Chapter 14: Acids and Bases

Flashcards covering key vocabulary and definitions related to acids and bases, including Arrhenius, Bronsted-Lowry, and Lewis definitions, acid strength, and acid-base reactions.

Arrhenius acid

A chemical compound that increases the concentration of hydrogen ions, H+, in aqueous solution.

Arrhenius base

A substance that increases the concentration of hydroxide ions, OH−, in aqueous solution.

Binary acid

An acid that contains only two different elements: hydrogen and one of the more electronegative elements.

Binary Acid Nomenclature

Begins with the prefix hydro- followed by the root of the name of the second element and ends with the suffix -ic.

Oxyacid

An acid that is a compound of hydrogen, oxygen, and a third element, usually a nonmetal.

Brønsted-Lowry acid

A molecule or ion that is a proton donor.

Brønsted-Lowry base

A molecule or ion that is a proton acceptor.

Monoprotic acid

An acid that can donate only one proton (hydrogen ion) per molecule.

Polyprotic acid

An acid that can donate more than one proton per molecule.

Diprotic acid

The type of polyprotic acid that can donate two protons per molecule

Triprotic acid

The type of polyprotic acid that can donate three protons per molecule.

Lewis acid

An atom, ion, or molecule that accepts an electron pair to form a covalent bond.

Conjugate base

The species that remains after a Brønsted- Lowry acid has given up a proton.

Amphoteric

Any species that can react as either an acid or a base.

Salt

Ionic compound composed of a cation from a base and an anion from an acid.

Acid rain

Very acidic rain.

Strong acid

A chemical that ionizes completely in aqueous solution

Weak acid

Releases few hydrogen ions in aqueous solution