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Article

The Effects of Coexisting Copper, Iron, Cobalt, Nickel, and Zinc Ions on Gold Recovery by Enhanced Cementation via Galvanic Interactions between Zero-Valent Aluminum and Activated Carbon in Ammonium Thiosulfate Systems

by
Sanghee Jeon
1,*,
Sharrydon Bright
2,
Ilhwan Park
1,
Carlito Baltazar Tabelin
3,
Mayumi Ito
1 and
Naoki Hiroyoshi
1,*
1
Division of Sustainable Resource Engineering, Faculty of Engineering, Hokkaido University, Sapporo 060-8628, Japan
2
Department of Mining, Chemical and Metallurgical Engineering, Faculty of Engineering, University of Zimbabwe, Harare 00263, Zimbabwe
3
School of Minerals and Energy Resource Engineering, The University of New South Wales, Sydney, NSW 2052, Australia
*
Authors to whom correspondence should be addressed.
Metals 2021, 11(9), 1352; https://doi.org/10.3390/met11091352
Submission received: 30 July 2021 / Revised: 20 August 2021 / Accepted: 25 August 2021 / Published: 27 August 2021
(This article belongs to the Special Issue Advances in Selective Flotation and Leaching Process in Metallurgy)
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Abstract

:
The use of galvanic interactions between zero-valent aluminum (ZVAl) and activated carbon (AC) to recover gold (Au) ions is a promising technique to overcome the challenges due to the poor recovery in ammonium thiosulfate systems, but the applicability to practical Au ore processing remains elusive so far. The present study describes (1) the recovery of Au ions from low Au concentrations, which are typical concentrations used in Au ore processing; and (2) an investigation into the effects of various coexisting base metal ions that can be present in pregnant ore-leached solutions. The results showed that high Au recovery (i.e., over 85%) was obtained even at low Au concentrations under the following conditions: 1:1 of 0.15 g of ZVAl and AC with 10 mL of ammonium thiosulfate solution containing 5 mg/L of Au ions at 25 °C for 1 h in an anoxic atmosphere. Selected coexisting metal ions (i.e., copper, iron, cobalt, nickel, and zinc) were studied to establish their effects on Au recovery, and the results showed that the Au recovery was enhanced (about 90%) when copper ions coexist in the solution with minimal effects from other competing base metal ions.

