Article Cite This: J. Chem. Eng. Data XXXX, XXX, XXX−XXX
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Studies on Phase Equilibria in the Quaternary Systems LiCl−KCl− MgCl2−H2O and Li2B4O7−Na2B4O7−MgB4O7−H2O at 273 K Lei Yang,† Xiao-Feng He,† Yun-Yun Gao,† Rui-Zhi Cui,† and Shi-Hua Sang*,†,‡ †
College of Materials and Chemistry and Chemical Engineering, Chengdu University of Technology, Chengdu 610059, China Mineral Resources Chemistry Key Laboratory of Sichuan Higher Education Institutions, Chengdu 610059, China
‡
ABSTRACT: The stable phase equilibria of the quaternary systems LiCl−KCl−MgCl2−H2O and Li2B4O7−Na2B4O7− MgB4O7−H2O at 273 K were studied using isothermal stable equilibrium method and the solubilities of the salts in the systems were also determined in turn. According to the experimental data and the corresponding equilibrium solid phases, the isothermal solubility diagrams, water content diagrams about two systems at 273 K were plotted, respectively. The first system has two double salts LiCl· MgCl2·7H2O and KCl·MgCl2·6H2O at 273 K, and its isothermal phase diagram of this system includes three invariant points, seven univariate curves, and five crystalline areas, those are LiCl·2H2O, MgCl2·6H2O, KCl, LiCl·MgCl2·7H2O and KCl·MgCl2·6H2O, respectively. The second system has no complex salt or solid solution and the system belongs to a simple cosaturated type, and its stable phase diagram is constituted by an invariant point, three univariant solubility curves, and three solid phase crystalline regions, where the three solid phases crystalline regions are Li2B4O7·3H2O, K2B4O7·4H2O, and MgB4O7·9H2O, respectively. equilibria of the quaternary system LiCl−NaCl−Li2B4O7− Na2B4O7−H2O18 at multiple temperatures have been studied, and the stable phase equilibria of the quaternary systems Li 2 B 4 O 7 −K 2 B 4 O 7 −MgB 4 O 7 −H 2 O, 19 Li 2 B 4 O 7 −Na 2 B 4 O 7 − K2B4O7−H2O,20 and Na2B4O7−K2B4O7−MgB4O7−H2O21 at 288 K were systematically researched. In addition, metastable phase equilibria of the systems LiCl−NaCl−Li 2B 4O 7− Na2B4O7−H2O22 and Li2B4O7−Na2B4O7−K2B4O7−H2O23 at 273 K, Li2B4O7−Na2B4O7−MgB4O7−H2O24 at 288 K have also been reported. The temperature of the Qinghai Tibet Plateau in winter is low, and the stable phase equilibria of quaternary systems LiCl−KCl−MgCl2−H2O and Li2B4O7−Na2B4O7−MgB4O7− H2O at 273 K have not been reported. Therefore, the study of phase equilibria of these two systems not only has a certain theoretical significance for studying the interaction of salts in salt lakes but also provides the relevant phase equilibrium data for the comprehensive utilization of salt lake brine resources.
