1. A Br๘nsted acid is a(n) _____.
A) proton donor
B) hydroxide ion donor
C) proton acceptor
D) electron donor
2. A Br๘nsted base _____.
A) is a cation
B) does not possess a lone pair of electrons
C) possesses a lone pair of electrons
D) is always an Arrhenius base
3. Which of the following can act both as a Br๘nsted acid and base?
A) NH3
B) H2O
C) CO32–
D) OH–
4. An example of a Br๘nsted base is _____.
A) BF3
B) NH4+
C) HCN
D) NH3
5. The conjugate base of formic acid, HCOOH, is _____.
A) OH –
B) CH3 COO –
C) HCOO –
D) CO22–
6. In the reaction
, _____.
A)
B)
C)
D)
HPO42– is a conjugate acid
HPO42– is a conjugate base
NH3 is an acid
NH4+ is a conjugate base
Page 1
7. The conjugate acid of HSO4ฏ is _____.
A) H2SO4
B) SO4 2–
C) SO32–
D) HSO3–
8. Which one of the following will act only as a Br๘nsted base?
A) H2C2O4
B) HC2O4–
C) C2O42–
D) H3O+
9. The conjugate base of HIO4 is _____.
A) HIO3
B) IO4+
C) IO4–
D) H2IO3+
10. Which of the following is correct relating [H+] and [OH–] in solution at 25°C?
A) [H+] + [OH–] = 1 × 10–14
B) [H+] + [OH–] = 14.0
C) [H+] [OH–] = 1 × 1014
D) [H+] [OH–] = 1 × 10–14
11. pH is_______
A) log [H+]
B) – log 1/[H+]
C) -log [H+]
D) 1/log[H+]
12. The pH of a solution cannot be _____.
A) 0
B) –1
C) 10
D) ∞
Page 2
13. The equation relating pH and pOH is _____.
A) pH × pOH = 14
B) pH × pOH = 10–14
C) pH + pOH = 14
D) pH + pOH = –14
14. The concentration of OH– ions in a 1.4 × 10–3 M HCl solution is _____.
A) 7.1 × 10–12 M
B) 7.1 × 1012 M
C) 1.4 × 10–11 M
D) 1.4 × 10 11 M
15. The pH of a 0.62 M KOH solution is _____.
A) 0.21
B) 13.79
C) 1.21
D) 12.79
16. The pH of 2.8 × 10–4 M Ba(OH)2 will be _____.
A) 10.45
B) 3.55
C) 9.86
D) 10.75
17. The hydrogen ion concentration of a solution having a pH of 2.42 is _____.
A) 3.8 × 10 –3 M
B) 3.8 × 10 –2 M
C) 3.8 × 10 2 M
D) 2.4 × 10 –3 M
18. The hydrogen concentration of a solution having a pH 16 is _____.
A) 1 × 10 –2 M
B) 1 × 10 –16 M
C) 0
D) 1 × 10 –14 M
Page 3
19. Which of the following is true for a solution having pH < 7?
A) [H+] < 10 –7 M
B) [OH–] > 10 –7 M
C) It is a basic solution.
D) [H+] > 10 –7 M
20. Which of the following statements is true?
A) pOH > 7; The solution is basic.
B) pH > 7; The solution is acidic.
C) pH< 7; The solution is acidic.
D) pOH < 7; The solution is acidic.
21. The pOH of a solution is 9.40. Its hydrogen ion concentration is _____.
A) 2.5 × 10 –3 M
B) 2.5 × 10 –5 M
C) 1.5 × 10 –5 M
D) 2.5 × 10 –9 M
22. The number of moles of KOH in 5.50 mL of a 0.360 M KOH solution is _____.
A) 1.98 × 10 –2
B) 1.52 × 10 –3
C) 1.98 × 10 –3
D) 1.98
23. The pOH of 0.360 M KOH solution is _____.
A) 0.444
B) 13.556
C) 4.444
D) 9.556
24. How much NaOH is needed to prepare 546 mL solution with a pH=10.00?
A) 2.2 g
B) 2.2 × 10 2 g
C) 2.2 × 10 –3 g
D) 2.2 × 10 –2 g
Page 4
25. An example of a strong acid is _____.
A) CH3COOH
B) HCN
C) H2CO3
D) HClO4
26. Which one of the following statements is true?
A) The conjugate base of a strong acid is strong.
