Research Article  Open Access
Yuliang Li, Xiaojia Lu, Jing Hao, Changquan Chen, "LiquidLiquid Equilibrium Data for the Ionic Liquid NEthylPyridinium Bromide with Several Sodium Salts and Potassium Salts", Journal of Chemistry, vol. 2013, Article ID 857272, 11 pages, 2013. https://doi.org/10.1155/2013/857272
LiquidLiquid Equilibrium Data for the Ionic Liquid NEthylPyridinium Bromide with Several Sodium Salts and Potassium Salts
Abstract
The liquidliquid equilibrium (LLE) data for systems containing Nethylpyridinium bromide ([EPy]Br), salt (, , , ), and water have been measured experimentally at K and the formations of these four aqueous twophase systems (ATPSs) have been discussed. Also, the effective excluded volume (EEV) values obtained from the binodal models for the four systems were determined and the saltingout abilities of different salts follow the order of . The solubility data were correlated by the Merchuk and other equations while the tieline data by the OthmerTobias, Bancroft, twoparameter, and Setschenowtype equations. The correlation coefficients evidenced that experimental data fitted well to all these equations. These four salts were proved successfully to form ATPSs with Nethylpyridinium bromide, making a significant contribution to the further study of this kind of ATPS.
1. Introduction
Aqueous twophase systems (ATPSs) [1] extraction, an economical and efficient technique for separation, extraction, and purification, have found wide application in comprehensive separation, concentration, and fractionation of biological solutes and particles such as cells and proteins [2, 3] for the past few years. An ATPS is essentially a mixture that exists in two phases and is usually formed by two high polymers, a high polymer and a salt, or a hydrophilic organic solvent and a salt [4]. Compared with traditional organic solvent extractions, ATPSs are more effective and can be carried out under mild processing conditions [5].
In recent years, a new type of ATPS based on ionic liquids (ILs) has been investigated, the ILATPS. The ILs are entirely composed of organic cation and organic or inorganic anion, which hold attention because of their chemical and physical properties such as a good thermal, chemical, and electrochemical stability, negligible volatility, a high ionic conductivity, and tenability [6, 7]. Thus, ILATPSs, combining both the advantages of traditional ATPSs and the aforementioned benefits of ILs, have been successfully used in the separation, concentration, and purification of proteins [8], heavy metal ions [9], and small organic molecules [10]. ILATPSs have also been applied to extract antibiotics, such as penicillin G [11] and roxithromycin [12].
Consequently, further work is necessary for the development, optimization, and scaleup of extraction process using ILATPSs. Recently, an aqueous biphasic system (ABS) containing 1butyl3methylimidazolium tetrafluoroborate ([C_{4}mim]BF_{4}) + saccharides + water [13, 14] has been reported in the literature. In addition, ATPSs composed of [C_{n}mim]X (X = Br and Cl) + salts (KOH, K_{2}HPO_{4}, KH_{2}PO_{4}, K_{2}CO_{3}, K_{3}PO_{4}, K_{3}C_{6}H_{5}O_{7} and sucrose) [13, 15–18] and [Bmim]BF_{4} + salts (Na_{3}PO_{4}, Na_{2}CO_{3}, Na_{2}SO_{4}, Na_{2}SO_{3}, (NH_{4})_{2}SO_{4}, NaH_{2}PO_{4}, NaCl, Na_{3}C_{6}H_{5}O_{7}, Na_{2}C_{4}H_{4}O_{6}, NaC_{2}H_{3}O_{2}, and (NH_{4})_{3}C_{6}H_{5}O_{7}) [19–22] also have been reported. For ATPSs containing pyridiniumbased ionic liquids, there are 4methylNbutyl pyridinium tetrafluoroborate + cyclohexane [23]. Furthermore, Bridges et al. described the phase diagrams for imidazolium, pyridium, and quaternary ammonium and phosphoniumbased chloride salts (all chaotropic salts) salted out by K_{3}PO_{4}, K_{2}HPO_{4}, K_{2}CO_{3}, KOH, and (NH_{4})_{2}SO_{4} (all kosmotropic salts) [24]. Phase diagrams of ATPS composed of Mpy CH_{3}SO_{4} and Na_{2}CO_{3} have also been experimentally ascertained at .15 K [25] and the effects of the cation core such as methylimidazolium, methylpyridinium, methylpyrrolidinium and methylpiperidinium, the length of the alkyl side chain, and the positional isomerism on ATPS formation ability of chloridebased ionic liquids such as [1C_{4}2C_{1}py]Cl, [1C_{4}3C_{1}py]Cl, [1C_{4}4C_{1}py]Cl have been investigated [26].
