Exam
Name___________________________________
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
1) In which of the following aqueous solutions does the weak acid exhibit the highest percentage
ionization?
1)
A) 0.01 M HF (Ka = 6.8 × 10-4 )
B) 0.01 M HC2 H3 O2 (Ka = 1.8 × 10-5 )
C) 0.01 M HNO2 (Ka = 4.5 × 10-4 )
D) 0.01 M HClO (Ka = 3.0 × 10-8 )
E) These will all exhibit the same percentage ionization.
2) The base-dissociation constant of ethylamine (C2 H5 NH2 ) is 6.4 × 10-4 at 25.0 °C. The of [H+ ] in a
1.6 × 10-2 M solution of ethylamine is __________ M.
2)
A) 3.1 × 10-12
B) 11.46
C) 2.9 × 10-3
D) 3.5 × 10-12
E) 3.2 × 10-3
3) A Br ∅nsted-Lowry base is defined as a substance that __________.
3)
A) acts as a proton acceptor
B) acts as a proton donor
C) increases [H+ ] when placed in H2 O
D) increases [OH- ] when placed in H2 O
E) decreases [H+ ] when placed in H2 O
4) Which of the following acids will be the strongest?
A) H2 SO3
B) H2 SeO4
4)
C) HSO3 -
1
D) HSO4 -
E) H2 SO4
5) In the gas phase reaction below, NH3 is acting as a(n) __________ base but not as a(n) __________
base.
. .
5)
H+
|
N + H+ → N
|
|
H H H
H H H
A) Arrhenius, Br ∅nsted-Lowry
B) Arrhenius, Lewis
C) Lewis, Br∅nsted-Lowry
D) Br∅nsted-Lowry, Lewis
E) Lewis, Arrhenius
6) Which of the following ions will act as a weak base in water?
6)
A) OHB) ClC) ClOD) NO3 E) None of the above will act as a weak base in water.
7) The molar concentration of hydroxide ion in pure water at 25 °C is __________.
A) 0.00
B) 1.0 ×10-14
C) 1.0 × 10-7
D) 7.00
7)
E) 1.00
8) Which solution below has the highest concentration of hydroxide ions?
A) pH = 3.21
B) pH = 7.00
C) pH = 9.82
9) Of the following, which is the strongest acid?
D) pH = 12.6
8)
E) pH = 7.93
9)
A) HIO4
B) HIO3
C) HIO
D) HIO2
E) The acid strength of all of the above is the same.
2
10) An aqueous solution at 25.0 °C contains [H+ ] = 0.0990 M. What is the pH of the solution?
10)
A) 0.0990
B) 1.00
C) 1.00× 10-13
D) -1.00
E) 13.0
11) Of the acids in the table below, __________ is the strongest acid.
Acid
11)
Ka
1.8 × 10-5
HCHO2 1.8 × 10-4
HClO
3.0 × 10-8
HOAc
HF
6.8 × 10-4
A) HClO
B) HOAc
C) HOAc and HCHO2
D) HCHO2
E) HF
12) The acid-dissociation constant at 25.0 °C for hypochlorous acid (HClO) is 3.0 × 10-8 . At
equilibrium, the molarity of H3 O+ in a 0.010 M solution of HClO is __________.
A) 4.76
B) 1.7 × 10-5
C) 2.00
D) 0.010
E) 5.8 × 10-10
3
12)
13) Using the data in the table, which of the conjugate bases below is the strongest base?
Acid
13)
Ka
1.8 × 10-5
HCHO2 1.8 × 10-4
HClO
3.0 × 10-8
HOAc
HF
6.8 × 10-4
A) FB) CHO2 C) OAcD) ClOE) OAc- and CHO2 14) Nitric acid is a strong acid. This means that __________.
14)
A) HNO3 dissociates completely to H+ (aq) and NO3 - (aq) when it dissolves in water
B) HNO3 cannot be neutralized by a weak base
C) HNO3 does not dissociate at all when it is dissolved in water
D) aqueous solutions of HNO3 contain equal concentrations of H+ (aq) and OH- (aq)
E) HNO3 produces a gaseous product when it is neutralized
15) According to the Arrhenius concept, an acid is a substance that __________.
