Ch 4 – Practice Problems
1.
T
F True or False? Nonelectrolytes are insoluble in water.
2.
A 12.0-g sample of HF is dissolved in water to give 3.1  102 mL of solution. The concentration of the solution is
A) 3.9 M
B) 3.7 M
C) 0.19 M
D) 1.9 M
E)
0.60 M
3.
The concentration of a 293.0-mL sample of a calcium chloride solution is 0.422 M. What is the mass of the solute?
A) 9.34 g
B) 13.72 g
C) 160 g
D) 46.8 g
E)
2.64 g
4.
What volume of 2.0 M HCl can be prepared from 2.00 L of 9.00 M HCl?
A) 444 mL
B) 2.25 L
C) 4.50 L
D) 9.00 L
E)
none of these
5.
How much water must be added to 20.0 mL of a 9.50 M sulfuric acid solution to make a 0.480 M solution? (Assume volumes
are additive.)
A) 81.0 mL
B) 101 mL
C) 376 mL
D) 396 mL
E)
none of these
6.
What volume of 12.0 M HCl is required to prepare 16.0 L of 0.250 M hydrochloric acid?
A) 130. mL
B) 333 mL
C) 585 mL
D) 768 mL
E)
none of these
7.
To calculate the concentration in molarity of a salt solution, you need to know
A) the mass of the salt added to the solution and the volume of water added to the solution.
B) the mass of the salt added to the solution and the total volume of the solution.
C) the mass of the salt added, the molar mass of the salt, and the total volume of the solution.
D) the molar mass of the salt and the total volume of the solution.
E)
the mass of the salt added, the molar mass of the salt, the volume of water added, and the total volume of the solution.
8.
Which of the following solutions contains the greatest total ion concentration?
A) One mole of potassium chloride dissolved in 1.0 L of solution.
B) One mole of iron(II) nitrate dissolved in 1.0 L of solution.
C) One mole of potassium hydroxide dissolved in 1.0 L of solution.
D) One mole of sodium phosphate dissolved in 1.0 L of solution.
E)
At least two of these solutions have an equal number of ions, and these contain the greatest total ion concentration.
9.
What volume of 0.450 M barium nitrate solution is needed to prepare 261.0 mL of a solution that is 0.272 M in nitrate?
A) 1.58  102 mL
B) 7.89  101 mL
C) 3.16  102 mL
D) 5.26  101 mL
E)
4.32  102 mL
10.
What volume of 5.50 M potassium hydroxide is required to prepare 46.0 mL of 0.295 M KOH?
A) 2.47 mL
B) 0.0353 mL
C) 0.76 mL
D) 858 mL
E)
4.51 mL
11.
A 230.-mL sample of a 0.275 M solution is left on a hot plate overnight; the following morning the solution is 1.10 M. What
volume of solvent has evaporated from the 0.275 M solution? (Assume volumes are additive.)
A) 58.0 mL
B) 63.3 mL
C) 172 mL
D) 230. mL
E)
288 mL
12.
If a student needs to make a 0.10 M solution of NaHCO3, how many milliliters of solution can be made using a 0.35-g sample of
NaHCO3?
A) 3.5 mL
B) 4.2 mL
C) 35 mL
D) 42 mL
E)
1.0  102 mL
13.
How many grams of Na2SO4 are required to make 150.0 mL of a 0.180 M sodium sulfate solution?
A) 2.78 g
B) 3.21 g
C) 3.40 g
D) 3.84 g
E)
none of these
14.
Consider five solutions that all have the same mass of solute in 100.0 mL of solution. Which has the highest concentration as
measured in molarity?
A) KCl
B) NaCl
C) Na2SO4
D) NaF
E)
CaCl2
15.
A 6.54-g sample consisting of a mixture of silver nitrate and sodium nitrate is dissolved in water. This aqueous mixture then
reacts with aqueous barium chloride to form 3.50 g of silver chloride. Calculate the percent by mass of silver nitrate in the first
mixture.
A) 41.5%
B) 45.2%
C) 77.7%
D) 63.4%
E)
43.7%
16.
You dissolve 15.71 g of NH4NO3 in 150.0 mL of solution (call this solution A). You take 20.0 mL of solution A and add water
until the total volume is 75.0 mL (call this solution B). You take 15.0 mL of solution B and add 25.0 mL of water to it (call this
solution C). You mix 10.0 mL of solution B and 10.0 mL of solution C (call this solution D). What is the concentration of
ammonium nitrate in solution D?
