[bblue]

Given the following half-reactions:

 Ce4+ + e− → Ce3+      E° = 1.72 V 
 Fe3+ + e− → Fe2+      E° = 0.771 V 

A solution is prepared by mixing 10. mL of 0.30 M Fe2+ with 9.0 mL of 0.12 M Ce4+.

What is the potential of a platinum electrode dipped into the resulting, equilibrated, solution (relative to SHE)?

I am not rly sure how to use the concentrations to calculate the potential. Is there some formula that I can use???

[Borek]

Nernst equation.

[bblue]

If the qn is asking for the E⁰_cell then can i not just substract the anode E⁰ from the cathode E⁰ because the solution is at equilibrium which means that the E will be = 0

or if i do use the nernst eqn then:
E⁰ = .05961 / n * log( [Ce³⁺][Fe³⁺] / [Ce⁴⁺][Fe²⁺]
I dont know how to find the [Fe³⁺] or [Ce³⁺]

[Borek]

Look for hints here:

http://www.titrations.info/potentiometric-titration-curve-calculation