However, to our knowledge, the experimental work devoted to ILATPSs is far from enough. Compared to the existing imidazoliumbased ionic liquids, pyridinebased ionic liquids provide lower cost, lower vapor pressure, better thermal, and chemical stability and are less polluting. An ATPS formed from an ionic liquid which is water soluble at room temperature, [BPy]BF_{4} (nitrogenbutyl pyridine tetrafluoroborate) and a phaseforming salt (NH_{4})_{2}SO_{4} was studied for the extraction and separation of rutin [27]. The ATPS formed by the [EPy]Br and K_{2}HPO_{4} for extracting and separating chloramphenicol (CAP) in eggs has also been reported [28]. However, studies regarding this type of ILATPSs are insufficient and require further development.
In this work, phase diagrams and liquidliquid equilibrium (LLE) data for the [EPy]Br and four kosmotropic salts (Na_{2}HPO_{4}, K_{2}HPO_{4}, K_{2}SO_{4}, C_{4}O_{6}H_{4}KNa) have been investigated. The solubility curves were fitted to three nonlinear equations, and the tielines were described using the OthmerTobias, Bancroft, and Setschenowtype equations and a twoparameter equation. Moreover, the effective excluded volume (EEV) values obtained from the binodal models for the four systems were determined, and the effect of salts on solubility curves and tielines were discussed. The asobtained results are necessary for the design and optimization of extraction processes as well as the development of both thermodynamic and mass transfer models of ILATPSs.
2. Experimental Section
2.1. Materials
The [EPy]Br was purchased from Chengjie Chemical Co., Ltd. (Shanghai, China) with a quoted purity of a mass fraction above 0.99 and was dried under high vacuum at 343.15 K using a semimicrodistiller with slow heating to remove impurities, mainly water. To prevent contact with the ambient air, the IL was kept in a sealed vessel and placed in refrigerator. The Na_{2}HPO_{4}·12H_{2}O, K_{2}HPO_{4}·3H_{2}O, K_{2}SO_{4} and C_{4}O_{6}H_{4}KNa·4H_{2}O were analytical grade reagents which were purchased from the Guanghua Chemical Factory Co., Ltd. (Guangdong, China). Doubledistilled deionized water was also used in the experiments.
2.2. Experimental Procedure
The solubility curves were determined using the cloud point method. First, an IL solution of known mass fraction was added into a vessel, and the salt solution of known mass fraction was added dropwise until the mixture became cloudy. The composition of the mixture was calculated and the water content of the ionic liquid was calculated into the water mass fraction in the experiment mass balance. Then water was added dropwise until the mixture became clear. The procedure was repeated to obtain all the points on the solubility curves until there was little precipitation at the bottom of the vessel. The vessel was placed in a DC2008 water thermostat throughout the process, so that the temperature of the system could be kept constant (at K). The temperature was controlled to within ±0.05 K. An analytical balance (model BS 124S, Beijing Sartorius Instrument Co., China) with a precision of kg was used to measure the composition of the mixture at each point.
To determine the tielines, a series of ATPSs formed from three known compositions (including salt and water) were placed in a temperaturecontrolled bath. The system was held for at least 24 h to allow the formation of two phases. Both the upper and the lower phases were sampled for analysis. The concentrations of the salts in the two phases were determined via flame photometry. The uncertainty in the mass fractions of the salts was estimated to be ±0.001. The mass fraction of [EPy]Br in both the top phase and bottom phase was determined using a UVvis spectrophotometer (model UV2450, Shimadzu Corporation, Japan) and the uncertainty was determined to be less than 7.5%. A suitable sample of the top phase or bottom phase was removed and placed into a vessel to be mixed with an appropriate quantity of water. The absorbance of the solution was then measured at a wavelength of 211 nm to obtain the mass fraction of the ionic liquid according to a standard curve.
The tieline length (TLL), which reflects the differences between composition of top and bottom phase and the slope of the tieline , which reflects the ability of phase formation to ATPS, were also calculated at different compositions, using the following two equations, respectively, [29]: where , , , and represent the equilibrium mass fraction of the [EPy]Br and salt in the top and bottom phases, respectively. The tieline data are provided in Table 1.

