liquid–liquid equilibria for the quaternary system h 3 po ...
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Liquid−Liquid Equilibria for the Quaternary System H3PO4−NaCl−H2O−TBP at 298.15 KChengqi Liu, Yongsheng Ren,* and Ya’nan Wang
Department of Chemistry and Chemical Engineering, Ningxia University, Yinchuan 750021, PR China
ABSTRACT: The equilibrium data of quaternary system phosphoric acid +sodium chloride + water + tri-n-butyl phosphate (TBP) was discussed at 298.15K and atmospheric pressure. It was investigated experimentally in the massconcentration range 0−15% of NaCl and 4−24% of H3PO4 in the initialaqueous phase. The experimental results show that the separation factor of H2Oand the distribution coefficient of H3PO4 increase when the content of H3PO4increases. The separation factor of NaCl decreases after an increase to amaximum value. Moreover, it was found out that the mass ratio of ternarysystem H3PO4−NaCl−H2O to the saturation point. It would separate easilywhen the mass percent of NaCl occupies more than 12% in the system. Theexperimental tie-line data was correlated with the nonrandom two-liquid activitycoefficient model.
1. INTRODUCTION
Phosphoric acid is widely used in many areas as a basic rawmaterial.1 There are two methods to produce phosphoric acid.One is a thermal method, and the other is a wet process.Although the impurity content is lower by using the thermalmethod, this method consumes a lot of energy and incurs highproduction costs. Moreover, it has serious impact on theenvironment. The wet method has many advantages, such as itneeds less power consumption, the equipment is easy to solve,it facilitate operation management, and has a low productioncost, so that many countries in the world are trying to purifywet-process phosphoric acid to satisfy the requirement ofproducing high purity phosphoric acid.There are multiple ways of purifying wet-process phosphoric
acid, for example, chemical precipitation,2 ion exchange,3 and acrystallization process.4 However, those methods have manylimitations such as high cost, a complex purification process,and serious environmental pollution. It is difficult to meet thedemand in the industry and further theoretical studies areneeded.Solvent extraction process is adopted for its user-friendly
control, safety production, environmental conservation, andeconomy. The method has obvious advantages of its applicationand it is extensively used. The core of extraction lies in theselection of extraction agent. Nowadays, many equilibrium datafor the aqueous mixtures of phosphoric acid with organicsolvents, such as isoamyl acetate, methyl isoamyl ketone,cyclohexane, methylcyclohexane, toluene and tri-n-butylphosphate (TBP), have been reported by several research-ers.5−8 TBP is a neutral extraction agent. It can react in aninorganic complexation reaction. The TBP can, for example,complex with acids in a ratio of 1:1 or 1:3, or complex withwater in a 1:1 ratio.9
Liquid−liquid equilibrium data is important for designingextraction equipment, evaluating the important parameters ofthe extraction process, and enlarging the database of thesimulation process. Using a small amount of experimental dataon liquid−liquid equilibrium data correlation and predictionwithin the range of measurement is very necessary.This research focuses on the determination of the basic data
of the quaternary system H3PO4−NaCl−H2O−TBP obtainingliquid−liquid equilibria at 298.15 K and atmospheric pressure.The mass compositions were measured. Distribution coef-ficients of H3PO4 and separation factors of H2O and NaCl aredetermined from tie-line data. The experimental data wascorrelated using the nonrandom two-liquid (NRTL) activitycoefficient model.
2. EXPERIMENTAL SECTION
2.1. Materials. Phosphoric acid (Sigma, 85%) and sodiumchloride were used as received. TBP was provided by the AodaChemical Company, China, and was used without any furtherpurification. All of the reagents were analytical grade. Doubledistilled water was used in the experiments.
2.2. Procedure. The experiments were carried out at T=(298.15 ± 0.01) K at atmospheric pressure with a thermostat.In the initial aqueous phase of the H3PO4−NaCl−H2O−TBPquaternary system, the concentration range of phosphoric acidstarted at ω (mass fraction) = 0.04% and increased at fourpercent intervals. The concentration of sodium chloride wasfrom 0 to 0.15%. The TBP was mixed with the initial aqueousphase in a 250 mL conical flask which was sealed with clingfilm. The mixture was shaken for an hour at constant
Received: September 10, 2013Accepted: December 17, 2013
Article
pubs.acs.org/jced
© XXXX American Chemical Society A dx.doi.org/10.1021/je400817m | J. Chem. Eng. Data XXXX, XXX, XXX−XXX
temperature and then allowed to sit for one hour to completelyseparate the to two liquid phases; the organic phase is superiorand the aqueous phase in inferior.The two liquids were separated in a separatory funnel, care
being taken to carefully leave a layer of aqueous solution at least1 cm below the interface. Then the remaining aqueous layer aswell as at least 1 cm thick of the organic phase in the separatoryfunnel was collected carefully in a 10 mL buret, in order tomake the sample of superior phase without contaminationbecome possible. The volume of the liquids in the buret wasrecorded and calculated into mass by using densities. Thencomposition analysis was respectively carried out in the twophases. Phosphoric acid concentration in the aqueous phasewas measured by the quinoline phosphomolybdate gravimetricmethod.10 Chloridion concentrations in both phases weredetermined by the Volhard method.11 Water in the organicphase was measured by the Karl Fischer apparatus.12,13 Thedensities of the two phases were determined by pycnometer.14
Phosphoric acid and water concentrations in the organic phaseand TBP concentrations in both phases could be calculated bymaterial balance. At least three parallel samples were carried outin each experiment. All results were expressed in mass fractions.The precision for volume, mass, and density is ± 0.1 mL, ±0.0001 g, ± 0.0001 g·mL−1, respectively, and the combineduncertainty is less than 0.03.15 All the determinations wererepeated three times to check reproducibility, and then anaverage value was given.
3. RESULTS AND DISCUSSION
The experimental results are shown in Table 1. Allconcentrations are expressed in ωi
ϕ, where i stands for thecomponent (i = 1 for phosphoric acid, i = 2 for sodiumchloride, i = 3 for water, i = 4 for TBP) and φ stands for thephase (φ = a for the aqueous phase and φ = o for the organicphase). Table 1 includes the compositions of the initialmixtures and equilibrium phases at 298.15 K. The initialaqueous phase contains mass fraction of 0.04 to 0.24phosphoric acid and 0.0 to 0.15 sodium chloride.Table 1 shows that the TBP in the aqueous phase is very
small. The combination of phosphoric acid with TBP is morethan sodium chloride. As phosphoric acid increases in the initialmixed phase, the content in the organic phase also increases.The case is the same for sodium chloride. In the experiment,the aqueous phase cannot dissolve NaCl completely when themass fraction of NaCl occupies more than 12% in the system.Distribution coefficient refers to the ratio between total
concentration of extracted substance in the organic phase andthat in the aqueous phase. It changes over experimentalconditions such as concentration of extracted substance, acidityof the solution, extractant concentration, and nature of diluentand so on. The material of high distribution coefficient moreeasily transfers from the aqueous phase to the organic phase.On the contrary, the material of the small distributioncoefficient exists in the aqueous phase. Thus, substances canbe separated. The extraction rate refers to the extraction ofmaterial into the organic phase of the two-phase percentage ofthe total. It indicates the extent of extraction. The greaterdistribution coefficient causes the higher extraction rate.The equations are shown as follows,
