Solving the Nernst Equation for Zn^2+ Concentration

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SUMMARY

The discussion focuses on solving the Nernst equation to determine the concentration of Zn2+ in a galvanic cell setup. The cell consists of a 0.10 M CuSO4 solution with Cu(s) and a 1 M NH3 solution with 0.05 M ZnSO4 and Zn(s). The measured cell potential is 1.31 V, and the Nernst equation is applied to find the reaction quotient Q, calculated as 7.61E-8. The confusion arises regarding the correct definition and application of Q in the context of the cell reactions.

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morgan8222
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I built a cell with one side containing the solution 0.10 M CuSO4 with Cu(s) in it. The other side has 1 M NH3 and 0.05 M ZnSO4 with Zn(s) in it. The measured cell potential was 1.31.

I am using the Nernst equation. I need to find the concentration of Zn^2+.

E=E"-(0.059/2)logQ

1.31 = 1.10 -(0.059/2) log Q

Q = 7.61E-8

I am confused about what Q is. I know its definition, but I am not sure about the reaction and which concentrations to use.
Could someone help me out?
 
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On both sides you have metal electrode submerged in the solution of its own ions. In both cases reaction is identical (although metal is different).
 

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