acids and bases · 2019. 9. 22. · acids and bases brønstedacids and bases (16.1) the acid-base...
TRANSCRIPT
![Page 1: Acids and Bases · 2019. 9. 22. · Acids and Bases BrønstedAcids and Bases (16.1) The Acid-Base Properties of Water ( 16.2) pH –A Measure of Acidity (16.3) Strength of Acids and](https://reader033.vdocuments.us/reader033/viewer/2022053119/60a037c60e53904c69481282/html5/thumbnails/1.jpg)
Acids and Bases
![Page 2: Acids and Bases · 2019. 9. 22. · Acids and Bases BrønstedAcids and Bases (16.1) The Acid-Base Properties of Water ( 16.2) pH –A Measure of Acidity (16.3) Strength of Acids and](https://reader033.vdocuments.us/reader033/viewer/2022053119/60a037c60e53904c69481282/html5/thumbnails/2.jpg)
Acids and Bases Brønsted Acids and Bases (16.1) The Acid-Base Properties of Water (16.2) pH – A Measure of Acidity (16.3) Strength of Acids and Bases (16.4) Weak Acids and Acid Ionization Constants (16.5) Weak Bases and Base Ionization Constants (16.6) The Relationship Between Conjugate Acid-Base
Ionization Constants (16.7) Molecular Structure and the Strength of Acids
(16.8) Acid-Base Properties of Salts (16.9) Acidic, Basic, and Amphoteric Oxides (16.10) Lewis Acids and Bases (16.11)
![Page 3: Acids and Bases · 2019. 9. 22. · Acids and Bases BrønstedAcids and Bases (16.1) The Acid-Base Properties of Water ( 16.2) pH –A Measure of Acidity (16.3) Strength of Acids and](https://reader033.vdocuments.us/reader033/viewer/2022053119/60a037c60e53904c69481282/html5/thumbnails/3.jpg)
General Chemistry I – Concepts Representations of matter (1.3-1.4) Formula calculations and stoichiometry (3.6-
3.9) Strong and weak acids and bases, molar
concentrations of solutions and solution stoichiometry (4.4-4.6)
Periodicity of the elements and descriptive chemistry (8.6)
Lewis dot structures and electronegativities(9.4 and 9.5)
Molecular shape and polarity (10.1 and 10.2)
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16.1 Brønsted Acids and Bases
What is an acid?◦ Review: Arrhenius acids◦ Review: Brønsted acids
Review: Which definition is more encompassing?
Review: What are weak versus strong acids and bases?
![Page 5: Acids and Bases · 2019. 9. 22. · Acids and Bases BrønstedAcids and Bases (16.1) The Acid-Base Properties of Water ( 16.2) pH –A Measure of Acidity (16.3) Strength of Acids and](https://reader033.vdocuments.us/reader033/viewer/2022053119/60a037c60e53904c69481282/html5/thumbnails/5.jpg)
16.1 Brønsted Acids and Bases
What is a base?◦ Review: Arrhenius bases◦ Review: Brønsted bases
Review: Which definition is more encompassing?
Review: What are weak versus strong acids and bases?
![Page 6: Acids and Bases · 2019. 9. 22. · Acids and Bases BrønstedAcids and Bases (16.1) The Acid-Base Properties of Water ( 16.2) pH –A Measure of Acidity (16.3) Strength of Acids and](https://reader033.vdocuments.us/reader033/viewer/2022053119/60a037c60e53904c69481282/html5/thumbnails/6.jpg)
16.1 Brønsted Acids and Bases
What is a conjugate acid/base pair?
Review: What is a better way to describe the
hydrogen ion in water? H+ or H3O+
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16.1 Brønsted Acids and Bases Describe the reaction in water of HF
forming H+ versus H3O+.
2HF aq H O l
HF aq
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16.1 Brønsted Acids and Bases
What is a conjugate acid/base pair?
Practice: What is the conjugate acid of ammonia? What is the conjugate base of acetic acid?
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16.2 The Acid-Base Properties of Water
What is the conjugate acid of water? What is the conjugate base of water? What the definition of amphoteric? How is this equilibrium represented
symbolically?
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16.2 The Acid-Base Properties of Water
2 2 3H O l H O l H O aq OH aq
2H O l H aq OH aq
Explain how water is amphoteric.
