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Quantification of the Liquid Window of Deep Eutectic Solvents† Cite This: Chem

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Quantification of the Liquid Window of Deep Eutectic Solvents† Cite This: Chem ChemComm View Article Online COMMUNICATION View Journal | View Issue Quantification of the liquid window of deep eutectic solvents† Cite this: Chem. Commun., 2018, 54, 13351 Laura J. B. M. Kollau, a Mark Vis, *a Adriaan van den Bruinhorst, a Received 17th July 2018, A. Catarina C. Esteves a and Remco Tuinier ab Accepted 19th October 2018 DOI: 10.1039/c8cc05815f rsc.li/chemcomm Deep eutectic solvents (DESs) have been considered as a new class the melting point of the solute.5–7 A solute in an ideal solution of green solvents with tunable physical properties based on the lowers the chemical potential of the solvent, resulting in a selective combination of their individual components. As the liquid decrease of the melting point of that mixture. Such melting window of a DES identifies the range of feasible applications, it is point depressions are often described using phase diagrams. Creative Commons Attribution-NonCommercial 3.0 Unported Licence. essential to determine, quantify, and predict their phase behavior. Examples of systems, which are accurately described by ideal Phase diagrams were measured for systems consisting of tetra- solution theory for all compositions, are binary mixtures of pentylammonium bromide and erythritol or succinic acid. Regular bibenzyl–biphenyl,8 carbon tetrachloride–benzene9 as well as solution theory is applied to quantitatively describe the liquid certain fatty acid mixtures.10 At the solid–liquid (S–L) binodal, window of DESs. The succinic acid mixture shows a larger deviation equilibrium thermodynamics dictates that the chemical potential s from ideal behavior, caused by the stronger hydrogen bond forming mi of component i in the solid phase equals the chemical s l acid groups. The interaction parameter between the two DES com- potential in the liquid phase, mi = mi. It follows that the chemical l ponents in regular solution theory could be determined directly from potential difference Dmi(xi)=mi(xi) À mi*ofcomponenti in the l the eutectic temperature of the mixture and this enables quantifica- liquid mixture (mi) and in the pure liquid (mi*) is related to the This article is licensed under a tion of the degree of non-ideality of DESs. melting enthalpy DHi, melting point Ti* of the individual component, and melting point of the mixture T: DESs have gained interest as a new class of solvents due to their Dm ðÞx DH 1 1 compliance with green chemistry principles,1 such as atom i i i : ¼ À Ã (1) Open Access Article. Published on 12 November 2018. Downloaded 11/27/2018 12:10:23 PM. RT R T T economy,2 and safer solvents and chemicals.3,4 Being considered i as designer solvents, hypothetically all the physical properties of For simplicity, it is assumed here that the enthalpy of fusion is DESs can be tailored by choosing the right combination of independent of temperature. In the case of an ideal solution, components. However, the fundamentals of the stable liquids Dmi depends on mole fraction xi according to: of these systems have yet gained limited attention, while for the Dmi applications of DESs, these are of great importance. Quantifying ¼ ln xi: (2) the non-ideality of DESs could provide guidelines for designing RT the desired properties based on the features of the individual Here we account for non-ideality through enthalpic interactions components. Although a wide range of liquid properties of DESs by using regular solution (RS) theory.11 For a binary mixture have been investigated by now, phase behavior studies reported this theory provides the following expression for Dmi: in the literature remain scarce.28 Binary phase diagrams enable Dm the mapping of the stable liquid window, which identifies where i ¼ ln x þ wðÞ1 À x 2: (3) RT i i applications could be feasible. For an ideal mixture at a given temperature, the solubility of The effective interaction parameter w quantifies the binary any solute in a solvent depends on the enthalpy of fusion and interactions. In Fig. 1 the predicted trends of the eutectic phase behavior a Laboratory of Physical Chemistry, Department of Chemical Engineering and are sketched. In the top panel, the influence of the different Chemistry & Institute for Complex Molecular Systems, Eindhoven University of enthalpies of fusion for the two components A and B is illus- Technology, The Netherlands. E-mail: [email protected] b Van’t Hoff Laboratory for Physical and Colloid Chemistry, Debye Institute for trated, while the middle panel depicts the effect of the melting Nanomaterials Science, Utrecht University, The Netherlands point Ti* of the individual components. The lower panel high- † Electronic supplementary information (ESI) available. See DOI: 10.1039/c8cc05815f lights the effect of the interaction parameter w on the phase This journal is © The Royal Society of Chemistry 2018 Chem. Commun., 2018, 54, 13351--13354 | 13351 View Article Online Communication ChemComm Fig. 2 Choline chloride–urea mixtures at 303 K. (Mole