Chemistry Vocabulary and Concepts

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