Chemistry 11th Edition By Raymond Chang – Test Bank

 

 

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Sample Questions 

 

Chapter 4: Reactions in Aqueous Solutions

 

1.    Which of the following compounds is a strong electrolyte?

2.    A) H₂O    B)  CH₃OH    C)  CH₃CH₂OH    D)  HF    E)  NaF

Ans:  E     Category:  Easy     Section:  4.1

 

2.    Which of the following compounds is a weak electrolyte?

3.    A) HNO₃    B)  NaNO₃    C)  HNO₂    D)  NaNO₂    E)  NaOH

Ans:  C     Category:  Easy     Section:  4.1

 

3.    Which of the following compounds is a strong electrolyte?

4.    A) H₂O                                                       D)      CH₃CH₂OH (ethanol)

5.    B) N₂                                                          E)      KOH

6.    C) CH₃COOH (acetic acid)

Ans:  E     Category:  Easy     Section:  4.1

 

4.    Which of the following compounds is a weak electrolyte?

5.    A) HCl                                                        D)      O₂

6.    B) CH₃COOH (acetic acid)                       E)      NaCl

7.    C) C₆H₁₂O₆ (glucose)

Ans:  B     Category:  Easy     Section:  4.1

 

5.    Which of the following compounds is a weak electrolyte?

6.    A) HCl    B)  NH₃    C)  C₆H₁₂O₆ (glucose)    D)  N₂    E)  KCl

Ans:  B     Category:  Easy     Section:  4.1

 

6.    Which of the following compounds is a nonelectrolyte?

7.    A) NaF                                                       D)      NaOH

8.    B) HNO₃                                                    E)      C₆H₁₂O₆ (glucose)

9.    C) CH₃COOH (acetic acid)

Ans:  E     Category:  Easy     Section:  4.1

 

7.    Which of the following compounds is a nonelectrolyte?

8.    A) NaOH                                                    D)      KF

9.    B) HNO₃                                                    E)      CH₃COOH (acetic acid)

10.  C) C₂H₆O (ethanol)

Ans:  C     Category:  Easy     Section:  4.1

 

8.    Identify the major ionic species present in an aqueous solution of Na₂CO₃.

9.    A) Na₂⁺, CO₃^2–                                           D)      Na⁺, C⁺, O^2–

10.  B) Na₂⁺, C^{2 –}, O₃                                         E)      Na⁺, CO₃^2–

11.  C) Na⁺, C⁴⁺, O₃^2–

Ans:  E     Category:  Easy     Section:  4.1

 

9.    Identify the major ionic species present in an aqueous solution of K₂SO₄.

10.  A) K²⁺, S⁶⁺, O₄^8–                                         D)      2K⁺, S⁶⁺, 4O^2–

11.  B) K²⁺, S⁶⁺, 4O^2–                                        E)      2K⁺, SO₄^2–

12.  C) 2K⁺, S⁶⁺, O₄^8–

Ans:  E     Category:  Easy     Section:  4.1

 

10.  Identify the major ionic species present in an aqueous solution of NH₄ClO₄.

11.  A) NH₄⁺, Cl^–, 4O^2-                                      D)      NH₄⁺, ClO₄^–

12.  B) N^3-, 4H⁺, Cl^–, 4O^2-                                 E)      NH₄Cl⁺, O₄^–

13.  C) 4NH⁺, 4ClO^–

Ans:  D     Category:  Easy     Section:  4.1

 

11.  Identify the major ionic species present in an aqueous solution of C₆H₁₂O₆ (glucose).

12.  A) 6 C^–, 12 H⁺, 6 O^–                                    D)      C₆⁺, 12 H⁺, 6 O^2-

13.  B) 6 C⁺, 12 H⁺, 6 O^2-                                  E)      no ions are present

14.  C) 6 CH²⁺, 6 O^2-

Ans:  E     Category:  Easy     Section:  4.1

 

12.  Identify the major ionic species present in an aqueous solution of FeCl₃.

13.  A) Fe⁺, Cl₃^–    B)  Fe³⁺, Cl₃^3-    C)  Fe³⁺, 3 Cl^–    D)  Fe²⁺, 3 Cl^–    E)  Fe⁺, 3 Cl^–

Ans:  C     Category:  Easy     Section:  4.1

 

13.  Identify the major ionic species present in an aqueous solution of C₁₂H₂₂O₁₁ (sucrose).

14.  A) 12 C^–, 22 H⁺, 11 O^–                                D)      C₁₂⁺, 22 H⁺, 11 O^2-

15.  B) 12 C⁺, 22 H⁺, 11 O^2-                              E)      no ions are present

16.  C) 12 CH²⁺, 11 O^2-

Ans:  E     Category:  Easy     Section:  4.1

 

14.  The distinguishing characteristic of all electrolyte solutions is that they

15.  A) contain molecules.                                 D)      always contain acids.

16.  B) conduct electricity.                                E)      conduct heat.

17.  C) react with other solutions.

Ans:  B     Category:  Easy     Section:  4.1

 

15.  Based on the solubility rules, which one of the following compounds should be insoluble in water?

16.  A) NaCl    B)  MgBr₂    C)  FeCl₂    D)  AgBr    E)  ZnCl₂

Ans:  D     Category:  Easy     Section:  4.2

 

16.  Based on the solubility rules, which of the following compounds should be insoluble in water?

17.  A) Na₂SO₄    B)  BaSO₄    C)  CuSO₄    D)  MgSO₄    E)  Rb₂SO₄

Ans:  B     Category:  Easy     Section:  4.2

 

17.  Based on the solubility rules, which of the following compounds should be insoluble in water?

18.  A) CaCO₃    B)  (NH₄)₂CO₃    C)  Na₂CO₃    D)  K₂CO₃    E)  KNO₃

Ans:  A     Category:  Easy     Section:  4.2

 

18.  Based on the solubility rules, which of the following should be soluble in water?

19.  A) Hg₂Cl₂    B)  Na₂S    C)  Ag₂CO₃    D)  Ag₂S    E)  BaSO₄

Ans:  B     Category:  Easy     Section:  4.2

 

19.  Based on the solubility rules, which of the following should be soluble in water?

20.  A) AgBr    B)  AgCl    C)  Ag₂CO₃    D)  AgNO₃    E)  Ag₂S

Ans:  D     Category:  Easy     Section:  4.2

 

20.  Based on the solubility rules, which of the following should be soluble in water?

21.  A) (NH₄)₃PO₄    B)  Ca₃(PO₄)₂    C)  AlPO₄    D)  Ag₃PO₄    E)  Mg₃(PO₄)₂

Ans:  A     Category:  Easy     Section:  4.2

 

21.  Based on the solubility rules, which of the following should be soluble in water?

22.  A) CaSO₄    B)  BaSO₄    C)  PbSO₄    D)  K₂SO₄    E)  AgCl

Ans:  D     Category:  Easy     Section:  4.2

 

