Solubilities, Densities, Refractive Indices, and pH Values of the

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Solubilities, Densities, Refractive Indices, and pH Values of the Aqueous Ternary Systems (LiCl + LiB5O8 + H2O) and (Li2SO4 + LiB5O8 + H2O) at 288.15 K and 101 kPa Yan Li, Shangqing Chen, Fei Yuan, Sen Sun, Yafei Guo,* and Tianlong Deng

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Tianjin Key Laboratory of Marine Resources and Chemistry, College of Chemical Engineering and Materials Science, Tianjin University of Science and Technology, Tianjin 300457, PR China ABSTRACT: Solubilities, densities, refractive indices, and pH values of the ternary systems (LiCl + LiB5O8 + H2O) and (Li2SO4 + LiB5O8 + H2O) at 288.15 K and 101 kPa were studied using the isothermal dissolution method and wet residue method. From the experimental data, the phase diagrams and the diagrams of the physicochemical properties including density, refractive index, and pH value against composition were plotted. The results show that the two systems belong to a simple saturation type, and no double salt or solid solution formed at 288.15 K. For the two systems, there are both in one invariant point, two isothermal dissolution curves, and two crystallization regions including lithium pentaborate pentahydrate (LiB5O8·5H2O, Lb5), lithium chloride dihydrate (LiCl·2H2O, Lc2, in the former), and lithium sulfate monohydrate (Li2SO4·H2O, Ls1, in the latter). It was found that the area of the crystallization region of Lb5 was larger than those of Lc2 in the former system and Ls1 in the latter system, and the results indicated that the solubility of lithium pentaborate was lower in the two systems. The densities and refractive indices in the two ternary systems at 288.15 K increased first and then decreased with the increase in LiCl and Li2SO4 concentrations in the solution. However, the pH values present a contrary trend, which decreased first and then increased. The calculated values of density and refractive index using empirical equations for the two ternary systems agree well with the experimental values.

1. INTRODUCTION

To establish the complex systems, some salt−water subsystems have been studied in the literature, including (LiBO2 + CaB2O4 + H2O) at 288.15 and 298.15 K,6 (Li2B4O7 + Li2SO4 + H2O) at 298.15 K,7 and (Li2SO4 + Li2B4O7 + H2O) and (K2SO4 + K2B4O7 + H2O) at 288.15 K.8 However, borates can exist in aqueous solution with several species, such as monoborate (BO2−), tetraborate (B4O72−), pentaborate (B5O8−), hexaborate (B6O102−), and so on, and the dissolving behavior of borate is very complicated.9 To the best of our knowledge, there are limited reports on the phase equilibria and phase diagrams concerning lithium pentaborate.10 Therefore, the isothermal solubilities and the relevant solution physicochemical properties including densities, refractive indices, and pH values for the two ternary systems (LiCl + LiB5O8 + H2O) and (Li2SO4 + LiB5O8 + H2O) at 288.15 K were proposed in this paper.

With the continuously growing applications of lithium-based products in the field of rechargeable batteries, electric vehicles, and nuclear fusion, the lithium requirements are increasing rapidly.1,2 Generally, lithium can be obtained from two major sources: solid mineral resources mainly including spodumene and petalite and liquid mineral resources such as salt lake brines and underground waters.3 Moreover, lithium resources in salt lake brines and underground waters often coexisted with other scattered and valuable elements such as borates, which are widely used in metallurgy, chemical industry, light industry, nuclear industry, agriculture, and new high-tech materials.4 In view of limited available ores and complex extraction process, salt lake brines are regarded as the most promising raw materials for lithium and borates production. Salt lake brines as a treasure house of lithium resources are widely distributed in Bolivia, Chile, Argentina, and China. Generally, the major chemical components of salt lake brines belong to the complex salt−water system (Li+, Na+, K+, Ca2+, Mg2+//Cl−, SO42−, borate−H2O).5 To exploit the valuable salt lake brines sustainably and economically, the phase equilibria and phase diagrams play an important role in describing physicochemical process of brines and guide the effective development and utilization of resources. © XXXX American Chemical Society

2. EXPERIMENTAL SECTION 2.1. Reagents. The reagents used through this experiment were analytical grade and are listed in Table 1. Double distilled water (DDW) with pH = 6.6 and conductivity of 2 × 10−6 S· Received: February 1, 2019 Accepted: June 20, 2019

