LiquidâLiquid Equilibrium for the Ternary System Isopropyl Acetate +

Article pubs.acs.org/jced

Liquid−Liquid Equilibrium for the Ternary System Isopropyl Acetate + Ethanol + Water at (293.15, 313.15, and 333.15) K Jun Gao,* Nannan Chen, Dongmei Xu, Lianzheng Zhang, Liwen Zhao, and Zhishan Zhang Department of Chemical and Environmental Engineering, Shandong University of Science and Technology, Qingdao 266590, China ABSTRACT: The ternary liquid−liquid equilibrium (LLE) experimental data for the system isopropyl acetate + ethanol + water have been measured at (293.15, 313.15, 333.15) K under pressure of 101.3 kPa in this work. The quality of the determined experimental data was checked by the Bachman and Hand equations, which the correlation coefficients of the Bachman equation were 0.9964, 0.9997, and 0.9994, and the those of the Hand equation were 0.9717, 0.9846, and 0.9934 for (293.15, 313.15 and 333.15) K. Moreover, the measured data were correlated by the nonrandom twoliquid (NRTL) and universal quasi-chemical (UNIQUAC) activity coefficient equations, and the parameters of the two equations were regressed. The comparison between the correlated values and the measured data was made, which the correlated values agree well with the determined LLE data. Meanwhile, the selectivity (S) and distribution coefficient (D) for this ternary system were calculated from the experimental data.

1. INTRODUCTION

2. EXPERIMENTAL SECTION 2.1. Chemicals. Isopropyl acetate and ethanol were used in present work, which the mass purities of isopropyl acetate and ethanol were 0.990, 0.995, respectively. No further purification was processed for all the chemicals. And ultrapure water was applied in this experiment. The purities of all the chemical reagents were checked by gas chromatography. Some detailed relevant information are given in Table 1. The refractive indices

As an important sulfur-containing compound, mercaptoacetic acid is widely applied in science and industry fields for its desirable properties.1,2 Usually, mercaptoacetic acid is a byproduct from the industrial production of thiourethane. However, during the extraction separation process of mercaptoacetic acid, in which isopropyl acetate is used as an extracant, a waste aqueous solution consists of isopropyl acetate, ethanol, and water is left. Thus, the separation of isopropyl acetate and ethanol from the waste aqueous solution caused by mercaptoacetic acid purification attracts much attention for its significance in both economy and environment protection. For the treatment of the waste aqueous solution, liquid− liquid extraction process is selected to separate isopropyl acetate and ethanol, in which isopropyl acetate and ethanol can be recovered and reused for the separation of mercaptoacetic acid. Therefore, the accurate experimental data of liquid−liquid equilibrium (LLE) for the system isopropyl acetate + ethanol+ water is needed, which is important for the extraction process optimization and design.3,4 Up to now, the experimental data of liquid−liquid equilibrium for the system isopropyl acetate + ethanol + water are not reported. Thus, it is necessary to determine the liquid−liquid equilibrium data for isopropyl acetate + ethanol + water system. The ternary LLE data for system of isopropyl acetate + ethanol + water were measured at (293.15, 313.15, and 333.15) K under atmospheric pressure of 101.3 kPa in present work. The consistency of the experimental tie-line data was checked by the Hand15 and Bachman16 equations. The experimental data were correlated by the universal quasichemical5 (UNIQUAC) and the nonrandom two-liquid6,7,8,9 (NRTL) activity coefficient equations. Meanwhile, the parameters of the two activity coefficient equations were obtained, which could be applied in the design of the extraction process.17 © XXXX American Chemical Society

Table 1. Suppliers and Mass Fractions of the Chemical Reagent component

CAS

suppliers

isopropyl acetate

10821-4

ethanol

6756-1

Chengdu Kelong Chemical Co., Ltd. Tianjin Fuyu Fine Chemical Co., Ltd.

a

mass fraction

purification method

analysis method

>0.99

none

GCa

>0.995

none

GCa

Gas chromatograph.

were measured at λ = 589.3 nm and 293.15 K by using an 2AWJ refractometer produced by Shanghai Experimental Instrument Co., Ltd., which was calibrated by water, and its measurement range was 1.3000 to 1.7000. The uncertainty was 0.0012. The information on the isopropyl acetate and ethanol are given in Table 2. 2.2. Apparatus and Procedure. The apparatus applied in present work was reported in the previous work,26 which mainly included a SP-6890 gas chromatography made by Shandong Lunan Rui Hong Chemical Instrument Co., Ltd., a SYC-15C super thermostatic water bath produced by Nanjing Huchuan Electronic Equipment Co., Ltd. with the temperature Received: May 25, 2016 Accepted: August 24, 2016