1. Introduction

Changing international regulations, consumer perceptions, and investor expectations in recent years have pushed for more sustainable and eco-friendly mineral processing and metal extraction technologies [1,2]. In gold (Au) hydrometallurgy, cyanide-based technologies such as carbon-in-pulp (CIP) and carbon-in-leach (CIL) remain widely used in both medium- and large-scale Au mining operations [3]. Unfortunately, cyanide is a very toxic compound that poses serious environmental and health hazards when improperly handled and disposed of, so its use is strictly controlled and prohibited in many countries [1,4].
Among the many alternative methods for Au extraction, copper (Cu)-catalyzed ammonium thiosulfate leaching is one of the most promising because it uses lixiviants that are non-toxic and less corrosive (Equation (1)) [4,5].
Au + 5S2O32− + Cu(NH3)42+ → Au(S2O3)23− + 4NH3 + Cu(S2O3)35−
Furthermore, this approach is effective for the treatment of secondary resources such as e-wastes that contain various types of materials such as plastics, resins, and ferrous, base, and precious metal alloys. Ha et al. [6], for example, reported that over 98% of Au was leached from waste mobile phones. Similarly, Jeon et al. [7] successfully leached 99% of Au from the printed circuit boards (PCBs) of waste mobile phones under the following conditions: 1 M of thiosulfate, 1 M of ammonia/ammonium, and 10 mM of Cu ions for 24 h at 25 °C. Another potential application of Cu-catalyzed ammonium thiosulfate leaching is in the treatment of carbonaceous-type and pyritic Au ores that are unsuitable for cyanide-based methods with the absence of preg-robbing. As a result, remarkable leaching studies for Au ores also have been reported as follows: Molleman and Dreisinger [8] extracted about 84% of Au from pyritic Au concentrate after 24 h using this method, while Ficeriova et al. [9] dissolved 99% of Au within 45 min with complex sulfide concentrates. Despite these promising results, applications of Cu-catalyzed ammonium thiosulfate leaching in industrial-scale plants remain limited to date because an acceptable method for Au ion recovery from pregnant leach liquors/solutions remains elusive [4,7].
Conventional CIP and CIL technologies employ activated carbon (AC) to recover Au ions from pregnant leach solutions, an approach that is simple and highly efficient [1,10]. Although activated carbon is very efficient when used with cyanide, it is ineffective when thiosulfate is employed because of the low adsorption affinity of the larger, more negative Au thiosulfate complex adsorption to the AC [1]. According to Navarro et al. [11], Au recovery by AC adsorption from an ammonium thiosulfate medium was only about 50% after 8 h. Cementation (reductive precipitation), an electrochemical process whereby Au ions are reduced to metallic Au by reductants, is also a well-established recovery technique for cyanide-based technologies. Metal reductants or cementation agents such as zero-valent base metals (e.g., copper (Cu), zinc (Zn), aluminum (Al), and iron (Fe)) are often used. In ammonium thiosulfate, however, cementation of Au ions is difficult because of various unwanted side reactions [7,12,13,14,15]: (1) reduction of Cu ions employed as a catalyst; (2) dissolution of the cementation agents, which leads to high reagent consumption; and (3) formation of oxide/sulfide layers on cementation agents that inhibit Au recovery. Furthermore, abundant sulfur and Cu ions present in the solution restrict the application of solvent extraction and electrowinning for Au ion recovery [1,15].
In our previous study, a novel recovery technique that uses synergistic interactions between zero-valent aluminum (ZVAl) and AC for enhanced Au recovery in the ammonium thiosulfate system was developed [15]. The results showed that ZVAl or AC alone could not recover Au ions, consistent with the results of many previous studies. When mixed, however, over 99% of Au ions could be recovered through the following mechanisms: (i) ZVAl acts as an electron donor while AC as an electron mediator to an Au thiosulfate complex; and (ii) making a galvanic cell, which finally leads to enhanced Au recovery [15]. Although the previous study established a high recovery of Au ions from ammonium thiosulfate solutions, this was obtained in a model solution, which contains only a high concentration of Au ions. This means that the applicability of this technique to real Au ore processing and/or e-waste recycling with a low Au ion concentration and coexisting metal ions remains untested.
The present study aims to assess the applicability of this simple and highly efficient novel recovery technique (ZVAl-AC recovery technique) to real Au ore processing. The objectives of this paper are specifically as follows: (a) to recover Au from the solution with less than 10 mg/L Au, and (b) to investigate the effects of various coexisting metal ions on Au recovery. The previous study on Au ion recovery by the ZVAl-AC technique obtained high Au recovery (i.e., 99%) from the solutions but contained a 100 mg/L concentration of Au ions, which is much higher than the typical Au concentration in ores. There are surely mines containing high Au concentrations such as 150 g/t in Australia [16], 94 g/t in Korea [17], and 60 g/t in China [18], but those mines with high Au contents have been actively explored; hence, currently operating/investigating mines mainly deal with refractory or complex ores with relatively low Au concentrations such as 6 g/t in Laos [19], 6.2 g/t in China [20], 6.2 g/t in Iran [21], or 11.2 g/t in Ghana [22]. Furthermore, Au ore contains minerals such as pyrite, arsenopyrite, chalcopyrite, and/or malachite in which various elements (e.g., Cu, Fe, Co, Ni, and Zn) are incorporated [23,24,25,26,27,28]. Once these elements are dissolved in the solution, they can affect Au recovery by competing and/or co-depositing with Au during the recovery process. Thus, identification of Au recovery mechanisms in solutions with low Au concentrations and coexisting metal ions will be essential in the industrial-scale application of ammonium thiosulfate leaching.
The first objective was achieved by batch-type experiments in ammonium thiosulfate solution containing only Au ions (i.e., Au-thiosulfate solution) at low concentrations (i.e., 5 and 10 mg/L), while for the second objective, different concentrations of coexisting metal ions (i.e., Cu, Fe, Co, Ni, or Zn ions) were added to the Au-thiosulfate solutions with and without Cu ions. The residues were also observed using a scanning electron microscope with energy dispersive X-ray spectroscopy. This study provides a bridge for the application of this simple, highly efficient recovery technique, which has remained in model testing for Au ore processing, and will be helpful for researchers interested in the recovery of Au ions as well as in the behavior of base metal ions in thiosulfate systems.

