59) Which of the following is the correct balanced equation for the neutralization of barium hydroxide
with hydrochloric acid?
A) Ba(OH)2 + 2 HCl → BaCl2 + 2 H2O
B) BaOH2 + 2 HCl → BaCl2 + H2O
C) Ba(OH)2 + HCl → BaCl2 + H2O
D) BaOH + HCl → BaCl + H2O
60) Which of the following is the correct balanced equation for the neutralization of barium hydroxide
with sulfuric acid?
A) Ba(OH)2 + H2SO4 → BaSO4 + 2 H2O
B) BaOH + H2SO4 → BaSO4 + 2 H2O
C) BaOH2 + H2SO4 → BaSO4 + H2O
D) Ba(OH)2 + 2 H2SO4 → Ba(SO4)2 + 2 H2O
61) Phenolphthalein has often been used to monitor the progress of an acid-base neutralization reaction.
What color will phenolphthalein be when there is an excess of acid present?
A) colorless
B) green
C) pink
D) yellow
62) Phenolphthalein has often been used to monitor the progress of acid-base neutralization reactions.
What color will phenolphthalein be if there is an excess of base present?
A) colorless
B) green
C) pink
D) yellow
63) What is produced in an acid-base neutralization reaction?
A) an acid
B) a base
C) a salt and water
D) an acid and water
64) A sample of rainwater has a pH of 3.5. What ion is sure to be present in relatively large concentration
in this rain sample?
A) H3O+
B) SO42-
C) OH–
D) HSO4–
65) The pH of a sample of water from a river is 6.0. A sample of effluent from a food processing plant has
a pH of 4.0. The concentration of hydronium ion in the effluent is
A) one and a half times (1.5x) larger than the river hydronium ion concentration.
B) two times (2x) larger than the river hydronium ion concentration.
C) four times (4x) larger than the river hydronium ion concentration.
D) 100 times (100x) larger than the river hydronium ion concentration.
66) A solution with a pH of 3 has a hydronium ion concentration of
A) 10-3 mol/L.
B) 103 mol/L.
C) 10 mol/L.
D) -10 mol/L.
67) A solution of toilet bowl cleaner has a pH of 9. The solution is
A) weakly basic.
B) strongly basic.
C) weakly acidic.
D) strongly acidic.
68) The pH = -log[H+] for a solution. The pOH = -log[OH–] for a solution. The pH and pOH are related,
and their sum is equal to 14 (pH + pOH = 14). If a solution has a pH of 6, what is the pOH?
A) 6
B) 7
C) 8
D) 14
69) A solution with a pH of 12 will be
A) weakly basic.
B) strongly basic.
C) weakly acidic.
D) neutral.
70) An unknown substance is added to a solution and the pH decreases. The substance is best described
as a(n)
A) acid.
B) base.
C) salt.
D) solvent.
71) An unknown substance is added to a solution and the pH increases. The substance is best described
as a(n)
A) acid.
B) base.
C) salt.
D) solvent.
72) Which substance has the lowest pH?
A) urine
B) lemon juice
C) unpolluted rainwater
D) 4% NaOH
73) Which substance has the highest pH?
A) bile
B) lemon juice
C) pure water
D) milk of magnesia
74) Identify the weakly basic solution.
A) urine
B) milk of magnesia
C) saliva
D) milk
75) The pH = -log[H+] for a solution. The pOH = -log[OH–] for a solution. The pH and pOH are related,
and their sum is equal to 14 (pH + pOH = 14). If the concentration of a dilute solution of potassium
hydroxide is 0.001 M, what is the pH of that solution?
A) 7
B) 3
C) 11
D) 2
76) If the concentration of a dilute solution of nitric acid is 0.0001 M, what is the pH of that solution?
A) 5
B) 4
C) 10
D) 3
77) Which of the following form a conjugate acid-base pair?
A) H2SO4 and SO42-
B) H3O+ and OH–
C) H2SO4 and HSO4–
D) CH4 and CH3OH
78) What is the conjugate acid of HSO3–?
A) H2SO4
B) H2SO3
C) HSO4–
D) SO32-
79) What is the conjugate base of HSO3–?
A) H2SO4
B) H2SO3
C) HSO4–
D) SO32-
80) A conjugate acid-base pair differ by one
A) H atom.
B) O atom.
C) pH unit.
D) proton.
81) A mixture of a weak acid and its conjugate base forms a(n)
A) acid-base indicator.
B) buffer.
C) antacid.
D) acid rain.
82) A buffer
A) resists changes in pH when small amounts of a strong acid or a strong base are added.
B) is made up of a weak acid and its conjugate base.
C) is made up of a weak base and its conjugate acid.
D) All of the above are true.
83) The pH of rain collected on a remote island in the Pacific is assumed to be unaffected by human
pollution. The pH of the rainwater will be
A) less than 7.
B) equal to 7.
C) greater than 7.
D) 0.
84) Which of the following does NOT contribute to acid rain?
A) coal-burning power plants
B) lightning
C) volcanic eruptions
D) All of the above contribute to acid rain.
