أسئلة اختيار من متعدد باللغة الإنجليزية للوحدة السادسة عشر Acid–Base Equilibria, Chapter 16 من كتاب CHEMISTRY THE CENTRAL SCIENCE

أسئلة اختيار من متعدد باللغة الإنجليزية للوحدة السادسة عشر Acid–Base Equilibria من كتاب CHEMISTRY THE CENTRAL SCIENCE

هذه الأسئلة أيضا تغطي :

• الوحدة السادسة عشر : Acid-Base Equilibria and Solubility Equilibria من كتاب  Chemistry  13^th edition by: Raymond Chang and Jason Overby
• الوحدة الخامسة عشر : Acid–Base Equilibria من كتاب Chemistry 9^th edition by: Zumdhal

(باللون الأحمر هي الإجابة الصحيحة)

1. The concentration of water in pure water is approximately:
A) 18 M

B) 100 M

C) 55 M

D) 0.100 M

E) 83 M

2. In basic solution
A) [H₃O⁺] = [OH^–]

B) [H₃O⁺] > [OH]

C) [H₃O⁺] < [OH^–]

D) [H₃O⁺] = 0 M

3. What is the concentration of hydronium ions in a solution with a hydroxide ion concentration of 2.31 x 10^-4 M ?
A) 4.33 x 10^-11 M

B) 2.31 x 10¹⁰ M

C) 9.72 x 10^-4 M

D) 1.01 x 10^-5 M

4. What is the pH of an aqueous solution at 25 °C in which [H⁺] is 0.0025 M?
A) +3.40

B) +2.60

C) -2.60

D) -3.40

E) +2.25

5. What is the pH of an aqueous solution at 25 °C in which [OH^–] is 0.0025 M?
A) +2.60

B) -2.60

C) +11.40

D) -11.40

E) -2.25

6. What is the pH of a solution that contains 3.98 x 10^-9 M hydronium ion?
A) 8.400

B) 5.600

C) 9.000

D) 3.980

E) 7.000

7. What is the pH of a solution that contains 3.98 x 10^-9 M hydroxide ion?
A) 8.400

B) 5.600

C) 9.000

D) 3.980

E) 7.000

8. What is the concentration of hydronium ions in a solution with pH = 4.282?
A) 4.282 M

B) 9.718 M

C) 1.92 x 10-10 M

D) 5.22 x 10-5 M

E) 1.66 x 104 M

9. What is the concentration of hydroxide ions in a solution with pH = 4.282?
A) 4.282 M

B) 9.718 M

C) 1.92 x 10-10 M

D) 5.22 x 10-5 M

E) 1.66 x 104 M

10. Calculate the pOH of a solution that contains 1.94 x 10^-10 M hydronium ions.
A) 1.940

B) 4.288

C) 7.000

D) 14.000

E) 9.712

11. Calculate the concentration of hydronium ions in a solution with a pOH of 4.223.
A) 5.98 x 10^-5 M

B) 1.67 x 10^-10 M

C) 1.67 x 10⁴ M

D) 5.99 x 10^-19 M

E) 1.00 x 10^-7 M

12. In basic solution at 25 °C, pH is ____ and pOH is ____.
A) = 7, = 7

B) >7, <7

C) <7, >7

13. Which solution below has the highest concentration of hydroxide ions?
A) pH = 3.21

B) pH = 12.59

C) pH = 7.93

D) pH = 9.82

14. Of the following, which is a weak acid?
A) HF

B) HCl

C) HI

D) HBr

E) HNO₃

F) HClO₄

15. According to Arrhenius, an acid is a substance that
A) is capable of donating one or more H⁺

B) causes an increase in the concentration of H⁺ in aqueous solutions

C) can accept a pair of electrons to form a coordinate covalent bond

D) reacts with the solvent to form the cation formed by autoionization of that solvent

16. Which one of the following would be considered a base according to the Bronsted-Lowry definition but not by the Arrhenius definition?
A) NH₃(g)

B) HBr(aq)

C) Ba(OH)₂(aq)

D) HF(g)

E) KOH(aq)

