chp18 exercise questions (2) 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 NaOH 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 more negative potential due to the formation of a nickel-hydroxide complex.<br /><br />In this case, the nickel electrode is part of an electrochemical cell where the following half-reaction occurs:<br /><br />Ni2+ + 2e- → Ni<br /><br />The standard electrode potential for this half-reaction is -0.25 V. However, when the nickel electrode is immersed in a 1.00 M NaOH solution saturated with Ni(OH)2, the potential becomes more negative due to the formation of a nickel-hydroxide complex.<br /><br />The formation of the nickel-hydroxide complex can be represented by the following reaction:<br /><br />Ni2+ + 2OH- → Ni(OH)2<br /><br />This reaction shifts the equilibrium of the half-reaction to the left, resulting in a more negative potential for the nickel electrode. Therefore, 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.