25) When an acid reacts with a metal, what is one of the usual products?
A) water
B) salt
C) carbon dioxide
D) hydrogen gas
E) none of the above
26) A 25.0 mL sample of 0.105 M HCl was titrated with of NaOH. What is the
concentration of the NaOH?
A) 0.0833 M
B) 0.132 M
C) 0.105 M
D) 0.075 M
E) none of the above
27) A 35.0 mL sample of 0.225 M HBr was titrated with 42.3 mL of KOH. What is the
concentration of the KOH?
A) 0.157 M
B) 0.303 M
C) 0.272 M
D) 0.186 M
E) none of the above
28) Exactly 17.0 mL of a H2SO4 solution was required to neutralize 45.0 mL of 0.235 M NaOH.
What was the concentration of the H2SO4 solution?
Given: H2SO4 (aq) + 2NaOH (aq) → 2H2O (l) + Na2SO4 (aq)
A) 5.63 M
B) 0.622 M
C) 0.00529 M
D) 0.311 M
E) none of the above
29) Pure water cannot conduct electricity so why do we have to be careful with electrical
appliances near water?
A) OSHA regulations
B) Water can be broken down by electricity.
C) Water always has some ions dissolved in it.
D) Water dissociates fully into its ions.
E) none of the above
30) Which of the following acids is diprotic?
A) HCl
B) HN
C) HI
D)
E) none of the above
31) Which of the following acids is a diprotic, weak acid?
A) sulfuric acid
B) phosphoric acid
C) hydrobromic acid
D) carbonic acid
E) none of the above
32) Which of the following acids is a monoprotic, strong acid?
A) sulfuric acid
B) phosphoric acid
C) hydrobromic acid
D) carbonic acid
E) none of the above
33) Which of the following is a weak base?
A) calcium hydroxide
B) sodium fluoride
C) potassium hydroxide
D) ammonia
E) none of the above
34) In which solution is the [H3O+] less than 0.250 M?
A) 0.250 M HC2H3O2 (aq)
B) 0.250 M HF (aq)
C) 0.250 M HCO2 (aq)
D) all of these
E) none of these
35) A 0.10 M solution of an electrolyte has a pH of 4.5. The electrolyte is:
A) a strong acid.
B) a strong base.
C) a weak acid.
D) a weak base.
E) none of the above
36) What is the concentration of H⁺ in 2.0 M acetic acid, HC2H3O2?
A) 1.0 M
B) 2.0 M
C) >2.0 M
D) < 2.0 M
E) none of the above
37) What is the concentration of H⁺ in 0.50 M hydroiodic acid?
A) 0.50 M
B) 1.0 M
C) <0.50 M
D) 1.50 M
E) none of the above
38) Ammonia (NH3) ionizes in water to form a basic solution. What is the concentration of OH–
ions in a 0.75 M NH3 solution?
A) 0.75 M
B) < 0.75 M
C) > 0.75 M
D) No OH– ions exist in a solution of NH3.
E) none of the above
39) Consider a 1.6 × 10-3 M solution of HNO3. Which of the following statements is NOT true?
A) This solution would turn litmus to red.
B) This solution could neutralize a base.
C) This solution has a pH of 11.20.
D) This solution could dissolve metal.
E) none of the above
40) Substances that can act both as an acid and as a base are called:
A) neutral.
B) buffers.
C) indicators.
D) amphoteric.
E) none of these
41) What is the value of the ion product constant for water ( )?
A) 0.0
B) 1.0
C) 1.0
D) 1.0
E) 1.0
42) What is the concentration of the hydroxide ion given that the concentration of the hydronium
ion is ?
A) 6.7 × M
B) 1.5 M
C) 1.0 M
D) 1.0 M
E) none of the above
43) What is the concentration of the hydronium ions in an acidic solution?
A) 0.0 M
B) 1.0 M
C) 1.0 M
D) > 1.0 M
E) < 1.0 M
44) The pH of a solution is 5.00. Which of the following is TRUE about the solution?
A) Its [H3O+] is 1.0 × 10-9 M
B) Its [H3O+] is 1.0 × 10-5 M
C) Its [H3O+] is 1.0 × 105 M
D) It is more acidic than a solution whose pH is 4.00.
E) none of the above
45) What is the concentration of the hydronium ions in a neutral solution?
A) 0.0 M
B) 1.0 M
C) 1.0 M
D) > 1.0 M
E) < 1.0 M
46) What is the concentration of hydronium ions in a solution given that the concentration of
hydroxide ions is 2.31 × 10-4 M?
A) 4.33 × 10-11 M
B) 2.31 × 1010 M
C) 2.31 × 10-18 M
D) 1.01 × 10-5 M
E) none of the above
47) Which solution below has the highest concentration of hydroxide ions?
A) pH = 3.21
B) pH = 12.49
C) pH = 7.00
D) pH = 10.12
E) pH = 7.93
48) In order for a solution to be acidic:
A) [H3O+] < [OH–]
B) [H3O+] > [OH–]
C) [H3O+] = [OH–]
D) pH = pOH
E) none of the above
49) In order for a solution to be basic:
A) [H3O+] > [OH–]
B) [H3O+] < [OH–]
C) [H3O+] = [OH–]
D) pH = pOH
E) none of the above
50) What is the concentration of the hydroxide ions in an acidic solution?
