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Acid Base Chemistry

Arrhenius Base Hydroxide ion producer
Arrhenius Acid Hydrogen ion producer
Lewis Acid electron acceptor
Lewis Base electron donor
Bronsted Lowery Acid H+ donor
Bronsted Lowery Base H+ acceptor
Strong acid or base equilibrium lies far to the right (completely dissociates)
Weak acid or base equilibrium lies far to the left (mostly stays intact)
pH of an acid 0-6.9
pH of a base 7.1-14
neutral pH 7
carboxylic acids are typically (strong or weak) weak
H+ concentration of a strong acid [H+]=[HA]
increase of H+ causes pH to decrease
Ka of a strong acid is (large or small) large
Ka of a weak acid is (large or small) small
amphoteric a substance that can be an acid or a base
Kw the dissociation constant for water
value of Kw for pure water at 25oC 1.0 x 10^-14
Created by: shudonmiller



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