chapter 16 acid-base equilibria
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Chapter 16 Acid-Base Equilibria. Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten. Troy Wood University of Buffalo Buffalo, NY 2006, Prentice Hall. Is NH 3 an acid, base, or could it be both?. Acid Base Both. Correct Answer:. - PowerPoint PPT PresentationTRANSCRIPT
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Chemistry, The Central Science, 10th edition
Theodore L. Brown; H. Eugene LeMay, Jr.;and Bruce E. Bursten
Chapter 16Acid-Base Equilibria
Troy WoodUniversity of BuffaloBuffalo, NY 2006, Prentice Hall
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Is NH3 an acid, base, or could it be both?
1. Acid
2. Base
3. Both
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Correct Answer:
In this chapter we learned that a more general definition for a base is a substance that can accept another proton, which is true for NH3 because of the lone electron pair on the N atom.
1. Acid
2. Base
3. Both
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Is H2O an acid, base, or could it be both?
1. Acid
2. Base
3. Both
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Correct Answer:
As indicated in the equilibrium below, water is an amphoteric substance that can either accept another proton or donate a proton.
OHH
H OHH
OHH+ H+
+
_
1. Acid
2. Base
3. Both
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Is the ion PO43 an acid, base, or could it
be both?
-P
O
-O
O-
O- P
O-
-O
O-
O+
1. Acid
2. Base
3. Both
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Correct Answer:
Phosphate is a proton acceptor, regardless of which resonance structure is being considered.
1. Acid
2. Base
3. Both
-P
O
-O
O-
O- P
O-
-O
O-
O+
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What is the approximate pH of an aqueous solution of 1 1012 M HCl?
1. 22. 7 3. 124. 145. None of the above
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Correct Answer:
This is an aqueous solution, therefore water will autoionize. The concentration of protons due to autoionization of water will dominate that of such a dilute strong acid.
1. 22. 7 3. 124. 145. None of the above
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What is [H+] in an aqueous solution whose pH = 3.72?
1. 1.9 103 M2. 5.1 103 M3. 1.9 104 M4. 5.1 104 M5. 5.1 1010 M
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Correct Answer:
3.72 = log[H+]
3.72 = log[H+]
[H+] = 1.9 10 4 M
1. 1.9 103 M2. 5.1 103 M3. 1.9 104 M4. 5.1 104 M5. 5.1 1010 M
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What is the pH of an aqueous solution of [OH] = 6.0 103 M?
1. 2.222. 3.223. 7.004. 10.785. 11.78
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Correct Answer:
There is more than one method to solve this problem. One is presented below:
pOH = log(6.0 103)
= 2.22
pH = 14.00 pOH
= 14.00 2.22
= 11.78
1. 2.222. 3.223. 7.004. 10.785. 11.78
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The [H+] in an 0.020 M solution of HNO2 is 3.0 103 M. What is the Ka of HNO2?
1. 4.5 104
2. 6.0 105
3. 9.0 106
4. 1.5 101 5. None of the
above
N
OHO
nitrous acid
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Correct Answer:
[HA]
]][A[H
aK
0.020
109.0
0.020
]10[3.0 623
aK
4104.5 aK
1. 4.5 104
• 6.0 105
• 9.0 106
• 1.5 101 • None of the
above
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The pH of a 0.050 M weak acid is 3.00. What is the percentage ionization?
1. 0.10%2. 0.20% 3. 1.0%4. 2.0%5. 3.0%
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Correct Answer:
100%[HA]
][Hionization %
eq
o
100%[0.050]
]10[1.0ionization %
-3
2.0%ionization %
Since pH = 3.00,
[H+] = 1.0 103 M, so 1. 0.10%2. 0.20% 3. 1.0%4. 2.0%5. 3.0%
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For a certain weak acid, Ka = 2.0 105. What is Kb for its conjugate base?
1. 4.5 103
2. 5.0 103
3. 1.0 109
4. 4.0 1010
5. 5.0 1010
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Correct Answer:
wba KKK
a
wb K
KK
10
5-
-14
105.0102.0
101.0
bK
1. 4.5 103
2. 5.0 103
3. 1.0 109
4. 4.0 1010
5. 5.0 1010
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Which of the following oxyacid species is the strongest acid?
1. HClO2. HClO2
3. HClO3
4. HClO4
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Correct Answer:
For oxyacids that have the same central atom Y, acid strength increases as the number of O atoms bound to Y increases.
Thus, HClO4 is the strongest acid of this series.
1. HClO2. HClO2
3. HClO3
4. HClO4