22.  Which of the following will occur when a solution of Pb(NO₃)₂(aq) is mixed with a solution of KI(aq) ?

23.  A) A precipitate of KNO₃ will form; Pb²⁺ and I^– are spectator ions.

24.  B) No precipitate will form.

25.  C) A precipitate of Pb(NO₃)₂ will form; K⁺ and I^– are spectator ions.

26.  D) A precipitate of PbI₂ will form; K⁺ and NO₃^– are spectator ions.

27.  E) A precipitate of PbI₂ will form; Pb²⁺ and I^– are spectator ions.

Ans:  D     Category:  Medium     Section:  4.2

 

23.  Which of the following will occur when solutions of CuSO₄(aq) and BaCl₂(aq) are mixed?

24.  A) A precipitate of CuCl₂ will form; Ba²⁺ and SO₄^2– are spectator ions.

25.  B) A precipitate of CuSO₄ will form; Ba²⁺ and Cl^– are spectator ions.

26.  C) A precipitate of BaSO₄ will form; Cu²⁺ and Cl^– are spectator ions.

27.  D) A precipitate of BaCl₂ will form; Cu²⁺ and SO₄^2– are spectator ions.

28.  E) No precipitate will form.

Ans:  C     Category:  Medium     Section:  4.2

 

24.  Which of the following will occur when solutions of ZnSO₄(aq) and MgCl₂(aq) are mixed?

25.  A) A precipitate of ZnCl₂ will form; Mg²⁺ and SO₄^2– will be spectator ions.

26.  B) A precipitate of ZnSO₄ will form ; Mg²⁺ and Cl^– will be spectator ions.

27.  C) A precipitate of MgSO₄ will form ; Zn²⁺ and Cl^– will be spectator ions.

28.  D) A precipitate of MgCl₂ will form ; Zn²⁺ and SO₄^2– will be spectator ions.

29.  E) No precipitate will form.

Ans:  E     Category:  Medium     Section:  4.2

 

25.  Identify the precipitate(s) formed when solutions of Na₂SO₄(aq), Ba(NO₃)₂(aq), and NH₄ClO₄(aq) are mixed.

26.  A) Ba(ClO₄)₂                                              D)      BaSO₄

27.  B) BaSO₄ and (NH₄)₂SO₄                          E)      NaClO₄

28.  C) NH₄NO₃ and NaClO₄

Ans:  D     Category:  Medium     Section:  4.2

 

26.  Identify the precipitate(s) formed when solutions of NH₄Cl(aq), AgClO₃(aq), and NaCl(aq) are mixed.

27.  A) AgCl                                                      D)      NH₄ClO₃

28.  B) AgCl and NH₄ClO₃                              E)      AgNH₄

29.  C) NH₄Cl and NaClO₃

Ans:  A     Category:  Medium     Section:  4.2

 

27.  Identify the precipitate(s) formed when solutions of Ca(ClO₄)₂(aq), K₂CO₃(aq), and NaNO₃(aq) are mixed.

28.  A) CaCO₃                                                   D)      CaCO₃ and Na₂CO₃

29.  B) Na₂CO₃                                                 E)      KClO₄ and Ca(NO₃)₂

30.  C) Ca(NO₃)₂ and NaClO₄

Ans:  A     Category:  Medium     Section:  4.2

 

28.  Identify the precipitate(s) formed when solutions of Pb(NO₃)₂(aq), Mg(ClO₄)₂(aq), and (NH₄)₂SO₄(aq) are mixed.

29.  A) PbSO₄                                                    D)      NH₄NO₃ and NH₄ClO₄

30.  B) MgSO₄                                                  E)      PbSO₄ and MgSO₄

31.  C) NH₄ClO₄

Ans:  A     Category:  Medium     Section:  4.2

 

29.  Identify  the correct net ionic equation for the reaction that occurs when solutions of Pb(NO₃)₂ and NH₄Cl are mixed.

30.  A) Pb(NO₃)₂(aq) + 2NH₄Cl(aq) ® NH₄NO₃(aq) + PbCl₂(s)

31.  B) Pb²⁺(aq) + 2Cl^–(aq) ® PbCl₂(s)

32.  C) Pb²⁺(aq) + 2NO₃^– (aq) + 2NH(aq) + 2Cl^–(aq) ® 2NH(aq) + 2NO₃^– (aq) + PbCl₂(s)

33.  D) NH₄⁺(aq)+ NO₃^– (aq) ® 2NH₄NO₃(s)

34.  E) No reaction occurs when the solutions are mixed.

Ans:  B     Category:  Medium     Section:  4.2

 

30.  Identify the correct net ionic equation for the reaction that occurs when solutions of AgNO₃ and NH₄Cl are mixed.

31.  A) AgNO₃(aq) + NH₄Cl(aq) ® AgCl(s) + NH₄Cl(aq)

32.  B) NH₄⁺(aq) + NO₃^–(aq) ® NH₄NO₃(s)

33.  C) AgNO₃(aq) + NH₄Cl(aq) ® AgCl(s) + NH₄Cl(s)

34.  D) Ag⁺(aq)  +  Cl^–(aq)  ®  AgCl(s)

35.  E) AgNO₃(aq) + NH₄⁺(aq) ® NH₄AgNO₃(s)

Ans:  D     Category:  Medium     Section:  4.2

 

31.  Identify the correct net ionic equation for the reaction that occurs when solutions of Ba(ClO₄)₂ and K₂SO₄ are mixed.

32.  A) Ba²⁺(aq) + SO₄^2-(aq) ® BaSO₄(s)

33.  B) 2K⁺(aq) + 2ClO₄^–(aq) ® K₂(ClO₄)₂(s)

34.  C) K⁺(aq) + ClO₄^–(aq) ® KClO₄(s)

35.  D) Ba(ClO₄)₂(aq) + K₂SO₄(aq) ® BaSO₄(s) + 2KClO₄(s)

36.  E) Ba²⁺(aq) + K⁺(aq)  + SO₄^2-(aq) ® KBaSO₄(s)

Ans:  A     Category:  Medium     Section:  4.2

 

32.  Identify the correct net ionic equation for the reaction that occurs when solutions of Na₃PO₄ and Ca(NO₃)₂ are mixed

33.  A) Ca²⁺ + PO₄^2-(aq) ® CaPO₄(s)

34.  B) 3Ca²⁺(aq) + 2PO₄^3-(aq) ® Ca₃(PO₄)₂(s)

35.  C) Na⁺(aq) + NO₃^– ® NaNO₃(s)

36.  D) Na⁺(aq) + Ca²⁺(aq) + PO₄^3-(aq) ® NaCaPO₄(s)

37.  E) 2 Na₃PO₄(aq) + 3Ca(NO₃)₂(aq) ® 6NaNO₃(s) + Ca₃(PO₄)₂(s)

Ans:  B     Category:  Medium     Section:  4.2

 

33.  The common constituent in all acid solutions is

34.  A) H₂    B)  H⁺    C)  OH^–    D)  H₂SO₄    E)  Cl^–

Ans:  B     Category:  Easy     Section:  4.3

 

34.  Which of the following compounds is a weak acid?

35.  A) HF    B)  HCl    C)  HBr    D)  HI    E)  HClO₄

Ans:  A     Category:  Easy     Section:  4.3

 

35.  Which of the following compounds is a strong acid?

36.  A) HF    B)  HI    C)  HClO₂    D)  H₂SO₃    E)  HNO₂

Ans:  B     Category:  Easy     Section:  4.3

 

36.  Which of the following compounds is a weak base?

37.  A) KOH    B)  Sc(OH)₃    C)  NH₃    D)  NH₄⁺    E)  CO₂

Ans:  C     Category:  Easy     Section:  4.3

 

37.  Which of the following ions is a weak acid?

38.  A) SO₄^2-    B)  H₂SO₄    C)  HSO₄^–    D)  HNO₃    E)  NO₃^–

Ans:  C     Category:  Easy     Section:  4.3

 

38.  Identify the major ions present in an aqueous LiOH solution.

39.  A) Li²⁺, O^–, H^–    B)  Li⁺, OH^–    C)  LiO^–, H⁺    D)  Li⁺, O^2–, H⁺    E)  Li^–, OH⁺

Ans:  B     Category:  Easy     Section:  4.1

 

39.  Identify the major ions present in an aqueous HNO₃  solution.

40.  A) HN⁺,  O^2–    B)  OH^–, NO₃^–    C)  OH^–, NO    D)  H⁺, N^3–, O^2–    E)  H⁺, NO₃^–

Ans:  E     Category:  Easy     Section:  4.3

 

40.  Identify the major ionic species present in an aqueous solution of H₂SO₄.

41.  A) S⁶⁺, O₃^6– (plus H₂O as a neutral species)

42.  B) H⁺, OH^–, S⁶⁺, 3O^2–

43.  C) 2H⁺, S⁶⁺, 4O^2–

44.  D) H⁺, HSO₄^–

45.  E) 2H⁺, SO₄^2–

Ans:  D     Category:  Medium     Section:  4.3

 

41.  Identify the correct net ionic equation for the reaction that occurs when solutions of HNO₃ and KOH are mixed?

42.  A) HNO₃(aq) + KOH(aq) ® H₂O(l) + KNO₃(aq)

43.  B) K⁺(aq)  +  NO₃^–(aq)  ®  KNO₃(aq)

44.  C) HNO₃(aq) + KOH(aq) ®  H₂O(l) + KNO₃(s)

45.  D) H⁺(aq) + OH^–(aq) ®  H₂O(l)

46.  E) HNO₃(aq) + OH^–(aq) ® H₂O(l) + NO₃^–(aq)

Ans:  D     Category:  Medium     Section:  4.3

 

42.  Identify the correct net ionic equation for the reaction that occurs when solutions of HClO₄ and Ba(OH)₂ are mixed.

43.  A) H⁺(aq)  + 2OH^–(aq) ® H₂O(l)

44.  B) H⁺(aq) + OH^–(aq) ® H₂O(l)

45.  C) 2HClO₄(aq) + Ba(OH)₂(s) ® 2H₂O(l) + Ba(ClO₄)₂(aq)

46.  D) 2HClO₄(aq) + Ba(OH)₂(s) ® 2H₂O(l) + Ba(ClO₄)₂(s)

47.  E) 2H⁺(aq) + Ba(OH)₂(s) ® 2H₂O(l) + Ba²⁺(aq)

Ans:  B     Category:  Medium     Section:  4.2

 

43.  Identify the correct net ionic equation for the reaction that occurs when solutions of HF and KOH are mixed.

44.  A) H⁺(aq) + OH^–(aq) ® H₂O(l)

45.  B) HF(aq) + OH^–(aq) ® H₂O(l) + F^–(aq)

46.  C) H⁺(aq) + KOH(aq) ® H₂O(l) + K⁺(aq)

47.  D) HF(aq) + KOH(aq) ® H₂O(l) + KF(s)

48.  E) HF(aq) + KOH(s) ® H₂O(l) + KF(aq)

Ans:  B     Category:  Medium     Section:  4.3

 

44.  The oxidation number of N in NaNO₃ is

45.  A) +6    B)  +5    C)  +3    D)  –3    E)  None of the above.

Ans:  B     Category:  Medium     Section:  4.4

 

45.  The oxidation number of S in K₂SO₄ is

46.  A) +6    B)  +4    C)  +2    D)  –1    E)  None of the above.

Ans:  A     Category:  Medium     Section:  4.4

 

46.  The oxidation number of Mn in KMnO₄ is

47.  A) +8    B)  +7    C)  +5    D)  –7    E)  –8

Ans:  B     Category:  Medium     Section:  4.4

 

47.  The oxidation number of Fe in K₃Fe(CN)₆ is

48.  A) +3    B)  +2    C)  +1    D)  –3    E)  –4

Ans:  A     Category:  Medium     Section:  4.4

 

48.  The oxidation number of Cr in Cr₂O₇^2– is

49.  A) –12    B)  –7    C)  –2    D)  +6    E)  +7

Ans:  D     Category:  Medium     Section:  4.4

 

49.  For the chlorate ion, ClO₃^– , what are the oxidation states of the Cl and O, respectively?

50.  A) – 1, – 2    B)  +5, – 2    C)  +6, – 2    D)  +7, – 2    E)  +2, – 1

Ans:  B     Category:  Medium     Section:  4.4

 

50.  For the perchlorate ion ClO₄^– , what are the oxidation states of the Cl and O, respectively?

51.  A) – 1, – 2    B)  +8, – 2    C)  +7, – 2    D)  +6, – 2    E)  +2, – 1

Ans:  C     Category:  Medium     Section:  4.4

 

51.  The highest possible oxidation number of nitrogen is

52.  A) +8    B)  +5    C)  +3    D)  +1    E)  –3

Ans:  B     Category:  Easy     Section:  4.4

 

52.  For which one of the following acids is chlorine in the +5 oxidation state?

53.  A) HCl    B)  HClO    C)  HClO₂    D)  HClO₃    E)  HClO₄

Ans:  D     Category:  Medium     Section:  4.4

 

53.  The highest possible oxidation number of carbon is

54.  A) +8    B)  +6    C)  +4    D)  +2    E)  –4

Ans:  C     Category:  Easy     Section:  4.4

 

54.  Select the compound in which sulfur has its highest possible oxidation number.

55.  A) H₂S    B)  SO₂    C)  SCl₂    D)  H₂SO₃    E)  Na₂SO₄

Ans:  E     Category:  Medium     Section:  4.4

 

55.  The oxidation number of N in N₂H₄ is

56.  A) +4    B)  –4    C)  +2    D)  –2    E)  0

Ans:  D     Category:  Medium     Section:  4.4

 

56.  Determine the correct oxidation numbers for all three elements in Rb₂SO₃ in the order that the elements are shown in the formula.

57.  A) –2, +6, –2    B)  –1, +4, –3    C)  +2, +4, –2    D)  +1, +4, –2    E)  +1, +6, –6

Ans:  D     Category:  Medium     Section:  4.4

 

57.  Determine the correct oxidation numbers for all three elements in Ca(ClO)₂ in the order that the elements are shown in the formula?

58.  A) +2, +1, –2    B)  +2, –2, +1    C)  +2, –3, +2    D)  –2, +2, –1    E)  –2, +3, –2

Ans:  A     Category:  Medium     Section:  4.4

 

58.  Using the redox reaction below determine which element is oxidized and which is reduced.

4NH₃ + 3Ca(ClO)₂ ® 2N₂ + 6H₂O + 3CaCl₂

1.    A) H is oxidized and N is reduced            D)      Cl is oxidized and O is reduced

2.    B) N is oxidized and Cl is reduced            E)      Cl is oxidized and N is reduced

3.    C) N is oxidized and O is reduced

Ans:  B     Category:  Medium     Section:  4.4

 

59.  How many total electrons are transferred in the following reaction?

B₂H₆(g) + 3O₂(g) ® B₂O₃(s) + 3H₂O(l)

1.    A) 2    B)  3    C)  4    D)  6    E)  12

Ans:  E     Category:  Medium     Section:  4.4

 

60.  How many total electrons are transferred in the following reaction?

4 P(s) + 5O₂(g) ® 2P₂O₅(s)

1.    A) 5    B)  10    C)  15    D)  20    E)  25

Ans:  D     Category:  Medium     Section:  4.4

 

61.  How many total electrons are transferred in the following reaction?

2Na(s) + Cl₂(g) ® 2NaCl(s)

1.    A) 1    B)  2    C)  3    D)  4    E)  5

Ans:  B     Category:  Medium     Section:  4.4

 

62.  Which one of the following is a redox reaction?

63.  A) 2Al(s) + 3H₂SO₄(aq) ® Al₂(SO₄)₃(aq) + 3H₂(g)

64.  B) 2KBr(aq) + Pb(NO₃)₂(aq) ® 2KNO₃(aq) + PbBr₂(s)

65.  C) CaBr₂(aq) + H₂SO₄(aq) ® CaSO₄(s) + 2HBr(g)

66.  D) H⁺(aq) + OH^– (aq) ® H₂O(l)

67.  E) CO₃^2– (aq) + HSO₄^–(aq) ® HCO₃^– (aq) + SO₄^2– (aq)

Ans:  A     Category:  Medium     Section:  4.4

 

63.  Which of the following equations does not represent an oxidation-reduction reaction?

64.  A) 3Al + 6HCl ® 3H₂ + AlCl₃

65.  B) 2H₂O ® 2H₂ + O₂

66.  C) 2NaCl + Pb(NO₃)₂ ® PbCl₂ + 3NaNO₃

67.  D) 2NaI + Br₂ ® 2NaBr + I₂

68.  E) Cu(NO₃)₂ + Zn ® Zn(NO₃)₂ + Cu

Ans:  C     Category:  Medium     Section:  4.4

 

64.  In the following chemical reaction the oxidizing agent is

5H₂O₂ + 2MnO₄^– + 6H⁺ ® 2Mn²⁺ + 8H₂O + 5O₂

1.    A) H₂O₂    B)  MnO₄^–    C)  H⁺    D)  Mn²⁺    E)  O₂

Ans:  B     Category:  Medium     Section:  4.4

 

65.  In the following chemical reaction the oxidizing agent is

5S + 6KNO₃ + 2CaCO₃ ® 3K₂SO₄ + 2CaSO₄ + CO₂ + 3N₂

1.    A) S    B)  N₂    C)  KNO₃    D)  CaSO₄    E)  CaCO₃

Ans:  C     Category:  Medium     Section:  4.4

 

66.  Identify the oxidizing agent in the following chemical reaction.

2MnO₄^– + 5H₂SO₃ ® 2Mn²⁺ + 5SO₄^2– + 4H⁺ + 3H₂O

1.    A) MnO₄^–    B)  H₂SO₃    C)  Mn²⁺    D)  SO₄^2–    E)  H⁺

Ans:  A     Category:  Medium     Section:  4.4

 

67.  Identify the reducing agent in the following chemical reaction.

5Fe²⁺(aq) + MnO₄^–(aq) + 8H⁺(aq) ® 5Fe³⁺(aq) + Mn²⁺(aq) + 4H₂O(l)

1.    A) Fe²⁺    B)  MnO₄^–    C)  H⁺    D)  Mn²⁺    E)  Fe³⁺

Ans:  A     Category:  Medium     Section:  4.4

 

68.  Identify the reducing agent in the following chemical reaction.

Cd + NiO₂ + 2H₂O ® Cd(OH)₂ + Ni(OH)₂

1.    A) Cd    B)  NiO₂    C)  H₂O    D)  Cd(OH)₂    E)  Ni(OH)₂

Ans:  A     Category:  Medium     Section:  4.4

 

69.  What element is oxidized in the following chemical reaction?

3Cu + 8HNO₃ ® 3Cu(NO₃)₂ + 2NO + 4H₂O

1.    A) Cu    B)  H    C)  N    D)  O    E)  H₂O

Ans:  A     Category:  Medium     Section:  4.4

 

70.  What element is oxidized in the following chemical reaction?

NiO₂ + Cd + 2H₂O ® Ni(OH)₂ + Cd(OH)₂

1.    A) Ni    B)  Cd    C)  O    D)  H    E)  This is not a redox reaction.

Ans:  B     Category:  Medium     Section:  4.4

 

71.  What element is oxidized in the following chemical reaction?

H₂SO₄ + Cd(OH)₂ ® 2H₂O + CdSO₄

1.    A) H    B)  S    C)  O    D)  Cd    E)  this is not a redox reaction

Ans:  E     Category:  Medium     Section:  4.4

 

72.  What element is reduced in the following chemical reaction?

Cu + 2H₂SO₄ ® CuSO₄ + SO₂ + 2H₂O

1.    A) Cu    B)  H    C)  S    D)  O    E)  H₂O

Ans:  C     Category:  Medium     Section:  4.4

 

73.  Identify the elements that are oxidized and reduced in the following reaction.

KClO₃(aq) + 6HBr(aq) ® KCl(aq) + 3Br₂(l) + 3H₂O(l)

1.    A) Br is oxidized and Cl is reduced           D)      O is oxidized and Cl is reduced

2.    B) Cl is oxidized and H is reduced            E)      Cl is oxidized and Br is reduced

3.    C) H is oxidized and O is reduced

Ans:  A     Category:  Medium     Section:  4.4

 

74.  Predict the products of the following single replacement reaction.

Fe(s) + CuSO₄(aq) ®

1.    A) Cu(s) + FeSO₄(aq)                                 D)      FeCuSO₄(aq)

2.    B) Fe(s) + Cu(s) + SO₄(aq)                        E)      FeO(s) + CuSO₃(aq)

3.    C) CuS(s) + Fe₂SO₄(aq)

Ans:  A     Category:  Medium     Section:  4.4

 

