Hydrometallurgical Recycling of Copper Anode Furnace Dust for a Complete Recovery of Metal Values

Abstract

Copper anode furnace dust is waste by-product of secondary copper production containing zinc, lead, copper, tin, iron and many other elements. Hydrometallurgical Copper Anode Furnace dust recycling method was studied theoretically by thermodynamic calculations and the proposed method was verified experimentally on a laboratory scale. The optimum condition for leaching of zinc from dust was identified to be an ambient leaching temperature, a liquid/solid ratio of 10 and H₂SO₄ concentration of 1 mol/L. A maximum of 98.85% of zinc was leached under the optimum experimental conditions. In the leaching step, 99.7% of lead in the form of insoluble PbSO₄ was separated from the other leached metals. Solution refining was done by combination of pH adjustment and zinc powder cementation. Tin was precipitated from solution by pH adjustment to 3. Iron was precipitated out of solution after pH adjustment to 4 with efficiency 98.54%. Copper was selectively cemented out of solution (99.96%) by zinc powder. Zinc was precipitated out of solution by addition of Na₂CO₃ with efficiency of 97.31%. ZnO as final product was obtained by calcination of zinc carbonates.

1. Introduction

Copper is the third most widely used metal and total global smelter production was approximately 24.5 million metric tons in the year 2020 [1,2,3]. Due to its wide use and unique properties, production is not expected to decrease in the future. High demand for copper increases the extraction of primary raw materials, which affects many environmental aspects [4]. The extraction of raw materials of this widely used metal can be reduced by introducing a circular economy, i.e., by recycling secondary raw materials containing copper and reintroducing them back into the economy. Copper recycling requires up to 85% less energy than primary production [5]. Around the world, it saves 100 million MWh of electrical energy and 40 million metric tons of CO₂ annually [6,7,8]. End of Life Recycling Input Rate for copper in the EU is currently only 17%, which create space for further recycling capacity increase [9]. The production of copper from secondary sources is different from the production from primary sources. The whole recycling process consists of several operations, the most important being:

• The reduction of Cu, Sn and Pb oxides and separation of these components from the rest of the batch, with most of the batch composed of Cu in metallic form;
• Zn separated into the off-gases and captured in the oxidized form in the filtration station;
• Transfer of unwanted components into slag;
• Converting of black copper and removal of Ni, Sn and Sb;
• Pyrometallurgical refining;
• Electrolytical refining [10];

Various chemical elements enter the process of recycling from secondary raw materials, which are later separated from copper in refining processing steps. This leads to the production of large amounts of waste with different chemical compositions. The most common waste are slags, which are the subject of many research papers, but in addition, dust (shown in Figure 1) is also generated.

The chemical composition of the dusts differs from the type of furnace in which they are produced. Dusts contain from 1.37 to 27% Cu, from 3.6 to 40.2% Zn, from 1.5 to 22.4% Pb and they can also contain smaller contents of elements such as Fe, Sn, Ca, As, Si and Ni [10,11,12,13,14,15,16,17,18,19,20,21,22,23,24]. The phase composition analysis of the dusts confirms the presence of oxides, chlorides, sulfates and sulfides of these elements.

The recycling of copper dust takes place both pyrometallurgically and hydrometallurgically. Common practice has been to recycle these dusts to the smelter to recover the copper content. The recycling of dust decreases furnace capacity, which reduces productivity. Hydrometallurgical processing consists of leaching of the dusts, refining of leach solutions and products’ recovery from leach solutions [25,26,27].

The leaching of the dust takes place in acidic (commonly in H₂SO₄ and HCl) and alkaline solutions (commonly in NaOH, but others, such as NH₄CO₃, are studied as well) [28]. The leaching efficiency in H₂SO₄ varies from 80 to 100% for copper and from 85 to 95% for zinc [14,17,18,21,22,29]. The leaching efficiency in HCl varies from 73 to 95% for copper and up to 95% for zinc [24,29,30]. In one case, a high zinc leaching efficiency in NaOH of 87% was achieved [11], but in other cases it was significantly less (4–11% Cu and 11–52% Zn) [18]. The comparison shows that the leaching efficiency depends on the chemical and phase composition of the dusts used, on the type of leaching medium, the temperature and the redox conditions during the leaching.

