Solutions Mock Test – Class 12 Chemistry

1. The mass percentage of a solute is defined using:

2. Warm water usually holds less dissolved gas than cold water because:

3. A student calculates mole fraction of solute by using . The main correction is:

4. A pure solvent boils at . A solution containing of a non-volatile nonelectrolyte in of solvent boils at . If , the molar mass of the solute is:

5. A solution of is completely dissociated. At the same temperature, its osmotic pressure is how many times that of glucose?

6. For an ideal binary solution containing a non-volatile solute in a volatile solvent, the solvent mole fraction is . The relative lowering of vapour pressure is:

7. For a non-volatile nonelectrolyte, the only composition data supplied are moles of solute and moles of solvent. To calculate relative lowering of vapour pressure, the next useful step is to find:

8. A bottle label says ethanol in water. This means:

9. A liquid mixture obeys Raoult's law over the composition range considered. For component , reducing from to at the same temperature will:

10. A pair of liquids is likely to form a nearly ideal solution when the two liquids have:

11. To prepare a solution using of solvent, the required amount of solute is:

12. A graph comparison is made for four binary liquid mixtures.

The row that is inconsistent is:

13. Antifreeze added to water in a radiator helps mainly because it:

14. A student uses instead of while calculating freezing point depression. The main error is:

15. Complete dissociation occurs in a aqueous solution. At , using , its osmotic pressure is:

16. A homogeneous mixture contains nitrogen, oxygen, argon, and carbon dioxide. Based on component count, it is best described as:

17. For an ideal binary solution of volatile liquids, the graph of against at fixed temperature is:

18. Two mixtures remain stable without visible settling. When a narrow beam of light is passed through them, the path of the beam is invisible in Mixture P but clearly visible in Mixture Q. The most suitable classification is:

19. A plant cell placed in pure water swells because:

20. Consider a solution that is ideal, dilute, and contains a non-volatile nonelectrolyte solute. The safest overall statement is:

21. Case P contains of sugar in of water, while Case Q contains of sugar in of water. Based on solute-to-solvent mass ratio:

22. A table is written for an ideal binary volatile solution.

The row that misapplies Raoult's law is:

23. The terms dilute and concentrated mainly compare:

24. Abnormal molar mass obtained from a colligative property usually indicates that the solute:

25. Consider the following statements for an ideal binary solution of volatile liquids.
Statement I: .
Statement II: .
Statement III: is found by multiplying with .

26. For an ideal binary solution with a non-volatile solute in solvent , the relation between relative lowering of vapour pressure and solute mole fraction is:

27. A mixture of liquids and follows Raoult's law over the entire composition range. It also shows no heat change and no volume change on mixing. This mixture is best described as:

28. A Henry's law value quoted at should not be used unchanged at because:

29. Equal-concentration glucose and urea solutions, each , are at the same temperature. If both behave ideally and do not dissociate, their osmotic pressures are:

30. Benzoic acid, with normal molar mass , gives an observed molar mass of in benzene. Assuming that benzoic acid undergoes only dimerisation, the degree of association is:

31. The vapour pressure of a pure liquid is the pressure exerted by:

32. A portion of liquid solute is diluted to a final solution volume of . The volume percentage of the solute is:

33. A mixture of benzene and toluene is often treated as nearly ideal because the two liquids have similar structures and intermolecular forces. The most reasonable expectation is:

34. A non-volatile nonelectrolyte solution shows in a solvent with . The same solution in the same solvent has . Its freezing point depression is nearest to:

35. A graph of versus molality for a non-volatile nonelectrolyte solution is a straight line. The slope of this graph is:

36. Two gases give straight-line Henry's law plots of versus at the same temperature. Line is steeper than line . At the same pressure, the dissolved mole fraction is:

37. Assertion: Molarity can change when the temperature of a solution changes.
Reason: Molarity uses volume of solution in its denominator, and liquid volume can expand or contract with temperature.

38. A student chooses for a question that gives solution volume, osmotic pressure, temperature, and solute mass. The main issue is:

39. For an electrolyte, a versus graph has slope . If the solvent has , the van't Hoff factor is:

40. A data table for aqueous solutions at the same temperature is shown below.

The decreasing order of osmotic pressure is:

41. Henry's law applies to a gas at a fixed temperature with . If the mole fraction of the gas in solution is , its partial pressure is:

42. A pure solvent freezes at . A solution of a non-volatile solute in it freezes at . The freezing point depression is:

43. In the notation of a binary solution, components and are used. The safest interpretation of and at this stage is that they are:

44. A solution has osmotic pressure at temperature . If its concentration is doubled and the absolute temperature is also doubled, the new osmotic pressure becomes:

45. The versus line at fixed temperature passes through the origin. This is expected because:

46. A crystal of the same solute is added to four solutions at the same temperature. The observation most consistent with an unsaturated solution is:

47. Consider the following statements.
Statement I: is calculated as .
Statement II: is calculated as .
Statement III: Both and are proportional to molality for dilute solutions.

48. Measured values are , , and . The van't Hoff factor is:

49. The membrane required for osmosis should:

50. Mole fraction of component in a solution is defined as: