Ladder diagrams are useful tools for understanding redox equilibrium reactions, especially the effects of concentration changes on the electrochemical potential of the reaction. The vertical axis in the redox ladder diagrams represents the electrochemical potential, E. The area of predominance is demarcated using the Nernst equation.

Consider the Fe³⁺/Fe²⁺ half-reaction, which has a standard-state potential of +0.771 V. At potentials more positive than +0.771 V, Fe³⁺ predominates, whereas Fe²⁺ predominates at potentials more negative than +0.771 V. When the Fe³⁺/Fe²⁺ half-reaction is coupled with the Sn⁴⁺/Sn²⁺ reaction, the concentration of Fe³⁺ can be reduced by adding Sn²⁺ to excess. In this case, the potential of the resulting solution approaches +0.154 V down to +0.771 V, and Fe²⁺ and Sn⁴⁺ predominate.

To understand the interdependence between change in solution pH and electrochemical potential, consider the example of UO₂²⁺/U⁴⁺ half-reaction, whose electrochemical potential varies with the pH of the solution. As the pH of the solution decreases, the electrochemical potential increases, changing the dominant species from U⁴⁺ to UO₂²⁺.