1. Addition of the common ion, CH3COO–, to a CH3COOH solution_____.
A) decreases the pH of the solution
B) increases the pH of the solution
C) increases the concentration of H+
D) has no effect on the pH of the solution
2. The following salts were added to aqueous solution of their respective acids or bases.
Which addition causes no change in pH?
A) Potassium acetate to acetic acid
B) HCOO Na to HCOOH
C) KCl to HCl
D) NH4NO3 to NH3(aq)
3. The pH of 0.40 M aqueous CH3COOH will be _____.
A) 2.57
B) 3.45
C) 4.12
D) 5.17
4. The pH of a solution containing 0.40 M CH3COOH and 0.20 M CH3COONa is _____.
A) 3.33
B) 2.22
C) 5.55
D) 4.44
5. The pH of a 0.20 M aqueous NH3 solution is _____.
A) 8.92
B) 11.28
C) 9.82
D) 10.12
6. The pH of a solution containing 0.20 M NH3 and 0.30 M NH4Cl is _____.
A) 8.09
B) 11.12
C) 9.07
D) 10.05
Page 1
7. A buffer solution can be prepared by mixing a_____ in required proportions
A) weak acid and its salt with a strong base
B) weak acid and its salt with a weak base
C) weak base and its salt with a weak acid
D) strong acid and its salt with a strong base
8. Which of the following represents the pKa of an acid?
A) 1/log Ka
B) log 1/Ka
C) log Ka
D) –log 1/Ka
9. The pKa values of acids A, B, C and D are 5.9, 8.1, 4.7 and 6.9, respectively. The
strongest acid is _____.
A) C
B) B
C) A
D) D
10. Which of the following would be a buffer solution?
A) KCl / HCl
B) NH3 / NH4Cl
C) Na2SO4 / H2SO4
D) KNO3 / HNO3
11. Which of the following would not be a buffer solution?
A) CH3COOK / CH3COOH
B) HCN / NaCN
C) NaClO4 / HClO4
D) NaHCO3 / H2CO3
12. The pH of a buffer solution containing 0.15 M NH3 and 0.35 M NH4Cl is _____.
A) 8.88
B) 10.8
C) 9.77
D) 11.42
Page 2
13. The pH of a buffer containing 0.20 M CH3COOH and 0.20 M CH3COONa is _____.
A) 3.72
B) 5.45
C) 5.01
D) 4.74
14. The pH of a bicarbonate (HCO3–)-carbonic acid (H2CO3) buffer is 8.00. The ratio of the
concentration of H2CO3 to HCO3– is _____.
A) 2.4
B) 0.024
C) 0.24
D) 4.00
15. The pH of a buffer solution containing 0.10 M Na2HPO4 and 0.15 M KH2PO4 is _____.
A) 7.03
B) 3.51
C) 11.08
D) 4.12
16. The pH of a CH3COONa / CH3COOH buffer is 4.50. The ratio of [CH3COO-] /
[CH3COOH] is _____.
A) 0.33
B) 0.45
C) 0.25
D) 0.58
17. The pH of blood plasma is 7.40. Assuming that the buffer action is due to HCO3–
/H2CO3 the ratio of [HCO3–] / [H2CO3] is _____.
A) 2.0
B) 10.
C) 4.0
D) 6.0
18. The pH of a buffer containing 0.20 M NH3 and 0.20 M NH4Cl is _____.
A) 8.25
B) 9.25
C) 10.75
D) 11.25
Page 3
19. What is the pH of the 0.20 M NH3 / 0.20 M NH4Cl buffer after the addition of 10.0 mL
of 0.10 M HCl to 65.0 mL of the buffer.
A) 8.05
B) 9.58
C) 10.25
D) 9.18
20. The pH of 1.00L of the buffer containing 1.0 M CH3COONa and 1.0 M CH3COOH is
_____.
A) 2.37
B) 4.74
C) 3.74
D) 5.68
21. The pH of 1.00L of the buffer containing 1.00 M CH3COONa and 1.00 M CH3COOH
after the addition of 0.080 mole NaOH is _____.
A) 3.82
B) 6.12
C) 4.81
D) 5.28
22. The pH of 1.00L of the buffer 1.00 M CH3COONa / 1.00 M CH3COOH after the
addition of 0.12 mol HCl is _____.
A) 4.64
B) 4.96
C) 3.86
D) 5.96
23. The ionization constants of a diprotic acid, H2A, are 1.1 × 10–3 and 2.5 × 10–6. To obtain
a buffer of pH 5.8 you would use _____.
