47) How many moles of H2O are produced when 1 mole of Mg(OH)2 reacts with 1 mole of H2SO4?
A) 1
B) 2
C) 3
D) 4
E) 5
48) In a neutralization reaction, how many moles of HClO4 react with 1 mole of Al(OH)3?
A) 1
B) 2
C) 3
D) 4
E) 5
49) Which of the following is a neutralization reaction?
A) KCl + NaNO3→ KNO3 + NaCl
B) HNO3+ KOH → H2O + KNO3
C) H2O + SO3 → H2SO4
D) 4Na + O2 → 2Na2O
E) 2NO2 → 2NO + O2
50) 25.0 mL of 0.212 M NaOH is neutralized by 13.6 mL of an HCl solution. The molarity of the HCl
solution is
A) 0.212 M.
B) 0.115 M.
C) 0.500 M.
D) 0.390 M.
E) 0.137 M.
51) What is the molarity of a KOH solution if 25.0 mL neutralizes 35.0 mL of a 0.200 M HCl solution?
A) 0.267 M
B) 0.143 M
C) 0.200 M
D) 0.280 M
E) 0.100 M
52) A 25.0 mL sample of H3PO4 requires 50.0 mL of 1.50 M NaOH for complete neutralization. What is
the molarity of the acid?
H3PO4 + 3NaOH →Na3PO4 + 3H2O
A) 0.333 M
B) 3.00 M
C) 1.50 M
D) 1.00 M
E) 0.750 M
53) A 25.0 mL sample of H2SO4 requires 20.0 mL of 2.00 M KOH for complete neutralization. What is the
molarity of the acid?
H2SO4 + 2KOH → K2SO4 + 2H2O
A) 2.00 M
B) 2.50 M
C) 0.800 M
D) 1.60 M
E) 1.25 M
54) A 10.0 mL of 0.121 M H2SO4 is neutralized by 17.1 mL of KOH solution. The molarity of the KOH
solution is
A) 0.207 M.
B) 0.4141 M.
C) 0.0708 M.
D) 0.428 M.
E) 0.142 M.
55) How many milliliters of 0.400 M NaOH are required to completely neutralize 20.0 mL of 0.200 M
HCl?
A) 50.0 mL
B) 40.0 mL
C) 0.100 mL
D) 20.0 mL
E) 10.0 mL
56) How many milliliters of 0.200 M NaOH are required to completely neutralize 5.00 mL of 0.100 M
H3PO4?
A) 7.50 mL
B) 2.50 mL
C) 0.833 mL
D) 5.00 mL
E) 15.0 mL
57) How many milliliters of 0.100 M Ba(OH)2 are required to neutralize 20.0 mL of 0.250 M HCl?
A) 100. mL
B) 50.0 mL
C) 25.0 mL
D) 0.250 mL
E) 0.50 mL
For the problem(s) that follow, consider the reaction in which magnesium reacts with an HCl solution .
Mg(s) + 2HCl(aq) → MgCl2 (aq) + H2(g)
58) If 2.00 g of Mg reacts completely with 50.0 mL of HCl solution, what is the molarity of the HCl
solution?
A) 1.65 M
B) 80.0 M
C) 8.00 M
D) 0.823 M
E) 3.29 M
59) The function of a buffer is to
A) change color at the end point of a titration.
B) maintain the pH of a solution.
C) be a strong base.
D) maintain a neutral pH.
E) act as a strong acid.
60) The normal blood pH is about
A) 6.8.
B) 7.0.
C) 7.2.
D) 7.4.
E) 7.6.
61) In a buffer system of HF and its salt, NaF,
A) the HF neutralizes added acid.
B) the HF neutralizes added base.
C) the HF is not necessary.
D) the F– neutralizes added H2O.
E) the F– neutralizes added base.
62) Which of the following is a buffer system?
A) NaCl and NaNO3
B) HCl and NaOH
C) H2CO3 and KHCO3
D) NaCl and NaOH
E) H2O and HCl
63) Which of the following could be a buffer?
A) NaF
B) HF + NaF
C) HF + H2O
D) NaF + H2O
E) NaCl + HF
64) What is the name of the medical condition of an asthmatic patient with a blood pH of 7.30?
A) respiratory acidosis
B) respiratory alkalosis
C) metabolic acidosis
D) metabolic alkalosis
E) diabetes mellitus
65) If a condition of hyperventilation occurs, the blood pH of the patient is expected to
A) saturate.
B) increase.
C) decrease.
D) stay the same.
E) concentrate.
66) When hyperventilation (rapid breathing) causes a patient to exhale large amounts of CO2, the blood
pH rises in a condition called
A) metabolic acidosis.
B) metabolic alkalosis.
C) respiratory acidosis.
D) respiratory alkalosis.
E) pulmonary distress.
67) Which solution has the highest pH?
A) a buffer made with 0.10 M acetic acid and 0.01 M sodium acetate
B) a buffer made with 0.10 M acetic acid and 0.10 M sodium acetate
C) a buffer made with 0.01 M acetic acid and 0.10 M sodium acetate
D) a buffer made with 0.01 M acetic acid and 0.01 M sodium acetate
E) All of the buffers have the same pH since they are all made with acetic acid and sodium acetate.
