Final answer:
The equivalence point volume, e, for the titration of 0.100 M Fe²+ with 0.100 M Ce4+ is 50.0 mL. This value allows for the construction of a titration curve and is essential for the quantitative analysis in a redox titration.
Step-by-step explanation:
The equivalence point volume, e, in a titration is the volume at which the amount of titrant added is stoichiometrically equivalent to the concentration of analyte in a solution. In the provided data for the titration of 0.100 M Fe²+ with 0.100 M Ce4+, the equivalence point volume is determined to be 50.0 mL. This information is crucial for sketching a titration curve, which involves plotting the titrant's volume against the potential (E) on a graph, and indicating the equivalence point with a vertical line at 50.0 mL of Ce4+ as seen in Figure 9.37a. The titration curve represents how the potential changes as the volume of Ce4+ added changes, reaching the equivalence point where Fe²+ has been completely reacted with Ce4+.
Understanding the equivalence point is central to performing a titration and interpreting the results. It helps in analyzing the reaction stoichiometry and calculating concentrations. For example, when the titrant volume exceeds the equivalence point volume as in the given example with a volume of 37.50 mL, the solution pH can be determined using the concentrations of hydroxide and hydronium ions remaining in the solution, illustrating the chemical principles of acid-base reactions and redox reactions that govern the process of titration in Chemistry.
Additional details provided, such as the effect of pH on the equivalence point potential and the description of redox buffers after the equivalence point, offer a complete understanding of the electrochemical context of the titration. Such comprehensive analysis forms the foundation for constructing accurate titration curves and subsequently, for successful quantitative chemical analysis.