Introduction
Decarbonising the world economy relies on a secure and sustainable supply of critical metals and minerals that underpin low-carbon technologies. The development of wind, hydro- and geothermal energy technologies, as well as energy storage systems and transport solutions with less environmental impact will continue to rely on primary mining for the foreseeable future, as more sustainable options, e.g. the recovery of metals from e-waste, cannot satisfy the demand for critical resources. However, although mining can bring numerous benefits to society and global economic development, almost all mining operations are associated with negative effects on the environment, including ecosystem loss and the heavy-metal pollution of water, soil, or dust. Mining is currently responsible for up to 7% of greenhouse-gas emissions globally (Delevingne et al., Reference Delevingne, Glazener, Grégoir and Henderson2020), of which emissions incurred directly through mining operations and power consumption make up ~1%. An additional 28% of global emissions are indirect and include coal-based power or gas combustion to process metals, and emissions generated upstream to produce mining equipment (Delevingne et al., Reference Delevingne, Glazener, Grégoir and Henderson2020).
The mitigation of greenhouse-gas emissions from mining operations can thus make a substantial contribution to climate change mitigation. This will require integration of clean energy technologies and carbon capture and storage (CCS) at different stages of the mining operation, from ore recovery to mineral processing. CCS can theoretically be achieved by either the injection of CO2 in situ into suitable geological formations, where it can be immobilised by several mechanisms (Matter and Kelemen, Reference Matter and Kelemen2009; Kelemen et al., Reference Kelemen, Matter, Streit, Rudge, Curry, Blusztajn, Jeanloz and Freeman2011; De Silva et al., Reference De Silva, Ranjith and Perera2015) or by the reaction of CO2 with feedstock materials to produce carbonate minerals. The latter is typically referred to as ex situ Carbon Capture and Storage by Mineralisation (CCSM). Recent advances in CCSM propose utilising carbonation as a metal recovery process (Wang et al., Reference Wang, Dreisinger, Jarvis, Hitchins and Trytten2021; Wang and Dreisinger, Reference Wang and Dreisinger2022, Reference Wang and Dreisinger2023). Some of the best feedstock materials for CCSM are magnesium (Mg)-rich ultramafic rocks, serpentinites and their weathering products (laterites). The last twenty years have seen significant progress in the understanding of mineralogical and geochemical factors controlling efficient carbonation (Zevenhoven et al., Reference Zevenhoven, Kavaliauskaite and Denafas2003; Maroto-Valer et al., Reference Maroto-Valer, Fauth, Kuchta, Zhang and Andresen2005; Fagerlund et al., Reference Fagerlund, Teir, Nduagu and Zevenhoven2009; Hanchen et al., Reference Hanchen, Prigiobbe, Baciocchi and Mazzotti2008; Fagerlund and Zevenhoven, Reference Fagerlund and Zevenhoven2011; Kelemen et al., Reference Kelemen, Matter, Streit, Rudge, Curry, Blusztajn, Jeanloz and Freeman2011; Werner et al., Reference Werner, Hariharan, Bortolan, Zingaretti, Baciocchi and Mazzotti2013; Harrison et al., Reference Harrison, Power and Dipple2013; Oskierski et al., Reference Oskierski, Dlugogorski and Jacobsen2013; Power et al., Reference Power, Wilson and Dipple2013; Lacinska et al., Reference Lacinska, Styles, Bateman, Wagner, Hall, Gowing and Brown2016; Lacinska et al., Reference Lacinska, Styles, Bateman, Hall and Brown2017; Power et al., Reference Power, Paulo, Long, Lockhart, Stubbs, French and Caldwell2021), or the economic assessment of the technology (Strunge et al., Reference Strunge, Renforth and Van der Spek2022) and CCSM is now advancing to pilot projects and medium-scale industrial applications (MCi Carbon, 2023; Macpherson, Reference Macpherson2023). In addition to their utilisation in CCSM, ultramafic rocks and laterites are also mined globally for battery and technology metals, such as nickel, cobalt and/or the platinum-group elements.