=DDDi
i
i
o
a(1)
=SDDi
i1,
1
(2)
In the equations, D stands for distribution coefficient and Sstands for separation factor; i stands for the material (i = 1 forphosphoric acid, i = 2 for sodium chloride, i = 3 for water, i = 4for TBP) and “a” stands for the aqueous phase, “o” stands forthe organic phase.16 Equations 1 and 2 can be used to calculatethe values in Table 1.The diagram shows that the distribution coefficient of
phosphoric acid and separation factor of water are increasinggradually when the concentration of sodium chloride isinvariant. The variation trend is shown in Figure 1, Figure 2,and Figure 3. The phosphoric acid composition in the initialaqueous phase is plotted on the x-axis.Figure 1 displays that when the phosphate content is
constant, the distribution coefficient is increasing with theincrease of sodium chloride composition. Meanwhile, when thesodium chloride content is constant, the distribution coefficientis also increasing with the increase of phosphoric acidcomposition. The reason for the increase of D1 is thatphosphoric acid transfers into the organic phase only in aneutral form rather than a dissociated form.17 As thephosphoric acid concentration increases, the proportion ofundissociated phosphoric acid increases.In Figure 2, the results indicate that when the sodium
chloride composition is between ω = 0.03 and 0.05, theseparation factor of sodium chloride (S1,2) decreases, S1,2increases to a maximum value with ω = 0.08 phosphoric acidand then decreases with a further increase in the phosphoricacid concentration, S1,2 increases to a maximum value with ω =0.12 phosphoric acid in the presence of ω = 0.10 to 0.13sodium chloride, when sodium chloride concentration is 0.15,S1,2 increases to a maximum value with ω = 0.16 phosphoricacid and then decreases.In Figure 3, the results indicate that S1,3 increases with an
increase in phosphoric acid concentration in the presence of ω= 0 to 0.15 sodium chloride. When the concentration ofsodium chloride remains unchanged, S1,3 also increases. In theliterature,18 the concentration ranges are from ω (massfraction) = 0.028 to 0.20 for phosphoric acid and ω = 0 to0.25 for calcium chloride in the initial aqueous phase; in ourresearch, ω = 0 to 0.15 for sodium chloride and ω = 0.04 to0.24 for phosphoric acid in the initial aqueous phase. Acomparison of the data of the same concentration range (ω = 0to 0.15) of calcium chloride in the literature with theexperimental data shows that the trend of densities of thetwo phases and distribution coefficient of phosphoric acid areidentical, the distribution coefficient of phosphoric acid is from0.07 to 0.56 in ref 18 and changes from 0.05 to 0.53 in ourexperimental data. It demonstrates that the distribution ofphosphoric acid in the two phases has certain regularity.The the nonrandom two-liquid (NRTL) model of Renon
and Prausnitz can be used for the association of a strongly polarsystem.19 The biggest advantage is that it can be used forcorrelation evaluation of the partially miscible system. H3−PO4−NaCl−H2O−TBP quaternary system is the partiallymiscible system and contains salt, which belongs to the strongpolarity system. Using NRTL is relatively appropriate. In thismodel, the first material is phosphoric acid, the second issodium chloride, and the third is water.