2. Materials and Methods

2.1. Recovery of Au Ions from Solutions with a Low Au Concentration

The stock ammonium thiosulfate solution containing Au ions (i.e., Au-thiosulfate solution) was prepared by dissolving 5 or 10 mg/L of Au powder (99.999%, Wako Pure Chemical Industries, Ltd., Osaka, Japan) in an ammonium thiosulfate solution containing 1 M of Na2S2O3, 0.5 M of NH3, 0.25 M of (NH4)2SO4, and 10 mM of CuSO4 (pH between 9.5 and 10) using a 300 mL Erlenmeyer flask shaken in a thermostat water bath shaker at 25 °C for 24 h with constant shaking at 120 min−1. The concentration of Au ions in the stock solution was measured by inductively coupled plasma atomic emission spectroscopy (ICP-AES, ICPE-9820, Shimadzu Corporation, Tokyo, Japan) (margin of error = ±2%). Subsequently, 0.15 g of ZVAl (99.99%, Wako Pure Chemical Industries, Ltd., Osaka, Japan) and/or 0.15 g of AC (99.99%, Wako Pure Chemical Industries, Ltd., Osaka, Japan) was mixed with 10 mL of Au-thiosulfate solution in 50 mL Erlenmeyer flasks at 25 °C (shaking at 120 min−1) under nitrogen purging conditions to remove the dissolved oxygen in the solution. After 1 h, the filtrate and residue were separated by filtration using 0.2 μm syringe-driven membrane filters (LMS Co., Ltd., Tokyo, Japan). The residues were washed thoroughly with deionized water (18 MΩ·cm, Mill-Q® Integral Water Purification System, Merck Millipore, Billerica, MA, USA), dried in a vacuum oven at 40 °C, and analyzed by a scanning electron microscope with energy-dispersive X-ray spectroscopy (SEM-EDX, Superscan SSX-550, Shimadzu Corporation, Tokyo, Japan). Meanwhile, the concentrations of Au ions remaining in the filtrates were analyzed by ICP-AES. For validity, accuracy, and replicability of results, experiments were conducted in triplicates.

2.2. Recovery of Au Ions from Solutions Containing Coexisting Metal Ions

In order to investigate the effects of coexisting metal ions on Au recovery using the ZVAl-AC technique, Au-thiosulfate solutions together with base metal ions (Cu, Fe, Co, Ni, and Zn ions) of concentration varying from 0 to 50 mM with and without Cu ions were prepared. The reagents used as sources of competing ions were analytical-grade powders of CuSO4·5H2O, NiSO4·6H2O, FeSO4·7H2O, ZnSO4·7H2O, and CoSO4·7H2O (Wako Pure Chemical Industries Ltd., Osaka, Japan). Subsequently, 10 mL of Au-thiosulfate solution containing each base metal ion was purged with ultra-pure N2 to remove any dissolved oxygen, and then mixed with 0.15 g of ZVAl and AC at 25 °C for 1 h, shaking at 120 min−1. After the predetermined mixing time, the suspension was filtered and the residues were washed thoroughly with deionized water, dried in a vacuum oven at 40 °C, and analyzed by SEM-EDX. Meanwhile, the filtrates were analyzed by ICP-AES. For validity, accuracy, and replicability of results, experiments were conducted in triplicates.

3. Results

3.1. Recovery of Au Ions from Solutions Containing a Low Au Concentration

Figure 1 shows the recovery of Au ions from the ammonium thiosulfate solution containing Au concentrations of 5, 10, and 100 mg/L by ZVAl and AC. Au recovery was calculated according to the following equation:
Au   recovery   ( % ) = [ A u ] ( i ) − [ A u ] ( f ) [ A u ] ( i ) × 100 %
where [Au](i) and [Au](f) are the initial and final Au concentrations, respectively.
The results showed that over 99% of Au was recovered when the initial concentration was 100 mg/L, while about 90% of Au was recovered when the initial concentration was 5 mg/L. The results indicate that recovery slightly decreases as the initial concentration decreases, similar to the results reported by Wang et al. [29] and Nguyen et al. [30] for the cementation of Au ions, but still showed a high recovery of 90%. Figure 1b shows the SEM photomicrographs with corresponding elemental maps of the residue at 10 mL/L of Au initial concentration, and the results showed that Au and Cu were detected on the surface of ZVAl.

3.2. Recovery of Au Ions from Solutions Containing Coexisting Metal Ions

3.2.1. Recovery of Au Ions with Varying Cu Concentrations in the Solution

This section focuses on the effects of Cu ions on Au recovery for the following reasons:
  • Cu ions are an essential catalyst in ammonium thiosulfate systems, increasing Au dissolution in ammonium thiosulfate systems 20- to 25-fold (Equation (1)) [1,4];
  • Cu ions could be introduced via the dissolution of Cu minerals such as chalcopyrite and malachite [23,24,25,26,27,28] found in Au ores.
Figure 2 presents how Cu ions affect Au recovery when using ZVAl and AC. The results show that the initial increase in Cu ion concentration by 10 mM enhanced Au recovery. This could be attributed to the formation of galvanic cells as a consequence of Cu cementation. Galvanic interactions enhance electron transfer from ZVAl to the Au thiosulfate complex, increasing Au recovery [15]. In the second region from 10 to 40 mM Cu, Au recovery was high and consistent at about 90%. In this region, all the Au that can be recovered was already cemented on the ZVAl; hence, increasing Cu ions did not affect Au recovery. In the final region above 40 mM Cu, excess Cu ions began to reduce Au recovery while Cu precipitation still increased. As shown in Figure 3, the decrease in Au recovery could be attributed to the competition between the reduction of Cu species (Equations (3) and (4)) and Au species (Equation (5)) [4,7,12].
SEM-EDX results showed that in the absence of Cu ions (residue at 0 mM Cu), Au was recovered as small point-like depositions on the surface of ZVAl (Figure 2b), while the area of Au deposition increased when Cu concentration increased by 10 and 50 mM (Figure 2b,c), and showed that deposited Au occurs together with deposited Cu.
Cu(NH3)42+ + 3S2O32− +e− → Cu(S2O3)35− + 4NH3
Cu(NH3)42+ + 2e− → Cu + 4NH3
Au(S2O3)23− +e− → Au0 + 2S2O32−