B) The conjugate base of a strong acid is weak.
C) The conjugate acid of a weak base is weak.
D) H2SO4 is a strong acid. Therefore, HSO4– is a strong conjugate base.
27. The weakest conjugate base below is _____.
A) CH3COO –
B) CN –
C) HSO4–
D) HCO3–
28. The weakest acid below is _____.
A) HCl
B) HClO4
C) HF
D) HNO3
29. The strongest base below is _____.
A) NH2–
B) Cl–
C) HSO4–
D) NH3
30. Which one of the following statements is true for a 1.0 M solution of a weak acid HA?
A) pH = 0
B) [H+] >> [A–]
C) [H+] = [A–]
D) pH < 1
Page 5
31. Which of the following statements is true for a 1.0 M solution of a strong acid HA?
A) [A–] > [H+]
B) [HA] = 1.0 M
C) pH = 1
D) pH = 0
32. Which of the following statements is true with respect to the reaction below?
A)
B)
C)
D)
The reaction favors the formation of F–(aq).
F– is a stronger base than OH–.
Hydrofluoric acid is a weaker acid than water.
The reaction favors the formation of HF(aq).
33. Which of the following statements is true with respect to the reaction below?
A)
B)
C)
D)
The reaction favours the formation of CH3COO–.
CH3COO– is a weaker base than Cl–.
Cl– is a weaker base than CH3COO–.
The reaction favours the formation of HCl.
34. Which of the following statements is correct with respect to an acid?
A) Stronger acids have smaller Ka values.
B) Weaker acids have smaller Ka values.
C) The strength of an acid is inversely proportional to its Ka value.
D) Weaker acids have greater H+ concentration.
35. Normally Ka values are quoted for an acid such as _____.
A) HCl
B) HNO3
C) H2SO4
D) HCN
36. Which of the following 0.40 M solutions has the highest pH?
A) HCOOH
B) HCl
C) HNO3
D) CH3COOH
Page 6
37. The pH of a 0.1 M benzoic acid solution (Ka = 6.5 × 10–5) is _____.
A) 3.6
B) 2.6
C) 2.0
D) 1.6
38. 0.056 g of CH3COOH (Ka = 1.8 × 10–5) is dissolved in enough water to obtain 50.0 mL
of solution. The concentration of H+ in the solution is _____.
A) 1.8 × 10–4 M
B) 1.8 × 10–3 M
C) 5.8 × 10–3 M
D) 5.8 × 10–4 M
39. What is the concentration of CH3COOH (Ka = 1.8 × 10–5) in 50.0 mL of a 0.0187 M
CH3COOH solution?
A) 0.0007 M
B) 0.0181 M
C) 0.0087 M
D) 1.87 × 10–3 M
40. The pH of a 0.010 M weak monoprotic acid is 6.20. The Ka of the acid is _____.
A) 4.0 × 10–11
B) 2.0 × 10–5
C) 4.0 × 10–8
D) 4.0 × 10–7
41. A formic acid (Ka = 1.7 × 10–4) solution has a pH of 3.26. What is the original molarity
of the HCOOH solution?
A) 4.6 × 10–2 M
B) 2.3 × 10–4 M
C) 4.6 × 10–3 M
D) 2.3 × 10–3 M
42. The percent ionization of 0.20 M benzoic acid (Ka = 6.5 × 10–5) is _____.
A) 18
B) 1.8
C) 4.3
D) 43
Page 7
43. The percent ionization of HF (Ka = 7.1 × 10–4) is greatest for which of the following HF
solutions?
A) 0.0046 M
B) 0.46 M
C) 0.00026 M
D) 1.6 M
44. A 0.040 M monoprotic acid solution is 14% ionized. Its Ka value is _____.
A) 9.1 × 10–4
B) 4.6 × 10–3
C) 2.3 × 10–6
D) 9.2 × 10–5
45. The percent ionization of a 0.20 M acetylsalicylic acid solution (Ka = 3.0 × 10–4) is
_____. (Acetylsalicylic acid is monoprotic)
A) 39%
B) 0.39%
C) 3.9%
D) 4.9%
46. The percent ionization of a 0.20 M acetylsalicylic acid solution in the stomach where
the pH is 1.00 is _____.
