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Structure of thermodynamic data sets

Element Master species Alkalinity mole mass in mg/L atomic mass of elements [Pg.78]

The contribution of each master species to the alkalinity in Table 22 is calculated according to the predominant species at a pH of 4.5. For example, Fe3+ forms at pH 4.5 the predominant species Fe(OH)2+ with two OH -ions that are able to bind two H+-ions. Therefore a factor of -2 results for the alkalinity. For inorganic C with the dominant species H2C03 and two FT -ions the factor will be +2. [Pg.78]

Column 4 in Table 22 specifies in which way the input in mg/L has to be done. In this example, C has to be defined as carbonate, however, nitrate, nitrite, ammonia each defined as elementary nitrogen, P as elementary phosphorous, S as sulfate and Si as Si02. If, for example, P is input as phosphate in mg/L, all [Pg.78]

For all reactions being put in data sets manually, the used master species, if not yet existent, have to be defined using the keyword SOLUTION MASTER SPECIES. [Pg.79]

For the species in solution (SOLUTIONSPECIES, Table 23), listed in the top row with current number, solubility constant log k and enthalpy delta h are given in kcal/mol or kJ/mol at a temperature of 25 °C. Using the sub-key-word gamma parameters for the calculation of the activity coefficient y according the WATEQ-DEBYE-HUCKEL ion dissociation theory (compare to chapter 1.1.2.6.1) are given. With the sub-key-word analytical , coefficients At to A5 are defined to calculate the temperature dependence of the solubility-product constant. [Pg.79]


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