3. Results and Discussion
3.1. Solubility Data and Correlation
The solubility data determined at K are listed in Table 2. The data were fitted using the empirical nonlinear expression developed by Merchuk et al. [30] as follows: where and are the mass fractions of the [EPy]Br and the salt, respectively. This expression has been used for the correlation of IL + salt ATPSs [31, 32] and IL + sugars ATPSs [14]. The parameters for this equation were determined from the experimental data obtained by the cloud point method. Coefficients , , and obtained from the correlation of the experimental solubility data with the corresponding standard deviations (sd) and correlation coefficient are given in Table 3.

 
sd = . Where is the experimental mass fraction of IL and is the corresponding data calculated using (2). The term “N” represents the number of solubility data. 
To obtain a more accurate fit, a nonlinear empirical expression [33] of the following form was proposed to correlate the solubility data where is the mass fraction of the IL, is the mass fraction of the salts, and the coefficients , , , and are fitting parameters. These parameters, along with the correlation coefficient and standard deviations (sd), are given in Table 4.
 
sd = . Where is the experimental mass fraction of IL and is the corresponding data calculated using (3). The term “N” represents the number of solubility data. 
The following equation was also successfully used in this work to correlate the data: where and are the mass fractions of the IL and salts, respectively. This equation has been extended to fit the results of the ATPSs based on hydrophilic organic solvents [34, 35]. The coefficients , , , , and along with the correlation coefficient and the standard deviations (sd) are listed in Table 5.
 
sd = . Where is the experimental mass fraction of IL and is the corresponding data calculated using (4). The term “N” represents the number of solubility data. 
The solubility curves determined at K for the [EPy]Br salt (Na_{2}HPO_{4}, K_{2}HPO_{4}, K_{2}SO_{4}, C_{4}O_{6}H_{4}KNa) + water systems, which provided the minimum concentration required for the formation of these four ATPSs, are plotted in Figure 1, from which it can be observed that an ATPS can be produced by adding an appropriate amount of one salt to an aqueous solution of [EPy]Br. Moreover, one can easily conclude that the phaseseparation abilities of the salts follow the order of by comparing different curves in the phase diagram.
Based on the asobtained and standard deviation values in Tables 3–5, it can be concluded that (2)–(4) are satisfactory for correlating the solubility curves of the investigated systems. The same levels of satisfactory results were obtained in other ILATPS as well [36]. Furthermore, the Merchuk equation performs best of the three while it possesses only three adjustable parameters.
3.2. Effective Excluded Volume (EEV) and Saltingout Ability
A binodal model based on the statistical geometry method developed by Guan et al. [37] for aqueous polymer systems was applied to correlate the experimental solubility data of ATPSs containing Na_{2}HPO_{4}, K_{2}HPO_{4}, K_{2}SO_{4}, and C_{4}O_{6}H_{4}KNa in this paper. The binodal equation can be written as follows:where , , , and are the scaled EEV of the salts, the volume fraction of the unfilled effective available volume after tightly packing the salt molecules into the network of ionic liquid molecules in the ionic liquid aqueous solutions, and the molar masses of the ionic liquid and salt, respectively. The values of and derived from the correlation of the experimental solubility data and the corresponding correlation coefficients () and standard deviations (sd) are given in Tables 6 and 7.
 
sd = . Where is the experimental mass fraction of IL and is the corresponding data calculated using (6). The term “N” represents the number of solubility data. 
 
