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The solubility of Ba(SeO 4 , SO 4 ) precipitates was determined as a function of the BaSeO 4  mole fractions, ranging from 0.0015 to 0.3830, and time with an equilibration period extending to as long as 302 days. Equilibrium/steady state conditions in this system are reached in ≤ 65 days. Pitzer's ion interaction model was used to calculate solid and aqueous phase activity coefficients. Thermodynamic analyses showed that the data do not satisfy Gibbs-Duhem equation, thereby demonstrating that a single-solid solution phase does not control both the selenate and sulfate concentrations. Our extensive data with log  10  [Ba] ranging from − 3.6 to −5.9 mol kg  – 1 , log  10  [SeO 4 ] ranging from − 3.6 to −5.2 mol kg  – 1 , and log  10  [SO 4 ] ranging from − 4.0 to −5.3 mol kg  – 1  can be explained with the formation of an ideal BaSeO 4  solid solution phase that controls the selenium concentrations and a slightly disordered/less-crystalline BaSO 4 (s) (log  10  K  ○  sp  =− 9.5 instead of − 10.05 for barite) that controls the sulfate concentrations. In these experiments the BaSO 4  component of the solid solution phase never reaches thermodynamic equilibrium with the aqueous phase. Thermodynamic interpretations of the data show that both the ideal BaSeO 4  solid solution phase and less-crystalline BaSO 4 (s) phase are in equilibrium with each other in the entire range of BaSeO 4  mole fractions investigated in this study.

Thermodynamic model for the solubility of Ba(SeO 4 , SO 4 ) precipitates