Conventional mining and processing of ultramafic rock-hosted ores is commonly associated with the generation and release of hexavalent chromium (Cr6+), a toxic carcinogenic pollutant. The total Cr concentration in ultramafic rocks is estimated at 2 g/kg, approximately 10 times more than in mafic and 100 times more than in felsic rocks (Motzer, Reference Motzer2004). Chromium is redox sensitive and can adopt oxidation states ranging from –4 to +6. Trivalent and hexavalent chromium are the two most common naturally-occurring forms (Motzer, Reference Motzer2004). The trivalent species is mainly immobile in the environment and does not pose environmental risk, whereas the highly mobile Cr6+ is toxic in the biosphere when present at concentrations above the guideline value of 50 μg/L (World Health Organization, 2020).
The extent of water–rock interactions during the weathering of ultramafic rocks and serpentinites affects the concentration of Cr in the surrounding waters and soils, with the oxidation state dependent on the degree of redox reaction with other electron donors and acceptors present (McClain and Maher, Reference McClain and Maher2016). For example, the occurrence of Cr6+ (~3–8% of the total chromium) in the lateritic regolith developed on ultramafic rocks in New Caledonia has been associated strongly with the presence of Mn3+ or Mn4+ (Fandeur et al., Reference Fandeur, Juillot, Morin, Olivi, Cognigni, Webb, Ambrosi, Fritsch, Guyot and Brown2009; Santos et al., Reference Santos, Dybowska, Schofield, Herrington, Cibin and Johnson2022). Notable amounts of Cr6+ found in natural systems have a direct anthropogenic origin, related to the sediment drainage from open pit mining (Gunkel-Grillon et al., Reference Gunkel-Grillon, Laporte-Magoni, Lemestre and Bazire2014) or pyro- and hydrometallurgical processing of ultramafic rocks and Ni laterites (PT Vale Indonesia Tbk, 2017).
Current Cr6+ remediation mechanisms include physical, chemical and/or biochemical processing of the waste materials. However, a recent review suggests that notwithstanding the significant capability of the various mechanisms, the associated cost, sustainability of the methods, sludge generation and huge amount of chemicals necessitate new innovative, environment-friendly propositions (Kumar and Dwivedi, Reference Kumar and Dwivedi2021). An alternative process for Cr6+ remediation is to remove it through precipitation. This occurs naturally through reduction to Cr3+ and precipitation of insoluble Cr3+ oxides and hydroxides (Palmer, Reference Palmer and Wittbrodt1991). In naturally forming carbonates, the scavenging of potentially toxic elements (PTE), e.g. Cr, has been reported previously from travertines (Olsson et al., Reference Olsson, Stipp and Gislason2014) and hydromagnesite (Boschi et al., Reference Boschi, Bedini, Baneschi, Rielli, Baumgartner, Perchiazzi, Ulyanov, Zanchetta and Dini2020). The pathway in which Cr can be incorporated crystallographically in minerals is determined primarily by its oxidation state. Trivalent Cr occupies the octahedral site of many minerals by substituting for Fe3+, Al3+, or Ti4+. In contrast, Cr6+, which is typically in the form of the chromate anion (CrO42–), assumes tetrahedral coordination (Liu et al., Reference Liu, Hystad, Golden, Hummer, Downs, Morrison, Ralph and Hazen2017). There are several naturally occurring minerals that contain both Cr3+ and carbonate ions in their crystal structures, including stichtite Mg6Cr2CO3(OH)16⋅4H2O and grguricite CaCr2(CO3)2(OH)4⋅4H2O, however there are currently no known minerals with concurrent chromate and carbonate anions listed in the International Mineralogical Association database (Pasero, Reference Pasero2023). Such a combination is theoretically possible, albeit in actuality not yet reported, in layered double hydroxide or the ettringite-group minerals (Juroszek et al., Reference Juroszek, Kruger, Galuskina, Kruger, Vapnik and Galuskin2020). Hexavalent chromium has been reported from experimentally produced Ca carbonates, where chromate substitutes for the carbonate groups in calcite (Tang et al., Reference Tang, Elzinga, Lee and Reeder2005; Hua et al., Reference Hua, Deng, Thornton, Yang and Amonette2007; Tang et al., Reference Tang, Elzinga, Lee and Reeder2007; Sanchez-Pastor et al., Reference Sanchez-Pastor, Gigler, Cruz, Park, Jordan and Fernandez-Diaz2011). The incorporation mechanism requires overcoming a geometric incompatibility between the tetrahedral sites hosting Cr with the planar triangular carbonate groups causing local strain of the crystal structure (Tang et al., Reference Tang, Elzinga, Lee and Reeder2007; Sanchez-Pastor et al., Reference Sanchez-Pastor, Gigler, Cruz, Park, Jordan and Fernandez-Diaz2011). Nevertheless, successful partitioning of Cr6+ into calcite has been observed, especially in strongly contaminated media, suggesting that the fate of this pollutant in natural environments can be influenced significantly by co-precipitation processes with carbonates (Sanchez-Pastor et al., Reference Sanchez-Pastor, Gigler, Cruz, Park, Jordan and Fernandez-Diaz2011).
