1. Acids
Bases&
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2. Definitions
• Acids – produce H+
• Bases - produce OH-
• Acids – donate H+
• Bases – accept H+
• Acids – accept e-
pair
• Bases – donate e-
pair
Arrhenius
Bronsted-Lowry
Lewis
only in water
any solvent
used in organic chemistry,
wider range of substances
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3. Examples
Arrhenius
Bronsted-Lowry
Lewis
HCl NaOH
HCl NH3
:NH3BF3
HCN
The hydrogen ion in aqueous solution
H+
+ H2O  H3O+
(hydronium ion)
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4. The Bronsted-Lowry Concept
Conjugate pairs
HCl Cl- CH3COOH CH3COO-
NH4
+
NH3 HNO3 NO3-
How does a conjugate pair differ?
H+
transfer
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5. H2O  H+
+ OH-
Does pure water conduct electrical current?
(H+
)(OH-
) = 10-14
For pure water: (H+
) = (OH-
) = 10-7
M
This is neutrality and
at 25o
C is a pH = 7.
Water is a very, very, very weak electrolyte.
How are (H+
) and (OH-
) related?
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6. Strong and Weak Acids/Bases
Strong acids/bases – 100% dissociation into ions
HCl NaOH
HNO3 KOH
H2SO4
Weak acids/bases – partial dissociation,
both ions and molecules
CH3COOH NH3
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7. What is acid rain?
CO2 (g) + H2O  H2CO3  H+
+ HCO3
-
Dissolved carbon dioxide lowers the pH
Atmospheric pollutants from combustion
NO, NO2 + H2O …  HNO3
SO2, SO3 + H2O …  H2SO4
both
strong
acids
pH < 5.3
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8. General properties
ACIDS
• Taste sour
• Turn litmus
• React with active
metals – Fe, Zn
• React with bases
BASES
• Taste bitter
• Turn litmus
• Feel soapy or
slippery (react with
fats to make soap)
• React with acids
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9. pH Table
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