The operations followed by leaching are different and not all of the studied scientific articles also study conditions of the leach solutions refining and recovery of products from leach solutions. Li Qiang et al. studied the leaching of dusts in 5M NaOH and subsequent electrolysis with a current density of 100–250 A.m⁻², by which they obtained Pb and in the second step they increased the current density to 1500–1200 A.m⁻² to obtain Zn [11]. Another method consists of dust leaching in the mixture of (NH₄)₂CO₃-NH₄OH, leach solution refining by zinc powder cementation and from the pH adjustment to obtain Zn(NH₃)₂CO₃·ZnO at pH 7. The precipitate was further roasted at 400 °C to obtain 99% pure ZnO [12]. T. Mukongo et al. investigated the leaching of zinc-containing dusts in spent electroplating zinc electrolyte for further reuse in electroplating [13]. Laubertová et al. studied lead cementation from more environmentally friendly acetate dust leach solution. The proposed method achieved almost 90% lead removal efficiency [31].

Of the articles studied, only a small amount cover the recovery of products and an even smaller amount include the selective recovery of by-products. In this study, copper anode furnace (CAF) dust was analyzed, thermodynamic study was conducted to simulate leaching, solution refining and product recovery from the dust and small-scale lab batch-type experiments were conducted to verify the thermodynamic calculations.

2. Materials and Methods

2.1. Used Materials

Copper Anode Furnace (CAF) dust samples used for the following experiments are waste material from pyrometallurgical secondary production of copper (Figure 1) supplied by Slovakian copperworks. Samples were collected during a ten-day period from the smelting operations. The as-received samples were re-weighed and subjected to coning, quartering and dividing sample preparation methods to obtain representative samples [32,33].

2.2. Material Characterization

Particle size analysis was performed using the laser diffraction method on a Malvern Mastersizer 2000E (Malvern Instruments, UK, precision: ±1%) with a Scirocco2000M dry sample feeder. The density of each sample was determined using a Micromeritics AccuPyc II 1340 gas pycnometer (Micromeritics Instrument Corporation, USA, accuracy: ±0.02% of nominal cell volume).

The chemical composition of the input samples, intermediates, solid residues and leaching solutions was determined using classical wet analysis using atomic absorption spectrometry (AAS) on a Varian Spectrophotometer SpectrAA20+ (Varian, detection limit: 0.3–6 ppb).

The phases present in the dust, intermediates and recycled products were identified by X-ray diffraction phase analysis (XRD). The samples were prepared according to the standardized Panalytical backloading system, which provides nearly random distribution of the particles. The samples were analyzed using a Philips X’Pert PRO MRD (Co-Kα) diffractometer (Philips, Netherlands) and identified using X’Per HighScore plus software.

Samples were subjected to morphology observation by optical microscopy using a Dino-Lite ProAM413T digital microscope (AnMo Electronics Corporation, Taiwan). Each sample was subjected to scanning electron microscopy (SEM) analysis along with energy dispersive spectrometry (EDS). The morphology and microstructure of the samples were studied using a MIRA3 FE-SEM (TESCAN, USA, resolution: 1.2 nm at 30 kV; 2.3 nm at 3 kV) scanning electron microscope (REM). This equipment also enabled multi-elemental semi- quantitative analysis also using EDS.

2.3. Methodology

The leaching experiments were carried out in an 800 mL glass reactor placed in a thermostatically controlled water bath. The experiments were performed at temperatures of 20, 60 and 80 °C using constant 300 rpm stirring speed. The aqueous solution of sulfuric acid at concentrations of 0.5M and 1M was used as leaching reagents. The pH of the solutions was measured using pH-meter (Inolab, WTW 3710, Germany). The volume of the leaching reagent was 400 mL. Ten grams of dust samples obtained by manual quartering were used for the first set of experiments, which represents the liquid to solid ratio L:S = 40. Subsequently, experiments were performed with an adjusted L:S ratio, where 20, 40 and 80 g of dust samples were used while maintaining a constant volume (400 mL) of sulfuric acid. The total duration of the experiment was 60 min with sampling time after 5, 10, 15, 30 and 60 min. The volume of liquid sample for AAS analysis was 10 mL and leaching efficiency was calculated with respect of volume change caused by sampling and evaporation of solution at higher temperatures.

Two step solution refining process consisted of removal of Fe and Sn ions from the solution by precipitation and of zinc powder cementation. Precipitation of Fe and Sn was achieved by pH adjustment with the addition of 4M NaOH to pH of 4. Cementation experiments were performed with the use of 1.5 and 3 g of Zn powder per 400 mL of leachate, at two different temperatures (20 and 80 °C) with the sampling time after 5, 10, 15, 30 and 60 min.

