How to Calculate Ksp for Ferrous Oxalate in a Galvanic Cell?

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To calculate the Ksp for ferrous oxalate in a galvanic cell setup, the student uses the Nernst Equation, considering the measured voltage of 100mV between the half-cells. The first half-cell contains 0.11M ferrous nitrate, while the second half-cell consists of 50.0ml of 0.15M oxalic acid mixed with 1.0ml of the ferrous nitrate solution. The challenge arises from the presence of multiple chemicals in one half-cell, complicating the determination of the reaction quotient, Q. The primary voltage source is the concentration difference of Fe2+ ions in the two half-cells. The student needs to derive Q to proceed with the Ksp calculation effectively.
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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).
 
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This is basically a concentration cell - the only source of voltage is the difference between concentrations of Fe2+ in both half cells.
 
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