J. Cent. South Univ. (2020) 27: 1351−1366 DOI: https://doi.org/10.1007/s11771-020-4371-5

Role and maintenance of redox potential on chalcopyrite biohydrometallurgy: An overview

HUANG Xiao-tao(黄小涛)1, 2, LIAO Rui(廖蕤)1, 2, YANG Bao-jun(杨宝军)1, 2, YU Shi-chao(于世超)1, 2,

WU Bai-qiang(邬柏强)1, 2, HONG Mao-xin(洪茂鑫)1, 2, WANG Jun(王军)1, 2, ZHAO Hong-bo(赵红波)1, 2, GAN Min(甘敏)1, 2, JIAO Fen(焦芬)1, 2, QIN Wen-qing(覃文庆)1, 2, QIU Guan-zhou(邱冠周)1, 2

1. School of Minerals Processing and Bioengineering, Central South University, Changsha 410083, China;

2. Key Laboratory of Biohydrometallurgy of Ministry of Education, Central South University, Changsha 410083, China

© Central South University Press and Springer-Verlag GmbH Germany, part of Springer Nature 2020

Abstract: Chalcopyrite is one of the most important copper minerals; however, the extracted efficiency of chalcopyrite is still not satisfactory in hydrometallurgy owing to its high lattice energy which leads to its low dissolution kinetics. To overcome the difficulties, many advanced technologies have been developed, including the selection of high effectively bacteria, the inhibition of the passivation film adhered onto the minerals surface, and the maintenance of solution redox potential under an optimum range. Up to date, considerable researches on the first two terms have been summarized, while the overview of the last term has been rarely reported. Based on corresponding works in recent years, key trends and roles of solution redox potential in copper hydrometallurgy, including its definition, effect and maintenance, have been introduced in this review. Key words: chalcopyrite; copper minerals; solution potential; hydrometallurgy process Cite this article as: HUANG Xiao-tao, LIAO Rui, YANG Bao-jun, YU Shi-chao, WU Bai-qiang, HONG Mao-xin, WANG Jun, ZHAO Hong-bo, GAN Min, JIAO Fen, QIN Wen-qing, QIU Guan-zhou. Role and maintenance of redox potential on chalcopyrite biohydrometallurgy: An overview [J]. Journal of Central South University, 2020, 27(5): 1351−1366. DOI: https://doi.org/10.1007/s11771-020-4371-5. 1 Introduction

Chalcopyrite is one of the most plentiful and widespread copper-bearing minerals, accounting for about 70% of copper resource in the earth [1−7], and its chemical formula is often believed in the valence state of Cu+Fe3+S2

2− instead of Cu2+Fe2+ S2

2− [8−11]. Hydrometallurgy technologies for mineral processing and waste processing have been widely developed in recent years, because of their low cost, simple operation and eco-friendly industrial structure [12−26]. The copper extraction from

chalcopyrite in hydrometallurgy process, however, is still recalcitrant due to its high lattice energy, thus leading to its low dissolution kinetics [27−34]. To overcome the worldwide problem in theory and practice, research in the following aspects of this filed has attracted much attention: 1) mutation breeding and screening of high activity strains; 2) inhibition for passivation film formed onto the minerals surface; 3) maintenance for solution redox potential within an optimum range.

It is necessary to breed and screen high activity microbial strains from strain library or nature. Their major role in bio-hydrometallurgical

HUANG Xiao-tao and LIAO Rui contributed equally to this work. Foundation item: Projects(51774332, U1932129, 51804350, 51934009) supported by the National Natural Science Foundation of China;

Project(2018JJ1041) supported by the Natural Science Foundation of Hunan Province, China Received date: 2020-05-04; Accepted date: 2020-05-15 Corresponding author: WANG Jun, PhD, Professor; Tel: +86-731-88876557; E-mail: wjwq2000@126.com; ORCID: 0000-0003-0931-

