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crystallized after 72h to get better crystallized product within 6 ~ 49h time crystallization system for the magnesium lithium silicate
Date: 2016/6/28 16:31:28

Jinhua season was the first to use alkali metal silicates and natural clays synthesized hectorite. Processing alkali metal silicates (sodium silicate, potassium silicate) with hydrochloric acid or sulfuric acid and natural clay (bentonite, kaolinite and attapulgite, etc.), decomposed to the corresponding oxides. Then follow the chemical composition of magnesium lithium silicate material slurry formulated within the range of 120 ~ 250 ° hydrothermal 1 ~ 6h to obtain high purity products. Zhou Chunhui and etc. use LiF, MgCl2, sodium silicate and ammonia as raw materials, 6h hydrothermal reaction that can generate lithium magnesium silicate, crystallized after 72h to get better crystallized product within 6 ~ 49h time crystallization system for the magnesium lithium silicate, silicon lithium, LiF and MgOH multiphase.

Fast atom bombardment mass spectrometry (FABMS) was applied to the direct detection of silica species dissolved in LiCl, NaCl, MgCl2, CaCl2 and SrCl2 solutions in order to investigate its dissolution process in solution. Several species of dissolved magnesium lithium silicate complexes in the solution were directly detected by FABMS. The peak intensities of [SiO2(OH)2Na]−, [SiO3(OH)Ca]− and [SiO3(OH)Sr]− increased with increasing concentrations of NaCl, CaCl2 and SrCl2, whereas the peak intensities of [SiO2(OH)2Li]− and [SiO3(OH)Mg]− did not increase with increasing concentrations of LiCl and MgCl2. These results indicte that silicate and cation bind in the solution not after but before ionization. The isotope pattern of Sr2+ confirmed the existence of the silicate–Sr complex not only with increase of the concentration of silica but also the mass numbers of Sr. The silicate complexes formed with Na+, Ca2+ and Sr2+ showed high stability in chloride solution. This is in good accordance with the fact that Na+, Ca2+ and Sr2+ accelerate the dissolution of silica to form complexes during solution equilibrium. Considering that the stability constant was examined and reported in other papers, this new findings that Mg2+ does not form a complex with silicic acid (Si(OH)4) is very important. 


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