Journal of Chemical & Engineering Data Article
dx.doi.org/10.1021/je400817m | J. Chem. Eng. Data XXXX, XXX, XXX−XXXB
Table1.Liqu
id−Liqu
idEqu
ilibriain
theSystem
H3PO
4(1)−
NaC
l(2)−H
2O(3)−
TBP(4)andthePhysicalR
esultof
DistributionCoefficientandSeparation
Factor
at298.15
Kand101.325kP
aa
initialmixtures
aqueousphase
organicphase
ρaρo
ω1
ω2
ω3
ω4
ω1
ω2
ω3
ω4
(g·mL−
1 )ω
1ω
2ω
3ω
4(g·mL−
1 )D
1D
2S 1
,2D
3S 1
,3
NaC
l=0.0in
InitialAqueous
Phase
1.99
0.00
48.11
49.90
3.99
0.00
94.80
1.21
1.0203
0.20
0.00
6.46
93.34
0.9762
0.0501
0.0681
0.7360
3.89
0.00
46.21
49.90
7.68
0.00
89.59
2.72
1.0424
0.45
0.00
6.68
92.87
0.9809
0.0581
0.0746
0.7792
5.88
0.00
44.22
49.90
11.05
0.00
87.30
1.65
1.0605
1.33
0.00
6.52
92.15
0.9837
0.1200
0.0747
1.6059
7.78
0.00
42.32
49.90
14.04
0.00
83.97
1.99
1.0814
2.38
0.00
6.68
90.94
0.9891
0.1696
0.0796
2.1316
9.77
0.00
40.33
49.90
17.78
0.00
81.98
0.24
1.1052
3.28
0.00
6.61
90.11
0.9964
0.1844
0.0807
2.2860
11.66
0.00
38.49
49.85
20.84
0.00
78.04
1.13
1.1278
4.00
0.00
5.66
90.34
1.0011
0.1920
0.0725
2.6466
NaC
l=0.03
inInitialAqueous
Phase
1.99
1.30
46.87
49.85
3.88
2.80
91.59
1.73
1.0405
0.26
0.01
6.17
93.57
0.9768
0.0664
0.0039
17.1514
0.0673
0.9860
3.89
1.30
44.91
49.90
7.44
2.62
89.36
0.58
1.0597
0.81
0.02
6.34
92.82
0.9816
0.1093
0.0083
13.1296
0.0710
1.5397
5.87
1.30
42.98
49.85
10.61
2.64
86.20
0.55
1.0835
1.83
0.05
6.14
91.98
0.9843
0.1727
0.0174
9.8995
0.0713
2.4228
7.78
1.30
41.02
49.90
14.08
2.46
82.47
1.00
1.1011
2.44
0.04
5.94
91.58
0.9926
0.1731
0.0179
9.6656
0.0721
2.4025
9.76
1.30
39.09
49.85
17.68
2.85
78.61
0.86
1.1204
3.05
0.08
5.75
91.12
0.9963
0.1726
0.0281
6.1493
0.0731
2.3590
11.67
1.30
37.13
49.90
20.30
2.77
76.37
0.56
1.1415
4.78
0.11
5.90
89.22
1.0042
0.2352
0.0389
6.0428
0.0772
3.0466
NaC
l=0.05
inInitialAqueous
Phase
1.99
2.50
45.62
49.90
3.89
4.95
90.18
0.98
1.0582
0.29
0.02
5.85
93.84
0.9776
0.0745
0.0036
20.4254
0.0648
1.1495
4.13
2.49
43.63
49.75
7.50
5.05
86.35
1.10
1.0814
1.16
0.05
6.08
92.71
0.9823
0.1548
0.0108
14.3216
0.0704
2.1995
5.88
2.50
41.73
49.90
10.53
5.21
83.29
0.98
1.1013
1.89
0.07
6.09
91.94
0.9890
0.1796
0.0139
12.9438
0.0731
2.4559
7.78
2.50
39.82
49.90
13.68
5.14
80.69
0.49
1.1196
2.90
0.10
5.96
91.03
0.9928
0.2119
0.0204
10.3946
0.0739
2.8670
9.76
2.49
37.90
49.85
16.67
5.74
77.41
0.18
1.1424
4.15
0.16
5.96
89.73
1.0006
0.2491
0.0279
8.9396
0.0770
3.2364
11.75
2.49
35.91
49.85
19.71
5.85
73.96
0.48
1.1623
5.38
0.21
5.73
88.68
1.0076
0.2729