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applications is to regenerate ferric irons from ferrous irons and protons from sulfur species by oxidation [35, 36]. Different bacteria may have influenced the dissolution kinetics of chalcopyrite, because the physicochemical properties (the hydrophobicity, oxidation-dissolution and dissolution-precipitation of surface elements) of chalcopyrite can be changed by these bacteria adsorbed onto the surface. One rough classification sorts these organisms according to their optimum growth temperature: mesophilic (<40 °C), moderately thermophilic (40−55 °C) and extremely microorganisms (55−80 °C) [37−47]. Passivation of chalcopyrite surface through the formation of an oxide layer can be easily found under the mesophilic conditions, thus leading to the low extraction rate for copper [48−59]. The extremely thermophilic microorganisms are first discovered in the 1960s, they can live and work in more extreme conditions, such as low pH, high temperature, and high-soluble metal concentrations. Due to the absence of cell war, however, they are easily deactivated by high shear stress made by high pulp density, thus affecting the copper extractions [60−65]. Compared with the above-mentioned two bacteria, moderately thermophilic strains have a wider application prospect for they can adapt well to the relatively high temperature in bioreactor and heap leaching process. Thus, they have been paid close attention in recent years [50, 66−70]. The considerably corresponding research completed by researchers is summarized in literatures [71−74]. The dissolution rate of chalcopyrite would be decreased or ceased by the formation of passivation layer coated onto its surface. So, a following problem with its processing at ambient temperatures in the ferric sulfate bioleaching solution is the passivation. The nature of the passivation films is still unclear, although there are many researches about chalcopyrite leaching. One hypothesis is that a sulfur layer would be the main passivating species with chalcopyrite leaching in ferric sulfate solution [75]. And the layer will then block the electron transfer at the solid-liquid interface, thus inhibiting the regeneration of ferric irons from ferrous irons [76]. Another hypothesis is that a copper polysulfide product would be the main products causing the passivation of chalcopyrite in bioleaching [77]. The last hypothesis is that an insoluble sulfate product mainly including jarosite

would be the main passivating species with chalcopyrite bioleaching [61, 78−85]. Therefore, three hypotheses can be summarized based on the above-mentioned as following: formation of a sulfur (S0) layer [79, 86−89], formation of a copper polysulfide (Sn

2−) product [16, 30, 90, 91], and formation of insoluble sulfate (SO4

2−) product [53, 61, 78−83, 92]. In 2019, ZHAO et al [76] summarized the passivation mechanism of chalcopyrite bioleaching. Solution redox potential plays a key role in the leaching of chalcopyrite [35, 93−100]. Fe3+ has been regarded as one of the most important oxidants for chalcopyrite oxidation according to Eq. (1), and then Fe2+ can be oxidized to Fe3+ by O2 and/or microorganisms according to Eq. (2). Redox potential is mainly determined by the ratio of Fe3+/Fe2+ in the ferric sulfate (bio)-leaching solution [101]. CuFeS2

+4Fe3+→Cu2++2S0+5Fe2+ (1) O2

+4Fe2++4H+→4Fe3++2H2O (2) The impact of redox potential on chalcopyrite leaching has been investigated. Preliminary conclusions can be drawn that higher recovery rate can be obtained by controlling the solution potential under an optimum range, even though the specific interaction mechanisms are still controversial [35, 102−111]. Previous work [109] proved a two-step dissolution model that used to explain the above preliminary conclusion, and a mathematic model was put forward to predict the range of optimum redox potential during chalcopyrite bioleaching. The relationship between copper extractions and redox potential under different leaching conditions, such as copper concentration, ferrous/ferric iron concentration and temperature, was revealed by the above model. Hence, the understanding of the role of redox potential and its maintenance would be useful in accelerating of chalcopyrite dissolution. This review is designed to further improve our previous review article that particularly discussed the role of redox potential and its control technology in chalcopyrite leaching. In this review, key trends and roles of solution redox potential in copper hydrometallurgy, such as its definition, effect and maintenance, have been summarized based on the existing research results. The purpose of this review is to provide a guidance for industrial application and waste processing, and

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further industrial application still requires far more effort in the future. 2 Definition of redox potential Redox potential is used to describe an overall reducing or oxidizing capacity in solution [112]. It is the volts of the affinity of a substance for electrons in a redox action compared with the standard hydrogen electrode (usually sets at 0). The electron transfer processes are from the reducing reactant into the oxidizing reactant. Each species has its own intrinsic redox potential, that is, a positive value represents an oxidizing agent that tends to gain electrons, and a negative value indicates a reducing reactant that tends to donate electrons. The redox potential is determined by measuring the difference between a stable reference electrode and an inserting electrode connected each other with a salt bridge, which is measured in millivolts (mV) [113]. It is commonly measured using a platinum electrode rather than gold and graphite electrode with a saturated calomel electrode as reference for its reliable performance. The rapid characterization of redox reaction and prediction on stability of various compounds can be known by measuring the redox potential in leaching solution. Hence, in order to know the detailed dissolution process of chalcopyrite, it is necessary to reveal the role of redox potential firstly. In our group, the role of redox potential in leaching solution has been investigated [95]. Figure 1 shows that the energy of Cu2+/Cu+ is much higher than that of conduction band, and filled states of cuprous overlap with the empty states of chalcopyrite. Therefore, chalcopyrite can capture electrons from cuprous and was reduced to chalcocite. The energy of Fe3+/Fe2+ locates in the band gap and is higher than the Fermi energy of chalcopyrite. Thus, it is difficult for Fe3+ to receive electrons from the chalcopyrite surface, which means that Fe3+ is difficult to leach chalcopyrite. 3 Role of redox potential in

