Introduction

With the increasing demand for aluminum (Al), current estimates suggest that the annual generation of bauxite residue is in excess of 150 million metric tons worldwide [1]. Prior to 1980, most of the inventory was stored in lagoon-type impoundments but, as available land became scarce, many plants have adopted dry-stacking methods instead. The residue is strongly alkaline and contains calcium- and sodium-aluminosilicates together with iron-, titanium- and other undissolved minerals from the Bayer process. It also typically contains 13–25% of residual alumina (Al2O3), depending on the grade of the initial bauxite ore and the efficiency of alumina extraction [2]. The large quantities of stockpiled residue constitute considerable losses in what is otherwise exploitable raw material resources and are inherently accompanied by substantial environmental challenges [3]. Adapting to circular principles will therefore be essential to ensure access to future materials. Stricter regulations like the European Mining Directive [4] and the European Waste Legislation [5] put increasing constraints on landfills, and forces the industry to find alternative and more sustainable solutions for their waste streams. Despite the development of numerous processes for recovery of components, industrial utilization of bauxite residue remains below 2.5% [1].

The Pedersen process was developed as an alternate route of refining Al2O3 and was employed at the Høyanger plant in Norway between 1928 and 1968 [6]. The process could, however, not compete with refinement of high-quality ores by the Bayer process and did not gain widespread adaptation. But as high-quality deposits are being depleted and problems related to storage of bauxite residue have escalated over the years, renewed interest has been given to the technology [7, 8]. The process was primarily developed with low-quality bauxite and other laterite ores in mind, with higher contents of iron- and silicon bearing oxides that is traditionally seen as uneconomical for the Bayer process. Extraction of iron and aluminum by carbothermic smelting and subsequent slag leaching in a sodium carbonate solution (Na2CO3) leaves a residue that consists primarily of calcium-carbonate and -silicates, which may be recycled by the agriculture and/or construction sectors. Similar concepts can also be adapted to treatment of already stockpiled bauxite residue [2]. Works by Azof et al. [9, 10] on synthetic binary calcium aluminate slags found that mayenite (C12A; Ca12Al14O33(s)) displays exceptional leaching properties, while tricalcium aluminate (C3A; Ca3Al2O6(s)) and monocalcium aluminate (CA; CaAl2O4(s)) display more moderate leaching properties. The high leachability of the C12A phase is primarily attributed to its clathrate structure, where oxygen anions located in the center of the cage allow for easy depolymerization. The phase has been well known in concrete research for a long time and is recognized for being thermodynamically unstable without access to secondary stabilizing template anions. It reacts readily with water and is known to retain enough hydroxyl ions to stabilize the phase up to high temperatures [11, 12]. On the other hand, it is known to decompose under dry and/or reducing conditions if no other stabilizing compounds are present [13]. Mechanisms and stability are still heavily debated, but recent works suggests that carbon may play an important role in stabilizing the C12A7 in reducing conditions [14, 15]. On the other hand, monocalcium dialuminate (CA2; CaAl4O4(s)) appear to be insoluble in a Na2CO3 solution. It was argued that the leaching is surface driven, and the reduced leachability was related to the build-up of an insoluble layer of calcite on the calcium aluminates that effectively inhibits the dissolution of Al2O3 [16]. Moreover, a less leachable calcium aluminate phase may also affect the leachability of others. Al can also be immobilized in gehlenite (C2AS; Ca2Al2SiO7) and the content of silica in the bauxite residue poses a great challenge for Al recovery [17]. The addition of CaO can be used for capture of SiO2 in a calcium silicate (C2S; Ca2SiO4) phase and may have a positive effect on the Al recovery [18, 19]. The high-temperature hexagonal α-polymorph of C2S is known to go through several transformations upon cooling [20], and the monoclinic β-C2S to the orthorhombic γ-C2S transformation is associated with an especially large volume expansion of 12% that is manifested as a disintegrating slag [21]. This work seeks to valorize bauxite residue farmed from Mytilineos, Aluminum of Greece, though carbothermic production of pig-iron and leachable calcium aluminate slags. Various amounts of CaO are added to the smelting experiments to investigate final slag mineralogy and properties for subsequent leaching tests. Slow cooling practices are employed to ensure slag phases with high aluminum leachability and to facilitate the transformation of calcium silicate via the β-C2S phase. The goal is to produce a self-disintegrating slag that reduces the need for crushing the slag before leaching.