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16.2 The Acid-Base Properties of Water
How is this equilibrium represented in an equilibrium expression?
What is the value of the equilibrium constant (at 25oC)?
What does this tell us about the concentration of the:◦ Hydrogen ion◦ Hydroxide ion
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16.2 The Acid-Base Properties of Water Ion-product constant (of water), Kw:◦ The product of the molar concentrations of H+ and
OH- ions at a particular temperature What is the equilibrium expression and what is
true when the solution is neutral? What does this tell us about the concentration of
the:◦ Hydrogen ion In acidic solution In basic solution
◦ Hydroxide ion In acidic solution In basic solution
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16.2 The Acid-Base Properties of Water
Ion-product constant (of water), Kw
Solution [H+] [OH-]Acidic, basic or neutral
1 10-7 M2 10-5 M3 10-9 M
2H O l H aq OH aq
o 1425 1.0 10wK C H OH
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16.2 The Acid-Base Properties of Water
Ion-product constant (of water), Kw
Solution [H+] [OH-]Acidic, basic or neutral
1 10-7 M 10-7 M neutral2 10-5 M3 10-9 M
2H O l H aq OH aq
o 1425 1.0 10wK C H OH
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16.2 The Acid-Base Properties of Water
Ion-product constant (of water), Kw
Solution [H+] [OH-]Acidic, basic or neutral
1 10-7 M 10-7 M neutral2 10-5 M 10-9 M acidic3 10-9 M
2H O l H aq OH aq
o 1425 1.0 10wK C H OH
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16.2 The Acid-Base Properties of Water
Ion-product constant (of water), Kw
Solution [H+] [OH-]Acidic, basic or neutral
1 10-7 M 10-7 M neutral2 10-5 M 10-9 M acidic3 10-9 M 10-5 M basic
2H O l H aq OH aq
o 1425 1.0 10wK C H OH
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16.2 The Acid-Base Properties of Water
What is present in an acidic solution? What is present in a basic solution?
Solution [H+] [OH-]Acidic, basic or neutral
1 10-7 M 10-7 M neutral2 10-5 M 10-9 M acidic3 10-9 M 10-5 M basic
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16.2 The Acid-Base Properties of Water
Acidic solution
Solution [HCl] [H+] [OH-] Strength?1 0.01 M2 0.001 M3 0.0001 M
2 3HCl aq H O l H O aq Cl aq
HCl aq H aq Cl aq
o14
2 , 251.0 10
w CH O l H aq OH aq K
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HCl aq H aq Cl aq
Concentration of HCl and H+ in solutionC
once
ntra
tion
/ M
0.01 M HCl (aq)In solution: 0.01 M H+
and 0.01 M Cl-
H+ / Cl-
HCl
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16.2 The Acid-Base Properties of Water
Acidic solution
Solution [HCl]0 [H+] [OH-] Strength?1 0.01 M 0.01 M2 0.001 M3 0.0001 M
2 3HCl aq H O l H O aq Cl aq
HCl aq H aq Cl aq
o14
2 , 251.0 10
w CH O l H aq OH aq K
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16.2 The Acid-Base Properties of Water
Acidic solution
Solution [HCl]0 [H+] [OH-] Strength?1 0.01 M 0.01 M2 0.001 M 0.001 M3 0.0001 M 0.0001 M
2 3HCl aq H O l H O aq Cl aq
HCl aq H aq Cl aq
o14
2 , 251.0 10
w CH O l H aq OH aq K
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16.2 The Acid-Base Properties of Water
Acidic solution
Solution [HCl]0 [H+] [OH-] Strength?1 0.01 M 0.01 M 10-12 M strongest2 0.001 M 0.001 M 10-11 M3 0.0001 M 0.0001 M 10-10 M weakest
2 3HCl aq H O l H O aq Cl aq
HCl aq H aq Cl aq
o14
2 , 251.0 10
w CH O l H aq OH aq K
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16.2 The Acid-Base Properties of Water
Basic solution
Solution [NaOH]0 [OH-] [H+] Strength?1 0.01 M2 0.001 M3 0.0001 M
NaOH aq Na aq OH aq
o14
2 , 251.0 10
w CH O l H aq OH aq K
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NaOH aq Na aq OH aq
Concentration of NaOH and OH- in solutionC
once
ntra
tion
/ M
0.01 M NaOH (aq)In solution: 0.01 M Na+
and 0.01 M OH-
Na+ / OH-
NaOH
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16.2 The Acid-Base Properties of Water
Basic solution
Solution [NaOH]0 [OH-] [H+] Strength?1 0.01 M 0.01 M2 0.001 M 0.001 M3 0.0001 M 0.0001 M
NaOH aq Na aq OH aq
o14
2 , 251.0 10
w CH O l H aq OH aq K
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16.2 The Acid-Base Properties of Water
Basic solution
Solution [NaOH]0 [OH-] [H+] Strength?1 0.01 M 0.01 M 10-12 M strongest2 0.001 M 0.001 M 10-11 M3 0.0001 M 0.0001 M 10-10 M weakest
NaOH aq Na aq OH aq
o14
2 , 251.0 10
w CH O l H aq OH aq K
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16.2 The Acid-Base Properties of Water
What is the trend of ◦ acid strength (acidity) and the concentration
of the hydrogen ion?◦ basic strength (basicity) and the concentration
of the hydroxide ion?◦ basic strength (basicity) and the concentration
of the hydrogen ion?
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16.3 pH – A Measure of Acidity
Acid strength and [H+]
0
0.002
0.004
0.006
0.008
0.01
Con
cent
rati
on /
M
Acidity
Acid strength decreasing
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0
0.002
0.004
0.006
0.008
0.01
Con
cent
rati
on /
M
Acidity
16.3 pH – A Measure of Acidity
Acid strength and [OH-]
Acid strength decreasing
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16.3 pH – A Measure of Acidity
Basic strength and [OH-]
0
0.002
0.004
0.006
0.008
0.01
Con
cent
rati
on /
M
Basicity
Basic strength decreasing
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0
0.002
0.004
0.006
0.008
0.01
Con
cent
rati
on /
M
Basicity
16.3 pH – A Measure of Acidity
Basic strength and [H+]
Basic strength decreasing
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16.3 pH – A Measure of Acidity
Acid strength and [H+]
0
0.002
0.004
0.006
0.008
0.01
Con
cent
rati
on /
M
Acidity
Acid strength decreasing
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16.3 pH – A Measure of Acidity
What if we plotted this on a log scale instead? First consider the data for an acidic solution[H+] log [H+] -log[H+] [OH-] Acidity
0.01 M0.001 M0.0001 M
10-5 M10-6 M
10-7 M
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16.3 pH – A Measure of Acidity
What if we plotted this on a log scale instead? First consider the data for an acidic solution[H+] log [H+] -log[H+] [OH-] Acidity
0.01 M Strong0.001 M0.0001 M
10-5 M10-6 M Weak
10-7 M neutral
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16.3 pH – A Measure of Acidity
What if we plotted this on a log scale instead? First consider the data for an acidic solution[H+] log [H+] -log[H+] [OH-] Acidity
0.01 M 10-12 M Strong0.001 M 10-11 M0.0001 M 10-10 M
10-5 M 10-9 M10-6 M 10-8 M Weak
10-7 M 10-7 M neutral
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16.3 pH – A Measure of Acidity
What if we plotted this on a log scale instead? First consider the data for an acidic solution[H+] log [H+] -log[H+] [OH-] Acidity
0.01 M -2 10-12 M Strong0.001 M -3 10-11 M0.0001 M -4 10-10 M
10-5 M -5 10-9 M10-6 M -6 10-8 M Weak
10-7 M -7 10-7 M neutral
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16.3 pH – A Measure of Acidity
What if we plotted this on a log scale instead? First consider the data for an acidic solution[H+] log [H+] -log[H+] [OH-] Acidity
0.01 M -2 2 10-12 M Strong0.001 M -3 3 10-11 M0.0001 M -4 4 10-10 M
10-5 M -5 5 10-9 M10-6 M -6 6 10-8 M Weak
10-7 M -7 7 10-7 M neutral
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16.3 pH – A Measure of Acidity
What if we plotted this on a log scale instead?
