Chem 1441 Test Questions from Previous Exams Page 1 of 7
Test 2 – Chapters 4 and 5 (Rogers Textbook)
Chapter 4 – Reactions in Aqueous Solutions
1. What mass of solute is contained in 125.0 mL of 1.50 M potassium chlorate solution?
a) 20.0 g
b) 23.0 g
c) 26.0 g
d) 30.3 g
e) 33.3 g
2. What is the final concentration if 10.0 mL of a 0.500 M NaOH solution is diluted to a volume of
500.0 mL?
a) 0.0100 M
b) 0.00500 M
c) 0.0250 M
d) 0.0200 M
e) 0.0125 M
3. A solution was prepared by dissolving 4.75 g of NaCl and 0.575 g of CaCl 2 in water and diluting to a volume of 500.0 mL.
What is the molarity of chloride ions in this solution?
a) 0.183 M
b) 0.163 M
c) 0.173 M
d) 0.0104 M
e) 0.233 M
4. A solution of ethanol (C2H5OH) is prepared by dissolving 35.0 mL of ethanol in enough water to make 120.0 mL of solution.
What is the molarity of the ethanol in this solution? (The molar mass of ethanol is 46.07 g/mol, and the density of ethanol is
0.790 g/mL.)
a) 17.0 M
b) 13.9 M
c) 8.67 M
d) 8.01 M
e) 5.00 M
5. What volume of 0.125 M nitric acid is required to completely neutralize 25.0 mL of 0.100 M barium hydroxide?
a) 20.0 mL
b) 25.0 mL
c) 40.0 mL
d) 10.0 mL
e) 35.0 mL
6. When 25.0 mL of 0.500 M AgNO3 solution is mixed with 40.0 mL of 0.250 M Na 2SO4, solid Ag2SO4 precipitates out. What
mass of Ag2SO4 is formed?
(The molar mass of Ag2SO4 is 311.8 g/mol.)
a) 1.95 g
b) 3.90 g
c) 3.12 g
d) 1.56 g
e) 7.80 g
, Chem 1441 Test Questions from Previous Exams Page 2 of 7
Test 2 – Chapters 4 and 5 (Rogers Textbook)
7. Which statement below best describes the difference between a strong electrolyte and a weak electrolyte?
a) A strong electrolyte is strongly conducting because it releases a lot of electrons when dissolved in water; a weak electrolyte
is weakly conducting because it releases few electrons when dissolved in water.
b) A strong electrolyte is more soluble in water than a weak electrolyte.
c) A strong electrolyte will react with a weak acid or a weak base; a weak electrolyte will not react with a weak acid or a
weak base.
d) A strong electrolyte completely dissociates into ions while a weak electrolyte only partially dissociates.
e) A strong electrolyte will participate in a precipitation reaction; a weak electrolyte will not.
8. Which of the following substances are strong electrolytes?
I. HF
II. NH4NO3
III. Ba(OH)2
IV. H2CO3
V. KBr
a) I and IV
b) II and V
c) II, III, and V
d) III, IV, and V
e) I, II, III, IV, and V
9. Which of the compounds listed below are weak electrolytes?
I. AgNO3
II. Ba(OH)2
III. NH3
IV. H2SO3
V. HBr
a) IV only
b) I and II
c) II, IV, and V
d) III and IV
e) III only
10. Which of the following salts is considered insoluble in water?
a) NaCl
b) Al(NO3)2
c) Mg(ClO4)2
d) K 2S
e) AgI
11. Which of the compounds listed below are insoluble in water?
I. MgBr2
II. K2CrO4
III. BaSO4
IV. Fe(OH)3
a) I and III
b) I and IV
c) III and IV
d) I, III and IV
e) I, II, III, and IV
12. A precipitate is expected when an aqueous solution of potassium sulfate is added to an aqueous solution of
a) ammonium sulfite
b) sodium hydroxide
c) copper(II) nitrate
d) magnesium bromide
e) lead(II) perchlorate
Test 2 – Chapters 4 and 5 (Rogers Textbook)
Chapter 4 – Reactions in Aqueous Solutions
1. What mass of solute is contained in 125.0 mL of 1.50 M potassium chlorate solution?
a) 20.0 g
b) 23.0 g
c) 26.0 g
d) 30.3 g
e) 33.3 g
2. What is the final concentration if 10.0 mL of a 0.500 M NaOH solution is diluted to a volume of
500.0 mL?
