Chapter 4 – Chemical Reactions
1. Which of the following concerning electrolytes and nonelectrolytes is/are true?
1.
Some molecular substances are electrolytes.
2.
All electrolytes are ionic substances.
3.
Strong electrolytes partially ionize in solution.
A)
1 only
B)
2 only
C)
3 only
D)
1 and 3
E)
2 and 3
2. Which of the following correctly describes one or more of the differences between a strong
and weak electrolyte?
A)
A strong electrolyte partially ionizes in solution and a weak electrolyte completely
ionizes in solution.
B)
Strong electrolytes are all classified as soluble ionic substances and weak
electrolytes are all classified as soluble molecular substances.
C)
Strong electrolytes produce more ions per mole of substance in solution than weak
electrolytes.
D)
Weak electrolytes inhibit the flow of electricity.
E)
Strong electrolytes are weak conductors of electricity.
3. Which of the following is a nonelectrolyte in aqueous solution?
A)
NH4F
B)
NH4Cl
C)
NaHS
D)
CH4
E)
Na2S
4. Which of the following solutions would be expected to be the best conductor of an electric
current at room temperature?
A)
0.10 M Na2SO4
B)
1.0 M CH3COOH
C)
0.10 M NaCl
D)
0.10 M CO(NH2)2
E)
0.10 M CH3COOH
5. Which of the following solutes, dissolved in 1000 g of water, would provide the greatest
number of particles?
A)
0.030 mol of urea, CO(NH2)2
B)
0.030 mol of ammonium nitrate, NH4NO3
C)
0.030 mol of barium chloride, BaCl2
D)
0.030 mol of acetic acid, CH3COOH
E)
0.030 mol of calcium sulfate, CaSO4
6. Which of the following aqueous solutions would be expected to be the best conductor of an
electric current at room temperature?
A)
0.10 M CH3COOH
B)
0.10 M HCl
C)
0.10 M Na2SO4
D)
0.10 M NaCl
E)
0.10 M H3PO4
7. Which of the following ions is most likely to form an insoluble sulfate?
A)
Ca2+
B)
Cl–
C)
K+
D)
Li+
E)
S2–
MSC: general chemistry
8. Which of the following compounds is soluble in water?
A)
Ga2O3
B)
Na3P
C)
ZnS
D)
Hg2Cl2
E)
CdS
9. Which of the following compounds is insoluble in water?
A)
FeCO3
B)
Li2CO3
C)
(NH4)2CO3
D)
K2CO3
E)
Na2CO3
10. Which of the following compounds is insoluble in water?
A)
Hg2SO4
B)
FeSO4
C)
Li2SO4
D)
(NH4)2SO4
E)
Cr2(SO4)3
11. Which of the following compounds is soluble in water?
A)
PbCl2
B)
PbBr2
C)
CaSO4
D)
Ca(NO3)2
E)
HgBr2
Test Bank General Chemistry, 10th edition 4
12. Which of the following compounds is insoluble in water?
A)
NH4I
B)
RbI
C)
CuCl2
D)
AgI
E)
LiI
13. Which of the following concerning electrolytes and the solubility rules is/are true?
1.
The solubility rules apply only to ionic substances.
2.
All soluble ionic compounds are considered strong electrolytes.
3.
The solubility rules apply to aqueous and non-aqueous solutions.
A)
1 only
B)
2 only
C)
3 only
D)
1 and 2
E)
1, 2, and 3
14. A student is given a sample in lab that contains one of the ions listed below. After adding a
few drops of AgNO3 solution to a portion of the unknown sample, the student observed a
grayish precipitate. After adding a few drops of Mg(NO3)2 solution to another portion of the
unknown sample, the student got a black precipitate. Based on these observations, what is
the only possible ion in this student’s sample?
A)
Cl–
B)
F–
C)
C2H3O2–
D)
S2–
E)
SO42–
15. Which anion will form a precipitate with Rb+?
A)
Cl–
B)
SO42–
C)
C2H3O2–
D)
S2–
E)
none of the above
16. Which anion will form a precipitate with Ca2+?
A)
Cl–
B)
SO42–
C)
C2H3O2–
D)
Br–
E)
none of the above
17. Identify the spectator ions in the following reaction.
Ca2+(aq) + 2NO3–(aq) + 2Na+(aq) + CO32–(aq) → CaCO3(s) + 2Na+(aq) + NO3–(aq)
A)
NO3– and CO32–
B)
Ca2+ and Na+
C)
Ca2+ and CO32–
D)
Ca2+ and NO3–
E)
Na+ and NO3–
18. Which of the following concerning molecular and ionic equations is/are correct?
1.
Molecular equations cannot be written for reactions involving ionic
substances.
2.
Charge must be balanced in a properly balanced net ionic reaction.
3.
In a balanced complete ionic reaction only the strong electrolytes are shown as
the individual aqueous ions.
A)
1 only
B)
2 only
C)
3 only
D)
1 and 3
E)
2 and 3
Test Bank General Chemistry, 10th edition 6
19. Which of the following would not be depicted as the individual ions on the reactant side of a
complete ionic reaction?
A)
RbOH
B)
HBr
C)
Cu(NO3)2
D)
CuCO3
E)
Ti(NO3)3
20. Which of the following would not be depicted as the individual ions on the reactant side of a
complete ionic reaction?
A)
LiOH
B)
HCl
C)
ZnBr2
D)
CH3COOH
E)
FeI3
21. Identify the spectator ion(s) in the following reaction.
Cu(OH)2(s) + 2H+(aq) + 2Cl–(aq) → Cu2+(aq) + 2Cl–(aq) + 2H2O(l)
A)
Cu2+ and Cl–
B)
Cu2+
C)
Cu(OH)2
D)
Cl–
E)
H+ and Cl–
22. Identify the spectator ion(s) in the following reaction.
Zn(OH)2(s) + 2K+(aq) + 2OH–(aq) → 2K+(aq) + Zn(OH)4–(aq)
A)
K+ and Zn(OH)42–
B)
K+
C)
Zn(OH)2
D)
Zn(OH)42–
E)
K+ and OH–
23. What precipitate forms when aqueous solutions of calcium bromide and potassium
phosphate are mixed?
A)
(KBr)2(s)
B)
Ca3(PO4)2(s)
C)
CaPO4–(s)
D)
KBr(s)
E)
CaPO4(s)
24. Which equation best represents the net ionic equation for the reaction that occurs when
aqueous solutions of potassium phosphate and iron(II) nitrate are mixed?
A)
3Fe2+(aq) + 2PO43–(aq) → Fe3(PO4)2(s)
B)
2K+(aq) + Fe(NO3)2(aq) → 2KNO3(aq) + Fe2+(aq)
C)
3Fe2+(aq) + 2PO43–(aq) → Fe3(PO4)2(aq)
D)
2K3PO4(aq) + 3Fe2+(aq) → Fe3(PO4)2(s) + (K+)6(aq)
E)
2K3PO4(aq) + 3Fe(NO3)2(aq) → Fe3(PO4)2(s) + 6KNO3(aq)
25. Which net ionic equation best represents the reaction that occurs when an aqueous solution
of lithium nitrate is mixed with an aqueous solution of ammonium bromide?
A)
Li+(aq) + Br–(aq) → LiBr(s)
B)
NH4+(aq) + NO3–(aq) → NH4NO3(aq)
C)
NH4Br(aq) + LiNO3(aq) → LiBr(s) + NH4NO3(aq)
D)
No net reaction occurs.
E)
Li+(aq) + NH4Br(aq) → LiBr(s) + NH4+(aq)
26. A precipitate is expected when an aqueous solution of potassium iodide is added to an
aqueous solution of
A)
calcium nitrate.
B)
barium hydroxide.
C)
lead perchlorate.
D)
iron(II) chloride.
E)
sodium sulfate.
27. Which of the following concerning precipitation reactions is/are correct?
1.
A precipitation reaction is a type of chemical reaction that forms a gaseous
product (such as CO2).
2.
A precipitation reaction is possible when two or more aqueous solutions of
strong or weak electrolytes are mixed.
3.
Only ionic compounds will react to form precipitates in a precipitation
reactions.
A)
1 only
B)
2 only
C)
3 only
D)
2 and 3
E)
1, 2, and 3
28. Which of the following combinations will produce a precipitate?
1.
AgNO3(aq) and HCl(aq)
2.
HCl(aq) and Na2CO3(aq)
3.
NaOH(aq) and K3PO4(aq)
A)
1 only
B)
2 only
C)
3 only
D)
2 and 3
E)
1, 2, and 3
29. Which of the following are classified as precipitation reactions?
1.
AgNO3(aq) + HCl(aq) → AgCl(s) + HNO3(aq)
2.
2Mg(s) + O2(g) → 2MgO(s)
3.
Zn(s) + 2Ag+(aq) → 2Ag(s) + Zn2+(aq)
A)
1 only
B)
2 only
C)
3 only
D)
2 and 3
E)
1, 2, and 3
30. A precipitate will form when a freshly prepared aqueous carbonic acid solution is added to
an aqueous solution of
A)
potassium carbonate.
B)
ammonium chloride.
C)
nitrous acid.
D)
calcium hydroxide.
E)
sodium chloride.
31. When a solution of lithium chloride and a solution of ammonium sulfate are mixed,
A)
a new salt is formed.
B)
no reaction occurs.
C)
a precipitate forms.
D)
an acid and a base are formed.
E)
a gas is evolved.
32. When solutions of barium chloride and lithium sulfate are mixed, the spectator ions in the
resulting reaction are
A)
only SO42–.
B)
both Li+ and Cl–.
C)
only Cl–.
D)
only Li+.
E)
only Ba2+.
Test Bank General Chemistry, 10th edition 10
33. Aqueous solutions of sodium sulfide and copper(II) chloride are mixed together. Which
statement is correct?
A)
CuS will precipitate from solution.
B)
NaCl will precipitate from solution.
C)
No precipitate will form.
D)
Both NaCl and CuS will precipitate from solution.
E)
No reaction will occur.
34. Which net ionic equation best represents the reaction that occurs when an aqueous solution
of barium chloride is mixed with an aqueous solution of lithium sulfate?
A)
2H+(aq) + 2Cl–(aq) → 2HCl(g)
B)
Ba2+(aq) + SO42–(aq) → BaSO4(s)
C)
Ba2+(aq) + 2Cl–(aq) + 2Li+(aq) + SO42–(aq) → BaSO4(s) + 2LiCl(aq)
D)
BaCl2(aq) + Li2SO4(aq)→ BaSO4(s)+ 2LiCl(aq)
E)
No net reaction occurs.
35. What products result from mixing aqueous solutions of Ni(NO3)2(aq) and NaNO3(aq)?
A)
Ni(OH)2(s), Na+(aq), and NO3−(aq)
B)
Ni(OH)2(s) and NaNO3(s)
C)
Ni2(OH)2(aq) and NaNO3(aq)
D)
Ni(OH)2(aq) and NaNO3(s)
E)
Ni(OH)2(s), N2(g), and H2O(l)
36. What products result from mixing aqueous solutions of Cu(C2H3O2)2(aq) and Rb3PO4(aq)?
A)
Cu2PO4(s) and Rb3(C2H3O2)2(aq)
B)
Cu3(PO4)2(s) and RbC2H3O2(s)
C)
CuP(s), CO2(g), H2O(l), RbOH(aq), and PH3(g).
D)
CuPO4(s) and Rb3(C2H3O2)2(aq)
E)
Cu3(PO4)2(s), Rb+(aq), and C2H3O2−(aq)
37. Which of the following is not an Arrhenius base?
A)
NH3
B)
KOH
C)
Ba(OH)2
D)
Ca(OH)2
E)
all are Arrhenius bases
38. Which of the following may be classified as an acid-base reaction?
1.
AgNO3(aq) + HCl(aq) → AgCl(s) + HNO3(aq)
2.
2Mg(s) + O2(g) → 2MgO(s)
3.
Zn(s) + 2Ag+(aq) → 2Ag(s) + Zn2+(aq)
A)
1 only
B)
2 only
C)
3 only
D)
1, 2, and 3
E)
none
39. Which of the following combinations will result in an acid-base reaction?
1.
AgNO3(aq) and HCl(aq)
2.
HCl(aq) and Na2CO3(aq)
3.
NaOH(aq) and K3PO4(aq)
A)
1 only
B)
2 only
C)
3 only
D)
1, 2, and 3
E)
none
Test Bank General Chemistry, 10th edition 12
40. Which of the following concerning acid-base reactions is/are correct?
1.
Only strong acids and strong bases will undergo an acid-base reaction.
2.
All acid-base reactions produce water and an ionic compound (salt) as a
product.
3.
All reactions that form a gas are also acid-base reactions.
A)
1 only
B)
2 only
C)
3 only
D)
1, 2, and 3
E)
none
41. Which of the following reactions best describes the dissolution of solid KOH(s) in water?
A)
KOH(s) + H2O(l) → KO–(aq) + H3O+(aq)
B)
KOH(s) → KO–(aq) + H+(aq)
C)
KOH(s) → K+(aq) + OH–(aq)
D)
KOH(s) → KO+(aq) + H–(aq)
E)
KOH(s) → KOH(aq)
42. Which of the following chemical equations best represents the dissolution of a soluble group
2A metal hydroxide in water?
A)
M(OH)2(s) → M+(aq) + (OH)2–(aq)
B)
M(OH)2(s) → M2+(aq) + 2OH–(aq)
C)
M(OH)2(s) + H2O(l) → MO(aq) + OH–(aq) + H3O+(aq)
D)
M(OH)2(s) → M(OH)2(aq)
E)
M(OH)2(s) → MO(aq) + H2O(l)
43. Which of the following reactions best describes the acid–base properties of ammonia (NH3)
in aqueous solution?
A)
NH3(aq) + 3H2O(l) → N3–(aq) + 3H3O+(aq)
B)
NH3(aq) → N3–(aq) + 3H+(aq)
C)
NH3(aq) + H2O(l) NH4+(aq) + OH–(aq)
Test Bank General Chemistry, 10th edition 13
D)
NH3(aq) + H2O(l) → NH4+(aq) + OH–(aq)
E)
NH3(aq) + 3H2O(l) N3–(aq) + 3H3O+(aq)
44. Which of the following reactions best describes the dissolution of gaseous hydrogen
chloride (HCl) in water?
A)
HCl(g) + 2H2O(l) → H3O+(aq) + ClO–(aq) + H2(g)
B)
2HCl(g) → H2(g) + Cl2(g)
C)
HCl(g) + H2O(l) → H3O+(aq) + Cl–(aq)
D)
HCl(g) + 5H2O(l) → H3O+(aq) + ClO4–(aq) + 4H2(g)
E)
HCl(g) + H2O(l) → H3O+(aq) + ClO–(aq)
45. Which of the following reactions best describes the acid–base properties of acetic acid
(HC2H3O2) in aqueous solution?
A)
HC2H3O2(aq) + H2O(l) → H3O+(aq) + C2H3O2–(aq)
B)
HC2H3O2(aq) + H2O(l) → C2H5O2+(aq) + OH–(aq)
C)
HC2H3O2(aq) + H2O(l) C2H5O2+(aq) + OH–(aq)
D)
HC2H3O2(aq) + H2O(l) H3O+(aq) + C2H3O2–(aq)
E)
HC2H3O2(aq) + 4H2O(l) 4H3O+(aq) + C2O24–(aq)
46. Which of the following is not a strong acid in aqueous solution?
A)
HBr
B)
HClO4
C)
HF
D)
HI
E)
HCl
47. Which of the following is a weak base in aqueous solution?
Test Bank General Chemistry, 10th edition 14
A)
HOCH2CH2OH
B)
Ba(OH)2
C)
CH3COOH
D)
NH3
E)
HI
48. Which of the following is a strong base in aqueous solution?
A)
HOCH2CH2OH
B)
Ba(OH)2
C)
H3PO4
D)
NH3
E)
HI
49. Which of the following is a strong acid in aqueous solution?
A)
HOCH2CH2OH
B)
Ba(OH)2
C)
CH3COOH
D)
NH3
E)
HClO4
50. All the following are strong acids in aqueous solution except
A)
HCl.
B)
HF.
C)
HI.
D)
HBr.
E)
H2SO4.
51. Which of the following is a strong acid in aqueous solution?
A)
H3PO3
Test Bank General Chemistry, 10th edition 15
B)
H3PO4
C)
H2CO3
D)
H2SO3
E)
H2SO4
52. Which of the following is not a strong base in aqueous solution?
A)
Sr(OH)2
B)
Ca(OH)2
C)
KOH
D)
LiOH
E)
NH3
53. Which of the following is a strong base in aqueous solution?
A)
LiCl
B)
CH3OH
C)
LiOH
D)
NH3
E)
HClO4
54. Which of the following is a strong electrolyte in aqueous solution?
A)
tartaric acid
B)
ascorbic acid
C)
hypochlorous acid
D)
citric acid
E)
hydroiodic acid
55. All of the following are weak electrolytes in aqueous solution except
A)
acetic acid.
B)
tartaric acid.
Test Bank General Chemistry, 10th edition 16
C)
nitric acid.
D)
citric acid.
E)
nitrous acid.
56. Which of the following is a weak electrolyte in aqueous solution?
A)
HClO4
B)
H2SO4
C)
H3PO4
D)
HNO3
E)
HI
57. Which of the following is a weak electrolyte in aqueous solution?
A)
Mg(OH)2
B)
NH3
C)
LiOH
D)
RbOH
E)
Sr(OH)2
58. Which of the following is a weak acid in aqueous solution?
A)
HCl
B)
H2SO4
C)
H2S
D)
HNO3
E)
HI
59. Which of the following is a weak base in aqueous solution?
A)
HOCl
B)
LiOH
C)
NH3
Test Bank General Chemistry, 10th edition 17
D)
HBr
E)
Ba(OH)2
60. Which of the following is a weak base in aqueous solution?
A)
H2CO3
B)
Ba(OH)2
C)
B(OH)3
D)
LiOH
E)
N2H4
61. Which of the following is a weak acid in aqueous solution?
A)
HClO4
B)
HCl
C)
H2SO4
D)
HNO3
E)
H2SO3
62. Which of the following is a strong acid in aqueous solution?
A)
HClO
B)
H3PO4
C)
HBr
D)
HNO2
E)
H3PO3
63. Which of the following is best described as an acid–base reaction?
A)
HNO3(aq) + NH3(aq) → NH4+(aq) + NO3–(aq)
B)
P4(s) + 3OH–(aq) + 3H3O(l) → PH3(g) + 3H2PO2–(aq)
C)
Cu(s) + H2S(g) → CuS(s) + H2(g)
D)
2H2(g) + O2(g) → 2H2O(l)
Test Bank General Chemistry, 10th edition 18
E)
2KClO3(aq) → 2KCl(s) + 3O2(g)
64. What is the net ionic equation for the acid–base reaction that occurs when acetic acid and
sodium hydroxide solutions are mixed?
A)
HC2H3O2(aq) + OH–(aq) → C2H3O2–(aq) + H2O(l)
B)
H+(aq) + OH–(aq) → H2O(l)
C)
H3O+(aq) + OH–(aq) → 2H2O(l)
D)
C2H3O2–(aq) + H+(aq) + Na+(aq) + OH–(aq) → Na+(aq) + C2H3O2–(aq) + H2O(l)
E)
HC2H3O2(aq) + NaOH–(aq) → NaC2H3O2–(aq) + H2O(l)
65. What is the net ionic equation for the reaction of acetic acid, CH3COOH, with NH3?
A)
CH3COOH(aq) + NH3(aq) → NH4+(aq) + CH3COO–(aq)
B)
H+(aq) + OH–(aq) → H2O(l)
C)
CH3COOH(aq) + NH3(aq) → NH4CH3COO(aq)
D)
CH3COO–(aq) + H+(aq) + NH3(aq) → NH4CH3COO(aq)
E)
H+(aq) + NH3(aq) → NH4+(aq)
66. What is the net ionic equation for the reaction of NH3 with HClO4?
A)
NH3(aq) + H+(aq) → NH4+(aq)
B)
NH3(aq) + HClO4(aq) → NH4ClO4(aq)
C)
NH3(aq) + ClO4–(aq) → NH2–(aq) + HClO4(aq)
D)
H–(aq) + H+(aq) → H2(g)
E)
H+(aq) + OH–(aq) → H2O(l)
67. What is the net ionic equation for the acid–base reaction between chlorous acid and sodium
hydroxide?
A)
H+(aq) + ClO2–(aq) + Na+(aq) + OH–(aq) → NaClO2(aq) + H2O(l)
B)
HClO2(aq) + OH–(aq) → ClO2–(aq) + H2O(l)
C)
HClO2(aq) + NaOH(aq) → NaClO2(aq) + H2O(l)
D)
H+(aq) + OH–(aq) → H2O(l)
E)
H+(aq) + ClO2–(aq) + Na+(aq) + OH–(aq) → Na+(aq) + ClO2–(aq) + H2O(l)
68. What is the net ionic equation for the acid–base reaction that occurs when an excess of a
potassium hydroxide solution is added to a solution of H2SeO3?
A)
H2SeO3(aq) + 2OH–(aq) → 2H2O(l) + SeO32–(aq)
B)
H+(aq) + OH–(aq) → H2O(l)
C)
2H+(aq) + 2OH–(aq) → 2H2O(l)
D)
2H+(aq) + SeO32–(aq) + 2K+(aq) + 2OH–(aq) → 2K+(aq) + SeO32–(aq) + 2H2O(l)
E)
H2SeO3(aq) + 2KOH(aq) → K2SeO3(aq) + 2H2O(l)
69. Which of the following salts may be obtained by the reaction of a weak acid with a strong
base?
A)
LiClO4
B)
NaCl
C)
K2SO3
D)
MgCl2
E)
NH4F
70. What is the net ionic equation for the complete neutralization of the triprotic acid citric acid,
H3C6H5O6, by a strong base?
A)
H3C6H5O6(aq) + 3OH–(aq) → 3H2O(l) + C6H5O63–(aq)
B)
H3C6H5O6(aq) + 3NaOH(aq) → 3H2O(l) + Na3C6H5O6(aq)
C)
H+(aq) + OH–(aq) → H2O(l)
D)
H3C6H5O6(aq) + NaOH(aq) → H2O(l) + NaH2C6H5O6(aq)
E)
3H+(aq) + 3OH–(aq) → 3H2O(l)
71. Which of the following salts cannot be obtained by the neutralization of a strong acid and a
strong base?
A)
NaCl
B)
LiNO3
C)
NH4Br
D)
Ba(ClO4)2
E)
Na2SO4
72. What is the net ionic equation for the complete neutralization of phosphoric acid with
potassium hydroxide?
A)
H3PO4(aq) + 3OH–(aq) → 3H2O(l) + PO43–(aq)
B)
H3P(aq) + 3KOH(aq) → 3H2O(l) + K3P(aq)
C)
H+(aq) + OH–(aq) → H2O(l)
D)
H3PO4(aq) + 3KOH(aq) → 3H2O(l) + K3PO4(aq)
E)
3H+(aq) + 3KOH(aq) → 3H2O(l) + 3K+(aq)
73. What is the net ionic equation for the neutralization of hydrofluoric acid with sodium
hydroxide?
A)
H+(aq) + NaOH(aq) → H2O(l) + Na+(aq)
B)
HF(aq) + OH–(aq) → H2O(l) + F–(aq)
C)
HF(aq) + NaOH(aq) → H2O(l) + NaF(aq)
D)
H+(aq) + OH–(aq) → H2O(l)
E)
HF(aq) + OH–(aq) → H2F+(aq) + O2–(aq)
74. What is the net ionic equation for the reaction of hydrobromic acid with sodium hydroxide?
A)
H+(aq) + OH–(aq) → H2O(l)
B)
H+(aq) + Br–(aq) + Na+(aq) + OH–(aq) → NaBr(aq) + H2O(l)
C)
H+(aq) + Br–(aq) + Na+(aq) + OH–(aq) → HBr(aq) + NaOH(aq)
D)
HBr(aq) + Na+(aq) + OH–(aq) → NaBr(aq) + H2O(l)
E)
HBr(aq) + NaOH(aq) → NaBr(aq) + H2O(l)