|
|
|
|
The following example illustrates how the stability or predominance diagram of water can be constructed from its basic thermodynamic information. The following equation describes the equilibrium between hydrogen ions and hydrogen gas in an aqueous environment:
Adding sufficient
At higher pH than neutral, this equation is a more appropriate representation of the situation. However, since the concentrations of [H+] and [
that becomes equation at 25oC and the hydrogen partial pressure of value unity.
This equation and its alkaline or basic form, delineate the stability of water in a reducing environment and are represented in a graphical form by the sloping line (a) on the Pourbaix diagram shown below.
E-pH stability diagram of water at 25oC
Below the equilibrium reaction shown as line (a) in this figure, the decomposition of H2O into hydrogen is favored while it is thermodynamically stable above the same line (a). As potential becomes more positive or noble, water can be decomposed into its other constituent, oxygen, as illustrated in equations and for respectively the acidic form and neutral or basic form of the same process.
And again these equivalent equations can be used to develop a Nernst expression of the potential in standard conditions of temperature and oxygen partial pressure of value unity.
The line labeled (b) in the previous Figure represents the behavior of E vs. pH for this last equation. The chemical behavior of water across all possible values of potential and pH is divided into three regions. In the upper region, water can be oxidized to produce oxygen while in the lower region it can be reduced to form hydrogen gas. Water is therefore only thermodynamically stable between lines (a) and (b). It is common practice to superimpose these two lines (a) and (b) on Pourbaix diagrams to mark the water stability boundaries.