Materials and Methods

Thermochemical Calculations

Thermodynamic calculations were carried out using FactSage 7.3 thermochemical software to design experiments and predict slag compositions at equilibrium [22]. The calculations were based on a simplified bauxite residue composition, marked with a in Table 1. Carbon and CaO was added to the calculations as pure components and the system temperature was set to respective smelting temperatures of the samples. Descriptions of oxide solutions, including liquid slag (SLAG) and monoxide (MeO) were taken from the FactSage FToxide database. The FSstel database was used to calculate the liquid metal (Liqu) solution, and thermodynamic properties of pure substances and gas species were taken from the FactPS database. Due to the lack of the pure mayenite specie in the databases, a custom database was created with thermodynamic data from Hallstedt [23].

Table 1 The chemical composition of the bauxite residue, charcoal and lime used in the current experiments, as measured by XRF
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Pre-treatment and Smelting

The bauxite residue held approximately 25 wt% moisture and dried at 130 °C for 12 h prior to smelting in an alumina crucible (Fig. 1a). Charcoal was dried under similar conditions and sized to a fraction of 4.75–16 mm. The chemical composition of the dried residue is summarized along with the remaining raw materials in Table 1. Prior to smelting, 1000 g of dried bauxite residue was mixed with 200 g charcoal and 150—350 g of CaO in graphite crucibles. The crucibles were placed in a 75 kW induction furnace (Fig. 1b), heated to temperatures of 1550–1750 °C and held for 90 min. An overview of the different samples, CaO-additions and smelting temperatures are shown in Table 2. Cooling proceeded by 10 °C/min down to 1330 °C, and the furnace was held at this temperature for another 30 min before it was shut down. The samples were left inside the furnace to be cooled down to room temperature overnight. Disintegrated slags were separated from the metal and sieved to below 125 µm with little effort. Solid slags were manually separated from the metal by hand, crushed and sieved to below 125 µm. Samples were also cut from the metals and cast into epoxy for elemental characterization.

Fig. 1
figure 1

a Bauxite residue after being dried at 130 °C for 12 h. b The 75 kW induction furnace with the graphite crucibles used in this work. c The XRD-diffractogram of dried bauxite residue contains signals for hematite (Fe2O3), boehmite (γ-AlO(OH)), diaspore (α-AlO(OH)), gibbsite (γ-Al(OH)3), katoite (Ca3Al2(SiO4)(OH)8), calcite (Ca(CO3)), cancrinite (Na6.6Ca0.9Si6.5Al5.5O24(CO3)1.44⋅2H2O), sodium aluminum silicate (Na1.15Al1.15Si0.85O4) and anatase (TiO2)

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Table 2 Samples are numbered according to melting temperature and lime addition
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Leaching

Parameters similar to those used in a previous study by Azof et al. were used [10]. Approximately 2.5 ± 0.01 g of slag was prepared for each experiment. A solution of 102.6 g/l Na2CO3(s) was heated to a temperature of 45 °C. The leaching was performed with a 20 ml/g liquid-to-solid ratio in an open beaker, heated by a hot plate under a magnetic stirring speed of 300 rpm, at residence time of 60 min. The final leachate and residue were filtered through an ashless grade filter paper, and the pregnant liquid solution (PLS) was stored in a vial while the residue was dried at 100 °C overnight.

