CHEM 100 Sample Test Chapter 5
SAMPLE TEST -CHPATER 5
Freshman Chemistry, La Tech-CHEM 100 sample, Test 3-Chapter 5.
1.
When a homogeneous liquid mixture is
formed from solid KNO3 and water, the KNO3
is called a
a. solution. b. solute. c. solvent. d. melt.
2. A supersaturated solution
a. contains more solute than a saturated
solution.
b. has extra solute at the bottom.
c. has an extremely high concentration.
d. is intensely colored.
10. Which salt below is insoluble?
a. Na2NO3. b. BaCl2. c. PbCl2. d. NH4SO4.
11. How much 12.6 M HCl is required to make
75.0 mL of 3.50 M HCl?
a. 20.8 mL b. 58.8 mL c. 270 mL d. 0.588 mL
12. An increase in oxidation number during the
course of a reaction is called
a. oxidation.
b. reduction.
c. disproportionation. d. titration.
3. Sugar is best classified as
a. a strong electrolyte. b. a nonelectrolyte.
c. a weak electrolyte.
d. insoluble.
13. The following species with the highest
oxidation
number for manganese is
b. MnO4-. c. MnO2. d.
a. MnSO4.
Mn2O3.
14. The oxidation number of I in IF5 is
a. -1/5.
b. +1/5. c. -5.
d. +5.
4. The compound NaCl is best classified as
a. a strong electrolyte. b. a nonelectrolyte.
c. a weak electrolyte. d. insoluble.
5. The compound NaC2H3O2 is best classified as
a. an acid. b. a base. c. a salt. d. a nonelectrolyte.
6.
7.
15. The reaction below that is NOT a redox
reaction is
a. 2 C2H6(g) + 7 O2(g) Æ 4 CO2(g) + 6 H2O (l).
b. 2 AgNO3(aq) +Cu(s)Æ 2Ag(s) +C
u(NO3)2(aq).
c. AgNO3(aq) + HCl(aq) Æ AgCl(s) + HNO3(aq).
d. 6 CO2(g) + 6 H2O(l) Æ C6H12O6(aq) + 6 O2(g).
When a solution of CuCl2 and one of AgNO3
are mixed, the net ionic equation is
a. Cu2+(aq) + 2 Cl-(aq) + 2 Ag+(aq) + 2 NO3-(aq)
--> Cu2+ (aq) + 2 NO3-(aq) + 2 AgCl(s).
b. CuCl2(aq)+ 2 AgNO3(aq)
--> Cu(NO3)2(aq) + 2 AgCl(s).
c. Cu2+(aq) + 2 NO3-(aq) --> Cu(NO3)2(aq).
d. Cl-(aq) + Ag+ (aq) --> AgCl(s).
When a solution of BaNO3 and one of Na2SO4
are mixed, what is/are the spectator ion(s) ?
16. For Pb(s) + PbO2(s) + 2 H2SO4(aq) Æ
2 PbSO4(s) + 2 H2O(l), the substance that is
reduced during the reaction is
a. Pb(s). b. PbO2(s). c. H2SO4(aq). d.
PbSO4(s).
Ba(NO3)2(aq) + Na2SO4(aq)
--> BaSO4(s) + 2NaNO3(aq)
a. Na+ and NO3-. b. SO42-.
d. there are no spectator ions.
c. Ba2+.
17. Which compound will not dissolve in
water?
a. KCl b. NH4NO3 c. CaS d.MgSO4 e.NaNO3
18. Which compound will dissolve in water?
a. BaSO4 b.MgS c.AgCl d.Al(OH)3
e.Na2SO4
8. The (w/w %) percent by mass KNO3 of a
solution prepared by dissolving 5.34 g of KNO3 in
34.7 g of water is
a. 15.4.
b. 13.3. c. 8.18. d. 5.34.
19. Which compounds will not dissolve in
water at 20°C?
CaSO4
PbCl2
KBr
KNO3
I
II
III
IV
9.
