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Article

Distribution of N-Methylimidazole in Ionic Liquids/Organic Solvents Systems

by
Milen G. Bogdanov
* and
Ivan Svinyarov
Faculty of Chemistry and Pharmacy, Sofia University St.Kl. Ohridski, 1 J. Bourchierblvd., 1164 Sofia, Bulgaria
*
Author to whom correspondence should be addressed.
Processes 2017, 5(4), 52; https://doi.org/10.3390/pr5040052
Submission received: 26 August 2017 / Revised: 20 September 2017 / Accepted: 20 September 2017 / Published: 22 September 2017
Browse Figures
Versions Notes

Abstract

:
The partition coefficients, Kmim, of N-methylimidazole (mim) in two-component systems composed of ionic liquid (IL) and a series of organic solvents immiscible with ILs (butyl acetate, ethyl acetate, tert-butyl methyl ether, diethyl ether and cyclohexane) were determined by a shake-flask method. The influence of different factors such as temperature, solvent polarity, mim concentration, and water content on Kmim by using 1-butyl-3-methylimidazolium chloride {[C4C1im]Cl} as a model compound was comprehensively studied. The calculated thermodynamic functions of transfer (∆trG0, ∆trH0, ∆trS0) showed that the mim migration (IL→organic phase) is a thermodynamically unfavorable and enthalpy-determined process in the temperature range of 298.15 to 328.15K; however, the results suggested that mim partition toward the organic phase can be enhanced by the rational manipulation of the extraction conditions. Experiments conducted with other 1-alkyl-3-methylimidazolim chlorides (CnC1im]Cl (n = 6, 8, 10) revealed that mim possesses similar behavior and can be successfully washed out from the ILs by extraction with organic solvents. The results obtained in this study give some clues toward the choice of an appropriate solvent and conditions to be employed for the purification of halide-based ILs by means of a liquid-liquid extraction.

1. Introduction

The interest in ionic liquids (ILs) has been continuously growing in the last two decades due to their unique properties and high potential as “green” alternatives to conventional harmful organic solvents [1,2,3,4,5,6]. Among others, a very special property of these “designers’ solvents” is that they can be tailored to fulfill certain requirements by simple variation of the ions. In order to address this issue, many researchers focused their efforts on understanding the behavior of ILs at a molecular level and on establishing structure-properties relationships that allow for the rational design of ILs for specific applications [7,8,9,10,11,12]. It is noteworthy that the ILs’ properties are strongly dependent on their purity [12,13,14]; therefore, the proper purification of ILs is a factor of immense importance, which allows consistent results to be obtained by different research groups. It is well established that the purification of ILs is more difficult than that for common volatile organic solvents, and that the success in this process is dependent on the attention devoted to each aspect of their production, including the starting materials’ purity, reaction conditions, post-treatment of the reaction mixtures, etc. The approach most applied for the synthesis of ILs is based on the quaternization reaction between appropriate N-, S-, or P-containing compounds and haloalkanes (mainly chlorides and bromides) followed by metathesis reaction in order for the halide anion to be further exchanged [15]. In this way, the production of halide-based ILs of high purity is a precondition for purer ILs to be obtained at the end of the reaction scheme. The quaternization step can be carried out both under solvent-free conditions or in the presence of appropriate solvents [15,16,17,18,19,20]. Usually, this first step is conducted at temperatures up to 80 °C, since reverse or side reactions that contribute negatively to the quality of the target IL take place at higher temperatures [18]. Some authors also suggest the above reactions to be conducted at a lower temperature in order to avoid the formation of colored impurities [20]. Unfortunately, this approach results in a limited extent of transformation and prolonged reaction times due to the constant increase of the reaction medium viscosity upon IL formation and reduced reactivity at low temperatures. Regardless of the chosen way of synthesis, the resulted halide-based ILs have to be properly purified. The main ‘‘contaminants” at that stage are the corresponding residual organic base and haloalkane [21,22], and their removal is typically accomplished by multiple liquid-liquid extractions with an organic solvent, followed by prolonged heating of the product under reduced pressure.It is noteworthy that, depending on the boiling points of the residuals and their affinity toward the IL, the entire procedure might require a repetitive performance, thus prolonging the time and increasing the consumption of organic solvents, particularly when one works on a multi-gram scale. Considering the short chain haloalkanes, they are highly volatile and it is unlikely that they will remain in the final IL sample after heating under reduced pressure. In contrast, alkylamines used for the synthesis, particularly N-methylimidazole, tend to have high boiling points and thus are not as easily removed in vacuo; hence, these are better removed by repetitive washing of the IL with organic solvents.
The partition coefficient of a species between two immiscible liquid phases can be considered as an important physicochemical parameter from an engineering perspective, since it can be useful in the recovery of compounds by liquid-liquid extraction [23,24,25,26,27,28,29,30,31]. In our present study [32], we introduced an improved apparatus for continuous liquid-liquid extraction to be used as a tool for the purification of halide-based ionic liquids after the quaternization step. The apparatus employs the heat of the evaporating solvent to heat up the extraction chamber, thus allowing for the process to be conducted at elevated temperatures. The purification carried out with this tool proved successful in the removal of impurities such as residual starting compounds under mild conditions. It was also shown to give ILs of high purity in a shorter time and with significantly reduced consumption of organic solvent as compared with the common procedure [32]. By using this liquid-liquid extraction approach, the following purification step consisting of prolonged heating under deep vacuum can be considerably shortened, because of the lower boiling point and the affinity of the nonpolar organic solvents to the IL [33] in comparison to that of the N-methylimidazole or some of the commonly used haloalkanes in the quaternization reaction. In continuation of this study, herein we present a more in-depth investigation on the distribution of N-methylimidazole (mim) in biphasic systems composed of ILs and IL-immiscible organic solvents. The influence of different factors such as temperature, solvent type and polarity, mim concentration, and water content on the partition coefficients, Kmim, by using 1-butyl-3-methylimidazolium chloride {[C4C1im]Cl} as a model compound was comprehensively studied. Thermodynamic functions of transfer (standard Gibbs energy (∆trG0), standard enthalpy (∆trH0), and standard entropy (∆trS0)) were calculated and used for a rational discussion of the mim migration from the IL phase to the organic phase. Additional preliminary data for other 1-alkyl-3-methylimidazolim chlorides (CnC1im]Cl (n = 6, 8, 10) were also reported. The results obtained in this study give some hints toward the choice of an appropriate solvent and conditions to be employed for the purification of halide-based ILs by means of a liquid-liquid extraction.

