Solutions Mock Test – Class 12 Chemistry

1. Consider the following statements about molarity.
Statement I: Molarity changes on dilution if the final volume changes.
Statement II: Molarity uses moles of solute per litre of solution.
Statement III: Molarity remains strictly unchanged with temperature because moles do not change.

2. The freezing point depression for an electrolyte solution is commonly written as:

3. A solute has normal molar mass , but its apparent molar mass from a colligative property is . The van't Hoff factor is:

4. Consider these statements for an ideal binary solution containing a non-volatile solute in volatile solvent .
Statement I: .
Statement II: .
Statement III: .

5. Assuming Raoult's law applies, a pure solvent has vapour pressure . After adding a non-volatile solute, the solute mole fraction is . The lowering of vapour pressure is:

6. For an solution, , , and is dissociated into two ions. The freezing point depression is:

7. When and are known, should be calculated using:

8. A table compares ideal-solution checks.

The row that does not match ideal behaviour is:

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

10. A table of composition terms is shown below.

The row that does not match the term is:

11. A data sheet lists some basic quantities used while discussing solutions.

The entry that connects solution composition directly with the mole concept is:

12. A graph of against for an ideal binary volatile solution is a straight line. Its slope is:

13. A prepared solution is heated slightly, causing its volume to expand without changing the masses of solute and solvent. The pair of concentration terms expected to remain unchanged on this basis is:

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

The row that misapplies Raoult's law is:

15. A problem gives a rise in boiling point, but the selected relation is . The relation that should replace it is:

16. 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:

17. A preparation uses of , and its final volume is made up to . If , the molarity is:

18. A sample contains of a gaseous impurity in of air. If both volumes are measured under the same conditions, the impurity concentration by volume is:

19. A student sees a straight-line graph passing through the origin with slope . The vertical axis is . The horizontal axis must be:

20. A pure solvent has vapour pressure . A solution has relative lowering of vapour pressure . The vapour pressure of the solvent over the solution is:

21. A graph is drawn for a gas obeying Henry's law at fixed temperature, with on the vertical axis and on the horizontal axis. The graph should be:

22. A binary ideal solution has . The partial vapour pressure of is calculated using:

23. Sugar dissolved completely in water is classified by the physical states of solute and solvent as:

24. A solution of a non-volatile nonelectrolyte is prepared in a solvent with . The boiling point elevation is:

25. Assertion: Relative lowering of vapour pressure is a colligative property.
Reason: It depends on the number of solute particles through solute mole fraction, not on the chemical identity of the solute in ideal dilute behaviour.

26. An ideal solution is formed when the interactions , , and are:

27. Gas mixtures used for deep-sea diving are chosen carefully because:

28. A problem gives for a non-volatile solute and asks for a colligative effect without any , , or data. The most likely property being tested is:

29. The nature of the solute and solvent affects solubility because:

30. For a dilute solution of a non-volatile nonelectrolyte, the freezing point depression is given by:

31. In ordinary solute-solvent language, the solute is usually the component that:

32. A classification note says: “All liquid solutions must have a liquid solute and a liquid solvent.” This note is faulty because:

33. An azeotrope is a liquid mixture that:

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

The row that is inconsistent is:

35. A student uses molarity instead of molality in . The main error is:

36. For a solute, the calculated normal boiling point elevation is , but the observed elevation is . The van't Hoff factor is:

37. At a fixed temperature, oxygen obeys Henry’s law in water with . A sample contains of water. The oxygen pressure is increased from to . Assuming no chemical reaction and negligible change in the amount of water, the increase in the mass of dissolved oxygen is:

38. Assertion: Association of solute particles can give a higher apparent molar mass.
Reason: Association decreases the number of independent solute particles in solution.

39. In fractional distillation of an ideal binary solution, the vapour is generally richer in:

40. Negative deviation from Raoult's law is expected when:

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

42. A mixture of acetone and chloroform shows negative deviation because strong hydrogen bonding can form between unlike molecules. The main vapour-pressure effect is:

43. A gas is dissolved in a liquid at constant temperature. Increasing the pressure of the gas above the liquid generally:

44. A laboratory note says . The most suitable interpretation is:

45. A saturated solution at a given temperature is one that:

46. A student says, “A solution is always hypertonic if it contains more grams of solute per litre.” The best correction is:

47. A graph of total vapour pressure versus composition for a binary solution lies above the ideal Raoult's law line over a composition region. The solution shows:

48. A solution is prepared by dissolving of a non-volatile nonelectrolyte in of solvent. The solvent has , and the boiling point elevation is . The molar mass of the solute is:

49. For a binary ideal solution of volatile liquids, , , and . The partial vapour pressure of is:

50. A salt dissociates as . If its degree of dissociation is , the van't Hoff factor is: