Acid-Base Reactions

BRØNSTED-LOWRY ACID

A substance that acts as a proton (H+) donor in an acid-base reaction

BRØNSTED-LOWRY BASE

A substance that acts as a proton (H+) acceptor in an acid-base reaction

ACID-BASE REACTION

A reaction defined by the transfer of a proton (H+) from an acid to a base

CONJUGATE ACID

The species that is formed when a Brønsted-Lowry Base accepts a proton (H+)

CONJUGATE BASE

The species that is formed when a Brønsted-Lowry Acid donates a proton (H+)

CONJUGATE ACID-BASE PAIR

Two species in a reaction that are chemically related because they differ only by the presence of a single proton (H+)

STRONG ACID

An acid that completely ionizes (dissociates) in water (100% ionization), meaning it is a strong electrolyte

WEAK ACID

An acid that only partially ionizes (dissociates) in water, meaning it remains mostly in its molecular form in solution

STRONG BASE

A base that completely dissociates or ionizes in water, often an ionic hydroxide of a Group 1 or heavy Group 2 metal

WEAK BASE

A base that only partially accepts protons in water, meaning it remains mostly non-ionized

WEAKER CONJUGATE RULE

A stronger acid will always form a weaker conjugate base, and a stronger base will always form a weaker conjugate acid

REACTION FAVORABILITY

An acid-base reaction will always favor the formation of the weaker acid and weaker base (the side of the equilibrium where the weaker pair resides)

AMPHOTERIC SUBSTANCE

A substance (like water, H2O) that is capable of acting as either a proton donor (acid) or a proton acceptor (base) depending on the chemical environment

HYDRONIUM ION (H3O+)

The ion formed when a water molecule accepts a proton (H+); it is the form in which H+ exists in aqueous solution