68) Which solution has the lowest pH?
A) a buffer made with 0.10 M acetic acid and 0.01 M sodium acetate
B) a buffer made with 0.10 M acetic acid and 0.10 M sodium acetate
C) a buffer made with 0.01 M acetic acid and 0.10 M sodium acetate
D) a buffer made with 0.01 M acetic acid and 0.01 M sodium acetate
E) All of the buffers have the same pH since they are all made with acetic acid and sodium acetate.
11.2 Short Answer Questions
1) The name of HCl is________.
2) The conjugate acid of H2PO42- is ________.
3) Identify the conjugate acid-base pairs in the following reaction:
HCl + NH3 → NH4+ + Cl–
4) Write the proper Ka expression for the ionization of acetic acid, HC2H3O2.
5) If an acid has a Ka << 1, is it classified as a weak acid or a strong acid?
6) The pH of 0.0010 M HCl is ________.
7) The pH of 0.0001 M KOH is ________.
8) In a titration experiment, a student used 24.13 mL of 0.111 M sodium hydroxide to neutralize 20.00 mL
of a hydrochloric acid solution. What was the molarity of the acid solution?
9) A student had 2.0 L of a sodium hydroxide solution that had a concentration of 0.4000 M. The student
needed to make 500 mL of a 0.1000 M solution. How many mL of the concentrated solution was needed?
10) A student had 25.0 mL of 0.100 M H2SO4 solution. How many mL of a 0.100 M NaOH solution will
the sulfuric acid neutralize?
11) What is the pH of a buffer made with 0.10 M acetic acid and 0.01 M sodium acetate?
11.3 True/False Questions
1) HCl is hydrochlorous acid.
2) The conjugate base of HCl is Cl–.
3) HCl is a strong acid.
4) A strong acid is completely dissociated in water.
5) In any water solution, [H3O+][OH–] = 1.0 × 10-7.
6) The pH of 0.001 M HCl is 12.0.
7) A solution with a pH of 4.0 is more acidic than a solution with a pH of 6.0.
8) A solution with a pH of 4.0 is basic.
9) Magnesium metal is not attacked by sulfuric acid solutions.
10) For most reactions of acids with bases, the resulting products are a salt and water.
11) If the carbon dioxide level in the blood is too high, more carbonic acid is produced, and this results in
the condition termed acidosis.
12) Alkalosis is the blood condition in which the blood pH is higher than normal.
13) A buffer is a solution that tends to maintain a neutral pH.
11.4 Matching Questions
Identify each of the following compounds as an acid, a base, or neither.
A) acid
B) base
C) neither
1) HCl
Objective: 11.1
Global Outcomes: GO2
2) NaOH
Objective: 11.1
Global Outcomes: GO2
3) NH3
Objective: 11.1
Global Outcomes: GO2
4) H2SO4
Objective: 11.1
Global Outcomes: GO2
5) CO32-
Objective: 11.1
Global Outcomes: GO2
6) NaCl
Objective: 11.1
Global Outcomes: GO2
7) CN–
Objective: 11.1
Global Outcomes: GO2
8) H2CO3
Objective: 11.1
Global Outcomes: GO2
In the following solutions, is the [OH–] greater than, less than, or equal to the [H3O+]?
A) less than
B) greater than
C) equal to
9) acid
Objective: 11.5
Global Outcomes: GO2
10) base
Objective: 11.5
Global Outcomes: GO2
11) [H3O+] = 1.0 × 10-6 M
Objective: 11.5
Global Outcomes: GO4
12) [H3O+] = 1.0 × 10–10 M
Objective: 11.5
Global Outcomes: GO4
13) [H3O+] = 1.0 × 10-7 M
Objective: 11.5
Global Outcomes: GO4
14) pH = 2
Objective: 11.5
Global Outcomes: GO4
15) pH = 9
Objective: 11.5
Global Outcomes: GO4
Identify the following as acids, bases, or neutral solutions.
A) neutral
B) acid
C) base
16) has a sour taste
Objective: 2.1
Global Outcomes: GO2
17) has a pH = 4.5
Objective: 2.1
Global Outcomes: GO2
18) turns blue litmus paper red
Objective: 2.1
Global Outcomes: GO2
19) contains more hydronium ions than hydroxide ions
Objective: 2.1
Global Outcomes: GO2
20) H2O
Objective: 2.1
Global Outcomes: GO2
21) [H3O+] = 3.4 × 10-5 M
Objective: 2.1
Global Outcomes: GO4
22) [OH–] = 2.8 × 10-2 M
Objective: 2.1
Global Outcomes: GO4
23) Ca(OH)2
Objective: 2.1
Global Outcomes: GO4
24) pH =9.0
Objective: 2.1
Global Outcomes: GO4
25) [H3O+] = 1.0 × 10-7 M
Objective: 2.1
Global Outcomes: GO4