Co-precipitation of chromium with magnesium carbonates has been less well studied, though nesquehonite (MgCO3⋅3H2O) has been shown to incorporate Cr3+ through substitution with Mg2+ (Hamilton et al., Reference Hamilton, Wilson, Morgan, Turvey, Paterson, MacRae, McCutcheon and Southam2016; Hamilton et al., Reference Hamilton, Wilson, Morgan, Turvey, Paterson, Jowitt, McCutcheon and Southam2018). Understanding the potential of Mg carbonates to trap chromium is of significant importance to mining and processing of ores hosted by ultramafic rocks. Here, we present an outlook on that potential based on experimental and microanalytical investigations.
Methodology
A series of co-precipitation experiments were conducted using aqueous solutions of MgCl2⋅6H2O (1.8 mol L−1), K2Cr2O7 (0.18 mol L−1) and Na2CO3 (1.8 mol L−1). Upon mixing at room temperature (20°C), the material became turbid immediately and a yellow gel formed. To monitor the speciation of chromate and its localisation in the resulting phases, a portion of the material was monitored continuously for eight hours by X-ray absorption near-edge structure (XANES) measurements during carbonate mineral crystallisation (Supplementary Fig. S1). A different portion of the same starting material was placed in an oven at 60°C for 6 hours, and XANES spectra were obtained subsequently. Additionally, an attempt to precipitate stichtite was made (Supplementary Figs S2 and S3), which resulted in poorly crystalline, albeit Cr-bearing, nano-scale particulates that are also the subject of investigation.
A multi-scale, multi-technique analytical programme was applied to elucidate the mineralogy and composition of the resulting materials, including overall material morphology by scanning electron microscopy (SEM), determination of crystalline phase composition by X-ray diffraction (XRD), element depth distribution profiles by energy-dispersive (EDX) X-ray analysis by SEM and laser-ablation inductively coupled plasma mass spectrometry (LA-ICP-MS) mapping. Determination of the chromium oxidation state and its local coordination environment in the crystal structure was achieved by XANES.
Scanning electron microscopy analyses were performed using a Zeiss Sigma 300 VP-FEG with Bruker Quantax XFlash 6|30 EDX detectors system at the British Geological Survey. Samples were analysed in the form of carbon sputter coated (≈25 nm thick) polished blocks and as rough materials distributed on an aluminium stub with carbon tab. The SEM was operated under conditions of high vacuum (1.2 × 10−6 Torr) at accelerating voltages ranging from 3–15 kV, with 8.5 mm optimal analytical working distance and an X-ray detector take-off angle of 35°. Qualitative compositional analyses of the mineral phases were performed using Bruker systems SDD EDS. Quantitative analysis was not undertaken due to analytical challenges associated with the fine grain size and beam sensitive nature of the experimental materials. High-resolution imagery was performed at low kV (3–5 kV) and using an in-lens secondary electron detector.
X-ray diffraction was performed using a Malvern PANalytical X'Pert Pro series X-ray diffractometer at the British Geological Survey, equipped with an X'Celerator detector, cobalt-target tube and generator operated at 45 kV and 40 mA, in Bragg-Brentano geometry. Samples for XRD were ground in an agate pestle and mortar and <10 mg subsamples mounted on silicon crystal ‘zero background’ substrates using a single drop of acetone. Diffraction data were analysed using Malvern PANalytical X'Pert HighScore Plus version 5.1 software coupled to the 2022 version of the International Centre for Diffraction Data (ICDD) PDF4+ database (https://www.icdd.com/).
