Cr2O72-(aq) + Fe2+(aq) Cr3+(aq) + Fe3+(aq) (in acidic solution)
Write the balanced half-reactions and the overall balanced redox equation forthe reaction between dichromate ion and iron (II) ion in acidic solution.
Here is what I got:
Reduction half-reaction: Cr2O7^2- + 14H+ +6e^- ---> 2Cr^3 + 7H2O
Oxidation half-reaction: 6Fe^2+ ---> 6Fe^3+ + 6e^-
Redox equation: 6Fe^2+ (aq) + Cr2O7^2- + 14H+ ---> 6Fe^3+ (aq) +2Cr^3+ +7H2O
How do I calculate part 2?
From the data given above and the following data, calculate the molarity of the original iron sulfate solution.
Volume of sample = 25.00 mL
Concentration of standard dichromate, Cr2O72-, solution = 0.04343 M
Initial burette reading = 0.47 mL
Final burette reading = 21.10 mL