Acid-Base Titrations

Flashcards about acid base titrations

Titration

A process used to determine the concentration of a solution (analyte) by reacting it with a solution of known concentration (titrant).

Equivalence Point

The point in a titration where the moles of titrant added are stoichiometrically equivalent to the moles of analyte in the sample.

Strong Acid + Strong Base Titration

Titration involving a strong acid and a strong base, resulting in a pH of 7 at the equivalence point at 25 degrees Celsius.

pH before Equivalence Point (Strong Acid + Strong Base)

pH is determined by the amount of excess [H+] remaining.

pH past Equivalence Point (Strong Acid + Strong Base)

pH is based on excess [OH-].

Weak Acid + Strong Base Titration

Titration involving weak acid and a strong base, where pH is based on Ka of HA before titrant is added. It also has an equivalence point and excess OH-.

pH before Equivalence Point (Weak Acid + Strong Base)

pH is determined by the buffer composition.

pH at Equivalence Point (Weak Acid + Strong Base)

pH is based on [A-], and Kb.

pH past Equivalence Point (Weak Acid + Strong Base)

pH is based on excess OH-.

Weak Base + Strong Acid Titration

Titration involving a weak base and a strong acid.

pH before Equivalence Point (Weak Base + Strong Acid)

pH is determined by the buffer composition.

pH at Equivalence Point (Weak Base + Strong Acid)

pH is based on [BH+] and Ka.

pH past Equivalence Point (Weak Base + Strong Acid)

pH is based on excess H+.

Multiple Ionizations

Acids with more than one proton or bases that can gain more than one proton, resulting in multiple equivalence points in the titration curve.

Limiting Reactant

The reactant that is completely consumed in a chemical reaction and determines the amount of product formed. Always calculate moles of analyte and titrant