A) NaHA + H2A
B) Na2A + NaHA
C) Na2A + H2A
D) NaHA + Na2A + H2A
Page 4
24. Which of the following weak acids is suitable for preparing a buffer of pH 8.6? HA (Ka
= 2.7 × 10–3), HB (Ka = 4.4 × 10–6), HC (Ka = 2.6 × 10–9), HD (Ka = 1.6 × 10–5)
A) HD
B) HA
C) HB
D) HC
25. 0.2688 g of a monoprotic acid neutralizes 16.4 mL of 0.08133 M KOH. The molar mass
of the acid is ____ g/mol.
A) 105
B) 304
C) 154
D) 202
26. 5.00 g of a diprotic acid was dissolved in water to make 250.0 ml of solution. If 25.0
mL of this solution required 11.1 mL of 1.00 M KOH for complete neutralization, the
molar mass of the acid is ____.
A) 180 g mol–1
B) 90.1 g mol–1
C) 45.5 g mol–1
D) 270 g mol–1
27. In a titration experiment 12.5 mL of 0.500 M H2SO4 neutralized 50.0 mL of NaOH. The
concentration of the NaOH solution is ____.
A) 0.500 M
B) 0.250 M
C) 0.125 M
D) 0.0250 M
28. In a titration experiment, 20.4 mL of 0.883 M HCOOH neutralized 19.3 mL of
Ba(OH)2. The concentration of Ba(OH)2 solution is ____.
A) 0.166 M
B) 0.066 M
C) 0.266 M
D) 0.467 M
Page 5
29. A 0.1276 g sample of a monoprotic acid was dissolved in 25.0 mL water and titrated
with 0.0633 M NaOH. The acid required 18.4 mL of the base to reach the equivalence
point. The molar mass of the acid is ____ g mol–1
A) 54.8
B) 95
C) 110
D) 140
30. 0.1276 g of a monoprotic acid (molar mass 110 g/mol) was dissolved in 25.0 mL of
water. The pH of the solution was found to be 5.87 after the addition of 10.0 mL of
0.0633 M NaOH. The Ka of the acid is ____.
A) 1.6 × 10–4
B) 1.8 × 10–2
C) 5.6 × 10–8
D) 1.6 × 10–6
31. Exactly 500 mL of 0.167 M NaOH was mixed with exactly 500 mL 0.100 M
CH3COOH. The equilibrium concentration of OH– is ____.
A) 0.0335 M
B) 0.0835 M
C) 0.067 M
D) 0.0125 M
32. The pH at the equivalence point of the titration of 0.20 M HCl vs. 0.20 M methylamine
is ____.
A) 8.42
B) 10.82
C) 9.18
D) 5.82
33. The pH at the equivalence point in the titration of 0.10 M HCOOH versus 0.10 M NaOH
is ____.
A) 4.61
B) 8.23
C) 5.75
D) 10.75
Page 6
34. The ionization constant Ka of an indicator is 1 × 10–6. The color of the non-ionized form
is red and that of the ionized form is yellow. The color of the indicator at pH 4 is ____.
A) green
B) red
C) yellow
D) orange
35. The Ka of an indicator is 2 × 10–6. It is green in the nonionized form and red in the
ionized form. The indicator will change its color at a pH of ____.
A) 2.7
B) 8.3
C) 6.3
D) 5.7
36. The solubility product of silver chromate (Ag2CrO4) is given by ____.
A) [Ag+] [CrO42–]
B) [Ag+]2 [CrO42–]
C) [Ag+][CrO42–]2
D) [CrO42–] / [Ag+]
37. The solubility product of mercury(I) chloride (Hg2Cl2) is given by ____.
A) [Hg+] [Cl–]
B) [Hg+]2 [Cl–]2
C) [Hg22+] [Cl–]
D) [Hg22+] [Cl–]2
38. The solubility product of manganese(II) phosphate, Mn3(PO4)2 is given by ____.
A) [Mn2+]2 [PO43–]3
B) [Mn2+] [PO43–]