A) 3.0%
B) 0.30%
C) 30%
D) 0.03%
47. Which of the following 0.2 M solutions has the highest pH?
A) NH3
B) C6H5OH
C) NaOH
D) C5H5N
48. The pH of a 0.1 M aqueous NH3 solution (Kb = 1.8 × 10–5) will be _____.
A) 2.89
B) 11.13
C) 3.89
D) 10.11
Page 8
49. The pH of a 0.30 M solution of a weak base is 10.66. What is the Kb of the base?
A) 4.8 × 10–10
B) 1.85 × 10–5
C) 7.0 × 10–8
D) 7.0 × 10–7
50. What is the original molarity of an ammonia solution whose pH = 11.22 ?
A) 1.5 M
B) 0.15 M
C) 0.015 M
D) 1.5 × 10–3 M
51. The percent of NH3 present as NH4+ in 0.080 M NH3 solution is _____.
A) 15%
B) 2.5%
C) 25%
D) 1.5%
52. What is the relationship between the Ka for a weak acid and the Kb for its conjugate
base?
A) Ka + Kb = Kw
B) Ka Kb = Kw
C) Ka/Kb = Kw
D) Kb/Ka = Kw
53. The value of Kb for NH3 is 1.8 × 10–5. The value of Ka of NH4+ is _____.
A) 5.6 × 10–10
B) 5.6 × 104
C) 1.8 × 10–19
D) 1.8 × 10–9
54. An example of a diprotic acid is _____.
A) benzoic acid
B) carbonic acid
C) formic acid
D) hydrofluoric acid
Page 9
55. Which of the following will act only as Br๘nsted base?
A) H3PO4
B) PO43–
C) H2PO4–
D) HPO42–
56. The first and second ionization constants of a certain diprotic acid H2A are Ka1 and Ka2
at a certain temperature. Under what conditions will [A2–] =Ka2?
A) Ka1 = Ka2
B) Ka1 << Ka2
C) Ka1 >> Ka2
D) Ka1 + Ka2 = Kw
57. Which one of the following will have the lowest pH?
A) 0.04 M H2SO4
B) 0.04 M CH3COOH
C) 0.04 M HCl
D) 0.04 M NH3
58. Which of the following will be present in the smallest concentration in an aqueous 0.025
M H2CO3 solution?
A) H2CO3
B) CO32–
C) HCO3–
D) H3O+
59. The strength of an acid depends on _____.
A) properties of the solvent
B) temperature
C) molecular structure of the acid
D) all of the above
60. The strength of an oxoacid depends on the _____ of the central atom.
A) electronegativity
B) oxidation state
C) electronegativity and oxidation state
D) electron affinity.
Page 10
61. The strongest binary acid below is _____.
A) H2S
B) H2Se
C) H2O
D) CH4
62. The correct order of the strength of the acids below is _____.
A) H2SeO4 > H2SO4
B) H2SO4 > H2SeO4
C) H3PO4 < H3AsO4
D) HClO > HClO4
63. The strongest acid below is _____.
A) CH3 COOH
B) CH2Cl COOH
C) CH2F COOH
D) CH3 CH2 COOH
64. The correct order of acid strength is _____.
A) C6H5OH < CH3OH
B) HCOOH < CH3COOH
C) C6H5OH > CH3OH
D) CH3OH > CH3COOH
65. The pH of a 1.0 M aqueous solution of NaNO3 will be _____.
A) 1.0
B) 0
C) 7.0
D) 14.0
66. The ion below most likely to undergo hydrolysis is _____.
A) Na+
B) SO42–
C) Cl–
D) Al3+
Page 11
67. Which of the following is a Br๘nsted acid?
A) [Al(H2O)6]3+
B) Al3+
C) Ca(OH)2
D) PO43–
68. Which salt will not undergo hydrolysis?
A) KF
B) Na2CO3
C) K2SO4
D) NaI
69. Which salt will not undergo hydrolysis?
A) CH3COONa
B) NH4NO2
C) FeCl3
D) NaNO3
70. The pH of an aqueous solution of KBr will be _____.
A) > 7
B) < 7
C) 0
D) 7
71. Which of the following salt solutions will have pH > 7?
A) Bi(NO3)3
B) KBr
C) CH3COO Na
D) BaCl2
72. The alkaline earth metal ion most likely to undergo hydrolysis is _____.
A) Ba2+
B) Be2+
C) Ca2+
D) Sr2+.