Zinc precipitation was performed by conversion of soluble zinc sulfates to less soluble zinc carbonates by the addition of sodium carbonate and ammonium carbonate.

3. Results and Discussion

3.1. Material Characterization

Physical–chemical characterization included particle size distribution, chemical analysis and phase analysis.

The laser diffraction method of measuring the particle size distribution showed that the grain size in the sample ranges from 0.224 µm to 632.456 µm, with the largest proportion of particles ranging in size from 2 µm to 10 µm (Figure 2).

The content of mayor and trace elements in the CAF dust sample is show in

Table 1. Chemical composition of the copper anode furnace dust analyzed by AAS.

Element	Zn	Pb	Cu	Sn	Fe	Ca	As	Si	Ni	Cl-
Content (% w/w)	28.35	10.28	7.51	1.50	0.67	0.22	0.08	0.09	0.02	13.71

. The sample contains 28.35% Zn, 10.28% Pb and 7.51% Cu as mayor metal elements. It also contains 1.5% Sn, 0.67% Fe and 0.22% Ca. Si, As and Ni were also detected by AAS method, but their content was under 0.1% and therefore they are not further studied in followed experiments.

XRD analysis of the dust is shown in Figure 3. The analysis shows that majority of zinc is present as ZnO and Zn₂SnO₄, tin is present as SnO₂, SnCl₂ and Zn₂SnO₄ and lead is present as PbCl₂. The copper phase is not clearly determined from the peaks of the diffractogram despite its high content in the sample. Copper phases with highest match were Cu₂Cl(OH)₃ and Cu₄₆Cl₂₄(OH)₆₈^.4H₂O. Elements with content below 1% are under the detection limit of XRD method and therefore their phase composition is unknown.

SEM-EDX semiquantitative analysis (Figure 4) identified 15.5% content of O and 15.1% of Cl, which confirms presence of oxide phases and chloride phases in the sample.

3.2. Leaching

3.2.1. Thermodynamic Analysis

The first step of hydrometallurgical treatment was leaching. Thermodynamic analysis studied the leaching of individual CAF dust phases in H₂SO_{4 and} reactions are expressed by Equations (1)–(5).

ZnO_(s) + H₂SO_4(aq) = ZnSO_4(aq) + H₂O_(l)

(1)

SnO_2(s) + 2 H₂SO_4(aq) = Sn(SO₄)_2(aq) + 2 H₂O_(l)

(2)

SnCl_4(s) + 2 H₂SO_4(aq) = Sn(SO₄)_2(aq) + 4 HCl_(aq)

(3)

PbCl_2(s) + H₂SO_4(aq) = PbSO_4(s) + 2 HCl_(aq)

(4)

CuCl_2(s) + H₂SO_4(aq) = CuSO_4(aq) + 2HCl_(aq)

(5)

Table 2. ΔG° values of CAF dust leaching in the H₂SO₄ system.

Temp. (°C)	∆G° (kJ)
	(1)	(2)	(3)	(4)	(5)	(6)	(7)
0	−118.33	−62.92	−199.69	−66.99	−23.95	−24	44.17
20	−111.86	−50.26	−182.74	−64.26	−22.08	−24.35	47.08
40	−105.08	−37.35	−165.18	−61.32	−20.3	−24.9	49.75
60	−97.98	−24.2	−147.02	−58.18	−18.61	−25.64	52.2
80	−90.58	−10.81	−128.28	−54.84	−17.03	−26.57	54.43
100	−82.86	2.81	−108.99	−51.32	−23.95	−27.66	56.45

shows negative values of the standard Gibbs energies change (ΔG°), which indicate that these reactions (Equations (1)–(5)) take place in the direction of product formation and should be spontaneous at temperatures from 0 to 100 °C. In Equation (4), a non-soluble compound PbSO₄ (K_{SP PbSO4} = 1.6 × 10⁻⁶) is formed, which indicates that the separation of the lead from other well-soluble elements should be possible by leaching and filtration. Products of tin, copper and lead chloride leaching in sulfuric acid (Equations (3)–(5)) are sulphates of these elements and hydrochloric acid. Hydrochloric acid further reacts with the zinc oxide present in the dust (Equation (6)) but does not react with tin dioxide (Equation (7)) according to ΔG° values shown in Table 2.

