If `E^(@)` for copper electrode is +0.34 V , will you calculate e.m.f, value when the solution in contact with it is 0.1 M in copper ions . How does e.m.f. for copper electrode change when concentration of `Cu^(2+)` ion in the solution is decreased ?

Explanation

To solve the problem, we will use the Nernst equation, which relates the standard electrode potential to the concentration of the ions involved in the half-reaction. The Nernst equation is given by:

\[ E = E^0 - \frac{RT}{nF} \ln Q \]

Where:
- \( E \) = cell potential (emf)
- \( E^0 \) = standard electrode potential
- \( R \) = universal gas constant (8.314 J/(mol·K))
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