Copper pourbaix diagram
Consideration is given only to equilibrium conditions in specified environment, and factors such as temperature and velocity are not considered, which may seriously affect the corrosion rate.These diagrams are purely based on thermodynamic data and do not provide any information on the reactions and not possible to measure the corrosion rates.Small amounts of impurities and alloying elements may change the diagram. The validity of the diagrams is limited to reactions between pure metals, pure water and the species that can be formed from these.Potential-pH diagrams for the copper-water system and the carbon-water system are shown in Figs. Pourbaix diagrams show the ranges of potential and pH over which various ions, oxides, pure metals, etc., are thermodynamically stable. To show which environmental pH and potential changes will reduce or prevent corrosion diagrams for the metal and the principal element in the reducing agent.To make a basis for estimation of the corrosion product compositions at various pH and potential combinations.To show the directions of the various reactions at given pH and potential.The diagram is computed for the equilibrium conditions at 77☏ (25☌).This equilibrium indicates electron transfer as well as pH. Sloping, straight lines give the redox potentials of a solution in equilibrium.
![copper pourbaix diagram copper pourbaix diagram](https://www.researchgate.net/profile/Eric-Van-Hullebusch/publication/340102631/figure/fig4/AS:872274831880192@1584977934149/Pourbaix-diagram-for-a-Cu-H2O-system-b-Cu-H2O-citrate-system-at-298-K-total-copper.jpg)
![copper pourbaix diagram copper pourbaix diagram](https://d3i71xaburhd42.cloudfront.net/d7c2a995b8f34dcaf8289365aab27b37b81d04cd/4-Figure3-1.png)
Pourbaix diagrams are plotted by using the Nernst equation (an equation used to calculate electrode potential).