75.  Predict the products of the following single replacement reaction.

Zn(s)  +  CoCl₂(aq)  ®

1.    A) No reaction occurs                                D)      ZnCo(aq)  +  Cl₂(g)

2.    B) Co(s)  +  ZnCl₂(aq)                                E)      ZnCoCl₂(aq)

3.    C) CoCl(aq) + ZnCl(aq)

Ans:  B     Category:  Medium     Section:  4.4

 

76.  Predict the products of the following single replacement reaction.

Ni(s)  +  Cu(NO₃)₂(aq)  ®

1.    A) No reaction occurs                                D)      Ni(NO₃)₂(aq)  +  Cu(s)

2.    B) NiNO₃(aq)  +  CuNO₃(aq)                    E)      Ni(NO₃)₂(aq)  +  Cu²⁺(aq)

3.    C) NiCu(aq)  2 NO₃^–(aq)

Ans:  D     Category:  Medium     Section:  4.4

 

77.  Which of the following is an example of a disproportionation reaction?

78.  A) 2C₂H₆(g) + 7O₂(g) ® 4CO₂(g) + 6H₂O(l)

79.  B) 2KBr(aq) + Cl₂(g) ® 2KCl(aq) + Br₂(l)

80.  C) 2H₂O₂(aq) ® 2H₂O(l) + O₂(g)

81.  D) CaBr₂(aq) + H₂SO₄(aq) ® CaSO₄(s) + 2HBr(g)

82.  E) 2Al(s) + 3H₂SO₄(aq) ® Al₂(SO₄)₃(aq) + 3H₂(g)

Ans:  C     Category:  Medium     Section:  4.4

 

78.  Which of the following is NOT a redox reaction?

79.  A) 2NaN₃(s) ® 2Na(s) + 3N₂(g)

80.  B) Fe₂O₃(s) + 2Al(s) ® 2Fe(s) + Al₂O₃(s)

81.  C) 3NO₂(g) + H₂O(l) ® 2HNO₃(aq) + NO(g)

82.  D) NH₄Cl(aq)  +  AgNO₃  ® NH₄NO₃(aq)  +  AgCl(s)

83.  E) 2ZnS(s) + 3O₂(g) ® 2ZnO(s) + 2SO₂(g)

Ans:  D     Category:  Medium     Section:  4.4

 

79.  Which of the following is NOT a redox reaction?

80.  A) 2KBr(aq) + Cl₂(g) ® 2KCl(aq) + Br₂(l)

81.  B) 2Na(s) + 2H₂O(l) ® 2NaOH(aq) + H₂(g)

82.  C) V₂O₅(s)  +  5 Ca(l) ®  2 V(l)  +  5 CaO(s)

83.  D) 2KNO₃(s) ® 2KNO₂(s) + O₂(g)

84.  E) 2LiOH(aq) + H₂SO₄(aq) ® Li₂SO₄(aq) + 2H₂O(l)

Ans:  E     Category:  Medium     Section:  4.4

 

80.  Which of the following represents a precipitation reaction?

81.  A) 2H₂(g) + O₂(g) ® 2H₂O(l)

82.  B) CaBr₂(aq) + H₂SO₄(aq) ® CaSO₄(s) + 2HBr(g)

83.  C) 2KNO₃(s) ® 2KNO₂(s) + O₂(g)

84.  D) 2KBr(aq) + Cl₂(g) ® 2KCl(aq) + Br₂(l)

85.  E) 2Al(s) + 3H₂SO₄(aq) ® Al₂(SO₄)₃(aq) + 3H₂(g)

Ans:  B     Category:  Easy     Section:  4.2

 

81.  Which of the following represents an acid-base neutralization reaction?

82.  A) 2Al(s) + 3H₂SO₄(aq) ® Al₂(SO₄)₃(aq) + 3H₂(g)

83.  B) SO₂(g) + H₂O(l) ® H₂SO₃(g)

84.  C) LiOH(aq) + HNO₃(aq) ® LiNO₃(aq) + H₂O(l)

85.  D) 2KBr(aq) + Cl₂(g) ® 2KCl(aq) + Br₂(l)

86.  E) CaBr₂(aq) + H₂SO₄(aq) ® CaSO₄(s) + 2HBr(g)

Ans:  C     Category:  Easy     Section:  4.3

 

82.  Which of the following represents a hydrogen displacement reaction?

83.  A) 2C₂H₆(g) + 7O₂(g) ® 4CO₂(g) + 6H₂O(l)

84.  B) 2KBr(aq) + Cl₂(g) ® 2KCl(aq) + Br₂(l)

85.  C) N₂(g) + 3H₂(g) ® 2NH₃(g)

86.  D) CaBr₂(aq) + H₂SO₄(aq) ® CaSO₄(s) + 2HBr(g)

87.  E) 2Al(s) + 3H₂SO₄(aq) ® Al₂(SO₄)₃(aq) + 3H₂(g)

Ans:  E     Category:  Medium     Section:  4.4

 

83.  Which of the following represents a combustion reaction?

84.  A) 2C₂H₆(g) + 7O₂(g) ® 4CO₂(g) + 6H₂O(l)

85.  B) LiOH(aq) + HNO₃(aq) ® LiNO₃(aq) + H₂O(l)

86.  C) N₂(g) + 3H₂(g) ® 2NH₃(g)

87.  D) 2Na(s) + 2H₂O(l) ® 2NaOH(aq) + H₂(g)

88.  E) 2Al(s) + 3H₂SO₄(aq) ® Al₂(SO₄)₃(aq) + 3H₂(g)

Ans:  A     Category:  Easy     Section:  4.4

 

84.  What type of reaction is the following?

Ca(OH)₂(s)  +  2 HNO₃(aq)  ®  Ca(NO₃)₂(aq)  +  2 H₂O(l)

1.    A) Combination reaction                            D)      Disproportionation reaction

2.    B) Acid-base neutralization reaction          E)      Combustion reaction

3.    C) Hydrogen displacement reaction

Ans:  B     Category:  Medium     Section:  4.4

 

85.  What type of reaction is the following?

C₂H₄(g)  +  3 O₂(g)  ®  2 CO₂(g)  +  2 H₂O(g)

1.    A) Combination reaction                            D)      Disproportionation reaction

2.    B) Acid-base neutralization reaction          E)      Combustion reaction

3.    C) Hydrogen displacement reaction

Ans:  E     Category:  Medium     Section:  4.4

 

86.  The reaction below can be classified as which  type of reaction ?

2 NO₂(g)  +  H₂O(l)  ®  HNO₂(aq)  +  HNO₃(aq)

1.    A) Combination reaction                            D)      Disproportionation reaction

2.    B) Acid-base neutralization reaction          E)      Combustion reaction

3.    C) Hydrogen displacement reaction

Ans:  D     Category:  Medium     Section:  4.4

 

87.  What mass of C₆H₁₂O₆ (glucose) is needed to prepare 450. mL of a 0.650 M solution of glucose in water?

88.  A) 293 g    B)  293 g    C)  0.692 g    D)  52.7 g    E)  125 g

Ans:  D     Category:  Medium     Section:  4.5

 

