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

2. If for the reaction at 300 K, the value of is

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

4. For most ionic solids dissolving endothermically in water , increasing temperature will:

5. For a weak acid solution, if concentration decreases 100 times, the degree of ionization increases approximately by a factor of

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

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

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

9. The ionization of acetic acid decreases on addition of sodium acetate because

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

11. Which statement best defines chemical equilibrium in a closed system?

12. The pH of a solution of sodium chloride ((NaCl)) is

13. Which of the following best represents the neutralization of an acid and a base according to Arrhenius?

14. The solubility product constant is defined as

15. For a gaseous system, the reaction quotient in terms of partial pressure is represented as

16. For with and initial , the equilibrium fraction of (A) converted is

17. The pH of sodium acetate solution is

18. For , the correct expression for is

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

20. Which of the following is an example of an acidic buffer?

21. Le Chatelier’s principle states that when a system at equilibrium is subjected to a change,

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

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

24. When equilibrium is attained in a reversible reaction:

25. Which of the following is the best Lewis base toward ?

26. A buffer solution is defined as a solution which

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

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

29. For gaseous reactions, the equilibrium constant is related to partial pressures by:

30. For a salt of a weak acid and strong base, the expression for pH is

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

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

3. In dissolution equilibrium of a solid in a liquid (at fixed (T)), which action increases the amount of undissolved solid without changing solubility?

4. In the reaction , the conjugate base of the acid (HCl) is

5. If the equilibrium constant for a reaction decreases with temperature, the reaction is

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

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

8. The main difference between a weak acid and a weak electrolyte is that

9. For a neutral solution at 25°C,

10. According to Le Chatelier’s principle, if the concentration of a reactant is increased, the system will

11. Which of the following best represents the neutralization of an acid and a base according to Arrhenius?

12. Which condition is required for a reversible reaction to reach equilibrium?

13. For a weak acid solution, if concentration decreases 100 times, the degree of ionization increases approximately by a factor of

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

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

16. If for a given reaction mixture, the reaction will

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

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

19. For , the equilibrium constant in concentration terms is

20. The relation is valid only when

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

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

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

24. Which of the following statements is true for homogeneous equilibrium systems?

25. If for a gaseous reaction, the relation between and is:

26. The salt of a weak acid and weak base gives a solution that is

27. The degree of ionization of a weak electrolyte generally

28. For the decomposition reaction , the unit of is

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

30. In the equilibrium , increasing total pressure shifts equilibrium

31. For the reaction with and initial concentrations , , the equilibrium concentration of (B) is

32. Which of the following statements correctly describes a limitation of the Arrhenius concept?

33. Decreasing pressure on a gaseous equilibrium mixture causes the equilibrium to shift

34. If , the reaction will proceed

35. Which of the following is an example of an Arrhenius base?

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

37. In the Contact process, lowering the temperature increases the yield of because the reaction is

38. The pH of ammonium acetate depends on

39. If for a certain gaseous system and the calculated , the direction of reaction is

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

41. When , the system’s free energy is

42. The concept of microscopic reversibility is supported by which scientific law?

43. The Henderson–Hasselbalch equation for a basic buffer is expressed as

44. Temperature generally affects degree of ionization of weak acids/bases by

45. In the Haber process, lowering the temperature will

46. Which statement best describes the “dynamic” nature of equilibrium?

47. In a homogeneous equilibrium, all the reactants and products are present in

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

49. According to Ostwald’s dilution law, for a weak acid ( HA ), the dissociation constant is given by

50. The base ionization constant expresses