Acids and Bases
Nov 15, 2014
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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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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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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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H2O H+ + OH-
Does pure water conduct electrical current?
(H+)(OH-) = 10-14
For pure water: (H+) = (OH-) = 10-7M
This is neutrality and at 25oC is a pH = 7.
Water is a very, very, very weak electrolyte.
How are (H+) and (OH-) related?
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Strong and Weak Acids/Bases
Strong acids/bases – 100% dissociation into ions
HCl NaOHHNO3 KOHH2SO4
Weak acids/bases – partial dissociation, both ions and molecules
CH3COOH NH3
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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
bothstrong acids
pH < 5.3© iTutor. 2000-2013. All Rights Reserved
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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pH Table
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