Unit 16 Practice Test

Name: ________________________ Class: ___________________ Date: __________
ID: A
Unit 16 Practice Test
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____
1) According to the Arrhenius concept, an acid is a substance that ________.
A) is capable of donating one or more H +
B) causes an increase in the concentration of H+ in aqueous solutions
C) can accept a pair of electrons to form a coordinate covalent bond
D) reacts with the solvent to form the cation formed by autoionization of that solvent
E) tastes bitter
____
2) A Brnsted-Lowry acid is defined as a substance that ________.
A) increases Ka when placed in H2O
B) decreases [H+] when placed in H2O
C) increases [OH–] when placed in H2O
D) acts as a proton acceptor
E) acts as a proton donor
____
3) A substance that is capable of acting as both an acid and as a base is ________.
A) autosomal
B) conjugated
C) ambiprotic
D) saturated
E) miscible
____
4) The magnitude of Kw indicates that ________.
A) water autoionizes very slowly
B) water autoionizes very quickly
C) water autoionizes only to a very small extent
D) the autoionization of water is exothermic
____
5) 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 ________.
A) H3O+ (aq)
B) OH– (aq) + H2 (g)
C) OH– (aq) + 2H+ (aq)
D) no reaction occurs
E) H2O2 (aq)
____
6) Of the following acids, ________ is not a strong acid.
A) HNO2
B) H2SO4
C) HNO3
D) HClO4
E) HCl
1
Name: ________________________
ID: A
____
7) The Ka of hypochlorous acid (HClO) is 3.0  10–8 at 25 °C. What is the percent ionization of hypochlorous
acid in a 0.015 M aqueous solution of HClO at 25 °C?
A) 4.5  10–8
B) 14
C) 2.1  10–5
D) 0.14
E) 1.4  10–3
____
8) Classify the following compounds as weak acids (W) or strong acids (S):
A)
B)
C)
D)
E)
____
hypochlorous acid
WSS
SSS
SWW
WWW
WSW
perchloric acid
chloric acid
9) HA is a weak acid. Which equilibrium corresponds to the equilibrium constant Kb for A –?
A) HA (aq) + H2O (l)
H2A+ (aq) + OH–(aq)
–
+
HA (aq) + H2O (l)
B) A (aq) + H3O (aq)
H2O (l) + H+ (aq)
C) HA (aq) + OH– (aq)
–
HA (aq) + OH– (aq)
D) A (aq) + H2O (l)
–
–
E) A (aq) + OH (aq)
HOA2– (aq)
____ 10) Classify the following compounds as weak bases (W) or strong bases (S):
A)
B)
C)
D)
E)
ammonia
WWS
SSS
SWW
WS S
WSW
fluoride ion
sodium hydroxide
____ 11) Using the data in the table, which of the conjugate bases below is the strongest base?
A)
B)
C)
D)
E)
OAc–
CHO2–
ClO–
F–
OAc– and CHO2–
2
Name: ________________________
ID: A
____ 12) Using the data in the table, which of the conjugate acids below is the strongest acid?
A)
B)
C)
D)
E)
HClO
HCO3–
H2S
NH3CH3+
H2S and HClO
____ 13) Using the data in the table, which of the conjugate acids below is the strongest acid?
A)
B)
C)
D)
E)
NH4+
C5H5NH+
H3NOH+
NH3CH3+
NH4+ and NH3CH3+
____ 14) Which of the following ions will act as a weak base in water?
A) OH–
B) Cl–
C) NO3–
D) ClO–
E) None of the above will act as a weak base in water.
____ 15) A 0.0035 M aqueous solution of a particular compound has pH = 2.46. The compound is ________.
A) a weak base
B) a weak acid
C) a strong acid
D) a strong base
E) a salt
3
Name: ________________________
ID: A
____ 16) Of the following substances, an aqueous solution of ________ will form basic solutions.
A)
B)
C)
D)
E)
NH4Cl
Cu(NO3)2
NH4Cl, Cu(NO3)2
K2CO3, NH4Cl
NaF only
NaF, K2CO3
NH4Cl only
K2CO3
NaF
____ 17) Of the following, which is the strongest acid?
A) HClO
B) HClO3
C) HClO2
D) HClO4
E) HIO
____ 18) The conjugate base of HSO4– is ________.
A) OH–
B) H2SO4
C) SO42–
D) HSO4+
E) H3SO4+
____ 19) The conjugate acid of HSO4– is ________.
A) SO42–
B) H2SO4
C) HSO4+
D) H+
E) HSO3+
____ 20) What is the conjugate base of OH–?
A) O2
B) O–
C) H2O
D) O2–
E) H3O+
____ 21) What is the pOH of an aqueous solution at 25.0 °C that contains 3.98  10–9 M hydronium ion?
A) 8.400
B) 5.600
C) 9.000
D) 3.980
E) 7.000
4
Name: ________________________
ID: A
____ 22) Calculate the concentration (in M) of hydroxide ions in a solution at 25.0 °C with a pOH of 4.223.
A) 5.98  10–5
B) 1.67  10–10
C) 1.67  104
D) 5.99  10–19
E) 1.00  10–7
____ 23) An aqueous solution contains 0.150 M HCl at 25.0 °C. The pH of the solution is ________.
A) 0.150
B) 1.00
C) 13.00
D) 7.00
E) 0.82
____ 24) 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 K a
for HBrO?
A) 2.0  10–9
B) 1.1  10–9
C) 6.0  10–5
D) 3.3  10–5
E) 3.0  104
____ 25) The pH of a 0.60 M aqueous solution of formic acid, HCHO 2, at 25.0 °C is 1.98. What is the value of K a for
formic acid?
A) 2.0  10–5
B) 1.8  10–4
C) 6.0  10–5
D) 3.5  10–4
E) none of the above
____ 26) 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
E) +4.61
____ 27) The acid-dissociation constants of sulfurous acid (H 2SO3) 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) 4.53
B) 1.28
C) 1.86
D) 6.21
E) 1.93
5
Name: ________________________
ID: A
____ 28) The pH of a 0.55 M aqueous solution ammonia, NH 3, at 25.0 °C is 11.50. What is the value of K b for NH3?
A) 2.0  10–9
B) 1.1  10–9
C) 6.0  10–5
D) 1.8  10–5
E) none of the above
____ 29) The pH of a 0.10 M solution of a weak base is 9.82. What is the K b for this base?
A) 2.1  10–4
B) 4.4  10–8
C) 8.8  10–8
D) 6.6  10–4
E) 2.0  10–5
____ 30) 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.
A) 0.050
B) 2.2  10–5
C) 2.9  10–3
D) 4.5  10–3
E) 4.7  10–3
____ 31) Ka for HCN is 4.9  10–10. What is the pH of a 0.068 M aqueous solution of sodium cyanide?
A) 0.74
B) 2.96
C) 11.07
D) 13.24
E) 7.00
____ 32) The conjugate base of H2PO4– is ________.
A) H3PO4
B) HPO42–
C) PO43–
D) H3O+
E) OH–
____ 33) Calculate the molarity of hydroxide ion in an aqueous solution that has a pOH of 3.00.
A) 1.0  10–3
B) 11.00
C) 1.0  10–11
D) 3.0  10–14
E) 1.1  10–13
____ 34) What is the pOH of an aqueous solution at 25.0 °C in which [OH –] is 0.0010 M?
A) 11.00
B) –3.00
C) 3.00
D) –11.00
E) 6.91
6
Name: ________________________
ID: A
____ 35) Which solution will be the most basic?
A) 0.10 M Ba(OH)2
B) 0.10 M KOH
C) 0.10 M H2O
D) 0.10 M CH3OH
E) All solutions have equal basicity.
____ 36) What is the pH of a 0.020 M aqueous solution of barium hydroxide?
A) 12.60
B) 12.30
C) 1.70
D) 10.41
E) 1.40
____ 37) The Ka of hypochlorous acid (HClO) is 3.0  10–8 at 25.0 °C. Calculate the pH of a 0.0385 M hypochlorous acid
solution.
A) 3.05
B) 9.53
C) 4.47
D) 6.52
E) –3.05
____ 38) Calculate the pH of a 0.500 M aqueous solution of NH 3. The Kb of NH3 is 1.77  10–5.
A) 8.95
B) 11.47
C) 2.53
D) 11.77
E) 2.23
____ 39) Calculate the pOH of a 0.0727 M aqueous sodium cyanide solution at 25.0 °C. K b for CN– is 4.9  10–10.
A) 9.33
B) 10.00
C) 5.22
D) 1.14
E) 8.78
____ 40) Kb for NH3 is 1.8  10–5. What is the pH of a 0.40 M aqueous solution of NH 4Cl at 25.0 °C?
A) 2.57
B) 11.43
C) 9.18
D) 4.82
E) 11.23
____ 41) The Ka for formic acid (HCO2H) is 1.8  10–4. What is the pH of a 0.20 M aqueous solution of sodium formate
(NaHCO2)?
