Chapter 4 Problems 1. Which of these compounds is a strong electrolyte?  A. H2O B. O2 C. H2SO4 D. C6H12O6 (glucose) E. CH3COOH (acetic acid) 2. Which of these compounds is a nonelectrolyte?  A. NaF B. HNO3 C. CH3COOH (acetic acid) D. NaOH E. C6H12O6 (glucose) 3. Based on the solubility rules, which one of these compounds should be insoluble in water?  A. NaCl B. MgBr2 C. FeCl2 D. AgBr E. ZnCl2 4. Based on the solubility rules, which of these processes will occur when a solution containing about 0.1 g of Pb(NO3)2(aq) is mixed with a solution containing 0.1 g of KI(aq)/100 mL?  A. KNO3 will precipitate; Pb2+ and I- are spectator ions. B. No precipitate will form. C. Pb(NO3)2 will precipitate; K+ and I- are spectator ions. D. PbI2 will precipitate; K+ and NO3- are spectator ions. E. Pb2+ and I- are spectator ions, and PbI2 will precipitate. 5. Give the oxidation # for the following atoms: a. N in NaNO3 _________ b. Mn in KMnO4 _________ c. Cl in ClO3- _________ 6. Which of these equations does not represent an oxidation-reduction reaction?   A. 3Al + 6HCl ( 3H2 + AlCl3 B. 2H2O ( 2H2 + O2 C. 2NaCl + Pb(NO3)2 ( PbCl2 + 3NaNO3 D. 2NaI + Br2 ( 2NaBr + I2 E. Cu(NO3)2 + Zn ( Zn(NO3)2 + Cu 7. What element is oxidized in the chemical reaction NiO2 + Cd + 2H2O ( Ni(OH)2 + Cd(OH)2?  A. Ni B. Cd C. O D. H E. This is not a redox reaction. 8. Which of these chemical equations describes a precipitation reaction?  A. 2H2(g) + O2(g) ( 2H2O(l) B. CaBr2(aq) + H2SO4(aq) ( CaSO4(s) + 2HBr(g) C. 2KNO3(s) ( 2KNO2(s) + O2(g) D. 2KBr(aq) + Cl2(g) ( 2KCl(aq) + Br2(l) E. 2Al(s) + 3H2SO4(aq) ( Al2(SO4)3(aq) + 3H2(g) 9. The common constituent in all acid solutions is  A. H2. B. H+. C. OH-. D. H2SO4. E. Cl-. 10. Which of these chemical equations describes an acid-base neutralization reaction?  A. 2Al(s) + 3H2SO4(aq) ( Al2(SO4)3(aq) + 3H2(g) B. SO2(g) + H2O(l) ( H2SO3(g) C. LiOH(aq) + HNO3(aq) ( LiNO3(aq) + H2O(l) D. 2KBr(aq) + Cl2(g) ( 2KCl(aq) + Br2(l) E. CaBr2(aq) + H2SO4(aq) ( CaSO4(s) + 2HBr(g) 11. Which of these chemical equations describes a combustion reaction?  A. 2C2H6(g) + 7O2(g) ( 4CO2(g) + 6H2O(l) B. LiOH(aq) + HNO3(aq) ( LiNO3(aq) + H2O(l) C. N2(g) + 3H2(g) ( 2NH3(g) D. 2Na(s) + 2H2O(l) ( 2NaOH(aq) + H2(g) E. 2Al(s) + 3H2SO4(aq) ( Al2(SO4)3(aq) + 3H2(g) 12. What is the molarity of a solution that contains 5.0 moles of solute in 2.00 liters of solution?  13. What mass of K2CO3 is needed to prepare 200. mL of a solution having a concentration of 0.150 M?  14. A 50.0 mL sample of 0.436 M NH4NO3 is diluted with water to a total volume of 250.0 mL. What is the ammonium nitrate concentration in the resulting solution?  15. During a titration the following data were collected. A 10. mL portion of an unknown monoprotic acid solution was titrated with 1.0 M NaOH; 40. mL of the base were required to neutralize the sample. What is the molarity of the acid solution?  16. 34.62 mL of.

