Chapter 4 Practice Test
1. A 20.0-g sample of HF is dissolved in water to give 2.0  102 mL of solution. The
concentration of the solution is:
a)
b)
c)
d)
e)
1.0 M
3.0 M
0.10 M
5.0 M
10.0 M
ANS: d)
5.0 M
PAGE: 4.3
2. Which of the following aqueous solutions contains the greatest number of ions?
a)
b)
c)
d)
e)
400.0 mL of 0.10 M NaCl
300.0 mL of 0.10 M CaCl2
200.0 mL of 0.10 M FeCl3
200.0 mL of 0.10 M KBr
800.0 mL of 0.10 M sucrose
ANS: b)
300.0 mL of 0.10 M CaCl2
PAGE: 4.3
3. What mass of calcium chloride, CaCl2, is needed to prepare 2.850 L of a 1.56 M
solution?
a)
b)
c)
d)
e)
25.9 g
60.8 g
111 g
203 g
493 g
ANS:
e)
493 g
PAGE: 4.3
4. What volume of 18.0 M sulfuric acid must be used to prepare 15.5 L of 0.195 M
H2SO4?
a)
b)
c)
d)
e)
168 mL
0.336 L
92.3 mL
226 mL
none of these
ANS: a) 168 mL
PAGE: 4.3
5. The net ionic equation for the reaction of aluminum sulfate and sodium hydroxide
contains which of the following species?
a)
b)
3Al3+(aq)
OH–(aq)
c)
d)
e)
ANS:
3OH–(aq)
2Al3+(aq)
2Al(OH)3(s)
c)
3OH–(aq)
PAGE: 4.6,8
6. Which of the following is a strong acid?
a)
b)
c)
d)
e)
HF
KOH
HClO4
HClO
HBrO
ANS: c) HClO4
7. Which of the following is not a strong base?
a)
b)
c)
d)
e)
PAGE: 4.2
Ca(OH)2
KOH
NH3
LiOH
Sr(OH)2
ANS: c) NH3
PAGE: 4.2
8. 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)
b)
c)
d)
e)
PbCl(s)
Pb2Cl(s)
NaNO3(aq)
2NaNO3(aq)
2PbCl2(s)
ANS: d) 2NaNO3(aq)
PAGE: 4.5,6
9. You mix 260. mL of 1.20 M lead(II) nitrate with 300. mL of 1.90 M potassium iodide.
The lead(II) iodide is insoluble. Which of the following is false?
a)
b)
c)
d)
e)
The final concentration of Pb2+ ions is 0.0482 M.
You form 131 g of lead(II) iodide.
The final concentration of K+ is 1.02 M.
The final concentration of NO3- is 1.02 M.
All are true.
ANS: d)
The final concentration of NO3- is 1.02 M.
PAGE: 4.5-7
10. The concentration of a salt water solution which sits in an open beaker decreases
over time.
ANS: False
11. The following reactions:
PAGE: 4.3
Pb2+ + 2I–  PbI2
2Ce4+ + 2I–  I2 + 2Ce3+
HOAc + NH3  NH4+ + OAc–
are examples of
a)
b)
c)
d)
e)
ANS:
acid-base reactions.
unbalanced reactions.
precipitation, acid-base, and redox reactions, respectively.
redox, acid-base, and precipitation reactions, respectively.
precipitation, redox, and acid-base reactions, respectively.
e)
precipitation, redox, and acid-base reactions,
respectively.
PAGE: 4.4-9
12–14. Aqueous solutions of barium chloride and silver nitrate are mixed to form solid
silver chloride and aqueous barium nitrate.
12. The balanced molecular equation contains which one of the following terms?
a)
b)
c)
d)
e)
AgCl(s)
2AgCl(s)
2Ba(NO3)2
BaNO3
3AgCl(s)
ANS: b)
2AgCl(s)
PAGE: 4.5,6
13. The balanced complete ionic equation contains which of the following terms?
a)
b)
c)
d)
2Ba2+(aq)
Cl–(aq)
2Ag+(aq)
NO3 – (aq)
e)
3NO3 – (aq)
ANS:
c)
2Ag+(aq)