15)
A) causes an increase in the concentration of H+ in aqueous solutions
B) reacts with the solvent to form the cation formed by autoionization of that solvent
C) tastes bitter
D) is capable of donating one or more H+
E) can accept a pair of electrons to form a coordinate covalent bond
16) Of the compounds below, a 0.1 M aqueous solution of __________ will have the highest pH.
A) KCN, Ka of HCN = 4.0 × 10-10
B) NH4 NO3 , Kb of NH3 = 1.8 × 10-5
C) NaClO, Ka of HClO = 3.2 × 10-8
D) NaHS, Kb of HS- = 1.8 × 10-7
E) NaOAc, Ka of HOAc = 1.8 × 10-5
4
16)
17) The hydride ion, H- , is a stronger base than the hydroxide ion, OH- . The product(s) of the reaction
of hydride ion with water is/ are __________.
17)
A) OH- (aq) + 2H+ (aq)
B) H2 O2 (aq)
C) OH- (aq) + H2 (g)
D) no reaction occurs
E) H3 O+ (aq)
18) Of the following, which is the strongest acid?
A) HClO3
B) HClO
18)
C) HClO2
D) HClO4
E) HIO
19) A substance that is capable of acting as both an acid and as a base is __________.
19)
A) conjugated
B) autosomal
C) miscible
D) saturated
E) amphoteric
20) Calculate the molarity of hydroxide ion in an aqueous solution that has a pOH of 5.33.
20)
A) 4.7 × 10-6
B) 2.1 × 10-9
C) 8.67
D) 8.7 × 10-14
E) 5.3 × 10-14
21) The Ka of hypochlorous acid (HClO) is 3.0 × 10-8 at 25.0 °C. What is the % ionization of
hypochlorous acid in a 0.015-M aqueous solution of HClO at 25.0 °C?
A) 4.5 × 10-8
B) 0.14
D) 1.4 × 10-3
C) 14
E) 2.1 × 10-5
22) A 0.0035-M aqueous solution of a particular compound has pH = 2.46. The compound is
__________.
A) a strong acid
B) a strong base
C) a salt
D) a weak base
E) a weak acid
5
21)
22)
23) Which of the following aqueous solutions has the highest [ OH- ]?
23)
A) a 1 × 10-3 M solution of NH4 Cl
B) a solution with a pH of 3.0
C) a solution with a pOH of 12.0
D) pure water
E) a 1 × 10-4 M solution of HNO3
24) The molar concentration of hydronium ion in pure water at 25 °C is __________.
24)
A) 1.0 × 10-7
B) 0.00
C) 1.0 × 10-14
D) 1.00
E) 7.00
25) Which one of the following is a Br ∅nsted-Lowry acid?
25)
A) CH3 COOH
B) HF
C) HNO2
D) (CH3 )3 NH+
E) all of the above
26) HA is a weak acid. Which equilibrium corresponds to the equilibrium constant Kb for A- ?
A) A- (aq) + OH- (aq) B) HA (aq) + H2 O (l) C) A- (aq) + H2 O (l) HOA2- (aq)
H2 A+ (aq) + OH- (aq)
HA (aq) + OH- (aq)
D) HA (aq) + OH- (aq) H2 O (l) + H+ (aq)
E) A- (aq) + H3 O+ (aq) HA (aq) + H2 O (l)
27) Of the following acids, __________ is not a strong acid.
A) HNO3
B) H2 SO4
C) HNO2
27)
D) HCl
E) HClO4
28) Classify the following compounds as weak acids (W) or strong acids (S):
hypochlorous acid
A) W W W
26)
perchloric acid
B) W S S
28)
chloric acid
C) S S S
6
D) S W W
E) W S W
29) An aqueous solution contains 0.10 M NaOH. The solution is __________.
29)
A) neutral
B) highly colored
C) very dilute
D) basic
E) acidic
30) An aqueous solution of __________ will produce a basic solution.
A) Na2 SO3
B) NH4 ClO4
C) NaHSO4
D) KBr
30)
E) NaCl
31) Classify the following compounds as weak acids (W) or strong acids (S):
nitrous acid
A) W S W
hydrochloric acid
B) W W W
31)
hydrofluoric acid
C) S W W
D) S S S
E) W S S
32) A 0.1 M aqueous solution of __________ will have a pH of 7.0 at 25.0 °C.