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DOI: 10.1021/acs.jced.9b00118 J. Chem. Eng. Data XXXX, XXX, XXX−XXX

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Table 1. Reagents Used in This Study chemical

CAS reg. no.

initial mass fraction purity

purification method

final mass fraction purity

analysis method

LiCla Li2SO4a H3BO3a LiOH·H2Ob LiB5O8·5H2Oc

7447-41-8 10377-48-7 1043-35-3 1310-66-3

0.98 0.99 0.99 0.98 0.98

recrystallization recrystallization recrystallization recrystallization recrystallization

0.998 0.996 0.995 0.992 0.995

titration for Cl− gravimetric method for SO42− gravimetric method for borate titration for OH− gravimetric method for borate

a

From Sinopharm Chemical Reagent Co., Ltd. bFrom Macklin Biochemical Co., Ltd. cSynthesized in this work.

Figure 1. X-ray diffraction pattern of lithium pentaborate pentahydrate (LiB5O8·5H2O, Lb5).

m−1 at 298.15 K was used in this work. Lithium pentaborate pentahydrate (LiB5O8·5H2O) was synthesized by boric acid and lithium hydroxide monohydrate in our laboratory according to the literature11 and verified by X-ray powder diffraction and chemical analysis. The XRD pattern of LiB5O8· 5H2O is shown in Figure 1, and the results indicated that the synthesized lithium pentaborate pentahydrate was available for further experiments. 2.2. Apparatus. A magnetic stirring thermostatic bath (HXC-500-12A, Beijing Fortune Joy Science Technology Co., Ltd., China) was used to control the temperature with a precision of 0.01 K. The densities (ρ) were measured by a vibrating tube densitometer (DMA4500, Anton Paar, Austria) with an uncertainty of 0.5 mg·cm−3. The refractive indices (nD) were measured by a refractometer (Abbemat 550, Anton Paar, Austria) with an uncertainty of ±0.0003. Before the experiment, the Abbe refractometer and densitometer should be calibrated at 298.15 K. The Abbe refractometer was calibrated with free-CO2 fresh DDW, and the deviation between the experimental and reference value was within 0.05%.12 The densitometer was calibrated with dry air and DDW, and the deviation between the experimental and reference data was within 0.003%.12 The pH values were determined by a highprecision pH meter (pH 7310, WTW Co., Ltd., Germany) with an uncertainty of ±0.01, which was calibrated with pH of 4.01, 7.00, and 10.01 standard solutions. An X-ray powder diffractometer equipped with Cu Kα radiation over a 2θ range of 10−70° and X-ray power of 36 kV/20 mA (MSAL XD-3, Beijing Purkinje General Instrument Co., Ltd., China) was used to identify the crystal structures of solid phases. 2.3. Experimental Method. The solid−liquid phase equilibrium experiment was studied using the isothermal

dissolution equilibrium method and the wet residue method.13 At first, a series of samples for the ternary system were prepared by adding different ratios of the crystallized solid salts of lithium chloride/lithium sulfate, lithium pentaborate pentahydrate, and DDW in a series of sealed hard polyethylene bottles then placed in the magnetic stirring thermostat and kept under stirring at a speed of 150 rpm to accelerate the solid−liquid phase equilibria. The temperature of the bath was set at 288.15 ± 0.01 K. To ensure the thermodynamic phase equilibria in a series of sealed hard polyethylene bottles, the clarified liquid-phase samples were taken out for chemical analysis in a certain interval (such as 7 days). For the chemical analytical results at each interval, when the relative errors of the compositions of the liquid-phase samples, that is, the concentration of Cl− at different times measured by titration was within 0.3% or the concentrations of SO42− and B5O8− analyzed by gravimetric analysis were both within 0.05%, in other words, the composition of the liquid phase remained constant; it indicated that the dissolved phase equilibrium in each bottle was reached. Then, the magnetic stirrer was turned off, and the bottles were suspended for 4 h to separate the liquid and solid phases. The supernatant was taken for the chemical composition analysis and the physicochemical properties including refractive index (nD), density (ρ), and pH value measurements. Generally, 90 days is needed for the solid−liquid phase equilibrium of pentaborate-containing systems. The wet residue of the solid phase with a small amount of liquid was sampled and quantitatively weighted into the volumetric flask filled with DDW for the chemical analysis. In addition, the equilibrium solid phase was identified combining the results of chemical analysis for the wet residue samples and further identification with XRD. B

