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Crystallization Kinetics of Mg-Borates Precipitating from Diluted Boron-Containing Brine of Da Qaidam Saline Lake

Jiao-Yu PENG ,  Bo ZHANG ,  Jing CHEN ,  Ya-Ping DONG ,  Wu LI

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Citation:  PENG Jiao-Yu, ZHANG Bo, CHEN Jing, DONG Ya-Ping, LI Wu. Crystallization Kinetics of Mg-Borates Precipitating from Diluted Boron-Containing Brine of Da Qaidam Saline Lake[J]. Chinese Journal of Inorganic Chemistry, 2019, 35(10): 1821-1833. doi: 10.11862/CJIC.2019.209 shu

大柴旦富硼浓缩盐卤中硼酸镁盐稀释结晶动力学

  • 1.

    中国科学院青海盐湖研究所, 中国科学院盐湖资源综合高效利用重点实验室, 西宁 810008

  • 2.

    青海省盐湖资源综合利用工程技术中心, 西宁 810008

  • 3.

    中国科学院大学, 北京 100049

  • 4.

    青海省盐湖资源化学重点实验室, 西宁 810008

    • 通讯作者: 董亚萍, Dongyaping@hotmail.com
  • 基金项目:

    和盐湖化工联合基金面上项目 U1607103

    中国科学院西部之光人才培养项目 Y710091015

    国家青年科学基金(No.21501187), 中国科学院西部之光人才培养项目(No.Y710091015)和盐湖化工联合基金面上项目(No.U1607103)资助

    国家青年科学基金 21501187

摘要: 采用动力学法研究了富硼浓缩盐卤稀释过程硼酸镁盐的结晶动力学，重点探讨了温度、稀释比和硼浓度对结晶过程的影响。利用单纯形优化法配合Runge-Kutta微分方程组数值解法对实验数据进行拟合，给出了结晶动力学方程和结晶速率。结果表明，低温、高硼浓度和中间稀释比有利于硼酸镁盐的结晶析出，最优条件下析硼率（以B2O3计）高达88%；结晶速率随硼浓度的增加和温度的降低快速增大；反应级数表明稀释结晶过程硼酸镁盐结晶主要受多核表面反应控制，同时提出了结晶相转化机理。

English

  • 0.   Introduction

    The new process of "crystallization by dilution" was firstly reported by Gao et al.[1-2] during study on the chemistry of borate in sulfate-type salt lake of Da Qaidam, in China. It refers to that borates could be accumulated in the concentrated brine throughout solar evaporation process, and keep stable at room temperature for a few months and do not crystallize until reach to the maximum solubility (5.82% in the form of B2O3)[3], while diluting this boron-concentrated brine with water can accelerate the precipitation of Mg-borates from aqueous solutions. Different hydrated Mg-borates, such as inderite (kurnakovite), hung-chaoite, and macallisterite, can be crystallized out after dilution for a period of time, not only from brines with different dilution ratios for the same time period, but also from the same diluted brine after setting different periods[1, 4-6]. This phenomenon explained the forming and mineralization of borate minerals deposited on Da Qaidam salt lake bottom[7-9], especially for the minerogenetic mechanism of pinnoite[10-12]. Furthermore, since the boron content in Mg-borate precipitates was more than 35% in the form of B2O3, which is much higher than boron ores (5%~30% B2O3) in China[13]. The high grade Mg-borate salts could be used as raw materials for industrial production of boron compound. Therefore, the "crystallization by dilution" would provide an economical method for the boron extraction from brine. However, since the magnesium borates have a high supersolubility and need a long time to achieve the solid-liquid equili-brium, which often causes a slow crystallization rate and low boron recovery during dilution process, it is of great importance to study the crystallization kinetics of Mg-borates from diluted brines. The objective of the present study was to investigate the crystallization kinetics and transformation mechanism of Mg-borates from different diluted brines by dynamical method. Factors such as temperature, dilution ratio and boron concentration on the Mg-borates crystallization were studied. The results obtained would provide funda-mental data and theories for the efficient separation of boron resource from brine using dilution method.

    1.   Dynamic model

    Gao et al.[14-19] had studied the crystallization kinetics of Mg-borates from MgO-nB2O3-MgCl2/MgSO4-H2O supersaturated solutions. In their studies, an appropriate mathematical modification of Nielsen′s polynuclear layer and mononuclear layer controlled growth mechanism[20-21] has been made, and the kinetic crystallization reaction equations of Mg-borates in supersaturated solutions are given as follows:

    MA model: -dc/dt=k1(c0-c)2/3(c0-c∞)p

    MB model: -dc/dt=k2(c0-c)4/3(c0-c∞)p

    where MA and MB models correspond to the polynuclear layer and mononuclear layer controlled growth mechanism, respectively; k1 and k2 are the rate constants, c0 and c∞ are the initial concentration and equilibrium concentration of boron in solution, respectively; p is the reaction order referring to 1, 2, 3, and 4. Thus, four kinetic equations such as MA-1(MB-1), MA-2 (MB-2), MA-3 (MB-3) and MA-4(MB-4) are obtained. Generally, the crystallization mechanism controlled by MB model needs higher reaction energy and longer inducing period compared with the MA model.

