An electrochemical method to investigate the effects of compound composition on gold dissolution in thiosulfate solution

Zhaohui Zhang; Bailong Liu; Mei Wu; Longxin Sun

doi:10.1515/gps-2020-0033

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An electrochemical method to investigate the effects of compound composition on gold dissolution in thiosulfate solution

Zhaohui Zhang , Bailong Liu , Mei Wu and Longxin Sun

Published/Copyright: September 22, 2020

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From the journal Green Processing and Synthesis Volume 9 Issue 1

Abstract

The electrochemical behavior of gold dissolution in the Cu²⁺–NH₃–S₂O₃²⁻–EDTA solution has been investigated in detail by deriving and analyzing the Tafel polarization curve, as this method is currently widely implemented for the electrode corrosion analysis. The dissolution rate of gold in Cu²⁺–NH₃–S₂O₃²⁻–EDTA solution was determined based on the Tafel polarization curves, and the effects of various compound compositions in a Cu²⁺–NH₃–S₂O₃²⁻–EDTA mixture on the corrosion potential and corrosion current density were analyzed. The results showed that the corrosion potential and polarization resistance decreased, whereas the corrosion current density increased for certain concentrations of S₂O₃²⁻–NH₃–Cu²⁺ and EDTA, indicating that the dissolution rate of gold had changed. The reason for promoting the dissolution of gold is also discussed.

Keywords: thiosulfate; anodic dissolution; Tafel polarization curve; electrochemical behavior

1 Introduction

Gold extraction has always been a highly polluting and toxic process due to the use of cyanide [1]. The leaching of gold in the thiosulfate solution is a promising noncyanide gold leaching method that is widely implemented [2,3,4,5]. In this method, the gold leaching rate can be optimized at room temperature when the thiosulfate, ammonia, and copper ions coexist in the gold leaching agent [6,7,8]. The leaching of gold in a copper–ammonia–thiosulfate system over a prolonged period was studied in detail [9,10,11,12,13]. A number of studies have shown faster gold leaching kinetics with thiosulfate in the presence of ammonia and copper(ii) in the form of a cupric tetraamine complex [14,15]. However, because the chemical reactions of a gold leaching process become complex when ammonia and copper ions coexist in the thiosulfate solution [16,17,18], the mechanism of gold leaching in the Cu²⁺–NH₃–S₂O₃²⁻–EDTA solution has yet to be fully elucidated. The electrochemical catalytic mechanism of gold leaching in the ammoniacal thiosulfate solution has been proposed [19,20,21] based on the results of electrochemical studies on the anodic and cathodic reactions in the gold leaching process. The electrochemical studies revealed the dependence of the electroleaching rate in thiosulfate–ammonia solutions on different processes controlled by the anodic potential [22,23]. The cathodic and anodic processes were evaluated in a potential window where the reduction of gold and copper and the oxidation of thiosulfate and Cu(i) species occur [23]. The reaction of Cu(NH₃)₄²⁺ transformation into Cu(S₂O₃)₃⁵⁻ plays the dominant role in the cathode reaction, which is a rapid process [24,25,26,27,28]. Conversely, the oxidation reaction of gold is inhibited in the anodic reaction. Currently, some views show that the gold dissolution process may be interfered due to the large amount of copper present in the solutions [29,30]. Thus, the present study aims to clarify the effects of compound composition on gold dissolution in the thiosulfate solution.

The dissolution of gold is an anodic corrosion process. The electron transfer rate is proportional to the rate of gold dissolution due to the electron transfer in the process of gold dissolution; thus, the dissolution rate of gold can be described by the corrosion current density (J_corr). It has been reported that the anodic dissolution of gold can be controlled by an electrochemical reaction under certain conditions [31,32]. In addition, previous researchers have studied the electrochemical behavior of gold dissolution in the Cu²⁺–NH₃–S₂O₃²⁻–EDTA solution by employing the standard electrochemical method and by subsequently deriving and analyzing the steady-state polarization curves and the constant-current step curves [21,22,23]. However, although the Tafel polarization curve is an important tool for the analysis of electrode corrosion, there are few reports on the dissolution mechanism of gold in Cu²⁺–NH₃–S₂O₃²⁻–EDTA solutions.

