Chapter
5 Kotz5e Multiple Choice Sample Test
1. Which of the following ionic compounds is insoluble in water?
|
NH4Cl |
|
|
b. |
Li2CO3 |
|
c. |
PbSO4 |
|
d. |
KI |
|
e. |
Na2S |
2. All of the following compounds are soluble in water EXCEPT
|
a. |
NaCl. |
|
b. |
ZnCl2. |
|
c. |
FeCl2. |
|
d. |
BaCl2. |
|
e. |
Hg2Cl2. |
3. All of the following compounds are insoluble in water EXCEPT
|
a. |
CuS. |
|
b. |
Hg2Cl2. |
|
c. |
(NH4)2S. |
|
d. |
Zn(OH)2. |
|
e. |
BaSO4. |
4. Solutions of the following are mixed. A precipitate would be formed by
|
a. |
NaNO3 and NH4Cl. |
|
b. |
CuSO4 and KCl. |
|
c. |
AgNO3 and CsBr. |
|
d. |
NaCl and Fe(NO3)2. |
|
e. |
HCl and NaOH. |
5. The net ionic equation for neutralization of benzoic
acid by a base is
C6H5COOH(aq)
+
Therefore,
|
a. |
benzoic acid is a strong acid. |
|
b. |
the base is a weak base. |
|
c. |
the C6H5COO- ion is a
spectator ion. |
|
d. |
the ion, K+, could be a spectator ion. |
|
e. |
the base in the titration could be NH3. |
6. The net ionic equation for the reaction of hydrobromic
acid with potassium hydroxide
isTop of Form
|
a. |
HBrO3(aq) + |
|
b. |
HBr(aq) + |
|
c. |
H+(aq) + |
|
d. |
HBrO3(aq) + KOH(aq) --> KBrO3(aq)
+ H2O(l) |
|
e. |
HBr(aq) + KOH(aq) --> KBr(aq) + H2O(l) |
|
|
7. All of the following are strong
acids and weak acids respectively EXCEPT
|
a. |
HNO3 and HNO2. |
|
b. |
H2SO4 and
H2SO3. |
|
c. |
HClO4 and HClO. |
|
d. |
HClO3 and HClO2. |
|
e. |
H3PO4 and HClO. |
8. Which of the following is a
weak electrolyte in aqueous solution?
|
a. |
H2S |
|
b. |
H2SO4 |
|
c. |
HI |
|
d. |
HNO3 |
|
e. |
HClO3 |
9. Which of the following nonmetal oxides is paired with the acid which will
result from the addition of water to the nonmetal oxide?
|
a. |
NO2 and HNO2 |
|
b. |
SO3 and H2SO4
|
|
c. |
P4O10 and
H3PO3 |
|
d. |
N2O5 and
HNO2 |
|
e. |
NO and HNO2 |
10. All of the following
statements represent characteristic properties of acids EXCEPT
|
a. |
proton donors. |
|
b. |
react with bases to produce a salt and water. |
|
c. |
will hydrolyze and produce hydroxide ions. |
|
d. |
turn blue litmus red. |
|
e. |
produce carbon dioxide from metal carbonates. |
11. Besides its ability to function as an acid, sulfuric acid is able to act as
an oxidizing agent. Which one of the following equations illustrates this
ability?