Page 12
73. Which metal ion will not undergo hydrolysis?
A) Al3+
B) Bi3+
C) Be2+
D) Cs+
74. The pH values of 0.10 M solutions of the four salts KW, KX, KY and KZ were found to
be 7, 11, 8, 10, respectively. The weakest acid is _____.
A) HW
B) HY
C) HX
D) HZ
75. The pH of a 0.36 M CH3COONa solution will be _____.
A) 8.15
B) 7.00
C) 11.15
D) 9.15
76. The pH of a 0.42 M NH4Cl solution will be _____.
A) 4.82
B) 7.0
C) 9.82
D) 0.38
77. An aqueous solution of NaHCO3 will have a pH _____.
A) < 7
B) 7
C) 0
D) > 7
78. An aqueous solution of K2HPO4 will be _____.
A) basic
B) acidic
C) neutral
D) amphoteric
Page 13
79. An example of a neutral oxide is _____.
A) K2O
B) CO2
C) SO3
D) CO
80. Al2O3 is a(n) _____ oxide.
A) acidic
B) amphoteric
C) neutral
D) basic
81. Which of the following statements is correct?
A) A metal oxide will be basic if the oxidation number of the metal is high.
B) A metal oxide will be acidic if the oxidation number of the metal is high.
C) A metal oxide will be acidic if its oxidation number is low.
D) A neutral oxide is always a metallic oxide.
82. An example of an acidic oxide is _____.
A) CaO
B) Al2O3
C) N2O5
D) CaO
83. Which of the following oxides is most acidic?
A) Cr2O3
B) CrO
C) CrO3
D) Na2O
84. The increasing order of basicity of the oxide is _____.
A) Al2O3 < BaO < K2O
B) Al2O3 > BaO > K2O
C) CrO3 > Cr2O3 > CrO
D) K2O < BaO < Al2O3
Page 14
85. Zn(OH)2 is a(n) _____ hydroxide.
A) basic
B) acidic
C) neutral
D) amphoteric.
86. Zn(OH)2 will react with _____.
A) HCl
B) KOH
C) HNO3
D) all of the above
87. Zinc hydroxide reacts with NaOH to yield _____.
A) ZnO
B) [Zn(OH)4]2–
C) Zn(OH)4
D) ZnO2
88. Al(OH)3 dissolves in excess NaOH to yield _____.
A) Al2O3
B) Al(OH)2–
C) Al(OH)4–
D) AlH3
89. According to Lewis:
A) An acid is an electron pair donor.
B) An acid is electron pair acceptor.
C) A base is electron pair acceptor.
D) AlCl3 is a base.
90. A Lewis acid is _____.
A) electron rich
B) an anion
C) electron deficient
D) an electron donor
Page 15
91. An example of a Lewis acid is _____.
A) NH3
B) OH–
C) BCl3
D) I–
92. Which of the following is a Lewis base?
A) CO2
B) H2O
C) SO2
D) AlCl3
93. In the reaction:
A)
B)
C)
D)
Cl– acts as a Lewis acid.
AlCl3 acts as a Lewis base.
Cl– acts as a Lewis base.
AlCl4 –acts as a Lewis acid.
94. The correct order of Lewis acid strength is _____.
A) BCl3 > BF3
B) Fe3+ < Fe2+
C) Ag > Ag+
D) BF3 > BCl3
95. An example of a Lewis acid that is not Br๘nsted acid is _____.
A) SO2
B) CH3COOH
C) HIO4
D) HNO3
96. Which of the following statements is correct with respect to formic acid?
A) It is a weaker acid than acetic acid.
B) It is a weaker acid at high temperature.
C) It is a stronger acid at high temperature.
D) It is a diprotic acid.
Page 16
97. What volume of CO2 gas is generated at 1atm and 37ฐC from the reaction of 0.350g of
NaHCO3 with excess gastric juice(HCl) according to :
A)
B)
C)
D)
1.06 L
0.106 L
10.6 L
106 L
98. To which of the following would the addition of an equal volume of 0.60 M NaOH lead
to a solution with a lower pH?