0.0363
7.5222
0.0774
3.5240
NaC
l=0.08
inInitialAqueous
Phase
1.99
3.79
44.38
49.85
3.76
7.89
86.83
1.52
1.0822
0.33
0.04
4.87
94.77
0.9757
0.0872
0.0048
18.0132
0.0561
1.5553
3.89
3.79
42.42
49.90
7.00
7.90
84.07
1.03
1.1019
1.09
0.06
4.86
93.99
0.9806
0.1556
0.0081
19.2691
0.0577
2.6951
5.87
3.79
40.49
49.85
10.31
7.65
80.45
1.59
1.1210
1.94
0.10
5.18
92.77
0.9914
0.1880
0.0137
13.7572
0.0644
2.9174
7.78
3.79
38.52
49.90
13.03
7.74
77.66
1.57
1.1428
3.21
0.16
5.31
91.31
0.9959
0.2465
0.0210
11.7524
0.0684
3.6023
9.76
3.79
36.60
49.85
16.09
8.14
74.29
1.49
1.1613
4.57
0.23
5.81
89.38
1.0058
0.2844
0.0285
9.9774
0.0782
3.6356
11.67
3.79
34.63
49.90
19.36
7.89
71.24
1.51
1.1829
5.39
0.29
5.16
89.15
1.0096
0.2785
0.0372
7.4958
0.0725
3.8444
NaC
l=0.10
inInitialAqueous
Phase
1.99
4.99
43.12
49.90
3.72
10.48
84.19
1.60
1.1027
0.40
0.13
5.47
94.01
0.9767
0.1067
0.0120
8.9124
0.0650
1.6416
3.89
4.99
41.22
49.90
6.65
10.52
81.73
1.10
1.1203
1.45
0.18
5.44
92.93
0.9823
0.2182
0.0168
12.9688
0.0666
3.2780
5.87
4.99
39.29
49.85
9.50
10.56
79.24
0.69
1.1405
2.77
0.22
5.16
91.84
0.9893
0.2921
0.0208
14.0233
0.0652
4.4832
7.78
4.99
37.33
49.90
12.30
11.47
75.56
0.67
1.1608
3.97
0.29
5.23
90.51
0.9980
0.3229
0.0253
12.7843
0.0692
4.6636
9.77
4.99
35.34
49.90
14.88
11.46
72.70
0.96
1.1785
5.70
0.37
5.76
88.18
1.0061
0.3831
0.0321
11.9433
0.0792
4.8384
11.89
4.98
33.39
49.75
18.21
11.65
70.09
0.04
1.2046
7.00
0.48
5.23
87.30
1.0156
0.3841
0.0409
9.3863
0.0746
5.1466
NaC
l=0.13
inInitialAqueous
Phase
1.99
6.28
41.88
49.85
3.51
13.59
81.50
1.40
1.1150
0.56
0.18
4.96
94.40
0.9774
0.1600
0.0131
12.2481
0.0609
2.6276
3.89
6.29
39.92
49.90
6.36
13.71
78.35
1.58
1.1390
1.64
0.25
5.22
92.88
0.9824
0.2576
0.0184
14.0002
0.0667
3.8644
5.87
6.28
38.00
49.85
8.92
13.87
74.89
2.33
1.1651
3.14
0.28
5.17
91.41
0.9942
0.3525
0.0202
17.4429
0.0690
5.1074
Journal of Chemical & Engineering Data Article
dx.doi.org/10.1021/je400817m | J. Chem. Eng. Data XXXX, XXX, XXX−XXXC
∑γτ
ττ
=∑
∑+
∑−
∑
∑
⎛⎝⎜⎜
⎞⎠⎟⎟
G x
G x
G x
G x
G x
G xln i
j ji ji j
k ki k j
ij j
k ki kij
l li lj l
k ki k
NC
NC
NC
NC
NC
NC
(3)
Table
1.continued
initialmixtures
aqueousphase
organicphase
ρaρo
ω1
ω2
ω3
ω4
ω1
ω2
ω3
ω4
(g·mL−
1 )ω
1ω
2ω
3ω
4(g·mL−
1 )D
1D
2S 1
,2D
3S 1
,3
NaC
l=0.13
inInitialAqueous
Phase
7.86
6.28
36.01
49.85
11.60
14.67
72.35
1.38
1.1787
4.67
0.38
5.53
89.42
0.9998
0.4029
0.0257
15.6482
0.0765
5.2682
9.76
6.28
34.11
49.85
14.39
14.50
69.87
1.24
1.2009
6.02
0.46
5.57
87.94