A

DOI: 10.1021/acs.jced.6b00428 J. Chem. Eng. Data XXXX, XXX, XXX−XXX

Journal of Chemical & Engineering Data

Article

Table 2. Mole weights, M, boiling temperatures, Tb, and refractive index, nD, at 293.15 K under atmospheric pressure of 0.1 MPaa

temperature for about 16 h until it reached the equilibrium state. Any disturbance from outside should be avoided when the equilibrium state was reached. Finally, the samples were drawn from the acetate-rich phase and water-rich phase respectively, for analysis by using different syringe without contamination. Each of all the samples was checked by GC three times, and the average value was used. 2.3. Analysis. The sample peak area was determined by GC (SP-6890) with a thermal conductivity detector (TCD), and a capillary column (DB-624, 30m × 0.53m × 3 μm). Hydrogen gas was used as the carrier gas with purity of 99.999%, which the flow rate of gas was 10 mL/min. The injection temperature was fixed at 443.15 K. The oven initial temperature was kept at 373.15 K for 3 min, and the column temperature increased at 10 K/min to reach 433.15 K, and was fixed for 8 min. The temperature of TCD detector was held at 443.15 K. Before analyzing the composition of the sample by GC, three mixtures with known compositions were prepared gravimetrically by a balance to calibrate the analysis result. The uncertainty of measured mole fractions of the samples was ±0.001.

nD component isopropyl acetate ethanol water

−1

M/g mol 102.13 46.07 18.02

Tb/K

experiment

literature

362.1510 351.4124 373.1524

1.3771 1.3616 1.3328

1.377310 1.361425 1.333025

a

Standard uncertainties u are u(nD) = 0.0012, u(T) = 0.01 K, u(P) = 1 kPa.

measurement accuracy of ±0.01 K, a 100 mL glass container and a magnetic stirrer. During the experiments, the volume of water was kept for constant, and those of isopropyl acetate and ethanol were varied with increasing one and decreasing another accordingly, which the entire two-phase region of the ternary samples could be covered as much as possible.24 First, the ternary mixtures of isopropyl acetate + ethanol + water were made in the equilibrium cell and stirred vigorously for 2 h to ensure that the sample was mixed completely. Second, the sample was settled in a super thermostatic water bath and kept at constant

Table 3. Experimental LLE Data, in Mole Fractions, for Isopropyl Acetate (1) + Ethanol (2) + Water (3) and Distribute Coefficient of Ethanol, D2, Water, D3, and Selectivity, S at T = (293.15, 313.15, and 333.15) K and Pressure P = 0.1 MPaa aqueous phase

a

organic phase

xI1

xI2

xI3

xII1

0.0038 0.0036 0.0041 0.0050 0.0068 0.0073 0.0080 0.0085 0.0120 0.0153

0.0211 0.0381 0.0597 0.0775 0.0866 0.0959 0.0970 0.1068 0.1098 0.1201

0.9751 0.9583 0.9362 0.9175 0.9066 0.8968 0.8920 0.8847 0.8781 0.8646

0.8572 0.8210 0.7372 0.6500 0.6032 0.5229 0.4891 0.4586 0.4273 0.3693

0.0028 0.0022 0.0056 0.0057 0.0081 0.0091 0.0087 0.0108 0.0137 0.0134

0.0376 0.0540 0.0719 0.0799 0.0874 0.0915 0.0959 0.1020 0.1067 0.1172

0.9596 0.9438 0.9225 0.9144 0.9045 0.8994 0.8954 0.8872 0.8796 0.8694

0.7934 0.7334 0.6268 0.5450 0.4800 0.4488 0.4263 0.4000 0.3663 0.3146

0.0007 0.0018 0.0057 0.0067 0.0078 0.0089 0.0103 0.0119 0.0152

0.0579 0.0734 0.0871 0.0924 0.0979 0.1025 0.1081 0.1138 0.1242

0.9414 0.9248 0.9072 0.9009 0.8943 0.8886 0.8816 0.8743 0.8606

0.6121 0.5171 0.4423 0.4083 0.3756 0.3412 0.3118 0.2857 0.2372

xII2 T = 293.15 K 0.0326 0.0582 0.1060 0.1500 0.1789 0.2187 0.2222 0.2445 0.2518 0.2709 T = 313.15 K 0.0781 0.1198 0.1592 0.2036 0.2200 0.2312 0.2416 0.2500 0.2638 0.2636 T = 333.15 K 0.1517 0.1916 0.2133 0.2225 0.2308 0.2380 0.2424 0.2456 0.2475