C) [Mn2+]3 [PO43–]2
D) [Mn2+] [PO43–]3
39. For precipitation to occur from a solution:
A) pH > pOH
B) ion product > solubility product
C) ion product < solubility product
D) ion product = solubility product
Page 7
40. The concentration of I– in a saturated AgI solution with [Ag+]=9.1 × 10–9 M is ____.
A) 8.3 × 10–17 M
B) 9.1 × 10–5 M
C) 8.3 × 10–7 M
D) 9.1 × 10–9 M
41. The concentration of Al3+ in a saturated Al(OH)3 solution with [OH–] = 2.9 × 10–9 M is
____.
A) 1.4 × 10–10 M
B) 7.4 × 10–8 M
C) 2.4 × 10–6 M
D) 1.4 × 10–9 M
42. The solubility of SrF2 is 7.3 × 10–2 g/L. The solubility product for SrF2 is _____.
A) 1.8 × 10–8 M
B) 9.6 × 10–11 M
C) 7.8 × 10–10 M
D) 7.2 × 10–8 M
43. The solubility of silver phosphate, Ag3PO4, is 6.7 × 10–3 g/L. Its solubility product is
_____.
A) 1.8 × 10–18
B) 1.8 × 10–10
C) 2.96 × 10–12
D) 5.76 × 10–14
44. The molar solubility of MnCO3 is 4.2 × 10–6 M. The Ksp of the compound is _____.
A) 2.1 × 10–6
B) 1.8 × 10–12
C) 1.8 × 10–11
D) 1.8 × 10–8
45. The solubility of an ionic compound MX (molar mass = 346 g) is 4.63 × 10–3 g/L. Its
Ksp is _____.
A) 1.8 × 10–10
B) 6.8 × 10–12
C) 1.8 × 10–8
D) 4.2 × 10–8
Page 8
46. The solubility of an ionic compound M2X3 (mw = 288) is 3.6 × 10–17 g/L. Its Ksp is
_____.
A) 4.8 × 10–13
B) 3.3 × 10–93
C) 4.6 × 10–23
D) 8.4 × 10–33
47. The solubility product of calcium fluoride, CaF2, is 4.0 × 10–11. Its solubility is _____
M.
A) 4.4 × 10–6
B) 1.8 × 10–5
C) 2.2 × 10–4
D) 6.3 × 10–6
48. The pH of a saturated solution of Zn(OH)2 is _____.
A) 8.53
B) 9.53
C) 10.47
D) 7.82
49. The pH of a saturated solution of MOH is 9.68. Its Ksp will be _____.
A) 4.2 × 10–7
B) 4.6 × 10–18
C) 3.6 × 10–12
D) 2.3 × 10–9
50. 75 mL of 0.060 M NaF is mixed with 25 mL of 0.15 Sr(NO3)2. The concentration of F–
in the final solution is _____. (Ksp of SrF2 is 2.0 ×10−10)
A) 1.1 × 10–4 M
B) 0.016
C) 0.076
D) 0.045
Page 9
51. Solid NaI is added to a solution containing 0.01 M each of Cu+, Ag+, K+ and Mg2+. The
ion that gets precipitated first is _____.
A) Ag+
B) Mg2+
C) K+
D) Cu+
52. A pH that is suitable for the separation by precipitation of Fe(OH)3 from a solution that
is initially 0.010 M in both Fe3+ and Zn2+ is _____.
A) 3.5
B) 8.5
C) 1.5
D) 10.5
53. The solubility of CaCO3 decreases in the presence of _____.
A) CO2
B) Na2CO3
C) HCl
D) NaCl
54. Which of the following statements is true with respect to AgCl?
A) Ksp is same as its solubility.
B) Ksp of AgCl is the same in 6.5 × 10–3 M AgNO3 as in water.
C) The solubility of AgCl is independent of the concentration of AgNO3.
D) [Ag+] in solution changes significantly after the addition of AgCl to 6.5 × 10–3 M
AgNO3.
55. How many grams of CaCO3 will dissolve in 3.0 × 102 mL of 0.050 M Ca(NO3)2?
A) 4.1 × 10–2 g
B) 5.1 × 10–4 g
C) 5.1 × 10–6 g
D) 5.1 × 10–3 g
56. The solubility product of PbBr2 is 8.9 × 10–6. Its solubility in 0.20 M KBr solution is
_____.
A) 4.4 × 10–4 M
B) 2.2 × 10–4 M
C) 3.5 × 10–3 M
D) 1.78 × 10–7 M
Page 10
57. Lead bromide will have the greatest molar solubility in 0.10 M _____.
A) KBr
B) MgBr2
C) Pb(NO3)2
D) NaBr.
58. The molar solubility of AgCl in a solution made by dissolving 10.0g of CaCl2 in 1.00 L
of solution is _____.