3.2.2. Recovery of Au Ions with Varying Fe, Co, Ni, and Zn Concentrations in the Solution

In this part of the study, various metal ions including Fe, Co, Ni, and Zn ions that could coexist in pregnant Au ore solutions were selected and their effects on Au recovery were elucidated.
The effects of Fe ions on Au recovery are shown in Figure 4. Figure 4a,b shows the recovery of Au ions with varying addition concentrations of Fe ions in the absence and presence of Cu ions in the solution, respectively. In both cases, the results showed that the effects of Fe ions on Au recovery were negligible. This could be explained by the very low solubility of Fe ions under basic conditions [31]; hence, Fe precipitates are readily formed in the solution, which neither favors nor hinders Au recovery. The precipitate in the solution was analyzed by SEM-EDX and showed that Fe precipitates were formed in the solution as shown in Figure 4c. When 10 mM of Cu ions were added to the solution, Au recovery was enhanced and consistently showed about 85–90% Au recovery (Figure 4b), which indicates that Au can be successfully recovered regardless of the presence of Fe ions.
Figure 5a,b shows the results of Au recovery with varying Co ion additions without and with Cu ions, respectively. In the absence of Cu ions (Figure 5a), Au recovery increased to 60% with the addition of 1 mM of Co ions, then decreased as the addition of Co ions increased due to the competitive reduction of Co ions and Au ions. In the presence of Cu ions in the solution, however, Au recovery was about 90%, indicating that the negative effects of Co ions on Au recovery were hindered in the presence of Cu ions and high Au recovery could be obtained (Figure 5b). Figure 5c presents the residue analysis by SEM-EDX. The results show that Co, Au, and Cu were recovered on the surface of ZVAl and deposition areas of Au were very close to that of Cu.
Figure 6a,b shows the effects of Ni ions on Au recovery with varying concentrations without and with Cu ions, respectively. The results showed that in the absence of Cu ions, Au recovery increased to 83% with the addition of 10 mM of Ni ions, then recovery decreased as the addition of Ni ions increased by the competitive reduction. In the presence of Cu ions, however, Au recovery was constantly high at all ranges of Ni ion additions [32]. Figure 6c presents the SEM-EDX analysis of the residue, showing that Ni, Cu, and Au were co-cemented on ZVAl particles.
Figure 7a,b shows the recovery of Au ions with varying additions of Zn ions in the solution from 0.1 to 50 mM without and with Cu ions in the solution, respectively. Without Cu ions, Au recovery increased with the increase in Zn ion addition, while Au recovery remained at an almost constant value of 90% with Cu ions, regardless of the addition of Zn. The SEM photomicrograph with corresponding elemental maps shows that both Zn and Cu were recovered on the surface of ZVAl with Au.
The observed results can be summarized by the following four effects with Figure 8:
  • Effect 1: Fe ions precipitated from solution phase, and they did not affect Au recovery.
  • Effect 2: Zn ions and low concentrations of Co and Ni ions enhanced Au recovery.
  • Effect 3: Higher concentrations of Co and Ni ions suppressed Au recovery.
  • Effect 4: In the presence of Cu ions, the effects of other coexisting metal ions were hindered, i.e., Au recovery was almost constant (the orange section illustrated in Figure 8), regardless of the presence of other coexisting metal ions.
For Effect 1, Fe ions had low solubility and precipitated in the current system and had no effect on Au recovery. Effect 2 (enhanced Au recovery with some of the metal ions) may have occurred due to the formation of new reaction sites for Au deposition: the coexisting metal ions were reduced on the AC (electron mediator) attached to ZVAl, and the deposit elemental metals acted as secondary electron mediators or new cathode sites for Au deposition. Effect 3 (suppressive effect of the coexisting metal ions on Au recovery) can be interpreted by assuming the competition of cementation reactions (reduction of metal ions) between Au and coexisting metal ions: a limited amount of electron flow from the donor (ZVAl) was shared with both the Au and coexisting metal ions, causing a decrease in the amount of Au deposition. At a certain concentration of metal ions, the enhanced effect (Effect 2) shifted to suppressive effect (Effect 3) and Au recovery reached its maximum at that point. The concentrations of coexisting metal ions promoting maximum Au recovery are shown as Memax in Figure 8. The Memax concentration was lowest for Co, followed by Ni, then highest for Zn. This order may correspond to the order of the standard redox potential of these metal ions, as shown in Table 1: the standard redox potential for Co(NH3)63+/Co is higher than that of the others, suggesting that reductive deposition of Co occurs at lower concentrations. This could be the reason why the enhanced Au cementation occurred at low concentrations of Co. For the Ni and Zn, the standard redox potentials are lower than Co, and higher concentrations are needed to form the new cathode site for Au deposition; hence, higher concentrations of Ni and Zn were needed for the enhanced Au recovery.
From an engineering viewpoint, Effect 4 is probably the most noteworthy result here. In the presence of Cu ions, the effects of other coexisting metal ions were hindered, and high Au recovery was achieved (i.e., 85–95%). As show in Table 1, with the exception of Co ions, standard redox potentials of Cu ions are higher than other metal ions [37,38]. When a high concentrations of Cu ions coexists, Cu ions would preferentially be reduced and deposited on AC/ZVAl surfaces [39]. Cu is an electro-conductor, and its conductivity is much higher than that of other metals (Table 2), and it acts as a high-efficiency secondary electron mediator or cathode site, enhancing electron transfer from ZVAl to Au ions (Figure 9). For that, the effects of other coexisting metal ions (especially the suppressive effect of the ions) on Au recovery would be minimized in the presence of Cu ions, and this is schematically illustrated in Figure 9.

3.2.3. Recovery of Au Ions from Solutions Containing Various Coexisting Metal Ions

Figure 10 shows the results of the experiment using the solution containing 10 mM of all base metal ions together with Au ions, like a model solution of pregnant leached solution. The results showed that over 90% of Au was recovered together with Co, Cu, Zn, and Ni, except for Fe ions, and SEM-EDX analysis of the solid product showed that Au and other base metals were deposited on the same sites. This result confirms that high Au recovery is achieved even when other base metal ions coexist in the presence of Cu ions.
The components/concentrations of the elements are different depending on the type as well as the location of the ores. Based on previous studies, typical Cu, Co, Ni, and Zn concentrations in the ore are: Cu at about 250 to 5000 ppm [38,42], Co at about 12 to 50 ppm [39,40], Ni at about 0.002% to 0.03% [43,44], and Zn at about 0.002% to 1.7% [5,43,44,45] (explanation of Fe content was excluded since it does not affect the current leaching/recovery system). In the absence of Cu ions in the solution, the results showed that Au recovery decreased from 0.03 Co/Al mass ratio and 0.04 Ni/Al mass ratio (in the case of Zn ion addition, Au recovery continuously increased to over 0.22 Zn/Al mass ratio) while high and constant Au recovery was obtained in the presence of Cu ions in the solution regardless of the Me/Al mass ratio under the current conditions. In the ammonium thiosulfate system, Cu ions are essentially employed as a catalyst for enhancing the Au extraction rate by 25-fold, and successful Au recovery was obtained from a solution containing various base metal ions. Note that a much higher concentration of the elements can be present in the ore and affect the recovery system, even in the presence of proper Cu ions. In this case, an increase in ZVAl mass ratio could be expected to increase Au recovery. Thus, this novel recovery technique using galvanic interactions between ZVAl and AC can be employed in the treatment of Au ore containing various elements.

4. Conclusions

The present study describes the applicability of a simple and high-efficiency recovery technique by enhanced cementation of galvanic interaction between ZVAl and AC for Au ore processing, which includes:
  • Recovery of Au ions from the solution with low Au concentrations of about less than 10 mg/L;
  • Investigation of the effects of various coexisting metal ions that could be present in ore for Au recovery.
The recovery results showed that recovery efficiency slightly decreases as the initial concentration decreases, but still showed over 85% recovery. Selected coexisting Cu, Fe, Co, Ni, and Zn ions were studied to establish their effects on Au recovery, and the results showed that the Au recovery improved (>85–90%) when Cu ions were present in the solution with minimal effects of other competing base metal ions. The recovery of Au ions from the solution containing Cu, Fe, Co, Ni, and Zn ions was also carried out and the results showed that even if various metal ions coexisted together with Au ions in the solution, over 90% of Au could be recovered. In the ammonium thiosulfate system, Cu ions are employed as an essential catalyst; thus, the results showed a high possibility of applicability to Au ore mining processes.