Characterization

Phase and compositional analysis of the bauxite residue and the produced slags were done by a Bruker D8 A25 DaVinci X-ray Diffractometer (XRD) with Cu-Kα radiation and a Philips PW 2404 X-ray Fluorescence spectrometer (XRF). Identification of obtained XRD peaks and a semi-quantitative analysis of slags before and after leaching was done in the DIFFRAC.EVA v.5.1 software. Despite the inherent limitations in the semi-quantitative analysis method it is primarily used to get an impression of the distribution of Al and silicon (Si) in the slags before and after leaching. Microscopic analysis of particles and phases were carried out by a JEOL JXA-8500F Electron Probe Microanalyzer (EPMA) and a Zeiss Ultra 55 FE-SEM. The elemental composition of the pig-iron samples was measured by the same EPMA instrument, where the reported values are averaged over three individual measurement points on each sample. A Thermo Scientific Element 2 high-resolution Inductively Coupled Plasma Mass Spectrometer (ICP-MS) instrument was also used to analyze extracted elements in the pregnant solution (PLS) after leaching.

Results

Characteristics of the Bauxite Residue

In addition to the chemical composition previously given in Table 1, mineralogical phase analysis done by XRD is presented in in Fig. 1c. The peaks of the XRD diffractogram have been identified to being related primarily to boehmite, diaspore, gibbsite, calcite, katoite, anatase, sodium aluminum silicate, hematite and cancrinite.

Thermochemical Calculations

The liquid slags are calculated to consist primarily of Al2O3, CaO, SiO2 and TiO2. Note that the FToxid database contains limited data concerning liquid slags in the presence of TiO2 and care must be taken. The total amount of TiO2 in the liquid slag is calculated to below 5wt% and the slags are extrapolated onto the Al2O3–CaO–SiO2 ternary phase diagram in Fig. 2a. The distribution of Ti at smelting temperatures in (b) does, however, suggest that the Ti-rich perovskite phase is not completely molten at 1550 °C. Subsequent Scheil-Gulliver cooling calculations on the liquid slags results in the phase distributions summarized in Fig. 2c. Commonly formed phases are C12A, C3A α-C2S and CaTi. The latter is a collective term for various calcium titanates formed, including CaTi(ss) (a Ca3Ti2O7(s)—Ca3Ti2O6(s) solid solution), Ca3Ti2O7(ss) and perovskite(ss) (Ca2Ti2O6(s)—Ca2Ti2O5(s) solid solution). Samples at low CaO-additions also form a melilite solution, which contains C2AS as an endmember, while samples at high CaO-additions also form CA.

Fig. 2
figure 2

a Calculated liquid slag compositions extrapolated onto the Al2O3–CaO–SiO2 ternary phase-diagram. b Distribution of Ti between liquid metal (Liquid), liquid slag (Slag), carbides (FCC), perovskite (Pero) and calcium titanate (CaTi) at melting temperatures. c Calculated phase distribution of samples after performing Scheil–Gulliver cooling calculations on the previously calculated liquid slags

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Smelting

Smelting produced pig-iron and slags and intact samples appear as in Fig. 3a. The graphite crucible cracked for several experiments (b) and repeating some of these samples resulted in similar outcomes. An overview of cracked samples is listed in Table 3, and the entries refer to Fig. 3c–f for the observed colors of the slags. The crucible for sample 3.1 did not crack but comprised of a combination of solid and powdered slag, and the sample is therefore noted as semi-intact. For cracked and semi-intact samples, the pig-iron slab was easily separable from the powdered slag, whereas the latter was sieved to below 125 µm with little effort.

Fig. 3
figure 3

a Intact samples consist of pig-iron on the bottom and slag on top. b Samples 1.1, 1.2 and 2.2 cracked during cooling and are already pulverized after solidification. Cracked slags display a white base color c with or d without a green tint. Intact slags from samples at 1550/1650 °C display a e grey color, while slags from samples at 1750 °C display f a dark green color

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Table 3 Overview over which samples resulted in intact or cracked crucibles. The color of the respective slags are marked and refers to Fig. 3c–f
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Pig-Iron Characteristics

With a concentration over 95%, Fe is found to be the primary component of all samples (Table 4). The concentration of Si remains low for all samples at 1550 °C and 1650 °C, but increases to 2.5–3.5% at 1750 °C. Small levels of dissolved chromium (Cr) and nickel (Ni) are also found. While not found to dissolve significantly in the metal, Ti is frequently found as precipitated titanium carbide (TiC) particles along graphite flakes, which are found in abundance throughout the metal phase (Fig. 4).