A) 8.9 × 10–10 M
B) 1.1 × 10–5 M
C) 8.9 × 10–8 M
D) 2.7 × 10–6 M
59. The molar solubility of BaSO4 in a solution containing 1.0 M SO42– ions is _____.
A) 1.1 × 10–10 M
B) 2.7 × 10–8 M
C) 1.0 × 10–5 M
D) 8.1 × 10–7 M
60. Which of the following compounds is not more soluble in acid than in water?
A) BaSO4
B) PbCl2
C) Fe(OH)3
D) HgS
61. A compound that is more soluble in HCl (aq) than in water is _____.
A) CaCO3
B) BaI2
C) AgCl
D) Hg2Cl2
62. The compound below whose solubility is unaffected by pH changes is _____.
A) BaC2O4
B) Ca3(PO4)2
C) Ag2CrO4
D) CuI
Page 11
63. Mg(OH)2 is most soluble at pH _____.
A) 7
B) 11
C) 8
D) 10
64. The molar solubility of Fe(OH)2 at pH 8.00 is _____.
A) 0.016 M
B) 1.6 M
C) 0.16 M
D) 1.6 × 10–3 M
65. Fe(OH)2 is least soluble at a pH of_____.
A) 10
B) 4
C) 0
D) 7
66. The solubility product of Mg(OH)2 is 1.2 × 10–11. The minimum concentration of NaOH
required to decrease the concentration of Mg2+ in 0.01 M Mg(NO3)2 to 1.0 × 10–10 M is
_____.
A) 0.035 M
B) 6 × 10–4 M
C) 0.35 M
D) 3.5 × 10–5 M
67. If 2.50 g of CuSO4 are dissolved in 9.0 × 102 mL of 0.30 M NH3, the concentration of
[Cu(NH3)4]2+ at equilibrium in the solution is _____.
A) 0.115 M
B) 0.0174 M
C) 0.0016 M
D) 1.18 × 10–4 M
68. The concentration of Cd2+ at equilibrium when 0.50 g of Cd(NO3)2 is dissolved in 500
mL of 0.50 M NaCN is _____. (The formation constant of Cd(CN)42– is 7.1 × 1016.)
A) 1.2 × 10–19 M
B) 5.6 × 10–9 M
C) 1.1 × 10–18 M
D) 3.8 × 10–12 M
Page 12
69. Sodium hydroxide is added to 0.010 M Al3+ until the pH becomes 14. The predominant
species at equilibrium is _____. (Kf for Al(OH)4– is 2.0 × 1033).
A) Al3+
B) Al(OH)4–
C) Al(OH)3
D) Al2O3
70. The molar solubility of AgI in a 1.0 M NH3 solution is _____.
A) 1.5 × 10–3 M
B) 0.035 M
C) 3.5 × 10–4 M
D) 3.5 × 10–5 M
71. AgOH is not soluble in _____.
A) NaOH
B) HNO3
C) NH3
72. Which of the following statements is not correct?
A) CuI2 dissolves in NH3.
B) AgBr dissolves in NaCN.
C) HgCl2 dissolves in KCl.
D) AgCl dissolves in NaCl.
73. An example of a metal ion in the second group of qualitative analysis is _____.
A) Hg22+
B) Cu2+
C) Ca2+
D) Mn2+
74. Silver chloride can be separated from lead chloride using _____.
A) K2CrO4
B) H2S
C) NH3
D) KI
Page 13
75. The concentration of Pb2+ in a solution that is 0.15 M in Cl– is _____.
A) 0.025
B) 0.011
C) 0.052
D) 0.035
76. NH4Cl can be distinguished from KCl by the addition of _____.
A) AgNO3
B) Conc. HCl
C) NaOH
D) Pb(NO3)2
77. AgNO3 can be distinguished from Cu(NO3)2 by using _____.
A) HNO3
B) H2S
C) HCl
D) Br2/H2O
78. The buffer range is defined as pH= pKa ± 1. The range of conjugate base to acid that
corresponds to this equation is _____.
A) 0.1 – 1.0
B) 10 – 100
C) 1 – 10
D) 0.1 – 10
79. The pKa of methyl orange is 3.46. Over what pH range does this indicator change from
90% HIn to 90% In–?
A) 2.5 – 4.4
B) 1.5 – 2.5
C) 4.5 – 6.5
D) 1.5 – 3.5
80. Which one of the following is true for an acid base titration at the half -neutralization
point (the point at which half of the acid has been neutralized)?
