Ebook Chemistry An Atoms First Approach 2Nd Edition Zumdahl Test Bank Full Chapter PDF

Chemistry An Atoms First Approach
2nd Edition Zumdahl Test Bank

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Chapter 6 - Types of Chemical Reactions and Solution Stoichiometry
1. An unknown substance dissolves readily in water but not in benzene (a nonpolar solvent). Molecules of what
type are present in the substance?
a. Neither polar nor nonpolar
b. Polar
c. Either polar or nonpolar
d. Nonpolar
e. None of these
ANSWER: b
POINTS: 1
2. The interaction between solute particles and water molecules, which tends to cause a salt to fall apart in
water, is called _____.
a. hydration
b. polarization
c. dispersion
d. coagulation
e. conductivity
ANSWER: a
POINTS: 1
3. Consider two organic molecules, ethanol and benzene. One dissolves in water and the other does not. Why?
a. They have different molar masses.
b. One is ionic, the other is not.
c. One is an electrolyte, the other is not.
d. Ethanol contains a polar O–H bond, and benzene does not.
e. Two of these are correct.
ANSWER: d
POINTS: 1
4. Which of the following is a strong acid?

a. HF
b. KOH
c. HClO4
d. HClO
e. HBrO
ANSWER: c
POINTS: 1
5. All of the following are weak acids except _____.

a. HCNO
b. HBr
c. HF
Copyright Cengage Learning. Powered by Cognero. Page 1
d. HNO2
e. HCN
ANSWER: b
POINTS: 1
6. A solid acid HX is mixed with water. Two possible solutions can be obtained. Which of the following is true?
I. II.
a. In case I, HX is acting like a weak acid, and in case II, HX is acting like a strong acid.
b. In case I, HX is acting like a strong acid, and in case II, HX is acting like a weak acid.
c. In both cases, HX is acting like a strong acid.
d. In both cases, HX is acting like a weak acid.
e. HX is not soluble in water.
ANSWER: b
POINTS: 1
7. Which of the following is not a strong base?

a. Ca(OH)2
b. KOH
c. NH3
d. LiOH
e. Sr(OH)2
ANSWER: c
POINTS: 1
8. Which of the following is paired incorrectly?

a. H2SO4 – strong acid
b. HNO3 – weak acid
c. Ba(OH)2 – strong base
d. HCl – strong acid
e. NH3 – weak base
ANSWER: b
POINTS: 1
9. The man who discovered the essential nature of acids through solution conductivity studies is _____.
a. Priestly
b. Boyle
c. Einstein
d. Mendeleev
e. Arrhenius
ANSWER: e
POINTS: 1
10. A 17.1-g sample of HF is dissolved in water to give 2.0 × 102 mL of solution. The concentration of the
solution is:
a. 0.85 M.
b. 0.17 M.
c. 0.09 M.
d. 4.3 M.
e. 8.6 M.
ANSWER: d
POINTS: 1
11. Which of the following aqueous solutions contains the greatest number of ions?
a. 400.0 mL of 0.10 M NaCl
b. 300.0 mL of 0.10 M CaCl2
c. 200.0 mL of 0.10 M FeCl3
d. 200.0 mL of 0.10 M KBr
e. 800.0 mL of 0.10 M sucrose
ANSWER: b
POINTS: 1
12. What mass of calcium chloride, CaCl2, is needed to prepare 3.350 L of a 1.57 M solution?
a. 237 g
b. 5.26 g
c. 52.0 g
d. 111 g
e. 584 g
ANSWER: e
POINTS: 1
13. A 80.8-g sample of SrCl2 is dissolved in 112.5 mL of solution. Calculate the molarity of this solution.
a. 57.3 M
b. 4.53 M
c. 113.9 M
d. 0.718 M
e. none of these
ANSWER: b
POINTS: 1
14. What mass of solute is contained in 256 mL of a 0.831 M ammonium chloride solution?
a. 11.4 g
b. 174 g
c. 16.5 g
d. 213 g
e. 3.25 g
ANSWER: a
POINTS: 1
15. How many grams of NaOH are contained in 5.0 × 102 mL of a 0.83 M sodium hydroxide solution?
a. 17 g
b. 83 g
c. 0.42 g
d. 33 g
e. 415 g
ANSWER: a
POINTS: 1
16. You have two solutions of chemical A. To determine which has the highest concentration of A in molarity,
what is the minimum number of the following you must know?
I. the mass in grams of A in each solution
II. the molar mass of A
III. the volume of water added to each
solution
IV. the total volume of the solution
a. 0
b. 1
c. 2
d. 3
e. You must know all of them.
ANSWER: c
POINTS: 1
17. Diabetics often need injections of insulin to help maintain the proper blood glucose levels in their bodies.
How many moles of insulin are needed to make up 45 mL of 0.0066 M insulin solution?
a. 0.00059 mol
b. 0.15 mol
c. 6.8 mol
d. 0.30 mol
e. 0.00030 mol
ANSWER: e
POINTS: 1
18. You have two solutions of sodium chloride. One is a 2.00 M solution, the other is a 4.00 M solution. You
have much more of the 4.00 M solution and you add the solutions together. Which of the following could be the
concentration of the final solution?
a. 2.60 M
b. 3.00 M
c. 3.40 M
d. 6.00 M
e. 7.80 M
ANSWER: c
POINTS: 1
19. Which of the following do you need to know to be able to calculate the molarity of a salt solution?
I. the mass of salt added
II. the molar mass of the salt
III . the volume of water added
IV. the total volume of the solution
a. I, III
b. I, II, III
c. II, III
d. I, II, IV
e. You need all of the information.
ANSWER: d
POINTS: 1
20. Phosphoric acid, H3PO4, is a triprotic acid. What is the total number of moles of H+ available for reaction in
3.50 L of 0.500 M H3PO4?
a. 0.167 mole
b. 1.50 mole
c. 0.583 mole
d. 3.00 moles
e. 5.25 moles
ANSWER: e
POINTS: 1
21. How many grams of NaCl are contained in 350. mL of a 0.265 M solution of sodium chloride?
a. 15.5 g

b. 5.42 g
c. 10.84 g
d. 92.8 g
e. none of these
ANSWER: b
POINTS: 1
22. An analytical procedure requires a solution of chloride ions. How many grams of MgCl2 must be dissolved
to make 1.55 L of 0.0520 M Cl–?
a. 9.90 g
b. 0.313 g
c. 3.84 g
d. 2.48 g
e. 15.3 g
ANSWER: c
POINTS: 1
23. You have equal masses of different solutes dissolved in equal volumes of solution. Which of the solutes
would make the solution having the highest molar concentration?
a. NaOH
b. KCl
c. KOH
d. LiOH
e. all the same
ANSWER: d
POINTS: 1
24. What volume of 18 M sulfuric acid must be used to prepare 2.40 L of 0.175 M H2SO4?
a. 23 mL
b. 0.42 mL
c. 1.3 × 103 mL
d. 3.6 mL
e. 7.6 mL
ANSWER: a
POINTS: 1
25. 1.00 mL of a 2.80 × 10–4 M solution of oleic acid is diluted with 9.00 mL of petroleum ether, forming
solution A. Then 2.00 mL of solution A is diluted with 8.00 mL of petroleum ether, forming solution B. What is
the concentration of solution B?
a. 2.80 × 10–6 M
b. 7.78 × 10–6 M
c. 5.60 × 10–5 M
d. 6.22 × 10–5 M
e. 5.60 × 10–6 M
ANSWER: e
POINTS: 1
26. A 63.61-g sample of Ba(OH)2 is dissolved in enough water to make 1.900 liters of solution. How many mL
of this solution must be diluted with water in order to make 1.000 L of 0.100 M Ba(OH)2?
a. 512 mL
b. 195 mL
c. 19.5 mL
d. 3.71 mL
e. 269 mL
ANSWER: a
POINTS: 1
27. A 230.0-mL sample of a 0.275 M solution is left on a hot plate overnight; the following morning the
solution is 1.31 M. What volume of solvent has evaporated from the 0.275 M solution?
a. 48.3 mL
b. 63.3 mL
c. 181.7 mL
d. 230. mL
e. 278.3 mL
ANSWER: c
POINTS: 1
28. 1.00 mL of a 3.40 × 10–4 M solution of oleic acid is diluted with 9.00 mL of petroleum ether, forming
solution A. Then 2.00 mL of solution A is diluted with 8.00 mL of petroleum ether, forming solution B. How
many grams of oleic acid are 5.00 mL of solution B? (Molar mass for oleic acid = 282 g/mol)
a. 4.79 × 10–6 g
b. 1.33 × 10–5 g
c. 1.92 × 10–2 g
d. 9.59 × 10–6 g
e. 4.79 × 10–4 g
ANSWER: d
POINTS: 1
29. For the reaction 4FeCl2(aq) + 3O2(g) → 2Fe2O3(s) + 4Cl2(g), what volume of a 0.620 M solution of FeCl2
is required to react completely with 8.12 × 1021 molecules of O2?
a. 6.45 × 103 mL
b. 11.1 mL
c. 16.3 mL
d. 29.0 mL
e. 6.27 mL
ANSWER: d
POINTS: 1
30. The following reactions:

Pb2+ + 2I– → PbI2
2Ce4+ + 2I– → I2 + 2Ce3+
HOAc + NH3 → NH4+ + OAc–
are examples of
a. acid-base reactions
b. unbalanced reactions
c. precipitation, acid-base, and redox reactions, respectively
d. redox, acid-base, and precipitation reactions, respectively
e. precipitation, redox, and acid-base reactions, respectively
ANSWER: e
POINTS: 1
31. The following reactions

2K(s) + Br2(l) → 2KBr(s)
AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq)
HCl(aq) + KOH(aq) → H2O(l) + KCl(aq)
are examples of
a. precipitation reactions
b. redox, precipitation, and acid-base, respectively
c. precipitation (two) and acid-base reactions, respectively
d. redox reactions
e. none of these
ANSWER: b
POINTS: 1
32. The following reactions

ZnBr2(aq) + 2AgNO3(aq) → Zn(NO3)2(aq) + 2AgBr(s)
KBr(aq) + AgNO3(aq) → AgBr(s) + KNO3(aq)
are examples of
a. oxidation-reduction reactions
b. acid-base reactions
c. precipitation reactions
d. A and C
e. none of these

ANSWER: c
POINTS: 1
33. All of the following reactions

2Al(s) + 3Br2(l) → 2AlBr3(s)
2Ag2O(s) → 4Ag(s) + O2(g)
CH4(l) + 2O2(g) → CO2(g) + 2H2O(g)
can be classified as
a. oxidation-reduction reactions
b. combustion reactions
c. precipitation reactions
d. A and B
e. A and C
ANSWER: a
POINTS: 1
34. Aqueous solutions of sodium sulfide and copper(II) chloride are mixed together. Which statement is
correct?
a. Both NaCl and CuS precipitate from solution.
b. No reaction will occur.
c. CuS will precipitate from solution.
d. NaCl will precipitate from solution.
e. A gas is released.
ANSWER: c
POINTS: 1
35. Aqueous solutions of potassium sulfate and ammonium nitrate are mixed together. Which statement is
correct?
a. Both KNO3 and NH4SO4 precipitate from solution.
b. A gas is released.
c. NH4SO4 will precipitate from solution.
d. KNO3 will precipitate from solution.
e. No reaction will occur.
ANSWER: e
POINTS: 1
36. Which of the following salts is insoluble in water?

a. Na2S
b. K2CO3
c. Pb(NO3)2
d. CaCl2
e. All of these are soluble in water.
ANSWER: e
POINTS: 1
37. How many of the following salts are expected to be insoluble in water?
sodium sulfide barium nitrate
ammonium sulfate potassium phosphate
a. none
b. 1
c. 2
d. 3
e. 4
ANSWER: a
POINTS: 1
38. Which of the following ions is most likely to form an insoluble sulfate?
a. K+
b. Li+
c. Ca2+
d. S2–
e. Cl–
ANSWER: c
POINTS: 1
39. Which of the following compounds is soluble in water?

a. Ni(OH)2
b. K3PO4
c. BaSO4
d. CoCO3
e. PbCl2
ANSWER: b
POINTS: 1
40. Which pair of ions would not be expected to form a precipitate when dilute solutions of each are mixed?
a. Al3+, S2–
b. Pb2+, Cl–
c. Ba2+, PO43–
d. Pb2+, OH–
e. Mg2+, SO42–
ANSWER: e
POINTS: 1
41. Consider an aqueous solution of calcium nitrate added to an aqueous solution of sodium phosphate. What is
the formula of the solid formed in the reaction?
a. Ca(PO4)2
b. CaPO4
c. Ca3(PO4)2
d. Ca3(PO3)2
e. none of these
ANSWER: c
POINTS: 1
42. You have exposed electrodes of a light bulb in a solution of H2SO4 such that the light bulb is on. You add a
dilute solution and the bulb grows dim. Which of the following could be in the solution?
a. Ba(OH)2
b. NaNO3
c. K2SO4
d. Cu(NO3)2
e. none of these
ANSWER: a
POINTS: 1
43. When NH3(aq) is added to Cu2+(aq), a precipitate initially forms. Its formula is _____.
a. Cu(NH)3
b. Cu(NO3)2
c. Cu(OH)2
d. Cu(NH3)22+
e. CuO
ANSWER: c
POINTS: 1
44. A solution contains the ions Ag+, Pb2+, and Ni2+. Dilute solutions of NaCl, Na2SO4, and Na2S are available
to separate the positive ions from each other. In order to effect separation, the solutions should be added in
which order?
a. Na2SO4, NaCl, Na2S
b. Na2SO4, Na2S, NaCl
c. Na2S, NaCl, Na2SO4
d. NaCl, Na2S, Na2SO4
e. NaCl, Na2SO4, Na2S
ANSWER: a
POINTS: 1
45. When sodium chloride and lead(II) nitrate react in an aqueous solution, which of the following terms will be
present in the balanced molecular equation?
a. PbCl(s)
b. Pb2Cl(s)
c. NaNO3(aq)
d. 2NaNO3(aq)
e. 2PbCl2(s)
ANSWER: d
POINTS: 1
46. When solutions of phosphoric acid and iron(III) nitrate react, which of the following terms will be present in
the balanced molecular equation?
a. HNO3(aq)
b. 3HNO3(aq)
c. 2FePO4(s)
d. 3FePO4(s)
e. 2HNO3(aq)
ANSWER: b
POINTS: 1
47. Consider an aqueous solution of calcium nitrate added to an aqueous solution of sodium phosphate. Write
and balance the equation for this reaction to answer the following question. What is the sum of the coefficients
when the molecular equation is balanced in standard form?
a. 4
b. 5
c. 7
d. 11
e. 12
ANSWER: e
POINTS: 1
48. Aqueous solutions of barium chloride and silver nitrate are mixed to form solid silver chloride and aqueous
barium nitrate.
The balanced molecular equation contains which one of the following terms?
Reference: Ref 10-1
a. AgCl (s)
b. 2AgCl (s)
c. 2Ba(NO3)2 (aq)
d. BaNO3 (aq)

e. 3AgCl (aq)
ANSWER: b
POINTS: 1
barium nitrate.
The balanced complete ionic equation contains which of the following terms?
Reference: Ref 10-1
a. 2Ba2+(aq)
b. Cl–(aq)
c. 2Ag+(aq)
d. NO3– (aq)
e. AgCl(aq)
ANSWER: c
POINTS: 1
barium nitrate.
The net ionic equation contains which of the following terms?
Reference: Ref 10-1
a. Ag+(aq)
b. Ba2+(aq)
c. NO3– (aq)
d. H+ (aq)
e. AgCl(aq)
ANSWER: a
POINTS: 1
51. In writing the complete ionic equation for the reaction (if any) that occurs when aqueous solutions of KOH
and Mg(NO3)2 are mixed, which of the following would not be written as ionic species?
a. KOH
b. Mg(NO3)2
c. Mg(OH)2
d. KNO3
e. All of the above would be written as ionic species.
ANSWER: c
POINTS: 1
52. The net ionic equation for the reaction of calcium bromide and sodium phosphate contains which of the
following species?
a. 2Br–(aq)
b. PO43–(aq)
c. 2Ca3(PO4)2(s)
d. 6NaBr(aq)
e. 3Ca2+(aq)
ANSWER: e
POINTS: 1
53. When solutions of cobalt(II) chloride and carbonic acid react, which of the following terms will be present
in the net ionic equation?
a. CoCO3(s)
b. H+(aq)
c. 2CoCO3(s)
d. 2Cl–(aq)
e. two of these
ANSWER: a
POINTS: 1
54. When solutions of strontium chloride and sodium sulfate react, which of the following is a spectator ion?
a. Strontium ion
b. Chloride ion
c. Sodium ion
d. Sulfate ion
e. Two of these
ANSWER: e
POINTS: 1
55. The net ionic equation for the reaction of aluminum sulfate and sodium hydroxide contains which of the
following species?
a. 3Al3+(aq)
b. OH–(aq)
c. 3OH–(aq)
d. 2Al3+(aq)
e. 2Al(OH)3(s)
ANSWER: c
POINTS: 1
56. You have 71.5 mL of a 2.50 M solution of Na2CrO4(aq). You also have 125 mL of a 2.50 M solution of
AgNO3(aq). Calculate the concentration of Na+ after the two solutions are mixed together.
a. 0.00 M

b. 0.91 M
c. 1.82 M
d. 5.00 M
e. 0.358 M
ANSWER: c
POINTS: 1
AgNO3(aq). Calculate the concentration of NO3– after the two solutions are mixed together.
a. 0.00 M
b. 0.706 M
c. 1.41 M
d. 2.82 M
e. 4.50 M
ANSWER: c
POINTS: 1
58. Consider the reaction between 15.0 mL of a 1.00 M aqueous solution of AgNO3 and 10.0 mL of a 1.00 M
aqueous solution of K2CrO4. When these react, a precipitate is observed. What is present in solution after the
reaction is complete? Note: the solid is not considered to be in solution.
a. Ag+, NO3–, K+, CrO42–, water
b. Ag+, NO3–, K+, water
c. K+, CrO42–, water
d. NO3–, K+, CrO42–, water
e. water
ANSWER: d
POINTS: 1
59. You mix 55 mL of 1.00 M silver nitrate with 25 mL of 1.17 M sodium chloride. What mass of silver
chloride should you form?
a. 4.2 g
b. 8.4 g
c. 4.6 g
d. 9.2
e. none of these
ANSWER: a
POINTS: 1
60. You mix 280.0 mL of 1.20 M lead(II) nitrate with 300.0 mL of 1.80 M potassium iodide. The lead(II) iodide
is insoluble. Which of the following is false?
a. The final concentration of Pb2+ ions is 0.114 M.

b. You form 124 g of lead(II) iodide.
c. The final concentration of K+ is 0.931 M.
d. The final concentration of NO3– is 0.931 M.
e. All are true.
ANSWER: d
POINTS: 1
AgNO3(aq). Calculate the concentration of CrO42– after the two solutions are mixed together.
a. 0.00 M
b. 0.281 M
c. 0.938 M
d. 0.263 M
e. 2.50 M
ANSWER: b
POINTS: 1
AgNO3(aq). Calculate the concentration of Ag+ after the two solutions are mixed together.
a. 0.00 M
b. 0.509 M
c. 1.02 M
d. 0.088 M
e. 0.204 M
ANSWER: a
POINTS: 1
63. If all of the chloride in a 4.519-g sample of an unknown metal chloride is precipitated as AgCl with 70.90
mL of 0.2010 M AgNO3, what is the percentage of chloride in the sample?
a. 50.52%
b. 11.18%
c. 1.425%
d. 8.945%
e. none of the above
ANSWER: b
POINTS: 1
64. A mixture of BaCl2 and NaCl is analyzed by precipitating all the barium as BaSO4. After addition of an
excess of Na2SO4 to a 3.831-g sample of the mixture, the mass of precipitate collected is 2.826 g. What is the
mass percentage of barium chloride in the mixture?
a. 82.70%
b. 73.77%
c. 43.39%
d. 65.80%
e. 13.61%
ANSWER: d
POINTS: 1
65. A 3.00-g sample of an alloy (containing only Pb and Sn) was dissolved in nitric acid (HNO3). Sulfuric acid
was added to this solution, which precipitated 2.90 g of PbSO4. Assuming that all of the lead was precipitated,
what is the percentage of Sn in the sample? (molar mass of PbSO4 = 303.3 g/mol)
a. 34.0% Sn
b. 0.956% Sn
c. 96.7% Sn
d. 66.0% Sn
e. 1.98% Sn
ANSWER: a
POINTS: 1
66. A mixture contained no fluorine compound except methyl fluoroacetate, FCH2COOCH3 (molar mass =
92.07 g/mol). When chemically treated, all the fluorine was converted to CaF2 (molar mass = 78.08 g/mol). The
mass of CaF2 obtained was 39.8 g. Find the mass of methyl fluoroacetate in the original mixture.
a. 67.5 g
b. 93.9 g
c. 33.8 g
d. 46.9 g
e. 23.5 g
ANSWER: b
POINTS: 1
67. A 1.75-g sample of a metal chloride, MCl2, is dissolved in water and treated with excess aqueous silver
nitrate. The silver chloride that formed weighed 3.73 g. Calculate the molar mass of M.
a. 70.9 g/mol
b. 32 g/mol
c. 63.5 g/mol
d. 67 g/mol
e. 72.4 g/mol
ANSWER: c
POINTS: 1
68. In the balanced molecular equation for the neutralization of sodium hydroxide with sulfuric acid, the
products are _____.
a. NaSO4 + H2O
b. NaSO3 + 2H2O
c. 2NaSO4 + H2O
d. Na2S + 2H2O
e. Na2SO4 + 2H2O
ANSWER: e
POINTS: 1
69. You have separate solutions of HCl and H2SO4 with the same concentrations in terms of molarity. You wish
to neutralize a solution of NaOH. Which acid solution would require more volume (in mL) to neutralize the
base?
a. The HCl solution.
b. The H2SO4 solution.
c. You need to know the acid concentrations to answer this question.
d. You need to know the volume and concentration of the NaOH solution to answer this question.
e. C and D
ANSWER: a
POINTS: 1
70. What mass of NaOH is required to react exactly with 25.0 mL of 2.8 M H2SO4?
a. 2.8 g
b. 0.7 g
c. 5.6 g
d. 140 g
e. none of these
ANSWER: c
POINTS: 1
71. With what volume of 5.00 M HF will 5.15 g of calcium hydroxide react completely, according to the
following reaction?
a. 13.9 mL
b. 139 mL
c. 695 mL
d. 27.8 mL
e. 36.0 mL
ANSWER: d
POINTS: 1
72. When solutions of carbonic acid and potassium hydroxide react, which of the following are NOT present in
the complete ionic equation?
a. Hydrogen ion
b. Carbonate ion
c. Potassium ion
d. Hydroxide ion
e. Water
ANSWER: a
POINTS: 1
73. When solutions of formic acid and potassium hydroxide react, which of the following are NOT present in
the net ionic equation?
I. hydrogen ion
II. formate ion
III. potassium ion
IV. hydroxide ion
a. I and II
b. I, II, and III
c. I and IV
d. I and III
e. II and III
ANSWER: d
POINTS: 1
74. When solutions of formic acid and copper(II) hydroxide react, which of the following are spectator ions?
a. hydrogen ion
b. formate ion
c. copper(II) ion
d. hydroxide ion
e. none of these
ANSWER: e
POINTS: 1
75. When solutions of formic acid and magnesium hydroxide react, which of the following are NOT present in
the net ionic equation?
I. hydrogen ion
II. formate ion
III. magnesium ion
IV. hydroxide ion
a. I and II
b. I, II, and III
c. I and IV
d. I and III
e. II and III
ANSWER: c
POINTS: 1
76. Sulfamic acid, HSO3NH2 (molar mass = 97.1 g/mol), is a strong monoprotic acid that can be used to
standardize a strong base:
A 0.169-g sample of HSO3NH2 required 19.4 mL of an aqueous solution of KOH for a complete reaction. What
is the molarity of the KOH solution?
a. 0.00174 M
b. 8.97 M
c. 0.0897 M
d. 0.0338 M
e. none of these
ANSWER: c
POINTS: 1
77. A student weighs out 0.559 g of KHP (molar mass = 204.22 g/mol) and titrates to the equivalence point with
36.78 mL of a stock NaOH solution. What is the concentration of the stock NaOH solution? KHP is an acid
with one acidic proton.
a. 0.00274 M
b. 0.101 M
c. 0.0152 M
d. 0.0744 M
e. none of these
ANSWER: d
POINTS: 1
78. A 0.307-g sample of an unknown triprotic acid is titrated to the third equivalence point using 35.2 mL of
0.106 M NaOH. Calculate the molar mass of the acid.
a. 247 g/mol
b. 171 g/mol
c. 165 g/mol
d. 151 g/mol
e. 82.7 g/mol
ANSWER: a
POINTS: 1
79. An unknown diprotic acid requires 30.31 mL of 0.107 M NaOH to completely neutralize a 0.780-g sample.
Calculate the approximate molar mass of the acid.
a. 617 g/mol
b. 481 g/mol
c. 241 g/mol
d. 120 g/mol
e. 308 g/mol
ANSWER: b
POINTS: 1
80. In which of the following does nitrogen have an oxidation state of +4?
a. HNO3
b. NO2
c. N2O
d. NH4Cl
e. NaNO2
ANSWER: b
POINTS: 1
81. The oxidation state of iodine in IO3– is _____.