a) 0.0100 M
b) 0.00500 M
c) 0.0250 M
d) 0.0200 M
e) 0.0125 M
3. A solution was prepared by dissolving 4.75 g of NaCl and 0.575 g of CaCl 2 in water and diluting to a volume of 500.0 mL.
What is the molarity of chloride ions in this solution?
a) 0.183 M
b) 0.163 M
c) 0.173 M
d) 0.0104 M
e) 0.233 M
4. A solution of ethanol (C2H5OH) is prepared by dissolving 35.0 mL of ethanol in enough water to make 120.0 mL of solution.
What is the molarity of the ethanol in this solution? (The molar mass of ethanol is 46.07 g/mol, and the density of ethanol is
0.790 g/mL.)
a) 17.0 M
b) 13.9 M
c) 8.67 M
d) 8.01 M
e) 5.00 M
5. What volume of 0.125 M nitric acid is required to completely neutralize 25.0 mL of 0.100 M barium hydroxide?
a) 20.0 mL
b) 25.0 mL
c) 40.0 mL
d) 10.0 mL
e) 35.0 mL
6. When 25.0 mL of 0.500 M AgNO3 solution is mixed with 40.0 mL of 0.250 M Na 2SO4, solid Ag2SO4 precipitates out. What
mass of Ag2SO4 is formed?
(The molar mass of Ag2SO4 is 311.8 g/mol.)
a) 1.95 g
b) 3.90 g
c) 3.12 g
d) 1.56 g
e) 7.80 g
, Chem 1441 Test Questions from Previous Exams Page 2 of 7
Test 2 – Chapters 4 and 5 (Rogers Textbook)
7. Which statement below best describes the difference between a strong electrolyte and a weak electrolyte?
a) A strong electrolyte is strongly conducting because it releases a lot of electrons when dissolved in water; a weak electrolyte
is weakly conducting because it releases few electrons when dissolved in water.
b) A strong electrolyte is more soluble in water than a weak electrolyte.
c) A strong electrolyte will react with a weak acid or a weak base; a weak electrolyte will not react with a weak acid or a
weak base.
d) A strong electrolyte completely dissociates into ions while a weak electrolyte only partially dissociates.
e) A strong electrolyte will participate in a precipitation reaction; a weak electrolyte will not.
8. Which of the following substances are strong electrolytes?
I. HF
II. NH4NO3
III. Ba(OH)2
IV. H2CO3
V. KBr
a) I and IV
b) II and V
c) II, III, and V
d) III, IV, and V
e) I, II, III, IV, and V
9. Which of the compounds listed below are weak electrolytes?
I. AgNO3
II. Ba(OH)2
III. NH3
IV. H2SO3
V. HBr
a) IV only
b) I and II
c) II, IV, and V
d) III and IV
e) III only
10. Which of the following salts is considered insoluble in water?
a) NaCl
b) Al(NO3)2
c) Mg(ClO4)2
d) K 2S
e) AgI
11. Which of the compounds listed below are insoluble in water?
I. MgBr2
II. K2CrO4
III. BaSO4
IV. Fe(OH)3
a) I and III
b) I and IV
c) III and IV
d) I, III and IV
e) I, II, III, and IV
12. A precipitate is expected when an aqueous solution of potassium sulfate is added to an aqueous solution of
a) ammonium sulfite
b) sodium hydroxide
c) copper(II) nitrate
d) magnesium bromide
e) lead(II) perchlorate