fraction urea from left to right: 0, 0.33, 0.5, 0.66, and 1). straightforwardly. From Fig. 3a, it follows that eqn (3) using w = 0 can accurately describe the eutectic composition, tempera- ture, and S–L equilibrium for the biphenyl–bibenzyl system. For the choline chloride–urea system, ideal behavior clearly Fig. 1 Schematic representation of the effect of (top) the enthalpy of fusion of the individual components, (middle) the melting point of the individual does not provide a proper description of the phase boundaries, Creative Commons Attribution-NonCommercial 3.0 Unported Licence. components, and (bottom) the attractive (w o 0) or repulsive (w 4 0) as illustrated by the comparison of the theoretical prediction interactions between the individual components on the phase behavior of and the experimental data shown in Fig. 3b. This deviation can binary mixtures. be explained by the strong effective attractions between choline chloride and urea. It should be noted that, although this system is the first reported DES, the choline chloride–urea system is behavior. The position where the two binodal curves meet is the especially complicated to describe and map because choline eutectic point with the corresponding eutectic temperature chloride decomposes21 before melting, requiring estimates for (Teut) and eutectic composition (xeut). From eqn (1), it follows T * and DH, and urea gradually evolves into ammonia near its that for an ideal mixture (w = 0), the melting point depression melting point.23 This article is licensed under a depends solely on the thermodynamic properties of the indi- The purpose of developing the DESs considered for this vidual components (melting point and enthalpy of fusion) and study was to illustrate the non-ideal behavior of well-defined 5 on the composition xi. DESs and to validate the RS theory to describe the DES phase At the beginning of this century, Abbott et al.12 reported that behavior. We chose to develop new DESs rather than using Open Access Article. Published on 12 November 2018. Downloaded 11/27/2018 12:10:23 PM. mixtures of urea and choline chloride exhibit a rather specta- previously published data to prevent the above mentioned cular melting point depression. Such a significant temperature challenges and to ensure that they possess specific require- drop can be achieved only, as shown in Fig. 1, by strong ments. Firstly, the DES components should not react with attractive interactions between the components of a eutectic themselves or each other, e.g., combinations of carboxylic groups mixture. The work of Abbott et al., and subsequent attention to and alcohols which can react to esters were avoided.24 Secondly, similar mixtures, gave rise to the development of the new DES the components should have well-defined melting points and field that focuses on the properties and applications of binary enthalpies of fusion, rather than decomposing upon heating. eutectic mixtures in the stable binary liquid window of DESs.13,14 Finally, the components should be able to crystallize sufficiently Fig. 2 depicts a few examples of choline chloride and urea when cooled below the eutectic temperature avoiding super- mixtures with different binary compositions at 303 K. cooling, in order to obtain reproducible data. All these require- Fig. 3 shows binary phase diagrams, in which the predicted ments are met with tetrapentylammonium bromide (TPABr), ideal (w = 0) melting point depressions calculated using eqn (1) erythritol, and succinic acid, and therefore they can act as DES and (3) are compared to the experimentally determined melting constituents for the systems TPABr–erythritol and TPABr–succinic points of the two literature examples of eutectic systems. The acid. The large difference in the melting points of succinic acid systems shown in Fig. 3 are biphenyl–bibenzyl,8 with quasi-ideal and erythritol also enables us to validate the predicted effects of interactions between the components, and choline chloride– asymmetry in Ti*. urea mixtures,15 with non-ideal interactions. Table 1 gives an The melting points (S–L equilibrium curve) were measured overview of various thermodynamic properties of the con- using a capillary melting point apparatus. The DES compositions sidered components. A characteristic that is often assigned to used were prepared inside a glove-box under a dry nitrogen DESs is the ability to form hydrogen bonds between the two atmosphere; the moisture levels were typically 1.5 ppm. The components,12–20 of which the strength cannot be quantified first partial melting of the mixture was considered as the 13352 | Chem. Commun., 2018, 54, 13351--13354 This journal is © The Royal Society of Chemistry 2018 View Article Online ChemComm Communication Fig. 3 Phase diagrams of binary mixtures from (semi-filled circles) experiments in literature8,15 compared to (dashed curves) theoretical predictions for ideal mixtures. Dashed horizontal line: predicted eutectic temperature. Table 1 Melting point Ti* and enthalpy of fusion DHi of the individual accurate with the use of only a single free parameter, the components of the considered binary mixtures shown in Fig.
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