A) pH = pOH
B) pH = ฝ pKa
C) pKa = ฝ pH
D) pH = pKa
Page 14
81. 200 mL of NaOH was mixed with 400 mL of a 2.00 M HNO2 solution. The pH of mixed
solution was 1.50 units greater than the original acid solution. The molarity of NaOH
used was _____.
A) 0.82 M
B) 1.28 M
C) 0.027 M
D) 2.15 M
82. The pKa of butyric acid is 4.7. The Kb of its conjugate base is _____.
A) 4 × 10–8
B) 5 × 10–4
C) 4 × 10–7
D) 5 × 10–10
83. Exactly 500 ml of 0.167 M NaOH was mixed with exactly 500 mL of 0.100 M
CH3COOH. The equilibrium concentration of CH3COO– is _____.
A) 0.0250 M
B) 0.050 M
C) 0.0125 M
D) 0.0670 M
84. 50.0 mL of 1.00 M Ba(OH)2 was mixed with 86.4 mL of 0.494 M H2SO4. The mass of
BaSO4 formed is _____.
A) 2.16 g
B) 7.12 g
C) 3.42 g
D) 9.96 g.
85. 50.0 mL of 1.00M Ba(OH) was mixed with 86.4 mL of 0.494 M H2SO4. The pH of the
resulting solution is _____.
A) 4.56
B) 13.04
C) 8.72
D) 1.27.
Page 15
86. For which of the following reactions is the equilibrium constant called the solubility
product?
A)
B)
C)
D)
87. Equal volumes of 0.12 M AgNO3 and 0.14 M ZnCl2 were mixed. The equilibrium
concentration of Cl– will be _____.
A) 0.016 M
B) 0.035
C) 0.080 M
D) 0.056.
88. The solubility product of silver carbonate, Ag2CO3, is 8.1 × 10–12. Its solubility in g/L is
_____.
A) 0.035
B) 0.072
C) 0.018
D) 4.1 × 10–6
89. In a solution that is initially 0.010 M in Zn2+, the Zn2+ can be precipitated at a pH of
_____.
A) 2.68
B) 8.11
C) 4.32
D) 6.79
90. In a solution that is initially 0.010 M Fe3+, Fe(OH)3 can be precipitated at a pH of
_____.
A) 2.16
B) 1.68
C) 2.68
D) 1.01
Page 16
91. 25.0 mL of 0.100 M HCl is titrated against 0.100 M CH3NH2. What will be the solution
pH after the addition of 10.0 mL of CH3NH2 solution?
A) 1.37
B) 2.73
C) 2.37
D) 0.37
92. The molar solubility of Pb(IO3)2 in 0.10 M NaIO3 is 2.4 × 10–11 M. The Ksp of Pb(IO3)2
is _____.
A) 1.7 × 10–5
B) 5.7 × 10–7
C) 2.4 × 10–13
D) 4.1 × 10–9
93. Mercury (II) chloride reacts with excess KI to yield _____.
A) Hg2I2
B) HgI42–
C) HgI2
D) HgI
94. The pKa of phenolphthalein is 9.10. Over what pH range does this indicator change
from 95% HIn to 95% In–?
A) 3.5–6.5
B) 10.5–11.9
C) 7.8–10.4
D) 4.5–6.5
95. Solid NaI is added to a solution which is 0.010M is Cu+ and 0.010M Ag+. The
concentration of Ag+ when CuI just begins to precipitate is _____.
A) 1.6 × 10–7 M
B) 4.1 × 10–9 M
C) 1.9 × 10–4 M
D) 1.1 × 10–5 M
Page 17
96. 20.00 mL of 0.0800 HCl as added to 0.1022 g of MCO3. The excess HCl required 5.64
mL of 0.1000 M NaOH for neutralization. The molar mass of the metal carbonate is
_____ g mol–1.
A) 137
B) 117
C) 197
D) 326
97. The equilibrium constant for the reaction between aqueous HCl and aqueous NaOH is
_____.
A) 1 × 10–14
B) 1 × 107
C) 1 × 1014
D) 1 × 10–7
98. The equilibrium constant for the reaction between CH3COOH and NaOH is _____.
A) 1.8 × 105
B) 1.8 × 109
C) 1 × 10–14
D) 1.8 × 10–9
99. 5.00g of a hydrated diprotic acid was dissolved in enough water to make 250ml of
solution and 25 mL of the resulting solution required 15.9 mL of 0.500 M NaOH for
neutralization. The number of molecules of water in the hydrate is _____. (The
molecular weight of the anhydrous acid is 90 g/mol.)