xII3

D2

D3

S

0.1102 0.1208 0.1568 0.2000 0.2179 0.2584 0.2827 0.2969 0.3209 0.3598

1.545 1.528 1.776 1.935 2.066 2.281 2.291 2.289 2.293 2.256

0.1130 0.1260 0.1675 0.2180 0.2404 0.2881 0.3169 0.3336 0.3654 0.4161

13.67 12.13 10.60 8.876 8.594 7.917 7.213 6.862 6.275 5.422

0.1285 0.1468 0.2140 0.2514 0.3000 0.3200 0.3321 0.3500 0.3699 0.4218

2.077 2.218 2.214 2.548 2.517 2.527 2.519 2.451 2.472 2.249

0.1340 0.1555 0.2318 0.2749 0.3317 0.3558 0.3709 0.3945 0.4205 0.4852

15.51 14.26 9.551 9.269 7.589 7.102 6.792 6.213 5.879 4.635

0.2362 0.2913 0.3444 0.3692 0.3936 0.4208 0.4458 0.4687 0.5153

2.620 2.610 2.449 2.408 2.358 2.322 2.242 2.158 1.993

0.2509 0.3150 0.3796 0.4098 0.4401 0.4736 0.5057 0.5361 0.5988

10.44 8.286 6.452 5.876 5.358 4.903 4.433 4.025 3.328

Standard uncertainties u are u(T) = 0.01 K, u(x) = 0.001, u(P) = 1 kPa. B



Article

3. RESULTS AND DISCUSSION 3.1. Experimental LLE Results. The experimental data of the system isopropyl acetate + ethanol + water were measured at T = (293.15, 313.15, 333.15) K and atmospheric pressure. The mole fractions of the acetate-rich and the water-rich phase are presented in Table 3, where the superscript I represents the water-rich phase, and II represents the acetate-rich phase, the subscript 1, 2, and 3 represent isopropyl acetate, ethanol, and water, respectively. The LLE data were plotted and shown in Figure 1, 2, and 3.

Figure 3. Liquid−liquid equilibrium phase diagram for the system isopropyl acetate (1) + ethanol (2) + water (3) at T = 333.15 K: ■−■, experimental data; ●···●, NRTL models; △···△, UNIQUAC models.

isopropyl acetate + ethanol + water was small. Considering the impact of the temperature, when the temperature increased from 293.15 K to 333.15 K, the immiscible area decreased slightly, since the solubility of isopropyl acetate and ethanol in water increased with increasing the temperature. Distribution coefficient (D) and selectivity (S) are important parameters for liquid−liquid extraction.11,12,13,14 D is used to evaluate the distribution of the composition in the equilibrium system and S is used to express the extraction ability of the solvent, which are presented as


⎛ x II ⎞ Di = ⎜ i I ⎟ ⎝ xi ⎠ S=

(1)

x 2IIx3I x 2Ix3II

xI2

(2)

xI3

where and represents the mole fraction of ethanol and water in water-rich phase, xII2 and xII3 represents the mole fractions of ethanol and water in acetate-rich phase, respectively. The selectivity S and distribution coefficient D are reported in Table 3. Compared with the values of D2, which is the distribution coefficient of ethanol, the values of D3 are small, which indicate that the solubility of isopropyl acetate in water is small. The calculated results of S for the ternary system were all higher than 1 at the temperature range investigated, which indicated that the separation of waste solution was possible. S decreased with increasing the concentration of ethanol, which showed that the separation capacity of isopropyl acetate decreased with increasing the concentration of ethanol. Meanwhile, the influence of temperature was not obvious. When the temperature increased, the extraction ability of the isopropyl acetate was weakened. Therefore, the suitable temperature, 293.15 K, was determined for the extraction separation of the aqueous mixture. 3.2. Validation of Data Reliability. The consistency of the LLE experimental data were always checked by Hand15 and Bachman16 equations. Both equations were adopted to confirm the consistency of the experimental data, which are expressed as


