Buffers and Acid-Base Titrations

A collection of vocabulary flashcards covering key concepts related to buffers and acid-base titrations.

Common Ion Effect

The shift in equilibrium caused by the addition of a compound having an ion in common with the dissolved substance.

Acetic Acid

A weak acid represented by the formula CH₃COOH.

Sodium Acetate

A strong electrolyte that can influence the equilibrium of acetic acid solutions.

Le Châtelier’s Principle

A principle stating that if a system at equilibrium is disturbed, the system shifts in a direction that counteracts the disturbance.

Buffer Solution

A solution that resists changes in pH upon the addition of small amounts of either acid or base, consisting of a weak acid or base and its salt.

Henderson–Hasselbalch Equation

An equation used to calculate the pH of buffer solutions, relating the pH to the pKa and the ratio of the concentrations of the conjugate base and acid.

Equivalence Point

The point in a titration at which the reaction between the titrant and analyte is complete.

Indicator

A substance that changes color at (or near) the equivalence point in a titration.

Titration Curve

A graph showing the change in pH as a function of the volume of titrant added in a titration.

Weak Base

A substance that does not fully ionize in solution, able to accept protons.

Acid-Base Indicator

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

pH

A measure of the acidity or basicity of a solution, calculated as the negative logarithm of hydrogen ion concentration.