1. Chapter 4 Problems
1.
Which of these compounds is a strong electrolyte?
A.
H2O
B.
O2
C.
H2SO4
D.
C6H12O6 (glucose)
E.
CH3COOH (acetic acid)
2. Which of these compounds is a nonelectrolyte?
A.
NaF
B.
HNO3
C.
CH3COOH (acetic acid)
D.
NaOH
E.
C6H12O6 (glucose)

2. 3. Based on the solubility rules, which one of these compounds
should be insoluble in water?
A.
NaCl
B.
MgBr2
C.
FeCl2
D.
AgBr
E.
ZnCl2
4. Based on the solubility rules, which of these processes will
occur when a solution containing about 0.1 g of Pb(NO3)2(aq)
is mixed with a solution containing 0.1 g of KI(aq)/100 mL?
A.
KNO3 will precipitate; Pb2+ and I- are spectator ions.
B.
No precipitate will form.
C.
Pb(NO3)2 will precipitate; K+ and I- are spectator ions.
D.
PbI2 will precipitate; K+ and NO3- are spectator ions.
E.
Pb2+ and I- are spectator ions, and PbI2 will precipitate.
5. Give the oxidation # for the following atoms:

3. a. N in NaNO3 _________
b. Mn in KMnO4 _________
c. Cl in ClO3- _________
6. Which of these equations does not represent an oxidation-
reduction reaction?
A.
3Al + 6HCl ( 3H2 + AlCl3
B.
2H2O ( 2H2 + O2
C.
2NaCl + Pb(NO3)2 ( PbCl2 + 3NaNO3
D.
2NaI + Br2 ( 2NaBr + I2
E.
Cu(NO3)2 + Zn ( Zn(NO3)2 + Cu
7. What element is oxidized in the chemical reaction
NiO2 + Cd + 2H2O ( Ni(OH)2 + Cd(OH)2?
A.
Ni
B.
Cd
C.
O
D.

4. H
E.
This is not a redox reaction.
8. Which of these chemical equations describes a precipitation
reaction?
A.
2H2(g) + O2(g) ( 2H2O(l)
B.
CaBr2(aq) + H2SO4(aq) ( CaSO4(s) + 2HBr(g)
C.
2KNO3(s) ( 2KNO2(s) + O2(g)
D.
2KBr(aq) + Cl2(g) ( 2KCl(aq) + Br2(l)
E.
2Al(s) + 3H2SO4(aq) ( Al2(SO4)3(aq) + 3H2(g)
9.
The common constituent in all acid solutions is
A.
H2.
B.
H+.
C.
OH-.

5. D.
H2SO4.
E.
Cl-.
10. Which of these chemical equations describes an acid-base
neutralization reaction?
A.
2Al(s) + 3H2SO4(aq) ( Al2(SO4)3(aq) + 3H2(g)
B.
SO2(g) + H2O(l) ( H2SO3(g)
C.
LiOH(aq) + HNO3(aq) ( LiNO3(aq) + H2O(l)
D.
2KBr(aq) + Cl2(g) ( 2KCl(aq) + Br2(l)
E.
CaBr2(aq) + H2SO4(aq) ( CaSO4(s) + 2HBr(g)
11. Which of these chemical equations describes a combustion
reaction?
A.
2C2H6(g) + 7O2(g) ( 4CO2(g) + 6H2O(l)
B.
LiOH(aq) + HNO3(aq) ( LiNO3(aq) + H2O(l)
C.
N2(g) + 3H2(g) ( 2NH3(g)

6. D.
2Na(s) + 2H2O(l) ( 2NaOH(aq) + H2(g)
E.
2Al(s) + 3H2SO4(aq) ( Al2(SO4)3(aq) + 3H2(g)
12.
What is the molarity of a solution that contains 5.0 moles of
solute in 2.00 liters of solution?
13. What mass of K2CO3 is needed to prepare 200. mL of a
solution having a concentration of 0.150 M?
14. A 50.0 mL sample of 0.436 M NH4NO3 is diluted with
water to a total volume of 250.0 mL. What is the ammonium
nitrate concentration in the resulting solution?
15. During a titration the following data were collected. A 10.
mL portion of an unknown monoprotic acid solution was titrated
with 1.0 M NaOH; 40. mL of the base were required to
neutralize the sample. What is the molarity of the acid
solution?
16. 34.62 mL of 0.1510 M NaOH was needed to neutralize 50.0
mL of an H2SO4 solution. What is the concentration of the
original sulfuric acid solution?
17. Which substance is acting as a Brønsted acid in the
following reaction?
HSO4- + NH4+ ( H2SO4 + NH3
18. Zinc dissolves in hydrochloric acid to yield hydrogen gas:
Zn(s) + 2HCl(aq) ( ZnCl2(aq) + H2(g)
What mass of hydrogen gas is produced when a 7.35 g chunk of
zinc dissolves in 500. mL of 1.200 M HCl? (Solve this the
same way you would any stoichiometry problem. First convert
both reagents to moles. For the HCl, use the molarity
equation).

