SUMMARY
The mole ratio of thiosulfate ions (S2O3 2-) to permanganate ions (MnO4-) is established as 5:1 based on the stoichiometry of the redox reactions involved. The reaction between potassium permanganate (KMnO4) and iodine (I2) produces a 2:5 ratio, while the subsequent reaction between iodine and thiosulfate yields a 1:2 ratio. Consequently, the relationship can be expressed as n(S2O3 2-) = n(MnO4-) x 5, clarifying the stoichiometric coefficients derived from the balanced half-reactions. Understanding these relationships is crucial for accurate titration calculations in redox chemistry.
PREREQUISITES
- Understanding of redox reactions and stoichiometry
- Familiarity with the half-reaction method in balancing equations
- Knowledge of titration techniques and their applications
- Basic chemistry concepts related to moles and molarity
NEXT STEPS
- Study the half-reaction method for balancing redox reactions
- Learn about the principles of titration and its applications in analytical chemistry
- Explore the role of iodine as an intermediate in redox reactions
- Investigate the properties and reactions of thiosulfate in various chemical contexts
USEFUL FOR
Chemistry students, educators, and laboratory technicians involved in analytical chemistry, particularly those focusing on redox titrations and stoichiometric calculations.