1. INTRODUCTION China is rich in brine resources, mainly distributed in the salt lake brines in arid areas and semiarid areas such as the QinghaiTibet Plateau. The Qinghai-Tibet Plateau salt lake brine belongs to Li+, Na+, K+, Mg2+//Cl−, SO42−, borate-H2O system. The study of this complex water-salt system can not only provide scientific basis for effective development of salt lake resources but also have practical significance for the extraction of lithium, boron, and potassium from natural brines.1,2 There have been a lot of researches about its related subsystems carried out by many scholars. The phase equilibria in the ternary system LiCl−MgCl2− H2O at 273 K,3 288.15 K4 and 348 K5 have been studied. Li used ion-interaction model to predict the solubility data of the ternary system MgCl2−LiCl−H2O at 273 and 293 K, and made a corresponding comparison with the experimental data.6 The stable phase equilibria of the ternary system KCl−MgCl2−H2O at 273,7 308,8 and 348 K9 and the metastable phase equilibria of the same system at 323 K10 have been reported. For the ternary system LiCl−KCl−H2O, it has been studied as early as in the 1960s. The stable phase equilibria in the quaternary system LiCl−KCl−MgCl2−H2O at 298 K,11 323 K,12 and the metastable phase equilibria in the same system at 323 K13 have been reported. For the systems containing borate salts, there many related phase equilibria that have been reported recently. The studies of the phase equilibria in the ternary systems Li2B4O7− MgB4O7−H2O at 27314 and 298 K15 and Li2B4O7−Na2B4O7− H2O at 28816 and 298 K17 have been reported. The phase © XXXX American Chemical Society
2. EXPERIMENTAL SECTION 2.1. Apparatus and Reagents. A standard analytical balance with a capacity of 110 g and a resolution of 0.0001 g (the Mettler Toledo Instruments Co., Ltd.; AL104 type) was used to quantify the weights of the samples. The equipment (Sichuan ULUPURE Ultrapure Technology Co., Ltd.; UPT-IIReceived: September 7, 2017 Accepted: March 6, 2018
A
DOI: 10.1021/acs.jced.7b00800 J. Chem. Eng. Data XXXX, XXX, XXX−XXX
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Table 1. Chemical Reagents chemical name
purity
CAS
source
lithium chloride anhydrous (LiCl) potassium chloride (KCl) magnesium chloride hexahydrate (MgCl2·6H2O) lithium tetraborate anhydrous (Li2B4O7) sodium tetraborate anhydrous (Na2B4O7) hungchaoite (MgB4O7·9H2O) magnesium oxide (MgO) boric acid (H3BO3)
0.985 0.995 0.995 0.995 0.995 0.99 0.99 0.995
7447−41-8 7447-40-7 7791-18-6 12007-60-2 1330-43-4
Chengdu Kelong Chemical Reagent Manufactory Chengdu Kelong Chemical Reagent Manufactory Chengdu Kelong Chemical Reagent Manufactory Sinopharm Chemical Reagent Co.,Ltd. Chengdu Kelong Chemical Reagent Manufactory Synthesized in Laboratory Chengdu Kelong Chemical Reagent Manufactory Chengdu Kelong Chemical Reagent Manufactory
1309-48-4 10043-35-3
analysis method chemical chemical chemical chemical chemical chemical chemical chemical
titration titration titration titration titration titration titration titration
method method method method method method method method
Figure 1. X-ray diffraction photograph of the synthesized MgB4O7·9H2O.
298 K water bath for 3 h when the solution was turbid. Stop stirring until the solution was completely clear, then filter the sample to remove the insoluble matter. After that the filtrate was placed in a beaker, stirring was continued in a constant 298 K water bath until a large amount of white precipitate appeared. The X-ray diffraction photograph of the synthesized product can be seen in Figure 1. 2.2. Analytical Methods.27 The concentrations of lithium ion (Li+) and sodium ion (Na+) were measured by the atomic absorption spectrophotometer method. The concentration of potassium ion (K+) concentration was determined by titration with sodium tetraphenyl borate−hexadecyl trimethylammonium bromide. The concentration of magnesium ion (Mg2+) was determined at pH = 10 using EDTA titration method with Eriochrome Black-T as the indicator. The concentration of chloride ion (Cl−) was determined by AgNO3 titration using K2CrO4 as indicator. The concentration of borate ion (B4O72−) was measured using basic titration in the presence of mannitol. The equilibrium solid phase was identified by chemical analysis and X-ray diffraction photograph.
