Two 20.0-mL samples, one 0.200 M KOH and the other 0.200 M CH₃NH₂, are titrated with 0.100 M HI. c. Which titration curve has the lower initial pH?

Key Concepts

Acid-Base Titration

An acid-base titration is a quantitative analytical method used to determine the concentration of an acid or base in a solution. During the titration, a solution of known concentration (the titrant) is added to a solution of unknown concentration until the reaction reaches its equivalence point, where the amount of acid equals the amount of base. The pH of the solution changes throughout the titration, and the resulting curve can provide insights into the strengths of the acids and bases involved.

pH Scale

The pH scale measures the acidity or basicity of a solution, ranging from 0 to 14. A pH less than 7 indicates an acidic solution, while a pH greater than 7 indicates a basic solution. The pH is logarithmically related to the concentration of hydrogen ions (H+) in the solution, meaning that each whole number change on the scale represents a tenfold change in acidity. Understanding the initial pH of the solutions being titrated is crucial for predicting the behavior of the titration curve.

Weak Base vs. Strong Base

In this context, KOH is a strong base that completely dissociates in solution, while CH3NH2 (methylamine) is a weak base that only partially dissociates. The initial pH of a strong base solution is typically higher than that of a weak base solution due to the complete ionization of the strong base. This difference in dissociation affects the initial pH of the solutions before titration begins, which is essential for determining which titration curve will have a lower initial pH.