sd = . Where is the experimental mass fraction of IL and is the corresponding data calculated using (7). The term “N” represents the number of solubility data. 
The saltingout ability of the salt could be related to the EEV [38–40]. The salt with higher saltingout ability has a larger EEV value at the same temperature. This is because with a increase in EEV, the solubility line moves to the left of the phase diagram and the singlephase area decreases correspondingly, resulting in the decline of salts content forming ILATPS, which means that saltingout ability becomes stronger. The EEV represents the smallest spacing of the individual ionic liquid that will adopt an individual salt, reflecting the compatibility of both components in a system. In this study, the EEVs have been calculated using the binodal model developed by Guan et al. [37]. In the original application, (7) was used to correlate the solubility data of polymerpolymer systems because the two components significantly vary in size. The value is so small that it can be neglected without obvious influence. From Table 7, it can be found that the parameter was small enough to be neglected for the investigated systems, and the standard deviation in (7) differed significantly from that in (6) for the solubility data fitting, rendering (7) unusable.
According to Table 6, the saltingout ability of the salts at a constant temperature follows the order: K_{2}SO_{4 }> K_{2}HPO_{4 }> Na_{2}HPO_{4 }> C_{4}O_{6}H_{4}KNa, which is in agreement with the phaseseparation abilities determined from Figure 1. Apparently, (6) satisfactorily reproduce the solubility curves of the investigated systems. However, when compared to the Merchuk and two other equations, there see a big gap.
Some also insist that saltingout abilities of different salts have something to do with ion hydration free energy (ΔG_{hyd}) [41], the more negative the ions, the stronger their saltingout abilities. K_{2}HPO_{4} and Na_{2}HPO_{4} share the same anion, the cation radius of cation K^{+} exceeds that of Na^{+}, and ΔG_{hyd} of K^{+} and Na^{+} are −295 and −365 kJ·mol^{−1}, respectively. In accordance with the ion hydration free energy theory, the saltingout ability of Na_{2}HPO_{4} should be stronger than K_{2}HPO_{4}. However, we found that in our study that although ΔG_{hyd} of K^{+} is greater than Na^{+}, the saltingout ability is much higher. Still, the anions promote the formation of ATPSs in the following order: (ΔG_{hyd} = −1080 kJ·mol^{−1}) > (ΔG_{hyd} = −1789 kJ·mol^{−1}), which also deviates from the ion hydration free energy theory.
3.3. TieLine Data and Correlation
The tieline compositions, tieline length (TLL), and average slopes determined at K are listed in Table 1 and Figures 2 and 3. In this work, the tieline compositions are closely connected by the OthmerTobias equation (6) and Bancroft equation (7) [42, 43] as follows:
In these equations, is the mass fraction of the IL in the top phase; is the mass fraction of the salt in the bottom phase; and are the mass fractions of water in the bottom and top phases, respectively. Recently, (6) and (7) have been successfully verified by other ATPS researchers, indicating that the two equations can accurately correlate the tieline data of the systems. The plots of log[] against log[/] and log against log shows linear relationships, indicating acceptable consistency of the results. The values of the fit parameters , , , and , the coefficient values (),and the standard deviations (sd) are listed in Table 8.
 
sd = . Where N is the number of tielines and j = 1 and j = 2, sd_{1} and sd_{2} represent the mass percent standard deviations for [EPy]Br and the salt, respectively. 
For further confirmation, the Setschenowtype equation [44] was used to correlate the tieline compositions of the [EPy]Br + Na_{2}HPO_{4}/K_{2}HPO_{4}/K_{2}SO_{4}/C_{4}O_{6}H_{4}KNa ATPSs at K:
In the above equation, , , , and represent the molality of the IL, the molality of the salt, a parameter relating the activity coefficient of the IL to its concentration, and the saltingout coefficient, respectively. The two superscripts “” and “” represent the ILrich phase and the saltrich phase, respectively. Assuming that the first term on the right side of this equation is negligible in comparison with the second term, a Setschenowtype equation can be obtained, implying that because the absolute values of exceed those of . This equation was successfully used for the correlation of tieline data for the IL + salt ATPSs [42]. The saltingout coefficients, , with the corresponding intercepts, correlation coefficient () as well as standard deviations (sd) are all listed in Table 9.
 
sd = . Where N is the number of tielines and j is the number of components in each phase. is the standard deviation for the fitting parameters of “”. is the standard deviation of the fitting parameters of the “intercept”. 
In our study, a correlating equation with two parameters has also been used to determine the tieline data which can be derived using the binodal theory [37]. The equation has the following form: in which is the saltingout coefficient, and is the constant most closely related to the activity coefficient. The superscripts “” and “” represent the ILrich phase and the saltrich phase, respectively. Recently, (9) was successfully used to correlate the tieline data for a polymersalt ATPS [45, 46]. The fitting parameters of this equation, the correlation coefficient values (), and the standard deviations (sd) are provided in Table 10.
 
