Acids and Bases (unfinished)
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23 Terms
Arrhenius Acid
Increases H+ in water
Arrhenius Base
Increases OH- in water
Bronsted-Lowry Acid
H+ donor
Bronsted-Lowry Base
H+ acceptor
Lewis Acid
Electron pair acceptor
Lewis Base
Electron pair donor
Conjugate Acid
When a base gains H+
Conjugate Base
When an acid loses H+
Amphoteric
Can either donate or accept a proton
Acidic
[H3O+] > [OH-] (pH scale 1-6)
Neutral
[H3O+] = [OH-] (pH scale 7)
Basic
[H3O+] < [OH-] (pH scale 8-14)
Lower pH
More H3O+
Higher pH
Less H3O+
Log scale of pH
Factor of 10 ex. pH 1 to 3 = 100 change in hydronium concentration
Concentration
How much acid/base is present?
Strength
How completely does it react with water?
Strong Acids
Ionizes completely when added to water creating high concentration of [H3O+].
Strong Bases
Ionizes completely when added to water creating high concentration of [OH-].
Weak Acids
Partial ionization with water creating weak concentration of [H3O+].
Weak Bases
Partial ionization with water creating weak concentration of [OH-].
Weak Acid Equilibrium