minerals

Mineral Stability

Whether a mineral is stable in any particular environment may depend on several factors, including pressure, temperature, acidity, whether the environment is oxidising or reducing and the concentration of different components which may affect alteration reactions. Stability diagrams maybe drawn showing the changes with respect to the two most important variables, keeping other possible variables at a constant value.
Common types of stability diagrams are

Pressure-Temperature plots

For example the stability ranges for the three paramorphs of Al2OSiO4, kyanite, andalusite and sillimanite

Aluminium silicate stability diagram























Standard ambient conditions are generally taken as temperature 25oC or 298.15 K, and pressure 1 bar or 105 pascals or 0.987 atm.

Pourbaix diagrams

Pourbaix diagrams plot Eh against pH at constant temperature of 25oC and pressure 1 bar.
pH is a measure of the acidity of the environment, that is a measure of the abundance of H+ ions; it takes values up to 14, with a higher value indicating a more alkaline environment (because of the way it is defined in thermodynamics, a bigger number means fewer H+ ions). pH=1 is for an extremely acid environment, pH=7 is neutral, and pH=14 is extremely alkaline. In natural near-surface environments pH usually ranges from about 4 to about 9 (KB p225).
Just as pH is a measure of abundance of H+ ions, so Eh corresponds to the abundance of O2- ions,available for oxidation; Eh is a measure of the oxidation potential of the environment. Again because of its definition in thermodynamics, possible values vary from about -0.8 volts to about +1.2 volts, with high values for oxidising environments and low or negative values for reducing environments.
For example the diagram below is a Pourbaix diagram for manganese, created by Andel Früh and available on Wikimedia Commons. It shows the relationship between akhtenskite MnO2, bixbyite Mn2O3, hausmannite Mn3O4 and pyrochroite Mn(OH)3.

Pourbaix manganese.jpg























Activity-pH diagrams

The concentration of various ions in solution can affect the solubility of different minerals, and therefore the likelihood of their formation as solid precipitates. In thermodynamics a quantity called "activity" is defined, which is closely connected with ionic concentration. This quantity is usually given the symbol "a", and aCu2+ denotes the activity of divalent copper ions in the solution. Because of the way in which it is defined, it is better to take the logarithm of the activity as an indication of the concentration of ions, with a higher value of the log representing a greater concentration. The logs are negative, so, for example, -2 represents a greater concentration than -5. See above for the meaning of pH.
The diagram below was calculated at 298.2 K for the main Cu2+ and Pb2+ arsenate minerals. Boundaries are calculated for constant activities (roughly equivalent to concentrations) of Pb2+ and Cl- in solution, over a range of values of pH and of Cu2+ activity. Higher chloride activites make the stability fields of bayldonite and duftite vanish, with respect to the encroachment of that of mimetite (LMW p269).

stability Cu Pb.jpg























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