Because the electron transfer rate is proportional to the gold dissolution rate in the oxidation–dissolution process of gold, the dissolution rate of gold can be characterized by the corrosion current density. The corrosion rate can be determined by the Tafel polarization curve [33,34,35,36]; more specifically, the corrosion potential (E_corr) and its corresponding corrosion current can be obtained based on the anodic polarization curve and cathodic polarization curve of the Tafel curve, which intersect at a single point. According to the Tafel polarization curves, the values of J_corr, E_corr, and polarization resistance (R_p) can be obtained by using ZSimpWin software to perform fitting.

In this study, the dissolution rate of gold in a Cu²⁺–NH₃–S₂O₃²⁻–EDTA mixture was determined by deriving and analyzing the Tafel polarization curves, and the effects of modifying the composition of a Cu²⁺–NH₃–S₂O₃²⁻–EDTA mixture on the dissolution behavior of gold were analyzed. The mechanisms for promoting gold dissolution and the main control steps of the gold leaching reaction are also discussed.

2 Experimental

This study was performed by employing a three-electrode scheme in an electrochemical system. Furthermore, the electrochemical behavior of gold dissolution in a mixture was investigated by using a CHI600E electrochemical workstation (Shanghai Huachen, China). In this study, Pt wire with a surface area of 1.0 cm², Ag/AgCl (in saturated KCl), and pure gold with a surface area 1.0 cm² were used as the counter electrode, reference electrode, and working electrode, respectively, to form a three-electrode system [37].

The polarization curves were obtained at a scan rate of 10 mV s⁻¹. The potential range used in this study was +1500 to −1500 mV Ag/AgCl. The surface of the working electrode was mechanically polished (using alumina powder) and rinsed off with distilled water.

The reagents used were as follows: pure gold (Au, 99.99%; Luoyang, China), copper(ii) sulfate (CuSO₄·5H₂O; Panreac), sodium thiosulfate (Na₂S₂O₃·5H₂O; Tianjin, China), ammonium hydroxide (NH₃·OH; Guangzhou, China), sodium hydroxide (NaOH; Guangzhou, China), and EDTA (C₁₀H₁₄N₂O₂Na₂·2H₂O; Tianjin, China). The reagents used in the experiment are all analytical reagents, and the experimental temperature was maintained at 25°C by implementing water bath immersion.

According to the literature [21,22,23], the concentration of S₂O₃²⁻ was increased from 0.01 to 0.9 mol/L in the Cu²⁺–NH₃–S₂O₃²⁻–EDTA solution. The concentration of NH₃ was 0–0.8 mol/L, and the concentration of Cu²⁺ was 0–0.8 mol/L. The pH of solution was determined, when the mixed solution was determined.

3 Results and discussion

3.1 Effect of S₂O₃²⁻ concentration

The Tafel polarization curves for gold dissolution are shown in Figure 1 for varying S₂O₃²⁻ concentrations in the absence of NH₃ and Cu²⁺; the corrosion rate was measured by fitting the polarization curve. Figure 2 shows that the corrosion current density of the gold dissolution process consistently increased with increasing S₂O₃²⁻ concentration, indicating that the composition of S₂O₃²⁻ contributes to the improvement of the corrosion rate of gold. Moreover, when the concentration of S₂O₃²⁻ was increased from 0.01 to 0.1 mol/L, the corrosion current density also increased from 0.540 × 10⁻⁶ to 1.714 × 10⁻⁶ A/cm². However, as the concentration of S₂O₃²⁻ continued to increase, the amplitude of J_corr was observed to progressively decrease.

Figure 1

Tafel plots of gold dissolution at different S₂O₃²⁻ concentrations.

Figure 2

Electrochemical parameters of gold dissolution at different S₂O₃²⁻ concentrations: (a) corrosion current density of gold dissolution; (b) corrosion potential of gold dissolution; and (c) polarization resistance of gold dissolution.

Increasing the S₂O₃²⁻ concentration was also found to correspond to a decrease of the corrosion potential from −0.119 to 0.208 V, resulting in a reduced E_corr value and increased corrosion. In addition, increasing the S₂O₃²⁻ concentration can reduce the corrosion potential of gold and thus facilitate dissolution. These findings indicate that the composition of S₂O₃²⁻, as it enhances the ability of the solution to corrode materials and accelerates the process of gold dissolution.

The kinetics of the corrosion rate of the electrode reaction are described by the linear polarization resistance. At lower polarization resistances, gold is more likely to be dissolved when the corrosion current density is higher. Furthermore, increasing the S₂O₃²⁻ concentration was found to initially decrease the linear polarization resistance before gradually increasing. Therefore, to promote the dissolution of gold in the system, the concentration of S₂O₃²⁻ should be controlled at approximately 0.1 mol/L.

3.2 Effects of NH₃ concentration

Figures 3 and 4 show that the corrosion current density increased with increasing NH₃ concentration. In addition, the decreasing corrosion potential observed in the figures indicates that the composition of NH₃ can also play a role in improving the corrosion rate of gold.

Figure 3

Tafel plots of gold dissolution with different ammoniacal concentrations.

Figure 4

Electrochemical parameters of gold dissolution with different ammoniacal concentrations: (a) corrosion current density of gold dissolution; (b) corrosion potential of gold dissolution; and (c) polarization resistance of gold dissolution.

As the concentration of NH₃ increased, the corrosion potential of −0.178 V decreased to −0.236 V. It was also found that further increasing the NH₃ concentration reduced the corrosion potential of gold, thereby facilitating the process of gold dissolution. Furthermore, as the concentration of NH₃ was increased, the linear polarization resistance decreased, making the gold more susceptible to corrosion. These results demonstrate that the corrosion resistance of the solution can be enhanced by adding NH₃ to the S₂O₃²⁻ solution, which can accelerate the dissolution of gold.

3.3 Effects of Cu²⁺ concentration

In the thiosulfate solution system, the composition of NH₃ stabilized the copper ion in the solution. When the concentration of NH₃ was insufficiently low, it was too difficult to stabilize Cu²⁺ to enable the production of Cu(OH)₂ in the solution. Therefore, it is necessary to introduce additives to stabilize Cu²⁺ in ammoniacal thiosulfate solutions with low NH₃ concentrations [20,38]. The Tafel curves for various copper concentrations are shown in Figure 5.

Figure 5

Tafel plots of gold dissolution with different copper concentrations.

Figure 6 shows that the corrosion current density significantly increased with the addition of Cu²⁺, while the corrosion potential was further reduced to −0.253 V. This indicates the significance of the role of thiosulfate solution-immersed copper in the catalytic oxidation of gold.

Figure 6

Electrochemical parameters of gold dissolution with different copper concentrations: (a) corrosion current density of gold dissolution; (b) corrosion potential of gold dissolution; and (c) polarization resistance of gold dissolution.

When the concentration of Cu²⁺ was increased from 0 to 0.2 mol/L, the polarization resistance was observed to rapidly decrease. However, further increase of the concentration of Cu²⁺ resulted in a slower polarization resistance decrease. This indicates that the Cu²⁺ in solutions can enhance the corrosion ability of the solution and accelerate the dissolution of gold.

3.4 Effects of EDTA concentration

The results illustrated in Figures 7 and 8 show that adding EDTA can reduce the corrosion potential and increase the gold dissolution tendency within the 0.05–0.2 g/L EDTA concentration range.

Figure 7

Tafel plots of gold dissolution at different EDTA mass concentrations.

Figure 8

Electrochemical parameters of gold dissolution at different EDTA mass concentrations: (a) corrosion current density of gold dissolution; (b) corrosion potential of gold dissolution; and (c) polarization resistance of gold dissolution.

As mentioned earlier, an increase in the corrosion current density was found to correspond to the decreased linear polarization resistance, which is suggested to accelerate the gold dissolution rate. This is because it is common for the complex stability constants of Cu²⁺ and EDTA to be larger than those of Cu²⁺ and NH₃ [11], which leads to the reduced electrode potential of Cu²⁺/Cu⁺. In addition, it has been confirmed in this study that the addition of EDTA can reduce the corrosion potential of gold from −0.253 to −0.302 V and that the dissolution of gold would be accordingly accelerated.