2. Materials and Methods

All organic chemicals used in this study were purchased from Sigma-Aldrich (FOT, Bulgaria) and were of analytical grade. Selected properties of materials, including solvents and ILs, are listed in Table 1. The ILs studied were 1-alkyl-3-methylimidazolium chlorides, [CnC1im]Cl (n = 4, 6, 8, 10), and were synthesized, purified, and characterized by the authors as described elsewhere [18]. Their structure and purity were unequivocally proven by 1H- and 13C-NMR spectroscopy [34]. All ILs were dried under reduced pressure and stored under inert atmosphere. N-Methylimidazole content was analyzed by means of HPLC.
The experiments for measuring of partition coefficients of N-methylimidazole in the IL/solvent systems were performed in graduated microtubes (2 mL). The dried ILs were contaminated with a known amount of mim and were put in contact with the corresponding solvents in a volume ratio of 1:1. The shaking time was set to 5 min, since it was found that prolonged shaking (up to 2 h) gave similar equilibrium results. The mixtures were allowed to separate for 3 h at the temperature studied, then centrifuged for better phase separation, and aliquots from the two phases were subjected to analysis. All experiments were performed in duplicate, with a variation in results of less than 5%. The corresponding partition coefficients, Kmim, and thermodynamic parameters of the transfer IL→organic phase (∆trG0, ∆trH0, ∆trS0) were calculated according to Equations (1)–(4):
Kmim = Corg/CIL,
∆trG0 = −RT ln (Kmim)
∆trG0 = ∆trH0−T∆trS0
ln (Kmim) = −∆trH0/R× 1/T + ∆trS0/R
where Corg and CIL are the concentrations of mim in the organic phase and the IL phase, respectively, R is the universal gas constant (8.314 J mol−1 K−1), and T is the temperature (K).

