JEE Main - Ionic equilibrium acids bases pH common ion effect hydrolysis and buffers Online Test (MCQ Quiz)

1. Which of the following is a characteristic of a strong acid?

A) It partially dissociates in water. B) It has a high pH value. C) It completely dissociates in water. D) It forms a stable conjugate base.

2. What is the pH of a 0.01 M solution of HCl?

A) 1 B) 2 C) 7 D) 13

3. According to the Brønsted-Lowry theory, a base is a substance that:

A) Accepts a proton B) Donates a proton C) Accepts an electron pair D) Donates an electron pair

4. The conjugate acid of NH3 is:

A) NH2- B) NH4+ C) OH- D) NH2OH

5. Which of the following is an amphoteric substance?

A) HCl B) NaOH C) H2O D) NaCl

6. The common ion effect describes the decrease in the solubility of a sparingly soluble salt when:

A) A common ion is added to the solution. B) The temperature of the solution is increased. C) The volume of the solvent is decreased. D) An acid is added to the solution.

7. Hydrolysis of a salt of a strong acid and weak base results in a solution that is:

A) Acidic B) Basic C) Neutral D) Amphoteric

8. A buffer solution resists changes in pH upon addition of small amounts of:

A) Strong acid or strong base B) Weak acid or weak base C) Salt of strong acid and strong base D) Water

9. The Henderson-Hasselbalch equation for an acidic buffer is:

A) pH = pKa + log([conjugate base]/[acid]) B) pOH = pKb + log([conjugate acid]/[base]) C) pH = pKw + log([acid]/[conjugate base]) D) pOH = pKa + log([acid]/[base])

10. Which of the following is a Lewis acid?

A) NH3 B) H2O C) BF3 D) OH-

11. The pH of pure water at 25°C is:

A) 0 B) 7 C) 14 D) 1

12. What is the pOH of a 0.001 M solution of NaOH?

A) 1 B) 2 C) 11 D) 13

13. The dissociation constant of a weak acid (Ka) is a measure of its:

A) Strength B) Concentration C) Solubility D) pH

14. For a weak base, a higher Kb value indicates:

A) Weaker base B) Stronger base C) Neutral character D) Amphoteric nature

15. The salt of a weak acid and strong base, when dissolved in water, undergoes:

A) Cationic hydrolysis B) Anionic hydrolysis C) Neutralization D) Dissociation only

16. Which of the following mixtures can act as a buffer solution?

A) CH3COOH and CH3COONa B) HCl and NaCl C) NaOH and NaCl D) H2SO4 and Na2SO4

17. The buffer capacity of a buffer solution is highest when:

A) pH = pKa B) pH > pKa C) pH < pKa D) pH = 7

18. In the autoionization of water, the equilibrium constant Kw is equal to:

A) [H+][OH-] B) [H+]/[OH-] C) [OH-]/[H+] D) [H+] + [OH-]

19. A solution with a pH of 3 is considered:

A) Acidic B) Basic C) Neutral D) Strongly basic

20. The conjugate base of H2SO4 is:

A) HSO3- B) SO42- C) HSO4- D) H3O+

21. Which factor affects the pH of a buffer solution the most?

A) Dilution B) Addition of a strong acid C) Addition of a strong base D) Addition of a salt of strong acid and strong base

22. The degree of dissociation of a weak electrolyte increases with:

A) Increase in concentration B) Decrease in concentration C) Addition of a common ion D) Addition of a strong acid

23. For a sparingly soluble salt like AgCl, the common ion effect leads to:

A) Increased solubility B) Decreased solubility C) No change in solubility D) Increased dissociation

24. Hydrolysis of a salt of a weak acid and weak base results in a solution that is:

A) Acidic B) Basic C) Neutral D) Depends on the relative strengths of the acid and base

25. Which of the following is NOT a component of an acidic buffer solution?

A) A weak acid B) Its conjugate base C) A strong acid D) A salt of the weak acid and strong base