88.  What mass of C₁₂H₂₂O₁₁ (sucrose) is needed to prepare 255 mL of a 0.570 M solution of sucrose in water?

89.  A) 8 g    B)  145 g    C)  153 g    D)  0.145 g    E)  447 g

Ans:  A     Category:  Medium     Section:  4.5

 

89.  What mass of K₂CO₃ is needed to prepare 200. mL of a solution having a potassium ion concentration of 0.150 M?

90.  A) 15 g    B)  10.4 g    C)  13.8 g    D)  2.07 g    E)  1.49 g

Ans:  D     Category:  Medium     Section:  4.5

 

90.  What mass of Na₂SO₄ is needed to prepare 350. mL of a solution having a sodium ion   concentration of 0.125 M?

91.  A) 11 g    B)  24.9 g    C)  12.4 g    D)  6.21 g    E)  8.88 g

Ans:  A     Category:  Medium     Section:  4.5

 

91.  What mass of Li₃PO₄ is needed to prepare 500. mL of a solution having a lithium ion concentration of 0.175 M?

92.  A) 75 g    B)  10.1 g    C)  19.3 g    D)  30.4 g    E)  3.38 g

Ans:  E     Category:  Medium     Section:  4.5

 

92.  A 50.0 mL sample of 0.436 M NH₄NO₃ is diluted with water to a total volume of 250.0 mL.  What is the ammonium nitrate concentration in the resulting solution?

93.  A) 8 M    B)  0.459 M    C)  2.18 × 10^–2 M    D)  8.72 × 10^–2 M    E)  0.109 M

Ans:  D     Category:  Easy     Section:  4.5

 

93.  A 20.00 mL sample of 0.1015 M nitric acid is introduced into a flask, and water is added until the volume of the solution reaches 250. mL.  What is the concentration of nitric  acid in the final solution?

94.  A) 27 M                                                   D)      3.25 × 10^–2 M

95.  B) 12 × 10^–3 M                                        E)      5.08 × 10^–4 M

96.  C) 406 M

Ans:  B     Category:  Easy     Section:  4.5

 

94.  A 3.682 g sample of KClO₃ is dissolved in enough water to give 375. mL of solution. What is the chlorate ion concentration in this solution?

95.  A) 00 × 10^–2 M                                        D)      1.65 × 10^–2 M

96.  B) 41 × 10^–2 M                                        E)      8.01 × 10^–2 M

97.  C) 118 M

Ans:  E     Category:  Medium     Section:  4.5

 

95.  A 4.691 g sample of MgCl₂ is dissolved in enough water to give 750. mL of solution. What is the magnesium ion concentration in this solution?

96.  A) 70 × 10^–2 M                                        D)      4.93 × 10^–2 M

97.  B) 05 × 10^–2 M                                        E)      0.131 M

98.  C) 57 × 10^–2 M

Ans:  C     Category:  Medium     Section:  4.5

 

96.  A 0.9182 g sample of CaBr₂ is dissolved in enough water to give 500. mL of solution. What is the calcium ion concentration in this solution?

97.  A) 19 × 10^–3 M                                        D)      4.59 × 10^–3 M

98.  B) 30 × 10^–3 M                                        E)      1.25 × 10^–3 M

99.  C) 72 × 10^–3 M

Ans:  A     Category:  Medium     Section:  4.5

 

97.  35.0 mL of 0.255 M nitric acid is added to 45.0 mL of 0.328 M Mg(NO₃)₂.  What is the concentration of nitrate ion in the final solution?

98.  A) 481 M    B)  0.296 M    C)  0.854 M    D)  1.10 M    E)  0.0295 M

Ans:  A     Category:  Difficult     Section:  4.5

 

98.  17.5 mL of a 0.1050 M Na₂CO₃ solution is added to 46.0 mL of 0.1250 M NaCl.  What is the concentration of sodium ion in the final solution?

99.  A) 205 M    B)  0.119 M    C)  0.539 M    D)  0.148 M    E)  0.165 M

Ans:  D     Category:  Difficult     Section:  4.5

 

99.  25.0 mL of a 0.2450 M NH₄Cl solution is added to 55.5 mL of 0.1655 M FeCl₃.  What is the concentration of chloride ion in the final solution?

100.          A) 607 M    B)  0.418 M    C)  1.35 M    D)  0.190 M    E)  0.276 M

Ans:  B     Category:  Difficult     Section:  4.5

 

100.          A 350. mL solution of 0.150 M HNO₃(aq) is mixed with a solution of 230. mL of 0.240 M HCl(aq). How many moles of H⁺(aq) are present in the final solution?

101.          A) 0525 moles H⁺                                    D)      0.0539 moles H⁺

102.          B) 108 moles H⁺                                      E)      0.195 moles H⁺

103.          C) 186 moles H⁺

Ans:  B     Category:  Difficult     Section:  4.5

 

101.          A 430. mL solution of 0.230 M HBr(aq) is mixed with a solution of 225 mL of 0.350 M HClO₄(aq). How many moles of H⁺(aq) are present in the final solution?

102.          A) 0989 moles H⁺                                    D)      0.178 moles H⁺

103.          B) 0888 moles H⁺                                    E)      0.271 moles H⁺

104.          C) 290 moles H⁺

Ans:  D     Category:  Difficult     Section:  4.5

 

102.          A 110. mL solution of 0.340 M HCl(aq) is mixed with a solution of 330. mL of 0.150 M HNO₃(aq). The solution is then diluted to a final volume of 1.00 L. How many moles of H⁺ are present in the final solution?

103.          A) 0869 moles H⁺                                    D)      0.374 moles H⁺

104.          B) 490 moles H⁺                                      E)      0.0435 moles H⁺

105.          C) 415 moles H⁺

Ans:  A     Category:  Difficult     Section:  4.5

 

103.          When 38.0 mL of 0.1250 M H₂SO₄ is added to 100. mL of a solution of PbI₂, a precipitate of PbSO₄ forms.  The PbSO₄ is then filtered from the solution, dried, and weighed.  If the recovered PbSO₄ is found to have a mass of 0.0471 g, what was the concentration of iodide ions in the original solution?

104.          A) 10 × 10^–4 M                                        D)      3.11 × 10^–3 M

105.          B) 55 × 10^–4 M                                        E)      1.55 × 10^–3 M

106.          C) 20 × 10^–3 M

Ans:  D     Category:  Difficult     Section:  4.6

 

104.          When 50.0 mL of a 0.3000 M AgNO₃ solution is added to 50.0 mL of a solution of MgCl₂, an AgCl precipitate forms immediately.  The precipitate is then filtered from the solution, dried, and weighed.  If the recovered AgCl is found to have a mass of 0.1183 g,  what as the concentration of magnesium ions in the original MgCl₂ solution?

