A solution at 25^∘ C contains 1.0M Cu^2+ and 1.0 ×10^-4 M Ag^+. Which metal will plate out first

step 1 So the key here is that you have two metals that can be reduced. So the one that has the greater

A solution at 25^∘ C contains 1.0M Cu^2+ and 1.0 ×10^-4 M...

A solution at $25^{\circ} \mathrm{C}$ contains 1.0$M \mathrm{Cu}^{2+}$ and $1.0 \times 10^{-4} M$ $\mathrm{Ag}^{+}$. Which metal will plate out first as the voltage is gradually increased when this solution is electrolyzed? (Hint: Use the Nernst equation to calculate $\mathscr{E}$ for each half-reaction.)

A solution at $25^{\circ} \mathrm{C}$ contains 1.0$M \mathrm{Cu}^{2+}$ and $1.0 \times 10^{-4} M$
$\mathrm{Ag}^{+}$. Which metal will plate out first as the voltage is gradually increased when this solution is electrolyzed? (Hint: Use the Nernst equation to calculate $\mathscr{E}$ for each half-reaction.)

Key Concepts

Concentration Effects in Redox Reactions

This concept highlights that the effective electrode potential of a half-reaction is influenced by the concentration of the ionic species involved. While standard potentials are measured under standard conditions, deviations such as decreased ion concentration can shift the actual reduction potential required for electrolysis, thereby affecting the order in which different metals plate out.

Electrodeposition

Electrodeposition is the process of depositing a substance, such as a metal, onto an electrode through the application of an electric current. The likelihood of a metal plating onto the electrode depends on its reduction potential, and the metal that reduces at a higher effective electrode potential will deposit first.

Standard Reduction Potential

This concept refers to the inherent tendency of a chemical species to gain electrons (be reduced) under standard conditions. It is expressed in volts and serves as a benchmark to predict the direction of electron flow in redox reactions. The species with the higher standard reduction potential is generally reduced first in an electrochemical process.

Nernst Equation

The Nernst equation is used to calculate the electrode potential of a half-cell reaction under non-standard conditions by accounting for the effect of ion concentrations. It helps in understanding how variations in the concentration of reacting species influence the effective voltage required for a redox reaction to occur.

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