ZnO_(s) + 2HCl_(aq) = ZnCl_2(aq) + H₂O_(l)

(6)

SnO_2(s) + 4HCl_(aq) = SnCl_4(aq) + 2H₂O_(l)

(7)

3.2.2. Effect of Temperature on the Leaching Efficiency

The zinc leaching and the effect of temperature on leaching efficiency was studied experimentally. Ten grams of CAF dust were leached in 400 mL of 0.5M (Figure 5a) and 1M (Figure 5b) solution of H₂SO₄ at 20, 60 and 80 °C. Zinc phases present in the dust were leached to the solution according to the thermodynamic study at relative high speed. The increase in leaching efficiency and its effect of temperature were observed in 0.5M solution (Figure 5c), where the efficiency increased from 89% at 20 °C to 97% at 80 °C. By leaching in 1M, a high leaching efficiency (99.18%) could be achieved at an ambient temperature. According to the thermodynamic study, Cu, Fe and Sn were also leached, while Pb was not, which corresponds to the chemical composition of the solution after leaching shown in

Table 3. Concentration of elements in solution after leaching in 1 M H₂SO₄ at 80 °C.

1 M H2SO4, 80 °C, L/S = 40	Zn	Cu	Sn	Fe	Pb
Concentration (mg/L)	8620	2089	407	168	6.91

. The leaching residue was filtered and analyzed by SEM-EDX (Figure 6) and XRD (Figure 7), both of which confirmed the presence of a PbSO₄ phase.

3.2.3. Effect of Liquid–Solid Ratio on the Leaching Efficiency

Previous leaching experiments have confirmed the high leaching efficiencies of zinc at the liquid–solid ratio of 40 and only a slight effect of acid concentration and temperature increase. In the following experiments, the L/S ratio is reduced to increase the zinc concentration in the solution. Figure 8 shows zinc leaching efficiency in 0.5 M H₂SO₄ (Figure 8a) and 1M H₂SO₄ (Figure 8b) at 20 °C and L/S ratio 40, 20, 10 and 5. The results confirmed that zinc leaching efficiency did not decrease significantly at L/S interval from 40 to 10. Further decrease in the L/S ratio to 5 led to a slight leaching efficiency decrease when 1 M H₂SO₄ solution was used and a significant leaching efficiency decrease to 60% occurs when 0.5M H₂SO₄ was used.

The conditions under which both a high concentration of zinc in the solution and high zinc leaching efficiency were achieved was determined as the L/S ratio of 10 in 1 M H₂SO₄ at ambient temperature. The chemical composition of the obtained solution ready for next steps of refining and Zn precipitation is shown in

Table 4. Concentration of elements in solution after leaching in 1M H₂SO₄ at 20 °C and L/S ratio 10.

Analyte	Zn	Cu	Pb	Sn	Fe
Concentration (mg/L)	33,000	10,712	31.98	1221	585.2
Leaching efficiency (%)	98.85%	94.86%	0.30%	79.37%	78.16%

.

3.3. Solution Refining

The refining of the leachate obtained by CAF dust leaching (Table 4) was firstly studied theoretically and results were subsequently verified experimentally. The aim of solution refining was to remove impurities, such as copper, tin, iron and lead, which affects a purity of products obtained in the subsequent zinc precipitation step. A combination of precipitation and cementation has been proposed as suitable refining methods for this specific solution.

3.3.1. Adjustment of pH and Precipitation

Precipitation can be defined as a process where metal ions react with other compounds to form a low solubility product. Metal hydroxide precipitation is the most common example of this process [34,35]. Figure 9 shows fraction diagrams for zinc, tin, iron and copper respectively. The concentrations of the individual elements were calculated from previous leach solution obtained by leaching at L/S ratio of 10. The measured pH of the solution for refining is 0.33.

