Question

Suppose that we titrate 100.0 ML of 0.0500 M Fe^+ with 0.100 M Ce^4+, by using the cell and figure 16-1. The equivalence point occurs when Vce^4+ = 50.0ml because the Ce^4+ is twice as concentrated as the Fe^2+.

Calculate the cell voltage at 36.0, 50.0 and 63.0ml 

Answer 1

E°_Ce⁴⁺_/Ce³⁺ = 1.44 V 

And E°_Fe³⁺_/Fe²⁺ = 0.77 V 

Thus by addition of Ce⁴⁺ as titrant to the solution, Fe²⁺ oxidises to Fe³⁺ .