The molarity of a solution made by dissolving
2.38 g of NH4NO3 (f.w.=80.06 g/mol) in 25.0
mL of solution is
a. 0.0952 M. b. 95.2 M. c. 1.19 M. d. 0.119 M.
25
a.
b.
c.
d.
e.
d. Al+ + OH- → AlOH
e. Al3+ + 3OH- → Al(OH)3
I & II
II & III
III & IV
I & IV
III & IV
24. Which of the following is not a property
of acids?
a. Acids taste sour.
b. Acids produce gas bubbles when reacting
with limestone.
c. Acids neutralize bases.
d. Acids form precipitates on reaction with
metals.
e. Acids increase the hydrogen ion
concentration of water when dissolved in it.
20. Which statement about the reaction
below is true?
NaCl + NH4NO3 → NaNO3 + NH4Cl
a. All compounds in the reaction are soluble in
water and no reaction occurs.
b. NaNO3 is insoluble in water and will
precipitate.
c. NH4Cl is insoluble in water and will
precipitate.
d. Both NaNO3 and NH4Cl are insoluble in
water and will precipitate.
e. NH4NO3 is insoluble in water and no
reaction will occur.
21. Which statement about the reaction
below is true?
Pb(NO3)2 + Na2SO4 → PbSO4 + 2NaNO3
a. All compounds in the reaction are soluble in
water and no reaction occurs.
b. PbSO4 is insoluble in water and will
precipitate.
c. NaNO3 is insoluble in water and will
precipitate.
d. Both NaNO3 and PbSO4 are insoluble in
water
and will precipitate.
e. Pb(NO3)2 is insoluble in water and no
reaction
will occur.
a.
b.
c.
d.
e.
23.
a.
b.
c.
a.
b.
c.
d.
e.
25. What is the correct formula for the
hydronium ion?
HNH4+
OHH3O+
H+
a.
b.
c.
d.
e.
26. What is the correct formula for the
hydroxide ion?
H
NH4+
OHH3O+
H+
27. Which statement about strong acids is
true?
a. Strong acids are weak electrolytes.
b. Strong acids are very concentrated.
c. Strong acids are almost entirely converted
to ions when dissolved in water.
d. Acetic acid is a strong acid.
e. All of the above are true.
28. Which statement about bases is false?
a. Bases increase the hydroxide ion
concentration of water when dissolved in it.
b. Bases turn red litmus paper blue.
c. Bases taste bitter.
d. Ammonia is a base.
e. Bases increase the hydronium ion
concentration of water when dissolved in it.
22. What is the net ionic equation for the
reaction of AgNO3 and KBr?
+
Ag + Br- → AgBr
Ag2+ + Br- → AgBr2
Ag2+ + Br2- → AgBr
K+ + NO3- → KNO3
K2+ + NO3- → K(NO3)2
What is the net ionic equation for the
reaction of AlCl3 and NaOH.
Al3+ + OH3- → AlOH
Na3+ + 3Cl- → NaCl3
Na+ + Cl- → NaCl
29. All of the following are strong
electrolytes except:
26
a.
b.
c.
d.
e.
HCl
NaOH
NH4OH
H2SO4
HNO3
a.
b.
c.
d.
e.
30. Which of the following is a nonelectrolyte?
HBr
Mg(OH)2
NaCl
C6H12O6
KI
a.
b.
c.
d.
e.
31. Which statement about neutralization
reactions is false?
The reaction of a strong base with a
strong acid
is an example of a neutralization
reaction.
Neutralization reactions produce salts.
The net ionic equation for a
neutralization
reaction shows the formation of water.
Organic acids can neutralize bases.
All of the above are true.
32. Which of the following factors cause
exchange reactions to occur?
formation of a gas only
formation of a precipitate only
formation of water only
formation of a gas or a precipitate
formation of a gas, precipitate or water
a.
b.
c.
d.
e.
33. What species is the reducing agent in
the reaction below?