3. Results

At the very beginning of this work, we studied the temperature dependence of mim partitioning in IL/organic solvent systems within the temperature range of 298.15–328.15 K (see Figure 1a). The solvents used for this experiments were butyl acetate, ethyl acetate, tert-butyl methyl ether, and cyclohexane, and [C4C1im]Cl was the model IL. On the basis of the Kmim obtained and by using Equations (2)–(4), the thermodynamic parameters of transfer (standard Gibbs energy (∆trG0), standard enthalpy (∆trH0), and standard entropy (∆trS0)) were calculated and are summarized in Table 2.
A short overview of the results presented in Table 2 reveals a number of notable regularities. First, the calculated Kmim < 1 for all systems show the preferential partition of mim in the IL-phase. It was also found that Kmim measured at same temperature, e.g., 298 K, strongly depends on the organic solvent used, following the order BuOAc (0.860) > EtOAc (0.586) > MTBE (0.117) > cyclohexane (0.018), and that this order stays unchanged regardless of the temperature applied. Regarding the temperature effect, Kmim were found to increase for all systems with the increase of temperature. It is noteworthy that this phenomenon is most pronounced for the less polar cyclohexane (Kmim enhancement of 167%) and less pronounced for the solvent of the highest polarity—BuOAc (Kmim enhancement of 12%). The van’t Hoff plots ln (Kmim) vs. 1/T exhibit linearity for all systems (see Figure 1a), which indicates that the standard enthalpy of transfer of mim is temperature-independent [23] in the temperature range studied. The calculated ∆trG0 and ∆trH0 values are positive for all systems; consequently, the partition of mim from the IL-phase to the organic phase is a thermodynamically unfavorable and endothermic structure-breaking process. The positive ∆trH0 is also an indication for stronger interactions between mim and the IL ions, the latter being realized by hydrogen bonding (see Section 4). In addition, ∆trH0 was found to increase with the decrease of the solvent polarity, following the order: BuOAc (1.52) < EtOAc (10.18) < MTBE (17.18) < cyclohexane (27.39). The latter suggests that the energy required for the mim migration toward the organic phase can be minimized by employing a solvent of higher polarity. The transfer entropy ∆trS0 is also positive in all cases. This indicates the higher mobility of the species in the transfer process, as well as the positive influence of that term on ∆trG0. Similar to the enthalpy, ∆trS0 has a reverse relationship with the solvent polarity, as indicated by the following order: BuOAc (3.83) < EtOAc (29.69) < MTBE (39.59) < cyclohexane (58.41), and this can be attributed to the decreased number of interactions in the solvents of lower polarity. The contribution of different factors to the partition of mim can be assessed by means of a graphical approach [41]. The region of the diagram presented as Figure 1b, where ∆trH0 > 0; T∆trS0 > 0; ∆trH0 > T∆trS0, i.e., sector VII, corresponds to the enthalpy-determined processes, and sector VIII, where ∆trH0 > 0; T∆trS0 > 0; ∆trH0 < T∆trS0, corresponds to the entropy-determined process. Isoenergetic curves of the ∆trG0 function are marked as dotted lines in this figure. As can be seen, all data points are situated in the same sector, sector VII, which means that the transfer processes of mim for the organic solvents obey same mechanism, which is enthalpy-determined. The minimum energy difference for the process is observed for BuOAc (∆trG0 = 0.38 kJ mol−1), and the maximum for cyclohexane (∆trG0 9.97 kJ mol−1), while ∆trG0 is additionally lowered by the increase of the temperature. To sum up, the removal of residual N-methylimidazole from [C4C1im]Cl by means of a liquid-liquid extraction is an entropy-driven, structure-breaking, not spontaneous process, which can be facilitated by employing solvents of high polarity and applying elevated temperatures.
The concentration of a solute recovered from a solvent by means of a liquid-liquid extraction decreases in a continuous manner after each extractive cycle. In order to investigate the influence of this factor on the partition of mim, we contaminated IL samples with different amounts of mim and performed extractions with organic solvents. Because these experiments were conducted at ambient conditions, diethyl ether (Et2O) was also included as an IL-immiscible solvent. The results obtained are presented in Figure 2a. As it can be seen, the extraction ability of the solvents is consistent with the results presented above, i.e., the mim partition into the organic phase is facilitated by an organic solvent with higher polarity according to the following order: BuOAc < EtOAc < MTBE ≈ Et2O < cyclohexane (for the sake of clarity, the latter was omitted from Figure 2a, Kmim = 0.018). Further, the solvents can be divided on two categories. The first one consists of esters—BuOAc and EtOAc, for which Kmim increases with the increase of mim concentration, and the second one—ethers and cyclohexane, for which Kmim is concentration-independent. A rough extrapolation of these results suggests that the polar solvents are more efficient at higher mim concentrations, whereas all organic solvents can be equally used for the removal of mim in low concentrations.
Another factor that might change the ILs’ properties is the presence of water [13,14]. To study the influence of the water content in ILs, we measured the partition of mim by using BuOAc, EtOAc, and MTBE as organic solvents. As can be seen from Figure 2b, Kmim decreases with the increase of water concentration for the three solvents used, and this phenomenon has a reverse relationship to the extraction ability of the latter. The observed effect is most pronounced for the BuOAc (80% reduction), best performed under “dry conditions”, and less pronounced for MTBE (45% reduction) upon increasing the water content from 0 to 20% (wt/wt). It is also noteworthy that the presence of even 5% of water changes the order of the solvents’ ability to extract mim; consequently, the water content can be considered as a factor of an immense importance that controls the mim partition in a significant manner, and that the use of a dry solvent is preferred in the purification of ILs.

