1. Introduction
Mineral processing and metallurgical operations have taken a new turn according to the type of copper production being used. Innovation and new mineral processing alternatives are essential to maintaining copper production [
1,
2,
3]. Production by hydrometallurgical processes has started to decline, and new techniques are required to overcome various processing challenges [
4,
5,
6,
7], one of which is the increasing arsenic content in copper deposits. According to government regulations, when arsenic cannot be recovered from a process and is eliminated as waste, it must be confined in a stable environment [
8,
9,
10].
Arsenic is one of the most toxic and carcinogenic elements. In solution, it can be absorbed by vegetation and pass through the food chain to human beings [
11,
12,
13,
14]. Arsenic can be found in a natural state, as well as in sulphides such as realgar, enargite and orpiment, as arsenide in oxides and as arsenate. Arsenopyrite (FeSAs) is the most common arsenic mineral [
15]. In copper ores, arsenic is often contained in tennantite (Cu
12As
4S
13) and enargite (Cu
3AsS
4) [
16], which are respectively 20.2% and 19.0% arsenic [
17]. This is why the final disposition of arsenic must be controlled, and to do this it is necessary to establish the form of arsenic that is present in order to stabilize and confine it over the long term.
Numerous studies have considered the most stable arsenic form for final disposal. It has been concluded that As
5+ is more stable than As
3+ [
18]. Studies by [
19] have indicated that arsenate (As
5+) can precipitate in the presence of (Mn
3+) in oxidizing environments. Therefore, the presence of a high concentration of manganese can positively influence arsenic precipitation. Precipitation with lime is a widespread practice despite consensus about the low arsenic concentration content and low long-term stability of the resulting precipitates. Precipitation of As
+5 with lime at room temperature results in the formation of various calcium arsenate compounds, including Ca
4(OH)
2(AsO
4)
2·4H
2O, Ca
5(AsO
4)
3OH and Ca
3(AsO
4)
2, as well as CaHAsO
4·
xH
2O and Ca
5H
2(AsO
4)
4. These compounds depend on the concentration and oxidation state of arsenic, calcium and SO
42− and/or HSO
4−. It should be noted that there is evidence that calcium arsenate compounds decompose upon contact with atmospheric CO
2 or carbonate ions to form calcium carbonate and a soluble arsenic acid [
18].
The best alternative for arsenic stabilization is the formation of scorodite (FeAsO
4·2H
2O) [
20,
21,
22], which is capable of containing between 20–25% of As [
23] and is stable under oxidizing conditions in the pH range of 2.0–6.0 [
18,
24]. The formation of scorodite at atmospheric pressure requires strict rigor with respect to the pH. It has been determined that As
+5 precipitation at ambient pressure is directly affected by the pH level, with values over 4 resulting in the oversaturation of iron and arsenic in the solution, thus forming amorphous iron-arsenic compounds that are not stable for depositing [
25]. Scorodite formation is reflected in the kinetics of its transformation, pH 1 is the established value, while at pH 2 it is moderate and at pH 4.5 the kinetics are slow [
26]. Another factor to consider in the coprecipitation of As is the oxidation of As
3+ to As
5+. Oxidation is important because the successful removal of arsenic requires that it be in the form of arsenate, especially when scorodite is formed [
21,
27].
This research analyzes the feasibility of incorporating the effluent solution from a metallurgical flue dust treatment plant (PLS-P) from a copper smelter to a copper hydrometallurgical plant. In this way, it is expected that the copper, acid and water, that are currently lost due to the high arsenic content, can be recovered and that the arsenic can be fixed in a stable form in the heap leaching residue, allowing for its disposal in a confined and environmentally safe area.
2. Materials and Methods
To determine the behavior of arsenic and iron in the effluent flue dust solution (PLS-P) of a copper smelter when it is incorporated into an industrial copper leaching process, a set of six column-leaching tests were performed.
Table 1 shows the details of the pH and solution potential (Eh) for the leaching columns (C-1, C2, C3, C4, C5 and C6).
A representative sample of mineral used in the Lomas Bayas mining process was characterized by chemical analysis using inductively coupled plasma atomic emission spectroscopy (ICP-AES) via the model Optima 2000 DV (PerkinElmer, Überlinge, Germany), with a detection limit of 0.01 ppm for Cu and Fe and 0.5 ppm for As. A pulverized mineral sample was analyzed by X-ray analysis (Siemens model D5600, Bruker, Billerica, MA, USA), with an analysis time of one hour. The ICDD (International Center for Diffraction Data) database was used to identify the species that were present.
To perform the microscopy analysis, a polished briquette (Buehler Simplimet 2 briquetting machine) was made with transoptic powders and was characterized by scanning electron microscopy (SEM) using JEOL 6360-LV equipment (JEOL USA Inc., Peabody, MA, USA) and by an energy-dispersive X-ray spectroscopy (EDX) microanalysis system (Zeiss Ultra Plus, Zeiss, Jena, Germany), operated at 30 kV under high vacuum conditions. Finally, the samples were also studied under a BX-51 reflected-light microscope (Olympus, Tokyo, Japan).
The size distribution was characterized in two stages, the first using mesh sizes of 1″, , , , 6#, 10# and −10# mesh (Tyler). In the second stage, a 500 g (−10#) mineral sample was classified using 20, 30, 50, 70, 100, 140, 200, 270, 325 and 400# meshes (Tyler). Moisture was determined by the weight difference of a mineral sample before and after being dried at 95 °C in an oven for 14 h.
The ore from the heap leaching was loaded into columns 48 cm high and 9.5 cm in diameter. The columns were irrigated independently in duplicate with a mixed solution of PLS-P and Lomas Bayas heap leaching solution in a 1/10.74 ratio, with 1 g/L arsenic. The initial pH (0.8) and the solution potential (510 mV) with respect to the standard hydrogen electrode (SHE), were the natural values of the blend. Both the pH and the solution potential were conditioned according to
Table 1, and NaOH and H
2SO
4 (Merk, analytical grade) were used to control the pH of the solution. To regulate the solution potential up to 540 mV, ozone was injected into the solution for 5 min, using an ozonator model L21 (Pacific Ozone, Benicia, CA, USA), fed with oxygen through an oxygen generator system. The conditioned solution was irrigated in the columns, and the pregnant leach solution (PLS) was recirculated in the columns until completion of a 94-day leaching cycle.
The columns were irrigated using a multi-head MasterFlex peristaltic pump at a rate of 10 (L/h)/m
2. The drained solutions from the columns were collected separately, sampled every five days and analyzed with an Absorption Spectrometer, (SpectrAA-50/55, Varian, Santa Clara, CA, USA) for As(total), As
3+, As
5+ using HG-FAAS (hydride generation with pH speciation), and using FAAS (flame atomic adsorption spectrometry with pH speciation) in the case of Fe
(total), Fe
2+, Fe
3+ and Cu
2+.
Figure 1 shows a schematic of the system used. At the end of the cycle (94 days), the irrigation was discontinued and the columns were drained for three days and discharged. A sample was taken from the leaching residue that was obtained in each column for physical, chemical, X-ray and SEM analysis.
Author Contributions
Conceptualization, O.B., M.C.H. and Y.Z.; methodology, O.B., M.C.H. and Y.S.; validation, O.B.; formal analysis, O.B., E.M. and V.Q.; investigation, O.B., and M.C.H.; resources, O.B., M.C.H., E.M. and Y.Z.; data curation, O.B. and Y.S.; writing—original draft preparation and writing—review and editing, O.B., E.M. and V.Q.; visualization, V.Q. and O.B.; supervision, O.B., M.C.H. and E.M.; project administration, O.B. and Y.Z.; funding acquisition, O.B. All authors have read and agreed to the published version of the manuscript.
Funding
This research received no external funding.
Acknowledgments
The authors thank the Universidad Católica del Norte and Compañia Minera Lomas Bayas for the opportunity and funding provided to develop this research. We also appreciate the contribution of the Scientific Equipment Unit-MAINI, Universidad Católica del Norte, for support in the preparation of samples, analysis and data generation.
Conflicts of Interest
The authors declare no conflict of interest.
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