The standard reduction potential for Cu²⁺, the voltage measured between a standard hydrogen electrode and a Cu electrode immersed in a solution where [Cu²⁺] = 1.00 M, is 0.340 V. The positive voltage indicates that the following reaction is spontaneous. H₂(g) + Cu²⁺(aq) → 2H⁺(aq) + Cu(s)
What would be the Cu²⁺ reduction potential if the standard hydrogen electrode was kept the same, but copper electrode were instead immersed in a solution of 0.450 M NaOH that was saturated with Cu(OH)₂? (The Ksp of Cu(OH)₂ is 2.20 × 10⁻²⁰).