HCl + Mg → MgCl2 + H2
HCl
Mg
MgCl2
H2
Mg and H2
a.
b.
c.
d.
e.
d. O2 and CaO
e. CaO
34. What species is the oxidizing agent in
the reaction below?
Ca + O2 → CaO
a. Ca
b. Ca and O2
c. O2
a.
b.
c.
d.
e.
35. Which of the following is a reducing
agent?
O2
F2
Br2
I2
Na
a.
b.
c.
d.
e.
36. Which of the following represents an
oxidation half reaction?
Na+ + 1e- → Na
Mg → Mg2+ + 2eCu2+ + 1e- → Cu
Al3+ + 3e- → Al
O + 2e- → O2-
a.
b.
c.
d.
e.
37. Which of the following represents a
reduction half reaction?
F- → F2 + 2eNi2+ → Ni3+ + 1eS + 2e- → S2K → K1+ + 1ePb → Pb2+ + 2e-
a.
b.
c.
d.
e.
38. Which substance is oxidized in the
reaction below?
NaNO3 + Pb → NaNO2 + PbO
NaNO3
NaNO2
Pb
PbO
none of the above
a.
b.
c.
d.
e.
39. Which substance is reduced in the
reaction below?
Na2SO4 + 4C → Na2S + 4CO
Na2S
Na2SO4
CO
S
none of the above
40. What is the oxidation number of Cl in
Cl2O5?
27
a.
b.
c.
d.
e.
41.
+2
-2
-3
-5
+5
What is the oxidation number of H in
MgH2?
a. -1
b. +1
c. 0
d. +2
e. -2
42. What is the oxidation number of F in F2?
a. -1
b. +1
c. 0
d. +2
e. -2
b.
c.
d.
e.
CO2
O2
H2O
O2 and CO2
47.
a.
b.
c.
d.
e.
48.
a.
b.
c.
d.
e.
Which element is most reactive?
Mg
Ag
Ba
Sn
Ni
Which element is least reactive?
Zn
Pb
Fe
Al
Cu
49. Which single replacement reaction will
not occur?
a. Mg + CaSO4 → MgSO4 + Ca
b. Ba + HCl → BaCl2 + H2
c. Al + SnCl2 → AlCl3 + Sn
d. H2 + AgNO3 → HNO3 + Ag
e. Mg + CuSO4 → Cu + MgSO4
43. What is the oxidation number of P in
PO43-?
a. -3
b. +3
c. -2
d. +5
e. -5
50. How many grams of NaOH are present in
25.0 mL of a 0.1000 M NaOH solution?
a. 100 g
b. 2.50 × 10-3 g
c. 0.100 g
d. 2.50 g
e. 25.0 g
44. What is the oxidation number of N in
NH4+?
a. +1
b. -1
c. 0
d. +3
e. -3
45. Which species is oxidized in the reaction
below?
I2O5 + CO → I2 + CO2
a. CO2
b. I2
c. I2O5
d. CO
e. CO and CO2
51. What is the molarity of a solution that
results when 14.2 g of (NH4)3PO4 is
dissolved in water and diluted to exactly
250.0 mL?
a. 1.52 M
b. 0.238 M
c. 56.8 M
d. 0.381 M
e. 1.07 × 10-4 M
46. Which species is oxidized in the reaction
below?
CH4 + O2 → CO2 + H2O
a. CH4
52. Determine the ammonium ion
concentration of a solution that results
when 4.53 g of (NH4)2SO4 is dissolved in
water and diluted to exactly 100.0 mL.
28
a.
b.
c.
d.
e.
0.686 M
0.343 M
1.03 M
1.37 M
2.51 M
b.
c.
d.
e.