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Table 2. Solubility, Density, and Refractive Index of the Binary Systems (LiCl + H2O) and (Li2SO4 + H2O) at 288.15 K and 101 kPaa solubility in water 100 wBb

binary system LiCl + H2O

solid phase

43.95 43.95 43.95 25.98 25.96 26.01 26.01

Li2SO4 + H2O

ρ (g·cm−3)

LiCl·2H2O

1.2870 -c 1.2832 1.2376 1.2466 1.2375 1.2382

Li2SO4·H2O

nD

literature

1.4744 1.4320 -c 1.3788 -c 1.3776

16 17 this work 16 18 19 this work

c

a

Standard uncertainties u are u(T) = 0.01 K and u(p) = 5 kPa. u(w) for LiCl and Li2SO4 are 0.004 and 0.0006 in mass fraction, and u(x) for nD and ρ are 0.0003 and 0.5 mg·cm−3 in this work. bw, mass fraction. cNo data reported.

Table 3. Solubility and Physicochemical Properties of the Ternary System (LiCl + LiB5O8 + H2O) at 288.15 K and 101 kPaa physicochemical properties composition of liquid phase 100 wBb

composition of wet residue 100 wB

no.

LiCl

LiB5O8

LiCl

1, A1 2 3 4, E1 5 6 7 8 9 10 11, B1

43.95 43.83 43.64 43.30 39.35 33.34 27.21 23.21 11.44 8.18 0.00

0.00 0.51 0.88 2.27 1.26 0.71 0.72 0.80 2.35 3.44 11.84

-d 49.31 48.23 42.63 -d -d -d -d -d -d -d

ρ (g·cm−3)

LiB5O8 experimental -d 0.23 0.50 6.50 -d -d -d -d -d -d -d

1.2832 1.2877 1.2922 1.3011 1.2698 1.2121 1.1684 1.1434 1.0842 1.0732 1.0914

nD

calculated

relative error (%)

experimental

calculated

relative error (%)

1.2832 1.2872 1.2894 1.3003 1.2618 1.2144 1.1728 1.1471 1.0852 1.0740 1.0914

0.00 −0.04 −0.22 −0.06 −0.63 0.19 0.38 0.32 0.09 0.07 0.00

1.4320 1.4327 1.4339 1.4351 1.4270 1.4086 1.3937 1.3848 1.3615 1.3562 1.3519

1.4320 1.4325 1.4327 1.4342 1.4234 1.4087 1.3948 1.3858 1.3621 1.3566 1.3519

0.00 −0.01 −0.08 −0.06 −0.25 0.00 0.07 0.08 0.05 0.04 0.00

pH 4.72 2.27 1.52 0.89 1.53 4.22 -d 5.67 6.43 6.50 7.03

equilibrium solid phasec Lc2 Lc2 Lc2 Lc2 + Lb5 Lb5 Lb5 Lb5 Lb5 Lb5 Lb5 Lb5

Standard uncertainties u are u(T) = 0.01 K and u(p) = 5 kPa. u(w) for LiCl and LiB5O8 are 0.004 and 0.0006 in mass fraction, and u(x) for nD, ρ, and pH are 0.0003, 0.5 mg·cm−3, and 0.01, respectively. bw, mass fraction. cLc2, LiCl·2H2O; Lb5, LiB5O8·5H2O. dNot determined. a

Figure 2. Phase diagram of the ternary system (LiCl + LiB5O8 + H2O) at 288.15 K and 101 kPa. Lc2, LiCl·2H2O; Lb5, LiB5O8·5H2O; left-pointing solid triangle, experimental points; left-pointing open triangle, experimental Schreinemakers points; , solubility curve; ----, Schreinemakers curve. (a) Phase diagram. (b) Part enlargement of Schreinemakers lines.