Table 4 Summary of the chemical composition of the pig-iron for all samples, as measured by EPMA
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Fig. 4
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Micrograph revealing the large number of graphite flakes and TiC-particles commonly found in all metal samples

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Slag Characteristics and Leaching

The chemical composition of the various slags prior to and after leaching is summarized in Tables 5 and 6, respectively. Both fractions of sample 3.1 (powder and solid) display similar chemical compositions and are represented by the same column. The slags are, as predicted, generally found to be rich in CaO and Al2O3, with lesser concentrations of SiO2, TiO2 and, in some cases, metallic Fe. Elevated Fe concentrations are primarily found in slags from intact samples (Table 3) that was crushed before further treatment and/or characterization.

Table 5 The chemical composition of the slags prior to leaching in wt%, as measured by XRF
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Table 6 The chemical composition of the slags after leaching, as measured by XRF in weight percent (wt%)
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From this point, the slags are divided into three groups based on similarities found in their respective XRD-diffractograms presented in Fig. 5. Note that the figure includes diffractograms of residual slag both prior to and after leaching. Samples 1.3 and 2.3 are grouped together in Group I, which display particularly strong signals for C3A together with signals for C12A, larnite (β-C2S) and CaTiO3 prior to leaching. Similar phases are also seen after leaching, i.e. C3A, C12A, β-C2S and CaTiO3, in addition to calcite and vaterite; both being polymorphs of CaCO3. Samples 1.1 and 2.1 are grouped together in Group II, displaying a particularly strong signal for C2AS together with signals for C12A, calcio-olivine (γ-C2S), β-C2S and CaTiO3 prior to leaching. These samples also display similar phases after as before leaching, i.e. C2AS, γ-C2S, β-C2S and CaTiO3, in addition to both polymorphs of CaCO3. However, the C12A signal has disappeared for both samples. Finally, samples 1.2, 2.2, 3.1 and 3.2 are grouped together in Group III, which generally display a particularly strong signal for C12A together with signals for γ-C2S, β-C2S and CaTiO3 prior to leaching. Sample 3.2 deviates from this trend by displaying an additional signal for C3A, and for sample 3.1 in that it lacks the signal for CaTiO3. After leaching, the samples in Group III display a strong calcite signal together with γ-C2S, β-C2S, CaTiO3 and vaterite. Sample 3.1 still deviates from this trend by lacking the signal for CaTiO3, and sample 3.2 for still displaying a C3A signal. The C12A signal is also much less pronounced than prior to leaching.

Fig. 5
figure 5

XRD diffractograms of slags before and after leaching. The slags are grouped together into three groups based on similar diffractograms

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The recovery of Al and Si to the PLS is summarized for all slags in Fig. 6, and, with values of 5–22%, Group I samples display the lowest recoveries. Equally low recoveries of 14–25% can also be observed for Group II samples, while the recoveries are generally found to be larger for Group III samples than for the other groups. Sample 1.2 displays the lowest value of Group III samples, while sample 3.2 displays an average value of 40%, and sample 2.2 and 3.1 display the highest recoveries of 50–60%. The concentration of Si in the PLS remains low for all samples. The distribution of Al has been calculated by correlating semi-quantitative XRD phase identification with measured XRF- and ICP-MS data in Fig. 7. However, due to the inherent limitations of this method, these results are considered to be semi-quantitative. Al is primarily found as C3A (72–87%) and a lesser fraction of C12A (12–28%) in Group I, primarily C2AS (66–78%) and a lesser fraction of C12A (22–33%) in Group II, and primarily in the form of C12A (100%) in Group III. Sample 3.2 deviates from the general trend of Group III by distributing aluminum between C12A (70%) and a lesser C3A fraction (30%).