32)
NaOCl KCl NH4 Cl Ca(OAc) 2
A) NaOCl
B) KCl
C) NH4 Cl
D) Ca(OAc)2
E) KCl and NH4 Cl
33) The concentration of water in pure water is approximately __________ M.
A) 55
B) 18
C) 0.100
D) 83
33)
E) 100
34) A 0.1 M solution of __________ has a pH of 7.0.
A) NaF
B) NH4 Cl
34)
C) KF
D) NaNO3
35) A Br ∅nsted-Lowry acid is defined as a substance that __________.
A) acts as a proton acceptor
B) increases [H+ ] when placed in H2 O
C) decreases [H+ ] when placed in H2 O
D) increases [OH- ] when placed in H2 O
E) acts as a proton donor
7
E) Na2 S
35)
36) A 7.0 × 10-3 M aqueous solution of Ca(OH) 2 at 25.0 °C has a pH of __________.
36)
A) 11.85
B) 1.85
C) 12.15
D) 7.1 × 10-13
E) 1.4 × 10-2
37) Of the following substances, an aqueous solution of __________ will form basic solutions.
37)
NH4 Cl Cu(NO3 )2 K2 CO3 NaF
A) K2 CO3 , NH4 Cl
B) NH4 Cl only
C) NaF only
D) NaF, K2 CO3
E) NH4 Cl , Cu(NO3 )2
38) In basic solution, __________.
38)
A) [H3 O+ ] = [OH- ]
B) [H3 O+ ] > [OH- ]
C) [OH- ] > 7.00
D) [H3 O+ ] < [OH- ]
E) [H3 O+ ] = 0 M
39) Which one of the following statements regarding K w is false?
39)
A) Kw changes with temperature.
B) pKw is 14.00 at 25°C
C) Kw is known as the ion product of water.
D) The value of Kw shows that water is a weak acid.
E) The value of Kw is always 1.0 × 10-14.
40) The magnitude of Kw indicates that __________.
40)
A) water autoionizes very slowly
B) the autoionization of water is exothermic
C) water autoionizes only to a very small extent
D) water autoionizes very quickly
8
41) Of the following, __________ is a weak acid.
A) HF
B) HBr
41)
C) HNO3
D) HClO4
E) HCl
42) Classify the following compounds as weak bases (W) or strong bases (S):
ammonia A) S W W
flouride ion
B) S S S
42)
sodium hydroxide
C) W S S
D) W W S
E) W S W
43) The pH of an aqueous solution at 25.0 °C is 10.66. What is the molarity of H+ in this solution?
43)
A) 1.1 × 10-13
B) 4.6 × 10-4
C) 4.6 × 1010
D) 3.3
E) 2.2 × 10-11
44) Which one of the following is the weakest acid?
44)
A) HF (Ka = 6.8 × 10-4 )
B) HNO2 (Ka = 4.5 × 10-4 )
C) HClO (Ka = 3.0 × 10-8 )
D) Acetic acid (Ka = 1.8 × 10-5 )
E) HCN (Ka = 4.9 × 10-10)
45) Ammonia is a __________.
45)
A) weak base
B) strong base
C) salt
D) strong acid
E) weak acid
46) The acid-dissociation constant of hydrocyanic acid (HCN) at 25.0 °C is 4.9 × 10-10. What is the pH
of an aqueous solution of 0.080 M sodium cyanide (NaCN)?
A) 7.8 × 10-12
B) 11.11
C) 1.3 × 10-3
D) 3.9 × 10-11
E) 2.89
9
46)
SHORT ANSWER. Write the word or phrase that best completes each statement or answers the question.
47) A solution of acetic acid is 2.0% dissociated at 25.0 oC. What was the original
concentration ( in M) of the acetic acid solution? The K a at 25.0 oC for acetic acid is 1.8 ×
47)
10-5 .
48) What is the pH of a sodium acetate solution prepared by adding 0.820 grams of sodium
acetate to 100.0 ml of water at 25.0 oC? The Ka at 25.0 oC for acetic acid is 1.8 × 10-5 .
48)
49) What is the pH of a sodium formate solution prepared by adding 0.680 grams of sodium
formate to 100.0 ml of water at 25.0 oC? The Ka at 25.0 oC for formic acid is 1.8 × 10-4 .
