Name: ________________________ Class: ___________________ Date: __________
fd
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____
1. Pure water contains
a. water molecules only.
b. hydronium ions only.
c. hydroxide ions only.
d. water molecules, hydronium ions, and hydroxide ions.
____
2. Pure water partially breaks down into charged particles in a process called
a. hydration.
c. self-ionization.
b. hydrolysis.
d. dissociation.
____
3. What is the concentration of H3O+ ions in pure water?
a. 10–7 M
c. 55.4 M
b. 0.7 M
d. 107 M
____
4. What is the concentration of OH– ions in pure water?
a. 10–7 M
c. 55.4 M
b. 0.7 M
d. 107 M
____
5. What is the product of H3O+ ion and OH– ion concentrations in water?
a. 10–28
c. 10–7
–14
b. 10
d. 55.4
____
6. Which expression represents the concentration of H3O+ ions in solution?
a. 10–14 – [OH–]
c. 10–14  [OH–]
–14
–
b. 10  [OH ]
d. [OH–]  10–14
____
7. Which expression represents the concentration of OH– ions in solution?
a. 10–14 – [H3O+]
c. 10–14  [H3O+]
b. 10–14  [H3O+]
d. [OH–]  10–14
____
8. Which expression represents the pH of a solution?
a. log[H3O+]
c. log[OH–]
+
b. –log[H3O ]
d. –log[OH–]
____
9. If [H3O+] of a solution is greater than [OH–], the solution
a. is always acidic.
c. is always neutral.
b. is always basic.
d. might be acidic, basic, or neutral.
____ 10. If [H3O+] of a solution is less than [OH–], the solution
a. is always acidic.
c. is always neutral.
b. is always basic.
d. might be acidic, basic, or neutral.
____ 11. What is the pH of a neutral solution at 25°C?
a. 0
b. 1
c.
d.
1
7
14
ID: A
Name: ________________________
ID: A
____ 12. The pH scale in general use ranges from
a. 0 to 1.
b. –1 to 1.
c.
d.
0 to 7.
0 to 14.
____ 13. The pH of an acidic solution is
a. less than 0.
b. less than 7.
c.
d.
greater than 7.
greater than 14.
____ 14. The pH of a basic solution is
a. less than 0.
b. less than 7.
c.
d.
greater than 7.
greater than 14.
____ 15. A water solution whose pH is 4
a. is always neutral.
b. is always basic.
c.
d.
is always acidic.
might be neutral, basic, or acidic.
____ 16. A water solution whose pH is 10
a. is always neutral.
b. is always basic.
c.
d.
is always acidic.
might be neutral, basic, or acidic.
____ 17. A water solution whose pH is 7
a. is always neutral.
b. is always basic.
c.
d.
is always acidic.
might be neutral, basic, or acidic.
____ 18. Which of the following liquids is basic?
a. lemons
b. vinegar
c.
d.
milk
tomatoes
____ 19. Which of the following liquids is acidic?
a. seawater
b. blood
c.
d.
milk of magnesia
orange juice
____ 20. To calculate the pH of a solution whose [OH–] is known, first calculate
a. [H3O+].
c. antilog[H3O+].
b. log[OH–].
d. [H2O].
____ 21. What is the pH of a 10–4 M HCl solution?
a. 4
b. 6
c.
d.
8
10
____ 22. What is the pH of a 10–5 M KOH solution?
a. 3
b. 5
c.
d.
9
11
____ 23. If [H3O+] = 1.7  10–3 M, what is the pH of the solution?
a. 1.81
c. 2.42
b. 2.13
d. 2.77
____ 24. If [H3O+] = 8.26  10–5 M, what is the pH of the solution?
a. 2.161
c. 4.083
b. 3.912
d. 8.024
2
Name: ________________________
ID: A
____ 25. What is the pH of a solution whose hydronium ion concentration is 5.03  10–1 M?
a. 0.2984
c. 1.542
b. 0.5133
d. 5.031
____ 26. What is the pH of a 0.027 M KOH solution?
a. 6.47
b. 12.43
c.
d.
____ 27. What is the pH of a 0.001 62 M NaOH solution?
a. 3.841
c.
b. 5.332
d.
12.92
14.11
9.923
11.210
____ 28. How would you classify KOH in the equation below?
KOH(aq)  K  (aq)  OH   aq 
a.
b.
a weak acid
a strong acid
c.
d.
a weak base
a strong base
____ 29. How would you classify HCl, in the equation below?
HCl(aq)  H 2 O(l)  H 3 O   aq   Cl  aq 
a.
b.
a weak acid
a strong acid
c.
d.
a weak base
a strong base
____ 30. How would you classify CH3COOH in the equation below?
H 3 O + (aq) + CH 3 CO  (aq)
CH 3 COOH(aq) + H 2 O(l)
a. a weak acid
c. a weak base
b. a strong acid
d. a strong base
____ 31. How would you classify NH3 in the equation below?
NH 4 (aq) + OH  (aq)
NH 3 (g) + H 2 O(l)
a. a weak acid
c. a weak base
b. a strong acid
d. a strong base
____ 32. The common logarithm of a number, N, is the
a. inverse of N.
b. square root of N.
c. power to which N must be raised to equal 10.
d. power to which 10 must be raised to equal N.
____ 33. The pH of a solution is 9.0. What is its H3O+ concentration?
a. 1  10-9 M
c. 1  10-5 M
b. 1  10-7 M
d. 9 M
____ 34. What is the hydronium ion concentration of a solution whose pH is 4.12?
a. 4.4  10–8 M
c. 6.4  10–5 M
–6
b. 5.1  10 M
d. 7.6  10–5 M
____ 35. What is the hydronium ion concentration of a solution whose pH is 7.30?
a. 1.4  10–11 M
c. 5.0  10–8 M
b. 3.8  10–8 M
d. 7.1  10–6 M
3
Name: ________________________
ID: A
____ 36. The pH of a solution is 10.00. What is its OH– concentration?
a. 1.0  10–10 M
c. 1.0  10–4 M
–7
b. 1.0  10 M
d. 10 M
____ 37. What is the OH– concentration of a solution whose pH is 12.40?
a. 2.5  10–2 M
c. 8.9  10–2 M
b. 4.4  10–-2 M
d. 1.0  10–1 M
____ 38. The antilogarithm of a number, y, is
a. the inverse of y.
b. the square root of y.
c.
d.
y raised to the power of 10.
10 raised to the power of y.
____ 39. Dyes with pH-sensitive colors are used as
a. primary standards.
b. indicators.
c.
d.
titrants.
None of the above
____ 40. The pH range over which an indicator changes color is its
a. equivalence point.
c. transition interval.
b. end point.
d. pH interval.
____ 41. Indicators are classified into three types according to
a. their molar mass.
c. their color.
b. their polarity.
d. the pH at which they change color.
____ 42. What is the transition interval for phenol red?
a. pH 3.1–4.4
c.
b. pH 6.4–8.0
d.
pH 6.2–7.6
pH 8.0–10.0
____ 43. What is the transition interval for bromthymol blue?
a. pH 3.1–4.4
c. pH 6.2–7.6
b. pH 6.4–8.0
d. pH 8.0–10.0
____ 44. What is the transition interval for phenolphthalein?
a. pH 3.1–4.4
c. pH 6.2–7.6
b. pH 6.4–8.0
d. pH 8.0–10.0
____ 45. What is the transition interval for methyl orange?
a. pH 3.1–4.4
c.
b. pH 6.4–8.0
d.
pH 6.2–7.6
pH 8.0–10.0
____ 46. Which indicator is used to study neutralizations of strong acids with strong bases?
a. phenolphthalein
c. bromthymol blue
b. methyl orange
d. None of the above
____ 47. Which indicator is used to study neutralizations of weak acids with strong bases?
a. phenolphthalein
c. bromthymol blue
b. methyl orange
d. None of the above
____ 48. Which indicator is used to study neutralizations of strong acids with weak bases?
a. phenolphthalein
c. bromthymol blue
b. methyl orange
d. None of the above
4
Name: ________________________
ID: A
____ 49. What process measures the amount of a solution of known concentration required to react with a measured
amount of a solution of unknown concentration?
a. autoprotolysis
c. neutralization
b. hydrolysis
d. titration
____ 50. In an acid-base titration,
a. base is always added to acid.
b. acid is always added to base.
c. base is added to acid or acid is added to base.
d. None of the above
____ 51. An acid-base titration involves a
a. composition reaction.
b. neutralization reaction.
c.
d.
single-displacement reaction.
decomposition reaction.
____ 52. Which quantity is directly measured in a titration?
a. mass
c. volume
b. concentration
d. density
____ 53. An acid-base titration determines the volumes of two solutions that
a. are chemically equivalent.
c. have equal mass.
b. have equal molarity.
d. have equal molality.
____ 54. What unknown quantity can be calculated after performing a titration?
a. volume
c. mass
b. concentration
d. density
____ 55. An acid-base titration is carried out by monitoring
a. temperature.
c. pressure.
b. pH.
d. density.
____ 56. In an acid-base titration, equivalent quantities of hydronium ions and hydroxide ions are present
a. at the beginning point.
c. at the end point.
b. at the midpoint.
d. throughout the titration.
____ 57. During an acid-base titration, a very rapid change in pH
a. occurs when the first addition of the known solution is made.
b. occurs when the amounts of H3O+ ions and OH– ions are nearly equivalent.
c. occurs at several points during the titration.
d. does not occur during titration.
____ 58. In an acid-base titration, the primary standard
a. is always a highly pure acid.
b. is always a highly pure base.
c. is either a highly pure acid or a highly pure base.
d. is neither an acid or a base.
____ 59. A standard solution always contains
a. a known concentration of solute.
b. an acid.
c.
d.
5
a base.
a primary standard.
Name: ________________________
ID: A