a. 0
b. +3
c. –3
d. +5
e. –5
ANSWER: d
POINTS: 1
82. The oxidation state of chlorine in ClO2– is _____.

a. 0
b. +3
c. -3
d. +5
e. -5
ANSWER: b
POINTS: 1
83. Which of the following statements is not true?

a. When a metal reacts with a nonmetal, an ionic compound is formed.
b. A metal-nonmetal reaction can always be assumed to be an oxidation-reduction reaction.
c. Two nonmetals can undergo an oxidation-reduction reaction.
d. When two nonmetals react, the compound formed is ionic.
e. A metal-nonmetal reaction involves electron transfer.
ANSWER: d
POINTS: 1
84. In the reaction 2Ca(s) + O2(g) → 2CaO(s), which species is oxidized?

a. O2
b. O2–
c. Ca
d. Ca2+
e. none of these
ANSWER: c
POINTS: 1
85. In the reaction 2Cs(s) + Cl2(g) → 2CsCl(s), Cl2 is:

a. the reducing agent.
b. the oxidizing agent.
c. oxidized.
d. the electron donor.
e. two of these.
ANSWER: b
POINTS: 1
86. In the reaction N2(g) + 3H2(g) → 2NH3(g), N2 is:

a. oxidized.
b. reduced.
c. the electron donor.
d. the reducing agent.
e. two of these.
ANSWER: b
POINTS: 1
87. In the reaction P4(s) + 10Cl2(g) → 4PCl5(s), the reducing agent is:
a. chlorine.
b. PCl5.
c. phosphorus.
d. Cl–.
e. none of these.
ANSWER: c
POINTS: 1
88. In the reaction C(s) + O2(g) → CO2(g) carbon is __________.

a. the reducing agent
b. the electron acceptor
c. reduced
d. the oxidizing agent
e. more than one of these
ANSWER: a
POINTS: 1
89. Which of the following reactions does not involve oxidation-reduction?

a. CH4 + 3O2 → 2H2O + CO2
b. Zn + 2HCl → ZnCl2 + H2
c. 2Na + 2H2O → 2NaOH + H2
d. MnO2 + 4HCl → Cl2 + 2H2O + MnCl2
e. All are oxidation-reduction reactions.
ANSWER: e
POINTS: 1
90. Which of the following are oxidation-reduction reactions?

I. PCl3 + Cl2 → PCl5
II. Cu + 2AgNO3 → Cu(NO3)2 + 2Ag
III. CO2 + 2LiOH → Li2CO3 + H2O
IV. FeCl2 + 2NaOH → Fe(OH)2 + 2NaCl
a. III
b. IV
c. I and II
d. I, II, and III
e. I, II, III, and IV
ANSWER: c
POINTS: 1
91. Which of the following statements is(are) true? Oxidation and reduction:
a. cannot occur independently of each other.
b. accompany all chemical changes.
c. describe the loss and gain of electron(s), respectively.
d. result in a change in the oxidation states of the species involved.
e. A, C, and D.
ANSWER: e
POINTS: 1

92. In the reaction Zn + H2SO4 → ZnSO4 + H2, which, if any, element is oxidized?
a. Zinc
b. Hydrogen
c. Sulfur
d. Oxygen
e. None of these
ANSWER: a
POINTS: 1
93. In the following reaction, which species is oxidized?

