ch.16. acids and bases (the fundamentals)
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Ch.16. Acids and Bases (the fundamentals). Contents. 16-1 The Arrhenius Theory: A Brief Review 16-2 Br ønsted-Lowry Theory of Acids and Bases 16-3 The Self-Ionization of Water and the pH Scale 16-4 Strong Acids and Strong Bases 16-5 Weak Acids and Weak Bases 16-6 Polyprotic Acids - PowerPoint PPT PresentationTRANSCRIPT
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Ch.16. Acids and Bases (the fundamentals)
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Contents16-1 The Arrhenius Theory: A Brief Review
16-2 Brønsted-Lowry Theory of Acids and Bases
16-3 The Self-Ionization of Water and the pH Scale
16-4 Strong Acids and Strong Bases
16-5 Weak Acids and Weak Bases
16-6 Polyprotic Acids
16-7 Ions as Acids and Bases
16-8 Molecular Structure Acid-Base Behavior
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16-1 The Arrhenius Theory: A Brief Review
HCl(g) → H+(aq) + Cl-(aq)
NaOH(s) → Na+(aq) + OH-(aq)H2O
H2O
Na+(aq) + OH-(aq) + H+(aq) + Cl-(aq) → H2O(l) + Na+(aq) + Cl-(aq)
H+(aq) + OH-(aq) → H2O(l)
Arrhenius theory did not handle non OH- bases such as ammonia very well.
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16-2 Brønsted-Lowry Theory of Acids and Bases
An acid is a proton donor. A base is a proton acceptor.
NH3 + H2O NH4+ + OH-
NH4+ + OH- NH3 + H2O
base acid
baseacid
conjugate acid
conjugate base
?? ??
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The Solvated Proton
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Base Ionization Constant
NH3 + H2O NH4+ + OH-
Kc= [NH3][H2O]
[NH4+][OH-]
Kb= Kc[H2O] = [NH3]
[NH4+][OH-]
= 1.810-5
base acidconjugate
acid
conjugate
base
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Acid Ionization Constant
CH3CO2H + H2O CH3CO2- + H3O+
Kc= [CH3CO2H][H2O]
[CH3CO2-][H3O+]
Ka= Kc[H2O] = = 1.810-5
[CH3CO2H]
[CH3CO2-][H3O+]
baseacidconjugate
acid
conjugate
base
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A Weak Base
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A Weak Acid
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A Strong Acid
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Worked Examples Follow:
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CRS Questions Follow:
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O HNH
H
H HN H
H
O H
- -
3NH 2H OOH 2NH + +
In the reaction depicted below, which species are acids?
3 21. NH , H O 3 22. NH , NH 23. OH , NH
24. OH , H O35. NH , OH
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O HNH
H
H HN H
H
O H
- -
3NH 2H OOH 2NH + +
In the reaction depicted below, which species are acids?
3 21. NH , H O 3 22. NH , NH 23. OH , NH
24. OH , H O35. NH , OH