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. At chemical equilibrium for a reversible reaction in a closed system, which statement is correct?

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

3. The optimum temperature for the Contact process is around

4. The of (AgCl) is expressed as

5. The pH of a solution of ammonium chloride is

6. For the decomposition at equilibrium, which is true?

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

8. A catalyst affects equilibrium by

9. For , at . Calculate .

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

11. The unit of for the reaction is

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

13. According to the Brønsted–Lowry concept, a base is a substance that

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

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

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

17. For a weak monoprotic acid of initial concentration (C) with , Ostwald’s dilution law gives

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

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

20. The value of depends upon

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

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

23. The relationship between Gibbs free energy and reaction quotient is

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

25. For a neutral solution at 25°C,

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

27. The relationship between hydrolysis constant , degree of hydrolysis (h), and concentration (C) for a salt of a weak acid and strong base is

28. A closed flask containing water at shows constant vapour pressure. Which measurement provides direct evidence that liquid–vapour equilibrium is dynamic?

29. For a weak base (B) of concentration (C), the degree of ionization satisfies

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

1. The weak base among the following is

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

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

4. The Contact process involves the oxidation of to : . Increasing pressure will

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

6. The ionization constant of acetic acid is . This indicates it is

7. The pair is an example of

8. The ability of a solvent to dissolve ionic compounds depends mainly on its

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

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

11. Henry’s law for a sparingly soluble gas in a liquid is correctly written as:

12. In the equilibrium (water–gas reaction), the pressure-form expression is

13. The (pH) of a salt solution formed by a weak base and strong acid is given by

14. A reaction is spontaneous in the forward direction when

15. A strong acid is one that

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

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

18. The expression for of is

19. Consider the reversible reaction . If the concentration of is increased at equilibrium, what happens initially?

20. The unit of for the reaction is

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

22. When in a basic buffer, the pH equals

23. Ostwald’s dilution law is not applicable to

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

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

26. The of (AgCl) is expressed as

27. For the gaseous reaction , the relation between and is given by

28. In the presence of a common ion, the degree of ionization of a weak acid (HA)

29. The reaction conditions in the Haber process are typically

30. For , lowering temperature generally leads to

31. For , the correct expression for is:

32. For the reaction , the value of is

33. At chemical equilibrium for a reversible reaction in a closed system, which statement is correct?

34. For the heterogeneous equilibrium , the mass-action law gives:

35. For , with and initial , equilibrium is

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

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

38. When ( Q < K ) for a reaction, the system will

39. Which statement differentiates “dynamic” chemical equilibrium from “static” equilibrium?

40. For an endothermic reaction with , increasing temperature typically

41. The common ion effect is an application of

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

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

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

45. The ionization equation for acetic acid is

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

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

48. Which of the following salts gives an acidic solution in water?

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

50. The (pH) of (0.1,M) increases when the solution is diluted because