A) water
B) 0.30 M HCl
C) 0.70 M KOH
D) 0.40 M NaNO3
99. HA and HB are both weak acids although HB is stronger than HA. 50.0 mL of 0.10 M
NaOH is required to neutralize 50 mL of 0.10 M HB. The volume of 0.10 M NaOH
required to neutralize 50.0 mL of 0.10 M HA is _____.
A) 50. ml
B) 55 ml
C) 45 ml
D) 100 ml
100. A solution contains the weak monoprotic acid HA and its sodium salt NaA, both at 0.10
M concentration. The concentration of OH– will be _____.
A) Ka/Kw
B) KaKw
C) Ka+Kw
D) Kw/Ka
101. The equilibrium constant for the reaction
is _____. (HCOOH : Ka
= 1.7 × 10 )
A) 1.7 × 10–10
B) 1.7 × 104
C) 1.7 × 1010
D) 1.7 × 10–8
–4
Page 17
102. The acid ionization constant for CH3COOH and HNO2 are 1.8 × 10–5 and 4.5 × 10–4,
respectively. The equilibrium constant for the reaction
is _____.
A)
B)
C)
D)
4.0 × 102
4.0 × 10–2
8.1 × 10–9
1.2 × 10–6
103. The hydride ion, H– reacts with water to yield _____.
A) O2
B) H2O2
C) H2
D) H2 and O2
104. The pH of a 0.20 M CH3COONH4 solution will be _____.
A) 3.00
B) 11.00
C) 0
D) 7.00
105. Novocaine is a weak base with Kb=8.91 × 10–6. What is the ratio of novocaine to that of
its conjugate acid at pH = 7.40?
A) 2.8
B) 0.028
C) 0.28
D) 0.0028
106. The strongest base below is _____.
A) NF3
B) NCl3
C) BCl3
D) NH3
107. The strongest base below is _____.
A) PH3
B) NH3
C) PCl3
D) BH3
Page 18
108. The ion product of D2O is 1.35 × 10–15 at 25ฐC. For a solution to be acidic pD must be
_____.
A) < 7.43
B) > 7.43
C) < 7.0
D) 7.0
109. The relation between pD and pOD for D2O (K = 1.35 × 10–15) is _____.
A) pD + pOD = 14
B) pD + pOD = 14.87
C) pD + pOD = 13.23
D) pD + pOD = 7.43
110. Which of the following is a weak acid?
A) HNO3
B) HClO4
C) HNO2
D) HIO4
111. The weakest acid below is _____.
A) HI
B) HNO3
C) H2SO4
D) HF
112. What is the pH of 250.0 mL of an aqueous solution containing 0.616g of the strong acid
trifluoromethane sulfonic(CF3SO3H) acid?
A) 4.79
B) 3.79
C) 2.79
D) 1.78
113. The hydronium ion is _____.
A) H+
B) H3O+
C) H–
D) OH–
Page 19
114. The pH of a 1.0 × 10–7 M aqueous HCl solution will be _____.
A) 7.2
B) 7.0
C) 6.8
D) 4.2
115. Hemoglobin( Hb) also exists in the protonated form as HbH+. The binding of oxygen
.
can be represented as
What form of hemoglobin is favoured in the lungs where the concentration of oxygen is
highest?
A) Hb
B) HbO2
C) HbH+
D) HbO
116. The concentration of H2PO4– in a 0.100 M H3PO4 solution is _______.
(Ka1 = 7.5 × 10–3, Ka2 = 6.2× 10–8, Ka3 = 4.8× 10–13)
A) 0.024 M
B) 0.012 M
C) 0.082 M
D) 0.042 M
117. The concentration of HCO3– in an aqueous solution of 0.10 M Na2CO3 is _____. The
ionization constants for H2CO3 are Ka1=4.2× 10–7 , Ka2=4.8× 10–11.
A) 4.6 × 10–3 M
B) 2.3 × 10–2 M
C) 2.3 × 10–3 M
D) 4.6 × 10–2 M
118. The Henry's law constant for CO2 at 38ฐC is 2.28 × 10–3 mol. L–1 atm–1. What is the pH
of a solution of CO2 at 38ฐC in equilibrium with CO2 gas at a partial pressure of 3.20
atm? The ionization constants for H2CO3 are Ka1=4.2 × 10–7 and Ka2=4.8 × 10–11
A) 5.26
B) 6.26
C) 4.26
D) 3.26
Page 20
119. How many grams of NaCN are needed to make 250.0 mL of a solution with a pH of
10.00?