0.0
2.0
4.0
6.0
8.0
10.0
12.0
14.0
-log
[H+]
Acidity
Acid strength decreasing
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16.3 pH – A Measure of Acidity
What if we plotted this on a log scale instead? First consider the data for a basic solution
[OH-] [H+] log[H+] -log[H+] Basicity0.01 M0.001 M0.0001 M
10-5 M10-6 M
10-7 M
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16.3 pH – A Measure of Acidity
What if we plotted this on a log scale instead? First consider the data for a basic solution
[OH-] [H+] log[H+] -log[H+] Basicity0.01 M Strong0.001 M0.0001 M
10-5 M10-6 M Weak
10-7 M neutral
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16.3 pH – A Measure of Acidity
What if we plotted this on a log scale instead? First consider the data for a basic solution
[OH-] [H+] log[H+] -log[H+] Basicity0.01 M 10-12 M Strong0.001 M 10-11 M0.0001 M 10-10 M
10-5 M 10-9 M10-6 M 10-8 M Weak
10-7 M 10-7 M neutral
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16.3 pH – A Measure of Acidity
What if we plotted this on a log scale instead? First consider the data for a basic solution
[OH-] [H+] log[H+] -log[H+] Basicity0.01 M 10-12 M -12 Strong0.001 M 10-11 M -110.0001 M 10-10 M -10
10-5 M 10-9 M -910-6 M 10-8 M -8 Weak
10-7 M 10-7 M -7 neutral
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16.3 pH – A Measure of Acidity
What if we plotted this on a log scale instead? First consider the data for a basic solution
[OH-] [H+] log[H+] -log[H+] Basicity0.01 M 10-12 M -12 12 Strong0.001 M 10-11 M -11 110.0001 M 10-10 M -10 10
10-5 M 10-9 M -9 910-6 M 10-8 M -8 8 Weak
10-7 M 10-7 M -7 7 neutral
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16.3 pH – A Measure of Acidity
What if we plotted this on a log scale instead?
0.0
2.0
4.0
6.0
8.0
10.0
12.0
14.0
log
[H+]
Basicity
Base strength increasing
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16.3 pH – A Measure of Acidity
What is pH◦ algorithmically?◦ as a measure of acid strength?
[H+] log [H+] -log[H+] [OH-] Acidity0.01 M -2 2 10-12 M Strong0.001 M -3 3 10-11 M0.0001 M -4 4 10-10 M
10-5 M -5 5 10-9 M10-6 M -6 6 10-8 M Weak
10-7 M -7 7 10-7 M neutral
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16.3 pH – A Measure of Acidity
pH and acid strength
0.0
2.0
4.0
6.0
8.0
10.0
12.0
14.0
pH
Acidity
Acid strength decreasing
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16.3 pH – A Measure of Acidity
What is pH◦ algorithmically?◦ as a measure of acid strength?
Type of solution
[H+] vs. [OH-] [H+] [OH-] pH
Acidic [H+] > [OH-] [H+] >10-7 M [OH-] <10-7 M pH < 7NeutralBasic
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16.3 pH – A Measure of Acidity
What is pOH◦ algorithmically?◦ as a measure of acid strength?
[H+] pH [OH-] pOH Acidity0.01 M 2 10-12 M Strong0.001 M 3 10-11 M0.0001 M 4 10-10 M
10-5 M 5 10-9 M10-6 M 6 10-8 M Weak
10-7 M 7 10-7 M neutral
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16.3 pH – A Measure of Acidity
What is pOH◦ algorithmically?◦ as a measure of acid strength?
[H+] pH [OH-] pOH Acidity0.01 M 2 10-12 M 12 Strong0.001 M 3 10-11 M 110.0001 M 4 10-10 M 10
10-5 M 5 10-9 M 910-6 M 6 10-8 M 8 Weak
10-7 M 7 10-7 M 7 neutral
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16.3 pH – A Measure of Acidity
What is pOH◦ algorithmically?◦ as a measure of acid strength?
How are pH and pOH related?
Type of solution
[H+] vs. [OH-] [OH-] pH pOH
AcidicNeutral [H+] = [OH-] [OH-] =10-7 M pH = 7 pOH = 7Basic
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16.3 pH – A Measure of Acidity
Practice:
What is the [H+] and pH of◦ 0.0015 M HNO3
◦ 0.0015 M Ba(OH)2
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16.4 Strength of Acids and Bases
Review: What is a strong acid?