17. Which one of the following is a Bronsted-Lowry acid?
A) (CH₃)₃NH⁺

B) CH₄COOH

C) HF

D) HNO₂

E) all of these

18. In the following reaction, which substance is acting as a base? HN₃ + H₂O → H₃O⁺ + N^₃–
A) H₂O

B) HN₃

19. A Bronsted-Lowry base is defined as a substance which
A) increases [H⁺] when placed in H₂O

B) decreases [H⁺] when placed in H₂O

C) increases [OH^–] when placed in H₂O

D) acts as a proton acceptor in any system

E) acts as a proton donor in any system

20. A Bronsted-Lowry acid is defined as a substance that
A) increases [H⁺] when placed in H₂O

B) decreases [H⁺] when placed in H₂O

C) increases [OH^–] when placed in H₂O

D) acts as a proton acceptor in any system

E) acts as a proton donor in any system

21. A substance that is capable of acting as both acid and as base is called
A) autosomal

B) conjugated

C) amphoteric

D) autocratic

22. What is the conjugate acid of NH₃?
A) NH₃

B) NH₂⁺

C) NH₃⁺

D) NH₄⁺

23. What is the conjugate base of OH^–?
A) O₂

B) O^–

C) H₂O

D) O₂^–

24. The [OH^–] and pH of 0.035 M KOH at 25 °C are respectively
A) 0.035 M and +1.46

B) 0.035 M and -1.46

C) 2.9 x 10-13 M and -12.54

D) 0.035 M and +12.54

E) 2.9 x 10-13 M and +12.54

25. The [OH^–] and pH of 0.0012 M Ba(OH)₂ at 25 °C are respectively
A) 0.00060 M and -2.62

B) 0.0012 M and +2.92

C) 0.0024 M and +11.38

D) 0.0024 M and +2.62

E) 0.0012 M and -2.9226.

26. Calculate the [OH^–] in a NaOH solution with a pH of 12.73.
A) 1.27

B) 1.9 x 10^-13

C) 0.054

D) 2.3 x 10^-12

27. Which of the following possesses the greatest concentration of hydroxide ion?
A) a solution with a pH of 3.0

B) a 1 X 10^-4 M solution of HNO₃

C) a solution with a pOH of 12.0

D) water

28. Which of the following acids is not a strong acid?
A) H₂CO₃

B) H₂SO₄

C) HNO₃

D) HClO₄

29. Which one of the following is the weakest acid?
A) HF (Ka = 6.8 x 10^-4)

B) HClO (Ka = 3.0 x 10^-8)

C) HNO₂ (Ka = 4.5 x 10^-4)

D) HCN (Ka = 4.9 x 10^-10)

30. HZ is a weak acid. An aqueous solution nominally 0.020 M in HZ has a pH of 4.93 at 25 °C. What is K_a for HZ?
A) 1.2 x 10^-5

B) 6.9 x 10^-9

C) 1.4 x 10^-10

D) 9.9 x 10-2

E) 2.8 x 10^-12

31. Acid K_a HOAc 1.8 X 10^-5,  HCHO₂ 1.8 X 10^-4,  HClO 3.0 X 10^-8,  HF 6.8 X 10^-4 Which one of the acids shown in the table is the strongest?
A) HOAc

B) HCHO₂

C) HClO

D) HF

32. What is the % ionization of hypochlorous acid (HClO) in a 0.015 M solution of HClO? (K_a = 3.0 x 10^-8)
A) 4.5 x 10^-8

B) 14

C) 2.1 x 10^-5

D) 0.14

33. The pH of a 0.55 M solution of HBrO is 4.48. What is the value of K_a for HBrO?
A) 2.0 x 10^-9

B) 1.1 x 10^-9

C) 6.0 x 10^-5

D) 3.3 x 10^-5

34. K_a for HClO is 3.0 x 10^-8. What is the pH at 25 °C of an aqueous solution that is 0.020 M in HClO?
A) +2.45

B) -2.45

C) -9.22

D) +9.22

E) +4.61

35. K_b for HN₃ is 1.9 X 10^-5. What is the pH of a 0.35 M solution of HN₃?
A) 11.41

B) 2.37

C) 5.18

D) 2.59

36. Of the following, which is the weakest acid?
A) H₃PO₄

B) H₂PO₄^–

C) HPO₄^2-

37. Calculate the pH of a solution of 0.163 M sulfurous acid, H₂SO₃, K_a1 = 1.7 x 10^-2, K_a2 = 6.4 x 10^-8.
A) 4.48

B) 1.35

C) 1.77

D) 7.19

38. Calculate the pOH of 0.0827 M sodium cyanide solution, NaCN, (for cyanide ion, K_b = 4.9 x 10-¹⁰.
A) 9.31

B) 10.39

C) 5.20

D) 1.08

39. Which one of the following is not a weak base?
A) (CH₃)₃N

B) NaOCl

C) NaF

D) NaClO₄

40. Calculate the pH of a solution made by dissolving 1.87 g of sodium caproate, NaC₆H₁₁O₂, K_b = 7.58 x 10^-10, in water and diluting to a total volume of 500.0 mL.
A) 5.344

B) 8.656

C) 5.494

D) 8.505

41. Determine the pH of a 0.15 M solution of KF (K_a = 7.0 x 10^-4).
A) 12.01

B) 5.83

C) 8.17

D) 2.33

42. Calculate the pH of a 0.50 M solution of NH3. The K_b of NH₃ is 1.8 x 10^-5.
A) 8.95

B) 11.48

C) 2.52

D) 5.05

43. Determine the pH of a 0.35 M solution of CH₃NH₂ (methylamine). The K_b of methylamine is 4.4 x 10^-4.
A) 10.19

B) 3.81

C) 12.09

D) 1.91

44. Given that the K_a for gallic acid, HC₇H₅O₅, is 4.57 x 10^-3, what is the K_b for sodium gallate, NaC₇H₅O₅?
A) 4.57 x 10^-3

B) 2.19 x 10^-12

C) 5.43 x 10^-5

D) 7.81 x 10^-6

45. K_b for NH₃ is 1.8 x 10^-5. What is the pH of a 0.35 M solution of NH₄Cl?
A) 9.71

B) 4.29

C) 9.14

D) 4.86

46. The K_a for formic acid (HCHO₂) is 1.8 x 10^-4. What is the pH of a 0.35 M solution of sodium formate (NaCHO₂)?
A) 10.71

B) 5.36

C) 3.29

D) 8.64

47. The K_a for HCN is 4.9 x 10^-10. What is the value of K_b for CN-?
A) 2.0 x 10^-5

B) 4.0 x 10^-6

C) 4.9 x 10⁴

D) 4.9 x 10^-24

48. A 0.10 M aqueous solution of which of the following salts will have the lowest pH?
A) KNO₃

B) Ca(NO₃)₂

C) Ni(NO₃)₂

D) KCl

E) BaBr₂

49. Of the following four substances, which would form basic solutions? NH₄Cl, Cu(NO₃)₂, K₂CO₃, NaF
A) NH₄Cl, Cu(NO₃)₂

B) K₂CO₃, NH₄Cl

C) NaF only

D) NaF, K₂CO₃

50. Which one of the following 0.1 M solutions would have a pH of 7.0?
A) NaOCl

B) KCl

C) NH₄Cl

D) Ca(OAc)₂

E) none of these

51. Which definition of acids and bases is the most general?
A) Bronsted-Lowry

B) Arrhenius

C) Lewis

52. Which one of the following cannot act as a Lewis base?
A) Cl^–

B) NH₃

C) Cr³⁺

D) CN^–

53. In the reaction BF₃ + F^– → BF₄^–, BF₃ is acting as what type of acid?
A) Arrhenius only

B) Bronsted-Lowry only

C) Lewis only

D) Arrhenius, Bronsted-Lowry, and Lewis

E) Arrhenius and Bronsted-Lowry

54. Which equation does NOT represent a Lewis acid-base reaction?
A) Cu²⁺(aq) + 4NH₃(aq) → [Cu(NH₃)₄]²⁺(aq)

B) HCl(g) + NH₃(g) → NH₄Cl(s)

C) H⁺(aq) + OH^–(aq) → H₂O(l)

D) 2Na(s) + Cl₂ (g) → 2NaCl(s)

55. Identify the Lewis base in the following equation: Cu²⁺(aq) + 4CN^–(aq) → Cu(CN)₄^2-(aq)
A) CN^–

B) Cu²⁺

C) Cu(CN)₄^2-

56. In the reaction NH₃ + H⁺ → NH₄⁺, the NH₃ is acting as a(n) _________ base but not as a(n) _________ base. :

A) Arrhenius, Bronsted-Lowry

B) Bronsted-Lowry, Lewis

C) Lewis, Arrhenius

D) Lewis, Bronsted-Lowry

57. calculate the K_a for an unknown monoprotic acid HX, given that a solution of 0.10 M LiX has a pH of 8.90.
A) 7.9 x 10^-6

B) 4.3 x 10^-8

C) 6.2 x 10^-10

D) 2.6 x 10^-10

E) 1.6 x 10^-5

 

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