    Based on the simple optimum method and Runge-Kutta digital solution of differential equations[14], the experimental data of c-t curve was fitted and the optimum kinetic equation of Mg-borates was calculated by computer, as shown in Fig. 1. The c0 value is considered as the boron concentration at the point of initial precipitation of solid phase, the c∞, 0 is the initial value of equilibrium concentration of boron estimated less than the last value of experimental data. Because Mg-borates often have a high super-solubility and require a long period of time (more than half a year) to establish the solid-liquid equilibrium, it is difficult to determine the c∞ value experimentally. The k0 is also the initial value of the rate constant. The relative error Er was defined as: Er=(cc, i-ce, i)/ce, i×100%. cc, i and ce, i are the calculation data and experi-mental data at ti time period, respectively. The preci-sion used was 10-7. Among all the obtained MA and MB kinetic equations, the suitable equation is selected when the values of Er are no more than 5.0%.

    Figure 1

    Figure 1.  Schematic diagram of calculation procedure
    下载: 全尺寸图片 幻灯片

    In the present study, the boron-concentrated brine system can be referred as MgO-2B2O3-MgSO4-MgCl2-H2O, which is similar to that of Gao′s studies. Therefore, we choose the MA and MB models to calculate the kinetic equations of Mg-borates precipitated from different diluted brines.

    2.   Experimental

    2.1   Materials

    A boron-containing brine (1.28% B2O3), saturated with bischofite (MgCl2·6H2O), was obtained from Da Qaidam salt lake and concentrated further by evapora-tion at (298.15±3) K after the addition of Na2SO4·10H2O solid. The concentration of boron in concen-trated brines was 2.60%, 3.78% and 4.96% in the form of B2O3 (Table 1). The Na2SO4·10H2O solid was recrystallized from mirabilite ores. Deionized water (resistivity, 18.25 MΩ·cm) was used in all experiments.

    Table 1

    Table 1.  Compositions of the brine used in experiments
    下载: 导出CSV
    BrineDensity/(g·cm-3)pHMass fraction of ion/%
    Na+Mg2+K+B3+ (B2O3)Cl-SO42-Li+
    Da Qaidam (L0)1.362 24.390.1078.860.0481.2824.472.290.144
    Brine L11.348 14.50-0.0518.700.0562.6022.903.230.246
    Brine L21.394 54.430.0168.800.0633.7823.222.910.301
    Brine L3—4.310.0558.710.0784.9622.323.420.353

    2.2   Measurement of crystallization kinetics

    The crystallization experiments were performed as follows[1]: an amount of the boron-concentrated brine was diluted with some water. The diluted brine was placed in a well-sealed glass vessel at constant temperature and stirred ca. 5 min each day to promote the precipitation of solid phase. When the solid phase began to precipitate from the diluted brine, some solution samples were taken out using a porous filter (Pore size: 3~4 μm) for boron concentration analysis. The sampling experiments were carried out every one or three days until the solution concentration of boron changed little or remained basically constant. Then the mixtures were filtered, and the resultant sediment was washed using some water and absolute alcohol, respectively, and dried in a vacuum drying oven for 24 h. The obtained solid phases were characterized by X-ray diffraction (XRD, PRO PANalytical X′Pert, Cu Kα1, λ=0.154 nm) with a tube voltage and current of 40 kV and 30 mA, respectively. The powder pattern was measured in a scanning range from 5° to 70°. The composition of solid was analyzed by titration.

    During the crystallization process, the boron concentrations used were 2.60%, 3.78% and 4.96% in the form of B2O3, and the mass dilution ratios (mwater/mbrine) tested were 0.50, 1.0 and 2.0. The temperature used was 258.15, 277.15 and 298.15 K. The experi-ments at low temperature (258.15 and 277.15 K) were achieved by placing in a refrigerator and that of 298.15 K was settled in water bath.

    2.3   Chemical analysis

    The titration analysis of brine and solid compositions was based on a previous publication[22]. The Mg2+ ion was analyzed by complexometric titration with ethylene diamine tetraacetic acid (EDTA). The K+ ion was analyzed by quaternary ammonium back titration. The Li+ ion was determined by the flame atomic absorption spectrophotometer (AAS, AAnalyst 800, PE of USA). The Cl- ion and boron was analyzed by mercurimetry and mannitol conversion acid base titration, respectively. The SO42- ion was analyzed by the gravimetric method. While the Na+ ion concentra-tion in brine was calculated using the ion charge balance principle. The accuracy of these analyses was ±0.1%~±0.3%.