Review: What species are present for HCl?
Review: What is a weak acid?
Review: What species are present for HF?
Figure 16.3 p. 555
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HCl aq H aq Cl aq
Concentration of HCl and H+ in solutionC
once
ntra
tion
/ M
0.01 M HCl (aq)In solution: 0.01 M H+
and 0.01 M Cl-
H+ / Cl-
HCl
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HF aq H aq F aq
Concentration of HF and H+ in solutionC
once
ntra
tion
/ M
0.01 M HF (aq)In solution: 0.00734 M HF
and 0.00266 M H+
HF
H+
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16.4 Strength of Acids and Bases
Review: What is a strong acid? Review: What is a weak acid? What is the conjugate base of the strong
acid, HCl?◦ What is the relative strength of the conjugate
base of HCl? What is the conjugate base of the weak
acid, HF?◦ What is the relative strength of the conjugate
base of HF?
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16.4 Strength of Acids and Bases
What is the general trend of relative strength of acid/base pairs?◦ Strong acids and their conjugate bases◦ Weak acids and their conjugate bases
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16.4 Strength of Acids and Bases
Table 16.2 p. 556
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16.4 Strength of Acids and Bases
What is the strongest acid that can exist in aqueous solution?
What is the strongest base that can exist in aqueous solution?
What does this mean for Table 16.2?
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16.4 Strength of Acids and Bases
Table 16.2 p. 556
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16.4 Strength of Acids and Bases
What is present in a solution of◦ HCl◦ HF◦ NaOH◦ NH3
What is the general trend of relative strength of acid/base pairs in terms of:◦ hydrogen ion concentration?◦ pH?
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16.5 Weak Acids and Acid Ionization Constants Review: What is the equilibrium
expression for the ionization of HF?
Review: What is the equilibrium expression for the ionization of any weak acid?
How does this equilibrium constant, Ka, tell us about acid strength?
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Table 16.3 p. 559
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16.5 Weak Acids and Acid Ionization Constants How does this equilibrium constant, Ka,
tell us about acid strength? Which solution will have a higher [H+]?◦ HF Ka = 7.1x10-4
◦ HNO2 Ka = 4.5x10-4
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16.5 Weak Acids and Acid Ionization Constants How does this equilibrium constant, Ka,
tell us about acid strength? Which solution will have a lower pH?◦ HF Ka = 7.1x10-4
◦ HNO2 Ka = 4.5x10-4
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16.5 Weak Acids and Acid Ionization Constants How does this equilibrium constant, Ka,
tell us about acid strength? What is the pH of 0.015 M:◦ HF Ka = 7.1x10-4
◦ HNO2 Ka = 4.5x10-4
When can you approximate and what is the 5% rule?
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16.5 Weak Acids and Acid Ionization Constants How does this equilibrium constant, Ka, tell
us about acid strength? Percent ionization:◦ The ratio of ionized acid concentration at
equilibrium over the initial concentration of the acid
How does this tell us about acid strength? Which solution would have a greater
percent ionization?◦ 0.015 M HF Ka = 7.1x10-4
◦ 0.015 M HNO2 Ka = 4.5x10-4
How does percent ionization tell us about acid strength?
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16.5 Weak Acids and Acid Ionization ConstantsHow do [H+], pH and percent ionization vary for the same acid but decreasing concentrations?
HF [H+] pH Percent ionization0.01 M
0.0015 M0.001 M
0.00015 M0.0001 M
0.000015 M
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16.5 Weak Acids and Acid Ionization ConstantsHow do [H+], pH and percent ionization vary for the same acid but decreasing concentrations?
HF [H+] pH Percent ionization0.01 M 0.0081 M
0.0015 M 0.0029 M0.001 M 0.0023 M
0.00015 M 0.00074 M0.0001 M 0.00056 M
0.000015 M 0.00013 M
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16.5 Weak Acids and Acid Ionization ConstantsHow do [H+], pH and percent ionization vary for the same acid but decreasing concentrations?
