Equilibrium Mock Test – Class 11 Chemistry

1. A basic buffer contains and . If and , its at is closest to

2. A mixture of and is an example of

3. A solution of is prepared. If and , the approximate at is

4. The table gives four dissolved substances and their usual behaviour in water.

The row that best represents a weak electrolyte is

5. For , , and the initial concentration of is with no . The equilibrium concentration of is

6. A salt solution is made from a cation that is the conjugate acid of a weak base and an anion that is the conjugate base of a strong acid. The solution is expected to be

7. A sealed container has liquid water and water vapour at equilibrium at . The volume of the container is increased slightly, but some liquid water remains after re-equilibration. The final vapour pressure is expected to

8. The ionic product of water is written as

9. In a solution containing , the molar solubility of with is approximately

10. For , of is taken initially. If the degree of dissociation is , the total moles at equilibrium are

11. For , at a temperature . The symbolic expression for is

12. A factory chooses a catalyst for an equilibrium process mainly to

13. A reaction begins with only reactants in a closed vessel. As the reaction proceeds toward equilibrium, the forward rate and reverse rate usually change in which way?

14. A weak acid has . Using , the degree of ionization is

15. In an ICE table for an equilibrium calculation, the letter represents

16. A weak electrolyte ionizes as . Its equilibrium expression is

17. For , if molar solubility is , the correct relation is

18. A final equilibrium mixture is described as having no net change, but it still responds when a common ion is added. This is possible because

19. For the equilibrium , the equilibrium concentrations are , , and . The value of is

20. For , of is taken initially. If the degree of dissociation is and total pressure is , is

21. The quantity that most directly tells how much solute is present in a given volume of solution is

22. A mixture for starts with and . At equilibrium, . The value of is

23. For , the concentration equilibrium expression is

24. A concentration-time graph for shows decreasing and increasing. After some time, both curves become horizontal. The horizontal region means that

25. A limitation of the Arrhenius base definition is shown by because

26. A graph for shows decreasing and increasing at first. Later, both curves become horizontal at different concentration values. The best conclusion is that

27. A reaction has . The equilibrium constant for is

28. The unit of becomes absent in the concentration-unit method for a reaction such as

29. A simple reversible physical change is represented by

30. A pressure disturbance graph for shows sudden compression followed by a gradual decrease in the amount of . This is consistent with a shift

31. For , . The equilibrium constant for is

32. A closed bottle contains some water and water vapour above it at a fixed temperature. The water level becomes constant after some time because

33. The relation means that, among acids at the same temperature,

34. In a solution, the molar solubility of is calculated using . The approximate solubility is

35. The reaction quotient has the same algebraic form as , but it is calculated using

36. For , the solubility product expression is

37. A physical equilibrium can be recognized most safely by

38. For a gaseous reaction, even though the reaction is not trivial. This can happen when

39. The graph description “a sudden concentration jump followed by a gradual shift” is best interpreted as

40. A liquid-vapour equilibrium fails to establish in an open container mainly because

41. A solution of a salt of weak base and strong acid has parent base . At , using , the approximate is closest to

42. A chemistry record says: “A weak acid buffer is prepared, then a small amount of is added, and later is added to test for .” The two main equilibrium ideas involved are

43. A rate-time graph for a reversible reaction shows the forward rate decreasing and the reverse rate increasing until both become equal. The point where the two rate curves meet represents

44. A solution is called saturated at a given temperature when

45. For , if the molar solubility is , the ion concentrations are

46. For the same pure liquid in a closed vessel, vapour pressure at equilibrium is higher at than at because

47. A pressure-based calculation for a gas mixture gives partial pressures before using . The step most likely to give a wrong answer is

48. A claim says, “If a pure solid and its liquid are present together, they must always be at equilibrium.” The claim needs the condition that

49. A weak acid solution has and . Using , the is

50. Two equations are related as shown:


The value of is