Author Contributions

Conceptualization, S.J., I.P., M.I. and N.H.; methodology, S.J. and N.H.; investigation, S.J. and S.B.; writing—original draft preparation, S.J. and S.B.; writing—review and editing, S.J., I.P., C.B.T., M.I. and N.H.; project administration, S.J., I.P., M.I. and N.H.; funding acquisition, S.J. All authors have read and agreed to the published version of the manuscript.

Funding

This study was financially supported by Japan Oil, Gas and Metals National Corporation (JOGMEC).

Data Availability Statement

Data available on request due to restrictions, as the research is ongoing.

Conflicts of Interest

The authors declare no conflict of interest.

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Metals 11 01352 g001 550
Figure 1. (a) Recovery of Au ions from ammonium thiosulfate solutions with varying initial concentrations from 5 to 100 mg/L, and (b) SEM photomicrographs with corresponding elemental maps of the recovery residue at 10 mL/L of Au initial concentration.
Figure 1. (a) Recovery of Au ions from ammonium thiosulfate solutions with varying initial concentrations from 5 to 100 mg/L, and (b) SEM photomicrographs with corresponding elemental maps of the recovery residue at 10 mL/L of Au initial concentration.
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Metals 11 01352 g002 550
Figure 2. (a) Recovery of gold ions from ammonium thiosulfate solution with varying additions of Cu ions with concentrations from 0 to 50 mM, and SEM photomicrographs with corresponding elemental maps of the residues at (b) 0 mM, (c) 10 mM, and (d) 50 mM of Cu ion additions.
Figure 2. (a) Recovery of gold ions from ammonium thiosulfate solution with varying additions of Cu ions with concentrations from 0 to 50 mM, and SEM photomicrographs with corresponding elemental maps of the residues at (b) 0 mM, (c) 10 mM, and (d) 50 mM of Cu ion additions.
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Metals 11 01352 g003 550
Figure 3. Schematic diagram of the competitive electron transfer from ZVAl to the Cu complex and the Au-thiosulfate complex.
Figure 3. Schematic diagram of the competitive electron transfer from ZVAl to the Cu complex and the Au-thiosulfate complex.
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Metals 11 01352 g004 550
Figure 4. Recovery of gold ions from an ammonium thiosulfate solution with varying addition of Fe ion concentrations from 0 to 50 mM (a) without and (b) with 10 mM of Cu ions in the solution, and (c) SEM photomicrographs with corresponding elemental maps of the precipitates in the solution.
Figure 4. Recovery of gold ions from an ammonium thiosulfate solution with varying addition of Fe ion concentrations from 0 to 50 mM (a) without and (b) with 10 mM of Cu ions in the solution, and (c) SEM photomicrographs with corresponding elemental maps of the precipitates in the solution.
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Figure 5. Recovery of gold ions from ammonium thiosulfate solutions with varying additions of Co ion concentrations from 0 to 50 mM (a) without and (b) with 10 mM of Cu ions in the solution, and (c) SEM photomicrographs with corresponding elemental maps of residue.
Figure 5. Recovery of gold ions from ammonium thiosulfate solutions with varying additions of Co ion concentrations from 0 to 50 mM (a) without and (b) with 10 mM of Cu ions in the solution, and (c) SEM photomicrographs with corresponding elemental maps of residue.
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Figure 6. Recovery of gold ions from ammonium thiosulfate solution with varying additions of Ni ion concentrations from 0 to 50 mM (a) without and (b) with 10 mM of Cu ions in the solution, and (c) SEM photomicrographs with corresponding elemental maps of the residue.
