Buffers and Titrations: Acid-Base Equilibria

These flashcards cover key terms and concepts related to buffers and titrations, focusing on acid-base equilibria.

Buffer

A solution that contains a weak acid and its conjugate base salt, or a weak base and its conjugate acid salt.

Common Ion Effect

The phenomenon where the addition of an ion common to a solution causes a shift in the equilibrium.

Henderson-Hasselbalch Equation

pH = pKa + log([base]/[acid]), used to calculate the pH of buffer solutions.

ICE Table

A tool used to track the Initial, Change, and Equilibrium concentrations in a reaction.

Buffer Capacity

The ability of a buffer solution to resist changes in pH upon the addition of acids or bases.

Weak Acid

An acid that partially dissociates in solution, leading to an equilibrium between the undissociated acid and its ions.

Conjugate Acid

The species formed when a base gains a proton.

Excess Strong Base

The amount of strong base remaining after it has reacted with a weak acid in a titration.

Indicator

A weak organic acid or base that changes color depending on the pH of the solution.

Titration

A method of quantitative chemical analysis used to determine the concentration of an identified analyte.

Equivalence Point

The point in a titration at which the amount of titrant is stoichiometrically equivalent to the amount of substance in the sample.