    3.   Results and discussion

    3.1   Solid phase analysis

    The XRD patterns of precipitates crystallized from diluted brines are shown in Fig. 2. And the solid phase composition is listed in Table 2. The water content in precipitates was obtained by subtracting the mass of MgO and B2O3 from the total mass. As shown in Table 2, at 1.0 dilution ratio, when boron concentration was less than 3.78% in B2O3, the only triborates such as magnesium borate hydroxide (MgB3O3(OH)5·6H2O) and inderite (MgB3O3(OH)5·5H2O) had crystallized out from the diluted brines. As the boron concentration increased to 4.96% B2O3, the tetraborate of hungchaoite (MgB4O5(OH)4·7H2O) appeared in the precipitates at temperature lower than 277.15 K. This is because the high boron concentra-tion and low temperature favored the formation of [B4O5(OH)4]2- ion by polymerization. Besides, the content of B2O3 in precipitates varied in a range of 35%~40%, much higher than the grade (wB2O3≥12%) requested for chemical processing of borate minerals in China.

    Figure 2

    Figure 2.  XRD patterns of solid phases crystallized from diluted brines with various boron concentrations: (a) 2.60%; (b) 3.78%; (c) 4.96%

    Dilution ratio=1.0

    下载: 全尺寸图片 幻灯片

    Table 2

    Table 2.  Analyses of solid phases crystallized from diluted brines
    下载: 导出CSV
    cboron/% (w/w)Dilution ratioT/℃wMgO/% (w/w)wB2O3/% (w/w)wH2O/% (w/w)nMgO:nB2O3:nH2OSolid phase determined by XRDFormula
    2.601.0298.1514.3837.8047.821.00:1.52:7.44Magnesium borate hydroxide hydrate2MgO·3B2O3·15H2O
    1.0277.1514.0536.9149.041.00:1.52:7.81Inderite+Magnesium borate hydroxide hydrate2MgO·3B2O3·15H2O+2MgO·3B2O3·17H2O
    1.0258.1513.5735.1051.341.00:1.50:8.47Magnesium borate hydroxide hydrate2MgO·3B2O3·17H2O
    3.781.0298.1514.4037.9447.661.00:1.53:7.41Inderite2MgO·3B2O3·15H2O
    1.0277.1513.6235.5250.861.00:1.51:8.36Magnesium borate hydroxide hydrate2MgO·3B2O3·17H2O
    1.0258.1513.5535.1651.301.00:1.50:8.47Magnesium borate hydroxide hydrate2MgO·3B2O3·17H2O
    4.961.0298.1514.3737.9947.651.00:1.53:7.42Inderite2MgO·3B2O3·15H2O
    1.0277.1512.7340.0647.211.00:1.82:8.29Inderite+Hungchaoite2MgO·3B2O3·15H2O+MgO·2B2O3·9H2O
    1.0258.1512.5038.3449.171.00:1.78:8.80Inderite+Hungchaoite2MgO·3B2O3·15H2O+MgO·2B2O3·9H2O

    3.2   Effects of temperature on crystallization

    Fig. 3 shows the effect of temperature on the crystallization process (cB2O3-t curve) of Mg-borates from 2.60% and 4.96% boron(B2O3) brines at 1.0 dilution ratio, respectively.

    Figure 3

    Figure 3.  Effect of temperature on crystallization of Mg-borates
    下载: 全尺寸图片 幻灯片

    As shown in Fig. 3, the crystallization process appeared in the shape of reversed S curve including inducing period, crystallization and phase equilibrium stages. The time of inducing period decreased with the increasing of temperature and boron concentrations. While the total time period, throughout the crystalliza-tion process, shortened greatly with the decreasing of temperature and an increasing in boron concentrations due to higher supersaturation. For instance, the crystallization time shortened twice (from 1 400 to 600 h) as boron(B2O3) concentration increased from 2.60% to 4.96% at 258.15 K. Besides, when the boron (B2O3) concentration increased to 4.96% (Fig. 3b), It was noted that the crystallization time changed little at temperature less than 277.15 K. Because the boron(B2O3) concentration of 4.96% in brine is closed to the maximum supersolubility of Mg-borate (5.71%~5.81% B2O3)[3] in concentrated salt lake brine, the influence of boron concentration is predominant and further temperature reduction makes little effect on crystallization.

    3.3   Effects of dilution ratio on crystallization

    The influence of mass dilution ratio (mwater/mbrine) on the crystallization is shown in Fig. 4. The boron(B2O3) concentration used was 2.60%. As can be seen, the phase equilibrium concentration of boron at dilution ratio of 0.50 was lower than that of 1.0 ratio at 258.15 K (Fig. 4a). But the crystallization time of the former was twice longer than the latter due to the slower crystallization rate of Mg-borates at ratio of 0.50. At 277.15 K (Fig. 4b), the crystallization time at ratio of 2.0 was shorter and the yield of boron was also lower compared with ratio of 1.0. According to our study, the diluted brine of 2.0 ratio would freeze when the temperature decreased from 277.15 to 258.15 K. Therefore, the dilution ratio ranging from 0.50 to 1.0 and the temperature below 277.15 K would be more preferable to the Mg-borates crystallization from salt lake brine.

