Solutions Mock Test – Class 12 Chemistry

1. 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:

2. A solution has density . If the solute molar mass is , the mass percentage of solute is:

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

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

4. With dimerisation in a solvent, a normal osmotic-pressure calculation gives . The observed osmotic pressure is:

5. For a gas at fixed partial pressure, a larger value of means:

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

7. A maximum-boiling azeotrope is commonly linked with:

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

9. For a dilute solution containing grams of a nonelectrolyte solute in volume , osmotic pressure is measured at temperature . The molar mass is given by:

10. A record for saturated solutions contains these statements.
Statement I: A saturated solution contains the maximum dissolved solute under stated conditions.
Statement II: In a saturated solution with undissolved solute present, dissolution and crystallisation can continue at equal rates.
Statement III: Once a solution is saturated at one temperature, it remains saturated at all temperatures.

11. For the association , the normal calculated freezing point depression is . If the degree of association is , the observed depression is:

12. A lake receives warm discharge water from a nearby plant. The dissolved oxygen level in the warmer region may decrease because:

13. 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:

14. A table for molar-mass determination from boiling point elevation is given below.

The row that needs correction is:

15. A aqueous solution contains:

16. For a non-volatile nonelectrolyte in a fixed solvent, the molality is . If this molality is increased to , both and become:

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

18. The phase of a solution is generally decided by the:

19. Consider the following statements about freezing point depression.
Statement I: is positive when written as .
Statement II: for dilute solutions of non-volatile solutes.
Statement III: is the molal elevation constant used for boiling point.

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

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

22. In an ideal binary solution, and . The total vapour pressure line plotted against has slope:

23. Assertion: In positive deviation from Raoult's law, molecules escape more easily from the solution.
Reason: The interactions are weaker than the and interactions.

24. The boiling point elevation formula corrected using van't Hoff factor is:

25. A table compares azeotrope types.

The row that needs correction is:

26. At and , a gas is moderately soluble in a liquid. The condition expected to give the highest gas solubility is:

27. The total-vapour-pressure graph versus composition for a binary solution lies below the ideal Raoult's law line. This indicates:

28. A table compares boiling point elevation and freezing point depression.

The row that needs correction is:

29. Glucose is dissolved in of water. If of water is , the freezing point of the solution is approximately:

30. A solution contains glucose in of water. If , the molality is:

31. Henry's law for a gas dissolved in a liquid at constant temperature is most suitably written as:

32. A liquid mixture contains of ethanol and of water. The mole fraction of ethanol is:

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

34. Two liquid preparations are described below.
Case 1: solute is made up to solution.
Case 2: solute is mixed with solvent, and volumes are assumed additive.
Under the stated assumption, the volume percentages in Case 1 and Case 2 are respectively:

35. The association summary below contains one faulty row.

The row that needs correction is:

36. The unit of in is:

37. A solution of a solute with is prepared in a solvent with . The boiling point elevation is:

38. A student reports a negative value of after using . The correction is:

39. A table for degree of dissociation is shown below.

The row that needs correction is:

40. 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:

41. A report compares four concentration terms for a dissolved solid.

The mismatched entry is:

42. Osmosis is the movement of:

43. A aqueous solution of a nonelectrolyte has density . If the solute molar mass is , its molarity is closest to:

44. A solution shows larger elevation in boiling point than expected from the formula using the molecular solute amount. A likely reason is:

45. A solution of a solute that associates as has observed osmotic pressure . The normal osmotic pressure calculated without association is . The degree of association is:

46. Adding a non-volatile solute to a volatile solvent generally lowers the solvent vapour pressure because:

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

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

49. dimerisation gives . The degree of association is:

50. The relation between van't Hoff factor, normal molar mass, and abnormal molar mass is: