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 reaction conditions in the Haber process are typically

2. The derivation of from assumes that:

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

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

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

6. For a neutral solution at 25°C,

7. When , the Gibbs free energy change for the reaction is

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

9. The reaction is a homogeneous equilibrium because

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

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

12. Which of the following pairs correctly shows the order of increasing ionization?

13. The reversible decomposition of calcium carbonate is an example of:

14. The pH of a solution is defined as

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

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

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

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

19. In the Contact process, the final step involves converting into sulfuric acid by

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

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

22. A buffer solution contains and . If , then pH = ?

23. For at 298 K with and initial , the direction to reach equilibrium is

24. Which statement best captures the scope advantage of the Lewis concept?

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

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

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

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

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

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

1. In the reaction , the equilibrium is

2. The solubility product differs from the ionic product in that

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

4. The pH of a basic buffer is given by

5. The equilibrium is homogeneous because

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

7. The of (AgCl) is expressed as

8. The relation is valid only when

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

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

11. The units of for are

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

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

14. The pH of a solution of ammonium chloride is

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

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

17. When in a basic buffer, the pH equals

18. In the reaction , the Brønsted–Lowry base is

19. The conjugate base of a strong acid is always

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

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

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

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

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

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

26. In the Contact process, the final step involves converting into sulfuric acid by

27. If , the reaction will proceed

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

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

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

31. If and are two concentrations of the same weak acid and are their ionizations, then

32. The conjugate acid of a strong base is

33. The pOH of a solution is defined as

34. In qualitative analysis, group II cations like , , and are precipitated as sulfides in acidic medium because

35. The reversible decomposition of calcium carbonate is an example of:

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

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

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

39. The term in the expression represents

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

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

42. If for a reaction and , the reaction will

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

44. For , at . Calculate .

45. Which of the following acids is weak?

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

47. The optimum temperature for the Contact process is around

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

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

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