A) 11.64
B) 5.48
C) 3.39
D) 8.52
E) 4.26
7
Name: ________________________
ID: A
____ 42) Of the following, which is the weakest acid?
A) HPO3–
B) H3PO4
C) H2PO4–
D) HPO4–
E) The acid strength of all of the above is the same.
8
ID: A
Unit 16 Practice Test
Answer Section
MULTIPLE CHOICE
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OBJ:
B
PTS:
16.1; G2
E
PTS:
16.2; G2
C
PTS:
16.2; G2
C
PTS:
16.3; G2
B
PTS:
16.5; G2
A
PTS:
16.6, 16.7; G2
D
PTS:
16.6, 16.7; G2
A
PTS:
16.6, 16.7; G2
D
PTS:
16.5; G2
A
PTS:
16.5; G2
C
PTS:
16.8; G2
C
PTS:
16.8; G2
B
PTS:
16.8; G2
D
PTS:
16.9; G2
C
PTS:
16.9; G2
D
PTS:
16.9; G2
D
PTS:
16.1; G2
C
PTS:
16.2; G2
B
PTS:
16.2; G2
D
PTS:
16.2; G2
B
PTS:
16.4; G4
1
DIF: 1
REF: Page Ref: 16.1
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DIF: 1
REF: Page Ref: 16.2
1
DIF: 1
REF: Page Ref: 16.2
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DIF: 2
REF: Page Ref: 16.3
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DIF: 3
REF: Page Ref: 16.5
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DIF: 1
REF: Page Ref: 16.6
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DIF: 4
REF: Page Ref: 16.6
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REF: Page Ref: 16.6
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DIF: 3
REF: Page Ref: 16.7
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DIF: 2
REF: Page Ref: 16.7
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DIF: 3
REF: Page Ref: 16.8
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DIF: 3
REF: Page Ref: 16.8
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DIF: 3
REF: Page Ref: 16.8
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DIF: 3
REF: Page Ref: 16.9
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DIF: 3
REF: Page Ref: 16.9
1
DIF: 3
REF: Page Ref: 16.9
1
DIF: 3
REF: Page Ref: 16.10
1
DIF: 2
REF: Page Ref: 16.2
1
DIF: 2
REF: Page Ref: 16.2
1
DIF: 2
REF: Page Ref: 16.2
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DIF: 2
REF: Page Ref: 16.4
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ID: A
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OBJ:
A
PTS:
16.4; G4
E
PTS:
16.5; G4
A
PTS:
16.6, 16.7; G4
B
PTS:
16.6, 16.7; G4
E
PTS:
16.6, 16.7; G4
B
PTS:
16.6, 16.7; G4
D
PTS:
16.6, 16.7; G4
B
PTS:
16.6, 16.7; G4
D
PTS:
16.6, 16.7; G4
C
PTS:
16.9; G4
A
PTS:
16.2; G2
A
PTS:
16.4; G4
C
PTS:
16.4; G4
A
PTS:
16.5; G2
A
PTS:
16.5; G4
C
PTS:
16.6, 16.7; G4
B
PTS:
16.6, 16.7; G4
C
PTS:
16.9; G4
D
PTS:
16.9; G4
D
PTS:
16.9; G4
A
PTS:
16.1; G2
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REF: Page Ref: 16.4
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REF: Page Ref: 16.5
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REF: Page Ref: 16.6
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REF: Page Ref: 16.7
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REF: Page Ref: 16.7
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REF: Page Ref: 16.9
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REF: Page Ref: 16.2
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REF: Page Ref: 16.4
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REF: Page Ref: 16.4
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REF: Page Ref: 16.5
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REF: Page Ref: 16.6
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REF: Page Ref: 16.7
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REF: Page Ref: 16.9
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REF: Page Ref: 16.9
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REF: Page Ref: 16.10
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Unit 16 Practice Test [Answer Strip]
D
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7)
C 12)
_____
ID: A
D 16)
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A 22)
_____
B
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1)
E 23)
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A
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8)
D 17)
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E
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2)
A 24)
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B 13)
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C 18)
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D
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9)
C
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3)
B 25)
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B 19)
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A 10)
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C
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4)
D 14)
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D 20)
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B
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5)
E 26)
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C 11)
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C 15)
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B 21)
_____
A
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6)
B 27)
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Unit 16 Practice Test [Answer Strip]
D 28)
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A 35)
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B 29)
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A 36)
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D 30)
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C 37)
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C 31)
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A 32)
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A 33)
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C 34)
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B 38)
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C 39)
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D 40)
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D 41)
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A 42)
_____
ID: A