hydrometallurgy of chalcopyrite Redox potential is mainly determined by the concentration ratio of Fe3+ to Fe2+ in aqueous solution during chalcopyrite leaching system, which

Figure 1 Schematic illustration for band structure of chalcopyrite [95] plays an important role in the copper extractive technology [82]. Therefore, this part is carried out to illustrate the effect of redox potential in hydrometallurgy processing. 3.1 Thermodynamic calculation Chalcopyrite can be reduced to chalcocite at a low redox potential, which is easier to dissolve than primary chalcopyrite [106, 108, 114−117]. A mathematic model based on the above was proposed to predict the optimum range of redox potential in chalcopyrite leaching [109]. The main dissolution process of chalcopyrite can be represented by: CuFeS2+3Cu2++3Fe2+→2Cu2S+4Fe3+ (3) CuFeS2+3Cu2++4e－→2Cu2S+Fe2+ (4) Cu2S+4Fe3+→2Cu2++4Fe2++S0 (5) 2Cu2S→4Cu2++8e－+2S0 (6) Equations (7)−(10) can be calculated using equation of Gibbs free energy and Nernst equation, respectively: EH1=482+47.3lgC(Cu2+)−15.77lgC(Fe2+) (7) EH2=481+47.3lgC(Cu2+)−15.77lgC(Fe2+) (8) EL1=362+31.5lgC(Cu2+) (9) EL2=401+29.5lgC(Cu2+) (10)

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where EH1 is the high critical potential for the reaction of Eq. (3); EH2 is the relatively low critical potential for the reaction of Eq. (4); EL1 is the low critical potential for the reaction of Eq. (5) and EL2 is the critical potential for the reaction of Eq. (6); C(Cu2+) and C(Fe2+) represent the concentrations of Cu2+ ions and Fe2+ ions, respectively. Equations (7) and (8) show the value of EH is mainly determined by the ratio of copper concentration and ferrous concentration. As long as the solution redox potential is lower than the value of EH, chalcopyrite can be reduced to chalcocite, then increasing its dissolved rate. Similarly, the copper concentration can determine the value of EL obtained from Eqs. (9) and (10). Therefore, under the optimum range of redox potential EL−EH conditions, the dissolution of chalcopyrite can be accelerated by the formation of chalcocite in both chemical leaching and bioleaching. 3.2 Promoting formation of intermediate

products The optimum range of redox potential is helpful to generate the intermediate products such as bornite or chalcocite onto the surface, thus accelerating the dissolution of chalcopyrite [118]. LIU et al [87] concluded that the above products could be observed in the early state when the redox potential was lower than 500 mV (vs SCE). As time goes, however, these products vanished and the copper extraction was stagnant whilst the redox potential was up to 550 mV (vs SCE). Similarly, the bornite can be observed in a low potential range, and then disappeared in the high range, using the analysis of the leaching residues in the different reaction stages [119]. ZENG et al [120] found that the formation of chalcocite (Cu2S) would be much easier than that of other intermediate products when the redox potential was about 477 mV (vs Ag/AgCl) and similar conclusion is given by other researchers [121, 122]. Furthermore, a two-step leaching mechanism of chalcopyrite was proposed by HIROYOSHI et al [103, 123]. They held that the first step is the reduction of chalcopyrite to chalcocite at low redox potential. Then the newly generated solid species can be oxidized more easily than CuFeS2 in the same condition. Also, GU et al [116] indicated that in the early state chalcopyrite was quickly reduced to chalcocite at a relatively low redox potential, but