A) 0.190 M
B) 0.279 M
C) 0.131 M
D) 0.240 M
E)
none of these
17.
1.00 mL of a 3.50  10–4 M solution of oleic acid is diluted with 9.00 mL of petroleum ether, forming solution A. 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 in 5.00 mL of
solution B? (molar mass for oleic acid = 282 g/mol)
A) 4.94  10–4 g
B) 7.00  10–6 g
C) 4.94  10–5 g
D) 1.97  10–6 g
E)
9.87  10–6 g
18.
Mixing 40.0 mL of a 4.00 M sodium chloride solution with 20.0 mL of a 5.00 M calcium chloride solution results in a solution
with a chloride ion concentration of
A) 4.33 M.
B) 4.50 M.
C)
D)
E)
6.00 M.
7.00 M.
none of these
19.
You have 130.0 mL of a 0.240 M solution of NaCl sitting in a beaker. After several days you test the solution and find that it
has a concentration of 0.410 M. How much water must have evaporated? (Assume volumes are additive.)
A) 76.1 mL
B) 53.9 mL
C) 206 mL
D) 130. mL
E)
129 mL
20.
A 51.24-g sample of Ba(OH)2 is dissolved in enough water to make 1.20 L of solution. How many milliliters of this solution
must be diluted with water in order to make 1.00 L of 0.100 molar Ba(OH) 2?
A) 400. mL
B) 333 mL
C) 278 mL
D) 1.20  103 mL
E)
249 mL
21.
You dissolve a 1.28-g sample of NaCl in a total volume of 125.0 mL of solution. Your lab partner has 1.50 M aqueous NaCl
and wants to make a solution with the same concentration and volume as yours. How much of the solution does your lab partner
need to use?
A) 1.83 mL
B) 14.6 mL
C) 107 mL
D) 125 mL
E)
none of these
22.
Consider the reaction between 50.0 mL of 0.200 M sodium hydroxide and 75.0 mL of 0.100 M HCl. Which of the following
statements is correct?
A) After the reaction, the concentration of Na+ is greater than the concentration of OH-.
B) The NaOH is the limiting reactant.
C) After the reaction, the concentration of Na+ is equal to the concentration of Cl-.
D) After the reaction, the concentration of Na+ is still 0.200 M because Na+ is a spectator ion.
E)
None of these are correct.
23.
High concentrations of aqueous solutions of potassium hydroxide and copper(II) nitrate are mixed together. Which statement is
correct?
A) Both KNO3 and Cu(OH)2 precipitate from solution.
B) No precipitate forms.
C) Cu(OH)2 will precipitate from solution.
D) KNO3 will precipitate from solution.
E)
No reaction will occur.
24.
Which pair of ions would not be expected to form a precipitate when dilute solutions of each are mixed?
A) Cu2+, S2–
B) Ag+, Cl–
C) Ca2+, PO43–
D) Mn2+, OH–
E)
Mg2+, SO42–
25.
An aqueous solution of silver nitrate is added to an aqueous solution of potassium chromate, and this reaction produces a solid.
What is the formula for the solid?
A) AgK
B) AgCrO4
C) KNO3
D) K2NO3
E)
Ag2CrO4
26.
When NH3(aq) is added to Cu2+(aq), a precipitate initially forms. What is its formula?
A) Cu(NH3)
B) Cu(NO3)2
C) Cu(OH)2
D)
Cu  NH3 
E)
CuO
2
2
27.
An aqueous solution of barium nitrate reacts with an aqueous solution of sodium sulfate. Identify the solid and indicate its
coefficient in the balanced equation.
A) NaNO3 , 1
B) BaSO4 , 1
C) NaNO3 , 2
D) BaSO2 , 2
E)
none of these
28.
Lead(II) nitrate reacts with sodium chloride in aqueous solution to form a precipitate. What is the net ionic equation for this
reaction?
A) Pb2+(aq) + 2NO3–(aq)  Pb(NO3)2(s)
B) Na+(aq) + Cl–(aq)  NaCl(s)
C) Pb2+(aq) + 2Cl–(aq)  PbCl2(s)
D) Na+(aq) + NO3–(aq)  NaNO3(s)
E)
Na+(aq) + Cl2–(aq)  Na2Cl(s)
29.