20T) was used to produce deionized water. An SHH-250 incubator with ±0.1 K uncertainty (Chongqing Yingbo Experimental Instrument Co., Ltd.) was used to control the temperature at 273 ± 0.1 K. A 1010AB electrothermal blowing drybox (Beijing Zhongxing Weiye Instrument Co., Ltd.) was employed to dry the solid samples. An oscillator (HY-5, supplied by the Jintan Kexi Instrument Co., Ltd.) was employed for accelerating equilibration of the samples. The GGX-9A atomic absorption spectrophotometer was applied to measure the concentrations of the samples. The crystal structures of the solid phases at invariant points were identified by a DX-2700 X-ray diffraction analyzer (Dandong Fangyuan Instrument Co., Ltd.). The deionized water with an electrical conductivity less than 1 × 10−5 s·m−1 and pH = 6.60 was used in the experiments. The sources and purities of the chemical reagents used in the experiments are shown in Table 1. Experimental Method. The stable phase equilibria were determined by isothermal dissolution equilibrium method.25 The samples were placed in an oscillator which was put in the incubator, whose temperature was controlled at 273 K (±0.1 K). The upper layer liquid was taken out for chemical analysis, and the unchanging composition of the liquid remained was regarded as a sign of equilibrium. After the equilibrium state of the system was confirmed, the upper liquid phase was taken out for chemical analysis, and at the same time the solid phases were removed for identification. Hungchaoite (MgB4O7·9H2O) was prepared by the method of chemical synthesis.26 The boric acid and active MgO were added into the water according to the mass ratio of MgO/ H3BO3/H2O at 1:8:66. The solution was placed in a constant
3. RESULTS AND DISCUSSION 3.1. The Quaternary System LiCl−KCl−MgCl2−H2O at 273 K. The composition of the liquid (mass fraction) and the dry salt composition of the quaternary system LiCl−KCl− MgCl2−H2O at 273 K are shown in Table 2. According to the composition of the dry salts, the isothermal phase diagram of the system is plotted in Figure 2, and its partial enlargement is plotted in Figure 3. At the same time, the diagram of water contents is shown in Figure 4. B
DOI: 10.1021/acs.jced.7b00800 J. Chem. Eng. Data XXXX, XXX, XXX−XXX
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Table 2. Solubilities of Solution in Quarternary System LiCl−KCl−MgCl2−H2O at 273 K and 94.77KPaa composition of the solution 100·w(B)
composition of dry salts J(MgCl2) + J(KCl) + J(LiCl) = 100
no
w(MgCl2)
w(KCl)
w(LiCl)
J(MgCl2)
J(KCl)
J(LiCl)
J(H2O)
solid phases
1,A 2 3 4 5 6 7 8 9 10 11 12,H1 13,B 14 15 16 17 18 19 20 21 22,H2 23,C 24 25 26 27,D 28 29,H3 30,E 31
26.74 26.31 25.02 24.49 23.31 22.83 17.08 13.19 11.06 5.70 4.17 1.89 34.62 34.47 33.84 32.85 30.93 28.23 21.54 19.64 12.13 9.84 10.43 7.40 3.70 3.20 8.13 7.61 7.16 0.00 0.50