|
a. |
CaF2(s) + H2SO4(aq) --> CaSO4(aq)
+ 2HF(aq) |
|
b. |
2NH3(g) + H2SO4(aq) --> 2NH4+(aq) + SO42-(aq) |
|
c. |
2H+(aq) + 2NaI(s) + H2SO4(aq) --> I2(s) + 2H2O + SO2(g)
+ 2Na+ |
|
d. |
|
|
e. |
NaCl(s) + H2SO4(aq) --> NaHSO4(aq)
+ HCl(aq) |
12. In the balanced equation
3Na+ + 3OH- + P4 + 3H2O --> 3Na+ + 3H2PO2- + PH3
the reducing agent is
|
a. |
Na+. |
|
b. |
|
|
c. |
P4. |
|
d. |
H2O. |
|
e. |
H2PO2-. |
13. The oxidation number of boron in the compound H3BO3
is
|
a. |
0. |
|
b. |
1. |
|
c. |
2. |
|
d. |
3. |
|
e. |
6. |
14. The oxidation number of nitrogen in Ca(NO2)2 is
|
a. |
1. |
|
b. |
2. |
|
c. |
3. |
|
d. |
4. |
|
e. |
5. |
15. Consider the reactions represented by the following net ionic equations:
1. 2Na(s) + 2H3O+(aq) --> 2Na+(aq) +
H2(g) + 2H2O(l)
2. O2-(aq) + H2O(aq) --> 2OH-(aq)
3. Cu2+(aq) + H2S(g) --> CuS(s)
+ 2H+(aq)
The equation(s) which would be classified as oxidation-reduction(s) is (are)
|
a. |
1 only. |
|
b. |
2 only. |
|
c. |
1 and 2 only. |
|
d. |
1 and 3 only. |
|
e. |
1, 2, and 3. |
16. The molarity
of a solution is defined as
|
a. |
the number of moles of solute per kilogram of solvent. |
|
b. |
the number of moles of solute per liter of solution. |
|
c. |
the number of gram-equivalent weights of solute per liter of
solution. |
|
d. |
the number of gram-equivalent weights of solute per kilogram
of solution. |
|
e. |
the number of moles of solute per liter of solvent. |
17. Calculate the molarity of a solution that
contains 56.0 g of HCl in 265 mL
of solution.
(Molar Mass HCl = 36.5 g/mol)
|
a. |
2.94 |
|
b. |
5.79 |
|
c. |
6.35 |
|
d. |
7.06 |
|
e. |
7.60 |
18. How many g of KOH are
contained in 400. mL of
0.250 M KOH solution?
|
a. |
5.61 g |
|
b. |
8.98 g |
|
c. |
12.4 g |
|
d. |
35.1 g |
|
e. |
89.8 g |
19. The number of mol of sulfate
ions in a 0.1 liter solution of 0.02 M Al2(SO4)3
is
|
a. |
0.002 mol |
|
b. |
0.004 mol |
|
c. |
0.006 mol |
|
d. |
0.024 mol |
|
e. |
0.06 mol |
20. What volume of 0.750 molar H2SO4
must be taken to obtain 0.273 moles of H2SO4?
|
a. |
0.205 L |
|
b. |
0.364 L |
|
c. |
1.12 L |
|
d. |
2.74 L |
|
e. |
3.00 L |
21. Which one of the following is an example of an oxidation-reduction
reaction?
|
a. |
SO3(g) + H2O(l)
--> H2SO4(aq) |
|
b. |
P4O10(s) +
6Na2O(s) --> 4Na3PO4(s) |
|
c. |
I2(aq) + H2O(l) --> HOI(aq) + HI(aq) |
|
d. |
CaCO3(s) --> CaO(s) + CO2(g) |
|
e. |
Al2O3(s) +
3H2O(aq) + 2OH-(aq) --> 2Al(OH)4-(aq) |
22. What volume of 0.500 molar
nitric acid, HNO3, is required to react with 3.70 g of calcium
hydroxide, Ca(OH)2, according to the
following equation?
|
a. |
25.0 mL |
|
b. |
50.0 mL |
|
c. |
82.0 mL |
|
d. |
100.0 mL |
|
e. |
200.0 mL |
2HNO3 + Ca(OH)2 --> Ca(NO3)2 +
2H2O
|
|
23. How many mL
of 0.300 M NaOH are required to react with 500. mL of 0.170 M H3PO4
to yield Na2HPO4? (First write a balanced equation.)
|
a. |
94.4 |
|
b. |
142 |
|
c. |
283 |
|
d. |
567 |
|
e. |
850 |
24. To prepare 100. ml of 0.50 M HCl from 2.00 M HCl, what volume of acid must you use?
|
a. |
25.0 ml |
|
b. |
50.0 ml |
|
c. |
100. ml |
|
d. |
200. ml |
|
e. |
400. ml |
25. How many grams of PbCl2
would be precipitated if an excess of Pb(NO3)2 solution were added to 75.0 mL of 0.200 M KCl solution?
(Formula mass PbCl2 = 278.1 g mol-1)
|
a. |
1.04 |
|
b. |
2.09 |
|
c. |
4.17 |
|
d. |
8.34 |
|
e. |
41.7 |