María Dolores Saquete

Procedure for checking and fitting experimental liquid-liquid equilibrium data

An objective method was developed to check and fit liquid-liquid equilibrium data obtained experimentally. The analytical concentrations are changed slightly within the interval given by the uncertainties of the determinations in order to satisfy the material balances. The method consists of a minimisation with constraints of a proposed objective function.

Liquid–liquid–solid equilibria for ternary systems water + lithium chloride + pentanols

The authors wish to thank the Ministerio de Ciencia y Tecnologia (Spain) for the financial aid with of Project BQU2000-0212.

Liquid-liquid-solid equilibria for ternary systems of water + potassium chloride + pentanols

The authors wish to thank the DGICYT (Spain) for the financial aid for the Project PB96-0338. N. Barnes acknowledges a grant from “Agencia Espanola de Cooperacion Internacional”, Programa de Cooperacion Interuniversitaria/AL.E (1999).

The influence of temperature on the liquid-liquid-solid equilibrium of the ternary system water-potassium chloride-2-propanol

Abstract The lowest temperature at which waterKCl2-propanol mixtures cannot be split has been determined as 25.3°C. Seven diagrams of liquid-liquid-solid equilibria for the ternary system waterpotassium chloride-2-propanol around this temperature have been measured and the transition between their two different shapes has been studied.

Unusual S-shaped binodal curves of the systems water + lithium chloride + 1-butanol or 2-butanol or 2-methyl- 1-propanol

Abstract Solid–liquid–liquid equilibrium data of the ternary systems water+LiCl+2-butanol, water+LiCl+2-methyl-1-propanol (i-butanol) and water+LiCl+1-butanol have been experimentally determined at 25°C. The equilibrium diagrams determined show differences between the systems. In the system with 1-butanol, the solid phase of the liquid–liquid–solid region is monohydrated salt. However, in the systems with 2-butanol and 2-methyl-1-propanol it is anhydrous salt. With respect to the liquid+liquid zone, the three diagrams are very similar with an unusual S-shaped solubility curve in the organic branch that can be explained depending on whether the organic solvent takes part in the solvation of ions. The more salt, the more numbers of ions solvated by water and organic solvent and the solubility of water and salt in the organic phase increase notably producing the unusual S-shaped solubility curve.