AP Chem Titrations Practice

A titration is a laboratory method used to determine the concentration of a solute in a solution by adding a titrant of known concentration until the reaction reaches completion.

The equivalence point is the stage in a titration where the amount of titrant added is stoichiometrically equivalent to the amount of substance in the sample solution.

The pH at the equivalence point for a strong acid-strong base titration is typically 7.0.

The pH at the equivalence point for a weak acid-strong base titration is greater than 7.0 due to the formation of a weak conjugate base.

The half-equivalence point is the point in a titration where half of the acid has been neutralized by the base, resulting in equal concentrations of the acid and its conjugate base.

The pKa of a weak acid can be determined from the half-equivalence point on the titration curve, where pH = pKa.

A buffer solution is a solution that resists changes in pH when small amounts of acid or base are added, typically composed of a weak acid and its conjugate base.

An indicator is a substance that changes color at a specific pH range, signaling the endpoint of a titration.

The formula is M1V1 = M2V2, where M is molarity and V is volume for the two solutions involved.

The titration curve visually represents the change in pH as a function of the volume of titrant added, indicating key points such as the equivalence point.