0.0469 moles
3.00 × 10-3 moles
46.9 moles
0.938 moles
58. How many moles of ions are in 285 mL of
0.0150 M MgCl2?
a. 4.128 × 10-3 mol
b. 5.26 × 10-2 mol
c. 5.26 × 10-1 mol
d. 1.28 × 10-2 mol
e. 1.05 × 10-1 mol
53. To what volume must 25.0 g of BaCl2 be
diluted to yield a solution that is 0.600 M?
a. 240. mL
b. 400. mL
c. 800. mL
d. 480. mL
e. 200. mL
54. A 50.0 mL sample of 0.108 M H2SO4 is
diluted to 250.0 mL. What is its new
molarity?
a. 0.542 M
b. 0.0216 M
c. 0.184 M
d. 0.461 M
e. 0.108 M
59. A solution is made by dissolving 12.5 g of
LiCl in enough water to make 500.0 mL
of solution. How many moles are in 35.0
mL of solution?
a. 0.0206 mol
b. 0.295 mol
c. 0.590 mol
d. 0.0103 mol
e. 0.438 mol
55. To which volume should a 25.0 ml sample
of 1.50 M Na2SO4 be diluted to yield a
final solution that is 0.300 M in sodium
ions?
a. 375 mL
b. 125 mL
c. 250 mL
d. 4.95 mL
e. 4950 mL
60. A solution is made by dissolving 60.0 g of
AlCl3 in enough water to make 250.0 mL
of solution. How many moles of ions are
in 5.00 mL of solution?
a. 5.00 × 10-3 mol
b. 9.00 × 10-3 mol
c. 1.25 × 10-3 mol
d. 1.01 × 10-3 mol
e. 3.60 × 10-2 mol
56. Which of the methods described below
will yield 500 mL of a 0.100 M KMnO4
solution?
a. Add exactly 500 mL of water to 7.90 g of
KMnO4.
b. Dissolve 15.8 g KMnO4 in water and dilute
to exactly 500 mL.
c. Add exactly 500 mL of water to KMnO4.
d. Dissolve 7.90 g of KMnO4 in water and
dilute to exactly 500 mL.
e. Dilute 220 mL of 1.00 M KMnO4 to exactly
500 mL.
61. How many grams of AgCl will precipitate
from the reaction of 37.0 mL of 0.280 M
AgNO3 with excess NaCl solution?
a. 149 g
b. 189 g
c. 1.49 g
d. 1.89 g
e. 0.60 g
62. Hydrochloric acid solutions are often
standardized by the reaction below. How
many grams of CaCO3 are required to
exactly react with 50.0 mL of 0.155 M
HCl?
57. How many moles are in 125.0 mL of 0.375
M KCl?
a. 3.00 moles
29
CaCO3(s) + 2HCl(aq) → CaCl2(aq) + H2O(l) +
CO2(g)
a. 0.341 g
b. 0.566 g
c. 0.387 g
d. 0.194 g
e. 0.283 g
63. Oxalic acid, H2C2O4, reacts with Y(NO3)3
as shown by the equation below. What
weight of yttrium oxalate is produced
from 50.0 mL of 0.265 M Y(NO3)3 and
excess oxalic acid?
b.
c.
d.
e.
0.1018 M
0.03122 M
0.1021 M
0. 09453 M
67. A 25.00 mL sample of H2SO4 solution is
neutralized by exactly 41.63 mL of 0.1363
M NaOH. What is the molarity of the
H2SO4 solution?
a. 0.2270 M
b. 0.2726 M
c. 0.06815 M
d. 0.1135 M
e. 0.05675 M
68. A 35.00 mL sample of HNO3 solution is
neutralized by exactly 42.63 mL of 0.4153
M Ba(OH)2. What is the molarity of the
HNO3 solution?
a. 0.5058 M
b. 0.1265 M
c. 0.2529 M
d. 0.2077 M
e. 1.012 M
69. A 25.00 mL sample of H3PO4 solution is
neutralized by exactly 54.93 mL of
0.04345 M Ca(OH)2. What is the molarity
of the H3PO4 solution?
a. 0.2148 M
b. 0.09546 M
c. 0.2897 M
d. 0.06363 M
e. 0.1432 M
70. Ammonia and sulfuric acid react according to
2Y(NO3)3(aq) + 3H2C2O4(aq) → Y2(C2O4)3(s) +
6HNO3(aq)
a. 5.85 g
b. 2.93 g
c. 1.82 g
d. 1.46 g
e. 3.64 g
64. Determine the mass of BaSO4 that is
produced by the reaction of 45.0 mL of
0.155 M H2SO4 and 60.0 mL of 0.125 M
BaCl2.
