Acids and Bases
Name ______________________________
Date ________________ Period _______
Neutralization: Acids and Bases Together
True or False: For each false statement, change the underlined word(s) to the correct word(s).
1. ________________ If you dip some blue litmus paper into a neutral solution, the litmus paper
turns pink.
2. ________________ If sodium hydroxide is mixed with hydrochloric acid, table salt is formed.
3. ________________ HOH is another way of writing a formula for a base.
4. ________________ Bases always contain a metal ion and a nonmetal ion.
5. ________________ To form a salt, an acid is mixed with a neutral solution.
6. ________________ If a base is added to an acid, one drop at a time, the phenolphthalein indicator in
the solution will change from colorless to pink.
7. ________________ A neutral solution contains less hydrogen ions than an acidic solution.
8. ________________ A basic solution contains less hydroxide ions than a neutral solution.
9. ________________ NaF is an example of a base.
10. ________________ An acid is the chemical opposite of a salt.
Completion: Write in the word(s) which best complete(s) each statement.
11. A ___________________ solution is neither acidic or basic.
12. If you mix an acid and a base, you produce a ________________ plus ___________________.
13. The above reaction is called ______________________.
14. When an acid and a base are mixed, the water is formed from the _________________ ion of the acid
and the _________________ ion of the base.
15. Potassium nitrate is made by mixing _________________ acid and __________________ hydroxide.
16. Whenever an acid is mixed with a base, the compound which is always produced is ______________.
17. Aluminum hydroxide is an example of a(n) ________________.
18. Aluminum chloride is an example of a(n) _________________.
19. HF is the formula for _________________________________.
20. If you mix hydrochloric acid and calcium hydroxide, you produce water and a salt called
______________________________.
Acids and Bases
pH: Acid or Base
True or False: For each false statement, change the underlined word(s) to the correct word(s).
21. _________________ A strong acid gives off many hydroxide ions in water.
22. _________________ The pH of a solution is found to be 5.5. This means the solution is basic.
23. _________________ A pH of 10 is more basic than a pH of 8.
24. _________________ Club soda is shown to have a pH of about 4, so club soda is an acidic solution.
25. _________________ The pH of a dilute solution of calcium hydroxide would be greater than 7.
26. _________________ The pH of a vinegar solution would be greater than 7.
27. _________________ A low pH tells you that few hydrogen ions are present.
28. _________________ As a solution becomes more basic, its pH decreases.
29. _________________ Air pollution from industry often causes rainwater to become acidic.
30. _________________ Unpolluted rainwater is slightly acidic.
Completion: Write in the word(s) which best complete(s) each statement.
31. You can think of pH as the _________________ of hydrogen ions.
32. A solution with a pH of 6 is a (slightly, strongly) __________________ acidic.
33. Methyl violet, which changes the color at different pH’s is known as a(n) __________________.
34. The pH of pure water should be __________.
35. An electrical device which can measure the pH is called a ____________________.
36. A strong _______________ gives off many hydroxide ions in water.
37. If you mix equal amounts of equal molarities of sodium hydroxide with hydrochloric acid, the pH will
be __________.
38. If vinegar is added to a potassium hydroxide solution, the pH __________________.
39. The pH of your blood should be between 7.2 and 7.4, this means blood is slightly ________________.
40. The pH of a sample of polluted rainwater is found to be 2. This means the rain is ________________.
Thought Questions:
41. Tell the difference between a strong acid and a weak acid.
42. Tell the difference between a strong base and weak base.
Naming Acids
Name the following acids:
43. HNO3
_____________________________________
44. HCl
_____________________________________
45. H2SO4
_____________________________________
46. H2SO3
_____________________________________
47. HC2H3O2 _____________________________________
48. HBr
_____________________________________
49. HNO2
_____________________________________
50. H3PO4
_____________________________________
51. H2S
_____________________________________
52. H2CO3
_____________________________________
Write the formulas for the following acids:
53. sulfuric acid
________________
54. nitric acid
________________
55. hydrochloric acid ________________
56. acetic acid
________________
57. hydrofluoric acid ________________
58. phosphorous acid ________________
59. carbonic acid
________________
60. nitrous acid
________________
61. phosphoric acid
________________
62. hydrosulfuric acid ________________
Oxo or
Binary
63
Chemical
Formula
H3BO3
64
65
CH3COOH
66
H2SO4
67
H2SO3
68
69
70
C17H35COOH
71
H2CO3
72
73
HClO4
74
75
H2S
Common Use or
Name
Boracic acid; eye
wash
Muriatic acid;
digestion
Vinegar
Oil of vitriol; most
used chemical
With H2SO4 is acid
rain
In many cleaners
Name of Acid
Hydrochloric acid
Oxalic acid
Fertilizer
production
In fats; to produce
soap
Carbonated
beverages
Fertilizer
production
The strongest acid
Phosphoric acid
Bleach
Hypochlorous acid
Stearic acid
Nitric acid
In sour gas wells
78
Etches glass
Hydrofluoric acid
79
Forms a yellow
solution
Chromic acid
Some common and
uncommon
laboratory acids
Nitrous acid
80
HCN
81
82
C6H5COOH
83
H2SiO3
84
Benzoic acid
Thiosulfuric acid
85.
pH
[H+]
pOH
(14 – pH)
[OH-]
1
1 x 10-1
13
1 x 10-13
2
1 x 10-2
12
1 x 10-12
3
4
5
6
7
8
9
10
11
12
13
14
The pH of a solution indicates how acidic or basic that solution is.
pH range of 0 – 7 acidic
7 neutral
7 – 14 basic
Since [H+] [OH−] = 1.0 x 10−14 at 25°C, if [H+] is known, the [OH−] can be calculated and vice versa.
pH = − log [H+]
So if [H+] = 1.0 x 10−6, pH = 6
pOH = − log [OH−]
So if [OH−] = 1.0 x 10−8, pOH = 8
Together, pH + pOH = 14
Complete the following chart.
86.
[H+]
pH
[OH−]
pOH
Acidic or Basic
1.0 x 10−5 M
5
1.0 x 10−9 M
9
Acidic
87.
7
1.0 x 10−4 M
88.
89.
1.0 x 10−2 M
90.
11
91.
12
1.0 x 10−5 M
92.
93.
1.0 x 10−11 M
94.
95.
13
6
Self-ionization of Water & pH
Name________________________________
15.2 Review
Period________Date____________________
Matching: On the line at left, write the letter of the best-matching definition.
_____ 96. self-ionization
_____ 97. pure water
a. has H3O+ concentration greater than 1 x 10−7 M
b. has H3O+ and OH− concentrations of 1 x 10−7 M
_____ 98. Kw - ion product constant c. has a pH greater than 7
_____ 99. pH scale
d. describes the reaction: H2O + H2O ↔ H3O+ + OH−
_____ 100. acidic solution
e. has a pH=7;may contain ions other than H3O+& OH−
_____ 101. basic solution
f. is equal to 1 x 10−14 at 25ºC
_____ 102. neutral solution
g. describes the acidity or basicity of a solution
Short Answer: Answer the following questions in the space provided.
True or False: If the statement is true write “true.” If it is false, change the underlined word or words to
make the statement true. Write your answer on the line provided.
___________________________ 103. An acidic solution contains only H3O+ ions.
___________________________ 104. A solution with a pH of 4 is acidic.
___________________________ 105. When the pH of a solution decreases from 9 to 7, the [H3O+]
increases by a factor of 2.
Problems: Solve each of the problems as directed. Show all your work.
106. Based on the given information, classify the following as neutral, acidic, or basic.
a. [H+] = 1 x 10−5 M
_______________________________________
b. [OH−] = 1 x 10−5 M
_______________________________________
c. [H+] = 1 x 10−7 M
_______________________________________
107. Given that a solution has a pH of 3, calculate the [H3O+] and [OH−].
108. Calculate the [OH−] for an aqueous solution in which [H3O+] is 1 x 10−10 M. Is the solution acidic,
basic, or neutral?
109. Determine the [H3O+] for aqueous solutions that have the following pH values.
a. 3
b. 6
c. 10
110. The concentration of H3O+ ions in a solution is 3.8 x 10-9 M. What is the pH of the solution? Is the
solution acidic, basic or neutral? What is the concentration of OH- ions?
pH Problems
111. What is the concentration of OH- ions in saturated limewater if [H3O+] = 3.98 x 10-13 M?
What is the pH of the limewater and is limewater acidic, basic or neutral?
112. What is the concentration of OH- ions in a potato and water solution if [H3O+] = 1.6 x 10-6
M? What is the pH of potatoes and water and is it acidic, basic or neutral?
113. What is the concentration of H3O+ ions in 0.1 M ammonia if [OH-] = 1.26 x 10-3 M? What
is the pH of ammonia and is it acidic, basic or neutral?
114. What is the concentration of OH- ions in butter if [H3O+] = 6.0 x 10-7 M? What is the pH
of butter and is it acidic, basic or neutral?
115. What is the concentration of H3O+ ions in peaches if [OH-] = 3.16 x 10-11 M? What is the
pH of peaches and are they acidic, basic or neutral?
116. What is the concentration of OH- ions in 0.1 M borax if [H3O+] = 6.31 x 10-10 M? What is
the pH of borax and is it acidic, basic or neutral?
117. What is the concentration of H3O+ ions in eggs if [OH-] = 6.0 x 10-7 M? What is the pH of
eggs and are they acidic, basic or neutral?
118. What is the concentration of OH- ions in 0.1 M bicarbonate of soda if [H3O+] = 3.98 x 10-9
M? What is the pH of bicarbonate of soda and is it acidic, basic or neutral?
119. During the course of the day, human salvia varies between being acidic and basic. What is
the concentration of H3O+ ions in salvia if [OH-] = 3.16 x 10-8 M? What is the pH of salvia
and is this sample acidic, basic or neutral?
120. Analysis of a sample of maple syrup reveals that the concentration of OH− is 5.0 x 10−8 M.
What is the pH of this syrup? Is it acidic, neutral, or basic?
121. In a sample of bananas and water, it is found that [H3O+] = 2.51 x 10−5 M. What is the
corresponding pH value, and are the bananas and water acidic, basic, or neutral?
122. [OH−] = 7.94 x 10−12 M in a sample of vinegar. What is the pH of the vinegar, and is it
acidic, neutral, or basic?
123. A sample of human blood plasma is found to have a concentration of H3O+ ions of 3.72 x
10−8 M. What is the pH of this sample? Is it an acid, a base, or neutral?
124. In a sample of saturated magnesia, it is found that [OH−] = 3.22 x 10−4 M. What is the pH
of this sample, and is it acidic, neutral, or basic?
125. Tomatoes are found to have a hydronium ion (H3O+) concentration of 6.12 x 10−5 M. What
is the pH of these tomatoes, and are they acidic, neutral, or basic?
126. A saturated solution of calcium carbonate has a hydroxide ion concentration of 2.44 x 10−4
M. What is the pH of this solution, and is it acidic, neutral, or basic?
127. The hydronium ion concentration in a urine specimen is measured to be 6.3 x 10−6 M.
What is the pH of this sample, and is it acidic, neutral, or basic?
128. What is the pH of sour pickles if [OH-] = 1.6 x 10-10 M? What is the pH of the pickles?
Are the pickles acidic, basic or neutral?
129. The hydroxide content of a popular soft drink is measured and found to be 4.11 x 10-9 M.
What is the pH of the soft drink, and is it acidic, basic or neutral?
Acid-Base Titration
Complete the following statements by filling in the appropriate word or phrase from the list below. Not
all choices will be used.
acid-base titration
equivalence point
phenolphthalein
water and a salt
end point
standard solution
equal
indicator
NaCl and water
titration curve
not equal
H2SO4 and water
130. The point at which exactly enough standard solution is added to neutralize the unknown solution is
the __________________________.
131. A(n) __________________________________ is used to represent pH data.
132. A(n) __________________________________ is a carefully controlled neutralization reaction.
133. A(n) __________________________________ changes color at certain pH values.
134. A(n) __________________________________ contains an acid or base in known concentration.
135. A common indicator used in titrations is ___________________________________.
136. The point at which the indicator changes color is the ____________________________ of the
reaction.
137. The reaction in a titration produces ______________________________________.
138. At the end point of a titration, the number of H+ ions donated by the acid is ______________ to the
number of H+ ions accepted by the base.
139. The titration between NaOH and HCl results in a solution of ______________________________.
140. A 30. mL volume of HCl is titrated with 23 of mL of 0.20 M NaOH. What is the molarity HCl in
this solution?
141. A 26 mL volume of NH3 is titrated with 23 mL of 0.20 M HCl. What is the molarity of the NH3 in
this solution?
142. A 40. mL volume of H2SO4 is titrated with 38 mL of 0.25 M NaOH. What is the molarity of the
H2SO4 solution?
143. A volume of 30. mL of 0.25 M HCl neutralizes a 50. mL sample of KOH solution. What is the
concentration of the KOH?
144. A volume of 9.0 mL of 0.70 M NH3 neutralizes a 35 mL sample of HClO4 solution. What is the
concentration of the HClO4?
145. A volume of 90. mL of 0.2 M HBr neutralizes a 60. mL sample of NaOH solution. What is the
concentration of the NaOH?
146. A volume of 37 mL of 0.36 M KCN neutralizes a 75 mL sample of HClO solution.What is the
concentration of the HClO?
147. A volume of 46 mL of 0.40 M NaOH neutralizes a 80. mL sample of HCN solution.What is the
concentration of the HCN?
148. A volume of 50. mL of 0.30 M HCl neutralizes a 60. mL sample of Ca(OH)2 solution. What is the
concentration of the Ca(OH)2?
149. A volume of 20. mL of 0.25 M Al(OH)3 neutralizes a 75 mL sample of H2SO4 solution. What is the
concentration of the H2SO4?
150. A volume of 135 mL of 0.40 M HCl neutralizes a 90. mL sample of Ca(OH)2 solution. What is the
concentration of the Ca(OH)2?
151. A volume of 60. mL of 0.60 M HBr neutralizes a 80. mL sample of Ca(OH)2 solution. What is the
concentration of the Ca(OH)2?
152. A volume of 10. mL of 0.75 M NaOH neutralizes a 30. mL sample of HClO solution. What is the
concentration of the HClO?
153. A standard solution of NaOH was prepared in order to determine the molarity of an unknown HCl
solution. 5.25 g of NaOH were dissolved in enough distilled water to prepare 100. mL of solution. If
18.5 mL of the HCl solution is used to neutralize 14.5 mL of the NaOH solution what is the molarity of
the HCl solution?
Titration Problems
Solve the following problems. Complete, balanced equations must be written for each!
154) A sodium hydroxide solution is titrated with a 3.0 M hydrochloric acid solution to
determine its molarity. If 15.8 mL of the hydrochloric acid is required to neutralize 28.9 mL
of the sodium hydroxide solution, determine the molarity of the sodium hydroxide.
155) 139.8 mL of 1.50 M potassium hydroxide is required to neutralize 50.0 mL of nitric acid.
What is the molarity of the nitric acid?
156) 24.9 mL of 2.88 M calcium hydroxide completely neutralizes 38.9 mL of a hydrobromic
acid solution. What is the molarity of the hyrdobromic acid?
157) 56.0 mL of lithium hydroxide is titrated with 27.4 mL of 0.500 M hydrofluoric acid.
Determine the molarity of the base solution.
158) 15.0 mL of phosphoric acid is titrated with 48.3 mL 0.612 M potassium hydroxide. What
is the molarity of the phosphoric acid solution?
159)
Determine the molarity of hydrochloric acid given the following data:
HCl +
NaOH
Initial buret reading (mL)
Final buret reading (mL)
160)
+
H2O
Hydrochloric acid
1.5
37.6
1.75 M sodium hydroxide
0
22.3
strontium hydroxide
11.0
49.2
0.202 M perchloric acid
5.0
38.6
Determine the molarity of phosphoric acid given the following data:
Initial buret reading (mL)
Final buret reading (mL)
162)
NaCl
Determine the molarity of strontium hydroxide given the following data:
Initial buret reading (mL)
Final buret reading (mL)
161)

phosphoric acid
0.0
42.5
0.25 M sodium carbonate
0.80
25.0
Determine the molarity of strontium hydroxide given the following data:
Initial buret reading (mL)
Final buret reading (mL)
2.00 M hydrochloric acid
1.5
37.6
strontium hydroxide
0
22.3
Acid - Base Review
I. Vocabulary:
163)
__________________________: An ionic compound formed
when an acid reacts with a base.
164)
__________________________: The reaction between an acid and a base.
165) __________________________: A substance that conducts an electric current when in
solution.
166)
__________________________: A proton donor.
167) __________________________: A substance that has different characteristic colors in
acids and bases.
168)
__________________________: A substance that supplies hydroxide ions in solution.
169)
__________________________: Can react as either an acid or a base.
170)
__________________________: The ion formed when a
proton is added to a water molecule.
II. Write A for acid, B for base or an X if the indicated property can apply to either.
_____171. feels slippery
_____189. sour taste
_____172. stings in open wounds
_____190. reacts with most metals
_____173. phenolphthalein is colorless
_____191. litmus paper turns red
_____174. does not react with metals
_____192. [H3O+] = 1.0 x 10-11
_____175. is an electrolyte
_____193. has a bitter taste
_____176. can produce a salt in some reactions
_____194. has a pH > 7
Acids, Bases and Salts
177.
Write an E if the indicated substance is an electrolyte or an N if it is a non-electrolyte.
_____ HBr
178.
_____ CaS
_____N2O5
_____KOH
Write an A for acids, B for bases and S for salts.
______ CO2
______ Fe(NO3)2
179.
_____ Zn(OH)2
_____ NH4Br
_____ LiOH
_____ HClO4
Write the name for the following acids:
a. HNO3
b. HBr
c. H2CO3
d. H2S
e. HNO2
f. HC2H3O2
180.
Write the formula for the following acids:
a. chloric acid
b. hydrofluoric acid
c. sulfurous acid
d. sulfuric acid
e. hydroiodic acid
f. phosphoric acid
181.
Write complete balanced equations for the following neutralization reactions
a. barium hydroxide + nitric acid →
b. hydrobromic acid + aluminum hydroxide →
c. sulfuric acid
+
rubidium hydroxide →
pH Problems
182. Determine the following quantities for a .00045 M HCl solution:
a. [H3O+]
b. [OH-]
c. pH
183. Determine the following quantities for a 0.0034 M NaOH solution:
a. [H3O+]
b. [OH-]
c. pH
184. Calculate the pH for the following solutions and indicate whether each solution is acidic, basic or
neutral?
a. [H3O+] = 2.9 x 10-9 M
b. [OH-] = 1.07 x 10-8 M
Titration Problems
185) A sodium hydroxide solution is titrated with a 3.0 M HCl solution to determine its
molarity. If 15.8 mL of the HCl is required to neutralize 28.9 mL of the NaOH solution,
determine the molarity of the sodium hydroxide.
186) 139.8 mL of 1.50 M KOH is required to neutralize 50.0 mL of H2SO4. What is the
molarity of the H2SO4?
187) 56.0 mL of LiOH is titrated with 27.4 mL of 0.500 M HF. Determine the molarity of the
base solution.
188)
15.0 mL of HI is titrated with 48.3 mL 0.612 M KOH. What is the molarity of HI?