105.          A) 300 M                                                 D)      2.06 × 10^–5 M

106.          B) 25 × 10^–3 M                                        E)      4.13 × 10^–3 M

107.          C) 65 × 10^–2 M

Ans:  B     Category:  Difficult     Section:  4.6

 

105.          When 20.0 mL of a 0.250 M (NH₄)₂S solution is added to 150.0 mL of a solution of Cu(NO₃)₂, a CuS precipitate forms.  The precipitate is then filtered from the solution, dried, and weighed.  If the recovered CuS is found to have a mass of 0.3491 g, what was the concentration of copper ions in the original Cu(NO₃)₂ solution?

106.          A) 65 × 10^–3 M                                        D)      4.87 × 10^–2 M

107.          B) 22 × 10^–2 M                                        E)      2.43 × 10^–2 M

108.          C) 33 × 10^–2 M

Ans:  E     Category:  Difficult     Section:  4.6

 

106.          34.62 mL of 0.1510 M NaOH was needed to neutralize 50.0 mL of an H₂SO₄ solution.  What is the concentration of the original sulfuric acid solution?

107.          A) 0229 M    B)  0.218 M    C)  0.0523 M    D)  0.209 M    E)  0.105 M

Ans:  C     Category:  Medium     Section:  4.7

 

107.          What volume (mL) of a 0.3428 M HCl(aq) solution is required to completely neutralize 23.55 mL of a 0.2350 M Ba(OH)₂(aq) solution?

108.          A) 34 mL    B)  11.07 mL    C)  16.14 mL    D)  32.29 mL    E)  47.10 mL

Ans:  D     Category:  Medium     Section:  4.7

 

108.          What volume (mL) of a 0.2450 M KOH(aq) solution is required to completely neutralize 55.25 mL of a 0.5440 M H₃PO₄(aq) solution?

109.          A) 06 mL    B)  165.8 mL    C)  90.17 mL    D)  22.09 mL    E)  368.0 mL

Ans:  E     Category:  Medium     Section:  4.7

 

109.          The concentration of oxalate ion (C₂O₄^2–) in a sample can be determined by titration with a solution of permanganate ion (MnO₄^–) of known concentration.  The net ionic equation for this reaction is

2MnO₄^– + 5C₂O₄^2– + 16H⁺ ® 2Mn²⁺ + 8H₂O + 10CO₂

                A 30.00 mL sample of an oxalate solution is found to react completely with 21.93 mL of  a 0.1725 M solution of MnO₄^–.  What is the oxalate ion concentration in the sample?

1.    A) 02914 M    B)  0.4312 M    C)  0.1821 M    D)  0.3152 M    E)  0.05044 M

Ans:  D     Category:  Medium     Section:  4.8

 

110.          One method of determining the concentration of hydrogen peroxide (H₂O₂) in a solution is through titration with the iodide ion.  The net ionic equation for this reaction is

H₂O₂ + 2I^– +2H⁺ ® I₂ + 2H₂O

A 50.00 mL sample of a hydrogen peroxide solution is found to react completely with 37.12 mL of a 0.1500 M KI solution.  What is the concentration of hydrogen peroxide in the sample?

5.    A) 568 × 10^–2 M                                      D)      0.4041 M

6.    B) 2227 M                                               E)      0.1114 M

7.    C) 1010 M

Ans:  A     Category:  Medium     Section:  4.8

 

111.          Zinc dissolves in hydrochloric acid to yield hydrogen gas:

Zn(s) + 2HCl(aq) ® ZnCl₂(aq) + H₂(g)

What mass of hydrogen gas is produced when a 7.35 g chunk of zinc dissolves in 500.  mL of 1.200M HCl?

1.    A) 605 g    B)  0.113 g    C)  0.302 g    D)  0.453 g    E)  0.227 g

Ans:  E     Category:  Medium     Section:  4.8

 

112.          Zinc dissolves in hydrochloric acid to yield hydrogen gas:

Zn(s) + 2HCl(aq) ® ZnCl₂(aq) + H₂(g)

When a 12.7 g chunk of zinc dissolves in 500. mL of 1.450M HCl, what is the  concentration of hydrogen ions remaining in the final solution?

1.    A) 776 M    B)  0.388 M    C)  0.674 M    D)  1.06 M    E)  0 M

Ans:  C     Category:  Medium     Section:  4.8

 

113.          Lithium metal dissolves in water to yield hydrogen gas and aqueous lithium hydroxide.  What is the final concentration of hydroxide ions when 5.500 g of lithium metal is dropped into 750. mL of water?

114.          A) 06 M    B)  0.528 M    C)  2.11 M    D)  0.792 M    E)  0.943 M

Ans:  A     Category:  Medium     Section:  4.8

 

114.          When solid iron(II) hydroxide is added to water, the resulting solution contains 1.4×10^–3g of dissolved iron(II) hydroxide per liter of solution.  What is the hydroxide ion concentration in this solution?

115.          A) 8×10^–6 M                                            D)      3.1×10^–5 M

116.          B) 6×10^–5 M                                            E)      4.0×10^–3 M

117.          C) 5×10^–10 M

Ans:  D     Category:  Difficult     Section:  4.5

 

115.          A 250. mL sample of 0.0328M HCl is partially neutralized by the addition of 100. mL of 0.0245M NaOH.  Find the concentration of hydrochloric acid in the resulting solution.

116.          A) 00700 M    B)  0.0164 M    C)  0.0383 M    D)  0.0230 M    E)  0.0575 M

Ans:  B     Category:  Difficult     Section:  4.7

 

116.          A 350. mL sample of 0.276M HNO₃ is partially neutralized by 125 mL of 0.0120M Ca(OH)₂.  Find the concentration of nitric acid in the resulting solution.

117.          A) 210 M    B)  0.00632 M    C)  0.203 M    D)  0.0240 M    E)  0.197 M

Ans:  E     Category:  Difficult     Section:  4.7

 

117.          158 mL of a 0.148M NaCl solution is added to 228 mL of a 0.369M NH₄NO₃ solution.  The concentration of ammonium ions in the resulting mixture is

118.          A) 157 M    B)  0.218 M    C)  0.625 M    D)  0.369 M    E)  0 M

Ans:  B     Category:  Medium     Section:  4.5

 

118.          1.40 g of silver nitrate is dissolved in 125 mL of water.  To this solution 5.00 mL of 1.50M hydrochloric acid is added, and a precipitate forms.  Find the concentration of silver ions remaining in solution.

119.          A) 7×10^–3 M                                            D)      0.121M

120.          B) 34×10^–2 M                                          E)      5.9×10^–3 M

121.          C) 77×10^–2 M

Ans:  A     Category:  Difficult     Section:  4.6

 

119.          Define the terms solution, solute, and solvent.

Ans:  A solution is a homogeneous mixture of two or more substances.

The substance present in a smaller amount is called the solute, while the substance present in the larger amount is called the solvent.

