“…Nevertheless, in the current investigation, the existence of acetic acid in the aqueous phase results also in the formation of complex salts with acetic acid. This result is in agreement with the data reported by Dunn and Philip, , who found that calcium acetate acetic acid hydrate crystallizes from calcium acetate solutions when the concentration of acetic acid in the solution is higher than 10.8 g/100 g of saturated solution, whereas calcium acetate monohydrate crystallizes at concentrations of acetic acid below this value, as shown in Figure . 3 Solubility of calcium acetate in aqueous solutions of acetic acid at 25 °C.…”
Extractive crystallization was employed for the preparation of deicing compositions of calcium
acetate (CA) and magnesium acetate (MA) at room temperature. The design system comprises
an aqueous phase as the source of calcium or magnesium ions and an organic phase as the
source of acetate ions. The process was designed with the consideration that acetic acid is used
in an organic phase as extracted from a fermentation broth. The conditions under which the
extractive crystallization method resulted in the formation of single crystals or aggregates of
calcium acetate and magnesium acetate were studied. Furthermore, the effect of acetic acid
concentration in the organic and aqueous phases on the characteristics of the obtained crystals
was investigated. Overall, the extractive crystallization process proved to be feasible at least in
the laboratory and resulted in the production of well-formed, nonporous, large single crystals
and clusters of either calcium acetate acetic acid hydrate [Ca(CH3COO)2·CH3COOH·H2O] or
magnesium acetate tetrahydrate [Mg(CH3COO)2·4H2O, α], depending on the type of salt (CaCO3
or MgCO3) used in each case.
“…Nevertheless, in the current investigation, the existence of acetic acid in the aqueous phase results also in the formation of complex salts with acetic acid. This result is in agreement with the data reported by Dunn and Philip, , who found that calcium acetate acetic acid hydrate crystallizes from calcium acetate solutions when the concentration of acetic acid in the solution is higher than 10.8 g/100 g of saturated solution, whereas calcium acetate monohydrate crystallizes at concentrations of acetic acid below this value, as shown in Figure . 3 Solubility of calcium acetate in aqueous solutions of acetic acid at 25 °C.…”
Extractive crystallization was employed for the preparation of deicing compositions of calcium
acetate (CA) and magnesium acetate (MA) at room temperature. The design system comprises
an aqueous phase as the source of calcium or magnesium ions and an organic phase as the
source of acetate ions. The process was designed with the consideration that acetic acid is used
in an organic phase as extracted from a fermentation broth. The conditions under which the
extractive crystallization method resulted in the formation of single crystals or aggregates of
calcium acetate and magnesium acetate were studied. Furthermore, the effect of acetic acid
concentration in the organic and aqueous phases on the characteristics of the obtained crystals
was investigated. Overall, the extractive crystallization process proved to be feasible at least in
the laboratory and resulted in the production of well-formed, nonporous, large single crystals
and clusters of either calcium acetate acetic acid hydrate [Ca(CH3COO)2·CH3COOH·H2O] or
magnesium acetate tetrahydrate [Mg(CH3COO)2·4H2O, α], depending on the type of salt (CaCO3
or MgCO3) used in each case.
“…Krasnicki and other works (10,12,16,20,25,26) (22) 319.15 3.0027 (22) 280.95 2.4547 (22) 300.65 2.8183 (22) 322.65 3.0255 (22) 281.05 2.4116 (27) (27) 336.15 2.9206 (27) 288.15 2.5750 308.15 2.9675 (27) 337.15 3.0532 (22) 290.65 2.7092 (27) 308.15 3.0215 338.65 3.0452 (22) 293.15 2.8677 (14) 312.75 3.0498 (27) 346.15 2.8775 (27) (22) 294.75 2.8501 (22) 313.65 3.0928 (27) 353.15 2.9729 (22) 297.25 3.0576 (27) 314.65 3.0811 (27) 357.15 2.8971 (27) 298.15 2.9288 (20) 317.65 3.0498 (27) solubility curve suggests changes in the solid phase and the solubility of calcium acetate in water is expressed for two regions by the equations:…”
Section: Resultsmentioning
confidence: 97%
“…(20,24,26,(41)(42)(43) , respectively, is postulated based on the solubility, X-ray, and thermal analysis measurements. Lumsden (23) noted that the dihydrate is stable up to T = 357.15 K (T = 356.45 K is given by Broul et al (39) ), calcium acetate monohydrate exists up to T = 331.15 K, (24) and above T = 331.15 K the hemihydrate exists.…”
Section: Resultsmentioning
confidence: 99%
“…The case of calcium acetate was investigated in 1887 by Krasnicki, (22) in 1902 by Lumsden, (23) and new solubilities were presented by Saury et al (24) at fixed temperatures. (10,12,16,20,25,26) Solubilities of barium acetate in water were determined in 1887 by Krasnicki, (22) and in 1903 by Walker and Fyffe, (27) and at constant a To whom correspondence should be addressed (E-mail: apelblat@bgumail.bgu.ac.il).…”
“…It is well-known that the preparing process of CMA is based on the phase diagram of the quinary Ca 2+ , Mg 2+ , H + // CH 3 COO ) -H 2 O system. Calcium acetate solubilities in water was investigated in 1887 by Krasnicki, [14] in 1902 by Lumsden, [15] in 1934 by Dunn [16] and new solubilities were presented by Saury et al [17] and Apelblat et al [18] Magnesium acetate solubilities were reported in 1926 by Rivett, [19] recently by Apelblat. [18,20] The solubilities of magnesium acetate and calcium acetate in water at studied temperatures (298, 313, and 323 K) are presented in Table 1.…”
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.
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