It can be seen that the phase diagrams for the ternary system of isopropyl acetate, ethanol, and water were classified as Treybal’s type I23 from Figures 1, 2, and 3. The experimental data showed that the solubility of water in the isopropyl acetate increased with the increasing mole fraction of ethanol. As shown in Figure1, 2, and 3, the immiscible area for the system C



Article

Table 4. Constants and Correlation Factor, R2, of the Bachman and Hand Equations for the Ternary System Isopropyl Acetate + Ethanol + Water at Different Temperatures Bachman

Hand 2

T/K

a

b

R

293.15 313.15 333.15

0.0127 −0.0139 −0.0423

0.9427 0.9944 1.0006

0.9964 0.9997 0.9994

⎛ x II ⎞ x1II = a + b⎜ 1I ⎟ ⎝ x3 ⎠

a

b

R2

−1.7086 −1.9071 −1.9417

0.5976 0.5438 0.5939

0.9717 0.9846 0.9934

(3)

and ⎛xI⎞ ⎛ x II ⎞ ln⎜ 2I ⎟ = a + b ln⎜ 2II ⎟ ⎝ x1 ⎠ ⎝ x3 ⎠

(4)

where xIi and xIIi represent the mole fraction of component i in the acetate-rich phase and in the water-rich phase. a and b are constants. All the experimental tie-line data were verified. The factors (R2) are higher than 0.9717, which indicate that the consistency of the experimental data are good. The parameters a, b, and R2 are presented in Table 4. Meanwhile, the linearity plots of the two models are given in Figure 4 and 5.

Figure 5. Hand plots of the system isopropyl acetate (1) + ethanol (2) + water (3) at different temperatures: ■, 293.15 K; ●, 313.15 K; ▲, 333.15 K.

UNIQUAC: ln γi = ln + qi −

ψi xi

ψi xi

3

+

θ z qi ln i − qi ln(∑ θτ j ji) + li 2 ψi j=1

3

θτ j ij 3 j = 1 ∑k = 1 θkτkj

∑ xjlj − qi ∑ j

(7)

And lj =

ψi =

Figure 4. Bachman plots of the system isopropyl acetate (1) + ethanol (2) + water (3) at different temperatures: ■, 293.15 K; ●, 313.15 K; ▲, 333.15 K.

ln γi =

3 ∑k = 1 Gkixk

3

+

xjGij 3 j = 1 ∑k = 1 Gkjxk

∑

3 ⎛ ∑ xτ G ⎞ ⎜τ − k = 1 k kj kj ⎟ 3 ⎜ ij ∑k = 1 xkGkj ⎟⎠ ⎝

bij T

Gij = exp( −αijτij)

xiqi m ∑i = 1 xiqi

⎛ bij ⎞ τij = exp⎜aij + ⎟ T⎠ ⎝

Table 5. Structural Parameters20 for the UNIQUAC Equation

(5)

and τij = aij +

θi =

where aij and bij are parameters of the models needed to regressed, γi represents the activity coefficient, x represents the experimental mole fraction, αij is the nonrandomness constant in NRTL model. The structural parameters20 ri and qi for the UNIQUAC equation are shown in the Table 5. Aspen Plus software were used to correlate the experimental LLE data in the present work. The activity objective function Fa and the concentration objective function Fx were used to determine the binary interaction parameters, which were

NRTL 3

xiri m ∑i = 1 xiri

(8)

(9)

3.3. LLE Data Correlation. The experimental LLE data were correlated by using NRTL and UNIQUAC activity coefficient models,18,19 which are expressed as ∑ j = 1 τjiGjixj

⎛z⎞ ⎜ ⎟(r − q ) − (r − 1) j j ⎝2⎠ j

(6) D

component

ri

qi

isopropyl acetate ethanol water

4.152 2.106 0.920

3.652 1.972 1.400



Article

Table 6. NRTL and UNIQUAC Parameters for the Ternary System Isopropyl Acetate + Ethanol + Water at T = (293.15, 313.15, and 333.15) K under Pressure of 101.3 kPa NRTL parameters