2.40 2.42 2.37 2.22 2.28 2.22 2.15 2.13 2.17 1.87 1.83 1.85 0.10 0.10 0.10 0.10 0.09 0.10 0.09 0.09 0.09 0.10 0.00 0.15 1.01 1.30 0.00 0.09 0.25 2.12 2.05
0.00 1.76 3.65 5.82 9.75 13.10 19.99 26.08 29.23 35.67 38.69 43.93 0.00 0.72 1.56 2.66 4.65 7.46 15.56 18.08 26.09 30.52 30.06 33.00 37.92 41.88 32.91 34.73 35.16 43.87 43.81
91.76 86.27 80.60 75.28 65.97 59.84 43.55 31.86 26.04 13.18 9.32 3.97 99.70 97.68 95.33 92.24 86.70 78.87 57.92 51.94 31.66 24.32 25.76 17.41 8.67 6.90 19.80 17.94 16.82 0.00 1.07
8.24 7.95 7.65 6.84 6.44 5.83 5.49 5.14 5.11 4.33 4.10 3.89 0.30 0.29 0.29 0.29 0.26 0.29 0.24 0.24 0.24 0.24 0.00 0.35 2.37 2.81 0.00 0.20 0.59 4.61 4.42
0.00 5.79 11.76 17.88 27.59 34.33 50.96 63.01 68.85 82.50 86.57 92.14 0.00 2.03 4.38 7.48 13.04 20.84 41.84 47.82 68.10 75.45 74.24 77.63 88.95 90.30 80.20 81.86 82.59 95.39 94.51
243.13 227.84 222.18 207.40 183.03 162.07 155.00 141.58 135.55 131.30 123.76 109.76 187.98 183.41 181.71 180.77 180.36 179.33 168.82 164.47 161.03 147.19 146.97 135.24 134.56 115.62 143.70 135.69 134.92 117.42 115.71
K + KM K + KM K + KM K + KM K + KM K + KM K + KM K + KM K + KM K + KM K + KM K + L + KM M + KM M + KM M + KM M + KM M + KM M + KM M + KM M + KM M + KM M + KM + LM M + LM LM + KM L + KM L + KM L + LM L + LM L + LM + KM L+K L+K
a
Standard uncertainties u are u(T) = 0.1 K, u(P) = 1 KPa, ur(w(LiCl)) = 0.003, ur(w(KCl)) = 0.003, ur(w(MgCl2)) = 0.004. L= LiCl·2H2O, K= KCl, M = MgCl2·6H2O, LM = LiCl·MgCl2·7H2O, KM= KCl·MgCl2·6H2O.
Figure 3. Partial enlargment of Figure 2.
Figure 2. Phase diagram of quaternary system LiCl−KCl−MgCl2− H2O at 273 K.
of KCl and KCl·MgCl2·6H2O are larger than those of MgCl2· 6H2O, LiCl·2H2O, and LiCl·MgCl2·7H2O so the solubilities of single salt MgCl2·6H2O and double salt LiCl·MgCl2·7H2O is bigger than those of single salt KCl and double salt KCl·MgCl2· 6H2O. Therefore, KCl and KCl·MgCl2·6H2O is easier to crystallize in the quaternary system. Seven univariant curves of this quaternary system are AH1, BH2, CH2, H2H3, DH3, H3H1, and EH1. Points H1, H2, and H3 are invariant points of this
As can be seen from Figures 2 and 3 and Table 2, there are two double salts at 273 K. The isothermal phase diagram of this system includes three invariant points, seven univariate curves, and five crystalline areas, where the solid phases are three single salts LiCl·2H2O, MgCl2·6H2O, KCl, and two double salts LiCl· MgCl2·7H2O and KCl·MgCl2·6H2O. The crystallization fields C
DOI: 10.1021/acs.jced.7b00800 J. Chem. Eng. Data XXXX, XXX, XXX−XXX
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Figure 4. Water content diagram of quaternary system LiCl−KCl− MgCl2−H2O at 273 K.
Figure 5. Phase diagram of quaternary system Li2B4O7−Na2B4O7− MgB4O7−H2O at 273 K.