Fig. 6
figure 6

The recovery of Al and Si has been calculated by correlating the concentrations measured in the PLS by ICP-MS with that measured in the slags both prior to (A; Table 5) and after (B; Table 6) leaching. The concentration of Al and Si in the PLS is included on a secondary y-axis

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Fig. 7
figure 7

Semi-quantitative (XRD) distribution of aluminum in each sample before and after leaching. The data has been correlated with XRF measurements and normalized to the amount of aluminum input before leaching. The difference between the two bars in each pair corresponds to the amount of recovered aluminum measured by ICP-MS (Fig. 6)

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Residual slag particles after leaching have been investigated by EPMA for samples 1.2, 2.2 and 3.1, and backscatter micrographs of particles are shown in Fig. 8a and b. Supplementary elemental maps are shown in (iii) and chemical compositions of marked phases (A-D) in Table 7. Particles marked with A holds a composition that resembles that of C2S. Remaining C12A particles, e.g. as B in (i), are often found to be surrounded by a darker peripheral layer of CaCO3 after leaching (C). Individual particles consisting of CaO, TiO2 and Al2O3 (D), which is believed to be Al-rich CaTiO3, can also be frequently found in the samples. The degree of overlap of the Ti-signal with the Al-signal in the EPMA maps in (iii) suggests that there is a significant incorporation of Al in the CaTiO3 structure.

Fig. 8
figure 8

Micrograph and EPMA maps of oxygen, aluminum, silicon, calcium and titanium for sample 2.2 after leaching. Marked particles are quantified in more detailed in Table 7

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Table 7 Averaged EPMA point measurements of phases in samples 1.2, 2.2 and 3.1 after leaching in wt%
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Discussion

Pig-Iron Characteristics

Most of the iron oxide present in the bauxite residue has been reduced to pig-iron in the bottom of the crucibles (Fig. 3a), which may have a wide range of use, including wrought iron, steels, cast irons and other ferroalloys. Restrictions in minor elements will, however, limit the usability of the iron phase, as they affect the mechanical properties of the metal in various ways. The abundance of graphite flakes found in Fig. 4 is a result of high carbon saturation. Cr, Ni and Si found in the pig-iron (Table 4) are all well-known alloying elements in steel- and ironmaking [24, 25]. Incorporation of silicon in the metal phase does, however, require high temperatures, and significant recovery of Si to the pig-iron phase is only observed in samples produced at 1750 °C (Table 4). Si units are sought after and optimizing the process for higher recoveries will be relevant. However, higher temperatures and silicon content will also lead to increased Ti-recovery, and even though low levels of Ti has found uses in steel- and ironmaking [25] it is generally not added intentionally. One should therefore find ways to limit its presence in the pig-iron phase. Although the alloyed elements may have their individual uses, the fact that they are present together may not be as propitious, and one may have to find solutions for limiting their presence in order to develop products that may be able to accommodate pig-iron produced from bauxite residue.

Slag Characteristics and Leaching

There is a general agreement between calculated (Fig. 2c) and experimental (Fig. 5) results in that the C12A phase can be formed if the addition of CaO is tuned appropriately. Adding too little CaO will reduce the amount of C12A, and Group II samples display the lowest aluminum recoveries of 10–20% (Fig. 6). Calculations suggest that CA and C2AS form at lower CaO additions but, according to Fig. 5, CA cannot be identified in any of the diffractograms. The low recoveries in Group II samples can be related to the small fraction of the highly leachable C12A phase found alongside the insoluble C2AS phase (Fig. 7). On the assumption that C2AS does not react with the sodium carbonate solution, there is a small discrepancy in the content of C2AS before and after leaching in the figure, hence manifesting the inherent uncertainty in the semi-quantitative XRD phase identification method and XRF measurements. However, with appropriate care, the data has been considered to be accurate enough to describe general trends in the samples.

