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 degree of ionization of a weak acid in the presence of its strong electrolyte salt is

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

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

4. For a reaction , the direction of the reaction can be predicted by comparing

5. For at 298 K, . The predicted extent toward (B) is

6. For , the correct expression for is:

7. For , with and initial , equilibrium is

8. The dissociation of is suppressed by adding

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

10. At the melting point of a pure solid in a closed system, solid–liquid equilibrium is characterized by:

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

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

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

14. In the Haber process, lowering the temperature will

15. Using the Henderson equation, the pH of a buffer containing (0.1,M) acetic acid and (0.1,M) sodium acetate is

16. According to the Lewis concept, a Lewis acid is defined as a species that

17. The relationship between and for a conjugate acid–base pair is

18. The conjugate base of a strong acid is always

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

20. Which of the following is NOT implied by the definition of chemical equilibrium?

21. For the reaction with and initial , the equilibrium is

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

23. If the ionic product equals the solubility product , the system is

24. Which statement is true about the relation between and ( C )?

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

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

27. The pH of ammonium chloride solution is

28. If , the hydroxide ion concentration is

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

30. Why does a chemical system at equilibrium appear static to the observer?

1. Which statement best explains why is a Lewis acid?

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

3. For a neutral solution at 25°C,

4. The conjugate base of is

5. Using the Henderson equation, the pH of a buffer containing (0.1,M) acetic acid and (0.1,M) sodium acetate is

6. Ostwald’s dilution law fails for strong electrolytes because

7. Which of the following is a strong acid?

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

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

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

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

12. The derivation of from assumes that:

13. Which of the following salts produces a basic solution when dissolved in water?

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

15. For , the correct expression for is

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

17. When ( Q > K ), the direction of spontaneous change is

18. In a buffer containing and , the pH is calculated using

19. The unit of for the reaction is

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

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

22. In the Haber process, which change increases the rate of attainment of equilibrium without changing the equilibrium composition?

23. Buffers are important in analytical chemistry because they

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

25. The relation between force of attraction ( F ) and dielectric constant ( D ) is

26. The pH of ammonium chloride solution is

27. Which of the following is not a weak electrolyte?

28. Identify the Lewis acid in the reaction .

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

30. For a system with , , the sign of is

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

32. The of (AgCl) is expressed as

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

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

35. If , the reaction will

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

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

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

39. In the equilibrium , the equilibrium constant in pressure form is

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

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

42. The (pH) of a (0.01,M) (NaOH) solution is

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

44. When a reversible reaction attains equilibrium, what remains constant?

45. For a reaction , the direction of the reaction can be predicted by comparing

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

47. For the reaction , the relation between and will be

48. Ostwald’s dilution law is not applicable to

49. Microscopic reversibility in a reaction means:

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