____ 60. When titrating a strong acid with a strong base, the equivalence point
a. will be below a pH of 7.0.
b. will be above a pH of 7.0.
c. will be at a pH of 7.0.
d. will be either above or below a pH of 7.0.
____ 61. When titrating a weak acid with a strong base, the equivalence point
a. will be below a pH of 7.0.
c. will be at a pH of 7.0.
b. will be above a pH of 7.0.
d. cannot be determined by pH.
____ 62. What is the molarity of an HCl solution if 50.0 mL is neutralized in a titration by 40.0 mL of 0.400 M
NaOH?
a. 0.200 M
c. 0.320 M
b. 0.280 M
d. 0.500 M
____ 63. What is the molarity of an HCl solution if 125 mL is neutralized in a titration by 76.0 mL of 1.22 M KOH?
a. 0.371 M
c. 0.617 M
b. 0.455 M
d. 0.742 M
____ 64. What is the molarity of an NaOH solution if 4.37 mL is titrated by 11.1 mL of 0.0904 M HNO3?
a. 0.230 M
c. 0.460 M
b. 0.355 M
d. 0.620 M
____ 65. What is the molarity of an H2SO4 solution if 49.0 mL is completely titrated by 68.4 mL of an NaOH solution
whose concentration is 0.333 M?
a. 0.116 M
c. 0.465 M
b. 0.232 M
d. 0.880 M
____ 66. Calculate the molarity of a Ba(OH)2 solution if 1900 mL is completely titrated by 261 mL of 0.505 M HNO3.
a. 0.0173 M
c. 0.0322 M
b. 0.0254 M
d. 0.0347 M
____ 67. If 72.1 mL of 0.543 M H2SO4 completely titrates 39.0 mL of KOH solution, what is the molarity of the KOH
solution?
a. 0.317 M
c. 1.00 M
b. 0.502 M
d. 2.01 M
____ 68. If 114 mL of 0.008 04 M NaOH completely titrates 118 mL of H3PO4 solution, what is the molarity of the
H3PO4 solution?
a. 0.002 59 M
c. 0.007 77 M
b. 0.005 18 M
d. 0.0105 M
____ 69. What is the molarity of a Ba(OH)2 solution if 93.9 mL is completely titrated by 15.3 mL of 0.247 M H2SO4?
a. 0.0101 M
c. 0.0402 M
b. 0.0201 M
d. 0.0805 M
____ 70. What is the molarity of an H3PO4 solution if 358 mL is completely titrated by 876 mL of 0.0102 M Ba(OH)2
solution?
a. 0.0111 M
c. 0.0250 M
b. 0.0166 M
d. 0.0333 M
6
Name: ________________________
ID: A
Choose the best answer from the options that follow each question.
____ 71. What are the highest concentrations of H3O+ions and OH  ions that can coexist in an aqueous solution?
a. 1.0  10 14 M each
b. 1.0  100 M and 1.0  10 14 M, respectively
c. 1.0  10 14 M and 1.0  100 M, respectively
d. 1.0  10 7 M each
____ 72. Which of the following is not true regarding the self-ionization of water?
a. It involves the formation of hydronium and hydroxide ions.
b. It is in equilibrium.
c. It shows that water is a strong electrolyte.
d. It involves two water molecules forming two ions.
____ 73. A solution that has a [H3O+] equal to 1  10 4 M
a. is neutral.
b. is acidic.
c. is basic.
d. could be neutral, basic, or acidic.
____ 74. The [OH  ] of an aqueous solution is 6.4  10  M. What is the [H3O+]?
a. 1.6  10  9 M
b. 3.6  10  9 M
c. 1.6  10  10 M
d. 3.6  10  10 M
____ 75. What is the [OH  ] in a 0.1 M HCl solution?
a. 1 10  1 M
b. 1 10  7 M
c. 1 10  13 M
d. 1 10  14 M
____ 76. What is the [H3O+] in a 0.0040 M solution of NaOH?
a. 2.5  1011 M
b. 4.0  1011 M
c. 2.5  1012 M
d. 4.0  1012 M
____ 77. A solution that has a pH of 4.0
a. is neutral.
b. is acidic.
c. is basic.
d. could be neutral, basic, or acidic.
7
Name: ________________________
ID: A
____ 78. What is the pH of a 0.0001 M HCl solution?
a. 1
b. 4
c. 7
d. 11
____ 79. What is the concentration of hydroxide ions in a solution that has a pH of 6.0?
a. 1  106 M
b. 1  10  6 M
c. 1  101 M
d. 1  10  8 M
____ 80. What is the concentration of hydroxide ions in a solution that has a pOH of 8.0?
a. 1  108 M
b. 1  10  8 M
c. 1  106 M
d. 1  10  6 M
____ 81. How many moles of NaOH must be dissolved in 1.00 L of water to make NaOH(aq) with a pH of 12.2?
a. 6.31  10  13 mol
b. 1.22  10  4 mol
c. 1.58  10  2 mol
d. 6.31  101mol
____ 82. How would you classify nitric acid (HNO3) in the reaction represented by the equation below?
HNO3(l) + H2O(l)  H3O+(aq) + NO 3 (aq)
a. weak acid
b. strong acid
c. weak base
d. strong base
____ 83. A strip of pH paper
a. gives a quick approximation of pH.
b. is a precise measure of pH.
c. shows very little color change over a wide pH range.
d. must be calibrated with a pH meter before it is used.
____ 84. A pH meter measures the pH of a solution by measuring the
a. amount of charge on the hydronium ion.
b. color of the solution.
c. concentration of the solution.
d. voltage difference between two electrodes in the meter’s probe.
____ 85. When you conduct an acid-base titration,
a. the pH of the solution must go up.
b. the pH of the solution must go down.
c. the pH of the solution must be 7.0 at the end point.
d. the equivalence point must be reached.
8
Name: ________________________
ID: A
____ 86. At the end point of a titration using an acid-base indicator,
a. the color of the acid-base indicator should stay the same.
b. the pH of the solution should change abruptly.
c. the color of the acid-base indicator should change.
d. Both (b) and (c)
____ 87. A standard solution
a. contains a precisely measured amount of solute.
b. must be compared with a solution of primary standard before use.
c. is the known solution used in a titration.
d. All of the above
Use the figure below to answer the following questions.
pH vs. mL NH3(aq) added during a titration
____ 88. The figure above shows an example of the titration of
a. a strong acid with a weak base.
b. a strong acid with a strong base.
c. a weak acid with a weak base.
d. a weak acid with a strong base.
____ 89. In the figure above, the pH at the equivalence point
a. is equal to 7.0.
b. is greater than 7.0.
c. is less than 7.0.
d. cannot be determined from the data given.
____ 90. In the figure above, the volume of titration standard necessary to reach the equivalence point is
a. 0 mL.
b. 40 mL.
c. 50 mL.
d. 90 mL.
9
Name: ________________________
ID: A
Choose the best answer from the options that follow each question.
____ 91.
Indicator
methyl orange
methyl red
bromthymol blue
phenolphthalein
pH range
3.1 - 4.4
4.4 - 6.2
6.2 - 7.6
8.0 - 10.0
According to the table above, which pH indicator would be the best choice when titrating acetic acid,
CH3COOH, with sodium hydroxide, NaOH?
a. methyl orange
b. methyl red
c. bromthymol blue
d. phenolphthalein
____ 92. In the titration of a solution of Sr(OH)2 with HCl, the mole ratio of hydroxide ions to hydronium ions
a. is 1:1.
b. is 2:1.
c. is 1:2.
d. cannot be determined from the data given.
____ 93. What is the molarity of an HCl solution if 50.0 mL is neutralized in a titration by 40. mL of 0.4000 M
NaOH?
a. 0.20 M
b. 0.28 M
c. 0.32 M
d. 0.50 M
____ 94. If 72.1 mL of 0.543 M H2SO4 completely titrates 39.0 mL of KOH solution, what is the molarity of the KOH
solution?
a. 0.317 M
b. 0.502 M
c. 1.00 M
d. 2.01 M
____ 95. What is the molarity of a Ba(OH)2 solution if 93.9 mL is completely titrated by 15.3 mL of 0.247 M H2SO4?
a. 0.0101 M
b. 0.0805 M
c. .0201 M
d. .0402 M
PART I Choose the best answer from the options that follow each question.
____ 96. The pH scale generally ranges from
a. 0 to 1.
b. 1 to 1.
c. 0 to 7.
d. 0 to 14.
10
Name: ________________________
ID: A
____ 97. During the titration of HCl with NaOH, a very rapid change in pH occurs
a. when the first addition of known solution is made.
b. when roughly equivalent amounts of H3O+ ions and OH ions become present.
c. at several points.
d. at no point.
____ 98. A water solution is neutral if
a. it contains no H3O+ ions.
b. it contains no ionized water molecules.
c. it contains no H3O+ ions or OH  ions.
d. the concentrations of H3O+ ions and OH  ions are equal.
____ 99. The antilog of a number N is
a. the inverse of N.
b. the square root of N.
c. 10 raised to the power of N.
d. N raised to the 10th power.
____ 100. Universal indicators
a. are mixtures of several indicator solutions.
b. are pure substances.
c. have very brief color-change intervals.
d. work well only for acidic solutions.
____ 101. A useful pH range for an indicator in neutralizations involving strong acids and weak bases is
a. 1.2 to 3.0.
b. 3.1 to 4.6.
c. 6.0 to 7.6.
d. 9.5 to 11.0.
____ 102. An acid-base titration determines the solution volumes that are
a. chemically equivalent.
b. of equal molarity.
c. of equal mass.
d. of equal molality.
____ 103. In acidic solutions, an indicator that is a weak acid, HIn, is primarily in the form
a. In+.
b. In  .
c. InOH.
d. HIn.
11
Name: ________________________
ID: A
Choose the best answer from the options that follow each question.
____ 104. What is the concentration of hydronium ions in pure water?
a. 1.0 3 1027 M
Kw
b. 

 OH  


c. The same as  OH  


d. All of the above
____ 105. As the [H3O+] of a solution increases, the value of
a. log [H3O+] increases.
b. -log [H3O+] decreases.
c. the solution’s pH decreases.
d. All of the above
____ 106. The pH of a solution is defined as
a. log [H3O+].
b. -log [OH2].
c. [H3O+]  10-7.
d. -log [H3O+].
____ 107. Which of the following is not a property of an acidic solution?
a. [H3O+] greater than 1  10-7 M
b. [HO2] greater than 1  10-7 M
c. pH value below 7
d. pOH value greater than 7
____ 108. A basic solution
a. has a higher concentration of hydronium ions than hydroxide ions.
b. has the same concentration of hydronium and hydroxide ions.
c. has a lower concentration of hydronium ions than hydroxide ions.
d. does not have hydronium ions.
____ 109. If the pH of a solution increases from 2.0 to 4.0, the H3O+ ion concentration
a. decreases by a factor of 2.
b. decreases by a factor of 100.
c. increases by a factor of 3.
d. increases by a factor of 1000.
____ 110. Which of the following substances is a weak base?
a. NH3
b. KOH
c. K2O
d. NaOH
12
Name: ________________________
ID: A
____ 111. A solution that has a pH of 13 is a
a. strong acid.
b. strong base.
c. weak acid.
d. weak base.
____ 112. What is the pH of household ammonia in which the [H3O+] is 1.0  10-12 M?
a. 2
b. 7
c. 10
d. 12
____ 113. What is the [OH  ] in a sample of lime juice with a pH of 2.0?
a.
b.
c.
d.
1.0  10-2 M
1.0  10-7 M
1.0  10-10 M
1.0  10-12 M
Choose the best answer from the options that follow each question.
____ 114. An acid-base indicator
a. is either a weak acid or a weak base.
b. has a different color at a different pH.
c. can be used to find the equivalence point.
d. All of the above
____ 115. A pH meter measures the
a. color change in solution.
b. voltage difference between two electrodes in solution.
c. concentration of acid-base indicator in solution.
d. All of the above
____ 116. When performing the calculation for a titration experiment, you need to have the balanced equation for the
neutralization reaction in order to determine
a. the volume of acid added to reach the equivalent point.
b. the volume of base added to reach the equivalent point.
c. the chemically equivalent amount of acid and base.
d. Both (a) and (b)
____ 117. A titration always involves the
a. controlled addition of a standard solution.
b. addition of a strong acid.
c. addition of a strong base.
d. addition of metal ions.
13
Name: ________________________
ID: A
____ 118. For any acid titrated with a base, the equivalence point occurs when the
a. pH of the mixture of acid and base is 7.0.
b. mass of the acid and mass of the base are equal.
c. acid and base are present in chemically equivalent amounts.
d. volume of the acid and the volume of the base are equal.
____ 119. What is monitored in an acid-base titration?
a. temperature
b. pH
c. pressure
d. density
____ 120. During an acid-base titration, a rapid change in pH
a. occurs when the first addition of the standard solution is made.
b. occurs when the amounts of H3O+ ions and OH  ions are nearly equal.
c.
d.
occurs at several points during the titration.
should not occur.
____ 121. An indicator, congo red, has a transition range of pH 3.0? –5.0. It would be a good indicator for titrating a
a. strong acid and a strong base.
b. strong acid and a weak base.
c. weak acid and a strong base.
d. weak acid and a weak base.
____ 122. Using an indicator to determine pH is preferred over using a pH meter when
a. a strong acid is reacted with a strong base.
b. high precision is required.
c. a quick and approximate answer is satisfactory.
d. a weak acid is reacted with a weak base.
____ 123. The neutralization of any strong acid and strong base produces mostly
a. H2O molecules.
b. H3O+ ions and OH  ions.
c.
d.
H3O+ ions.
OH  ions.
Completion
Complete each statement.
1. An acidic solution makes the color of litmus paper turn ____________________.
2. A basic solution makes the color of litmus paper turn ____________________.
3. A substance that ionizes nearly completely in aqueous solutions and produces H3O+ ions is a strong
____________________.
14
Name: ________________________
ID: A
4. A substance that ionizes nearly completely in aqueous solutions and produces OH– ions is a strong
____________________.
5. The ____________________ of a solution is calculated by taking the negative of the common logarithm of
the hydroxide concentration.
6. During a titration, the volume of the titrant is measured with a(n) ____________________.
PART II
Write the correct term (or terms) in the space provided.
7. Pure water partially breaks down into ions in a process called ____________________.
8. If [H3O+] in a solution is less than [OH  ], the solution is ____________________.
9. The pH range over which an indicator changes color is called the indicator’s ____________________.
10. The negative of the common logarithm of the hydronium ion concentration is called
____________________.
11. The product of [H3O+] and [OH  ] in a water solution equals ____________________.
12. The sum of the pH and the pOH of a neutral solution at 25C is ____________________.
13. As the concentration of hydronium ions increases, a solution becomes more acidic and the pH
____________________.
14. In a titration, an indicator changes color at the ____________________ of the titration.
15. When a weak acid is titrated with a strong base, the pH of the solution at the equivalence point is
____________________ than 7.
16. When a strong acid is titrated with a weak base, the pH of the solution at the equivalence point is
____________________ than 7.
17. A ____________________ is a highly purified solid used to check the concentration of a standard solution.
18. A 1 M solution of NaOH will have a pH that is ____________________ than the pH of a 1 M solution of
NH3.
Short Answer
1. What does the equation 2H 2 O (l)
H 3 O (aq) + OH – (aq)represent?
2. Describe a method to visually detect the end point of a titration without the use of instrumentation.
15
Name: ________________________
ID: A
3. How can the equivalence point in a titration be detected by using a pH meter?
Use the graph below to answer the following questions.
4. What is the approximate volume of the titration standard added to reach the equivalence point, and what is
the pH of the solution at this point?
5. Is the unknown solution an acid or a base, and what is its relative strength (weak or strong)? Is the titration
standard an acid or base, and what is its relative strength?
6. Suggest an appropriate acid-base indicator that could be successfully used to conduct the acid-base titration.
In the space provided, identify each of the following values as true of acidic or basic solutions at 25C.
7. pH = 4.0
8. [H3O+] = 1  10  2
9. [OH  ] = 1  10  8
10. pH = 9.0
11. [OH  ] = 1  10  4
PART III Write the answers to the following questions in the space provided.
12. How does a pH meter measure the pH of a solution?
13. What can be observed about the rate of change in the pH of a solution during a titration?
16
Name: ________________________
ID: A
14. Write the general equilibrium expression for the dissociation of an acid-base indicator that is a weak acid,
HIn, and explain how this equilibrium determines the color of the indicator at a given pH.
PART IV
Identify each of the following substances as acidic, basic, or neutral.
15. grapefruit
16. pure water
17. seawater
18. eggs
19. blood
Calculate the [H3O+] and [OH  ] for each of the following. Write your answers in the spaces provided.
20. 1  10  4 M HCl
21. 1  10  4 M NaOH
22. 1  10  4 M Ca(OH)2
23. 1  10  4 M HNO3
24. 5  10  3 M HClO4
PART V Write the answers to the following problems on the line to the left, and show your work in the
space provided.
25. What is the hydronium ion concentration of an aqueous solution that has a pH of 5.0?
26. What is the pH of a 10  4 M HCl solution?
27. What is the hydroxide ion concentration of a solution with a pH of 12.40?
28. What is the molarity of a solution of H2SO4 if 49.0 mL of it are neutralized by 68.4 mL of 0.333 M NaOH
solution?
29. If 72.1 mL of 0.543 M H2SO4 are needed to neutralize 39.0 mL of KOH solution, what is the molarity of the
KOH solution?
30. What is the molarity of an NaOH solution if 130.0 mL of the solution are neutralized by 61.3 mL of 0.0124
M H3PO4?
17
Name: ________________________
ID: A
Essay
1. Do the terms strong and concentrated mean the same thing? Do the terms weak and dilute mean the same
thing? Explain your answers.
2. When titrating an acid from a buret against a base in a flask, a student accidentally continues to add acid after
the equivalence point has been reached. What can be done, if anything, to obtain useful results from this
experiment?
3. Why is it important to choose an indicator that has an end point that closely matches the equivalence point
during a titration?
Problem
1. What is the pH of a solution that has a hydronium ion concentration of 8.26  10–5 M?
2. What is the pH of a solution with a [OH–] of 3.31  10–7 M?
3. What is the pH of a 0.004 50 M HCl solution?
4. What is the pH of a 0.067 0 M KOH solution?
5. What is the hydronium ion concentration of a solution that has a pH of 4.120?
6. What is the hydroxide ion concentration of a solution that has a pH of 8.570?
7. What is the hydroxide ion concentration of a solution that has a pOH of 8.750?
8. What is the hydronium ion concentration of a solution that has a pOH of 4.120?
9. What is the molarity of an HCl solution if 49.0 mL is completely titrated by 68.4 mL of an NaOH solution
whose concentration is 0.333 M?
10. Calculate the molarity of a Ba(OH)2 solution if 1950 mL is completely titrated by 26.1 mL of 0.505 M HNO3.
11. A 20.0 mL sample of potassium hydroxide (KOH) solution is titrated to the equivalence point with 23.5 mL
of 0.350 M hydrobromic acid (HBr) solution. What is the molarity of the potassium hydroxide solution?
12. A 30.0 mL sample of an aqueous ammonia (NH3) solution is titrated to the equivalence point with 53.93 mL
of 0.400 M sulfuric acid (H2SO4) solution. What is the molarity of the aqueous ammonia solution?
13. A 25.0 mL sample of an aqueous solution of calcium hydroxide, Ca(OH)2, is titrated to the equivalence point
with 21.2 mL of 0.620 M sulfuric acid, H2SO4, acid solution. What is the molarity of the calcium hydroxide
solution?
18
Name: ________________________
ID: A
14. What volume of 4.35 M HCl solution would be required to reach the equivalence point with 0.285 mol
Mg(OH)2 dissolved in some deionized water?
15. What volume of 4.494 M H2SO4 solution would be required to reach the equivalence point with 7.2280 g
LiOH dissolved in some deionized water?
19
ID: A
fd
Answer Section
MULTIPLE CHOICE
1. ANS:
REF:
2. ANS:
REF:
3. ANS:
REF:
4. ANS:
REF:
5. ANS:
REF:
6. ANS:
REF:
7. ANS:
REF:
8. ANS:
REF:
9. ANS:
REF:
10. ANS:
REF:
11. ANS:
REF:
12. ANS:
REF:
13. ANS:
REF:
14. ANS:
REF:
15. ANS:
REF:
16. ANS:
REF:
17. ANS:
REF:
18. ANS:
REF:
19. ANS:
REF:
20. ANS:
REF:
D
PTS: 1
DIF:
d1a0bce3-f97e-11de-9c72-001185f0d2ea
C
PTS: 1
DIF:
d1a31f40-f97e-11de-9c72-001185f0d2ea
A
PTS: 1
DIF:
d1a34650-f97e-11de-9c72-001185f0d2ea
A
PTS: 1
DIF:
d1a5819d-f97e-11de-9c72-001185f0d2ea
B
PTS: 1
DIF:
d1a7e3fa-f97e-11de-9c72-001185f0d2ea
C
PTS: 1
DIF:
d1a80b0a-f97e-11de-9c72-001185f0d2ea
C
PTS: 1
DIF:
d1aa4657-f97e-11de-9c72-001185f0d2ea
B
PTS: 1
DIF:
d1aca8b4-f97e-11de-9c72-001185f0d2ea
A
PTS: 1
DIF:
d1accfc4-f97e-11de-9c72-001185f0d2ea
B
PTS: 1
DIF:
d1af0b11-f97e-11de-9c72-001185f0d2ea
C
PTS: 1
DIF:
d1b16d6e-f97e-11de-9c72-001185f0d2ea
D
PTS: 1
DIF:
d1b1947e-f97e-11de-9c72-001185f0d2ea
B
PTS: 1
DIF:
d1b3cfcb-f97e-11de-9c72-001185f0d2ea
C
PTS: 1
DIF:
d1b63228-f97e-11de-9c72-001185f0d2ea
C
PTS: 1
DIF:
d1b65938-f97e-11de-9c72-001185f0d2ea
B
PTS: 1
DIF:
d1b89485-f97e-11de-9c72-001185f0d2ea
A
PTS: 1
DIF:
d1b8bb95-f97e-11de-9c72-001185f0d2ea
C
PTS: 1
DIF:
d1baf6e2-f97e-11de-9c72-001185f0d2ea
D
PTS: 1
DIF:
d1bd593f-f97e-11de-9c72-001185f0d2ea
A
PTS: 1
DIF:
d1bd804f-f97e-11de-9c72-001185f0d2ea
1
I
OBJ: 1
I
OBJ: 1
I
OBJ: 1
I
OBJ: 1
I
OBJ: 1
I
OBJ: 1
I
OBJ: 1
I
OBJ: 2
I
OBJ: 2
I
OBJ: 2
I
OBJ: 3
I
OBJ: 3
I
OBJ: 3
I
OBJ: 3
I
OBJ: 3
I
OBJ: 3
I
OBJ: 3
I
OBJ: 3
I
OBJ: 3
I
OBJ: 4
ID: A
21. ANS: A
Solution:


pH  log  H 3 O    log 10 4  4


PTS: 1
DIF: III
REF: d1bfbb9c-f97e-11de-9c72-001185f0d2ea
OBJ: 4
22. ANS: C
Solution:


 10 14 1.00  10 14
9
 H O    1.00

   5   1.00  10 M
 3 
 OH  
 10 






pH  log  H 3 O    log 1.00  10 9  9


PTS: 1
OBJ: 4
23. ANS: D
Solution:
DIF:
PTS: 1
OBJ: 4
24. ANS: C
Solution:
DIF:
PTS: 1
OBJ: 4
25. ANS: A
Solution:
DIF:
III
REF: d1c21df9-f97e-11de-9c72-001185f0d2ea


pH  log  H 3 O    log1.7  10 3  2.77


III
REF: d1c24509-f97e-11de-9c72-001185f0d2ea


pH  log  H 3 O    log 8.26  10 5  4.083


III
REF: d1c48056-f97e-11de-9c72-001185f0d2ea


pH  log  H 3 O    log 5.03  10 1  0.2984


PTS: 1
DIF: III
REF: d1c6e2b3-f97e-11de-9c72-001185f0d2ea
OBJ: 4
26. ANS: B
Solution:
14
1.00  10 14

 1.00  10
13
 H 3 O    



  3.707  10 M



2


 OH 
 2.7  10 






pH  log  H 3 O    log3.707  10 13  12.43


PTS: 1
OBJ: 4
DIF:
III
REF: d1c709c3-f97e-11de-9c72-001185f0d2ea
2
ID: A
27. ANS: D
Solution:


 10 14
1.00  10 14
12
 H O    1.00




  6.173  10 M
 3 
 OH  

3 



 1.62  10 




pH  log  H 3 O    log 6.173  10 12  11.210


28.
29.
30.
31.
32.
33.
PTS: 1
DIF: III
REF:
OBJ: 4
ANS: D
PTS: 1
DIF:
REF: d1cba76d-f97e-11de-9c72-001185f0d2ea
ANS: B
PTS: 1
DIF:
REF: d1cbce7d-f97e-11de-9c72-001185f0d2ea
ANS: A
PTS: 1
DIF:
REF: d1ce09ca-f97e-11de-9c72-001185f0d2ea
ANS: A
PTS: 1
DIF:
REF: d1ce30da-f97e-11de-9c72-001185f0d2ea
ANS: D
PTS: 1
DIF:
REF: d1d06c27-f97e-11de-9c72-001185f0d2ea
ANS: A
Solution:


 H O    10 ph  10 9.0  1  10 9 M
 3 
d1c94510-f97e-11de-9c72-001185f0d2ea
II
OBJ: 4
II
OBJ: 4
II
OBJ: 4
II
OBJ: 4
I
OBJ: 4
PTS: 1
DIF: II
REF: d1d2ce84-f97e-11de-9c72-001185f0d2ea
OBJ: 5
34. ANS: D
Solution:


 H O    10 ph  10 4.12  7.58  10 5 or 7.6  10 5 M
 3 
PTS: 1
DIF: III
REF: d1d2f594-f97e-11de-9c72-001185f0d2ea
OBJ: 5
35. ANS: C
Solution:


 H O    10 ph  10 7.30  5.012  10 8 or 5.0  10 8 M
 3 
PTS: 1
OBJ: 5
DIF:
III
REF: d1d530e1-f97e-11de-9c72-001185f0d2ea
3
ID: A
36. ANS: C
Solution:


 H O    10 ph  10 10.00  1.0  10 10 M
 3 


 1014
1.00  10 14
4
 OH    1.00



  1.0  10 M




10 



 H 3 O 
 1.0  10 




PTS: 1
DIF: III
REF: d1d7933e-f97e-11de-9c72-001185f0d2ea
OBJ: 5
37. ANS: A
Solution:


 H O    10 ph  10 12.40  3.98  10 13 M
 3 
OH  
38.
39.
40.
41.
42.
43.
44.
45.
46.
47.
48.
49.
50.
PTS:
OBJ:
ANS:
REF:
ANS:
REF:
ANS:
REF:
ANS:
REF:
ANS:
REF:
ANS:
REF:
ANS:
REF:
ANS:
REF:
ANS:
REF:
ANS:
REF:
ANS:
REF:
ANS:
REF:
ANS:
REF:
1.00  10 14
1.00  1014
2



  2.5  10 M


13 



 H 3 O 
 3.98  10 




1
DIF: III
REF:
5
D
PTS: 1
DIF:
d1d9f59b-f97e-11de-9c72-001185f0d2ea
B
PTS: 1
DIF:
d1dc57f8-f97e-11de-9c72-001185f0d2ea
C
PTS: 1
DIF:
d1dc7f08-f97e-11de-9c72-001185f0d2ea
D
PTS: 1
DIF:
d1deba55-f97e-11de-9c72-001185f0d2ea
B
PTS: 1
DIF:
d1e11cb2-f97e-11de-9c72-001185f0d2ea
C
PTS: 1
DIF:
d1e143c2-f97e-11de-9c72-001185f0d2ea
D
PTS: 1
DIF:
d1e37f0f-f97e-11de-9c72-001185f0d2ea
A
PTS: 1
DIF:
d1e3a61f-f97e-11de-9c72-001185f0d2ea
C
PTS: 1
DIF:
d1e5e16c-f97e-11de-9c72-001185f0d2ea
A
PTS: 1
DIF:
d1e843c9-f97e-11de-9c72-001185f0d2ea
B
PTS: 1
DIF:
d1e86ad9-f97e-11de-9c72-001185f0d2ea
D
PTS: 1
DIF:
d1eaa626-f97e-11de-9c72-001185f0d2ea
C
PTS: 1
DIF:
d1ed0883-f97e-11de-9c72-001185f0d2ea
4
d1d7ba4e-f97e-11de-9c72-001185f0d2ea
I
OBJ: 5
I
OBJ: 1
I
OBJ: 1
I
OBJ: 1
I
OBJ: 1
I
OBJ: 1
I
OBJ: 1
I
OBJ: 1
I
OBJ: 1
I
OBJ: 1
I
OBJ: 1
I
OBJ: 2
I
OBJ: 2
ID: A
51. ANS: B
PTS: 1
DIF:
REF: d1ed2f93-f97e-11de-9c72-001185f0d2ea
52. ANS: C
PTS: 1
DIF:
REF: d1ef6ae0-f97e-11de-9c72-001185f0d2ea
53. ANS: A
PTS: 1
DIF:
REF: d1f1cd3d-f97e-11de-9c72-001185f0d2ea
54. ANS: B
PTS: 1
DIF:
REF: d1f1f44d-f97e-11de-9c72-001185f0d2ea
55. ANS: B
PTS: 1
DIF:
REF: d1f42f9a-f97e-11de-9c72-001185f0d2ea
56. ANS: C
PTS: 1
DIF:
REF: d1f456aa-f97e-11de-9c72-001185f0d2ea
57. ANS: B
PTS: 1
DIF:
REF: d1f691f7-f97e-11de-9c72-001185f0d2ea
58. ANS: C
PTS: 1
DIF:
REF: d1f8f454-f97e-11de-9c72-001185f0d2ea
59. ANS: A
PTS: 1
DIF:
REF: d1f91b64-f97e-11de-9c72-001185f0d2ea
60. ANS: C
PTS: 1
DIF:
REF: d1fb56b1-f97e-11de-9c72-001185f0d2ea
61. ANS: B
PTS: 1
DIF:
REF: d1fdb90e-f97e-11de-9c72-001185f0d2ea
62. ANS: C
Solution:
M OH  V OH   M H 3 O  V H 3 O 
MH3O 
PTS: 1
OBJ: 3
OBJ: 2
I
OBJ: 2
I
OBJ: 2
I
OBJ: 2
I
OBJ: 2
I
OBJ: 2
I
OBJ: 2
I
OBJ: 2
I
OBJ: 2
II
OBJ: 2
II
OBJ: 2
M OH  V OH  (0.400 M)(40.0 mL)

 0.320 M HCl
VH 3 O 
50.0 mL
PTS: 1
DIF: III
OBJ: 3
63. ANS: D
Solution:
M OH  V OH   M H 3 O  V H 3 O 
MH3O 
I
REF: d1fde01e-f97e-11de-9c72-001185f0d2ea
M OH  V OH  (1.22 M)(76.0 mL)

 0.742 M HCl
VH 3 O 
125 mL
DIF:
III
REF: d2001b6b-f97e-11de-9c72-001185f0d2ea
5
ID: A
64. ANS: A
Solution:
M OH  V OH   M H 3 O  V H 3 O 
M OH  
M H 3 O  VH 3 O 
V OH


(0.0904 M)(11.1 mL)
 0.230 M NaOH
4.37 mL
PTS: 1
DIF: III
OBJ: 3
65. ANS: B
Solution:
M OH  V OH   M H 3 O  V H 3 O 
MH3O 
M OH  V OH  (0.333 M)(68.4 mL)

 0.4648 M
VH 3 O 
49 mL
M H 2 SO 4 
1
1
(M H 3 O  )   0.4648 M  0.232 M H 2 SO 4
2
2
PTS: 1
DIF: III
OBJ: 3
66. ANS: D
Solution:
M OH  V OH   M H 3 O  V H 3 O 
M OH  
REF: d2027dc8-f97e-11de-9c72-001185f0d2ea
M H 3 O  VH 3 O 
V OH 
M Ba(OH) 2 

REF: d202a4d8-f97e-11de-9c72-001185f0d2ea
(0.505 M)(261 mL)
 0.06937 M
1900 mL
1
1
(M OH  )   0.06937 M  0.0347 M Ba(OH) 2
2
2
PTS: 1
DIF: III
REF: d204e025-f97e-11de-9c72-001185f0d2ea
OBJ: 3
67. ANS: D
Solution:
M OH  V OH   M H 3 O  V H 3 O  , M H 3 O   2M H 2 SO 4
M OH  
PTS: 1
OBJ: 3
2M H 2 SO 4 V H 2 SO 4
V OH 

DIF:
2(0.543 M)(72.1 mL)
 2.01 M KOH
39.0 mL
III
REF: d2074282-f97e-11de-9c72-001185f0d2ea
6
ID: A
68. ANS: A
Solution:
M OH  V OH   M H 3 O  V H 3 O 
MH3O 
M OH  V OH  (0.008 04 M)(114 mL)

 0.007 767 M
VH 3 0 
118 mL
M H 3 PO 4 
1
1
(M H 3 O  )   0.007 767 M  0.002 59 M H 3 PO 4
3
3
PTS: 1
DIF: III
OBJ: 3
69. ANS: C
Solution:
2M OH  V OH   2M H 3 O  V H 3 O 
M OH 
M H 3 O  VH 3 O 

V OH 

(0.247 M)(15.3 mL)
 0.0402 M Ba(OH) 2
93.9 mL
PTS: 1
DIF: III
OBJ: 3
70. ANS: B
Solution:
2M OH  V OH   3M H 3 O  V H 3 O 
MH3O 
71.
72.
73.
74.
75.
76.
77.
78.
79.
80.
81.
82.
83.
84.
85.
86.
PTS:
OBJ:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
1
3
D
C
B
C
C
C
B
B
D
B
C
B
A
D
D
D
REF: d2076992-f97e-11de-9c72-001185f0d2ea
REF: d209a4df-f97e-11de-9c72-001185f0d2ea
2M OH  V OH  2(0.0102 M)(876 mL)