4. Discussion

The results presented above showed that the transfer of mim from the IL to the organic phase is not a spontaneous process, and that is dependent on factors such as solvent type and polarity, temperature, mim concentration, and water content. In order for these results to be rationalized, a short description of the ILs’ structure both in the pure state and in the presence of other molecules should be given.
Pure ILs can be considered as self-assembly amphiphiles, which form H-bonded-polymeric networks as a general structural pattern for both solid and liquid phases [42,43]. The introduction of other species into pure ILs, however, disrupts this H-bond network [44] and generates different secondary nano-structures with polar and non-polar domains, which in turn affects ILs’ properties such as polarity, viscosity, reactivity, and solvating ability, to name just a few [2,12,13,14,18,37]. In case of dilution with solvents, depending on the solvent polarity and H-bonding ability, supramolecular aggregates, triple ions, contact ion pairs, or solvent-separated ions can be formed [42]. Regarding 1-alkyl-3-methyimidazolium-based ILs, there are three main binding sites in the imidazolium ion capable of participating as hydrogen bond donors, and these are at positions H–(4C), H–(5C), and H–(2C). Indeed, it was shown that the IL anion prefers to bind to the proton at the (2C) position, the latter being the most acidic amongst the others [45,46,47], and that the introduction of a solute/solvent to the IL leads to a competition for the active sites of both ions, the outcome of which strongly depends on the differences between the acidic/basic properties of the participants [44,45,46,47,48,49,50,51,52]. In other words, solutes with pronounced acidic properties will compete with the imidazolium ion to form H-bonds with Cl−, whereas those with basic properties will compete with the chloride anion for the acidic sites of the cation. A short overview of the data presented in Table 1 shows that the organic solvents used in this study have zero acidity and that their basicity is almost equal to each other (an exception is cyclohexane); consequently, the second scenario will take place when an IL interacts with them. Considering the lower basicity of the solvents in comparison to that of the ILs, and the fact that this property of ILs is dominated by the anion [37], it can be assumed that Cl− will win the competition for the position at H–(2C), thus pushing solvent molecules to interact with H–(4C) and H–(5C). In this way, the presence of hydrogen-bonded species “solvent-IL” in the IL-phase can be suggested. In contrast to that, the existence of such complexes in the organic phase is not expected due to the negligible solubility of ILs in these solvents [51].
Having this simplified description of the systems under study, our next goal is to explain the results for the mim partition. It is evident from Table 2 that Kmim is always lower than unity, which suggests that “mim-IL” interactions are rather preferable to ”mim-solvent” and “solvent-IL” interactions. This suggestion can be supported by the fact that mim possesses pronounced basicity and weak acidity. By a comparison of the solvent basicity (SB) and solvent acidity (SA) values of all participants in the competition (see Table 1), it can be concluded that mim will compete both with Cl− and solvent molecules for the acidic binding sites of the imidazolium ion. Simultaneously, mim will offer alternative H-binding centers to the Cl−, which will additionally strengthen the mim-IL interactions and will hinder its transfer to the organic phase. Based on the above reasoning, it can be concluded that the organic solvent, which can extract mim from the IL phase in a more efficient manner, is able to substitute it from the H-bond embedded mim-IL network. Considering the basic properties of the compounds under study, however, it can be seen that this is not the case here, and that another approach based on different types of interactions that facilitate the formation of “mim-solvent” complexes has to be given in order for the apparent partition coefficients to be explained. It was observed that Kmim strongly depends on the solvent polarity, decreasing in the following order: BuOAc > EtOAc > MTBE ≈ Et2O > cyclohexane, regardless of the temperature applied. Interestingly, we obtained a very good linear correlation between the averaged Kmim values and the solvents’ polarities expressed in the Reichardt’s ETN scale ((ln (Kmim) = a×ETN + b, R2 = 0.994). On the one hand, this relationship gives some clues toward the mechanism of extraction, and on the other, it can be used as a tool for solvent selection in the liquid-liquid extraction of mim, i.e., IL-immiscible solvents, possessing higher ETN value are expected to be more efficient in this process. In 2009, Catalan showed [38] that the Reichardt polarity parameter [40] is composed of several components, including solvent dipolarity (SdP), acidity (SA), and basicity (SB), and that its value is mainly determined by the SA term, followed by SdP and SB, with contributing factors of 2:1:0.3, respectively. Based on the above reasoning, and taking into account the zero acidity and equal basicity of the solvents used in this study, we can conclude that the solvent dipolarity can be regarded as the main factor that governs the mim transfer from the IL phase to the organic solvent. However, as it can be seen from Table 