UNIQUAC parameters

T/K

i−j

aij

aji

bij

bji

α

RMSD

aij

aji

bij

bji

RMSD

293.15−333.15

1−2 1−3 2−3

−18.89 6.606 −0.913

4.263 27.91 −4.633

6263 −1366 629.8

−1301 −6459 1723

0.30 0.30 0.30

0.0132 0.0122 0.0137

−12.42 −0.755 0.484

4.188 −6.619 5.818

2995 −193.5 23.05

−945.2 1738 −1864

0.0091 0.0181 0.0154

■

applied by many scholars in the previous work.21,22 Fa and Fx were optimized by reducing the differences between the experimental and calculated mole fractions for each of the components. Also, the objective functions are presented as the following: M

Fx =

2

∑ min ∑ ∑ (xijk − xijk̂ ) +Q ∑ Pn j=1 j=1

k=1

⎛aI ⎜ ikI a k = 1 I = 1 ⎝ ik M

Fa =

3

∑∑

Corresponding Author

*E-mail: [email protected]. Tel.: +86 532 8605 7798. Funding

Financial support from National Natural Science Foundation of China (Project 21306106) is gratefully acknowledged.

3 2

− +

n

2 aikII ⎞ ⎟ +Q aikII ⎠ n

∑ Pn2

2

Notes

(10)

The authors declare no competing financial interest.

■

(11)

RMSD =

2

3

∑k = 1 ∑ j = 1 ∑i = 1 (xijk − xijk ̂ )2 6M

REFERENCES

(1) Chazin, E. Mercaptoacetic Acid. Synlett 2013, 24, 775−776. (2) Kakharev, B. F.; Stankevich, V. K.; Klimenko, G. R. Reaction of vinyloxyalkylamines with mercaptoacetic acid. Russ. Chem. Bull. 1996, 45, 637−639. (3) Esteban, J.; Vorholt, A. J.; Behr, A.; Ladero, M.; Garcia-Ochoa, F. Liquid-liquid equlibria for the system acetate + solketal + glycerol at (303.2, 313.2, and 323.2) K. J. Chem. Eng. Data 2014, 59, 2850−2855. (4) Simoni, L. D.; Lin, Y.; Brennecke, J. F.; Stadtherr, M. A. Reliable computation of binary parameters in activity coefficient models for liquid−liquid equilibrium. Fluid Phase Equilib. 2007, 255, 138−146. (5) Abrams, D. S.; Prausnitz, J. M. Statistical Thermodynamics of liquid mixtures: A new expression for the Excess Gibbs Energy of Partly or Completely Miscible Systems. AIChE J. 1975, 21, 116−128. (6) Renon, H.; Prausnitz, J. M. Local Compositions in Thermodynamic Excess Functions for Liquid Mixtures. AIChE J. 1968, 14, 135− 144. (7) Ince, E.; Lalikoglu, M.; Constantinescu, D. Liquid Phase equilibria of water + formic Acid + dimethyl Carbonate ternary system at several temperatures. J. Chem. Eng. Data 2014, 59, 2781− 2787. (8) Aljimaz, A. S.; Fandary, M. S. H.; Alkandary, J. A.; Fahim, M. A. J. Chem. Eng. Data 2000, 45, 301−303. (9) Renon, H.; Prausnitz, J. M. Local. AIChE J. 1968, 14, 135−144. (10) Zhang, W.; Wang, X.; Meng, N. Liquid−Liquid Equilibria of the Ternary Mixtures with Sulfolane at 303.15 K. J. Chem. Data 1996, 41, 634−638. (11) Yamaguchi, F.; Katsube, T. European Patent 0995736 A2, 2000. (12) Yoshizawa, T.; Yodogawa, S.; Osaka, F. European Patent 0967193 A2, 1999. (13) Kadir, S.; Decloux, M.; Giampaoli, P.; Joulia, X. J. Chem. Eng. Data 2008, 53, 910−912. (14) Bunch, D. S.; Gay, D. M.; Welsch, R. E. Algorithm 717: Subroutines for Maximum Likelihood and Quasi-likelihood Estimation of Parameters in Nonlinear Regression Models. ACM Trans. Math. Softw. 1993, 19, 109−130. (15) Hand, D. Dineric Distribution. J. Phys. Chem. 1929, 34, 1961− 2000. (16) Bachman, I. Tie lines in Ternary Liquid Systems. Ind. Eng. Chem., Anal. Ed. 1940, 12, 38−39. (17) Hu, M. C.; Zhu, X.; Li, S. N.; Zhai, Q. G.; Jiang, Y. C.; Lin, X. Y.; Tuo, C. S. Liquid−Liquid Equilibria for Methanol/Ethanol + Rubidium Carbonate + Water Systems at Different Temperatures. J. Chem. Eng. Data 2009, 54, 2866−2870. (18) Fernández-Torres, M. J.; Gomis-Yagües, V.; Ramos-Nofuentes, M.; Ruíz-Beviá, F. The influence of the temperature on the liquid− liquid equilibrium of the ternary system 1-pentanol−ethanol−water. Fluid Phase Equilib. 1999, 164, 267−273.

