Zero Potential Point and Equilibrium Point
In electrochemical systems, the zero potential point is used to refer to the point of electrochemical equilibrium at which the potential of an aqueous solution is the same for all components. It is a point on the electrochemical potential of a reaction where the potential of that reaction is equal to zero. When an aqueous solution is at zero potential, there is no net flux in any direction, and all of its reactants are in equilibrium. This is due to the fact that the electrochemical potential of each of the reactants is the same in all directions.
The zero potential point can be measured using potentiometry, a method in which the potential of a solution is measured relative to a reference electrode. In order to accurately measure the zero potential point, a reference electrode of the same material as the reacting species must be used. When the two are perfectly matched, the zero potential point is reached.
The equilibrium point is a point on the electrochemical potential of a reaction at which the reaction and its reverse reaction occur at equal rates. At the equilibrium point, the system has no net change in reactant or product concentration. This occurs because all of the reactants, products, and solutes in the system are converted into each other at the same rate, resulting in no net movement of any of the components in either direction.
The equilibrium point is an important concept in electrochemical systems, as it allows for the determination of equilibrium constants and the steady-state concentrations of the reactants and products. The equilibrium point is also used to calculate thermodynamic quantities such as Gibbs free energy and enthalpy.
In summary, the zero potential point is the point at which the potential of an aqueous solution is the same for all components. It can be measured using potentiometry, and requires a reference electrode of the same material as the reacting species to give accurate results. The equilibrium point is a point on the electrochemical potential of a reaction at which the reaction and its reverse reaction occur at equal rates, and is used to calculate thermodynamic quantities.
