Acid–Base Titration: Overview

Acid-base titration determines the unknown concentration of an acid or base using a titrant of known concentration. The titrant is gradually added to the unknown solution, causing predictable pH changes. This technique is fundamental in analytical chemistry for quantifying acid or base content in samples.

A titration curve plots pH changes against the volume of titrant added, displaying an S-shaped pattern. The curve reveals how the solution's pH evolves during titration and helps identify the equivalence point. Different acid-base combinations produce curves with distinct characteristics, making them instrumental in monitoring titration progress.

For strong acids neutralized by strong bases, the equivalence point occurs at pH 7, indicating complete neutralization of hydronium ions. Weak acids reach their equivalence point above pH 7 because the conjugate base produced undergoes hydrolysis, making the solution slightly basic. This difference reflects the strength of the acid being neutralized.

Strong acid titrations exhibit a steep, sudden pH jump near the equivalence point. In contrast, weak acid titrations show a more gradual pH shift in this region. The buffer region present in weak acid titrations resists rapid pH changes, resulting in a less pronounced vertical section on the titration curve.

At the half-equivalence point, the concentrations of the weak acid and its conjugate base are equal. At this point, the pH equals the pKa of the acid. This relationship is useful for determining acid strength and understanding the buffer capacity of the solution during titration.

When titrating strong or weak bases with strong acid, the titration curve is inverted compared to acid titrations. The curve starts from a higher pH and decreases as strong acid is added. This inverted S-shaped pattern reflects the decreasing basicity of the solution as the titrant neutralizes the base.

Titration curves vary based on whether strong or weak acids and bases are involved. Strong acid-strong base combinations produce symmetric S-curves with equivalence points at pH 7. Weak acid-strong base and strong acid-weak base combinations produce asymmetric curves with equivalence points shifted away from pH 7, reflecting the hydrolysis of conjugate species.