sd = . Where N is the number of tielines and j is the number of components in each phase. 
The standard deviations in Tables 8–10 are small, indicating that (6)–(9) are appropriate for correlating the tieline data of the ATPSs especially the Setschenowtype equation. For more details about the relationship between the Setschenowtype behavior and the phase diagrams, the Setschenowtype plots of the tieline data for the investigated systems are also shown in Figure 4. The Setschenowtype plots with data from Table 9 indicate that the larger the slope, the larger the . When combining with Figure 1, the larger the , the higher saltingout ability. This behavior is in agreement with the reported results for other ATPSs [47].
3.4. Calculation of the Plait Point
Plait points are points on the solubility curves where the length of tielines shrank to almost zero, indicating that the two liquid phases become identical [48]. The plait points data for the investigated ATPSs in this study were calculated via the following linear equation: in which and are the fitting parameters. For the four systems, the estimated values of the plait points along with the fitting parameters obtained from (10) and the corresponding correlation coefficients are given in Table 11.
 
sd = . Where is the experimental mass fraction of IL and is the corresponding data calculated using (10). The term “N” represents the number of solubility data. 
3.5. Effect of Salts on Solubility Curves and TieLines
Figure 1 presents the effect of different salts on the solubility curves. It is clear that different salts possess twophase areas of different sizes. In this study, K_{2}SO_{4} owns the largest area of two phase; therefore, the phaseseparation ability of K_{2}SO_{4} precedes the other three.
Considering that the salts Na_{2}HPO_{4} and K_{2}HPO_{4} share a common anion but contain different cations, one can conclude that the saltingout ability of K^{+} is higher than that of Na^{+} at a constant temperature, which is contrary to what Chen and Wang [49] obtained from their research. This may be due to the relatively large radius of . Also, the K_{2}HPO_{4} and K_{2}SO_{4} share a common cation K^{+}, but the EEV for K_{2}SO_{4} is higher than that of K_{2}HPO_{4}; therefore, the saltingout ability of is higher than that of at the same temperature. When it comes to C_{4}O_{6}H_{4}KNa, which owns both K^{+ }and Na^{+}, it might be the organic ion C_{4}O_{6} that brings about the weakest saltingout ability.
Figures 2 and 3 present the effect of different salts on the phase compositions, from which it can be informed that the slopes of tielines differ greatly towards different salt types. The slopes of tielines for ATPS containing K_{2}SO_{4} are of the largest value, illustrating that K_{2}SO_{4} hydrates the most water, thus decreasing the amount of water available to hydrate [EPy]Br.
4. Conclusions
The liquidliquid equilibrium data have been determined for [EPy]Br + salt (Na_{2}HPO_{4}, K_{2}HPO_{4}, K_{2}SO_{4} and C_{4}O_{6}H_{4}KNa) ATPSs at K. The effect of salt on solubility curves as well as tielines was studied. The volume (EEV) values obtained from the binodal model together with the phase diagram indicated the order of phase separation abilities of the four salts. The Merchuk equation and two other equations were used to correlate the solubility data and the OthmerTobias, Bancroft, and Setschenowtype equations and a twoparameter equation were used to correlate the tieline data. The results indicate that the calculation method and the corresponding tieline data are reliable. At fixed temperatures, the saltingout ability of K^{+} is higher than that of Na^{+}, and that of anions follows .
List of Symbols
:  Number of solubility data 
:  Number of tielines 
:  Temperature (K) 
TLL:  Tieline length 
:  Slope of the tieline 
:  Mass fraction 
, :  Saltingout coefficient 
:  Interaction parameter 
:  Scaled EEV of salt 
:  Volume fraction 
:  Molar mass 
:  Fitting parameters 
:  Correlation coefficient 
sd:  Standard deviation. 
:  Bottom phase 
:  Top phase 
cal:  Calculated value 
exp:  Experimental value 
1:  [EPy]Br 
2:  Salt 
3:  Water. 
Conflict of Interests
None of the authors for this paper have a direct financial relation with the commercial identity mentioned in this paper.
Acknowledgments
This work was sponsored by the Research and Development Project of Science and Technology of Shaanxi Province (no. 2013JQ2019), the Fundamental Research Funds for the Central Universities (no. 2013G2291015, 2013G1291071, and 2013G1502038) and the National Training Projects of the University Students’ Innovation and Entrepreneurship program (no. 201310710057).
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