8-6. The standard electrode potential for the reduction of Ni^2+ to Ni is -0.25V Would the potential of a nickel electrode immersed in a l .00 M NaO H solu- tion saturated with Ni(OH)_(2) be more negative than E_(Ni^2+/Ni)^0 or less? Explain.

The potential of a nickel electrode immersed in a 1.00 M NaOH solution saturated with Ni(OH)2 would be more negative than the standard electrode potential for the reduction of Ni2+ to Ni, which is -0.25 V. This is because the presence of Ni(OH)2 and NaOH in the solution creates a nickel-hydroxide battery, where the Ni electrode acts as the negative electrode and undergoes oxidation, while the hydroxide ions in the solution act as the positive electrode and undergo reduction. The overall reaction in this battery is:<br /><br />Ni(s) + 2OH-(aq) → Ni(OH)2(s) + 2e-<br /><br />The potential of the nickel electrode in this reaction is determined by the Nernst equation, which takes into account the concentration of the reactants and products in the solution. In this case, the concentration of Ni(OH)2 is high, which means that the potential of the nickel electrode will be more negative than the standard electrode potential for the reduction of Ni2+ to Ni.