Final answer:
The titration with KIO3 is used to determine stoichiometry in redox reactions, while titration with NaOH is typically used in neutralization reactions. The equivalence point in NaOH titration varies distinctly between strong and weak acids due to different pH changes.
Step-by-step explanation:
The titration with KIO3 involving the oxidizing agent IO3- and KI allows us to determine the stoichiometry between the analyte NaOCl and the titrant Na2S2O3. The key reactions involve the oxidation of I- to I3- by OCl- and then the titration of this I3- with Na2S2O3, a reducing agent.
Meanwhile, the titration with NaOH typically involves neutralization reactions. A titration curve produced with NaOH and a strong acid shows a steep rise in pH at the equivalence point, enabling clear identification of this point when using indicators. However, with a weak acid, such as acetic acid, and NaOH, the choice of indicator is critical as the pH change is more gradual.
Comparing KIO3 titration with NaOH titration reveals differences in reaction types (redox vs neutralization), stoichiometry, and the precision in identifying the equivalence point depending on the strength of acids or the presence of a strong base.