BaCl2(aq) + H2SO4(aq) → BaSO4(s) + 2HCl(aq)
a. 0.775 g
b. 3.24 g
c. 1.62 g
d. 1.79 g
e. 1.45 g
65. Ammonia and sulfuric acid react
according to the equation given below.
How many milliliters of 0.110 M sulfuric
acid are required to exactly neutralize
25.0 mL of 0.0840 M NH3 solution?
2NH3(aq) + H2SO4(aq) → (NH4)2SO4(aq)
a. 5.85 g
b. 9.55 g
c. 1.82 g
d. 1.46 g
e. 3.64 g
66. A 25.00 mL sample of HCl solution is
neutralized by exactly 31.22 mL of
0.08152 M NaOH. What is the molarity of
the HCl solution?
a. 0.08152 M
the equation below. How many milliliters of
0.110 M sulfuric acid are required to exactly
neutralize 25.0 mL of 0.0840 M ammonia
solution?
2NH3(aq) + H2SO4(aq) → (NH4)2SO4(aq)
a.
b.
c.
d.
e.
12.5 mL
25.0 mL
4.77 mL
9.55 mL
19.1 mL
Answers to Sample Test
1. > b
2. > a
3. > b
4. > a
30
solute.
contains more solute than a saturated solution.
a non-electrolyte.
a strong electrolyte.
47.
48.
49.
50.
51.
52.
53.
54.
55.
56.
c. Ba
e. Cu
a. Mg + CaSO4 → MgSO4 + Ca
c. 0.100 g
d. 0.381 M
a. 0.686 M
e. 200. mL
b. 0.0216 M
c. 250 mL
d. Dissolve 7.90 g of KMnO4 in water and
dilute to exactly 500 mL.
57. b. 0.0469 moles
58. d. 1.28 × 10-2 mol
59. a. 0.0206 mol
60. e. 3.60 × 10-2 mol
61. c. 1.49 g
62. c. 0.387 g
63. b. 2.93 g
64. c. 1.62 g
65. b. 9.55 g
66. b. 0.1018 M
67. d. 0.1135 M
68. e. 1.012 M
69. d. 0.06363 M
70. d. 9.55 mL
5. > c a salt.
6. > d Cl-(aq) + Ag+ (aq) --> AgCl(s).
7. > a Na+ and NO3-.
8. > b 13.3.
9. > c 1.19 M.
10. > c PbCl2.
11. > a 20.8 mL
12. > a oxidation.
13. > b. MnO4-.
14. > d +5.
15. > c AgNO3(aq) + HCl(aq) Æ AgCl(s) +
NO3(aq).
16. > b. PbO2(s).
17.
e. CaS
18. e. Na2SO4 REF: Section 5.1
19. a. I & II
20. a. All compounds in the reaction are soluble
in water
21. b. PbSO4 is insoluble in water and will
precipitate
22. a. Ag+ + Br- → AgBr
23. e. Al3+ + 3OH- → Al(OH)3
24. d. Acids form precipitates on reaction with
metals.
25. c. H3O+
26. c. OH27. c. Strong acids are almost entirely converted
to ions when dissolved
28. e. Bases increase the hydronium ion
concentration of water when dissolved in it.
29. c. NH4OH
30. d. C6H12O6
31. e. All of the above are true.
32. e. formation of a gas, precipitate or water
33. b. Mg
34. c. O2
35. e. Na
36. b. Mg → Mg2+ + 2e37. c. S + 2e- → S238. c. Pb
39. d. S
40. e. +5
41. a. -1
42. c. 0
43. d. +5
44. e. -3
45. d. CO
46. a. CH4
31