When the amount of EDTA was excessive, the corrosion current density was observed to rapidly decrease, while the polarization resistance rapidly increased. During this time, the corrosion rate of gold was significantly less than that of the solution without EDTA. The reason for this is that the addition of EDTA to the Cu²⁺–NH₃–S₂O₃²⁻ mixture would produce CuY²⁻ by complexing with Cu²⁺. The complexes in the solution would thus significantly reduce the concentration of free Cu²⁺ [18]. Therefore, when the potential of the mixed solution is excessively low, gold cannot be easily dissolved. Furthermore, it was found that the amount of EDTA should be maintained within the 0.05–0.2 g/L range.

4 Conclusions

Under the experimental conditions of an S₂O₃²⁻ concentration of 0–0.09 mol/L, NH₃ concentration of 0–0.8 mol/L, and a Cu²⁺ concentration of 0–0.8 mmol/L, the corrosion potential and polarization resistance decreased with increasing concentrations of S₂O₃²⁻ and NH₃, whereas the corrosion current density increased. In addition, the corrosion current density significantly increased with the addition of Cu²⁺. The experimental results indicate that the presence of Cu²⁺ can strengthen the catalytic ability of gold oxidation in the thiosulfate solution.
Under the condition of 0.1 mol/L S₂O₃²⁻, 0.4 mol/L NH₃, 0.8 mmol/L Cu²⁺, and 0.05–0.2 g/L EDTA, the addition of EDTA can reduce the corrosion potential and increase the corrosion current density, thereby facilitating the dissolution of gold. However, a high concentration of EDTA will decrease the corrosion current density and increase the corrosion potential, leading to a decreased gold corrosion rate.

References

[1] Ma HZ, Yan C, Wang YN. Pretreatment of arsenic-bearing gold ore with microwave-assisted alkaline leaching. Green Proc Synth. 2016;5(3):269–73.10.1515/gps-2015-0122Search in Google Scholar

[2] Zhong J, Hu X, Zi F, Yu H. Current situation and development of gold leaching with thiosulfate. Mining Metall. 2014;23(2):65–69.Search in Google Scholar

[3] Sandenbergh R, Miller J. Catalysis of the leaching of gold in cyanide solutions by lead, bismuth and thallium. Min Eng. 2015;14(11):1379–86.10.1016/S0892-6875(01)00152-2Search in Google Scholar

[4] Puente-Siller D, Fuentes-Aceituno J, Nava-Alonso F. A kinetic–thermodynamic study of silver leaching in thiosulfate–copper–ammonia–EDTA solutions. Hydrometallurgy. 2013;134–5:124–31.10.1016/j.hydromet.2013.02.010Search in Google Scholar

[5] Wang F, Dai H, Cui Y. Review on recovery of gold and silver from thiosulfate leaching solution by cementation method. J Kunming Univ Sci Technol. 2017;42(2):1–6.Search in Google Scholar

[6] Breuer P, Jeffrey M. An electrochemical study of gold leaching in thiosulfate solutions containing copper and ammonia. Hydrometallurgy. 2002;65:145–57.10.1016/S0304-386X(02)00086-5Search in Google Scholar

[7] Aylmore M, Muir D. Thermodynamic analysis of gold leaching by ammoniacal thiosulfate using Eh/pH and speciation diagrams. Min Metall Proc. 2001;18(4):221–7.10.1007/BF03403254Search in Google Scholar

[8] Munive G, Romero MA, Vazquez VM, et al. Dissolution of gold and silver with ammonium thiosulfate from mangano-argentiferous ores treated in acid-reductive conditions. JOM. 2017;69(10):1901–8.10.1007/s11837-017-2338-2Search in Google Scholar

[9] Porvali A, Rintala L, Aromaa J, Kaartinen T, Forsen O, Lundström M. Thiosulfate–copper–ammonia leaching of pure gold and pressure oxidized concentrate. Physicochem Probl Miner Process 2017;53(2):1079–91.Search in Google Scholar

[10] Xu B, Li K, Zhong Q, Li Q, Yang Y, Jiang T. Study on the oxygen pressure alkaline leaching of gold with generated thiosulfate from sulfur oxidation. Hydrometallurgy. 2018;177:178–86.10.1016/j.hydromet.2018.03.006Search in Google Scholar