1, BuOAc has a lower SdP value than that of EtOAc, but performs the best in the extraction of mim in the absence of water. This can be attributed to the increased hydrophobicity of the former due to the presence of two additional methylene groups in its structure. Consequently, the solvent hydrophobicity, which seems to be reflected by the ETN polarity parameter, also plays an important role in the extraction of mim. In support of the conclusions made above is the data obtained for the thermodynamic parameters of transfer (see Table 2), which reveals that the enthalpy ∆trH0 increases with the decrease of the solvent polarity, following the order:BuOAc (1.52) < EtOAc (10.18) < MTBE (17.18) < cyclohexane (27.39). Furthermore, despite the fact that it is entropy favored (∆trS0 > 0), it was found that the process of mim transfer toward the organic phase is not spontaneous (∆trG0 > 0), but is endothermic (∆trH0 > 0) and enthalpy-determined (∆trH0 > T∆trS0) for all systems studied (see Figure 1b). This data can also be employed to clarify what the driving force of the process is by analysis of the signs of the thermodynamic parameters. Usually, ΔH > 0 and ΔS > 0 imply a hydrophobic association; ΔH < 0 and ΔS < 0 reflect van der Waals forces or hydrogen bond formation; and ΔH < 0 and ΔS > 0 suggest an electrostatic force. Considering this data, it can be seen that the transfer of mim is entropy-driven with a main driving force of hydrophobic interactions between the organic solvent and mim, which is in line with the above discussion about the H-bonding ability of mim and its influence on the partition. Moreover, if one calculates the thermodynamic parameters of mim transfer for the reverse process, i.e., solvent → IL, one can see that both ∆trH0 and ∆trS0 are negative, which suggests a process that is governed by the formation of hydrogen bonds.
The above discussion is also consistent with the ILs’ behavior at different temperatures. It was put forward by Skarmoutsos et al. [53] that the H-bonds network in pure ILs is continuously reorganizing, and that the number and lifetime of the H-bonds between the ions of ILs, particularly for [C4C1im]Cl, are strongly dependent on the temperature. The authors showed that in a hot IL, H-bonds are mainly formed between two ions and are rapidly breaking and reforming, whereas in a cold IL, a higher proportion of bifurcated state H-bonds occurs, with a dramatic extension of the lifetime of individual H-bonds [53]. In this way, the observed increase of Kmim with the increase of temperature seen in this study can be attributed to the disruption of the H-bond-embedded network at high temperatures, which allows the hydrophobic interactions between mim and the solvent to take place in a more efficient manner, hence facilitating the transfer of the former to the organic phase. In contrast to that, the addition of a polar species with pronounced acidic properties, e.g., water (see Table 1), will increase the number of centers capable of participating as H-bond donors in the IL-phase. It was shown [46,47] that the water molecules preferably bind to the Cl− anion, which lowers it basicity and allows mim to form stronger H-bonds with the IL cation by changing its position from the less acidic H–(4C) and H–(5C) to the more acidic H–(2C) at low water concentrations, and to interact with water itself at higher concentrations. This stronger structure reduces the ability of the solvent molecules to efficiently solvate mim, thus lowering the respective Kmim (Figure 2b).
Changing the alkyl chain length in the ILs ions can be considered a direct way to tune their hydrophobic properties [54,55]. 1-Alkyl-3-methylimidazolium chlorides with alkyl chain lengths varying from 4 to 10 were chosen to conduct a preliminary study on the influence of that factor on the mim partition in IL/organic solvents biphasic systems. The corresponding experimental data is presented in Figure 3. It is noteworthy that the solubility of the organic solvents in ILs increases with the increase of the alkyl chain length, which causes deviation in the phase ratio solvent to IL, e.g., from 1:1 in the case of [C4C1im]Cl to 0.4:1.6 in the case of [C10C1im]Cl when BuOAc or EtOAc were used as organic solvents. Furthermore, MTBE was completely soluble in [C10C1im]Cl at a mixing ratio of 1:1. Therefore, for comparison purposes, the results are presented and discussed in terms of extraction efficiency (EE%), the latter being defined as: EE% = [Kmim/(1 +1/RV)] × 100, thus taking into account the apparent phase ratio RV.
As it can be seen from Figure 3, the above observed order of extraction ability of the organic solvents stays intact (BuOAc > EtOAc > MTBE) regardless of the IL. Further, EE% decreases upon increasing the number of carbon atoms in the alkyl side chain, and this change is again more pronounced for the better performed solvents (BuOAc and EtOAc). The latter phenomenon can be attributed to the increasing hydrophobicity of ILs upon the inclusion of additional methylene groups [54,55], which enhance the hydrophobic interactions in the IL phase and hinder the unopposed transfer of mim for the organic phase. On the other hand, the increased solubility of the solvent into ILs also can contribute to the apparent reduction of extraction ability. Nevertheless, the results presented here suggest that mim can be successfully washed out from the ILs by extraction with organic solvents such as BuOAc, EtOAc, and MTBE.

