Consider the curve shown here for the titration of a weak base with a strong acid and answer each question.
c. At what volume of added acid does pH = 14 - pK_b?

Key Concepts

Titration

Titration is a quantitative analytical technique used to determine the concentration of a solute in a solution. It involves the gradual addition of a titrant (a solution of known concentration) to a sample until a reaction reaches its endpoint, which is often indicated by a color change or a pH change. In this case, the titration of a weak base with a strong acid will show a characteristic curve that reflects the pH changes as the acid is added.

pH and pK_b

pH is a measure of the acidity or basicity of a solution, defined as the negative logarithm of the hydrogen ion concentration. The pK_b is the negative logarithm of the base dissociation constant (K_b) and indicates the strength of a weak base. The relationship between pH and pK_b is crucial in titration, as it helps determine the pH at various points during the titration process, particularly at the equivalence point.

Equivalence Point

The equivalence point in a titration is the stage at which the amount of titrant added is stoichiometrically equivalent to the amount of substance in the sample. For a weak base titrated with a strong acid, this point is characterized by a significant change in pH. At this point, the weak base has been completely neutralized, and the resulting solution's pH can be calculated using the relationship between pH, pK_b, and the concentrations of the resulting species.