Chapter 9 Acids, Bases, and Salts

Practice flashcards covering key vocabulary and concepts from Chapter 9 on Acids, Bases, and Salts.

Brønsted Acid

Any hydrogen-containing substance capable of donating a proton (H+) to another substance.

Brønsted Base

Any substance capable of accepting a proton (H+) from another substance.

Self-Ionization of Water

The process in which pure water dissociates into equal amounts of H3O+ and OH− ions.

Neutral Solution

A solution where the concentrations of H3O+ and OH− are equal.

pH Concept

A measure of the acidity or basicity of a solution; defined as the negative logarithm of the molar concentration of H+ (H3O+).

Weak Acid

An acid that partially dissociates into its ions in solution.

Strong Acid

An acid that completely dissociates in solution.

Acid Dissociation Constant (Ka)

The equilibrium constant for the dissociation of an acid, describing the extent of dissociation.

Titration

An analytical procedure in which a solution of known concentration is added to a measured volume of an unknown solution.

Conjugate Acid

The species formed when a Brønsted base accepts a proton (H+).

Conjugate Base

The species remaining when a Brønsted acid donates a proton (H+).

Buffer Capacity

The amount of acid or base a buffer can absorb without a significant change in pH.

Monoprotic Acid

An acid that donates only one proton (H+) per molecule in solution.

Diprotic Acid

An acid that donates two protons (H+) per molecule in solution.

Triprotic Acid

An acid that donates three protons (H+) per molecule in solution.

Equivalence Point

The point in a titration where the amount of titrant added is stoichiometrically equivalent to the amount of substance being titrated.