The fraction diagram for zinc (Figure 9a) shows presence of Zn²⁺ ions, Zn(SO₄)₂⁻² complex and as a well-soluble ZnSO₄ at pH range from 0.33 to 6.5. Further increase of pH to values above 6.5 leads to precipitation of Zn₄(OH)₆SO₄ and therefore solution refining is possible only at this pH range. According to following diagram (Figure 9b), copper ions start to precipitate out at pH 4 as Cu₃SO₄(OH)₄. The tin precipitates from solution depending on the oxidation number from pH 0 to 1 for Sn⁴⁺ ions (Figure 9c) and from 2.5 to 4 for Sn²⁺ ions (Figure 9d). Phase analysis and leaching thermodynamics predict the presence of Sn⁴⁺ ions, but they can act as oxidizing reagents and be reduced to Sn²⁺. Iron ion precipitation depends on the oxidation state as well. Fe³⁺ precipitate out from solution at pH range from 2.2 to 3.2 (Figure 9e), but Fe²⁺ ions cannot be removed by precipitation before zinc, because pH range of precipitation is from 7.8 to 9 (Figure 9f). Therefore, the combination of precipitation and cementation must be used for recovery of high purity zinc products.

Solution of 4M NaOH was added slowly to 200 mL of leachate, while pH was continuously measured. The addition of NaOH caused dilution of leachate and therefore the impurity removal efficiency was calculated based on from Equation (8):

$$Inpurityremovalefficiency=1-\left(\frac{V_1·c_1}{V_0·c_0}\right)$$

(8)

where V₀ and V₁ are volumes before and after pH adjustment and c₀ and c₁ are concentrations of individual elements before and after pH adjustment. The pH was adjusted in two steps to pH 3 and 4, between which the solution was filtered and the solid residues and solutions obtained were analyzed. Solutions and filtered solid residues from pH adjustment are shown in Figure 10 and results from AAS analysis are shown in

Table 5. Chemical analysis of solution before and after refining by pH adjustments.

Solution Description	Analyte	Zn	Cu	Pb	Sn	Fe
pH 0.33 200 mL	Concentration (mg/L)	33,000	10,712	31.98	1221	585.2
	Absolute amount (g)	6.6	2.142	0.006	0.244	0.118
pH 3 415 mL	Concentration (mg/L)	15,860	5 162	14.76	<LOD	237.5
	Absolute Me amount (g)	6.582	2.142	0.006	0	0.099
	Me precipitation efficiency (%)	0.274%	0.008%	4.231%	100%	15.787%
pH 4 425 mL	Concentration (mg/L)	15,478	5,038	10.51	<LOD	4.03
	Absolute Me amount (g)	6.578	2.141	0.004	0	0.002
	Me precipitation efficiency (%)	0.331%	0.058%	30.163%	100%	98.537%

. Tin concentration was under the level of detection (LOD) already at pH 3, indicating that the tin was quantitatively removed from the solution according to the theory of fraction diagrams (Figure 9). In addition to tin, 15.79% of iron was precipitated at this pH too and remaining 82.75% of iron was precipitated out of the solution after a pH increase from 3 to 4 with a total 98.54% precipitation efficiency. Zinc losses were 0.27% at pH 3 and 0.33% at pH 4, which confirm good selectivity of the refining step.

3.3.2. Cementation

Cementation, an electrochemical deposition of noble metal ions by a less noble metal as an electron donor, is usually applied to remove/recover metal ions from dilute aqueous solutions [36,37,38,39]. In addition to zinc and copper, a small amount of other impurities were present in the solution after previous refining steps.

Table 6. Oxidation-reduction potentials of elements present in the CAF dust.

Mex+	⇌	Me(s)	E°
Zn2+ + 2 e−	$\overleftarrow{Oxidation}$	Zn(s)	−0.7618
Fe2+ + 2 e−	$\overrightarrow{Reduction}$	Fe(s)	−0.44
Ni2+ + 2 e−	$\overrightarrow{Reduction}$	Ni(s)	−0.25
Sn2+ + 2 e−	$\overrightarrow{Reduction}$	Sn(s)	−0.13
Pb2+ + 2 e−	$\overrightarrow{Reduction}$	Pb(s)	−0.126
Cu2+ + 2 e−	$\overrightarrow{Reduction}$	Cu(s)	0.34

shows redox potentials (E°) of elements present in the CAF dust. Specific E° values confirm the possibility to replace Fe²⁺, Ni²⁺, Sn²⁺, Pb²⁺ and Cu²⁺ ions from solutions with metallic zinc according to Equation (9).

mN⁰ + nM^m+ → mNⁿ⁺ + nM⁰

(9)

where N represent zinc and M are dissolved ions.

In the preliminary cementation experiment, 400 mL of the refined solution with pH 4 was cemented by 6 g of zinc powder at temperature of 20 and 80 °C for the duration of 60 min. The copper concentration change over time is showed in Figure 11.