HF [H+] pH Percent ionization0.01 M 0.0081 M 2.09
0.0015 M 0.0029 M 2.530.001 M 0.0023 M 2.63
0.00015 M 0.00074 M 3.130.0001 M 0.00056 M 3.25
0.000015 M 0.00013 M 3.90
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16.5 Weak Acids and Acid Ionization ConstantsHow do [H+], pH and percent ionization vary for the same acid but decreasing concentrations?
HF [H+] pH Percent ionization0.01 M 0.0081 M 2.09 8.1%
0.0015 M 0.0029 M 2.53 19.5%0.001 M 0.0023 M 2.63 23.3%
0.00015 M 0.00074 M 3.13 49.1%0.0001 M 0.00056 M 3.25 55.9%
0.000015 M 0.00013 M 3.90 84.8%
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16.5 Weak Acids and Acid Ionization Constants What happens to percent ionization as
concentration decreases? Why is this only true for weak
acids/bases?
Figure 16.4 p. 565
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16.5 Weak Acids and Acid Ionization Constants What about acids with more than one
acidic hydrogen?◦ What species do these acids have in solution?◦ How do we write the equilibrium
expressions?◦ What would you predict about the relative
size of Ka1 versus Ka2 versus Ka3?
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Table 16.4 p. 563
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16.5 Weak Acids and Acid Ionization Constants Practice:
What is the concentration of all species at equilibrium of a 1.0 M phosphoric acid solution?
What is the order of the highest concentration to lowest concentration of all species in 1.0 L of solution?
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16.6 Weak Bases and Base Ionization Constants Review: What is a strong base? Review: What is a weak base? Review: How do we represent this
symbolically? Review: What species are present for
NaOH versus NH3?
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16.6 Weak Bases and Base Ionization Constants Review: What is the equilibrium
expression for the ionization of NH3?
Review: What is the equilibrium expression for the ionization of any weak base?
How does this equilibrium constant, Kb, tell us about base strength?
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Table 16.5 p. 570
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16.6 Weak Bases and Base Ionization Constants How does this equilibrium constant, Kb,
tell us about base strength? Which solution will have a higher [OH-]?◦ NH3 Kb = 1.8x10-5
◦ CH3NH2 Kb = 4.4x10-4
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16.6 Weak Bases and Base Ionization Constants How does this equilibrium constant, Kb,
tell us about base strength? Which solution will have a lower pOH?◦ NH3 Kb = 1.8x10-5
◦ CH3NH2 Kb = 4.4x10-4
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16.6 Weak Bases and Base Ionization Constants How does this equilibrium constant, Kb,
tell us about base strength? What is the pOH of 0.015 M:◦ NH3 Kb = 1.8x10-5
◦ CH3NH2 Kb = 4.4x10-4
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16.6 Weak Bases and Base Ionization Constants How does this equilibrium constant, Kb,
tell us about base strength? What is the pH of 0.015 M:◦ NH3 Kb = 1.8x10-5
◦ CH3NH2 Kb = 4.4x10-4
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16.5 Weak Acids and Acid Ionization Constants How does this equilibrium constant, Kb, tell
us about base strength? Percent ionization:◦ The ratio of ionized base concentration at
equilibrium over the initial concentration of the base
How does this tell us about base strength? Which solution would have a greater
percent ionization?◦ 0.015 M NH3 Kb = 1.8x10-5
◦ 0.015 M CH3NH2 Kb = 4.4x10-4
How does percent ionization tell us about base strength?
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16.7 The Relationship Between Conjugate Acid-Base Ionization Constants
Review: What is the conjugate base of HF?
What is the equilibrium expression for the reaction of HF in water?
What is the equilibrium expression for the reaction of F- in water?
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16.7 The Relationship Between Conjugate Acid-Base Ionization Constants
Review: What are the rules for multiple reactions and the equilibrium constants?
How is Ka related to Kb? What is the value of Kb of the fluoride
ion? What does Ka > Kb mean? What does Ka < Kb mean?
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16.7 The Relationship Between Conjugate Acid-Base Ionization Constants
Practice:
What is Kb for the acids listed below?◦ HNO2
◦ HCN
Which acid is the strongest? Which conjugate base is the strongest?