where a represents the activity that calculated from NRTL or UNIQUAC model; Q is a constant that the objective function to be minimized by data regression; x represents the mole fraction of the experimental data; x̂ represents the mole fraction of the calculated values; Pn represents the NRTL or UNIQUAC parameters; i, j, k, represent the components; the phase and the tie lines, respectively. The binary interaction parameters of the NRTL and UNIQUAC models for correlation of the ternary LLE data are listed in Table 6. The correlation reliability was verified by the RMSD defined as follows: M

AUTHOR INFORMATION

(12)

where M represents the number of tie-lines. The calculated results of RMSD are presented in Table 6, which indicates that the calculated results of the NRTL and UNIQUAC equations are in better agreement with the LLE experimental data.

4. CONCLUSIONS The experimental ternary LLE data for isopropyl acetate + ethanol + water were determined at T = (293.15, 313.15, and 333.15) K, under pressure of 101.3 kPa. The distribution coefficient (D) and selectivity (S) were calculated and discussed. The selectivity values were all higher than 1, which indicate that the separation of the system is feasible. The immiscible zone was slightly affected by temperature. Meanwhile, the consistency of the LLE data were checked by the Hand and Bachman equations, in which the linear correlation coefficients were close to 1. The NRTL and UNIQUAC models were applied to correlate the experimental LLE data, from which the parameters of the two models were also regressed. The values of RMSD of the NRTL are 0.0132, 0.0122, and 0.0137, and the those of the UNIQUAC were 0.0091, 0.0181, and 0.0154 for temperatures at (293.15, 313.15, and 333.15) K, respectively. The values indicate that the correlated results by the NRTL and UNIQUAC models agree well with experimental LLE data. Thus, the measured LLE data and the regressed parameters for the two models are helpful for the design of the extraction process. E



Article

(19) Gomis-Yagües, V.; Ruíz-Beviá, F.; Ramos-Nofuentes, M.; Fernández-Torres, M. J. The influence of the temperature on the liquid−liquid equilibrium of the ternary system 1-butanol−1propanol−water. Fluid Phase Equilib. 1998, 149, 139−145. (20) Gmehling, J.; Kolbe, B.; Kleiber, M.; Rarey, J. Chemical Thermodynamics for Process Simulation; Wiley: New York, 2012. (21) Arce, A.; Rodriguez, O.; Soto, A. Liquid-Liquid Equilibria for Butyl tert-Butyl ether + (Methanol or Ethanol) + Water at Several Temperatures. Fluid Phase Equilib. 2004, 224, 185−192. (22) Aljimaz, A. S.; Fandary, M. S. H.; Alkandary, J. A.; Fahim, M. A. Liquid-Liquid Equilibria of the Ternary System Water + Acetic Acid + 1-Heptanol. J. Chem. Eng. Data 2000, 45, 301−303. (23) Treybal, R. E. Liquid−Liquid Extraction; McGraw-Hill: New York, 1963. (24) Xu, C.; Wu, C.; Zhang, Q.; Zhang, H; Wang, Y.; Gao, J. Liquid− liquid equilibrium for the ternary systems water + 2-methyl-1-propanol + butyl acetate and water + 2-methyl-2-propanol + butyl acetate at (298.15 and 323.15) K. Fluid Phase Equilib. 2014, 381, 60−66. (25) Kleiber, M. Chemical Thermodynamics for Process Simulation; Wiley-VCH: Weinheim, Germany, 2012. (26) Gao, J.; Zhang, L.; Xu, D.; Wei, Y.; Zhang, Z.; Cui, Z. LiquidLiquid equilibrium for the ternary system 2,2,3,3,4,4,5,5-Octafluoro-1Pentanol + Ethanol + Water at (298.15, 308.15, and 318.15) K. J. Chem. Eng. Data 2015, 60, 2733−2738.

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