    Figure 4

    Figure 4.  Effects of dilution ratio on crystallization of Mg-borates
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    3.4   Effects of boron concentration in brine on crystallization

    As shown in Fig. 5, the boron concentration affected dramatically on the yield of Mg-borates at ratio of 1.0, as well as the crystallization time. When boron(B2O3) concentration increased from 2.60% to 4.96%, the boron yield increased substantially from 61.4% to 88.0% in the form of B2O3. This result would offer considerable benefits to the boron extraction from salt lake brine by dilution method.

    Figure 5

    Figure 5.  Effects of boron concentration in brine on crystallization of Mg-borates
    下载: 全尺寸图片 幻灯片

    3.5   Crystallization kinetics of Mg-borates

    After calculations of the kinetic equation both from MA and MB models, the optimum kinetic equations of Mg-borates at 1.0 ratio with different temperature and boron concentrations were obtained as follows:

    (1) 2.60% B2O3 boron-concentrated brine at 1.0 dilution ratio

    298.15 K: -dc/dt=0.0343 9(1.290-c)2/3(c-0.540)2

    277.15 K: -dc/dt=0.0239 1(1.293-c)2/3(c-0.490)2

    258.15 K: -dc/dt=0.0200 9(1.295-c)2/3(c-0.440)

    (2) 3.78% B2O3 boron-concentrated brine at 1.0 dilution ratio

    298.15 K: -dc/dt=0.013 16(1.879-c)2/3(c-0.650)2

    277.15 K: -dc/dt=0.025 46(1.863-c)2/3(c-0.630)2

    258.15 K: -dc/dt=0.023 24(1.854-c)2/3(c-0.570)2

    (3) 4.96% B2O3 boron-concentrated brine at 1.0 dilution ratio

    298.15 K: -dc/dt=0.009 82(2.479-c)2/3(c-0.850)2

    277.15 K: -dc/dt=0.013 73(2.427-c)2/3(c-0.250)2

    258.15 K: -dc/dt=0.049 01(2.477-c)2/3(c-0.220)3

    The corresponding crystallization results of Mg-borates with boron(B2O3) concentration of 2.60%, 3.78% and 4.96% are shown in Table 3 to 5, respe-ctively. The relative errors between the experimental and calculated data were plotted in Fig. 6. As shown in Fig. 6, most of the absolute values of relative error were less than 5% except for the minorities, suggesting the calculated data agreed well with the experiment one. According to the kinetic equations, it is known that the crystallization of Mg-borates is dominated by the polynuclear layer controlled growth mechanism. While the boron concentration increases to the maximum supersaturation level, the mononuclear layer controlled growth mechanism changes to be the predominant one at temperature of 258.15 K.

    Table 3

    Table 3.  Concentrations of B2O3 and their errors calculated by dynamic model during crystallization from 2.60% B2O3 diluted brine at ratio of 1.0*
    下载: 导出CSV
    298.15 K277.15 K258.15 K
    Time/hce/%cc/%Er(MA-2)/%Time/hce/%cc/%Er(MA-2)/%Time/hce/%cc/%Er(MA-2)/%
    01.29201.30301.302
    118.01.29289.91.303310.81.2951.2950.00
    140.71.2901.289-0.08125.11.2931.292-0.08350.41.2771.274-0.23
    166.71.2461.2701.93148.21.2891.281-0.62378.61.2201.216-0.33
    190.51.1631.2214.99170.91.2771.255-1.72406.51.1281.114-1.24
    213.31.0921.1505.31195.51.2401.205-2.82446.10.9620.923-4.05
    235.80.9641.07011.00220.21.1851.139-3.88470.90.7660.8034.83
    259.80.9180.9907.84268.11.0310.999-3.10501.30.6480.6804.94
    307.60.8640.8670.35291.90.9680.938-3.10525.80.5950.6061.85
    332.10.8390.821-2.15315.80.9060.885-2.32552.10.5580.548-1.79
    355.80.8100.786-2.96339.80.8630.840-2.67587.50.5230.500-4.40
    384.30.7900.753-4.68363.90.8100.802-0.99622.60.5040.472-6.35
    408.50.7700.730-5.19411.70.7440.743-0.13662.10.4920.456-7.32
    452.30.7320.699-4.51458.80.6960.7020.86707.40.4700.447-4.89
    500.00.7070.674-4.67506.80.6660.6700.60788.80.4550.442-2.86
    550.10.6870.655-4.66554.80.6300.6462.54906.40.4400.4400.00
    620.00.6650.635-4.51626.70.6020.6202.991 097.40.4400.4400.00
    723.90.6330.615-2.84735.40.5660.5934.77
    869.10.6080.598-1.64862.70.5470.5724.57
    1 028.60.5860.5870.17999.50.5200.5587.31
    1 197.30.5670.5781.941 167.90.5070.5457.50
    1 397.10.5600.5722.141 368.70.5030.5356.36
    *ce: experimental data; cc: calculated data

