent will not.
27. Statement I: Molecular mass of polymers cannot be calculated using boiling point or freezing point method.
Statement II: Polymer solutions do not possess a constant boiling point or freezing point.
Hint: Polymer solutions possess very little elevation in boiling point or depression in freezing point.
28. Statement I: If cells of living organisms are placed in pure water, they swell and burst.
Statement II: Due to osmosis, the movement of wa- ter molecules into the cell dilutes the salt content.
29. Statement I: Reverse osmosis is used in the desali- nation of sea water.
Statement II: When the applied pressure is more than the osmotic pressure, pure water is squeezed out of sea water through the membrane.
30. Statement I: Camphor is used as solvent in the de- termination of molecular masses of naphthalene, anthracene, etc.
Statement II: Camphor has high molal elevation constant.
Answer
Class-11
Class-12
1. If both Statement I and Statement II are correct and Statement II is the correct explanation of Statement I
2. If both Statement I and Statement II are correct but Statement II is not the correct explanation of Statement I
3. If Statement I is correct but Statement II is false
4. If Statement I is false but Statement II is correct
1. Statement I: The vapour pressure of a liquid deceases if some non-volatile solute is dissolved in it.
Statement II: The relative lowering of vapour pressure of a solution containing a non-volatile solute is equal to the mole fraction of the solute in the solution.
2. Statement II: The vapour pressure of 0.1 M sugar solution is more than that of 0.1 M KCl solution.
Statement II: Lowering of vapour pressure is directly proportional to the number of species present in the solution.
3. Statement I: The solubility of the gas in a liquid increases with increase of pressure at constant temperature.
Statement II: The solubility of the gas in a liquid is directly proportional to the pressure of the gas at constant temperature.
4. Statement I: The freezing point of 0.05 M urea solution is different from that of 0.05 M NaCl solution.
Statement II: The depression in freezing point is directly proportional to the number of particles in the solution.
5. Statement I: Vapour pressure of water is less than 1.013 bar at 373 K.
Statement II: Water boils at 373 K as the vapour pressure of water at this temperature becomes equal to atmospheric pressure.
6. Statement I: The molecular weight of acetic acid in benzene is more than the actual value of the solute.
Statement II: Molecules of acetic acid dimerize in benzene due to hydrogen bonding.
7. Statement I: Addition of ethylene glycol (non volatile) to water lowers the freezing point of water, hence used as antifreeze.
Statement II: Addition of any substance to water lower freezing point of water.
8. Statement I: The freezing point of water is depressed by the addition of glucose.
Statement II: Entropy of solution is less than entropy of pure solvent.
9. Statement I: Mercuric iodide dissolves in potassium iodide solution forming K2HgI4 and the freezing point gets elevated.
Statement II: The number of particles in K2HgI4 is same as those in HgI2.
10. Statement I: In solution different parts show different composition.
Statement II: Solution is homogeneous mixture.
11. Statement I: Stirring a solution leads to high solubility.
Statement II: Due to stirring solvent molecules surrounding solute increases.
12. Statement I: Molarity of a solution is always greater than that of molality.
Statement II: Ratio of molarity and molality depends on density of solvent.
13. Statement I: Raoult’s law is applicable to ideal solutions only.
Statement II: In ideal solutions association or dissociation does not takes place.
14. Statement I: Relative lowering of vapour pressure is independent of temperature.
Statement II: Relative lowering of vapour pressure is nothing but the mole fraction of solution.
15. Statement I: With increase in temperature molarity increases.
Statement II: Molarity consists with volume terms.
16. Statement I: Molarity of 0.02N HNO3 is 0.02M.
Statement II: Molarity and normality of a solution are always same.
17. Statement I: The solution having greater vapour pressure has higher boiling point.
Statement II: More volatile liquids have low boil- ing point.
18. Statement I: If hydration energy is greater than lat- tice energy, the solid dissolves in liquid.
Statement II: The solubility of solid in a liquid depends upon lattice energy and hydration energy.
19. Statement I: Cooking time is reduced in a pressure cooker.
Statement II: Boiling point of water inside is elevated.
20. Statement I: Strength and normality are the different methods of expressing the concentration of the solution.
Statement II: Strength is equal to normality of a solution.
21. Statement I: Normality and molarity can be calculated from each other.
Statement II: Normality is equal to the product of molarity and n.
22. Statement I: If 100 cm3 of 0.1 N HCl is mixed with 100 cm3 of 0.2N HCl, the normality of the final solution will be 0.30N.
Statement II: Normalities of similar solutions like HCl can be added.
23. Statement I: The vapour pressure of 0.1 M sugar solution is less than that of 0.1M KCl solution.
Statement II: Lowering of vapour pressure is directly proportional to the number of species present in solution.
24. Statement I: At the same temperature, water has higher vapour pressure than acetic acid.
Statement II: Hydrogen bonding in water is weaker than in acetic acid.
25. Statement I: Osmotic pressure is a colligative property.
Statement II: Osmotic pressure depends on the number of particles dissolved in solution.
26. Statement I: If a liquid solute is added to a solvent which is more volatile than solvent, then vapour pressure of solution may increase, that is, Ps > Po.
Statement II: In the presence of a more volatile liquid solute, only the solute will form the vapours and solvent will not.
27. Statement I: Molecular mass of polymers cannot be calculated using boiling point or freezing point method.
Statement II: Polymer solutions do not possess a constant boiling point or freezing point.
Hint: Polymer solutions possess very little elevation in boiling point or depression in freezing point.
28. Statement I: If cells of living organisms are placed in pure water, they swell and burst.
Statement II: Due to osmosis, the movement of wa- ter molecules into the cell dilutes the salt content.
29. Statement I: Reverse osmosis is used in the desali- nation of sea water.
Statement II: When the applied pressure is more than the osmotic pressure, pure water is squeezed out of sea water through the membrane.
30. Statement I: Camphor is used as solvent in the de- termination of molecular masses of naphthalene, anthracene, etc.
Statement II: Camphor has high molal elevation constant.
Answer
| 1 - 2 | 2 -1 | 3 - 3 | 4 - 1 | 5 - 4 | 6 - 1 |
| 7 - 3 | 8 - 3 | 9 - 3 | 10 - 4 | 11 - 1 | 12 - 4 |
| 13 - 1 | 14 - 1 | 15 - 1 | 16 - 3 | 17 - 4 | 18 - 1 |
| 19 - 1 | 20 - 3 | 21 - 1 | 22 - 4 | 23 - 4 | 24 - 1 |
| 25 - 1 | 26 - 3 | 27 - 3 | 28 - 1 | 29 - 1 | 30 - 3 |
Class-11
Class-12
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