Category:  Easy     Section:  4.1

 

120.          Identify the following compound as a strong electrolyte, weak electrolyte, or nonelectrolyte: Al(NO₃)₃

Ans:  strong electrolyte

Category:  Easy     Section:  4.1

 

121.          Identify the following compound as a strong electrolyte, weak electrolyte, or nonelectrolyte: NH₄NO₃

Ans:  strong electrolyte

Category:  Easy     Section:  4.1

 

122.          Identify the following compound as a strong electrolyte, weak electrolyte, or nonelectrolyte: H₃PO₄

Ans:  weak electrolyte

Category:  Easy     Section:  4.3

 

123.          Identify the following compound as a strong electrolyte, weak electrolyte, or nonelectrolyte: H₂CO₃

Ans:  weak electrolyte

Category:  Easy     Section:  4.3

 

124.          Identify the following compound as a strong electrolyte, weak electrolyte, or nonelectrolyte: CH₃OH (methanol).

Ans:  nonelectrolyte

Category:  Easy     Section:  4.1

 

125.          Identify the following compound as a strong electrolyte, weak electrolyte, or nonelectrolyte: CH₃COOH.

Ans:  weak electrolyte

Category:  Easy     Section:  4.1

 

126.          Identify the following compound as a strong electrolyte, weak electrolyte, or nonelectrolyte: NH₃.

Ans:  weak electrolyte

Category:  Medium     Section:  4.1

 

127.          Identify the following compound as a strong electrolyte, weak electrolyte, or nonelectrolyte: NH₄Cl.

Ans:  strong electrolyte

Category:  Easy     Section:  4.1

 

128.          Identify the precipitate(s) formed when solutions of Na₃PO₄(aq), Ca(NO₃)₂(aq), and NH₄ClO₃(aq) are mixed.

Ans:  Ca₃(PO₄)₂

Category:  Medium     Section:  4.2

 

129.          Identify the precipitate(s) formed when solutions of Hg₂(ClO₄)₂(aq), (NH₄)₂SO₄(aq), and Rb₂SO₄(aq) are mixed.

Ans:  Hg₂SO₄

Category:  Medium     Section:  4.2

 

130.          Identify the precipitate(s) formed when solutions of NaOH(aq), Ca(ClO₃)₂(aq), and Ba(OH)₂(aq) are mixed.

Ans:  Ca(OH)₂

Category:  Medium     Section:  4.2

 

131.          Give an example of a monoprotic acid.

Ans:  HNO₃ (for example)

Category:  Easy     Section:  4.3

 

132.          Give an example of a diprotic acid.

Ans:  H₂CO₃ (for example)

Category:  Easy     Section:  4.3

 

133.          Name and give the formulas for six strong acids.

Ans:  hydrochloric acid, HCl; hydrobromic acid, HBr; hydroiodic acid, HI; nitric acid, HNO₃; sulfuric acid, H₂SO₄; perchloric acid, HClO₄

Category:  Easy     Section:  4.3

 

134.          Give an example of a triprotic acid.

Ans:  H₃PO₄

Category:  Easy     Section:  4.3

 

135.          Write the net ionic equation for reaction that occurs when aqueous iron(III) sulfate is added to aqueous sodium sulfide to produce solid iron(III) sulfide and aqueous sodium sulfate.

Ans:  2Fe³⁺(aq) + 3S^2– (aq) ® Fe₂S₃(s)

Category:  Medium     Section:  4.2

 

136.          Determine the oxidation number of each of the elements in Cs₂Cr₂O₇?

Ans:  the oxidation number of Cs is +1; the oxidation number of Cr is +6; the oxidation number of O is –2

Category:  Easy     Section:  4.4

 

137.          Identify the element being oxidized in the following reaction.

4Al + 3O₂  ® 2Al₂O₃

Ans:  Al

Category:  Medium     Section:  4.4

 

138.          Identify the element being reduced in the following reaction.

4Al + 3O₂  ® 2Al₂O₃

Ans:  O

Category:  Medium     Section:  4.4

 

139.          Identify the oxidizing agent in the following reaction.

4Al + 3O₂ ® 2Al₂O₃

Ans:  O₂

Category:  Medium     Section:  4.4

 

140.          Identify the reducing agent in the following reaction.

4Al + 3O₂  ® 2Al₂O₃

Ans:  Al

Category:  Medium     Section:  4.4

 

141.          Identify the element being oxidized in the following reaction.

2KBr + F₂ ® Br₂ + 2KF

Ans:  Br

Category:  Medium     Section:  4.4

 

142.          Identify the element being reduced in the following reaction.

2KBr + F₂ ® Br₂ + 2KF

Ans:  F

Category:  Medium     Section:  4.4

 

143.          Identify the oxidizing agent in the following reaction.

2KBr + F₂ ® Br₂ + 2KF

Ans:  F₂

Category:  Medium     Section:  4.4

 

144.          Identify the reducing agent in the following reaction.

2KBr + F₂ ® Br₂ + 2KF

Ans:  Br^– (or KBr)

Category:  Medium     Section:  4.4

 

145.          Determine the oxidation number of each of the elements in BaNaPO₄?

Ans:  the oxidation number of Ba +2; the oxidation number of Na is +1; the oxidation number of P is +5; the oxidation number of O is –2

Category:  Easy     Section:  4.4

 

146.          Determine the oxidation number of each of the elements in NaAl(OH)₄?

Ans:  the oxidation number of Na is +1; the oxidation number of Al is +3; the oxidation number of O is –2, the oxidation number of H is +1

Category:  Easy     Section:  4.4

 

147.          Thorium metal is prepared by reacting thorium oxide with calcium as shown below.

ThO₂ + 2Ca ® Th + 2CaO

Which substance is reduced in this process?

Ans:  Th⁴⁺ is reduced

Category:  Medium     Section:  4.4

 

148.          Thorium metal is prepared by reacting thorium oxide with calcium as depicted below.

ThO₂ + 2Ca ® Th + 2CaO

What is the reducing agent in this process?

Ans:  Ca

Category:  Medium     Section:  4.4

 

149.          Thorium metal is prepared by reacting thorium oxide with calcium as shown below.

ThO₂ + 2Ca ® Th + 2CaO

Which substance is oxidized in this process?

Ans:  Ca

Category:  Medium     Section:  4.4

 

150.          Thorium metal is prepared by reacting thorium oxide with calcium as shown below.

ThO₂ + 2Ca ® Th + 2CaO

What is the oxidizing agent in this process?

Ans:  ThO₄

Category:  Medium     Section:  4.4

 

151.          Batteries in our cars generate electricity by the following chemical reaction.

Pb + PbO₂ + 2H₂SO₄ ® 2PbSO₄ + 2H₂O

Which substance is reduced in this process?

Ans:  Pb⁴⁺

Category:  Medium     Section:  4.4

 

152.          Batteries in our cars generate electricity by the following chemical reaction.

Pb + PbO₂ + 2H₂SO₄ ® 2PbSO₄ + 2H₂O

What is the reducing agent in this process?

Ans:  Pb

Category:  Medium     Section:  4.4

 

153.          Batteries in our cars generate electricity by the following chemical reaction.

Pb + PbO₂ + 2H₂SO₄ ® 2PbSO₄ + 2H₂O

Which substance is oxidized in this process?

Ans:  Pb

Category:  Medium     Section:  4.4