[11] Aylmore M, Muir D, Staunton W. Effect of minerals on the stability of gold in copper ammoniacal thiosulfate solutions – the role of copper, silver and polythionates. Hydrometallurgy. 2014;143:12–22.10.1016/j.hydromet.2013.12.001Search in Google Scholar

[12] Liu X, Xu B, Yang Y, Li Q, et al. Effect of galena on thiosulfate leaching of gold. Hydrometallurgy. 2017;171:157–64.10.1016/j.hydromet.2017.05.011Search in Google Scholar

[13] Li X, Xu B, Min X, Li Q, et al. Effect of pyrite on thiosulfate leaching of gold and the role of ammonium alcohol polyvinyl phosphate (AAPP). Metals. 2017;278(7):1–17.10.3390/met7070278Search in Google Scholar

[14] Sitando O, Senanayake G, Dai X, Nikoloski AN, Breuer P. A review of factors affecting gold leaching in non-ammoniacal thiosulfate solutions including degradation and in-situ generation of thiosulfate. Hydrometallurgy. 2018;178:151–75.10.1016/j.hydromet.2018.02.016Search in Google Scholar

[15] Xu B, Kong W, Li Q, Yang Y, Jiang T, et al. A review of thiosulfate leaching of gold: focus on thiosulfate consumption and gold recovery from pregnant solution. Metals. 2017;7(6):222.10.3390/met7060222Search in Google Scholar

[16] Breuer PL, Jeffrey MI. Thiosulfate leaching kinetics of gold in the presence of copper and ammonia. Min Eng. 2000;13(10–11):1071–81.10.1016/S0892-6875(00)00091-1Search in Google Scholar

[17] Zhang S, Nicol M. An electrochemical study of the dissolution of gold in thiosulfate solutions part I: alkaline solutions. J Appl Electrochem. 2003;33(9):767–75.10.1023/A:1025502303122Search in Google Scholar

[18] Zelinsky AG, Novgorodtseva ON. Effect of thiourea on the rate of anodic processes at gold and graphite electrodes in thiosulfate solutions. Electrochim Acta. 2013;109(11):482–8.10.1016/j.electacta.2013.07.103Search in Google Scholar

[19] Zhang S, Nicol M. An electrochemical study of the dissolution of gold in thiosulfate solutions. Part II: effect of copper. J Appl Electrochem. 2005;35(3):339–45.10.1007/s10800-004-7469-9Search in Google Scholar

[20] Aazami M, Lapidus G, Azadeh A. The effect of solution parameters on the thiosulfate leaching of Zarshouran refractory gold ore. Int J Min Proc. 2014;131(43–45):43–50.10.1016/j.minpro.2014.08.001Search in Google Scholar

[21] Cui J, Zhang L. Metallurgical recovery of metals from electronic waste: a review. J Hazardous Mater. 2008;158(2–3):228–56.10.1016/j.jhazmat.2008.02.001Search in Google Scholar PubMed

[22] Urzúa-Abarca DA, Fuentes-Aceituno JC, Uribe-Salas A, Lee JC. An electrochemical study of silver recovery in thiosulfate solutions. A window towards the development of a simultaneous electroleaching-electrodeposition process. Hydrometallurgy. 2018;176:104–17.10.1016/j.hydromet.2018.01.017Search in Google Scholar

[23] Tamayo JA, Gómez S, Calderón JA, Tamayo JA, et al. Selective electrochemical gold recovery from leaching solutions of thiosulfate. J Electrochem Soc. 2017;164(7):363–70.10.1149/2.0341707jesSearch in Google Scholar

[24] Heath F, Jeffrey M, Zhang H, Rumball J. Anaerobic thiosulfate leaching: development of in situ gold leaching systems. Min Eng. 2008;21(6):424–33.10.1016/j.mineng.2007.12.006Search in Google Scholar

[25] Chandra I, Jeffrey M. An electrochemical study of the effect of additives and electrolyte on the dissolution of gold in thiosulfate solutions. Hydrometallurgy. 2004;73:305–12.10.1016/j.hydromet.2003.12.002Search in Google Scholar

[26] Breuer P, Jeffrey M, Tan E, Bot A. The electrochemical quartz crystal microbalance as a sensor in the gold thiosulfate leaching process. J Appl Electrochem. 2002;32(10):1167–74.10.1023/A:1021203309602Search in Google Scholar

