| Article ID | Journal | Published Year | Pages | File Type |
|---|---|---|---|---|
| 4699880 | Chemical Geology | 2011 | 7 Pages |
Pure-iron end-member hibbingite, Fe2(OH)3Cl(s), may be important to geological repositories in salt formations, as it may be a dominant corrosion product of steel waste canisters in an anoxic environment in Na–Cl- and Na–Mg–Cl-dominated brines. In this study, the solubility of Fe2(OH)3Cl(s), the pure-iron end-member of hibbingite (FeII, Mg)2(OH)3Cl(s), and Fe(OH)2(s) in 0.04 m to 6 m NaCl brines has been determined. For the reactionFe2(OH)3Cl(s) + 3H+ ↔ 3 H2O + 2 Fe2+ + Cl−,the solubility constant of Fe2(OH)3Cl(s) at infinite dilution and 25 °C has been found to be log10K = 17.12 ± 0.15 (95% confidence interval using F statistics for 36 data points and 3 parameters). For the reactionFe(OH)2(s) + 2H+ ↔ 2 H2O + Fe2+,the solubility constant of Fe(OH)2 at infinite dilution and 25 °C has been found to be log10K = 12.95 ± 0.13 (95 % confidence interval using F statistics for 36 data points and 3 parameters). For the combined set of solubility data for Fe2(OH)3Cl(s) and Fe(OH)2(s), the Na+–Fe2+ pair Pitzer interaction parameter θNa+/Fe2+ has been found to be 0.08 ± 0.03 (95% confidence interval using F statistics for 36 data points and 3 parameters). In nearly saturated NaCl brine we observed evidence for the conversion of Fe(OH)2(s) to Fe2(OH)3Cl(s). Additionally, when Fe2(OH)3Cl(s) was added to sodium sulfate brines, the formation of green rust(II) sulfate was observed, along with the generation of hydrogen gas. The results presented here provide insight into understanding and modeling the geochemistry and performance assessment of nuclear waste repositories in salt formations.
Research Highlights► log10 K of Fe2(OH)3Cl(s) = 17.12 ± 0.15. ► log10 K of Fe(OH)2(s) = 12.95 ± 0.13. ► θNa+/Fe2+ = 0.08 ± 0.03. ► GR(II)SO4(s) and hydrogen were generated when Fe2(OH)3Cl was added to Na2SO4 brine under anoxic conditions.
