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

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

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

4. For a system at constant (T) and (P), a spontaneous process always has

5. For a general reaction , the expression for is

6. The pH of an acidic buffer can be calculated using

7. For an endothermic reaction with , increasing temperature typically

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

9. The unit of for the reaction is

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

11. If , the reaction will

12. For a weak acid where is very small, Ostwald’s dilution law simplifies to

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

14. Which of the following is a strong acid?

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

16. A catalyst affects equilibrium by

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

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

19. For , the correct expression for is:

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

21. Which of the following reactions illustrates amphoteric behavior of water?

22. In the reaction , the equilibrium is

23. For a weak acid with and , the degree of ionization is

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

25. Which of the following pairs will show a common ion effect?

26. If for a reaction and , the reaction will

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

28. The dissociation of is suppressed by adding

29. A reaction is spontaneous in the forward direction when

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

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

2. For the reaction , what type of equilibrium is established?

3. If the dielectric constant of a medium increases, the force of attraction between ions

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

5. For the reaction , the unit of is

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

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

8. For the reaction , the units of are

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

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

11. The pH of ammonium acetate depends on

12. Buffers are important in analytical chemistry because they

13. The relationship between pH and pOH at 25°C is

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

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

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

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

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

19. The solubility product constant is defined as

20. For , lowering temperature generally leads to

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

22. The relationship between and for a gas-phase equilibrium is:

23. For the reaction , the relation between and is

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

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

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

27. The (pH) of a salt solution formed by a weak acid and strong base can be expressed as

28. The equilibrium is homogeneous because

29. The pH of a solution of potassium nitrate is

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

31. If for a base, the strength of the base is

32. For , the correct expression is

33. For at , . If initially and , the reaction will:

34. 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

35. A buffer solution is defined as a solution which

36. The salt of a strong base and a weak acid shows alkaline reaction because

37. The pH of a solution of sodium acetate is

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

39. For , with and initial , equilibrium is

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

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

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

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

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

45. When , the reaction

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

47. Which of the following is a basic buffer?

48. When in an acidic buffer, the pH equals

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

50. The dissociation of is suppressed by adding