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

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

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

4. Which of the following is NOT implied by the definition of chemical equilibrium?

5. Applying pressure to ice near causes it to melt more easily because:

6. Which interaction most clearly illustrates Lewis acidity of a metal cation in solution?

7. Which kinetic observation most directly evidences dynamic equilibrium in a reversible reaction mixture?

8. When temperature increases, the numerical value of relative to :

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

10. The conjugate acid of the base is

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

12. Consider in a closed vessel. The equilibrium constant depends on

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

14. In the reaction , the conjugate base of is

15. Removing a product from a reversible reaction mixture will

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

17. The common ion effect refers to

18. The equilibrium constant for a gaseous reaction increases with temperature if the reaction is:

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

20. For a weak base solution where , the hydroxide ion concentration is

21. 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

22. For a weak base ( BOH ), Ostwald’s dilution law is expressed as

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

24. The variation of the degree of ionization with concentration (( C )) for a weak electrolyte is represented by

25. For an endothermic reaction, decreasing temperature causes

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

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

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

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

30. A catalyst affects equilibrium by

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

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

3. When a solution is just saturated with a salt, the ionic product is

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

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

6. The Arrhenius concept is limited to

7. Which of the following represents a homogeneous equilibrium?

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

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

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

11. The pH of a basic buffer is given by

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

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

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

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

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

17. Which of the following statements is true about ?

18. Which of the following salts gives an acidic solution in water?

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

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

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

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

23. The blood buffer system primarily consists of

24. The reaction quotient for is given by

25. Ostwald’s dilution law fails for strong electrolytes because

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

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

28. The value of depends upon

29. The pOH of a solution is defined as

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

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

32. The (pH) of (0.1,M) increases when the solution is diluted because

33. For with starting from , , the approximate equilibrium is

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

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

36. Which of the following graphs best represents Ostwald’s dilution law?

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

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

39. In at equilibrium, , , and . What value provides evidence of dynamic equilibrium through rate equality?

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

41. According to Le Chatelier’s principle, if the concentration of a reactant is increased, the system will

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

43. The Henderson–Hasselbalch equation is derived from

44. The conjugate acid of a strong base is

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

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

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

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

49. The strength of an acid is determined by the magnitude of its

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