The C12A phase is found to be the predominant Al-bearing phase in Group III and, with the exception of sample 1.2, they display the highest Al-recoveries of all sample (Fig. 6). The high recoveries can be related to Al being contained within the highly leachable C12A phase (Fig. 7). However, residual C12A in the samples after leaching indicates incomplete leaching. The surface of the calcium-aluminate particles gets covered in a passivating CaCO3 layer during leaching (Fig. 8a), which is known to limit the reaction between particles and the leaching solution [16]. This suggests that the recovery is sensitive to the physical properties of the particles, such as particle size and the presence of cracks. In the current work, slags were only sieved to below 125 µm before leaching, and the lower recovery of sample 1.2 may simply be a result of a less propitious particle size distribution. However, the reduced recoveries may also be related to the presence of Ti (Table 5), primarily in the form of CaTiO3(s) (Fig. 5). Particles, marked as D in Table 7, are on average also found to contain approximately 15 wt% Al. Previous studies confirm that Al may be introduced into the structure as a CaTi1−xAlxO3-δ solid solution, while still showing a single CaTiO3(s) phase in the range of 0 ≤ x ≤ 0.4 [26]. The change in unit cell parameters is, however, hampered by the complexity of the diffractograms in the current work. These particles are found in both samples 1.2 and 2.2 and cannot explain the difference in recoveries between them. Equilibrium calculations in Fig. 2b suggest that the majority of Ti still remains as a solid perovskite solution up to 1650 °C. CaTi1−xAlxO3-δ was previously synthesized by sintering at temperatures of 1450 °C [26], and one can argue that incorporation may depend upon the degree of smelting of the perovskite phase. Consequently, from a qualitative standpoint, the fact that Al appears to be incorporated and immobilized in the perovskite structure may have negative implications on its recovery. The low Ti-level of sample 3.1 is assumed to be related to the high smelting temperature, where Ti-oxides have been reduced and precipitated as carbides from the liquid metal upon solidification. As a result, no Al-bearing perovskites have currently been found in this sample. The lower recovery of sample 3.2, although being molten at the same temperature, may be related to the copresence of C3A (Fig. 5) and increased stabilization of Ti in the slag phase (Table 5), due to increased CaO addition.

The C12A phase will be replaced by C3A if too much CaO is added, represented by the Group I samples. A lesser C12A signal is still present, but the diffractograms are clearly dominated by C3A. The recovery of Al is also considerably lower, as only a small fraction of the Al is contained within the C12A phase. For sample 1.3, the recovery of Al surpasses the amount which can be related to C12A (Fig. 7). However, while C3A is known to be a leachable phase, it cannot be said with certainty if this can be related to combined leaching of C12 and C3A or the semi-quantitative nature of the data that was used to calculate the distribution in Fig. 7. Samples 2.3 and 3.2, on the other hand, suggest insignificant leaching of the C3A phase in current experiments, and different leaching parameters may be required to accommodate for leaching of this phase [9]. Thermodynamics suggests that the C12A phase can be promoted by increasing the smelting temperature of the samples with lowest CaO additions (150 g; Fig. 2c). The higher temperature increases the preference of Si for entering the pig-iron and escaping the melt as SiO(g), altering the slag composition to one that is favorable in terms of C12A and preventive in terms of C2AS formation.