49)
50) A solution of ammonia is 2.0% dissociated at 25.0 oC. What was the original concentration
( in M) of the ammonia solution? The K b at 25.0 oC for ammonia is 1.8 × 10-5 .
50)
51) A solution of formic acid is 3.0% dissociated at 25.0 oC. What is the original concentration
(in M) of the formic acid solution? The K a at 25.0 oC for formic acid is 1.8 × 10-4 .
51)
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
52) The Ka of hydrofluoric acid (HF) at 25.0 °C is 6.8 × 10-4 . What is the pH of a 0.35 M aqueous
solution of HF?
A) 0.46
B) 3.6
C) 1.8
D) 3.2
E) 12
53) What is the pH of an aqueous solution at 25.0 °C that contains 3.98 × 10-9 M hydronium ion?
A) 5.60
B) 7.00
C) 3.98
D) 8.40
B) 8.40
C) 5.60
D) 3.98
53)
E) 9.00
54) What is the pH of an aqueous solution at 25.0 °C that contains 3.98 × 10-9 M hydroxide ion?
A) 7.00
52)
54)
E) 9.00
55) The acid-dissociation constant for chlorous acid, HClO 2 , at 25.0 °C is 1.0 × 10-2 . Calculate the
55)
concentration of H + if the initial concentration of acid is 0.10 M.
A) 3.7 × 10-2
B) 2.7 × 10-2
C) 1.0 × 10-2
D) 1.0 × 10-3
E) 3.2 × 10-2
56)
56) What is the conjugate acid of NH3 ?
A) NH2 +
B) NH4 OH
C) NH3 +
10
D) NH4 +
E) NH3
57) HZ is a weak acid. An aqueous solution of HZ is prepared by dissolving 0.020 mol of HZ in
sufficient water to yield 1.0 L of solution. The pH of the solution was 4.93 at 25.0 °C. The Ka of HZ
57)
is __________.
A) 6.9 × 10-9
B) 1.4 × 10-10
C) 1.2 × 10-5
D) 2.8 × 10-12
E) 9.9 × 10-2
58) The conjugate base of HSO4 - is
A) H2 SO4
B) H3 SO4 +
58)
C) SO4 2-
D) OH-
E) HSO4 +
59) What is the pH of an aqueous solution at 25.0 °C in which [OH- ] is 0.00250 M?
A) +2.60
B) -2.60
C) +11.4
D) -11.4
59)
E) -2.25
60) What is the pH of a 0.0150 M aqueous solution of barium hydroxide?
A) 12.5
B) 12.2
C) 1.52
D) 10.4
60)
E) 1.82
61) Calculate the pH of 0.726 M anilinium hydrochloride (C6 H5 NH3 Cl) solution in water, given that
Kb for aniline is 3.83 × 10-4 .
A) 5.36
B) 8.64
C) 12.2
D) 12.4
61)
E) 1.77
62) The Ka for HCN is 4.9 × 10-10. What is the value of Kb for CN- ?
62)
A) 2.0 × 109
B) 4.0 × 10-6
C) 2.0 × 10-5
D) 4.9 × 104
E) 4.9 × 10-24
63)
63) The pH of a 0.10 M solution of a weak base is 9.82. What is the Kb for this base?
A) 4.3 × 10-8
B) 2.1 × 10-4
C) 8.8 × 10-8
11
D) 2.0 × 10-5
E) 6.6 × 10-4
64) The acid-dissociation constants of phosphoric acid (H3 PO4 ) are Ka1 = 7.5 × 10-3 , Ka2 = 6.2 × 10-8 ,
and Ka3 = 4.2 × 10-13 at 25.0 °C. What is the molar concentration of phosphate ion in a 2.5 M
64)
aqueous solution of phosphoric acid?
A) 9.1 × 10-5
B) 2.0 × 10-19
C) 0.13
D) 8.2 × 10-9
E) 2.5 × 10-5
65) The pH of a 0.55 M aqueous solution of hypobromous acid, HBrO, at 25.0 °C is 4.48. What is the
value of Ka for HBrO?
A) 6.0 × 10-5
B) 2.0 × 10-9
C) 3.0 × 104
D) 1.1 × 10-9
65)
E) 3.3 × 10-5
66) The base-dissociation constant, Kb, for pyridine, C5 H5 N, is 1.4 × 10-9 . The acid-dissociation
constant, Ka , for the pyridinium ion, C5 H5 NH+ , is __________.
