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

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

3. The value of depends upon

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

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

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

7. In a sealed vessel containing at fixed (T), the brown colour intensity becomes constant after some time. Which test shows molecular turnover persists?

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

9. For , the correct expression is:

10. The ionization equation for acetic acid is

11. The equilibrium is homogeneous because

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

13. The (pH) of a (0.05,M) solution is

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

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

16. The common ion effect refers to

17. If the hydrogen ion concentration of a solution is , its pH is

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

19. In a gaseous equilibrium, decreasing the concentration of reactants will cause

20. The equilibrium constant for the reaction in terms of partial pressures is:

21. The unit of for the reaction is

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

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

24. The solubility of a salt in terms of is given by

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

26. Which observation best demonstrates that equilibrium is dynamic rather than static in a saturated solution of sugar at constant (T)?

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

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

29. For an endothermic reaction, increasing temperature shifts equilibrium

30. In , a tiny pulse of is injected into an equilibrated, sealed vessel. Which observation confirms dynamic equilibrium after relaxation?

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

2. For , if initial concentrations of all species are and , the equilibrium will be

3. The (pH) of a (0.01,M) (NaOH) solution is

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

5. A weak acid is characterized by

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

7. The blood buffer system primarily consists of

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

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

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

11. The pH of a basic buffer is given by

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

13. In the reaction , if and , the reaction will

14. The Henderson–Hasselbalch equation is derived from

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

16. Ostwald’s dilution law is not applicable to

17. In the equilibrium , increasing total pressure shifts equilibrium

18. The importance of the solubility product lies in its use for

19. For at , , and rate constants , . Which calculation indicates dynamic equilibrium?

20. If the ionic product (Q) is less than , the solution is

21. The smaller the value of , the

22. For the reaction , the units of are

23. According to Lewis acidity/basicity trends, which order of acid strength is most reasonable toward a hard donor like ?

24. The reaction conditions in the Haber process are typically

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

26. The pH of a solution of sodium acetate is

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

28. For , the correct expression is

29. The reaction has at 500 K. If initially is high and are low, the reaction will

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

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

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

33. For , lowering temperature generally leads to

34. The expression for the acid dissociation constant of is

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

36. For the equilibrium , increasing pressure will

37. The principle of microscopic reversibility implies that:

38. When equilibrium is attained in a reversible reaction:

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

40. If , the reaction will proceed

41. For the reaction , the value of is

42. The pH of a (0.001,M) (NaOH) solution is

43. According to Arrhenius theory, neutralization occurs when

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

45. For , with and initial , equilibrium is

46. The unit of for the reaction is

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

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

49. In , a tiny pulse of is injected into an equilibrated, sealed vessel. Which observation confirms dynamic equilibrium after relaxation?

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