    Table 4

    Table 4.  Concentrations of B2O3 and their errors calculated by dynamic model during crystallization from 3.78% B2O3 diluted brine at ratio of 1.0*
    下载: 导出CSV
    298.15 K277.15 K258.15 K
    Time/hce/%cc/%Er(MA-2)/%Time/hce/%cc/%Er(MA-2)/%Time/hce/%cc/%Er(MA-2)/%
    0.001.8791.8790.000.001.8800.001.874
    47.51.8411.830-0.6098.31.8631.8630.0095.61.868
    93.01.6481.6530.30162.11.4251.4793.79144.51.8541.8540.00
    149.71.3611.3761.10211.81.1021.1151.18192.31.5331.6316.39
    198.51.1831.1951.01259.80.9750.947-2.87245.21.2511.164-6.95
    248.91.0661.0700.38336.20.8360.827-1.08321.40.8710.8750.46
    325.10.9680.953-1.55412.50.7770.771-0.77396.50.7480.7672.54
    400.20.8980.885-1.45510.10.7400.732-1.08484.10.6920.7082.31
    487.20.8510.834-2.00604.30.7170.711-0.84604.40.6590.6661.06
    607.20.8060.791-1.86726.50.7020.693-1.28735.00.6420.6420.00
    710.30.7650.7670.26839.70.6960.682-2.01843.40.6310.630-0.16
    809.10.7460.7510.67963.60.6910.674-2.46970.80.6240.620-0.64
    906.20.7300.7381.10
    1 023.10.7240.7270.41
    1 116.00.7120.7201.12
    *ce: experimental data; cc: calculated data

    Table 5

    Table 5.  Concentrations of B2O3 and their errors calculated by dynamic model during crystallization from 4.96% B2O3 diluted brine at ratio of 1.0*
    下载: 导出CSV
    298.15 K277.15 K258.15 K
    Time/hce/%cc/%Er(MA-2)/%Time/hce/%cc/%Er(MA-2)/%Time/hce/%cc/%Er(MA-2)/%
    0.002.4792.4790.000.002.4800.002.477
    61.62.4302.299-5.3971.62.4272.4270.0088.82.4772.4770.00
    92.32.0952.066-1.3893.41.9132.0336.27118.72.4332.4761.77
    134.81.5771.75111.03122.91.3401.115-16.79145.52.0782.46718.72
    186.41.4751.4860.75161.30.7510.687-8.52169.31.5951.6090.88
    230.41.3731.344-2.11189.10.5200.5648.46193.30.7230.686-5.12
    263.31.3051.270-2.68233.70.4290.4637.93238.80.4600.4763.48
    335.01.2091.162-3.89281.00.3700.40810.27288.30.3910.4094.60
    407.21.1471.095-4.53364.10.3470.3583.17362.40.3590.3651.67
    502.01.0771.041-3.34477.70.3270.325-0.61480.80.3440.332-3.49
    598.81.0201.005-1.47600.00.3100.307-0.97604.20.3210.314-2.18
    697.50.9890.979-1.01723.00.3000.295-1.67768.60.3080.300-2.60
    794.00.9560.9610.52843.50.2970.288-3.03909.80.3020.291-3.64
    889.50.9360.9481.28
    997.80.9270.9360.97
    1 100.60.9210.9270.65
    1 246.10.9170.9170.00
    *ce: experimental data; cc: calculated data

    Figure 6

    Figure 6.  Concentrations of B2O3 and their errors between the experimental and calculated data during
    下载: 全尺寸图片 幻灯片

    Fig. 7 shows the crystallization rate (-dc/dt) of Mg-borates calculated by kinetic equations during crystallization. It is noted that the crystallization rate initially increases exponentially to a maximum value and then decreases dramatically with the crystalliza-tion time, particularly for the high boron concentration and low temperature. Furthermore, it is noticeable that the crystallization rate increases with the increasing of boron concentrations and the drops of temperature, which explains the reason that the crystallization time of Mg-borates shortened dramatically with the rising in boron concentrations and also the lowering of temperature.

