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 of the following is the best Lewis base toward ?

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

3. For a reaction at 298 K where , (K) is approximately

4. For a reaction at temperature (T), which equation connects the definition of equilibrium with thermodynamics?

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

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

7. The reaction quotient for is given by

8. For a general reaction , the expression for is

9. The Henderson–Hasselbalch equation for an acidic buffer is

10. In the Contact process, the catalyst used to oxidize is

11. In the Haber process, the catalyst used is

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

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

14. For the dissociation , the correct mass-action expression in pressure terms is:

15. The ionization equation for acetic acid is

16. If at 298 K for with initial and , the reaction extent toward (B) at equilibrium will be

17. The Henderson–Hasselbalch equation is derived from

18. The Henderson–Hasselbalch equation is most useful for

19. The main difference between and is that

20. When a reversible reaction reaches equilibrium, what remains unchanged at the macroscopic level?

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

22. The of (AgCl) is expressed as

23. Microscopic reversibility in a reaction means:

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

25. The derivation of from assumes that:

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

27. Which of the following statements is true regarding the common ion effect?

28. The dielectric constant of a solvent affects the ionization of an electrolyte because it

29. When the concentration of a product is increased in a reversible reaction, the equilibrium

30. The conjugate base of is

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

2. For the reaction , the equilibrium constant in terms of concentration is derived by equating:

3. Which of the following statements correctly describes acetic acid solution?

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

5. If , the hydroxide ion concentration is

6. For the reaction , the units of are

7. The dielectric constant of water at 25°C is approximately

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

9. If for a reaction and , the reaction will

10. When the concentration of a product is increased in a reversible reaction, the equilibrium

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

12. In the reversible reaction , what will happen if the pressure is increased?

13. For at fixed (T), raising the external pressure of an inert gas at constant volume changes the extent of decomposition

14. Ostwald’s dilution law helps to determine

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

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

17. The degree of ionization of an electrolyte is higher in solvents having

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

19. For a salt of a weak acid and strong base, the expression for pH is

20. The unit of for the reaction is

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

22. For the decomposition reaction , the unit of is

23. In the Brønsted–Lowry theory, the strength of an acid is inversely related to

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

25. A solution with has hydrogen ion concentration

26. The of (AgCl) is expressed as

27. For the equilibrium , the equilibrium constant expression is

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

29. Which is a correct necessary condition embedded in the definition of chemical equilibrium for a gas-phase reaction?

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

31. The pH of a solution is defined as

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

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

34. Which of the following pairs does not form a buffer solution?

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

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

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

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

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

40. The conjugate base of is

41. The equilibrium is homogeneous because

42. If , the reaction will

43. The term in the expression represents

44. A salt formed by a strong acid and a strong base (e.g., ( NaCl )) gives a solution that is

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

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

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

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

49. The Arrhenius concept is limited to

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