 0.0166 M H 3 PO 4
3V H 3 O 
3(358 mL)
DIF:
III
REF: d20c073c-f97e-11de-9c72-001185f0d2ea
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
TOP:
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7
Chapter 15 Test A
Chapter 15 Test A
Chapter 15 Test A
Chapter 15 Test A
Chapter 15 Test A
Chapter 15 Test A
Chapter 15 Test A
Chapter 15 Test A
Chapter 15 Test A
Chapter 15 Test A
Chapter 15 Test A
Chapter 15 Test A
Chapter 15 Test A
Chapter 15 Test A
Chapter 15 Test A
Chapter 15 Test A
ID: A
87.
88.
89.
90.
91.
92.
93.
94.
95.
96.
97.
98.
99.
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D
A
C
C
D
B
C
D
D
D
B
D
C
A
B
A
D
D
D
D
B
C
B
A
B
D
D
D
B
C
A
C
B
B
B
C
A
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1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
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Chapter 15 Test A
Chapter 15 Test A
Chapter 15 Test A
Chapter 15 Test A
Chapter 15 Test A
Chapter 15 Test A
Chapter 15 Test A
Chapter 15 Test A
Chapter 15 Test A
Chapter 15 Test B
Chapter 15 Test B
Chapter 15 Test B
Chapter 15 Test B
Chapter 15 Test B
Chapter 15 Test B
Chapter 15 Test B
Chapter 15 Test B
Chapter 15 - Section Quiz 1
Chapter 15 - Section Quiz 1
Chapter 15 - Section Quiz 1
Chapter 15 - Section Quiz 1
Chapter 15 - Section Quiz 1
Chapter 15 - Section Quiz 1
Chapter 15 - Section Quiz 1
Chapter 15 - Section Quiz 1
Chapter 15 - Section Quiz 1
Chapter 15 - Section Quiz 1
Chapter 15 - Section Quiz 2
Chapter 15 - Section Quiz 2
Chapter 15 - Section Quiz 2
Chapter 15 - Section Quiz 2
Chapter 15 - Section Quiz 2
Chapter 15 - Section Quiz 2
Chapter 15 - Section Quiz 2
Chapter 15 - Section Quiz 2
Chapter 15 - Section Quiz 2
Chapter 15 - Section Quiz 2
DIF:
I
REF: d20c2e4c-f97e-11de-9c72-001185f0d2ea
COMPLETION
1. ANS: red
PTS: 1
OBJ: 1
8
ID: A
2. ANS: blue
PTS: 1
OBJ: 3
3. ANS: acid
DIF:
I
REF: d20e6999-f97e-11de-9c72-001185f0d2ea
PTS: 1
OBJ: 3
4. ANS: base
DIF:
I
REF: d210cbf6-f97e-11de-9c72-001185f0d2ea
PTS: 1
OBJ: 3
5. ANS: pOH
DIF:
I
REF: d210f306-f97e-11de-9c72-001185f0d2ea
PTS: 1
OBJ: 4
6. ANS: buret
DIF:
I
REF: d2132e53-f97e-11de-9c72-001185f0d2ea
PTS: 1
DIF:
OBJ: 2
7. ANS: self-ionization
I
REF: d21590b0-f97e-11de-9c72-001185f0d2ea
PTS: 1
8. ANS: basic
TOP: Chapter 15 Test B
PTS: 1
TOP: Chapter 15 Test B
9. ANS: transition interval
PTS: 1
10. ANS: pH
TOP: Chapter 15 Test B
PTS: 1
11. ANS: 10  14
TOP: Chapter 15 Test B
PTS: 1
12. ANS: 14
TOP: Chapter 15 Test B
PTS: 1
13. ANS: decreases
TOP: Chapter 15 Test B
PTS: 1
14. ANS: end point
TOP: Chapter 15 Test B
PTS: 1
15. ANS: higher
TOP: Chapter 15 Test B
PTS: 1
TOP: Chapter 15 Test B
9
ID: A
16. ANS: lower
PTS: 1
TOP: Chapter 15 Test B
17. ANS: primary standard
PTS: 1
18. ANS: higher
TOP: Chapter 15 Test B
PTS: 1
TOP: Chapter 15 Test B
SHORT ANSWER
1. ANS:
The equation represents the self-ionization of water.
PTS: 1
DIF: I
REF: d215b7c0-f97e-11de-9c72-001185f0d2ea
OBJ: 1
2. ANS:
An indicator dye that changes color at different pH values works well as a visual detection method for
titrations.
PTS: 1
DIF: II
REF: d217f30d-f97e-11de-9c72-001185f0d2ea
OBJ: 1
3. ANS:
The equivalence point is detected by noting a shape change in the titration graph.
PTS: 1
DIF: I
REF: d21a556a-f97e-11de-9c72-001185f0d2ea
OBJ: 2
4. ANS:
Approximately 23 mL of titration standard is added to reach the equivalence point.
The pH is about 5.0 at this point.
PTS: 1
DIF: III
REF: d21a7c7a-f97e-11de-9c72-001185f0d2ea
OBJ: 2
5. ANS:
The graph is an example of a weak base titrated with a strong acid.
PTS: 1
DIF: II
REF: d21cb7c7-f97e-11de-9c72-001185f0d2ea
OBJ: 2
6. ANS:
Methyl red, pH range 4.4–6.2, would be a good indicator to choose.
PTS: 1
OBJ: 1
7. ANS:
acidic
PTS: 1
DIF:
II
REF: d21cded7-f97e-11de-9c72-001185f0d2ea
TOP: Chapter 15 Test B
10
ID: A
8. ANS:
acidic
PTS: 1
9. ANS:
acidic
TOP: Chapter 15 Test B
PTS: 1
10. ANS:
basic
TOP: Chapter 15 Test B
PTS: 1
11. ANS:
basic
TOP: Chapter 15 Test B
PTS: 1
TOP: Chapter 15 Test B
12. ANS:
A pH meter measures the pH of a solution by measuring the voltage between the two electrodes that are
placed in the solution. This works because the voltage is proportional to the hydronium ion concentration.
PTS: 1
TOP: Chapter 15 Test B
13. ANS:
The pH changes slowly at first, then rapidly through the equivalence point, then slowly again.
PTS: 1
TOP: Chapter 15 Test B
14. ANS:
HIn + H2O  H3O+ + In  or HInH+ In 
In acidic solutions, the H3O+ ions in solution drive the equation toward the nonionized form. HIn is present in
largely nonionized form in acidic solutions, and In  ions are present in largely ionized form in basic
solutions. HIn is a different color than the In  ion.
PTS: 1
15. ANS:
acidic
TOP: Chapter 15 Test B
PTS: 1
16. ANS:
neutral
TOP: Chapter 15 Test B
PTS: 1
17. ANS:
basic
TOP: Chapter 15 Test B
PTS: 1
18. ANS:
basic
TOP: Chapter 15 Test B
PTS: 1
TOP: Chapter 15 Test B
11
ID: A
19. ANS:
basic
PTS: 1
TOP: Chapter 15 Test B
20. ANS:
[H3O+] = 1  10  4 M;
[OH  ] = 1  10  10 M
PTS: 1
TOP: Chapter 15 Test B
21. ANS:
[H3O+] = 1.0  10  10 M;
[OH  ] = 1.0  10  4 M
PTS: 1
TOP: Chapter 15 Test B
22. ANS:
[H3O+] = 5.0  10  11 M;
[OH  ] = 2.0  10  4 M
PTS: 1
TOP: Chapter 15 Test B
23. ANS:
[H3O+] + 1  10  4 M;
[OH  ] + 1  10  10 M
PTS: 1
TOP: Chapter 15 Test B
24. ANS:
[H3O+] = 5  10  3 M;
[OH  ] = 2  10  12 M
PTS: 1
25. ANS:
1  10  5 M
TOP: Chapter 15 Test B
PTS: 1
26. ANS:
4.0
TOP: Chapter 15 Test B
PTS: 1
27. ANS:
2.5  10  2 M
TOP: Chapter 15 Test B
PTS: 1
28. ANS:
0.232 M
TOP: Chapter 15 Test B
PTS: 1
TOP: Chapter 15 Test B
12
ID: A
29. ANS:
2.01 M
PTS: 1
30. ANS:
0.0175 M
PTS: 1
TOP: Chapter 15 Test B
TOP: Chapter 15 Test B
ESSAY
1. ANS:
The terms concentrated and dilute refer to the amount of solute per unit of solvent. The terms strong and
weak refer to the degree of ionization. A solution containing a small amount of acid per unit of solvent is
dilute even if the acid is a strong acid (highly ionized). Alternatively, a solution containing a large amount of
acid per unit of solvent is concentrated even though the acid is a weak acid (only slightly ionized).
PTS: 1
DIF: II
REF: d21f1a24-f97e-11de-9c72-001185f0d2ea
OBJ: 3
2. ANS:
The experiment can still produce useful results if a known volume of base is now added to the flask in an
amount that makes the solution basic. Then acid is added to reach a sharp end point. The total volume of acid
and base used in the titration should yield accurate results because, at the second end point, exactly
equivalent amounts of acid and base are present in the reaction flask.
PTS: 1
DIF: III
REF: d2217c81-f97e-11de-9c72-001185f0d2ea
OBJ: 2
3. ANS:
At the equivalence point of a titration there will be a quick change in the pH because the two solutions are
present in chemically equivalent amounts. If an indicator has an end point at a similar pH value as the
equivalence point, the indicator will turn color when the volume of the titrant contains a chemically
equivalent amount as the volume of the solution of unknown concentration.
PTS: 1
OBJ: 2
DIF:
II
REF: d221a391-f97e-11de-9c72-001185f0d2ea
PROBLEM
1. ANS:
4.083
Solution:


pH=  log  H 3 O     log(8.26  10 5 )  4.083


PTS: 1
OBJ: 4
DIF:
II
REF: d223dede-f97e-11de-9c72-001185f0d2ea
13
ID: A
2. ANS:
7.520
Solution:
14
K


 H O     w   1.00  10  3.02  10 8 M
 3  

3.31  10 7
 OH  


pH  log  H 3 O    log(3.02  10 8 )  7.520


PTS: 1
OBJ: 4
3. ANS:
2.347
Solution:
DIF:
PTS: 1
OBJ: 4
4. ANS:
12.826
Solution:


 H 3 O   


DIF:
III
REF: d228a398-f97e-11de-9c72-001185f0d2ea


pH= –log  H 3 O     log(4.50  10 3 )  2.347


II
REF: d22b05f5-f97e-11de-9c72-001185f0d2ea
Kw
1.00  10 14

 1.49  10 13 M


2
 OH  
6.70

10




pH   log  H 3 O     log(1.49  10 13 )  12.826


PTS: 1
DIF: III
REF: d22b2d05-f97e-11de-9c72-001185f0d2ea
OBJ: 4
5. ANS:
7.59 10–9
Solution


pH
 H 3 O    10  10 4.12  7.59  109 M


PTS: 1
DIF: II
REF: d22d6852-f97e-11de-9c72-001185f0d2ea
OBJ: 5
6. ANS:
3.7210–6 M
Solution:
pH


 H 3 O    10
 10 8.57  2.69  10 9 M


14
 OH    K w  1.00  10
 3.72  10 6 M



9
H3 O
2.69  10
PTS: 1
OBJ: 5
DIF:
III
REF: d22fcaaf-f97e-11de-9c72-001185f0d2ea
14
ID: A
7. ANS:
1.7810–9 M
Solution:


 OH    10 pOH  10 8.75  1.78  10 9 M


PTS: 1
DIF: II
REF: d22ff1bf-f97e-11de-9c72-001185f0d2ea
OBJ: 5
8. ANS:
1.3210–10 M
Solution:


 OH    14  pOH  14  4.12  9.88


 H O    10 ph  10 9.88  1.32  10 10 M
 3 
PTS: 1
OBJ: 5
9. ANS:
0.465 M
Solution:
MH3O 
DIF:
III
M OH - V OH - (0.333 M)(0.0684 L)

 0.465 M
VH 3 O 
0.0490 L
PTS: 1
DIF: II
OBJ: 3
10. ANS:
3.3810–3 M
Solution:
2M Ba(OH) 2 V Ba(OH) 2  M H 3 O  V H 3 O +
M OH  
M H 3 O  VH 3 O +
2V Ba(OH) 2

PTS: 1
OBJ: 3
M H 3 O + VH 3 O +
V OH


REF: d2348f69-f97e-11de-9c72-001185f0d2ea
(0.505 M)(0.0261 L)
 3.38  10 3 M
2(1.95 L)
PTS: 1
DIF: III
OBJ: 3
11. ANS:
0.411 M
Solution:
M OH  V OH   M H 3 O + V H 3 O +
M OH  
REF: d2322d0c-f97e-11de-9c72-001185f0d2ea
REF: d234b679-f97e-11de-9c72-001185f0d2ea
0.350 M(0.0235 L)
 0.411 M
0.200 L
DIF:
II
REF: d236f1c6-f97e-11de-9c72-001185f0d2ea
15
ID: A
12. ANS:
1.44 M
Solution:
M OH  V OH   2M H 2 SO 4 V H 2 SO 4
M OH  
2M H 2 SO 4 V H 2 SO 4
V OH 

2(0.200 M)(0.053 93 L)
 1.44 M
0.030 00 L
PTS: 1
DIF: III
OBJ: 3
13. ANS:
0.526 M
Solution:
2M Ca(OH) 2 V Ca(OH) 2  2M H 2 SO 4 V H 2 SO 4
M OH  
M H 3 O  VH 3 O 
V OH 

(0.620 M)(0.021 2 L)
 0.526 M
0.025 0 L
PTS: 1
DIF: III
OBJ: 3
14. ANS:
131 mL
Solution:
M H 3 O  V H 3 O   2 mol Mg(OH) 2
VH 3 O  
7.2280 g LiOH 
PTS: 1
OBJ: 3
REF: d2397b33-f97e-11de-9c72-001185f0d2ea
2 mol Mg(OH) 2 2(0.285 mol)

 131 mL
MH3O
4.35 M
PTS: 1
DIF: II
OBJ: 3
15. ANS:
0.033 58 L or 33.58 mL
Solution:
2M H 2 SO 4 V H 2 SO 4  mol LiOH
V H 2 SO 4 
REF: d2395423-f97e-11de-9c72-001185f0d2ea
REF: d23bb680-f97e-11de-9c72-001185f0d2ea
1 mol LiOH
 0.30180 mol LiOH
23.950 g LiOH
mol OH  0.30180 mol

 0.033 58 L or 33.58 mL
2M H 2 SO 4
2(4.494 M)
DIF:
II
REF: d23e18dd-f97e-11de-9c72-001185f0d2ea
16