66)
A) 1.4 × 10-23
B) 7.1 × 10-4
C) 7.1 × 10-6
D) 1.0 × 10-7
E) 1.4 × 10-5
67) The acid-dissociation constants of phosphoric acid (H3 PO4 ) are Ka1 = 7.5 × 10-3 , Ka2 = 6.2 × 10-8 ,
67)
and Ka3 = 4.2 × 10-13 at 25.0 °C. What is the pH of a 2.5 M aqueous solution of phosphoric acid?
A) 0.40
B) 2.5
C) 0.87
D) 1.8
E) 0.13
68) What is the concentration (in M) of hydroxide ions in a solution at 25.0 °C with pH = 4.282?
68)
A) 1.91 × 10-10
B) 1.66 × 104
C) 5.22 × 10-5
D) 9.72
E) 4.28
69) The Ka of hydrazoic acid (HN3 ) is 1.9 × 10-5 at 25.0 °C. What is the pH of a 0.35 M aqueous
solution of HN3 ?
A) 2.4
B) 5.2
C) -2.4
D) 2.6
E) 11
70) Ka for HCN is 4.9 × 10-10. What is the pH of a 0.068 M aqueous solution of sodium cyanide?
A) 7.0
B) 0.74
C) 11
D) 13
12
69)
E) 2.9
70)
71) Calculate the pOH of a 0.0827 M aqueous sodium cyanide solution at 25.0 °C. Kb for CN- is
71)
4.9 × 10-10.
A) 8.8
B) 5.2
C) 1.1
D) 10
E) 9.3
72) An aqueous solution contains 0.050 M of methylamine. The concentration of hydroxide ion in this
solution is ________M. K b for methylamine is 4.4 × 10-4 .
72)
A) 0.050
B) 4.5 × 10-3
C) 2.2 × 10-5
D) 4.7 × 10-3
E) -4.9 × 10-3
73) The Ka of hypochlorous acid (HClO) is 3.00 × 10-8 at 25.0 °C. Calculate the pH of a 0.0385 M
hypochlorous acid solution.
A) -1.41
B) 1.41
C) 8.94
D) 4.47
73)
E) 7.52
74) Calculate the concentration (in M) of hydronium ions in a solution at 25.0 °C with a pOH of 4.223.
74)
A) 5.99 × 10-19
B) 1.67 × 104
C) 1.67 × 10-10
D) 1.00 × 10-7
E) 5.98 × 10-5
75) Calculate the pH of a 0.500 M aqueous solution of NH3 . The Kb of NH3 is 1.77 × 10-5 .
A) 2.52
B) 11.5
C) 3.01
D) 5.05
75)
E) 8.95
76) What is the concentration (in M) of hydronium ions in a solution at 25.0 °C with pH = 4.282?
76)
A) 1.66 × 104
B) 9.71
C) 5.22 × 10-5
D) 4.28
E) 1.92 × 10-10
77) Calculate the pOH of a solution at 25.0 °C that contains 1.94 × 10-10 M hydronium ions.
A) 4.29
B) 7.00
C) 14.0
D) 1.94
13
E) 9.71
77)
78) A 0.15 M aqueous solution of the weak acid HA at 25.0 °C has a pH of 5.35. The value of Ka for HA
78)
is __________.
A) 3.0 × 10-5
B) 7.1 × 10-9
C) 1.8 × 10-5
D) 3.3 × 104
E) 1.4 × 10-10
79) What is the conjugate base of OH- ?
A) H3 O+
B) O2
79)
C) H2 O
D) O2-
E) O-
80) An aqueous solution contains 0.100 M NaOH at 25.0 °C. The pH of the solution is __________.
A) 0.100
B) 1.00
D) -1.00
C) 13.0
E) 7.00
81) Determine the pH of a 0.35 M aqueous solution of CH3 NH2 (methylamine). The Kb of
methylamine is 4.4 × 10-4 .
A) 3.8
B) 12
C) 1.9
D) 13
B) 2.25
D) -2.60
C) 2.60
81)
E) 10
82) What is the pH of an aqueous solution at 25.0 °C in which [H+ ] is 0.00250 M?