A) 2
B) 7
C) 5
D) 4
100. A buffer solution of pH 4.74 can be prepared by mixing CH3COOH and CH3COONa in
the proportion _____.
A) 500 mL of 0.80 M CH3COOH + 500 mL 0.80 M CH3COONa
B) 500 mL of 0.80 M CH3COOH + 500 mL 0.40 M CH3COONa
C) 500 mL of 0.40 M CH3COOH + 500 mL 0.80 M CH3COONa
D) 50 mL of 0.80 M CH3COOH + 25 mL of 0.04 M CH3COONa
Page 18
101. The pKa of phenolphthalein is 9.10. The ratio of non-ionized form to the ionized form of
the indicator at pH 8.00 is _____.
A) 1.26
B) 17.1
C) 1.1
D) 12.6
102. Oil paintings containing lead compounds become dark due to the formation of _____.
A) PbSO4
B) PbS
C) PbCl2
D) PbO
103. Sodium ions can be separated from Ba2+ ions by the addition of _____.
A) HCl
B) HNO3
C) CH3COOH
D) H2SO4
104. Zn2+ ions can be separated from Hg2+ ions by using _____.
A) NaCl
B) KI
C) HCl
D) H2S
105. The concentration of Sr2+ is a solution saturated with both BaSO4 and SrSO4 is _____.
A) 1.1 × 10–10 M
B) 1.05 × 10–5 M
C) 3.8 × 10–7 M
D) 6.2 × 10–4 M
106. The substance having the greatest solubility among the following is _____.
A) CaSO4 (Ksp = 2.4 × 10−5)
B) BaSO4
C) Ag2SO4
D) AgI
Page 19
107. How many mL of 1.0 M NaOH must be added to 200 mL of 0.10 M NaH2PO4 to obtain
a buffer solution of pH 7.50?
A) 23 mL
B) 30 mL
C) 43 mL
D) 13 mL
108. Which of the following has the highest [H+]?
A) 0.10 M H F
B) 0.10 M H F in 0.10 M NaF
C) 0.10 M H F in 0.10 M SbF5 (SbF5 reacts with F- to form SbF6-)
D) 0.01 M H F
109. A distribution curve shows how the fractions of nonionized acid and its conjugate base
vary as a function of pH. At the point of intersection of the distribution curves of
[CH3COOH] and [CH3COO–]:
A) pH = pOH
B) pH = pKa
C) pH + pOH = pKa
D) pH = pKa + pKb
110. A distribution curve shows how the fractions of nonionized acid and its conjugate base
vary as a function of pH. The curves of the plot of [CH3COOH] vs. pH and [CH3COO–]
vs. pH will intersect at a pH of _____.
A) 7.47
B) 2.83
C) 3.85
D) 4.74
111. The addition of washing soda (Na2CO3 ท10H2O) removes ––––––– ions present in hard
water.
A) Mg2+
B) SO42–
C) Ca2+
D) Cl–
Page 20
112. Most of the acid–base indicators change their color at pH equal to _____.
A) pKa
B) pKb
C) pKa + pKb
D) pKa ± 1
Page 21
Answer Key
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
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22.
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25.
26.
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31.
32.
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35.
36.
37.
38.
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40.
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43.
44.
B
C
A
D
B
C
A
B
A
B
C
A
D
B
A
D
B
B
D
B
C
A
B
D
D
B
B
D
C
D
A
D
B
B
D
B
D
C
B
D
B
C
A
C
Page 22
45.
46.
47.
48.
49.
50.
51.
52.
53.
54.
55.
56.
57.
58.
59.
60.
61.
62.
63.
64.
65.
66.
67.
68.
69.
70.
71.
72.
73.
74.
75.
76.
77.
78.
79.
80.
81.
82.
83.
84.
85.
86.
87.
88.
89.
90.
A
B
C
B
D
A
A
A
B
B
C
B
C
A
A
B
A
D
A
A
A
C
B
C
B
D
A
D
B
C
B
C
C
D
A
D
B
D
B
D
B
D
C
A
B
C
Page 23
91.
92.
93.
94.
95.
96.
97.
98.
99.
100.
101.
102.
103.
104.
105.
106.
107.
108.
109.
110.
111.
112.
A
C
B
C
A
C
C
B
A
A
D
B
D
B
D
C
D
C
B
D
C
D
Page 24