When 0.2 M sodium hydroxide and 0.2 M barium nitrate are mixed, a precipitate is formed. What is the net ionic equation for
the formation of this precipitate?
A) Ba2+(aq) + 2NO3–(aq)  Ba(NO3) 2(s)
B) Na+(aq) + OH–(aq)  NaOH(s)
C) Ba2+(aq) + 2OH–(aq)  Ba(OH)2(s)
D) Na+(aq) + NO3–(aq)  NaNO3(s)
E)
none of these
30.
Select the unbalanced net ionic equation for the reaction between aqueous lead nitrate and aqueous potassium iodide.
A) Pb(NO3)2(aq) + KI(aq)  PbI2(s) + KNO3(aq)
B) Pb2+(aq) + NO3–(aq) + K+(aq) + I–(aq)  Pb2+(aq) + I–(aq) + K+(aq) + NO3–(aq)
C) Pb2+(aq) + NO3–(aq) + K+(aq) + I–(aq)  PbI2(s) + K+(aq) + NO3–(aq)
D) Pb2+(aq) + I–(aq)  PbI2(s)
E)
none of these
31.
When aqueous sodium hydroxide is added to aqueous nitric acid, what is the balanced molecular equation for the reaction that
takes place?
A) 2NaOH(aq) + H2NO3(aq)  Na2NO3(aq) + 2H2O(l)
B) Na(OH)2(aq) + H2NO3(aq)  Na2NO3(aq) + 2H2O(l)
C) NaOH(aq) + HNO3(aq)  NaNO3(aq) + H2O(l)
D) NaOH(aq) + HNO4(aq)  NaNO4(aq) + H2O(l)
E)
NaOH(aq) + HNO2(aq)  NaNO2(aq) + H2O(l)
32.
What is the net ionic equation for the reaction of aqueous sodium hydroxide with aqueous nitric acid?
A) Na+(aq) + OH–(aq) + H+(aq) + NO3–(aq)  Na+(aq) + NO3–(aq) + H2O(l)
B) Na+(aq) + OH–(aq) + H+(aq) + NO3–(aq)  NaOH(s) + HNO3(l)
C) H+(aq) + OH–(aq)  H2O(l)
D) Na+(aq) + OH–(aq)  NaOH(s)
E)
none of these
33.
Which one of the following basic solutions will not neutralize 25.0 mL of a 1.0 M sulfuric acid solution?
A) 25.0 mL of 1.0 M NaOH
B) 25.0 mL of 2.0 M KOH
C) 50.0 mL of 1.0 M NaOH
D) 100.0 mL of 0.50 M NaOH
E)
All of these will neutralize 25.0 mL of a 1.0 M sulfuric acid solution.
34.
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
35.
A 4.000-g sample of the metal nitrate M(NO3)2 was dissolved in water and treated with excess aqueous sodium sulfate. The
sulfate salt that formed weighed 3.318 g. Determine the identity of the metal.
A) Pb
B) Ba
C) Ca
D) K
E)
none of these
36.
Reacting 47.4 mL of 0.320 M AgNO3 with 48.0 mL of 0.300 M K2CrO4 results in what mass of solid formed?
A) 4.78 g
B) 2.52 g
C) 3.40 g
D) 3.22 g
E)
1.46 g
37.
If all of the chloride in a 5.000-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) 50.55%
B) 10.10%
C) 1.425%
D) 20.22%
E)
none of these
38.
Magnesium metal reacts with hydrochloric acid to form aqueous magnesium chloride and hydrogen gas. When 3.65 g of
magnesium is added to 50.0 mL of 3.00 M hydrochloric acid, what mass of hydrogen is produced, assuming a complete
reaction?
A) 0.123 g
B) 0.151 g
C) 0.246 g
D) 0.302 g
E)
none of these
39.
A mixture contained no fluorine compound except methyl fluoroacetate, FCH 2COOCH3 (molar mass = 92.1 g/mol. When
chemically treated, all the fluorine was converted to CaF2 (molar mass = 78.1 g/mol). The mass of CaF2 obtained was 12.1 g.
Find the mass of methyl fluoroacetate in the original mixture.
A) 92.0 g
B) 28.5 g
C) 24.2 g
D) 14.3 g
E)
12.1 g
40.
You mix 50.0 mL of 2.00 M lead(II) nitrate with 50.0 mL of 2.00 M sodium chloride. What mass of lead(II) chloride should you
form?