The results confirmed the effect of temperature on the rate of cementation in the first minutes of experiment, but the efficiency of cementation was the same for both temperature after 30 min. Copper concentration decreased from 5038 to 2.22 mg/L (99.96%) at 20 °C, while zinc concentration was increased from 15,478 to 21,021 mg/L. The copper deposited on the surface of zinc powder (Figure 12b) and transparent solution (Figure 12c) was clearly visible after experiments. Followed method further reduced lead concentration in the solution according to study of Laubertová et al. [31]. Concentration of elements in input and output solution after cementation step is shown in

Table 7. Chemical analysis of solution before and after cementation.

Solution Description	Analyte	Zn	Cu	Pb	Sn	Fe
Leachate after pH adjustment	Concentration (mg/mL)	15,478	5038	10.51	<LOD	4.03
	Absolute amount (g)	6.578	2.141	0.004	0	0.002
Leachate after cementation at 20 °C	Concentration (mg/mL)	21,021	2.22	0.65	<LOD	2.01
	Absolute amount (g)	8.4084	0.000888	0.00026	0	0.000804
Cementation efficiency (%)		-	99.96%	93.50%	-	59.80%

.

3.4. Zinc Recovery

The recovery of zinc from the zinc sulfate solution is the last step in the CAF dust treatment. Zinc can be recovered in several ways, including crystallization, electrolysis, hydrolysis and precipitation. According to fraction diagram (Figure 9a) it is possible to obtain zinc in the form of Zn₄(OH)₆SO_4(s) by further addition of hydroxide, but presence of sulfur can reduce a purity of obtained products and therefore, zinc carbonate precipitation followed by calcination is studied in this article.

3.4.1. Zinc Carbonate Precipitation

Theoretical study of precipitation consists of thermodynamic calculations and constructions of fraction diagrams. Zinc carbonate is insoluble substance with K_sp = 1.4 × 10⁻¹¹. Precipitation reagent should be soluble and therefore Na₂CO₃ (solubility = 21.5 g/100 mL) and (NH₄)₂CO₃ (solubility = 25 g/100 mL) are considered as suitable for this purpose. Figure 13 shows fraction diagrams for precipitation with sodium carbonate and Equations (10)–(12) shows reactions of precipitation reagent with zinc sulfate. Thermodynamic values confirm negative ∆G° values (

Table 8. ΔG° values of CAF dust precipitation by Na₂CO₃ at temperatures from 0 to 100 °C.

Temperature (°C)	∆G° (kJ)
	(10)	(11)	(12)
0	−85.067	−60.782	−392.710
20	−84.738	−63.351	−458.227
40	−84.387	−65.837	−527.329
60	−84.015	−68.245	−590.405
80	−83.627	−70.579	−648.151
100	−83.225	−72.843	−691.628

) indicating the formation of ZnCO₃, ZnOH or Zn₅(OH)₆(CO₃)₂.

ZnSO_4(aq) + Na₂CO_3(s) = ZnCO_3(s) + Na₂SO_4(aq)

(10)

ZnSO_4(aq) + Na₂CO_3(s) + H₂O_(l) = Zn(OH)_2(s) + Na₂SO_4(aq) + CO2_(g)

(11)

5 ZnSO_4(aq) + 5 Na₂CO_3(s) + 3 H₂O_(l) = Zn₅(OH)₆(CO₃)_2(s) + 5 Na₂SO_4(aq) + 3 CO_2(g)

(12)

According to the fraction diagram, pH 7 should be sufficient for the removal of the zinc from the solution. Solid Na₂CO₃ was slowly added to stirred 25 mL of refined solution and pH value was measured continuously. Two grams were added until pH 6.9 was reached, but only 81.5% zinc precipitation efficiency was achieved. The main reason for lower zinc precipitation is the complexation of zinc [35]. With increased ionic strength of the solution (Figure 14), the fraction of soluble Zn(SO₄)₄⁶⁻ complexes increases (green arrow) causing lower Zn recovery (red arrow). Further addition Na₂CO₃ to total 3 g per 25 mL resulted in pH increase to 9 and zinc precipitation efficiency 97.31%. Only 566 mg/L were in the solution. The chemical composition of solution before and after precipitation steps is showed in

Table 9. Chemical analysis of solution before and after precipitation.

