Abstract
ABSTRACTBased on the principles of ionic balance, electro-neutrality and the existing thermodynamic data, the thermodynamics equilibrium on calcium dissolution in the system of Ca(II)-NH3-NH4Cl-H2O was theoretically calculated. The results show that the equilibrium pH values in the system vary from 11.43 to 12.59, and the solubility of Ca(II) is significant in the system of NH4Cl-NH3-H2O. The c(NH4OH) has little influence on c(Ca2+)T and when the ammonia concentration is kept constant, the total calcium concentration (c(Ca2+)T) with a maximum concentration of 2.03 mol/L increases linearly with the increase of concentration of c(NH4Cl). Calcium mainly presents in the form of calcium-bearing complexes instead of calcium ion in the system. The reaction degrees of Ca2+ with ammonium hydroxide and H2O are less in the system. The absolute average error of calcium equilibrium concentration between the experimental and theoretical calculated values is 7.07% in confirmatory experiments. The results are helpful to clarify the leaching behaviour of calcium ions in the system of Ca(II)-NH3-NH4Cl-H2O and provide the theoretical foundation to improve the calcium yield and remove impurities in the leaching stage of the indirect aqueous CO2 sequestration process.
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