A) 12.1 g
B) 13.9 g
C) 24.3 g
D) 27.8 g
E)
none of these
41.
When aqueous solutions of silver nitrate and potassium chromate are mixed, the blood-red precipitate silver chromate is formed.
If 10.0 mL of 0.25 M aqueous silver nitrate is mixed with 15.0 mL of 0.14 M aqueous potassium chromate, what is the total
concentration of ions in the solution after the precipitate is formed?
A) 0.14 M
B) 0.25 M
C) 0.30 M
D) 0.39 M
E)
0.50 M
42.
What volume of 0.25 M HNO3 is necessary to react exactly with 7.4 g of Ca(OH) 2?
A) 2.0 102 mL
B) 2.5  102 mL
C) 4.0  102 mL
D) 8.0  102 mL
E)
1.2  102 mL
43.
You are titrating a solution of sodium hydroxide of unknown concentration with a solution of phosphoric acid that has a
concentration of 0.240 M. Starting with 29.0 mL of the sodium hydroxide solution, you use 16.2 mL of the acid to titrate the
base to completion. Calculate the concentration of the sodium hydroxide solution.
A) 0.134 M
B) 0.0447 M
C) 0.430 M
D) 0.402 M
E)
0.268 M
44.
You have separate aqueous solutions of NaOH and Ca(OH)2 with the same concentrations. You wish to neutralize an aqueous
solution of HCl. Which basic solution would require more volume to neutralize the acid?
A) the NaOH solution
B) the Ca(OH)2 solution
C) You need to know the concentrations of the basic solutions to answer this question.
D) You need to know the volume and concentration of the HCl solution to answer this question.
E)
You need to know the concentrations of the acid and bases and the volume of the acid to answer this question.
45.
A 0.350-g sample of an acid, HX, requires 25.4 mL of a 0.140 M NaOH solution for complete reaction. Calculate the molar
mass of the acid.
A) 42.3 g/mol
B) 68.4 g/mol
C) 98.4 g/mol
D) 121.3 g/mol
E)
none of these
46.
A 0.396-g sample of an unknown triprotic acid is titrated to the third equivalence point using 31.2 mL of 0.199 M NaOH.
Calculate the molar mass of the acid.
A) 1.91  102 g/mol
B) 63.8 g/mol
C) 21.3 g/mol
D) 6.21 g/mol
E)
62.1 g/mol
47.
Sulfamic acid, HSO3NH2 (molar mass = 97.1 g/mol), is a strong monoprotic acid that can be used to standardize a strong base:
HSO3NH2(aq) + KOH(aq)  KSO2NH2(aq) + H2O(l)
A 0.179-g sample of HSO3NH2 required 19.4 mL of an aqueous solution of KOH for complete reaction. What is the molarity of
the KOH solution?
A)
B)
C)
D)
E)
9.25 M
9.50  10–5 M
0.0950 M
0.194 M
none of these
48.
A student weighs out 0.568 g of KHP (molar mass = 204 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) 0.100 M
B) 3.15 M
C) 0.943 M
D) 0.0757 M
E)
none of these
49.
Calculate the concentration of NaOH if 20.8 mL reacts exactly with 24.6 mL of 0.275 M HCl.
A) 0.650 M
B) 0.233 M
C) 0.325 M
D) 0.275 M
E)
0.163 M
50.
What volume of 0.350 M KOH is required to react completely with 24.0 mL of 0.650 M H3PO4?
A) 26.0 mL
B) 52.0 mL
C) 104 mL
D) 156 mL
E)
none of these
51.
Which of the following statements is(are) true?
Oxidation and reduction
I.
II.
III.
IV.
A)
B)
C)
D)
E)
cannot occur independently of each other.
accompany all chemical changes.
describe the loss and gain of electron(s), respectively.
result in a change in the oxidation states of the species involved.
I only
II only
III only
IV only
I, III, and IV
52.
In the reaction Zn + H2SO4  ZnSO4 + H2, which element, if any, is oxidized?
A) zinc
B) hydrogen
C) sulfur
D) oxygen
E)
none of these
53.
Which of the following is not an oxidation-reduction reaction?
A) A precipitation reaction
B) A reaction in which a metal reacts with a nonmetal
C) A combustion reaction
D) A metal reacting with an acid
E)
All of these are oxidation-reduction reactions
Use the following to answer question 54:
The following reaction occurs in aqueous acid solution:
NO3– + I –  IO3– + NO2
54.
