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

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

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

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

5. The common ion effect refers to

6. The equilibrium is homogeneous because

7. For a weak acid with small , the degree of ionization is approximately proportional to

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

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

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

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

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

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

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

15. If , the reaction will

16. The hydrolysis constant of at 25°C is . If , then the base dissociation constant of is approximately

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

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

19. Which of the following is a basic buffer?

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

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

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

23. In the adduct formation , water behaves as a

24. For , the correct expression for is:

25. According to Arrhenius, which of the following aqueous solutions has the highest concentration of ions?

26. For the decomposition reaction , the unit of is

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

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

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

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

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

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

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

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

5. The molar solubility (S) of a salt in terms of is

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

7. The of (AgCl) is expressed as

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

9. The conjugate base of is

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

11. The degree of hydrolysis ((h)) of a salt of a weak acid and strong base is given by

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

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

14. Buffers are important in analytical chemistry because they

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

16. The degree of ionization of a weak electrolyte generally

17. The pH of a weak acid solution increases upon addition of its salt because

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

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

20. The common ion effect refers to

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

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

23. When , the reaction

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

25. According to Arrhenius theory, neutralization occurs when

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

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

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

29. For a weak acid with small , the degree of ionization is approximately proportional to

30. In deriving the mass-action rate law for products, the reaction rate at fixed (T) is proportional to:

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

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

33. If a solution has , what is its ( pH ) value?

34. If for a reaction and , the reaction will

35. In the Haber process , increasing the pressure will

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

37. Which statement about a catalyst and equilibrium is correct?

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

39. Consider with at 298 K. Starting from , the expected equilibrium is

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

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

42. For , the correct expression for is

43. The Henderson–Hasselbalch equation is most useful for

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

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

46. The pH of ammonium chloride solution is

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

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

49. In a mixture of acetic acid and sodium acetate, the concentration of ions is governed mainly by

50. The ionization equation for acetic acid is