no reduced product can be detected at a high redox potential of about 550 mV (vs SCE). XRD patterns of their residues at different leaching stages were carried out to observe the change of generated products. The results indicated that leached residue after 5 days had obvious peaks of chalcocite Cu2S, confirming the reduction of chalcopyrite according to Eq. (5). It is comparatively easy for chalcocite to be leached in the same condition. As time goes, the peaks of chalcocite disappear after 15 and 21 d chalcopyrite bioleaching. It is represented that chalcopyrite is difficult to be reduced to chalcocite during this period. The final copper extraction is much higher in the early states as the redox potential is located at its low point. Similar conclusion is drawn that the chalcocite might be a possible intermediate product during the leaching process [111, 124−127]. Therefore, one effect of redox potential is to prompt the formation of intermediated products, then increasing the dissolution rate of chalcopyrite. Based on the above discussion, a brief model for the effect of redox potential can be proposed in Figure 2. 3.3 Inhibiting formation of passivation layer Redox potential in a suitable range can effectively inhibit the formation of passivation layer covered onto the chalcopyrite surface. Many researchers [30, 61, 79, 128−133] indicated that the low dissolution rate of chalcopyrite mainly owed to the formation of passivation layer coated on the minerals surface, which led to the interaction of reagents with the surface of chalcopyrite becoming more difficult. No passivation layers of chalcopyrite surface were detected in a suitable potential range, whilst its dissolution rate increased greatly at about 420 mV (vs Ag/AgCl) rather than in a high potential range >600 mV [61]. Similar conclusions are drawn by CÓRDOBA et al [134−136], cyclic voltammetry (CV) studies of electrodes with different mass ratios of chalcopyrite to pyrite in sulfuric acid were designed to explain the dynamic process of the products on the surface [137]. It was shown that an obvious anodic peak could be found mainly due to the dissociation of chalcopyrite to the metal- deficient polysulfide, as shown in Eq. (11). It can be clearly known that the current density of peak significantly decreased with the addition of pyrite, confirming that the formation of passivation layer

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Figure 2 A model for effect of redox potential in chalcopyrite leaching polysulfide onto the chalcopyrite surface was obviously inhibited by adding pyrite. In other word, the occurrence of Eq. (11) was inhibited by the addition of pyrite, thus resulting in fast dissolution of chalcopyrite. CuFeS2→Cu1−xFe1−yS2+xCu2++yFe2++2(x+y)e− (y>x)

(11) Therefore, one of the effects of redox potential is to inhibit the formation of passivation layers onto the chalcopyrite surface, leading to the higher copper extractions [138]. To combine the effects of redox potential and apply in complicated leaching solution, bacteria were considered. Figure 3 shows the dissolution and passivation mechanisms model for the effects of redox potential during chalcopyrite bioleaching by moderately thermophilic microorganisms. 4 Maintenance of redox potential It is of great importance to find an eco-friendly way to maintain redox potential so that there is no side effect on chalcopyrite leaching, because redox potential plays a key role in chalcopyrite leaching. Therefore, the main attention of this part is to introduce how to maintain the redox potential in an optimum range, and give some brief comments on existing methods according to our work. 4.1 Using an electro-bioreactor In order to deepen the understanding of

electrochemical bioleaching for the treatment of complex sulfide ores and to use this understanding for analyzing the potential of this process for copper extraction, AHMADI et al [51] employed an electro-bioreactor to control the solution potential in the chalcopyrite leaching. The working electrode using was a reticulated Ti-Pt immersed into the cathodic compartment. The counter electrode was a Pt foil put into the anodic compartment. Ag/AgCl electrode was used as the reference electrode which was close to the working electrode. The potential of the working electrode was maintained with respect to the Ag/AgCl electrode using a potentiostat device. The author found that chalcopyrite can be effectively leached by controlling the redox potential at the range of 400−425 mV (vs. Ag/AgCl), and the copper recovery could be increased up to 35% compared to the chemical leaching and bioleaching. Under this condition, the precipitation of iron oxy-hydroxides onto the surface of chalcopyrite decreased significantly. Although this device can control the potential, some side effect on chalcopyrite leaching could occur such as higher energy consumption in industrial application, and the influence of reactive species •OH based on the result from Refs. [139, 140]. 4.2 Limiting oxygen concentration THIRD et al [108] proposed that redox potential in the leaching solution can be controlled at a fixed setpoint by a computer-controlled solenoid valves with the oxygen limitation (air