7. 19. Complete and balance the following molecular equation
(including states of matter). Then write the ionic and net ionic
equations.
Fe2(SO4)3 + Na2S (
Chapter 3 Problems
1. If 0.274 moles of a substance weighs 62.5 g, what is the
molar mass of the substance, in units of g/mol?
2. Which of these quantities does not represent 1.00 mol of the
indicated substance?
A. 6.02 ( 1023 C atoms
B.
26.0 g Fe
C.
12.01 g C
D.
65.4 g Zn
E.
6.02 ( 1023 Fe atoms
3. How many silicon atoms are there in 1.00 g of silicon?
4. Determine the number of moles of aluminum in 96.7 g of Al.
5. What is the molar mass of acetaminophen, C8H9NO2?
6. What is the mass of 0.0250 mol of P2O5?

8. 7. The molecular formula of aspirin is C9H8O4. How many
aspirin molecules are present in one 500-milligram tablet?
8. How many moles is 25.7 g of CaSO4?
9. What is the mass of 8.25 ( 1019 UF6 molecules?
10. Calculate the percent composition by mass of all elements in
Na2CO3.
11. What is the empirical formula of a compound of uranium
and fluorine that is composed of 67.6% uranium and 32.4%
fluorine?
12. The percent composition by mass of a compound is 76.0%
C, 12.8% H, and 11.2% O. The molar mass of this compound is
284.5 g/mol. What is the molecular formula of the compound?
13. Balance the following equation with the smallest set of
whole numbers.
___ Na + ___ H2O ( ___ NaOH + ___ H2
14. Balance the following equation with the smallest set of
whole numbers.
__ C2H4 + __ O2 ( __ CO2 + __ H2O
15. Balance the following equation using the smallest set of
whole numbers.
___ Al + ___ H2SO4 ( ___ Al2(SO4)3 + ___ H2

9. 16. Aluminum hydroxide reacts with nitric acid to form
aluminum nitrate and water. What mass of water can be formed
by the reaction of 15.0 g of aluminum hydroxide with excess
nitric acid?
Al(OH)3 + 3HNO3 ( Al(NO3)3 + 3H2O
17. Ammonia reacts with diatomic oxygen to form nitric oxide
and water vapor:
4NH3 + 5O2 ( 4NO + 6H2O
When 40.0 g NH3 and 50.0 g O2 are allowed to react, which is
the limiting reagent? How many grams of NO are produced?
18. How many grams of Cl2 can be prepared from the reaction
of 16.0 g of MnO2 and 30.0 g of HCl according to the following
chemical equation?
MnO2 + 4HCl ( MnCl2 + Cl2 + 2H2O
19. Hydrochloric acid can be prepared by the following
reaction:
2NaCl(s) + H2SO4(aq) ( 2HCl(g) + Na2SO4(s)
How many grams of HCl can be prepared from 2.00 mol H2SO4
and 150 g NaCl?
20. Calculate the mass of SO3 that can be produced by the
reaction of 90.0 g of SO2 and 100.0 g of O2.
2SO2 + O2 ( 2SO3
21. The first step in the Ostwald process for producing nitric

10. acid is
4NH3(g) + 5O2(g) ( 4NO(g) + 6H2O(g).
If the reaction of 150. g of ammonia with 150. g of oxygen gas
yields 87. g of nitric oxide (NO), what is the percent yield of
this reaction?
22. What is the theoretical yield of aluminum that can be
produced by the reaction of 60.0 g of aluminum oxide with 30.0
g of carbon according to the following chemical equation?
Al2O3 + 3C ( 2Al + 3CO
22b. How many grams of the excess reagent remains?
23. Calculate the mass of FeS formed when 9.42 g of Fe reacts
with 8.50 g of S.
Fe(s) + S(s) ( FeS(s)
23b. How many grams of the excess reagent remains?