Phase Diagram of Ternary Calcium Acetate—Magnesium Acetate—Water System at 298 K, 313 K and 323 K

Abstract

The solubility data of the calcium acetate-magnesium acetate-water system at 298, 313, and 323 K were measured using the SchreinemakerÕs wet residue method, the corresponding phase diagram for the system were constructed. The solid phase in the system at different temperatures was confirmed by the SchreinemakerÕs wet residue method, which correspond to Mg(CH 3 COO) 2 AE4H 2 O and Ca(CH 3 COO) 2 AE2H 2 O. At the studied temperature, no double salt was formed. The crystalline region of Ca(CH 3 COO) 2 AE2H 2 O is larger than that of Mg(CH 3 COO) 2 AE4H 2 O. The solubility of Mg(CH 3 COO) 2 increases with the increasing of the temperature, while the solubility of Ca(CH 3 COO) 2 decreases with the increasing of the temperature.

Experimental investigation of enhanced carbonation by solvent extraction for indirect CO2mineral sequestration

“…Owing to the concentration of unreacted calcium acetate still increased with the initial concentration of calcium acetate aqueous solution, this promotion was enhanced, and consequently the crystallization conversion as well as acetic acid extraction ratio increased. However, with the initial concentration increased, the interaction between acetate ions and calcium ions at high initial concentration becomes stronger, so promotion of low concentration is more significant than the high concentration of calcium acetate. Therefore, the extent of the increase in crystallization conversion and acetic acid extraction ratio at the high initial concentration was less than the extent of the decrease at the low initial concentration.…”

“…All of the stock solutions including Ca(Ac) 2 and a mixture of Ca(Ac) 2 with Mg(Ac) 2 , were freshly prepared by dilution with distilled water at ambient temperature The pH values of the prepared aqueous solutions were adjusted from 5.0 to 12.0 before it yield the desired concentrations by either adding calcium hydroxide pellucid solution or acetic acid. Due to limitation in solubility, the concentration of Ca(Ac) 2 in fresh solution was varied from 0.20 to 1.85 mol/L, while the concentration of Ca(Ac) 2 in the mixed solution decreased to 1.2 mol/L with the concentration of Mg(Ac) 2 increased to 0.8 mol/L.…”

Kinetics of chemical absorption of carbon dioxide into aqueous calcium acetate solution

“…For these experiments, pure carbon dioxide gas was used and temperature was kept constant at 293.15 ± 0.5 K. The concentration of the bulk aqueous calcium acetate solution was changed in the range from 0.1 to 1.14 M (ie, approximately between 2 and 20 wt%). The reason for choosing the maximum concentration as 1.14 M (or approximately 20%) is that the solubility of calcium acetate is 26 g/100 g solution at 298.15 K. [47][48][49][50] The concentrations of aqueous calcium acetate solutions with the indicated solubility limitation were arranged as 2.00, 4.01, 6.02, 8.00, 10.01, 15.01, and 20.01% w/w (or 113.7, 227.5, 341.9, 454.3, 568.4, 851.8, and 1135.6 mol/m 3 , respectively), and experiments for all concentration values were repeated three times. For all experiments, a reaction rate was calculated and the effect of concentration of calcium acetate solution on the kinetics of reaction was obtained.…”

Phase Diagram of Ternary Magnesium Acetate-Acetic Acid-Water System at 298.1 and 333.1 K

“…The two binary subsystems, Mg(CH 3 COO) 2 -H 2 O [9][10][11] and Ca(CH 3 COO) 2 -H 2 O, [18] and the ternary subsystem, Mg (CH 3 COO) 2 -Ca(CH 3 COO) 2 -H 2 O, [18] have been investigated, but the investigation of this latter ternary system involved only solubility studies and no phase diagram was proposed. The present investigation was undertaken to construct, at least, partial phase diagrams for the Mg(CH 3 COO) 2 -CH 3 COOH-H 2 O system at 298.1 ± 0.1 K and at 333.1 ± 0.1 K.…”