Phase identification (Fig. 5) clearly shows that γ- and β-C2S are the primary silicate phases in the slags. The high-temperature α-polymorph transforms into its β- and γ-counterparts when reaching temperatures of 675 and 490 °C, respectively. The β- to γ- transformation is associated with a particularly large volume expansion of 12% that may be utilized for achieving slags that disintegrate upon cooling [20]. Several slags cracked during cooling, leaving a powdery slag (Table 3), and semi-quantitative phase identification has been used to calculate the γ-to-β ratio of all samples in Table 8, and there is a clear correlation between the cracking behavior and γ-to-β ratios. Samples with ratios below unity remained intact, while samples with ratios much higher than unity cracked. Sample 3.1, with a ratio of 1.2, was found to be semi-intact. It is therefore reasonable to assume that the observed cracking can be related to formation of γ-C2S. However, the reason behind the varying γ-to-β ratios is still unclear. β-C2S is metastable at room-temperature and will preferably transform into γ-C2S if stabilizing conditions are not met. This transformation is unwanted e.g. in production of cement and steels, and a significant effort is put on developing methods for stabilizing β-C2S. Disintegration can be prevented by physical and chemical stabilization techniques, and methods covered in literature include (i) rapid cooling at rates higher than 5 °C/s, (ii) altering the slag chemistry to limit/avoid formation of C2S altogether and (iii) chemical stabilization by additives [27]. Current experiments are not compatible with (i) and (ii) in that samples are cooled by natural convection and that one does not seek to avoid formation of C2S. Samples 1.1 and 2.1 display opposite cracking behavior, despite both capturing significant amounts of Si in C2AS. Small concentrations of various oxides have proven to have a stabilizing effect by forming solid solutions with C2S [28]. A recent study found that the addition of up to 3% of TiO2 effectively stabilized the β-polymorph by substituting Si4+ in the SiO42− tetrahedron with Ti4+ [29]. This suggests that the content of Ti may offer some stabilization to the β-C2S phase in the current samples, but the results require additional analysis that may be targeted in a later study.

Table 8 Ratio of γ-Ca2SiO4 versus β-Ca2SiO4 in the slags, as calculated from semi-quantitative XRD phase analysis
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All in all, this work has successfully synthesized pig-iron and calcium aluminate slags with various properties. The usability of the pig-iron is assumed to be limited to production of certain cast irons that may be able to handle the inhomogeneous nature of the bauxite residue and its impurities. Recovery of Al correlate well with the occurrence of the highly leachable C12A phase. The study shows no clear evidence for Al recovery from the C3A phase, and one should not rule out the possibility of higher recoveries by further optimization of the leaching process. Too low CaO additions may capture Al and Si in the undesirable C2AS phase, which will reduce the leachability of the slags and potentially their capability of disintegrating. Disintegration took place for samples displaying high γ-to-β C2S ratio, although the reasons for variable transformation from β- to γ-C2S is still unclear. Disintegration will reduce the need for post-processing, but the recovery will still be limited by the formation of an inhibiting layer of CaCO3 on the reaction surface of the calcium-aluminate particles during leaching. The force exerted by the expanding slags was large enough to crack several crucibles, which is something that needs to be handled. Finally, one should consider if it is propitious to recover Ti and Si to the pig-iron. While exceptions do exist, Ti is generally unwanted in pig-iron, due to the formation of hard carbides and nitrides. On the other hand, numerous possible implications involving the occurrence of Ti in the slag have also been discussed. First and foremost, observations suggest that Al can be immobilized in the CaTiO3(s) structure. Furthermore, literature suggests that Ti may stabilize the β-C2S phase and thereby prevent slag disintegration. Increased concentration of Si in the pig-iron will increase its market value but will also require higher costs. It may therefore be more feasible to retain Si in the slag, where it can be recycled together with CaCO3 e.g. by the construction industry.

Conclusions

Pig-iron and calcium aluminate slags have been successfully synthesized from bauxite residue at temperatures of 1550–1750 °C. Fe recovers primarily to the pig-iron, and CaO are added to optimize the composition of the slag to one that favors formation of the highly leachable mayenite phase. While there is a clear correlation between the amount of Al recovered and the occurrence of the mayenite phase, it is still limited to a maximum of 50–60%. The formation of an inhibiting layer of CaCO3 on the surface of the calcium aluminate particles and immobilization of Al in CaTiO3 particles are suggested to play important roles in the total recovery of Al. Samples with low CaO additions are vulnerable to formation of the undesirable gehlenite phase, which effectively immobilizes Al and reduces the recovery considerably. Slags with high γ-to-β C2S ratios are also found to disintegrate, which can be advantageous for post-processing of slags.