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Figure 3 A model for effects of redox potential in chalcopyrite bioleaching supply). The solenoid valves were used to control the redox potential through turning the airflow on or off based on whether the potential was lower or higher than the setpoint in the solution. In other word, redox potential was controlled at a fixed range using the oxygen limitation proposed during bioleaching of chalcopyrite. Redox potential fluctuations in response to the air supply during chalcopyrite bioleaching are shown in Figure 4. The horizontal line at 380 mV is the redox potential setpoint. The intermittent air supply is represented by the second horizontal line, perforations indicate air supply off and continuous line indicates air on. As long as the redox potential fell below the value of setpoint, the air supply was automatically switched on. Within seconds, the redox potential increased to above the setpoint as a result of oxidation from renewed ferrous iron to ferric iron. They found that the dissolution of chalcopyrite is

Figure 4 Redox potential fluctuations in response to air supply during chalcopyrite bioleaching (solid black line) prohibited by redox potential as high as 420 mV (vs Ag/AgCl) and a constant redox potential (380 mV vs Ag/AgCl) resulted in higher copper extractions

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of 52%−61% which was twice that of the former redox potential. Similar conclusions can be found in Ref. [141]. The main problem of this method, however, is that the tube is much easier to plug and damage in industrial application, although the air could be obtained easily. 4.3 Adding different ions Fe3+ has been regarded as one of the most important oxidants for chalcopyrite dissolution, and its reaction product Fe2+ can be oxidized to Fe3+ by O2 and/or microorganisms. In recent work [95], we studied the impact of Fe2+ and Fe3+ on chalcopyrite leaching. The redox potential can be controlled by the ratio of Fe2+ and Fe3+. The copper extractions increased with the addition of ferrous iron, but it decreased with the addition of ferric iron. Moreover, it was lower in the ferric sulfate solution than in blank solution. The initial redox potentials were 270, 420 and 510 mV for 0.1 mol/L Fe2+, 0.05 mol/L Fe3++0.05 mol/L Fe2+, and 0.1 mol/L Fe3+, respectively. In the last two items, the redox potential decreased with the leaching time as a result of the precipitation of ferric iron and/or reduction of ferric iron to ferrous iron. What is interesting is that it increased from 270 to 340 mV in the first 3 d (0.1 mol/L Fe2+), and then increased from 340 to 370 mV slowly. The recovery of copper from chalcopyrite in 0.1 mol/L Fe2+ solution was much higher than that in the 0.05 mol/L Fe3+ + 0.05 mol/L Fe2+, and 0.1 mol/L Fe3+ solutions. Therefore, high copper extractions can be obtained at a low redox potential, in other word, the low redox potential was beneficial to chalcopyrite leaching. Other similar works had been investigated to monitor potential and the rate of reduction Fe3+ by adding ferric ions, ferrous ions and cupric ions, and certain success achieved [142−144]. 4.4 Adding chemical reagents like potassium

permanganate or H2O2 NICOL et al [145] indicated that redox potential can be controlled through the injection of 0.05 mol/L potassium permanganate (K2Cr2O7) solution. Redox potential was monitored using a Pt-ring electrode as working electrode with a combined Ag/AgCl electrode as a reference electrode (3 mol/L KCl). They indicated that the dissolution rate of pyrite was significantly higher at

a potential of 850 mV than at 800 mV (vs SHE). A similar conclusion was drawn by CHANDRA et al [146] who used 15 wt.% H2O2 to control the solution redox potential at solution pH of 1, in the leaching media of HCl, H2SO4 and HClO4. It can be known that the dissolution rate of pyrite was significant faster at solution redox potential of 900 mV (vs SHE) than at 700 mV. And they further found that the leaching rate of pyrite did not increase, although the activity of Fe3+ increased gradually. SUN et al [147] adjusted the redox potential to a setpoint with 15 wt.% H2O2, and found dissolution rate increased fivefold with increasing the redox potential by 100 mV. These investigations confirmed that the solution redox potential significantly affects the mineral dissolution, and can be controlled well by adding chemical reagents like potassium permanganate or H2O2 [148]. 4.5 Adding ferric reductant Pyrite (FeS2, iron disulfide) is the most abundant and widespread sulfide mineral in the earth. O2 and Fe3+ have been recognized as two of the most important oxidants for pyrite oxidation [142−144, 149−156]. Hence, we used pyrite to maintain the solution redox potential. The result for chalcopyrite bioleaching indicated that solution potential was in a relatively lower value after adding pyrite, and it decreased as the mass of pyrite increased. The best control effect is when the mass of pyrite was 3 g (the ratio of chalcopyrite and pyrite is 1:3). The redox potential consistently remains in a relatively stable value 350−370 mV (vs Ag/AgCl) in the first 25 d of bioleaching after adding 3 g pyrite. It arises from the dynamical balance between Fe3+ and Fe2+ concentration. From the results of copper extractions during bioleaching process, no significant difference was found when the mass ratio of chalcopyrite to pyrite was lower than 1:3. And their copper extractions are almost stagnant at about 27% after leaching for 30 d. However, the copper extractions promoted conspicuously and reached up to 70% when the mass ratio of chalcopyrite and pyrite is 1:3. The above results confirmed the conclusions that the optimum range of redox potential can accelerate the dissolution of chalcopyrite resulting in much higher copper extractions.