quaternary system. Invariant point H1 is saturated with three salts LiCl·2H 2 O + KCl + KCl·MgCl 2 ·6H 2 O and the composition of the corresponding liquid phase is w(LiCl) = 43.93%, w(KCl) = 1.85%, w(MgCl2) = 1.89%. Invariant point H2 is saturated with three salts MgCl2·6H2O + LiCl·MgCl2· 7H2O + KCl·MgCl2·6H2O, and the composition of the corresponding liquid phase is w(LiCl) = 30.52%, w(KCl) = 0.1%, and w(MgCl2) = 9.84%. Invariant point H3 is saturated with three salts LiCl·2H2O + LiCl·MgCl2·7H2O + KCl·MgCl2· 6H2O and the composition of the corresponding liquid phase is w(LiCl) = 35.16%, w(KCl) = 0.25%, and w(MgCl2) = 7.16%. 3.2. The Quaternary System Li 2B4 O7−Na2B 4O7− MgB4O7−H2O at 273 K. The content of the liquid (mass fraction) and the dry salt composition of the quaternary system Li2B4O7−Na2B4O7−MgB4O7−H2O at 273 K are shown in Table 3. According to the composition of the dry salts, the isothermal phase diagram of the system is plotted in Figure 5. At the same time, the relation graph of water contents is also
shown in Figure 6. Furthermore, the equilibrium solid phase is identified and Figure 7 is the X-ray diffraction photograph of the invariant point G. According to Table 3 and Figure 7, it can be seen that this quaternary system is a simple eutectic type and there is no double salt or solid solution at 273 K. The isothermal phase diagram of this system is composed of one invariant point, three univariate curves, and three crystalline areas, where the solid phases are corresponding to the three single salts Li2B4O7· 3H2O, Na2B4O7·10H2O, and MgB4O7·9H2O. The crystallization field of MgB4O7·9H2O is larger than those of Na2B4O7· 10H2O and Li2B4O7·3H2O, so the solubilities of single salts Na2B4O7·10H2O and Li2B4O7·3H2O are bigger than that of single salt MgB4O7·9H2O. Therefore, MgB4O7·9H2O is easier to crystallize in this quaternary system. Three univariant curves of this quaternary system are E1G, E2G, and E3G. Point G is invariant point of this system. This invariant point is saturated
Table 3. Solubilities of Solution in Quarternary System Li2B4O7−Na2B4O7−MgB4O7−H2O at 273 K and 94.77KPab composition of dry salts J(MgB4O7) + J(Na2B4O7) + J(Li2B4O7) = 100
composition of the solution 100·w(B) no.
w(Li2B4O7)
w(Na2B4O7)
w(MgB4O7)
J(Li2B4O7)
J(Na2B4O7)
J(MgB4O7)
J(H2O)
solid phases
1,E1 2 3 4 5 6,G 7,E214 8 9 10 11 12 13,E3 14 15 16 17 18 19
2.44 2.44 2.35 2.30 2.26 2.22 2.31 2.31 2.30 2.28 2.25 2.24 0.00 0.37 0.71 1.20 1.47 1.69 1.93
0.42 0.42 0.41 0.41 0.41 0.41 0.00 0.17 0.26 0.31 0.35 0.38 0.99 0.92 0.84 0.72 0.66 0.62 0.57
0.00 0.02 0.04 0.05 0.06 0.06 0.10 0.09 0.09 0.08 0.08 0.07 0.08 0.08 0.07 0.06 0.06 0.06 0.06
85.26 84.72 83.93 83.33 82.78 82.53 96.01 89.86 86.81 85.39 83.96 83.27 0.00 27.26 43.79 60.41 67.07 71.31 75.37
14.67 14.58 14.64 14.86 15.02 15.24 0.00 6.64 9.80 11.61 13.06 14.13 92.79 66.92 51.89 36.51 30.20 26.14 22.34
0.00 0.69 1.43 1.81 2.20 2.23 3.99 3.50 3.40 3.00 2.99 2.60 7.21 5.82 4.32 3.08 2.73 2.55 2.29
3393.61 3372.22 3471.43 3523.19 3563.00 3617.47 4059.99 3790.14 3674.20 3645.32 3631.34 3617.47 9300.95 7173.92 6077.27 4953.88 4456.20 4113.90 3804.70
LB + NB LB + NB LB + NB LB + NB LB + NB LB + NB + MB LB + MB LB + MB LB + MB LB + MB LB + MB LB + MB NB + MB NB + MB NB + MB NB + MB NB + MB NB + MB NB + MB
b
Standard uncertainties u are u(T) = 0.1 K, u(P) = 1 KPa, ur(w(Li2B4O7)) = 0.005, ur(w(Na2B4O7)) = 0.005, ur(w(MgB4O7)) = 0.005. LB = Li2B4O7·3H2O; NB = Na2B4O7·10H2O; MB = MgB4O7·9H2O. D
DOI: 10.1021/acs.jced.7b00800 J. Chem. Eng. Data XXXX, XXX, XXX−XXX
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Table 4. Comparison Data of Invariant Points in Ternary System KCl−MgCl2−H2O at 273 K25 literature values
experimental values
no.
