Solutions Mock Test – Class 12 Chemistry

1. For an ideal solution, the enthalpy change of mixing and volume change of mixing are respectively:

2. An osmotic-pressure sample contains of a nonelectrolyte solute in solution. Its osmotic pressure at is . Using , the molar mass of the solute is:

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

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

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

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

7. 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.

8. A semipermeable membrane separates pure solvent from a solution. The pressure required to just stop osmosis is called:

9. A mixture contains dissolved in water under pressure. For the usual description of this solution, the solute and solvent are respectively:

10. In two boiling point elevation experiments using the same solvent, equal masses of non-volatile nonelectrolyte solutes, and the same mass of solvent, the smaller observed corresponds to:

11. A gas has partial pressure over a liquid at a fixed temperature. If , the mole fraction of the gas in the solution is:

12. A table about Henry's law applications is shown below.

The row that needs correction is:

13. 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:

14. A non-volatile solute lowers the freezing point of a solvent because:

15. A comparison of solubility trends is shown below.

The row that needs correction is:

16. Association of solute molecules affects colligative properties because it:

17. Boiling point elevation and freezing point depression are similar because both:

18. The membrane required for osmosis should:

19. A table compares deviation types.

The row that needs correction is:

20. 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:

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

22. A liquid solution is called non-ideal when it:

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

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

25. The osmotic pressure of a dilute solution at temperature is related to moles of solute , solution volume , and gas constant by:

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

27. A table gives four situations.

The row that needs correction is:

28. A non-volatile nonelectrolyte is dissolved in a volatile solvent. The solution shows , , and . These observations are best explained by:

29. A water sample contains of a dissolved impurity in of water sample. Assuming the solution mass is , the concentration of impurity is:

30. 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.

31. The unit of molarity is:

32. For complete dissociation of , the van't Hoff factor is:

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

34. Molarity of a solution is expressed as:

35. In a molality calculation, of solute is dissolved in of water. The mass that belongs in the denominator is:

36. In a sealed carbonated drink, is kept dissolved in a larger amount mainly by:

37. 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:

38. At high altitude, oxygen availability to the body decreases mainly because:

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

The row that needs correction is:

40. A supersaturated solution is best described as a solution that:

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

42. The total vapour pressure of an ideal binary solution of volatile liquids is:

43. 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:

44. Osmosis is the movement of:

45. The general relation between , degree of dissociation , and number of particles formed per formula unit is:

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

47. 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:

48. 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:

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

50. A sealed carbonated drink contains dissolved under high pressure. When the bottle is opened, bubbles appear mainly because: