الرئيسية » الكيمياء العامة المبسطة » أسئلة اختيار من متعدد باللغة الإنجليزية للوحدة السادسة عشر Acid–Base Equilibria من كتاب CHEMISTRY THE CENTRAL SCIENCE

أسئلة اختيار من متعدد باللغة الإنجليزية للوحدة السادسة عشر Acid–Base Equilibria 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 :

(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+ + N3
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 Ka 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 Ka 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? (Ka = 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 Ka 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. Ka 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. Kb 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) HPO42-

37. Calculate the pH of a solution of 0.163 M sulfurous acid, H2SO3, Ka1 = 1.7 x 10-2, Ka2 = 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, Kb = 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, Kb = 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 (Ka = 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 Kb 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 Kb of methylamine is 4.4 x 10-4.
A) 10.19

B) 3.81

C) 12.09

D) 1.91

44. Given that the Ka for gallic acid, HC7H5O5, is 4.57 x 10-3, what is the Kb 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. Kb 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 Ka 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 Ka for HCN is 4.9 x 10-10. What is the value of Kb 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)42-(aq)
A) CN

B) Cu2+

C) Cu(CN)42-

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 Ka 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

مقالات قد تفيدك :

عن Akram Amir El Ali

استاذ الكيمياء التحليلية ومصمم غرافيك

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