    Figure 7

    Figure 7.  (-dc/dt)-t curves of solid phases crystallized from diluted brines with different boron concentrations and temperatures
    下载: 全尺寸图片 幻灯片

    3.6   Transformation mechanism of Mg-borates

    According to our earlier study[5, 23], the Raman spectra of the diluted brine (cboron=2.5%~4.7%) and the mother solution after precipitation were recorded at room temperature and it is found that the main boron forms in the diluted brine at ratio of 1.0 are B(OH)3, [B(OH)4]-, and [B3O3(OH)4]- anions. Species of [B5O6(OH)4]- and [B4O5(OH)4]2- ions are the minorities. But it changed after Mg-borates precipitation from the brine. The Raman intensity of the [B3O3(OH)4]- ion decreased and the [B(OH)4]-, [B5O6(OH)4]- and [B4O5(OH)4]2- ions disappeared in the mother solution. This is because the [B3O3(OH)4]- ion was used for Mg-borates precipitation and the boron concentration in solution decreased rapidly, which promotes the de-polymerization of [B5O6(OH)4]- and [B4O5(OH)4]2- in solution. Besides, the pH value of solution also decreased after precipitation and the solution became weak acidic. This reveals that the OH- ion is also consumed for the Mg-borates precipitation. In this paper, since the boron concentration, dilution ratio, and the solid phases are similar to the earlier report, the phase transformations of inderite, magnesium borate hydroxide and hungchaoite happening in the diluted brine at ratio of 1.0 can be deduced as follows:

    For the triborates, the trimers of [B3O3(OH)4]- ion present in solution would couple a OH- to form the [B3O3(OH)5]2- ion and then react with [Mg(H2O)6]2+ ion in solution to precipitate the triborates, the main reactions can be:

    $ \left[\mathrm{B}_{3} \mathrm{O}_{3}(\mathrm{OH})_{4}\right]^{-}+\mathrm{OH}^{-} \rightleftharpoons\left[\mathrm{B}_{3} \mathrm{O}_{3}(\mathrm{OH})_{5}\right]^{-} $

    		(1)

    $ \mathrm{Mg}^{2+}+6 \mathrm{H}_{2} \mathrm{O} \rightleftharpoons\left[\mathrm{Mg}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+} $

    		(2)

    $ \begin{array}{r}{\left[\mathrm{B}_{3} \mathrm{O}_{3}(\mathrm{OH})_{5}\right]^{2-}+\left[\mathrm{Mg}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+} \rightleftharpoons} \\ {\mathrm{MgB}_{3} \mathrm{O}_{3}(\mathrm{OH})_{5} \cdot 5 \mathrm{H}_{2} \mathrm{O} \downarrow+\mathrm{H}_{2} \mathrm{O}} \\ {\text { (inderite) }}\end{array} $

    		(3)

    $ \begin{array}{r}{\left[\mathrm{B}_{3} \mathrm{O}_{3}(\mathrm{OH})_{5}\right]^{2-}+\left[\mathrm{Mg}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+} \rightleftharpoons} \\ {\mathrm{MgB}_{3} \mathrm{O}_{3}(\mathrm{OH})_{5} \cdot 6 \mathrm{H}_{2} \mathrm{O} \downarrow}\end{array} $

    		(4)

    (magnesium borate hydroxide hydrate)

    Among the reactions, since the [B3O3(OH)4]- coupled a OH- to form the [B3O3(OH)5]2- ion, the solution pH value decreases after solid precipitation.

    For the tetraborates, the lower temperature and increasing boron concentration favor the polymerizaiton of the [B3O3(OH)4]- with [B(OH)4]- to form the [B4O5(OH)4]2- ion, and then [B4O5(OH)4]2- react with [Mg(H2O)6]2+ ion to precipitate the hungchaoite. The main reactions can be:

    $ \begin{array}{r}{\left[\mathrm{B}_{3} \mathrm{O}_{3}(\mathrm{OH})_{4}\right]^{-}+\mathrm{OH}^{-}+\mathrm{B}(\mathrm{OH})_{3} \rightleftharpoons} \\ {\left[\mathrm{B}_{4} \mathrm{O}_{5}(\mathrm{OH})_{4}\right]^{2-}+2 \mathrm{H}_{2} \mathrm{O}}\end{array} $

    		(5)

    $ \mathrm{Mg}^{2+}+6 \mathrm{H}_{2} \mathrm{O} \rightleftharpoons\left[\mathrm{Mg}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+} $

    		(6)

    $ \begin{array}{r}{\left[\mathrm{B}_{4} \mathrm{O}_{5}(\mathrm{OH})_{4}\right]^{2-}+\left[\mathrm{Mg}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons} \\ {\quad \operatorname{MgB}_{4} \mathrm{O}_{5}(\mathrm{OH})_{4} \cdot 7 \mathrm{H}_{2} \mathrm{O} \downarrow} \\ {\text { (hungchaoite) }}\end{array} $

    		(7)

    4.   Conclusions

    The boron-concentrated brine with system of MgO·2B2O3-MgSO4-MgCl2-H2O was obtained by evapo-ration and the crystallization of Mg-borates from diluted brines was studied by the kinetic method. The major conclusions are as follows:

    (1) The crystallization time, crystallization rate and boron yield are greatly influenced by temperature, dilution ratio and boron concentration. High boron concentration with medium dilution ratio and low temperature are found to be more beneficial to the boron crystallization and the boron yield obtained was more than 88% (cB2O3), which is favorable to the boron extraction from salt lake brine by dilution method.