26. The solubility product (Ksp) of a sparingly soluble salt is the product of the concentrations of its ions, each raised to the power of its stoichiometric coefficient in the equilibrium equation. For CaF2, Ksp = [Ca2+][F-]^2. If [Ca2+] = x and [F-] = y, then Ksp is:

A) xy B) x2y C) xy2 D) x2y2

27. What is the relationship between pH and pOH at 25°C?

A) pH + pOH = 14 B) pH - pOH = 14 C) pH * pOH = 14 D) pH / pOH = 14

28. A substance that can act as both an acid and a base is called:

A) Amphipathic B) Amphoteric C) Anhydrous D) Azeotrope

29. The pH of a 0.1 M solution of acetic acid (Ka = 1.8 x 10^-5) is approximately:

A) 2.87 B) 3.42 C) 4.15 D) 5.00

30. Which of the following species is NOT a Brønsted-Lowry acid?

A) H3O+ B) CH3COOH C) NH4+ D) Cl-

31. The hydrolysis of the salt of a strong acid and a strong base results in a solution that is:

A) Acidic B) Basic C) Neutral D) Highly alkaline

32. A buffer solution is prepared by mixing a weak acid with:

A) Its conjugate base B) Its conjugate acid C) A strong base D) A strong acid

33. The Ostwald's dilution law is applicable to:

A) Strong electrolytes B) Weak electrolytes C) Non-electrolytes D) All electrolytes

34. If the solubility of a sparingly soluble salt M(OH)2 is 's', then its solubility product (Ksp) is:

A) 4s3 B) 27s4 C) s D) s2

35. Which of the following is a Lewis base?

A) BF3 B) AlCl3 C) CO2 D) NH3

36. The pH of a 0.01 M solution of a monoprotic strong acid is:

A) 1 B) 2 C) 3 D) 13

37. The pKa of a weak acid is 5. What is the Ka?

A) 5 x 10^-5 B) 10^-5 C) 10^5 D) 5 x 10^5

38. Which type of hydrolysis occurs when a salt of a weak acid and strong base is dissolved in water?

A) Cationic hydrolysis B) Anionic hydrolysis C) Neutral hydrolysis D) No hydrolysis

39. The buffer range of a buffer solution is typically:

A) pKa ± 1 B) pKa ± 2 C) pKa ± 0.5 D) pKa ± 0.1

40. The common ion effect is an application of:

A) Le Chatelier's principle B) Hess's law C) First law of thermodynamics D) Law of conservation of mass

41. For a polyprotic acid, the first dissociation constant (Ka1) is generally:

A) Greater than Ka2 B) Less than Ka2 C) Equal to Ka2 D) Zero

42. Which of the following statements is true for a neutral solution at 25°C?

A) [H+] > [OH-] B) [H+] < [OH-] C) [H+] = [OH-] D) pH = 0

43. The pH of a 0.0001 M solution of NaOH is:

A) 1 B) 4 C) 10 D) 13

44. The conjugate base of H2O is:

A) H3O+ B) OH- C) O2- D) H2O2

45. Which of the following will decrease the pH of a solution?

A) Adding NaOH B) Adding HCl C) Adding NaCl D) Adding water

46. If the solubility of AgCl is 's', then its Ksp is:

A) s B) 2s C) s^2 D) 4s

47. A buffer solution is made from a weak base and its conjugate acid. The Henderson-Hasselbalch equation for this buffer is:

A) pOH = pKb + log([conjugate acid]/[base]) B) pH = pKa + log([base]/[conjugate acid]) C) pOH = pKa + log([conjugate base]/[acid]) D) pH = pKb + log([conjugate base]/[base])

48. The ionization of a weak acid is favored by:

A) Low concentration B) High concentration C) Addition of common ion D) Addition of strong base

49. Which of the following is the most acidic?

A) pH = 7 B) pH = 5 C) pH = 2 D) pH = 9

50. When a salt of a weak acid and strong base dissolves in water, the pH of the solution will be:

A) < 7 B) = 7 C) > 7 D) Depends on concentration

Ionic equilibrium acids bases pH common ion effect hydrolysis and buffers - Online Test

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