An electrochemical cell consists of a standard hydrogen...

An electrochemical cell consists of a standard hydrogen electrode and a copper metal electrode. If the copper electrode is placed in a solution of 0.10 $M$ NaOH that is saturated with $\mathrm{Cu}(\mathrm{OH})_{2},$ what is the cell potential at $25^{\circ} \mathrm{C} ?\left[\mathrm{For} \mathrm{Cu}(\mathrm{OH})_{2}\right.$ $K_{\mathrm{sp}}=1.6 \times 10^{-19} \cdot \mathrm{J}$

An electrochemical cell consists of a standard hydrogen electrode and a copper metal electrode. If the copper electrode is placed in a solution of 0.10 $M$ NaOH that is saturated with $\mathrm{Cu}(\mathrm{OH})_{2},$ what is the cell potential at $25^{\circ} \mathrm{C} ?\left[\mathrm{For} \mathrm{Cu}(\mathrm{OH})_{2}\right.$
$K_{\mathrm{sp}}=1.6 \times 10^{-19} \cdot \mathrm{J}$

Key Concepts

Electrochemical Cell and Cell Potential

An electrochemical cell consists of two electrodes where redox reactions occur. The overall cell potential is determined by the difference between the electrode potentials of the two half-cells. Using the measured or calculated ion concentrations and standard potentials, the individual electrode potentials are computed, and their difference yields the net cell potential, indicating the driving force for the redox reaction in the cell.

Nernst Equation

The Nernst equation relates the electrode potential to the concentration (or activity) of the ionic species involved in the half?reaction under non?standard conditions. It allows correction of the standard electrode potential by accounting for the effect of ion concentration through the logarithmic term, which is crucial when the solution conditions deviate from the standard state.

Standard Electrode Potentials

Standard electrode potentials are the intrinsic potentials of half?reactions measured under standard conditions. They provide a reference for comparing the tendency of different electrodes to be reduced or oxidized. In a cell, the difference between these potentials determines the spontaneity and magnitude of the current flow.

Solubility Product Equilibrium

The solubility product (Ksp) expresses the equilibrium between a sparingly soluble compound and its constituent ions in solution. It is used to calculate the concentration of ions when a compound is in equilibrium with its solid form. In electrochemical problems, this concept is applied to deduce the actual ion concentrations, which then modify the electrode potentials via the Nernst equation.

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