w(KCl)
w(MgCl2)
w(KCl)
w(MgCl2)
1,A 13,B
2.4 0.1
26.2 34.4
2.40 0.10
26.74 34.62
Table 5. Comparison Data of Invariant Points in Ternary System LiCl−MgCl2−H2O at 273 K6 literature values w(LiCl)
w(MgCl2)
w(LiCl)
w(MgCl2)
23,C
30.15 30.12 30.17 32.20 33.23 33.14
10.45 10.44 10.45 8.11 8.11 8.12
30.06
10.43
32.91
8.13
Figure 6. Water content diagram of quaternary system Li2B4O7− Na2B4O7−MgB4O7−H2O at 273 K. 27,D
with three salts Li2B4O7·3H2O + Na2B4O7·10H2O + MgB4O7· 9H2O, and the composition of the corresponding liquid phase is w(Li2B4O7) = 2.22%, w(Na2B4O7) = 0.41%, and w(MgB4O7) = 0.06%. 3.3. Method Verification. In the process of the experiment, we selected some samples for at least three groups of parallel samples to verify the repeatability of the experiment, especially the boundary points and the invariant points. For example, in the first point (A) of Table 2, the mass fraction of MgCl2 measured is 26.74% whereas that reported in the literature25 is 26.2%; in the 13th point (B) of Table 2, the mass fraction of MgCl2 measured is 34.62%, whereas that reported in the literature25 is 34.4%; In the 23th point (C) of Table 2, the mass fraction of MgCl2 measured is 10.43% and that of LiCl measured is 30.06%, whereas the mass fraction of MgCl2 reported in the literature6 is 10.45% and that of LiCl is 30.15%; the data of other invariant points are listed in Tables 4 and 5. The results of the determination and the results reported in the literature are within the scope of the experimental error.
experimental values
no.
The solubility data of salts and the compositions of the equilibrium solid phases are obtained. The isothermal phase diagrams and the water content diagrams of the systems were plotted according to the experimental data. The study of the quaternary system LiCl−KCl−MgCl2−H2O at 273 K shows that there are two double salts LiCl·MgCl2· 7H2O and KCl·MgCl2·6H2O. The isothermal phase diagram of this system is composed of three invariant points. The solid phases in five crystallization areas are LiCl·2H2O, MgCl2·6H2O, KCl, LiCl·MgCl2·7H2O, and KCl·MgCl2·6H2O, respectively. The crystallization fields of the single salts KCl and the complex salts KCl·MgCl2·6H2O are larger than those of MgCl2·6H2O, LiCl·2H2O, and LiCl·MgCl2·7H2O. We can see that the quaternary system Li2B4O7−Na2B4O7− MgB4O7−H2O at 273 K is a simple cosaturation type and no solid solution or complex salts formed. The isothermal phase diagram of this system has only one invariant point. The solid phases in three crystallization areas are Li2B4O7·3H2O, Na2B4O7·10H2O, and MgB4O7·9H2O, respectively. The crystallization field of MgB4O7·9H2O is the largest, whereas the crystallization area of Li2B4O7·3H2O is the smallest.
4. CONCLUSIONS The phase equilibria of the quaternary systems LiCl−KCl− MgCl2−H2O and Li2B4O7−Na2B4O7−MgB4O7−H2O at 273 K were studied by isothermal dissolution equilibrium method.