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Based on the obtained results, a model for revealing the effect of pyrite in chalcopyrite bioleaching is proposed in Figure 5. When the redox potential E is lower than EH, chalcopyrite can be reduced to the chalcocite which is oxidized quickly during bioleaching process. Then the higher copper extraction can be obtained. The proper amount of pyrite addition (high pyrite ratio) is helpful to control the redox potential at an optimal range, which can accelerate the reduction of chalcopyrite and the oxidation of chalcocite, and similar conclusions can be obtained from previous work [137]. Otherwise, for some other ferric reductant such as n-type or p-type chalcopyrite, ascorbic acid may be used to control the potential, and these works have been investigated in our group. 4.6 Adding iron removal agent One of the most feasible schemes for controlling redox potential is to remove ferric (Fe3+) ions in the chalcopyrite leaching. The jarosite, hematite and goethite have been used as iron removing agent to remove iron from acidic solution [157, 158]. Thus, a strategy for controlling the redox potential in an appropriate range through the addition of limonite was proposed by our group and we found it promoted chalcopyrite dissolution through the removal of ferric (Fe3+) ions [159]. Its result for chalcopyrite bioleaching shows that the redox potential increased sharply in the first 5 d and reached a plateau in chalcopyrite bioleaching without adding limonite. Adversely, it can be well controlled at levels lower than 480 mV (vs Ag/AgCl ) by add ing l imoni te . Otherwise ,

chalcopyrite dissolved relatively fast in the first 5 d whilst the redox potential was relatively low in the bioleaching process without the addition of limonite. When it was added into the bioleaching solution, the copper extractions from chalcopyrite was significantly increased, indicating that the addition of iron removal agent can be used to control the redox potential and to prompt the dissolution of chalcopyrite. Based on the above-mentioned discuss, a model for interpreting the strategy to accelerate the dissolution of chalcopyrite through the goethite precipitation process is proposed in Figure 6. The added limonite acted as a role of seed crystals, and induced the goethite precipitation process on the surface of crystal seeds. Otherwise, the precipitation process can remove ferric irons in solution and control the redox potential under an optimal range, thus accelerating the dissolution of chalcopyrite. Furthermore, the presence of crystal seeds can lead to the iron precipitation to occur on their surfaces, rather than the chalcopyrite surfaces, thus inhibiting the formation of passivation layer onto the surfaces of chalcopyrite. 5 Conclusions and prospect 1) Chalcopyrite has low extraction rate and low dissolution kinetics mainly because of the high lattice energy. Three common ways are briefly summarized to solve the problems: select the high effective bacteria, reduce the formation of passivation layers coated onto the surface of minerals, and control redox potential under an optimum range.

Figure 5 A model for revealing effect of pyrite in chalcopyrite bioleaching

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Figure 6 A model for interpreting strategy to accelerate dissolution of chalcopyrite through goethite precipitation process [159] 2) The main effect of redox potential is to prompt the formation of intermediate products and to inhibit the formation of passivation products. 3) The controlling solution redox potential methods can be concluded to employing an electro-bioreactor, limiting oxygen input, adding different ions, adding chemical reagents like potassium permanganate and hydrogen peroxide, and adding ferric reductant or/and iron removal agents. 4) In the future, adding ferric reductant or/and iron removal agents will be a priority for us to solve the problems of high energy consumption caused by using electro-bioreactors and insecurity problems caused by adding chemical reagents (potassium permanganate and hydrogen peroxide). References [1] CORDOBA E M, MUNOZ J A, BLAZQUEZ M L,

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(Edited by YANG Hua)

中文导读

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