Solution Description	Analyte	Zn	Cu	Pb	Sn	Fe
Leachate after cementation at 20 °C	Concentration (mg/L)	21 021	2.22	0.65	0	2.01
	Absolute amount (g)	0.526	5.5 × 10−5	1.63 × 10−5	0	5.03 × 10−5
Leachate after precipitation Na2CO3	Concentration (mg/L)	566	2.45	0.65	0	1.98
	Absolute amount (g)	0.014	6.1 × 10−5	1.63 × 10−5	0	4.95 × 10−5
Precipitation efficiency (%)		97.31%	-	-	-	-

.

Solid residue was dried and solid residue from a parallel trial was washed with distilled water and dried. Figure 15 and Figure 16 shows XRD analysis of these products. Zinc is present as Na₂Zn₃(CO₃)₄(H₂O)₃ phase in non-washed precipitated residue and further washing results in a Zn₃CO₃(OH)₆·H₂O phase.

3.4.2. Zinc Carbonate Calcination

Calcination of scrubbed zinc precipitates was carried on to obtain marketable product in form of ZnO according to Equation (13). The temperature of 900 °C was chosen to verify the possibility of calcination of the precipitated zinc phases. Figure 17 shows XRD pattern of that material, which confirm presence of ZnO.

ZnCO_3(s) = ZnO_(s) + CO_2(g)

(13)

3.5. Process Flow Sheet

Based on the results obtained in previous stages, an integral multi-step hydrometallurgical processing route for recovery of Zn, Pb, Cu and Sn was developed. The overall process of CAF dust treatment with the achieved concentrations in the solution is shown in Figure 18.

4. Conclusions

Copper anode furnace dust used in this study is by-product of the pyrometallurgical production of copper from secondary sources. The majority of the scientific articles are focused on leaching conditions, but further product recovery is not completely studied yet. Copper anode furnace dust consists of both oxides and chlorides of zinc (28.35%), lead (10.28%), copper (7.51%), tin (2.5%), iron (0.69%) and other elements with content below 0.5%, which were not studied is this paper. The theoretical recycling procedure was designed on the basis of theoretical calculations. The proposed process consists of dust leaching in sulfuric acid, pH adjustment, zinc cementation, precipitation and calcination of the zinc containing products. The proposed procedure was verified by an experimental study and the results were compared with the theoretically simulated process. The experimental study shows:

• Dust phases present in the sample reacts with H₂SO₄ and forms sulphates of these elements;
• Sulphates of present elements are well soluble except for the lead, which forms insoluble PbSO₄;
• Lead sulphate is selectively removed from the zinc, copper, tin, iron and others dissolved elements by filtration;
• Optimum conditions for zinc leaching were determined as liquid to solid ratio of 10, ambient leaching temperature, leaching time of 1 h and 1M H₂SO₄;
• Zinc leaching efficiency of 98.85% was achieved at these conditions;
• Refining of the leach solution consisted of adjusting the pH to value 3, to value 4 and by cementation;
• pH increase to 3 resulted in quantitative precipitation of the tin from the solution with 15.79% co-precipitation of iron;
• Further pH increase to 4 led to precipitation of iron remaining 82.75% of iron;
• No copper or zinc were precipitated during followed pH adjustments;
• Zinc powder cementation was used in order to remove the copper from the solution;
• Copper concentration decreased from 5038 to 2.22 mg/L which represent 99.96% removal efficiency of cementation, while zinc concentration was increased from 15,478 to 21,021 mg/L;
• The increased cementation temperature has no positive effect on the efficiency after 30 min of the experiment;
• Zinc was then precipitated from refined solution by the addition of Na₂CO₃, which caused further pH increase;
• Theoretical increase to pH of 6 was not sufficient for quantitative recovery of the zinc from solution due to zinc complexation and therefore the addition of Na₂CO₃ was increased to 3 g per 50 mL until pH 9 was reached;
• The concentration of zinc in solution decreased from 21,021 mg/L to 566 mg/L, which represents 97.31% precipitation efficiency;
• The solid residue scrubbing removes sodium and calcination at 900 °C decompose ZnCO₃ into ZnO and CO₂;
• A total of 96.16% of the zinc in the form of ZnO was recovered from the CAF dust waste by proposed method.

In further research, the optimal conditions of solution refining and conditions of zinc recovery from solution will be studied in order to reduce zinc powder usage in cementation step and in order to achieve the highest possible efficiency and selectivity of each individual operation.