A) 0.0 M
B) 1.0 M
C) 1.0 M
D) > 1.0 M
E) < 1.0 M
51) In a solution that has a pH = 7.0:
A) [H3O+] > [OH–]
B) [H3O+] < [OH–]
C) [H3O+] = [OH–]
D) [H3O+] + [OH–] = Kw
E) none of the above
52) A solution at 25°C has a hydrogen ion concentration of 2.6 × 10-5 M. Which of the
following is TRUE?
A) [H3O+] > [OH–]
B) [H3O+] < [OH–]
C) [H3O+] = [OH–]
D) [H3O+] =
E) none of the above
53) What is the pH of a solution that has a H⁺ concentration equal to ?
A) 4.77
B) 5.20
C) 0.22
D) 10.20
E) none of the above
54) Consider a 1.0 M HCl solution and a 1.0 M NaOH solution. Which statement
below is true?
A) The HCl solution is acidic.
B) The NaOH solution is basic.
C) Only the HCl solution is neutral.
D) Only the NaOH solution is neutral.
E) Both of these solutions are neutral.
55) If the pH of an aqueous solution changed from 9.10 to 4.67, what happened to the hydronium
ion concentration?
A) It decreased.
B) It became zero.
C) It became less than zero.
D) It increased.
E) none of the above
56) What is the [H⁺] in a solution that has a pH of 3.35?
A) 1 × M
B) 2.2 × M
C) 4.5 × M
D) 3.35 × M
E) none of the above
57) What is the pOH of a solution that has a OH– concentration equal to ?
A) 9.89
B) 4.29
C) -4.3
D) 4.12
E) none of the above
58) What is the [OH–] in a solution that has a pOH of 9.65?
A) 4.5 × M
B) 4.5 × M
C) 9.8 × M
D) 2.2 × M
E) none of the above
59) Which solution below is considered to have basic character?
A) pOH = 7
B) pH = 2
C) pOH = 4
D) pOH = 13
E) none of the above
60) Which of the following is TRUE of alkaloid compounds?
A) Alkaloids are organic bases.
B) Alkaloids occur naturally in many plants.
C) Some narcotic drugs are alkaloids.
D) Some alkaloids are addictive.
E) All of the above are true.
61) A buffer solution is all of the following EXCEPT:
A) a solution that resists a change in pH when a base is added.
B) a solution that resists a change in pH when an acid is added.
C) a solution that contains both a weak acid and its conjugate base.
D) a solution that regulates pH because it is such a strong acid or base.
E) All of the above are true.
62) Which of the following statements are TRUE of buffer solutions?
1. A buffer solution can be made by mixing equal concentrations of
acetic acid and sodium acetate.
2. A buffer solution can be made by mixing equal concentrations of
hydrochloric acid and sodium chloride.
3. A buffer solution resists changes in pH when small quantities of acid
or base are added.
A) 1 and 2 only
B) 2 and 3 only
C) 1 and 3 only
D) All of 1, 2, and 3
E) None of 1, 2, and 3
63) Which combination below will be a buffer solution?
A) HCl and Cl⁻
B) HNO3 and NaNO3
C) H and Na
D) NaBr and NaOH
E) All of the above are true.
64) Which of the following contributes to acid rain?
A) The use of volatile acids in industry.
B) The reaction of metal oxides with water.
C) The reaction of nonmetal oxides with water.
D) The reaction of alkali metals with water.
E) all of the above
65) Acid rain legislation targeted the release of which compound by industry?
A) C
B) S
C) dioxin
D) benzene
E) none of the above
14.3 Algorithmic Questions
1) The titration of 25.00 mL a 0.125 M HCl solution required 21.37 mL of KOH to reach the
endpoint. What is the concentration of the KOH?
A) 0.292 M
B) 0.0668 M
C) 0.146 M
D) 0.134 M
E) none of the above
2) What is the concentration of in a 0.121 M HCl solution?
A) 1.0 M
B) < 0.121 M
C) 0.121 M
D) not enough information
E) none of the above
3) What is the concentration of in solution given the [OH⁻] = 2.54 × ?
A) 3.94 × M
B) 2.54 × M
C) 1.0 × M
D) not enough information
E) none of the above
4) What is the pH of a solution that has a [ ] = 0.0045 M?
A) 1.35
B) 2.35
C) 3.35
D) 7.0045
E) none of the above
5) What is the pH of a solution that has a [ ] = 0.0033 M?
A) 2.48
B) 7.0033
C) 11.52
D) 3.3
E) none of the above
6) Which solution below would be considered the most acidic?
A) 2.9 × 10 -4 M HCl
B) 4.5 × 10 -5 M HNO3
C) 1.0 × 10 -7 M NaCl
D) 1.5 × 10 -2 M KOH
E) none of the above
7) What is the concentration of in a solution with pH = 2.50?
A) 4.5 M
B) 1.3 M
C) 0.0032 M
D) 0.40 M
E) none of the above