Figure 7. X-ray diffraction photograph of the invariant point of the quaternary system Li2B4O7−Na2B4O7−MgB4O7−H2O at 273 K. E
DOI: 10.1021/acs.jced.7b00800 J. Chem. Eng. Data XXXX, XXX, XXX−XXX
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+ H2O) and (Na2B4O7 + MgB4O7 + H2O) at 298.15 K. J. Chem. Eng. Data 2017, 62 (1), 253−258. (16) Sang, S. H.; Yin, H. A.; Tang, M. L.; Lei, N. F. Solubility Investigations in the Systems K2B4O7 + Li2B4O7 + H2O and Na2B4O7 + Li2B4O7 + H2O at T = 288 K. J. Chem. Eng. Data 2004, 49 (6), 1586−1589. (17) Sang, S. H.; Deng, T. L.; Tang, M. L.; Yin, H. A. Study on the Correlation and Physicochemical Properties of Ternary System Li2B4O7-Na2B4O7-H2O at 25°C(in Chinese). J. ChengDu Univ. Technol. 1997, 24 (4), 87−92. (18) Ma, P. C.; Chen, P. H. Li+, Na+//Cl−, B4O72−−H2O Reciprocal Quaternary System Solubility Phase Diagrams. Chem. J. Chin. Univ. (English Edition) 1988, 4 (4), 77−83. (19) Xiao, L. J.; Sang, S. H.; Zhao, X. P. Study on Phase Equilibrium of The Quaternary System K2B4O7-Li2B4O7-MgB4O7-H2O at 288 K(in Chinese). J. Salt Chem. Ind. 2010, 39 (1), 18−20. (20) Sang, S. H.; Tang, M. L.; Yin, H. A. Equilibria Solubilities and Properties of Quaternary System K2B4O7-Na2B4O7-Li2B4O7-H2O at 288 K(in Chinese). Chem. Eng. (China) 2003, 31 (4), 68−71. (21) Sang, S. H.; Peng, J. (Solid+Liquid) Equilibria in the Quaternary System Na2B4O7-MgB4O7-K2B4O7-H2O at 288 K. Chin. J. Chem. 2010, 28 (5), 687−862. (22) Zhang, J. Q.; Zeng, Y.; Peng, Y.; Zong, B. Metastable Phase Diagram of the Quaternary System Li+, Na+// Cl−, B4O72−−H2O at 273 K. J. Chem. Eng. Data 2013, 58 (2), 441−445. (23) Sang, S. H.; Yin, H. A.; Ni, S. J.; Zhang, C. J. Metastable Equilibrium Solubilities of Solutions in the Quaternary System of K2B4O7−Na2B4O7−Li2B4O7−H2O at 273 K(in Chinese). Acta. Phys. Chim. Sin 2007, 23 (8), 1285−1287. (24) Peng, J.; Sang, S. H.; Wei, F. Metastable Equilibrium Solubilities of Solutions in the Quaternary System of MgB4O7−Na2B4O7− Li2B4O7−H2O at 288K(in Chinese). Ind. Miner. Process 2008, 37 (2), 11−13. (25) Deng, T. L.; Zhou, H.; Chen, X. Salt-Water System Phase Diagrams and Applications; Chemical Industry Press: Beijing, 2013. (26) Jing, Y. A new method of synthesis of hungtsaoite(in Chinese). Sea-Lake Salt Chem. Ind. 2000, 29 (2), 24−25. (27) Institute of Qinghai Salt-Lake, Chinese Academy of Sciences. Analytical methods of brines and salts (in Chinese); Science Press: Beijing, 1988.
AUTHOR INFORMATION
Corresponding Author
*E-mail:
[email protected];
[email protected]. ORCID
Rui-Zhi Cui: 0000-0001-6861-8227 Shi-Hua Sang: 0000-0002-5948-3882 Funding
This work was supported by the National Natural Science Foundation of China-Qaidam Saline Lake chemical engineering science research joint fund of Qinghai Provincial People’s Government (U1407108) and scientific research and innovation team in Universities of Sichuan Provincial Department of Education (15TD0009). Notes
The authors declare no competing financial interest.
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REFERENCES
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DOI: 10.1021/acs.jced.7b00800 J. Chem. Eng. Data XXXX, XXX, XXX−XXX
