Solutions Mock Test – Class 12 Chemistry

1. The terms dilute and concentrated mainly compare:

2. Solubility is best understood as a quantity that depends on:

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

4. The van't Hoff factor is used in colligative properties mainly to account for:

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

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

The row that is inconsistent is:

7. A boiling-point experiment uses of a non-volatile nonelectrolyte of molar mass in of solvent. If , the boiling point elevation is:

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

9. Four labels are written for concentration expressions.

The label that is not consistent with percentage convention is:

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

11. A versus graph for a solute in a solvent has slope smaller than of that solvent. The solute most likely:

12. For an ideal binary solution with non-volatile solute , . The ratio is:

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

14. A beaker contains a saturated salt solution with some undissolved salt at the bottom. At constant temperature, the particle-level process in the solution is best described as:

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

16. In a positive-deviation solution, the boiling point compared with the ideal expectation is often lower because:

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

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

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

20. An ideal solution has , , and . The total vapour pressure and vapour-phase mole fraction of are respectively:

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

The row that needs correction is:

22. Reverse osmosis occurs when:

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

24. For an ideal solution, a plot of solvent vapour pressure against solvent mole fraction follows:

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

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

The row that misapplies Raoult's law is:

27. A table about van't Hoff factor is shown below.

The row that needs correction is:

28. The missing conversion in the statement “ ______ ” is:

29. In a binary solution containing components and , the word binary tells us that the solution contains:

30. For a solution containing a non-volatile solute in a volatile solvent , Raoult's law for the solvent is:

31. Use the descriptions below. Vessel P contains sugar dissolved completely in water, Vessel Q contains oil and water in two visible layers, Vessel R contains uniformly mixed air, and Vessel S contains muddy water that settles on standing. The pair that represents homogeneous solutions is:

32. A carboxylic acid forms hydrogen-bonded dimers when dissolved in benzene. Compared with the values expected if no association occurred, the solution should show:

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

34. During preparation of a molar solution, a solid solute is dissolved in water and then the solution is made up to the mark in a volumetric flask. The volume used in is:

35. The osmotic pressure equation modified for association or dissociation is:

36. The mass by volume percentage of a solution is based on:

37. A solution of is dissociated into and . At the same temperature, its osmotic pressure compared with a nonelectrolyte solution is:

38. In a Henry's law graph of versus , the slope represents:

39. A non-volatile nonelectrolyte solution is prepared in water. If , the freezing point depression is:

40. A solute undergoes dimerisation in a solvent. The van't Hoff factor is:

41. A table compares some records involving molarity.

The record that needs correction is:

42. Molarity of a solution is expressed as:

43. In a final check of a colligative-property calculation, the result was obtained for a solute claimed to dissociate into ions. The result suggests that:

44. A weak electrolyte gives and dissociates as . Its degree of dissociation is:

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

46. A student uses total solution mass instead of solvent mass while finding molar mass from . The main error is that:

47. A patient is placed in an oxygen-rich environment where the partial pressure of is increased. The expected effect on dissolved oxygen in blood, at the same temperature and within suitable limits, is:

48. An ideal solution has , , and contains a non-volatile solute. The solute mole fraction is:

49. A record says that mole fraction has no unit. The reason is that:

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