Gneiss\|distilled water interaction at room temperature was investigated with batch\|reactors to study water\|rock reaction and geochemical evolution of the aqueous phase with time. The ion concentrations in water wer...Gneiss\|distilled water interaction at room temperature was investigated with batch\|reactors to study water\|rock reaction and geochemical evolution of the aqueous phase with time. The ion concentrations in water were controlled not only by the dissolution of primary minerals, but also by the precipitation of secondary minerals. The decreasing fraction sizes of gneiss could favor dissolution and precipitation simultaneously. Ca\+\{2+\} and K\++ were the major cations, and HCO\+-\-3 was the major anion in water. All the ions except Ca\+\{2+\} increased in concentration with time. The Ca\+\{2+\} release from the rock to the aqueous phase was initially much faster than the release of K\++, Na\++ and Mg\+\{2+\}. But after about 5-24 hours, the Ca\+\{2+\} concentrations in water decreased very slowly with time and became relatively stable. During the experiment, the water varied from the Ca\|(K)\|HCO\-3\|type water to the K\|Ca\|HCO\-3\|type water, and then to the K\|(Ca,Na)\|HCO\-3\|type water. The water\|gneiss interaction was dominated by the dissolution of K\|feldspar in the solution. The remaining secondary minerals were mainly kaolinite, illite and K(Mg)\|mica.展开更多
文摘Gneiss\|distilled water interaction at room temperature was investigated with batch\|reactors to study water\|rock reaction and geochemical evolution of the aqueous phase with time. The ion concentrations in water were controlled not only by the dissolution of primary minerals, but also by the precipitation of secondary minerals. The decreasing fraction sizes of gneiss could favor dissolution and precipitation simultaneously. Ca\+\{2+\} and K\++ were the major cations, and HCO\+-\-3 was the major anion in water. All the ions except Ca\+\{2+\} increased in concentration with time. The Ca\+\{2+\} release from the rock to the aqueous phase was initially much faster than the release of K\++, Na\++ and Mg\+\{2+\}. But after about 5-24 hours, the Ca\+\{2+\} concentrations in water decreased very slowly with time and became relatively stable. During the experiment, the water varied from the Ca\|(K)\|HCO\-3\|type water to the K\|Ca\|HCO\-3\|type water, and then to the K\|(Ca,Na)\|HCO\-3\|type water. The water\|gneiss interaction was dominated by the dissolution of K\|feldspar in the solution. The remaining secondary minerals were mainly kaolinite, illite and K(Mg)\|mica.