1.22.14 The concentration of B5O8− was determined using gravimetric method of mass titration in the presence of joint indicator of methyl red with an uncertainty of ±0.0005 in mass fraction.15 Frankly, the concentration of Li+ could be obtained by ion balance; in our work, it was also evaluated by the instrumental analysis of ICP-OES (Prodigy, Leeman Corporation, America) with an uncertainty of ±0.02 in mass fraction further. So, according to the analytical data on the

2.4. Analytical Methods. The compositions of LiCl, Li2SO4, and LiB5O8 in the solution were calculated via the chemical analytical results of Cl−, SO42−, and B5O8−. In other words, the concentration of Cl− was analyzed by titration using the standard mercuric nitrate (pH = 3.0 to 3.5) using diphenyl carbazone as the indicator with an uncertainty of ±0.003 in mass fraction.14 The concentration of SO42− was analyzed by gravimetric analysis with barium sulfate precipitation at pH = C

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Figure 3. Physicochemical properties versus composition of lithium chloride concentration in the ternary system (LiCl + LiB5O8 + H2O) at 288.15 K and 101 kPa. Red and black solid squares, experimental points at 288.15 K. (a) Density and refractive index versus LiCl composition. (b) pH versus LiCl composition.

Table 4. Solubility and Physicochemical Properties of the Ternary System (Li2SO4 + LiB5O8 + H2O) at 288.15 K and 101 kPaa physicochemical properties liquid phase composition 100 wBa

ρ (g·cm−3)

nD

no.

Li2SO4

LiB5O8

experimental

calculated

relative error (%)

experimental

calculated

relative error (%)

pH

equilibrium solid phasec

1, A2 2 3 4, E2 5 6 7 8 9, B2

26.01 25.19 25.12 24.90 16.95 10.30 5.88 3.06 0.00

0.00 1.34 0.82 2.10 3.82 5.65 7.18 9.20 11.84

1.2382 1.2378 1.2384 1.2398 1.1817 1.1305 1.1056 1.0951 1.0914

1.2382 1.2422 1.2367 1.2463 1.1823 1.1346 1.1065 1.0975 1.0914

0.00 0.36 −0.14 0.53 0.05 0.36 0.08 0.22 0.00

1.3776 1.3782 1.3782 1.3786 1.3682 1.3591 1.3546 1.3526 1.3519

1.3776 1.3783 1.3774 1.3790 1.3681 1.3596 1.3546 1.3530 1.3519

0.00 0.01 −0.06 0.04 −0.01 0.04 −0.00 0.03 0.00

8.51 6.99 7.54 6.50 6.79 6.87

Ls1 Ls1 Ls1 Ls1 + Lb5 Lb5 Lb5 Lb5 Lb5 Lb5

-d 7.02 7.03

a

Standard uncertainties u are u(T) = 0.01 K and u(p) = 5 kPa. u(w) for Li2SO4 and LiB5O8 are 0.0006 and 0.0006 in mass fraction, and u(x) for nD, ρ, and pH are 0.0003, 0.5 mg·cm−3, and 0.01, respectively. bw, mass fraction. cLs1, Li2SO4·H2O; Lb5, LiB5O8·5H2O. dNot determined.

concentrations of B5O8−, Cl−, and SO42− in the solution, the LiB5O8, LiCl, and Li2SO4 contents were calculated with uncertainties of ±0.0006, ± 0.004, and ± 0.0006 in mass fraction, respectively.

to hydrate type I. Solubilities of single salts LiCl and LiB5O8 in the liquid phase were 100w(LiCl) = 43.95 in point A1 and 100w(LiB5O8) = 11.84 in point B1. The compositions of point E1 cosaturated with two salts of LiB5O8 and LiCl in 100w are 2.27 and 43.30, respectively. To further identify the crystallization hydrate of the equilibrium solid-phase LiCl in E1, the wet residue method (i.e., Schreinemakers rule) was used. As to the wet residue method,13 the solid-phase position is located in the cross point of a series of extending lines, which lines are connected to the composition points between equilibrium liquid phases and the corresponding composition points of wet residues. As indicated in Figure 2b, the dashed lines cross through the position of the solid-phase lithium chloride as in the form of Lc2, which agrees with the literature.20 The area of the crystallization region of Lb5 is much larger than that of Lc2, and the results demonstrate that the solubility of lithium chloride is much higher than that of lithium pentaborate. Figure 3 shows the relationship between the physicochemical properties including densities (ρ), refractive indices (nD), and pH value against the composition of lithium chloride in the ternary system (LiCl + LiB5O8 + H2O) at 288.15 K. The densities (ρ) and refractive indices (nD) in Figure 3a have the same varying trend. Both of them increased first along with curve B1E1 to reach the maximum values of 1.3011 g·cm−3 and 1.4351 at the invariant point E1 and then decreased along with

