Solutions Mock Test – Class 12 Chemistry

1. A binary ideal solution has , , and . The contribution of to the total vapour pressure is:

2. A non-volatile nonelectrolyte solution has and . If , the value of for the same solvent is:

3. A solution shows and . This observation most directly suggests:

4. A student writes after starting from Henry's law . The correction is:

5. In reverse osmosis used for desalination, the semipermeable membrane mainly allows:

6. A density-linked concentration conversion is most likely required when:

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

The row that needs correction is:

8. A student calculates relative lowering as . The correction is to divide by:

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

10. A statement says, “The vapour pressure of a solution is discussed without fixing temperature because temperature has no effect on vapour pressure.” The best correction is:

11. Assertion: An ideal solution obeys Raoult's law over the entire composition range.
Reason: In an ideal solution, unlike interactions are very different from like interactions.

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

The decreasing order of osmotic pressure is:

13. A true solution is best described as a mixture in which the components are:

14. 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:

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

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

The mismatched entry is:

17. A saline solution is separated from pure water by a semipermeable membrane. A pressure larger than its osmotic pressure is applied on the saline side. The expected result is:

18. A weak electrolyte dissociates as . If the degree of dissociation is , the van't Hoff factor is:

19. A table compares ideal-solution checks.

The row that does not match ideal behaviour is:

20. Trimer formation gives . The degree of association is:

21. The situation-relation pairing that is mismatched is:

22. Simple fractional distillation cannot separate an azeotropic mixture at its azeotropic composition because:

23. A table gives four situations.

The row that needs correction is:

24. A non-volatile solute dimerizes in a solvent. If its normal calculated freezing point depression is , the observed freezing point depression is:

25. A student is comparing two colligative-property questions. Case gives , , solute mass, and solvent mass. Case gives , , , and solute mass. The correct pairing is:

26. Assertion: Soda water is classified as a liquid solution.
Reason: The phase of a solution is generally determined by the solvent, and water is the solvent in soda water.

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

28. For a very dilute aqueous solution, by mass most nearly represents:

29. The molecular reason for non-ideal behaviour is best stated as:

30. For an ideal solution of two volatile liquids and , Raoult's law for component is:

31. 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.

32. A sample contains glucose dissolved in water to make solution. Given , the concentration term that can be calculated directly from the given data without density is:

33. The unit of in the Henry's law relation is:

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

35. A gas chemically reacts with water after dissolving. A simple Henry's law calculation may fail because:

36. A hot saturated solution of is cooled carefully without disturbance and remains clear, even though its concentration is higher than the normal solubility at the lower temperature. The solution is:

37. A learner calculates mass percentage by using . The main error is:

38. The unit of in is:

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

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

The row that needs correction is:

41. 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:

42. Consider the following statements about true solutions.
Statement I: A true solution has uniform composition throughout.
Statement II: A true solution may be solid, liquid, or gas.
Statement III: A true solution must always be colourless.

43. 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:

44. The association summary below contains one faulty row.

The row that needs correction is:

45. The association result that is not consistent with the stated process is:

46. A pure solvent freezes at . A solution has . The freezing point of the solution is:

47. A substance has molar mass . The amount of substance in of it is:

48. A solute shows in a solvent. If the normal calculated osmotic pressure is , the observed osmotic pressure is:

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

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