5. Conclusions

This article represents a comprehensive study on the influence of different factors such as solvent type and polarity, temperature, solute concentration, and water content on the partition of N-methylimidazole in biphasic systems of ILs and organic solvents (butyl acetate, ethyl acetate, tert-butyl methyl ether, diethyl ether, and cyclohexane). By using the thermodynamic functions of transfer (∆trG0, ∆trH0, ∆trS0), we showed that the mim transfer (IL→organic phase) is a thermodynamically unfavorable, structure-breaking process, and that mim is predominantly partitioned into the IL regardless of the conditions applied. However, mim transfer toward the organic phase can be facilitated by employing solvents of higher polarity and by the elevation of the temperature. The presence of water in the system has a negative effect on the process of transfer, the latter suggesting that the use of dry solvents is preferred in the purification of ILs. The results obtained in the present study contribute to the understanding of ILs’ behavior at a molecular level and give some clues toward the rational selection of solvents and conditions to be employed for the purification of halide-based ILs by means of a liquid-liquid extraction, which is a precondition for purer ILs to be obtained after metathesis reaction. This can be of great importance from an applied standpoint, since a considerable amount of time and energy could be economized.

Acknowledgments

The financial support of the National Science Fund of Bulgaria at the Ministry of Education and Science (project DFNI T 02/23) is greatly acknowledged. The authors also would like to acknowledge the contribution of the COST Action CM1206-Exchange on Ionic Liquids.

Author Contributions

I.S. and M.B. contributed equally to this work and have approved the final manuscript.

Conflicts of Interest

The authors declare no conflict of interest.

