Calculating Ksp in Galvanic Cells

[reising1]

Homework Statement

A student constructs a galvanic cell with one half-cell containing 0.11M ferrous nitrate, Fe(NO3)2, and the other half-cell made from 50.0ml of 0.15M oxalic acid and 1.0ml of the 0.11M ferrousnitrate. Ferrous oxalate is only slightly soluble. The half-cells contain iron electrodes and they are connected with a salt bridge. The student measures a voltage of 100mV between the two half-cells. Calculate the experimental Ksp for ferrous oxalate based on this data.

Homework Equations

Nernst Equation: E = E(standard) - (.05971/n)log Q
Ferrous Nitrate: Fe(NO3)2
Oxalic Acid: C2H2O4

The Attempt at a Solution

I'm not sure what to do because one of the half cells contains multiple chemicals. In addition, I'm not sure what the equation would look like (meaning, I'm having trouble finding Q).

 

[Borek]

This is basically a concentration cell - the only source of voltage is the difference between concentrations of Fe²⁺ in both half cells.