Figure 6. Recovery of gold ions from ammonium thiosulfate solution with varying additions of Ni ion concentrations from 0 to 50 mM (a) without and (b) with 10 mM of Cu ions in the solution, and (c) SEM photomicrographs with corresponding elemental maps of the residue.
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Figure 7. Recovery of gold ions from an ammonium thiosulfate solution with varying additions of Zn ion concentrations from 0 to 50 mM (a) without and (b) with 10 mM of Cu ions in the solution, and (c) SEM photomicrographs with corresponding elemental maps of residue.
Figure 7. Recovery of gold ions from an ammonium thiosulfate solution with varying additions of Zn ion concentrations from 0 to 50 mM (a) without and (b) with 10 mM of Cu ions in the solution, and (c) SEM photomicrographs with corresponding elemental maps of residue.
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Figure 8. The competitive cementation tendency between Au ions and other base metal ions reacted on the surface of AC attached to ZVAl in the absence of Cu ions.
Figure 8. The competitive cementation tendency between Au ions and other base metal ions reacted on the surface of AC attached to ZVAl in the absence of Cu ions.
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Figure 9. Schematic diagram of the competitive electron transfer from ZVAl to Cu-ammine, Co-ammine, and Au-thiosulfate complex (a) without and (b) with Cu ions in the system.
Figure 9. Schematic diagram of the competitive electron transfer from ZVAl to Cu-ammine, Co-ammine, and Au-thiosulfate complex (a) without and (b) with Cu ions in the system.
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Figure 10. (a) Metal ion recovery from the ammonium thiosulfate solution containing all metal ions (i.e., Au, Co, Cu, Fe, Ni, and Zn ions) over time, and (b) SEM photomicrographs and corresponding elemental maps of the residue.
Figure 10. (a) Metal ion recovery from the ammonium thiosulfate solution containing all metal ions (i.e., Au, Co, Cu, Fe, Ni, and Zn ions) over time, and (b) SEM photomicrographs and corresponding elemental maps of the residue.
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Table
Table 1. Standard redox potentials of Au, Cu, Co, Ni, and Zn in ammonium thiosulfate systems [33,34,35,36,37].
Table 1. Standard redox potentials of Au, Cu, Co, Ni, and Zn in ammonium thiosulfate systems [33,34,35,36,37].
MetalsE0/V
Au(S2O3)23−/Au0.27
Cu(NH3)42+/Cu (S2O3)23−0.22
Co(NH3)63+/Co(NH3)x2+ (x is mainly 5 under the current conditions)0.21
Co(NH3)63+/Co0.1
Cu(NH3)42+/Cu–0.05
Cu(NH3)42+/Cu2S–0.2
Ni(NH3)62+/Ni–0.49
Zn(NH3)42+/Zn–1.04
Table
Table 2. Conductivity of Cu, Zn, Co, and Ni [40,41].
Table 2. Conductivity of Cu, Zn, Co, and Ni [40,41].
MetalsConductivity (S/m × 107 at 25 °C)
Cu5.98
Zn1.7
Co1.6
Ni1.4
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Jeon, S.; Bright, S.; Park, I.; Tabelin, C.B.; Ito, M.; Hiroyoshi, N. The Effects of Coexisting Copper, Iron, Cobalt, Nickel, and Zinc Ions on Gold Recovery by Enhanced Cementation via Galvanic Interactions between Zero-Valent Aluminum and Activated Carbon in Ammonium Thiosulfate Systems. Metals 2021, 11, 1352. https://doi.org/10.3390/met11091352

AMA Style

Jeon S, Bright S, Park I, Tabelin CB, Ito M, Hiroyoshi N. The Effects of Coexisting Copper, Iron, Cobalt, Nickel, and Zinc Ions on Gold Recovery by Enhanced Cementation via Galvanic Interactions between Zero-Valent Aluminum and Activated Carbon in Ammonium Thiosulfate Systems. Metals. 2021; 11(9):1352. https://doi.org/10.3390/met11091352

Chicago/Turabian Style

Jeon, Sanghee, Sharrydon Bright, Ilhwan Park, Carlito Baltazar Tabelin, Mayumi Ito, and Naoki Hiroyoshi. 2021. "The Effects of Coexisting Copper, Iron, Cobalt, Nickel, and Zinc Ions on Gold Recovery by Enhanced Cementation via Galvanic Interactions between Zero-Valent Aluminum and Activated Carbon in Ammonium Thiosulfate Systems" Metals 11, no. 9: 1352. https://doi.org/10.3390/met11091352

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