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. For , if and initial concentrations of all species are , then equilibrium concentrations will

2. The Henderson–Hasselbalch equation is most useful for

3. For at equilibrium, the concentration form predicted by the mass-action law is:

4. The weak base among the following is

5. For liquid–vapour equilibrium of benzene at , which observation verifies molecular exchange despite constant vapour pressure?

6. Which of the following solvents would favor maximum ionization of NaCl?

7. When temperature increases, the numerical value of relative to :

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

9. A saturated solution of (AgCl) at 25°C has . What is ?

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

11. For , the correct expression is

12. When the concentration of a weak acid is decreased to one-fourth, the degree of ionization

13. The conjugate base of is

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

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

16. A nonvolatile solute is dissolved in a solvent with at a given (T). If the solute mole fraction is , the solution’s vapour pressure is:

17. For a weak electrolyte whose limiting molar conductivity at infinite dilution is and measured molar conductivity at concentration (C) is , the degree of ionization is

18. The salt of a weak base and a strong acid shows acidic reaction because

19. When , the relation between and becomes

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

21. If , the hydroxide ion concentration is

22. Which of the following best expresses the definition of physical equilibrium?

23. For , if and initial concentrations , the equilibrium is approximately

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

25. The product of and ( C ) for a weak acid at a given temperature is

26. The Henderson–Hasselbalch equation for an acidic buffer is

27. In the Contact process, the final step involves converting into sulfuric acid by

28. Consider in a closed vessel. The equilibrium constant depends on

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

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

1. If and are two concentrations of the same weak acid and are their ionizations, then

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

3. In at constant temperature, the equilibrium constant is numerically equal to

4. For the general reaction , the unit of can be expressed as

5. For at 298 K with and initial , the direction to reach equilibrium is

6. The expression for the hydrolysis constant of a salt of a weak base and a strong acid is

7. Which of the following compounds cannot be classified as an Arrhenius acid or base?

8. For , the equilibrium constant in concentration terms is

9. For a reaction at temperature (T), which equation connects the definition of equilibrium with thermodynamics?

10. In a gaseous equilibrium, decreasing the concentration of reactants will cause

11. The pH of a basic buffer is given by

12. Which of the following is a basic buffer?

13. The importance of the solubility product lies in its use for

14. The Arrhenius concept is limited to

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

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

17. In the Brønsted–Lowry theory, the strength of an acid is inversely related to

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

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

20. A strong acid is one that

21. Which of the following is a weak base?

22. For , the appropriate constant at (T) is

23. For the decomposition reaction , the equilibrium constant is derived as:

24. The conjugate base of is

25. For a weak electrolyte whose limiting molar conductivity at infinite dilution is and measured molar conductivity at concentration (C) is , the degree of ionization is

26. For the reaction , the equilibrium constant in terms of concentration is derived by equating:

27. In the reaction , the equilibrium is

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

29. The low ionizing power of solvents like benzene is due to

30. When , the system’s free energy is

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

32. If , the hydroxide ion concentration is

33. The degree of ionization of an electrolyte is higher in solvents having

34. If an inert gas is added at constant volume to a gaseous equilibrium mixture, the equilibrium position

35. Which observation best demonstrates that equilibrium is dynamic rather than static in a saturated solution of sugar at constant (T)?

36. In a closed system at equilibrium, what would indicate microscopic reversibility?

37. Which statement best captures the scope advantage of the Lewis concept?

38. For liquid–vapour equilibrium of benzene at , which observation verifies molecular exchange despite constant vapour pressure?

39. The equilibrium constant for the reaction in terms of partial pressures is:

40. The salt formed from (NaOH) and (HCl) will have a pH value of

41. Which interaction most clearly illustrates Lewis acidity of a metal cation in solution?

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

43. Which condition is inherently included in the definition of equilibrium for a reaction mixture?

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

45. The Haber process is exothermic. Which change increases the equilibrium yield of ?

46. Removing a product from a reversible reaction mixture will

47. According to Arrhenius, an acid is a substance that

48. The relation between hydrogen ion concentration and the initial concentration ( C ) of a weak acid is

49. The common ion effect is an application of

50. The conjugate base of a strong acid is always