1.0103
0.4186
0.0321
13.0558
0.0797
5.2511
11.66
6.28
32.21
49.85
16.87
14.61
66.97
1.55
1.2221
7.62
0.52
5.53
86.33
1.0194
0.4519
0.0357
12.6486
0.0825
5.4754
NaC
l=0.15
inInitialAqueous
Phase
1.99
7.49
40.63
49.90
3.34
16.17
78.75
1.73
1.1385
0.71
0.67
4.71
93.91
0.9787
0.2114
0.0417
5.0738
0.0598
3.5341
3.89
7.49
38.72
49.90
5.90
16.09
76.23
1.77
1.1555
2.04
0.29
4.74
92.93
0.9871
0.3460
0.0182
19.0106
0.0622
5.5651
5.88
7.49
36.74
49.90
8.44
16.38
73.28
1.90
1.1748
3.60
0.24
4.90
91.26
0.9964
0.4263
0.0147
29.0358
0.0669
6.3724
7.78
7.49
34.83
49.90
11.07
16.78
71.08
1.07
1.1953
5.06
0.17
4.93
89.83
1.0058
0.4572
0.0103
44.1695
0.0694
6.5860
9.76
7.48
32.91
49.85
13.32
17.36
67.89
1.43
1.2170
6.86
0.41
4.93
87.79
1.0162
0.5151
0.0238
21.6428
0.0727
7.0889
11.67
7.49
30.94
49.90
15.68
18.13
64.00
2.19
1.2400
8.24
0.91
4.64
86.22
1.0210
0.5253
0.0501
10.4866
0.0725
7.2481
aThe
standard
uncertaintyforu(ω)=0.01,u(T
)=0.05
Kandu(ρ)
=0.0001
g·mL−
1 .Figure 1. Distribution coefficient of phosphoric acid (D1) as a functionof phosphoric acid composition in the initial aqueous phase at 298.15K: ■, ω = 0 NaCl; □, ω = 0.03 NaCl; ●, ω = 0.05 NaCl; ○, ω = 0.08NaCl; ▲, ω = 0.10 NaCl; △, ω = 0.13 NaCl; ▼, ω = 0.15 NaCl.
Figure 2. Separation factor of sodium chloride (S1,2) as a function ofphosphoric acid composition in the initial aqueous phase at 298.15 K:□, ω = 0.03 NaCl; ●, ω = 0.05 NaCl; ○, ω = 0.08 NaCl; ▲, ω = 0.10NaCl; △, ω = 0.13 NaCl; ▼, ω = 0.15 NaCl.
Journal of Chemical & Engineering Data Article
dx.doi.org/10.1021/je400817m | J. Chem. Eng. Data XXXX, XXX, XXX−XXXD
τ = − =g g RT g g( )/ , ( )ji ji ii ji ij (4)
α τ α α= − =G exp( ), ( )ji ji ji ij ji (5)
τ τ= = 0ii jj (6)
= =G G 1ii jj (7)
− =g g B( )ji ii ij (8)
In eq 3, NC stands for the number of material, i stands for thecomponent (i = 1 for phosphoric acid, i = 2 for sodiumchloride, i = 3 for water).The interaction parameter for the NRTL model, in the
present work, the value of the nonrandomness is fixed at α =0.3, Bij is regressed using the firstOpt software. The regressedNRTL parameters of the quaternary system are shown in Table2 with the root-mean-square error (RMSE) values. The RMSEvalues are a measure of the agreement between the calculatedand the experimental data.
= Σ −N
x xRMSE1
( )i ical exp 2
(9)
In eq 6, N is the number of experimental data points. TheRMSE values for the experiments are < 0.01 when theexperimental data are regressed with the NRTL model.