8NaI + 5H2SO4 → 4I2 + H2S + 4Na2SO4 + 4H2O
a. Sodium
b. Iodine
c. Sulfur
d. Hydrogen
e. Oxygen
ANSWER: b
POINTS: 1
94. How many of the following are oxidation-reduction reactions?

NaOH + HCl → NaCl + H2O
Cu + 2AgNO3 → 2Ag + Cu(NO3)2
Mg(OH)2 → MgO + H2O
N2 + 3H2 → 2NH3
a. 0
b. 1
c. 2
d. 3
e. 4
ANSWER: c
POINTS: 1
95. In the reaction shown below, what species is oxidized?

2NaI + Br2 → 2NaBr + I2
a. Na+
b. I–
c. Br2
d. Br–
e. I2
ANSWER: b
POINTS: 1
96. Given the reaction:

2MnO4– + 5H2O2 + 6H+ → 2Mn2+ + 8H2O + 5O2
determine the number of electrons involved in this reaction.
a. 10
b. 8
c. 6
d. 4
e. 2
ANSWER: a
POINTS: 1
97. Balance the following oxidation-reduction reaction using the oxidation number method:
Fe3+ + I– → Fe2+ + I2
In the balanced equation, the coefficient of Fe2+ is:
a. 1.
b. 2.
c. 3.
d. 4.
e. none of these.
ANSWER: b
POINTS: 1
98. Balance the following oxidation-reduction reaction using the oxidation number method:
Fe + Cl2 → Fe3+ + Cl–
In the balanced equation, the coefficient of Cl– is:
a. 2.
b. 3.
c. 4.
d. 6.
e. none of these.
ANSWER: d
POINTS: 1
99. Consider the following unbalanced oxidation-reduction reaction:

Fe + Cl2 → Fe2+ + Cl–
In the balanced equation, the number of electrons transferred is:
a. 1.
b. 6.
c. 2.
d. 4.
e. none of these.
ANSWER: c
POINTS: 1
100. The MnO4– is often used to analyze for the Fe2+ content of an aqueous solution via the reaction
MnO4–(aq) + Fe2+(aq) + H+(aq) → Fe3+(aq) + Mn2+(aq) + H2O(l)
What is the ratio of Fe2+ : MnO4– in the balanced equation?
a. 1 : 1
b. 2 : 1
c. 3 : 1
d. 4 : 1
e. 5 : 1
ANSWER: e
POINTS: 1
101. Polar molecules have an unequal distribution of charge within the molecule.
a. True
b. False
ANSWER: True
POINTS: 1
102. An acid is a substance that produces OH– ions in water.

a. True
b. False
ANSWER: False
POINTS: 1
103. The concentration of a salt water solution that sits in an open beaker decreases over time.
a. True
b. False
ANSWER: False
POINTS: 1
104. The filtrate is the solid formed when two solutions are mixed.
a. True
b. False
ANSWER: False
POINTS: 1
105. A chemical that changes color at the endpoint of a reaction is called a colorimeter.
a. True
b. False
ANSWER: False
POINTS: 1
106. Oxidation is the gain of electrons.

a. True
b. False
ANSWER: False
POINTS: 1
107. A reducing agent is an electron donor.

a. True
b. False
ANSWER: True
POINTS: 1
108. A molecule with an unequal charge distribution is said to be a __________ molecule.
ANSWER: polar
POINTS: 1
109. Soluble ionic compounds containing the hydroxide ion are called strong __________.
ANSWER: bases
POINTS: 1
110. A __________ is a substance dissolved in a liquid to make a solution.
ANSWER: solute
POINTS: 1
111. A __________ electrolyte dissociates to a great extent in an aqueous solution.
ANSWER: strong
POINTS: 1
112. Molarity is defined as __________ of solute per volume of solution in ___________.
ANSWER: moles, liters

POINTS: 1
113. Selecting from the following reagents, indicate which reagents would be mixed to give the compounds
described.
CuSO4(aq) Fe2(CO3)3(s) NH3(aq)
CuCO3(s) FeCl3(aq) Na2SO4(aq)
Cr(OH)3(s) H2SO4(aq)

Cu(OH)2(s)
Reference: Ref 10-2
ANSWER: CuSO4(aq) and NH3(aq)