What is the oxidation state of iodine in IO3–?
A) 0
B) +3
C) –3
D) +5
E)
–5
55.
What are the oxidation numbers of carbon in CO2 and CO32-, respectively?
A) +2, +6
B) +4, +6
C) -4, -4
D) -4, -6
E)
+4, +4
56.
What is the oxidation state of chromium in K2CrO4?
A) +2
B) +4
C) +6
D) -3
E)
-4
57.
In which state of the following compounds does nitrogen have the most positive oxidation state?
A) HNO3
B) NH4Cl
C) N2O
D) NO2
E)
NaNO2
58.
Which of the following reactions does not involve oxidation-reduction?
A) CH4 + 2O2  2H2O + CO2
B) Mg + 2HCl  MgCl2 + H2
C) 2Na + 2H2O  2NaOH + H2
D) MnO2 + 4HCl  Cl2 + 2H2O + MnCl2
E)
.NaOH + HBr  H2O + NaBr
59.
In the reaction Mg(s) + Pb(NO3)2(aq)  Mg(NO3)2(aq) + Pb(s), identify the oxidizing agent.
A) Mg
B) Pb(NO3)2
C) Mg(NO3)2
D) Pb
E)
O3
60.
In the following reaction, which species is the reducing agent?
3Cu + 6H+ + 2HNO3  3Cu2+ + 2NO + 4H2O
A)
B)
C)
D)
E)
61.
H+
Cu
N in NO
Cu2+
N in HNO3
Which of the following is(are) oxidation-reduction reactions?
I.
PCl3 + Cl2  PCl5
II.
Cu + 2AgNO 3  Cu(NO 3)2 + 2Ag
III.
CO2 + 2LiOH  Li2CO3 + H2O
IV.
FeCl2 + 2NaOH  Fe(OH) 2 + 2NaCl
A)
B)
C)
D)
E)
III only
IV only
I and II only
I, II, and III only
I, II, III, and IV
62.
True or False? The equation 2C2H6 + 7O2  4CO2 + 6H2O is an oxidation-reduction reaction.
A) True; the carbon is oxidized and oxygen is reduced.
B) True; the carbon is reduced and the oxygen is oxidized.
C) True; the carbon is oxidized and the hydrogen is reduced.
D) True; the oxygen is reduced and the hydrogen is oxidized.
E)
False
63.
The following unbalanced reaction occurs in basic media:
Fe2+ + Cr2O72–  Fe3+ + Cr3+
The coefficient for water in the balanced equation is __________, and water appears on the __________ side of the equation.
A)
B)
C)
D)
E)
64.
When the following reaction is balanced in acidic solution, what is the coefficient of water?
Zn(s) + NO3–(aq)  Zn2+(aq) + NH4+(aq)
A)
B)
C)
D)
E)
65.
7, left
7, right
14, left
14, right
none of these
1
2
3
4
none of these
For the redox reaction 2Fe2+ + Cl2  2Fe3+ + 2Cl–, which of the following are the correct half-reactions?
I.
Cl2 + 2e–  2Cl–
II.
Cl  Cl– + e–
III.
Cl2  2Cl– + 2e–
Fe2+  Fe3+ + e–
Fe2+ + e–  Fe3+
IV.
V.
A)
B)
C)
D)
E)
66.
In the balanced equation for the following redox equation, what is the sum of the coefficients?
Fe3+ + I–  Fe2+ + I2
A)
B)
C)
D)
E)
67.
I and IV
I and V
II and IV
II and V
III and IV
4
5
6
7
8
For the reaction of sodium bromide with chlorine gas to form sodium chloride and bromine, what are the appropriate halfreactions? (ox = oxidation and re = reduction)
A) ox: Cl2 + 2e–  2Cl–;
re: 2Br–  Br2 + 2e–
B) ox: 2Br–  Br2 + 2e–; re: Cl2 + 2e–  2Cl–
C) ox: Cl + e–  Cl–;
re: Br  Br– + e–
–
2–
D) ox: Br + 2e  Br ;
re: 2Cl–  Cl2 + 2e–
+
–
E)
ox: 2Na + 2e  2Na; re: 2Cl–  Cl2 + 2e–
Use the following to answer question 68:
The following reaction occurs in aqueous acid solution:
NO3– + I –  IO3– + NO2
68.