A) -3.40
80)
82)
E) 3.40
83) The acid-dissociation constant, Ka , for gallic acid is 4.57 × 10-3 . What is the base-dissociation
constant, Kb, for the gallate ion?
83)
A) 2.19 × 102
B) 2.19 × 10-12
C) 7.81 × 10-6
D) 5.43 × 10-5
E) 4.57 × 10-3
84) What is the pOH of a 0.0150 M solution of barium hydroxide?
A) 12.5
B) 10.4
C) 12.2
84)
D) 1.82
E) 1.52
85) The pH of a 0.15 M aqueous solution of NaZ (the sodium salt of HZ) is 10.7. What is the Ka for
HZ?
A) 3.3 × 10-8
B) 1.6 × 10-6
C) 6.0 × 10-9
D) 8.9 × 10-4
E) 1.3 × 10-12
14
85)
86) Determine the pH of a 0.15 M aqueous solution of KF. For hydrofluoric acid, Ka = 7.0 × 10-4 .
A) 5.8
B) 8.2
C) 12
D) 6.6
E) 2.3
87) The conjugate acid of HSO4 - is
A) H+
B) SO4 2-
87)
C) HSO3 +
D) H2 SO4
E) HSO4 +
88) Kb for NH3 is 1.8 × 10-5 . What is the pH of a 0.35 M aqueous solution of NH4 Cl at 25.0 °C?
A) 4.3
B) 9.1
86)
C) 9.7
D) 4.9
88)
E) 11
89) Ka for HF is 7.0 × 10-4 . Kb for the fluoride ion is __________.
89)
A) 1.4 × 103
B) 1.4 × 10-11
C) 2.0 × 10-8
D) 7.0 × 10-4
E) 7.0 × 10-18
90) The Ka for formic acid (HCO2 H) is 1.8 × 10-4 . What is the pH of a 0.35 M aqueous solution of
sodium formate (NaHCO2 )?
A) 4.2
B) 5.4
C) 11
D) 3.3
E) 8.6
91) The acid-dissociation constants of sulfurous acid (H2 SO3 ) are Ka1 = 1.7 × 10-2 and
Ka2 = 6.4 × 10-8 at 25.0 °C. Calculate the pH of a 0.163 M aqueous solution of sulfurous acid.
A) 7.2
B) 1.4
C) 4.5
D) 1.8
B) 1.9
C) 7.9
D) 12
92)
E) 6.0
93) The Ka of hypochlorous acid (HClO) is 3.00 × 10-8 . What is the pH at 25.0 °C of an aqueous
solution that is 0.0200 M in HClO?
A) +2.45
B) -2.45
C) -9.22
D) +9.22
91)
E) 1.3
92) Ka for HX is 7.5 × 10-12. What is the pH of a 0.15 M aqueous solution of NaX?
A) 8.0
90)
93)
E) +4.61
TRUE/FALSE. Write ʹTʹ if the statement is true and ʹFʹ if the statement is false.
94) A Lewis acid is an electron-pair acceptor, and a Lewis base is an electron -pair donor.
94)
95) When the proton in the COOH group in an amino acid is transferred to the N H2 group of that
same amino acid molecule, a zwitterion is formed.
95)
15
96) In the reaction
96)
BF3 + F- → BF4 BF3 acts as a Br∅nsted-Lowry acid.
97) The simplest amino acid is glycine.
97)
98) An acid containing the COOH group is called a carbo-oxy acid.
98)
16
Answer Key
Testname: ACIDBASE
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28)
29)
30)
31)
32)
33)
34)
35)
36)
37)
38)
39)
40)
41)
42)
43)
44)
45)
46)
47)
48)
49)
50)
A
D
A
E
E
C
C
D
A
B
E
B
D
A
A
A
C
D
E
A
B
A
D
A
E
C
C
B
D
A
A
B
A
D
E
C
D
D
E
C
A
D
E
E
A
B
0.045
8.87
8.37
0.045
17
Answer Key
Testname: ACIDBASE
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)
91)
92)
93)
94)
95)
96)
97)
98)
0.20
C
D
C
B
D
A
C
C
A
A
C
A
B
B
C
C
A
D
C
B
B
D
C
B
C
A
E
D
C
B
C
B
E
C
B
D
D
B
E
B
D
E
TRUE
TRUE
FALSE
TRUE
FALSE
18