4. CONCLUSIONSLiquid−liquid equilibrium data for the (H3PO4−NaCl−H2O−TBP) quaternary systems were obtained at T = (298.15) K andatmosphere pressure. With increasing content of phosphoricacid and sodium chloride, the distribution coefficient ofphosphoric acid increases. That is to say, the content ofphosphoric acid complexing with TBP is gradually increased.The separation factor of water increases with the increasecontents of phosphoric acid and sodium chloride, while theseparation factor of sodium chloride decreases after an increaseto a maximum value. The NRTL (α = 0.3) thermodynamicmodel is acceptably used to correlate the experimental liquid−liquid equilibrium data. It indicates that the model gives goodresult for the investigated system.
■ AUTHOR INFORMATION
Corresponding Author*E-mail: [email protected]. Tel.: (0086 0951) 3951036.Fax: (0086 0951) 3951036. Address: Department of Chemistryand Chemical Engineering, Ningxia University, No.539,Helanshan Road, Xixia District, Yinchuan, 750021, PR China.
NotesThe authors declare no competing financial interest.
■ NOMENCLATURE
Bij, coefficient as defined in eq 8; D1, distribution coefficient ofphosphoric acid; Di, distribution coefficient of material i; Di
a,distribution coefficient of material i in the aqueous phase; Di
o,distribution coefficient of material i in the organic phase; gij,energies of interaction between an i−j pair of molecules; Gij,coefficient as defined in eq 5; N, number of tie-lines; NC,number of molecules; R, gas constant; RMSE, root-mean-square error; T, absolute temperature; xi, overall mole fractionof substance i; xi
cal, calculated mole fraction; xiexp, experimental
mole fraction
Greek Lettersαij, nonrandomness constant for binary ij interaction; γ, activitycoefficient; τji, coefficient as defined in eq 4
Subscripti, component i
Figure 3. Separation factor of water (S1,3) as a function of phosphoricacid composition in the initial aqueous phase at 298.15K: ■, ω = 0NaCl; □, ω = 0.03 NaCl; ●, ω = 0.05 NaCl; ○, ω = 0.08 NaCl; ▲, ω= 0.10 NaCl; △, ω = 0.13 NaCl; ▼, ω = 0.15 NaCl.
Table 2. Quaternary System in the Different SodiumChloride Concentrations of Binary Interaction Parametersof the NRTL Equation
i j Bij Bji 108 RMSE
NaCl = 0.0 in the Initial Aqueous Phase1 2 171.41 512.96 0.0011 3 406.24 0.00242 3 −1046.27 252.63
NaCl = 0.03 in the Initial Aqueous Phase1 2 87.77 386.98 2.851 3 91.26 −53.842 3 −328.22 164.55
NaCl = 0.05 in the Initial Aqueous Phase1 2 −141.72 386.68 12.51 3 96.78 −2.902 3 1020.66 10.79
NaCl = 0.08 in the Initial Aqueous Phase1 2 100.76 17.71 0.131 3 300.72 −1.142 3 262.33 −106.33
NaCl = 0.10 in the Initial Aqueous Phase1 2 −108.14 274.05 8.911 3 −313.12 35.302 3 29.61 −0.79
NaCl = 0.13 in the Initial Aqueous Phase1 2 9.69 208.78 7.511 3 −152.87 193.192 3 675.52 0.56
NaCl = 0.15 in the Initial Aqueous Phase1 2 −76.47 155.82 2.551 3 119.10 −10.562 3 986.12 −0.024
Journal of Chemical & Engineering Data Article
dx.doi.org/10.1021/je400817m | J. Chem. Eng. Data XXXX, XXX, XXX−XXXE
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Journal of Chemical & Engineering Data Article
dx.doi.org/10.1021/je400817m | J. Chem. Eng. Data XXXX, XXX, XXX−XXXF