3. RESULTS AND DISCUSSION A comparison on the binary systems (LiCl + H2O) and (Li2SO4 + H2O) at 288.15 K between this work and the literature is presented in Table 2.16−19 It could be found that the experimental results in this work agree well with the literature and that indicated our experimental procedure and analysis are reliable. 3.1. Phase Diagram of the Ternary System (LiCl + LiB5O8 + H2O). The solubility data and physicochemical properties of the ternary system (LiCl + LiB5O8 + H2O) at 288.15 K are listed in Table 3. The compositions of the equilibrium liquid phase were expressed in mass fraction. According to solubility date in Table 3, the ternary system phase diagram is drawn in Figure 2a, and Figure 2b is the part enlargement. In Figure 2a,b, there are two crystallizations regions corresponding to lithium chloride dihydrate (LiCl·2H2O, Lc2) and lithium pentaborate pentahydrate (LiB5O8·5H2O, Lb5), two isothermal dissolution curves A1E1 of Lc2 and B1E1 of Lb5, and one invariant point E1 (Lc2 + Lb5). No solid solution and double salt were found, and this system belonged D

DOI: 10.1021/acs.jced.9b00118 J. Chem. Eng. Data XXXX, XXX, XXX−XXX

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Figure 4. Phase diagram of the ternary system (Li2SO4 + LiB5O8 + H2O) at 288.15 K and 101 kPa. L, equilibrium liquid phase; Ls1, Li2SO4·H2O; Lb5, LiB5O8·5H2O. ■, experimental points; , solubility curve. (a) Phase diagram. (b) Part enlargement.

Figure 5. X-ray diffraction pattern of the invariant point E2 (Li2SO4·H2O + LiB5O8·5H2O) for the ternary system (Li2SO4 + LiB5O8 + H2O) at 288.15 K.

Figure 6. Physicochemical properties versus composition of lithium sulfate concentration in the ternary system (Li2SO4 + LiB5O8 + H2O) at 288.15 K and 101 kPa. Red and black solid squares, experimental points at 288.15 K. (a) Density and refractive index versus Li2SO4 composition. (b) pH versus Li2SO4 composition.

E1A1 with the increase in the lithium chloride concentration in the solution. The minimum value of pH is 0.89 at the invariant point E1.

curve E1A1. As to pH in this ternary system, there is an opposite trend in Figure 3b, that is, the pH values decreased first along with curve B1E1 and then increased along with curve E

DOI: 10.1021/acs.jced.9b00118 J. Chem. Eng. Data XXXX, XXX, XXX−XXX

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3.2. Phase Diagram of the Ternary System (Li2SO4 + LiB5O8 + H2O). The solubility data and physicochemical properties of the ternary system (Li2SO4 + LiB5O8 + H2O) at 288.15 K are presented in Table 4, and the corresponding phase diagram was plotted in Figure 4. In Figure 4a,b, there are two crystallization regions including lithium sulfate monohydrate (Li2SO4·H2O, Ls1) and lithium pentaborate pentahydrate (LiB5O8·5H2O, Lb5), two isothermal dissolution curves A2E2 and B2E2, and one invariant point E2 cosaturated with two solid phases of Li2SO4·H2O and LiB5O8·5H2O, that is, Ls1 + Lb5. Solubilities of two single salts LiB5O8 and Li2SO4 with mass fractions corresponding to 100w(Li2SO4) = 26.01 (A2) and 100w(LiB5O8) = 11.84 (B2). At the invariant point E2, the compositions in the liquid phase are 100w(LiB5O8) = 2.10 and 100w(Li2SO4) = 24.90, and the XRD pattern of E2 is shown in Figure 5, which verified the cosaturation solid phases of (Li2SO4·H2O + LiB5O8·5H2O). In addition, the area of the crystallization region of Lb5 is much larger than that of Ls1. Figure 6 shows the relationships between the physicochemical properties including densities, refractive indices, and pH values versus the concentration of lithium chloride in the ternary system (Li2SO4 + LiB5O8 + H2O) at 288.15 K. In Figure 6a, the densities (ρ) and refractive indices (nD) have a similar varying trend, that is, they increased first along with curve B2E2 and then decreased from E2 to A2 and reached the maximum values of 1.2398 g·cm−3 and 1.3785 at the invariant point E2 with the increase in the lithium chloride concentration in the solution. Nevertheless, Figure 6b shows the pH values that present a contrary trend, which decreased first and then increased after reaching the minimum values of 6.50 at the invariant point E2. Compared with the ternary system (LiCl + LiB5O8 + H2O), it was found that the content of LiB5O8 gradually decreased with the increasing mass fraction of LiCl and Li2SO4 in the solution, which was more markedly in the latter system, indicating a stronger salting-out effect of Li2SO4 on LiB5O8. These results may provide a theoretical basis for the separation and purification of pentaborates from borate-containing brines. 3.3. Calculated Densities and Refractive Indices. The empirical equations of the density and refractive index in electrolytes developed in the previous study have been widely used, which can be used for the predictions of density and refractive index in the solid−liquid phase equilibrium saturated solution.21 The following empirical equations for the density and refractive index were adopted to correlate the experimental results ρ = ∑ Ai wi ln ρ0 ln