In the balanced equation, what is the coefficient of NO3–?
A) 2
B) 3
C) 4
D) 5
E)
6
69.
Balance the reaction below in acidic aqueous solution, using the oxidation number method. In the balanced equation, what is
the coefficient of Sn2+?
ClO3– + Sn2+  Cl– + Sn4+
A)
B)
C)
D)
E)
1
3
5
7
8
Use the following to answer question 70:
The following reaction occurs in aqueous acid solution:
NO3– + I –  IO3– + NO2
70.
In the balanced equation, what is the coefficient of water?
A) 1
B) 2
C) 3
D) 4
E)
5
71.
When the equation Cl2  Cl– + ClO3– (basic solution) is balanced using the smallest whole-number coefficients, what is the
coefficient of OH–?
A) 1
B) 2
C) 3
D) 4
E)
6
72.
With what volume of 2.6 M HF will 6.8 g of calcium hydroxide react completely, according to the reaction 2HF + Ca(OH) 2 
CaF2 + 2H2O?
A) 3.5  101 mL
B) 2.6  101 mL
C) 1.7  101 mL
D) 7.1  101 mL
E)
1.8  102 mL
73.
Balance the reaction below in acidic solution.
IO3– +I–  I2
What volume of 0.352 M HCl is needed to produce 2.48  10-3 mol of iodine, I2, with an excess of KIO3 and KI?
A)
B)
C)
D)
E)
74.
2.48 mL
4.96 mL
7.05 mL
14.1 mL
none of these
The ion MnO4– is often used to analyze for the Fe2+ content of an aqueous solution by using the reaction
MnO4– + Fe2+  Fe3+ + Mn2+
in acidic solution. A 48.6-mL sample of a solution containing Fe2+ requires 33.5 mL of a 0.022 M KMnO4 solution for complete
reaction. What is the concentration of the Fe2+ in the original solution?
A)
B)
C)
D)
E)
75.
7.6  10-2 M
1.5  10-2 M
4.5  10-2 M
3.2  10-1 M
3.0  10-3 M
The following equation describes the oxidation of ethanol to acetic acid by potassium permanganate:
3C2H5OH + 4KMnO4  3HC2H3O2 + 4MnO2 + 4KOH + H2O
5.0 g of ethanol and an excess of aqueous KMnO4 are reacted, and 5.9 g HC2H3O2 results. What is the percent yield?
A)
B)
C)
D)
E)
76.
100%
91%
67%
30.%
5.9 g HC2H3O2 is impossible because it represents more than a 100% yield.
In the reaction
3Cu(s) + 8HNO3(aq)  3Cu(NO3)2(aq) + 4H2O(l)+ 2NO(g)
6.3 g of Cu and 100.0 mL of 1.0 M HNO3 are combined. Which of the following statements is true?
A)
B)
C)
D)
E)
77.
Cu and HNO3 react in a 1:1 mole ratio.
Cu is the limiting reagent, and 0.062 mol HNO3 does not react.
HNO3 is the limiting reagent, and 0.062 mol Cu does not react.
Cu and HNO3 are present in stoichiometric amounts; neither is in excess.
0.080 mol H2O is produced
In the reaction
2MnO4– + 5H2O2 + 6H+  2Mn2+ + 8H2O + 5O2
what volume of 0.150 M KMnO4 solution is needed to titrate 75.0 mL of a 0.150 M H2O2 solution?
A)
B)
C)
D)
E)
15.0 mL
30.0 mL
45.0 mL
75.0 mL
none of these
Answer Key
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
T
D
B
D
C
B
C
D
B
A
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
C
D
D
D
D
D
E
D
B
A
21.
22.
23.
24.
25.
26.
27.
28.
29.
30.
B
A
C
E
E
C
B
C
C
D
31.
32.
33.
34.
35.
36.
37.
38.
39.
40.
C
C
A
A
C
B
B
B
B
B
41.
42.
43.
44.
45.
46.
47.
48.
49.
50.
C
D
D
A
C
A
C
D
C
E
51.
52.
53.
54.
55.
56.
57.
58.
59.
60.
E
A
A
D
E
C
A
E
B
B
61.
62.
63.
64.
65.
66.
67.
68.
69.
70.
C
A
A
C
A
D
B
E
B
C
71.
72.
73.
74.
75.
76.
77.
E
D
D
A
B
C
B