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Table 16.3 p. 559
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16.8 Molecular Structure and the Strength of Acids Review: What do we learn from a Lewis
dot structure? How does bond enthalpy and
electronegativity contribute to the strength of acid?
What about HCl versus HBr?Table 16.6 p. 573
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16.8 Molecular Structure and the Strength of Acids
How can we verify this trend with experimental data?
(Can the solvent for the system be water?)
What does the equilibrium constant and equilibrium concentrations of HCl versus HBr in acetic acid tell us about acid strength?
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16.8 Molecular Structure and the Strength of Acids
What are the Lewis dot structures of:◦ HNO2 versus HNO3
◦ HClO versus HClO2
What are the rules for oxoacid strength? Which structure has a higher oxidation
state of N? Review: What is formal charge? How the Lewis dot structures of the
acids above relate oxoacid strengths?
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16.9 Acid-Base Properties of Salts
Review: What is the conjugate base of HF?
Review: What is the conjugate acid of NH3?
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16.9 Acid-Base Properties of Salts
To work through these salts:◦ Consider first what happens when the salt
dissociates in water◦ Then consider the reaction of each ion with
water (are either a conjugate acid/base of a weak acid/base)◦ Then consider the production of the
hydroxide ion or hydrogen ion
What happens when NaCl is put in water?
What is the pH of this solution?
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16.9 Acid-Base Properties of Salts
To work through these salts:◦ Consider first what happens when the salt
dissociates in water◦ Then consider the reaction of each ion with
water (are either a conjugate acid/base of a weak acid/base)◦ Then consider the production of the
hydroxide ion or hydrogen ion
What happens when NaF is put in water? What is the pH of this solution?
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16.9 Acid-Base Properties of Salts
To work through these salts:◦ Consider first what happens when the salt
dissociates in water◦ Then consider the reaction of each ion with
water (are either a conjugate acid/base of a weak acid/base)◦ Then consider the production of the
hydroxide ion or hydrogen ion
What happens when NH4Cl is put in water?
What is the pH of this solution?
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16.9 Acid-Base Properties of Salts
To work through these salts:◦ Consider first what happens when the salt
dissociates in water◦ Then consider the reaction of each ion with
water (are either a conjugate acid/base of a weak acid/base)◦ Then consider the production of the
hydroxide ion or hydrogen ion
What happens when AlCl3 is put in water?
What is the pH of this solution?
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16.9 Acid-Base Properties of Salts
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16.9 Acid-Base Properties of Salts
To work through these salts:◦ Consider first what happens when the salt
dissociates in water◦ Then consider the reaction of each ion with
water (are either a conjugate acid/base of a weak acid/base)◦ Then consider the production of the
hydroxide ion or hydrogen ion
What happens when NH4F is put in water?
What is the pH of this solution?
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16.9 Acid-Base Properties of Salts
Table 16.7 p. 580
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16.10 Acidic, Basic and Amphoteric Oxides
What are oxides? What is the oxide of sodium? What is the reaction of sodium oxide in
water?◦ What is the pH of this solution?
What is the general rule of metal oxides?
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16.10 Acidic, Basic and Amphoteric Oxides
What are oxides? What is the reaction of dinitrogen
pentoxide in water?◦ What is the pH of this solution?
What is the general rule of nonmetal oxides?
What are amphoteric oxides? What group of elements would you
expect to be amphoteric oxides?
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16.10 Acidic, Basic and Amphoteric Oxides
Figure 16.8 p. 582
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16.10 Acidic, Basic and Amphoteric Oxides
What type of element forms basic oxides? What type of element forms acidic
oxides? What type of element forms amphoteric
oxides?
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16.11 Lewis Acids and Bases What is an acid?◦ Review: Arrhenius acids◦ Review: Brønsted acids◦ Lewis acids A substance that can accept a pair of electrons
What is a base?◦ Review: Arrhenius bases◦ Review: Brønsted bases◦ Lewis bases A substance that can donate a pair of electrons
Which definition is the most encompassing?
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16.11 Lewis Acids and Bases
How do Lewis dot structure assist in assigning the Lewis acid or Lewis base in a reaction?
Practice: Carbon dioxide reacts with water. What
is the Lewis acid and Lewis base in this reaction?
Can the ammonium ion be a Lewis base?