nD = nD0

in the ternary system at 298.15 K. So, the constants of Ai for LiB5O8, LiCl, and Li2SO4 are calculated to be 0.00746, 0.00569, and 0.00825, respectively, and the constants Bi for LiB5O8, LiCl, and Li2SO4 are 0.00117, 0.00162, and 0.00125, respectively. wi is the salt of i in the solution with mass percentage. The calculated densities and refractive indices for the two ternary systems at 288.15 K are presented in Tables 3 and 4, respectively. Comparisons between the calculated and the experimental data on densities and refractive indices are also shown in Tables 3 and 4, and the maximum relative errors for the densities and refractive indices were less than 0.63 and 0.25%, respectively. The calculated values agree well with the experimental data, and it indicates that the experimental results obtained in this work are reliable and can provide fundamentals for further studies on more complicated systems containing lithium compounds.

4. CONCLUSIONS The solubilities and physicochemical properties including densities, refractive indices, and pH values for the two ternary systems (LiCl + LiB5O8 + H2O) and (Li2SO4 + LiB5O8 + H2O) at 288.15 K were determined with the isothermal dissolution equilibrium method and wet residue method. In the ternary systems (LiCl +LiB5O8 + H2O) and (Li2SO4 + LiB5O8 + H2O), there are, both in one invariant points, two isothermal dissolution curves and two crystallization regions of LiCl·2H2O and LiB5O8·5H2O in the former system as well as Li2SO4·H2O and LiB5O8·5H2O in the latter system. The area of the crystallization region of LiB5O8·5H2O is larger in both two ternary systems, which indicates that lithium pentaborate has lower solubility compared with lithium chloride and lithium sulfate. Densities, refractive indices, and pH values in the two ternary systems at 288.15 K increased at first and then decreased with the concentration increase of LiCl and Li2SO4. The pH value decreased first and then increased with the concentration increase of LiCl and Li2SO4. Conclusively, phase equilibria and phase diagrams of the ternary systems at 288.15 K could not only replenish the salt−water system database but also provide a theoretical foundation for the development and utilization of lithium resources in salt lake brines.

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AUTHOR INFORMATION

Corresponding Author

*E-mail: [email protected]. Tel/Fax: +86 22-60601156. ORCID

Yafei Guo: 0000-0003-0698-3565 Funding

The authors gratefully acknowledge the partial financial support from the National Natural Science Foundation of China (U1607123 and 21773170), the Key Projects of Natural Science Foundation of Tianjin (18JCZDJC10040), the Innovative Research Team in Tianjin Universities (TD135008), and the Yangtze Scholars and Innovative Research Team of the Chinese University (IRT_17R81).

∑ Bi wi

where ρ and ρ0 refer to the densities of the solution and the pure water at the same temperature, respectively, and the ρ0 value of the pure water at 288.15 K is 0.99909 g cm−3.22 nD and nD0 refer to the refractive indices of the solution and the pure water at the same temperature, respectively, and the nD0 value of the pure water at 288.15 K is 1.33339.22 Ai and Bi are the constants for the ith component in the ternary systems, and they can be easily obtained from the densities or refractive indices at the cosaturated point in the each boundary binary systems (LiB5O8 + H2O), (LiCl + H2O), and (Li2SO4 + H2O)

Notes

The authors declare no competing financial interest.

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REFERENCES

(1) Grosjean, C.; Miranda, P. H.; Perrin, M.; Poggi, P. Assessment of world lithium resources and consequences of their geographic

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DOI: 10.1021/acs.jced.9b00118 J. Chem. Eng. Data XXXX, XXX, XXX−XXX