[27] Choo W, Jeffrey M. An electrochemical study of copper cementation of gold(i) thiosulfate. Hydrometallurgy. 2004;71(3–4):351–62.10.1016/S0304-386X(03)00087-2Search in Google Scholar

[28] Jeffrey M, Ritchie I. The leaching of gold in cyanide solutions in the presence of impurities II. The effect of silver. J Electrochem Soc. 2000;147(9):3272–6.10.1149/1.1393894Search in Google Scholar

[29] Grosse AC, Dicinoski GD, Shaw MJ, Haddad PR. Leaching and recovery of gold using ammoniacal thiosulfate leach liquors (a review). Hydrometallurgy. 2003;69:1–21.10.1016/S0304-386X(02)00169-XSearch in Google Scholar

[30] Aylmore M, Muir D. Thiosulfate leaching of gold – a review. Min Eng 2001;14(2):135–74.10.1016/S0892-6875(00)00172-2Search in Google Scholar

[31] Guzman L, Segarra M, Chimenos J, Cabot P, Espiell F. Electrochemistry of conventional gold cyanidation. Electrochim Acta. 1999;44(15):2625–32.10.1016/S0013-4686(98)00392-2Search in Google Scholar

[32] Jeffrey M. Kinetic aspects of gold and silver leaching in ammonia–thiosulfate solutions. Hydrometallurgy. 2001;60:7–16.10.1016/S0304-386X(00)00151-1Search in Google Scholar

[33] Bandy R. The simultaneous determination of tafel constants and corrosion rate – a new method. Corros Sci. 1980;20(8):1017–28.10.1016/0010-938X(80)90081-5Search in Google Scholar

[34] Feng D, Deventer J. Ammoniacal thiosulphate leaching of gold in the presence of pyrite. Hydrometallurgy. 2006;82(3):126–32.10.1016/j.hydromet.2006.03.006Search in Google Scholar

[35] Senanayake G, Zhang X. Gold leaching by copper(ii) in ammoniacal thiosulphate solutions in the presence of additives. Part II: effect of residual Cu(ii), pH and redox potentials on reactivity of colloidal gold. Hydrometallurgy. 2010;96(4):21–29.10.1016/j.hydromet.2011.11.010Search in Google Scholar

[36] Phan TB, Mai TX, Nauyen TD, Pham TT, et al. Improving the electrochemical behavior of sustainable polyaniline titanium dioxide composite by intercalation of carbon nanotubes. Green Proc Synth. 2016;5(6):549–56.10.1515/gps-2016-0109Search in Google Scholar

[37] Yang Y. Electrochemical sensor for ultrasensitive determination of bisphenol a based on gold nanoparticles/β-cyclodextrin functionalized reduced graphene oxide nanocomposite. Int J Electrochem Sci. 2016;11(4):2778–89.10.1016/S1452-3981(23)16140-2Search in Google Scholar

[38] Feng D, Deventer J. Thiosulphate leaching of gold in the presence of ethylenediaminetetraacetic acid (EDTA). Min Eng. 2010;23(2):143–50.10.1016/j.mineng.2009.11.009Search in Google Scholar

Received: 2019-12-01

Revised: 2020-05-05

Accepted: 2020-05-06

Published Online: 2020-09-22

This work is licensed under the Creative Commons Attribution 4.0 International License.

Articles in the same Issue

https://doi.org/10.1515/gps-2020-0033

Keywords for this article

thiosulfate; anodic dissolution; Tafel polarization curve; electrochemical behavior

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An electrochemical method to investigate the effects of compound composition on gold dissolution in thiosulfate solution

Article

Abstract

1 Introduction

2 Experimental

3 Results and discussion

3.1 Effect of S2O32− concentration

3.2 Effects of NH3 concentration

3.3 Effects of Cu2+ concentration

3.4 Effects of EDTA concentration

4 Conclusions

References

Articles in the same Issue

Articles in the same Issue

Articles in the same Issue

3.1 Effect of S₂O₃²⁻ concentration

3.2 Effects of NH₃ concentration

3.3 Effects of Cu²⁺ concentration