PAGE: 4.5,6
14. The net ionic equation contains which of the following terms?
a)
b)
c)
Ag+(aq)
Ba2+(aq)
NO3 – (aq)
d)
2NO3 – (aq)
e)
none of these
ANS:
a)
Ag+(aq)
15. When NH3(aq) is added to Cu2+(aq), a precipitate initially forms. Its formula is:
PAGE: 4.5,6
2+
a)
Cu(NH3)4
b)
Cu(NO3)2
c)
Cu(OH)2
d)
Cu(NH3)2
e)
CuO
2+
ANS: c) Cu(OH)2
PAGE: 4.5
16. 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)
b)
c)
d)
e)
ANS:
Na2SO4, NaCl, Na2S
Na2SO4, Na2S, NaCl
Na2S, NaCl, Na2SO4
NaCl, Na2S, Na2SO4
NaCl, Na2SO4, Na2S
a)
Na2SO4, NaCl, Na2S
PAGE: 4.5
17. In the balanced molecular equation for the neutralization of sodium hydroxide with
sulfuric acid, the products are:
a)
b)
c)
d)
e)
NaSO4 + H2O
NaSO3 + 2H2O
2NaSO4 + H2O
Na2S + 2H2O
Na2SO4 + 2H2O
ANS: e) Na2SO4 + 2H2O
PAGE: 4.6,8
18. Which of the following do you need to know to be able to calculate the molarity of a
salt solution?
I.
II.
III.
IV.
a)
b)
c)
d)
e)
the mass of salt added
the molar mass of the salt
the volume of water added
the total volume of the solution
I, III
I, II, III
II, III
I, II, IV
You need all of the information.
ANS: d)
I, II, IV
19. 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
PAGE: 4.3
b)
c)
d)
e)
ANS:
the H2SO4 solution
You need to know the acid concentrations to answer this question.
You need to know the volume and concentration of the NaOH solution to
answer this question.
c and d
a)
the HCl solution
PAGE: 4.8
20. In which of the following does nitrogen have an oxidation state of +4?
a)
b)
c)
d)
e)
HNO3
NO2
N2O
NH4Cl
NaNO2
ANS: b)
NO2
PAGE: 4.9
21. In the reaction 2Ca(s) + O2(g)  2CaO(s), which species is oxidized?
a)
O2
b)
c)
d)
e)
O2–
Ca
Ca2+
none of these
ANS:
c)
Ca
PAGE: 4.9
22. In the reaction N2(g) + 3H2(g)  2NH3(g), N2 is
a)
b)
c)
d)
e)
oxidized.
reduced.
the electron donor.
the reducing agent.
two of these
ANS: b) reduced.
PAGE: 4.9
23. For the reaction of sodium bromide with chlorine gas to form sodium chloride and
bromine, the appropriate half-reactions are (ox = oxidation and re = reduction):
a)
b)
c)
d)
e)
ox:
ox:
ox:
ox:
ox:
ANS: b)
Cl2 + 2e–  2Cl–;
2Br–  Br2 + 2e–;
Cl + e–  Cl–;
Br + 2e–  Br2–;
2Na+ + 2e–  2Na;
re:
re:
re:
re:
re:
ox: 2Br–  Br2 + 2e–;
2Br–  Br2 + 2e–
Cl2 + 2e–  2Cl–
Br  Br– + e–
2Cl–  Cl2 + 2e–
2Cl–  Cl2 + 2e–
re:
Cl2 + 2e–  2Cl–
24. How many of the following are oxidation-reduction reactions?
NaOH + HCl  NaCl + H2O
PAGE: 4.10
Cu + 2AgNO3  2Ag + Cu(NO3)2
Mg(OH)2  MgO + H2O
N2 + 3H2  2NH3
a)
b)
c)
d)
e)
0
1
2
3
4
ANS: c) 2
25. Given the following reaction in acidic media:
PAGE: 4.9
Fe2+ + Cr2O72–  Fe3+ + Cr3+
answer the following question: The coefficient for water in the balanced reaction
is
a)
b)
c)
d)
e)
1.
3.
5.
7.
none of these
ANS: d)
7
PAGE: 4.10
26. The following unbalanced equation represents a reaction that occurs in basic
solution:
MnO42– + C2O42–  MnO2 + CO32–
How many moles of MnO42– are required to produce 1 mole of CO32–?
a)
b)
c)
d)
e)
4
3
2
1
none of these
ANS:
e)
none of these
PAGE: 4.10
27. When the equation Cl2  Cl– + ClO3– (basic solution) is balanced using the smallest
whole-number coefficients, the coefficient of OH– is:
a)
b)
c)
d)
e)
ANS:
1
2
3
4
6
e)
6
PAGE: 4.10