POINTS: 1
114. Selecting from the following reagents, indicate which reagents would be mixed to give the compounds
described.
CuSO4(aq) Fe2(CO3)3(s) NH3(aq)
CuCO3(s) FeCl3(aq) Na2SO4(aq)
Cr(OH)3(s) H2SO4(aq)
FeCl3(aq) + Na2SO4(aq)
Reference: Ref 10-2
ANSWER: FeCl3(aq) + Na2SO4(aq)
POINTS: 1
115. Write balanced equations for each of the processes, choosing from the following substances as reactants:
BaCl2 O2 H2SO4 HNO3
C2H5OH H2O Ca(OH)2 K
Na2CrO4 KOH Pb(NO3)2
Precipitation of BaSO4 from solution
Reference: Ref 10-3
ANSWER: H2SO4 + BaCl2 → BaSO4 + 2HCl

POINTS: 1
BaCl2 O2 H2SO4 HNO3
Neutralization of sulfuric acid
Reference: Ref 10-3
ANSWER: H2SO4 + 2KOH → K2SO4 + 2H2O or H2SO4 + Ca(OH)2 → CaSO4 + 2H2O

POINTS: 1
BaCl2 O2 H2SO4 HNO3

Combustion reaction
Reference: Ref 10-3
ANSWER: C2H5OH + 3O2 → 2CO2 + 3H2O

POINTS: 1
BaCl2 O2 H2SO4 HNO3
Dissolution of calcium hydroxide with another reagent
Reference: Ref 10-3
ANSWER: Ca(OH)2 + 2HNO3 → Ca(NO3)2 + 2H2O

POINTS: 1
BaCl2 O2 H2SO4 HNO3
Formation of hydrogen gas
Reference: Ref 10-3
ANSWER: 2K + H2O → 2KOH + H2

POINTS: 1
120. Balance the following equation: KI + HNO3 → KNO3 + NO + I2 + H2O

ANSWER: 6KI + 8HNO3 → 6KNO3 + 2NO + 3I2 + 4H2O
POINTS: 1
121. Balance the following equation: C3H5(NO3)3 → N2 + CO2 + H2O + O2
ANSWER: 4C3H5(NO3)3 → 6N2 + 12CO2 + 10H2O + O2

POINTS: 1

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Chemistry An Atoms First Approach

2nd Edition Zumdahl Test Bank

4. Which of the following is a strong acid?

5. All of the following are weak acids except _____.

7. Which of the following is not a strong base?

8. Which of the following is paired incorrectly?

Copyright Cengage Learning. Powered by Cognero. Page 5

30. The following reactions:

31. The following reactions

32. The following reactions

Copyright Cengage Learning. Powered by Cognero. Page 8

33. All of the following reactions

36. Which of the following salts is insoluble in water?

39. Which of the following compounds is soluble in water?

Copyright Cengage Learning. Powered by Cognero. Page 12

Copyright Cengage Learning. Powered by Cognero. Page 14

Copyright Cengage Learning. Powered by Cognero. Page 15

81. The oxidation state of iodine in IO3– is _____.

82. The oxidation state of chlorine in ClO2– is _____.

83. Which of the following statements is not true?

84. In the reaction 2Ca(s) + O2(g) → 2CaO(s), which species is oxidized?

85. In the reaction 2Cs(s) + Cl2(g) → 2CsCl(s), Cl2 is:

86. In the reaction N2(g) + 3H2(g) → 2NH3(g), N2 is:

88. In the reaction C(s) + O2(g) → CO2(g) carbon is __________.

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89. Which of the following reactions does not involve oxidation-reduction?

90. Which of the following are oxidation-reduction reactions?

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93. In the following reaction, which species is oxidized?

94. How many of the following are oxidation-reduction reactions?

95. In the reaction shown below, what species is oxidized?

96. Given the reaction:

99. Consider the following unbalanced oxidation-reduction reaction:

102. An acid is a substance that produces OH– ions in water.

106. Oxidation is the gain of electrons.

107. A reducing agent is an electron donor.

108. A molecule with an unequal charge distribution is said to be a __________ molecule.

110. A __________ is a substance dissolved in a liquid to make a solution.

111. A __________ electrolyte dissociates to a great extent in an aqueous solution.

112. Molarity is defined as __________ of solute per volume of solution in ___________.

ANSWER: moles, liters

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ANSWER: CuSO4(aq) and NH3(aq)

ANSWER: FeCl3(aq) + Na2SO4(aq)

ANSWER: H2SO4 + BaCl2 → BaSO4 + 2HCl

ANSWER: H2SO4 + 2KOH → K2SO4 + 2H2O or H2SO4 + Ca(OH)2 → CaSO4 + 2H2O

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ANSWER: C2H5OH + 3O2 → 2CO2 + 3H2O

ANSWER: Ca(OH)2 + 2HNO3 → Ca(NO3)2 + 2H2O

ANSWER: 2K + H2O → 2KOH + H2

120. Balance the following equation: KI + HNO3 → KNO3 + NO + I2 + H2O

121. Balance the following equation: C3H5(NO3)3 → N2 + CO2 + H2O + O2

ANSWER: 4C3H5(NO3)3 → 6N2 + 12CO2 + 10H2O + O2

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112. Molarity is defined as of solute per volume of solution in _.