    (2) According to the kinetic equations, the crystallization of Mg-borates in diluted brine is dominated by the mechanism of polynuclear layer controlled growth. However, as the boron concentra-tion increases to the maximum supersaturation level and the temperature decreases to 258.15 K, the mononuclear layer controlled growth mechanism becomes the predominant one. Furthermore, the phase transformation mechanism of Mg-borates was also proposed based on the Raman spectra of borate ions in solution before or after precipitation.

    The above results can provide useful information and technical support for the application of dilution method in boron separation from salt lake.


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  • Figure 1  Schematic diagram of calculation procedure

    下载: 全尺寸图片 幻灯片

    Figure 2  XRD patterns of solid phases crystallized from diluted brines with various boron concentrations: (a) 2.60%; (b) 3.78%; (c) 4.96%

    Dilution ratio=1.0

    下载: 全尺寸图片 幻灯片

    Figure 3  Effect of temperature on crystallization of Mg-borates

    下载: 全尺寸图片 幻灯片

    Figure 4  Effects of dilution ratio on crystallization of Mg-borates

    下载: 全尺寸图片 幻灯片

    Figure 5  Effects of boron concentration in brine on crystallization of Mg-borates

    下载: 全尺寸图片 幻灯片

    Figure 6  Concentrations of B2O3 and their errors between the experimental and calculated data during

    下载: 全尺寸图片 幻灯片

    Figure 7  (-dc/dt)-t curves of solid phases crystallized from diluted brines with different boron concentrations and temperatures

    下载: 全尺寸图片 幻灯片

    Table 1.  Compositions of the brine used in experiments

    BrineDensity/(g·cm-3)pHMass fraction of ion/%
    Na+Mg2+K+B3+ (B2O3)Cl-SO42-Li+
    Da Qaidam (L0)1.362 24.390.1078.860.0481.2824.472.290.144
    Brine L11.348 14.50-0.0518.700.0562.6022.903.230.246
    Brine L21.394 54.430.0168.800.0633.7823.222.910.301
    Brine L3—4.310.0558.710.0784.9622.323.420.353
    下载: 导出CSV

    Table 2.  Analyses of solid phases crystallized from diluted brines

    cboron/% (w/w)Dilution ratioT/℃wMgO/% (w/w)wB2O3/% (w/w)wH2O/% (w/w)nMgO:nB2O3:nH2OSolid phase determined by XRDFormula
    2.601.0298.1514.3837.8047.821.00:1.52:7.44Magnesium borate hydroxide hydrate2MgO·3B2O3·15H2O
    1.0277.1514.0536.9149.041.00:1.52:7.81Inderite+Magnesium borate hydroxide hydrate2MgO·3B2O3·15H2O+2MgO·3B2O3·17H2O
    1.0258.1513.5735.1051.341.00:1.50:8.47Magnesium borate hydroxide hydrate2MgO·3B2O3·17H2O
    3.781.0298.1514.4037.9447.661.00:1.53:7.41Inderite2MgO·3B2O3·15H2O
    1.0277.1513.6235.5250.861.00:1.51:8.36Magnesium borate hydroxide hydrate2MgO·3B2O3·17H2O
    1.0258.1513.5535.1651.301.00:1.50:8.47Magnesium borate hydroxide hydrate2MgO·3B2O3·17H2O
    4.961.0298.1514.3737.9947.651.00:1.53:7.42Inderite2MgO·3B2O3·15H2O
    1.0277.1512.7340.0647.211.00:1.82:8.29Inderite+Hungchaoite2MgO·3B2O3·15H2O+MgO·2B2O3·9H2O
    1.0258.1512.5038.3449.171.00:1.78:8.80Inderite+Hungchaoite2MgO·3B2O3·15H2O+MgO·2B2O3·9H2O
    下载: 导出CSV

    Table 3.  Concentrations of B2O3 and their errors calculated by dynamic model during crystallization from 2.60% B2O3 diluted brine at ratio of 1.0*

