Chapter 19, Problem 35E

Interpretation Introduction

Interpretation:

The value of $\left[{\text{Ag}}^{+}\right]$ in the cell should be calculated.

Concept introduction:

In an electrochemical cell there are two electrodes that can be observed. Electrodes are named according to their tendency of oxidation or reduction.

If oxidation takes place on an electrode, that electrode is called anode. The removal of electrons takes place from the species present in anode.

If reduction takes place on an electrode, that electrode is called cathode. The addition of electrons takes place to the species present in cathode. The electrode potential of cell is calculated from reduction electrode potential of cathode and anode as follows:

$E^0{}_{\text{cell}}=E^0{}_{\text{cathode}}-E^0{}_{\text{anode}}$

Nernst equation is as follows:

${\text{E}}_{cell}={\text{E}}^0{}_{cell}-\frac{0.0592\text{ V}}{\text{z}}\text{ log Q}$

Z = number of moles of electrons transferred in the cell.

Q is ratio of concentration of product to reactant.