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Processes 05 00052 g001 550
Figure 1. (a) van’t Hoff plots of ln (Kmim) vs. 1/T for mim in a systems [C4C1im]Cl/organic solvent; (b) Relationship between the enthalpic and entropic terms of transfer functions from [C4C1im]Cl to solvent for N-methylimidazole at 298.15 K. The isoenergetic curves of ∆trG0 function are marked by dotted lines.
Figure 1. (a) van’t Hoff plots of ln (Kmim) vs. 1/T for mim in a systems [C4C1im]Cl/organic solvent; (b) Relationship between the enthalpic and entropic terms of transfer functions from [C4C1im]Cl to solvent for N-methylimidazole at 298.15 K. The isoenergetic curves of ∆trG0 function are marked by dotted lines.
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Figure 2. (a) Effect of mim concentration and (b) water content on the partition of mim in a [C4C1im]Cl/organic solventsystem.
Figure 2. (a) Effect of mim concentration and (b) water content on the partition of mim in a [C4C1im]Cl/organic solventsystem.
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Figure 3. Effect of alkyl side chain in the imidazolium ion on mim partition in different IL/solvent systems.
Figure 3. Effect of alkyl side chain in the imidazolium ion on mim partition in different IL/solvent systems.
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Table
Table 1. Polarity (ETN), dipolarity (SdP), acidity (SA), and basicity (SB) of solvents used in this study 1.
Table 1. Polarity (ETN), dipolarity (SdP), acidity (SA), and basicity (SB) of solvents used in this study 1.
Materials (Abbreviation)ETNSdPSASB
Water1.0000.9971.0620.025
N-methylimidazole (mim)n.a. 20.9590.0690.658
butyl acetate (BuOAc)0.2410.53500.525
ethyl acetate (EtOAc)0.2280.60300.542
tert-butyl methyl ether (MTBE)0.1240.42200.567
diethyl ether (Et2O)0.1170.38500.562
Cyclohexane0.006000.073
[C4C1im]Cl0.6141.1720.1670.869
[C6C1im]Cl0.5621.1390.1590.932
[C8C1im]Cl0.5491.0960.1591.001
[C10C1im]Cln.a.21.1150.1590.932
1 Data was extracted from References [35,36,37,38,39,40]; 2 n.a. refers to not available.
Table
Table 2. Partition coefficients and thermodynamics functions of mim transfer IL → organic solvent.
Table 2. Partition coefficients and thermodynamics functions of mim transfer IL → organic solvent.
TemperatureKKmimln(Kmim)∆trG0kJ mol−1∆trH0kJ mol−1∆trS0J mol−1T∆trS0kJ mol−1ζHtr 1%ζTStr 2%
Butyl Acetate
298.150.860−0.150.381.523.831.145743
308.150.900−0.110.34
318.150.840−0.170.30
328.150.940−0.060.26
Correlationequation: ln (Kmim) = 0.46 − 183× 1/T; R2 = 0.243
Ethyl Acetate
298.150.586−0.531.3210.1829.698.855347
308.150.662−0.411.03
318.150.780−0.250.73
328.150.841−0.170.43
Correlationequation: ln (Kmim) = 3.75 − 1224 × 1/T; R2 = 0.99
tert-Butyl Methyl Ether
298.150.117−2.155.3817.1839.5911.805941
308.150.138−1.984.98
318.150.177−1.734.59
328.150.217−1.534.19
Correlationequation: ln (Kmim) = 4.76 − 2067 × 1/T; R2 = 0.99
Cyclohexane
298.150.018−4.029.9727.3958.4117.426139
308.150.025−3.719.39
318.150.038−3.268.81
328.150.048−3.058.22
Correlationequation: ln (Kmim) = 7.02 − 3295 × 1/T; R2 = 0.99
Parameters ζHtr and ζStr were used to describe the relative fraction of enthalpy and entropy of transfer: 1 %ζHtr = (∆trH0/(∆trH0 + T·∆trS0))·100; 2 %ζStr = (∆trS0/(∆trH0 + T∆trS0))·100.

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Bogdanov, M.G.; Svinyarov, I. Distribution of N-Methylimidazole in Ionic Liquids/Organic Solvents Systems. Processes 2017, 5, 52. https://doi.org/10.3390/pr5040052

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Bogdanov MG, Svinyarov I. Distribution of N-Methylimidazole in Ionic Liquids/Organic Solvents Systems. Processes. 2017; 5(4):52. https://doi.org/10.3390/pr5040052

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Bogdanov, Milen G., and Ivan Svinyarov. 2017. "Distribution of N-Methylimidazole in Ionic Liquids/Organic Solvents Systems" Processes 5, no. 4: 52. https://doi.org/10.3390/pr5040052

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