    298.15 K277.15 K258.15 K
    Time/hce/%cc/%Er(MA-2)/%Time/hce/%cc/%Er(MA-2)/%Time/hce/%cc/%Er(MA-2)/%
    01.29201.30301.302
    118.01.29289.91.303310.81.2951.2950.00
    140.71.2901.289-0.08125.11.2931.292-0.08350.41.2771.274-0.23
    166.71.2461.2701.93148.21.2891.281-0.62378.61.2201.216-0.33
    190.51.1631.2214.99170.91.2771.255-1.72406.51.1281.114-1.24
    213.31.0921.1505.31195.51.2401.205-2.82446.10.9620.923-4.05
    235.80.9641.07011.00220.21.1851.139-3.88470.90.7660.8034.83
    259.80.9180.9907.84268.11.0310.999-3.10501.30.6480.6804.94
    307.60.8640.8670.35291.90.9680.938-3.10525.80.5950.6061.85
    332.10.8390.821-2.15315.80.9060.885-2.32552.10.5580.548-1.79
    355.80.8100.786-2.96339.80.8630.840-2.67587.50.5230.500-4.40
    384.30.7900.753-4.68363.90.8100.802-0.99622.60.5040.472-6.35
    408.50.7700.730-5.19411.70.7440.743-0.13662.10.4920.456-7.32
    452.30.7320.699-4.51458.80.6960.7020.86707.40.4700.447-4.89
    500.00.7070.674-4.67506.80.6660.6700.60788.80.4550.442-2.86
    550.10.6870.655-4.66554.80.6300.6462.54906.40.4400.4400.00
    620.00.6650.635-4.51626.70.6020.6202.991 097.40.4400.4400.00
    723.90.6330.615-2.84735.40.5660.5934.77
    869.10.6080.598-1.64862.70.5470.5724.57
    1 028.60.5860.5870.17999.50.5200.5587.31
    1 197.30.5670.5781.941 167.90.5070.5457.50
    1 397.10.5600.5722.141 368.70.5030.5356.36
    *ce: experimental data; cc: calculated data
    下载: 导出CSV

    Table 4.  Concentrations of B2O3 and their errors calculated by dynamic model during crystallization from 3.78% B2O3 diluted brine at ratio of 1.0*

    298.15 K277.15 K258.15 K
    Time/hce/%cc/%Er(MA-2)/%Time/hce/%cc/%Er(MA-2)/%Time/hce/%cc/%Er(MA-2)/%
    0.001.8791.8790.000.001.8800.001.874
    47.51.8411.830-0.6098.31.8631.8630.0095.61.868
    93.01.6481.6530.30162.11.4251.4793.79144.51.8541.8540.00
    149.71.3611.3761.10211.81.1021.1151.18192.31.5331.6316.39
    198.51.1831.1951.01259.80.9750.947-2.87245.21.2511.164-6.95
    248.91.0661.0700.38336.20.8360.827-1.08321.40.8710.8750.46
    325.10.9680.953-1.55412.50.7770.771-0.77396.50.7480.7672.54
    400.20.8980.885-1.45510.10.7400.732-1.08484.10.6920.7082.31
    487.20.8510.834-2.00604.30.7170.711-0.84604.40.6590.6661.06
    607.20.8060.791-1.86726.50.7020.693-1.28735.00.6420.6420.00
    710.30.7650.7670.26839.70.6960.682-2.01843.40.6310.630-0.16
    809.10.7460.7510.67963.60.6910.674-2.46970.80.6240.620-0.64
    906.20.7300.7381.10
    1 023.10.7240.7270.41
    1 116.00.7120.7201.12
    *ce: experimental data; cc: calculated data
    下载: 导出CSV

    Table 5.  Concentrations of B2O3 and their errors calculated by dynamic model during crystallization from 4.96% B2O3 diluted brine at ratio of 1.0*

    298.15 K277.15 K258.15 K
    Time/hce/%cc/%Er(MA-2)/%Time/hce/%cc/%Er(MA-2)/%Time/hce/%cc/%Er(MA-2)/%
    0.002.4792.4790.000.002.4800.002.477
    61.62.4302.299-5.3971.62.4272.4270.0088.82.4772.4770.00
    92.32.0952.066-1.3893.41.9132.0336.27118.72.4332.4761.77
    134.81.5771.75111.03122.91.3401.115-16.79145.52.0782.46718.72
    186.41.4751.4860.75161.30.7510.687-8.52169.31.5951.6090.88
    230.41.3731.344-2.11189.10.5200.5648.46193.30.7230.686-5.12
    263.31.3051.270-2.68233.70.4290.4637.93238.80.4600.4763.48
    335.01.2091.162-3.89281.00.3700.40810.27288.30.3910.4094.60
    407.21.1471.095-4.53364.10.3470.3583.17362.40.3590.3651.67
    502.01.0771.041-3.34477.70.3270.325-0.61480.80.3440.332-3.49
    598.81.0201.005-1.47600.00.3100.307-0.97604.20.3210.314-2.18
    697.50.9890.979-1.01723.00.3000.295-1.67768.60.3080.300-2.60
    794.00.9560.9610.52843.50.2970.288-3.03909.80.3020.291-3.64
    889.50.9360.9481.28
    997.80.9270.9360.97
    1 100.60.9210.9270.65
    1 246.10.9170.9170.00
    *ce: experimental data; cc: calculated data
    下载: 导出CSV
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  • 发布日期:  2019-10-10
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