85) Acid rain is caused by acidic pollutants in the air. Which of the following pollutants does NOT
contribute to acid rain?
A) ammonia, NH3
B) sulfur dioxide, SO2
C) nitrogen dioxide, NO2
D) nitric oxide, NO
86) By definition, acid rain has a pH
A) below 4.
B) below 5.6.
C) below 7.
D) above 8.5.
87) Rain with which of the following pH of values would be considered to be acid rain?
A) 9.5
B) 9.0
C) 7
D) 1.5
88) Hyperacidity means
A) too much acid.
B) too little acid.
C) too much antacid.
D) too much base.
89) Sodium bicarbonate is an old standby antacid. It is not recommended for persons suffering from high
blood pressure because
A) it is too strong an acid.
B) it is too strong a base.
C) of the presence of sodium ion.
D) of the presence of bicarbonate ion.
90) Sodium bicarbonate is the common name for what compound?
A) sodium carbonate
B) sodium carbide
C) sodium hydrogen carbonate
D) sodium bismuth carbonate
91) Sodium bicarbonate is commonly known as
A) baking soda.
B) baking powder.
C) washing soda.
D) cherry soda.
92) All antacids are
A) acids.
B) bases.
C) neutral.
D) salts.
93) Calcium carbonate is a common antacid. A problem with regular use of calcium carbonate based
antacids is they cause
A) constipation.
B) diarrhea.
C) high blood pressure.
D) destruction of the stomach lining.
94) Which antacid also acts as an antidiarrheal agent?
A) lithium hydroxide
B) nitric acid
C) lithium bicarbonate
D) calcium carbonate
95) Aluminum hydroxide is a popular antacid. The formula of aluminum hydroxide is
A) AlOH.
B) Al(OH)2.
C) Al(OH)3.
D) Al3OH.
96) When the pH of the blood is too high, the condition is called
A) acidosis.
B) alkalosis.
C) hyperacidity.
D) anemia.
97) Hard water deposits (calcium carbonate) have built up around your bathroom sink. Which one of the
following would be best to dissolve the deposit?
A) ammonia
B) bleach
C) lye
D) vinegar
98) The acid in automobile batteries is
A) hydrochloric acid.
B) nitric acid.
C) phosphorus acid.
D) sulfuric acid.
99) A common name for hydrochloric acid is
A) lye.
B) muriatic acid.
C) lime.
D) ammonia.
100) The cheapest and most widely used commercial base is
A) NH3 (ammonia).
B) Na2O (sodium oxide).
C) CaO (lime).
D) NaOH (lye).
101) Most of the sulfuric acid produced in this country is used for
A) cleaning products.
B) manufacturing mortar and cement.
C) manufacturing fertilizer.
D) sweetening acidic soil.
102) Another name for NaOH is
A) baking soda.
B) lime.
C) lye.
D) lysol.
103) Which of the following ingredients would NOT be an active ingredient in an antacid?
A) NaBr
B) Mg(OH)2
C) NaHCO3
D) CaCO3
104) Lutefisk is a traditional Scandinavian food that is prepared by soaking a white fish, such as cod, in
lye (NaOH). How does soaking the fish in lye “cook” it?
A) A strong base will allow the fish to be heated to higher temperatures more quickly.
B) A strong base will break down or “denature” the protein in the fish.
C) A strong base will neutralize the fatty acids in the fish.
D) A strong base will raise the pH of blood in the fish.
7.2 True/False Questions
1) Acid-base indicators will change color when the amount of acid present changes.
2) Many acid-base indicators can be extracted from fruit skins or flower petals.
3) Biodiesel fuels are more toxic to the environment than petroleum fuels are.
4) The production of biodiesel fuel and of soap both require the addition of base and both produce
glycerol.
5) If a compound is a base according to the Arrhenius definition, it will also be a base according to the
Bronsted-Lowry definition.
6) The Arrhenius theory explains why ammonia, NH3, is basic, but the Bronsted-Lowry theory does not.
7) A metal oxide will form an acid when it is dissolved in water.
8) Most acids are strong acids.
9) A strong acid will not ionize completely in water.
10) A weak acid will always be less concentrated than a strong acid.
11) When an acid and a base react in a neutralization reaction, the products will be acidic.
12) A solution which has more H+ ions than OH– ions will have a pH equal to 7.
13) Rainwater has a pH below 7 because raindrops absorb CO2 which can react with water to form
carbonic acid.
14) A conjugate acid-base pair form a buffer solution.
15) A buffer solution will become much more acidic when even a small amount of a strong acid is added.
16) Antacids are basic compounds.
17) Sulfuric acid is an excellent dehydrating agent and will remove water from the cells of skin.
7.3 Short Answer Questions
1) The cheapest base is ________.
7.4 Essay Questions
1) Why are acids sometimes referred to as “proton donors?”
2) Lime is used in farming to reduce the acidity of the soil. The chemical name for lime is calcium oxide.
When water in the soil reacts with lime, what base is formed? Write the reaction.
3) List three strong acids.
4) Write the balanced chemical reaction for the neutralization of calcium hydroxide with nitric acid.