Class 11 Chemistry — Chapter 7: Equilibrium Online Test

1. In qualitative inorganic analysis, group IV cations are precipitated in ammoniacal medium because

2. If the solubility of (AgCl) is , the value is

3. When in a basic buffer, the pH equals

4. The hydrolysis constant is defined as

5. The pH of a (0.1,M) solution of is

6. The (pH) of a (0.2,M) solution is

7. The pH of a solution is defined as

8. According to Ostwald’s law, the degree of ionization is related to

9. For a weak base solution where , the hydroxide ion concentration is

10. The ionization constant of an acid is a measure of its

11. In the reaction , the Brønsted–Lowry base is

12. When the concentration of a reactant is increased in a system at equilibrium, the equilibrium

13. The main difference between and is that

14. For a general reaction , the expression for is

15. For at fixed (T), raising the external pressure of an inert gas at constant volume changes the extent of decomposition

16. For at a temperature where , starting with stoichiometric at 1 atm, the equilibrium extent toward is

17. The reaction has at 500 K. If initially is high and are low, the reaction will

18. For the equilibrium , the equilibrium constant expression is

19. For a heterogeneous equilibrium such as , the equilibrium constant is expressed as:

20. For at , . If initially and , the reaction will:

1. A salt formed by a strong acid and a weak base gives a solution that is

2. If the ionic product (Q) is less than , the solution is

3. A salt of a weak acid and a strong base gives a solution that is

4. The variation of the degree of ionization with concentration (( C )) for a weak electrolyte is represented by

5. In the Contact process, the catalyst used to oxidize is

6. Which of the following pairs does not form a buffer solution?

7. The reaction quotient for is given by

8. In at equilibrium, , , and . What value provides evidence of dynamic equilibrium through rate equality?

9. The equilibrium constant for a reaction is expressed as:

10. The principle of fractional precipitation in qualitative analysis is based on

11. A beaker with solid and saturated solution at shows constant conductivity. Which experiment proves dynamic equilibrium at the solid–solution boundary?

12. Which of the following is a correct example of physical equilibrium?

13. The pH of a (0.01,M) solution of (HCl) is

14. The pH of an acidic buffer can be calculated using

15. The degree of ionization of a weak acid is related to its concentration (( C )) as

16. For at a temperature where , starting with stoichiometric at 1 atm, the equilibrium extent toward is

17. For , at . Calculate .

18. Applying pressure to ice near causes it to melt more easily because:

19. For a gaseous equilibrium involving equal moles of reactants and products, a change in pressure

20. In a closed container at fixed (T), liquid–vapour equilibrium is reached when:

21. The main function of a buffer in biological systems is to

22. According to Arrhenius, a base is a substance that

23. For at , . If initially and , the reaction will:

24. When equilibrium is reached in the reaction , what best explains macroscopic constancy?

25. Strong bases are those that

26. The pH of ammonium acetate depends on

27. The coexistence of macroscopic constancy and microscopic reversibility means that:

28. If the solubility of (AgCl) is , the value is

29. If , the hydroxide ion concentration is

30. The optimum temperature for the Contact process is around

1. A solution with has hydrogen ion concentration

2. Which change decreases the solubility of oxygen in water at equilibrium?

3. If an inert gas is added at constant pressure, the equilibrium shifts

4. The Henderson–Hasselbalch equation is most useful for

5. The law of mass action at equilibrium for states that the ratio is:

6. The relation between and obtained from the mass-action law for a gas reaction is:

7. The degree of ionization of a weak acid is related to its concentration (( C )) as

8. The most appropriate thermodynamic statement of chemical equilibrium at constant (T) and (P) is:

9. For at , . If initially and , the reaction will:

10. When , the relation between and becomes

11. According to Lewis acidity/basicity trends, which order of acid strength is most reasonable toward a hard donor like ?

12. In at equilibrium, , , and . What value provides evidence of dynamic equilibrium through rate equality?

13. Which statement about catalysts relates correctly to the definition of equilibrium?

14. The degree of ionization of a weak monoprotic acid (HA) in water is defined as

15. The expression for the acid dissociation constant of is

16. Which of the following statements correctly describes acetic acid solution?

17. For a heterogeneous equilibrium such as , the equilibrium constant is expressed as:

18. What does “macroscopic constancy” mean in a system at equilibrium?

19. If the of is , then the of its conjugate acid is

20. In the reaction , if and , the reaction will

21. When pressure on a gaseous equilibrium is increased, the system shifts

22. Which statement about buffers is true?

23. Which pair correctly represents a Lewis acid–base adduct?

24. The common ion effect is an application of

25. When , the Gibbs free energy change for the reaction is

26. In the esterification system , which experimental result evidences dynamic equilibrium at constant (T)?

27. When equilibrium is reached in the reaction , what best explains macroscopic constancy?

28. Which condition is essential for establishing chemical equilibrium in the laboratory?

29. The (pH) of a (0.05,M) solution is

30. If , the reaction will

31. The equilibrium constant for a gaseous reaction increases with temperature if the reaction is:

32. A salt derived from a weak acid and a weak base gives a solution that is

33. The (pH) of a (0.1,M) acetic acid solution is approximately

34. For the reaction , the difference in gaseous moles is

35. For , if initial and , the equilibrium is

36. A catalyst affects equilibrium by

37. Which kinetic observation most directly evidences dynamic equilibrium in a reversible reaction mixture?

38. In the adduct formation , water behaves as a

39. Weak electrolytes have

40. The degree of ionization of a weak electrolyte generally

41. Which of the following has the smallest degree of ionization in water?

42. For gases behaving ideally, the mass-action expression in terms of partial pressures for is:

43. For an ideal binary solution of volatile components (A) and (B), Raoult’s law states:

44. Which of the following is an example of an Arrhenius acid?

45. Among the following, which has the highest (pH) value for 0.1 M solution?

46. Which of the following best represents a reversible chemical reaction?

47. For , the mass-action expressions are and . At equilibrium, the condition implied is:

48. For a salt , the relationship between and molar solubility (S) is

49. When the ionic product (Q) of a salt solution exceeds , it means

50. The pH of a (0.001,M) (NaOH) solution is