A) 7.4 × 10–2 g
B) 7.4 × 10–3 g
C) 3.7 × 10–2 g
D) 7.4 g
120. A solution of formic acid has a pH of 2.53. How many grams of formic acid are there in
100.0 mL of the solution?
A) 2.4g
B) 0.24g
C) 0.024g
D) 0.0024g
121. What is the pH of a 1liter solution containing 0.150 mole of CH3COOH and 0.100 mole
of HCl?
A) 0.60
B) 1.30
C) 2.30
D) 1.00
122. 1.87g of Mg reacts with 80.0 mL of a HCl solution whose pH = -0.544. The pH of the
solution at the end of the reaction is _____.
A) –0.20
B) 0.20
C) 0.244
D) –0.244
123. Which of the following statements is correct with respect to a weak acid HB and a
strong acid HA of the same concentration?
A) pH of HA > pH of HB
B) pH of HA < pH of HB
C) HB will have greater conductance than HA.
D) [H+] in HB > [H+] in HA
124. Which of the following statements is correct with respect to the hydrolysis of NaNO2?
A) Addition of HCl enhances hydrolysis.
B) Addition of HCl decreases hydrolysis.
C) Addition of NaOH enhances hydrolysis.
D) Addition of NaCl enhances hydrolysis.
Page 21
125. Which of the following is a Lewis acid-base reaction?
A) oxidation of Fe2+ to Fe3+
B) hydration of SO2
C) ionization of NaCl
D) reduction of CH2O
126. Which of the following statements is true with respect to amines?
A) They are acids like formic acid.
B) They are bases like ammonia.
C) They react with ammonia to form salts.
D) They are Br๘nsted acids.
127. A solution of methylamine (CH3NH2) has a pH of 10.64. How many grams of
methylamine are present in 100.0 mLof the solution? (Kb = 4.4 × 10–4)
A) 2.6 × 10–2 g
B) 0.26
C) 2.6 × 10–3 g
D) 2.6 g
128. A 0.400M aqueous solution of a weak monoprotic acid freezes at –0.758ฐC. What is the
Ka for the acid? (Assume that the molarity of the solution is equal to the molality.)
A) 1.6 × 10–3
B) 1.6 × 10–4
C) 1.6 × 10–2
D) 1.6 × 10–5
129. Which among the following statements is correct with respect to NH2– and N3–?
A) NH2– reacts with water to yield NH3 and O2.
B) N3– reacts with water to yield NH3 and OH–.
C) N3– reacts with water to yield NH4+ and OH–.
D) NH2– reacts with water to yield NH4+ and H2O2.
130. Atmospheric air in some region contains 0.12 ppm of SO2 by volume. The pH of
rainwater due to this pollutant is _____. Assume that the dissolution of SO2 does not
affect its pressure. (Ka1 for H2SO3 is 1.3 × 10–2)
A) 3.40
B) 5.40
C) 2.40
D) 4.40
Page 22
131. The ionization constant of HClO is 3.0 × 10–8. The percent of ClO– present at a pH of
7.80 is _____.
A) 66%
B) 26%
C) 36%
D) 46%
Page 23
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42.
43.
44.
A
C
B
D
C
B
A
C
C
D
C
D
C
A
B
D
A
B
D
C
B
C
A
C
D
B
C
C
A
C
D
A
C
B
D
D
B
D
B
A
D
B
C
A
Page 24
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.
C
B
C
B
D
B
D
B
A
B
B
C
A
B
D
C
B
B
C
C
C
D
A
D
D
D
C
B
D
C
D
A
D
A
D
B
B
C
C
A
D
D
B
C
B
C
Page 25
91.
92.
93.
94.
95.
96.
97.
98.
99.
100.
101.
102.
103.
104.
105.
106.
107.
108.
109.
110.
111.
112.
113.
114.
115.
116.
117.
118.
119.
120.
121.
122.
123.
124.
125.
126.
127.
128.
129.
130.
131.
C
B
C
D
A
C
B
C
A
D
C
B
C
D
B
D
B
A
B
C
D
D
B
C
B
A
A
C
B
B
D
A
B
A
B
B
C
B
B
D
A
Page 26