Looks like no one added any tags here yet for you.
Hydronium Ion
H3O+ formed when H+ from an acid combines with water
Conjugate Acid
Formed when a base gains a hydrogen ion
Conjugate Base
Remains after an acid donates a hydrogen ion
Lewis Acid
Accepts a pair of electrons to form a covalent bond
Lewis Base
Donates a pair of electrons to form a covalent bond
Neutral Solution
Aqueous solution with equal hydronium and hydroxide concentrations
Ion-Product Constant
Product of hydronium and hydroxide concentrations
Strong Acid
Completely dissociates to form hydronium ions
Strong Base
Fully dissociates to form hydroxide ions
Weak Acid
Partially ionizes to produce hydronium ions
Weak Base
Produces minimal hydroxide ions when reacting with water
Neutralization Reaction
Acid and base react to form salt and water
Titration
Adding known concentration to unknown to determine concentration
Equivalence Point
Hydronium and hydroxide ions are equal in moles
Titration Curve
Graph of pH vs. volume of standard solution added
Buffer
Maintains constant pH when acid/base added
Buffer Capacity
Amount of acid/base before significant pH change
Buffer Range
pH range where buffer system maintains constant pH
Arrhenius Acid
Dissociates into H+ ions (H3O+), e.g., HCl
Arrhenius Base
Dissociates into OH-, e.g., NaOH
Lewis Acid
Accepts electron pairs, e.g., BF3
Lewis Base
Donates electron pairs, e.g., F-
Bronsted-Lowry Acid
Donates H+, e.g., HCl
Bronsted-Lowry Base
Accepts H+, e.g., NH3
pH
Measure of acidity, 7 is neutral
pOH
Measure of basicity, 7 is neutral