Aqueous phase diagrams containing t-aconitic acid+(1-pentanol or +isobutyl acetate or +methyl isobutyl ketone) at 303.15 K

Phase diagrams of ternary systems, water+ t-aconitic acid (AA)+(1-pentanol (P) or +isobutyl acetate (iBuAc) or +methyl isobutyl ketone (MIK)), were obtained at 303.15±0.05 K. Experimental results show that all aqueous AA systems have one liquid–liquid equilibria region and three solid–liquid equilib...

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Bibliographic Details
Published inFluid phase equilibria Vol. 168; no. 2; pp. 217 - 227
Main Authors Barnes, Norma, Gramajo de Doz, Mónica, Sólimo, Horacio N
Format Journal Article
LanguageEnglish
Published Amsterdam Elsevier B.V 29.02.2000
Elsevier Science
Subjects
Chemical equilibria
Chemistry
Data
Exact sciences and technology
General and physical chemistry
Liquid–liquid equilibria
Phase equilibria
Solid–liquid equilibria
Ternary aqueous t-aconitic acid systems
Ternary aqueous t-aconitic acid systems
Data
Liquid–liquid equilibria
Solid–liquid equilibria
Chemical equilibria
Water
Ternary system
Phase composition
Phase diagram
Solubility
Group contribution method
Liquid solid equilibrium
Acetic acid derivative
Experimental study
Ketone
Correlation method
Propene-1,2,3 tricarboxylic acid
Primary alcohol
Chemical equilibrium
Ester
Carboxylic acid
Trans stereoisomer
Aqueous solution
Phase equilibrium
Liquid liquid equilibrium
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Summary:Phase diagrams of ternary systems, water+ t-aconitic acid (AA)+(1-pentanol (P) or +isobutyl acetate (iBuAc) or +methyl isobutyl ketone (MIK)), were obtained at 303.15±0.05 K. Experimental results show that all aqueous AA systems have one liquid–liquid equilibria region and three solid–liquid equilibria zones, where the solid is the AA. The recovery of this acid from aqueous solutions was evaluated by analyzing its distribution coefficients, selectivities, and distribution curves on a solvent-free basis. Although the experimental distribution coefficients are practically always less than unity for the three systems, the selectivities are higher due to the lower solubility of the non-consolutes, particularly for MIK, which appears as the best solvent among those studied here. The experimental data were also compared with values calculated by the NRTL and UNIQUAC equations for these ternary mixtures.
ISSN:0378-3812
1879-0224
DOI:10.1016/S0378-3812(99)00334-9