X-ray absorption near-edge structure (XANES) data were collected at the B18 beamline at the Diamond Light Source in Harwell, United Kingdom. The measurement conditions for reference data and the sample were the same. The Cr K XANES were recorded in fluorescence-yield mode with a 36-element solid-state Ge detector. A Si(111) double crystal monochromator was used, which provides an energy range from 4 to 11 keV (Dent et al., Reference Dent, Cibin, Ramos, Smith, Scott, Varandas, Pearson, Krumpa, Jones and Robbins2009). The spectra were acquired in continuous scanning (‘quick EXAFS’, QEXAFS) mode from 5790 eV to 6630 eV with a step size of 0.25 eV. X-ray absorption spectroscopy (XAS) data analysis was performed using the Demeter software package (Ravel and Newville, Reference Ravel and Newville2005). Data were extracted using WebPlotDigitizer (Rohatgi, Reference Rohatgi2015).
Laser ablation inductively couple plasma mass spectrometry (LA-ICP-MS) analyses were done on polished blocks using Elemental Scientific Lasers imageGEO193 (British Geological Survey). For mapping these samples, the 193 nm excimer laser spot was a 10 × 10 μm square and the laser set to 20Hz repetition rate and a fluence of 4.4 J/cm2; the beam was then rastered as a series of lines at 25 μm/s across the target area, all being controlled by the proprietary ‘AV2’ software. The ICP-MS was an Agilent 8900 series instrument controlled by MassHunter software, data were collected in a time resolved fashion for isotopes 23Na, 24Mg, 39K, 42Ca and 52Cr with a dwell time of 14 ms except Cr with 35 ms. As well as the samples, standards SRM610 (NIST, USA) and GSD-1G (USGS, USA) were analysed as calibrants. All calibration calculations and mapping were performed using the Elemental Scientific Lasers Iolite4 software taking the both the time resolved counts/s data from an Agilent file and the laser log file; for concentration calculation Mg was used as an internal standard with an assumed stoichiometric concentration of 288,000 mg/kg.
Results
The room-temperature (20°C) experiments with stirring resulted in the formation of prismatic crystals (<1 mm) of nesquehonite (MgCO3⋅3H2O) and lesser amounts of hydromagnesite [Mg5(CO3)4(OH)2⋅4H2O] as spherules. Combined microbeam analyses on the nesquehonite crystals provided evidence that neither Cr6+ nor Cr3+ were incorporated into the structure of this mineral (Fig. 1a,e), however element-distribution maps did show Cr-bearing nano-scale particulates located at the surfaces of the main components (Fig. 1b). The surface particulates also contain Mg, Na, Cl and O though they were too fine grained for separation and further analysis to identify the phase.
Secondary electron images of (a) prismatic crystals of nesquehonite locally covered by nano-sized Cr-bearing material, shown in detail in (b); (c) spherulites of hydromagnesite formed at 20°C and (d) hydromagnesite/dypingite formed at 60°C; (e) back-scattered electron and LA-ICP-MS maps showing the distribution of Mg and Cr nesquehonite prismatic crystals; (f) back-scattered electron and LA-ICP-MS maps showing the distribution of Mg and Cr in the hydromagnesite, 20°C; (g) LA-ICP-MS maps showing the distribution of Mg and Cr in the 60°C precipitates. Note: Mg is shown in cps as it was used as an internal standard.
The experiments at 60°C without stirring, resulted in the precipitation of spherical aggregates (<200 μm) of both hydromagnesite and dypingite, Mg5(CO3)4(OH)2⋅5H2O. Although no nesquehonite was detected by XRD or SEM analyses, trace amounts might be present. These spherules and the similarly sized spherules of hydromagnesite from the 20°C precipitation are shown in Fig. 1d and 1c, respectively.
Microbeam raster analyses and compositional mapping of hydromagnesite (20°C experiment) revealed a notable (6–8 g/kg) association of chromium with the spherulite cores, commonly seen with Na and/or Cl, probably originating from halite (NaCl) and/or other nano-sized phases, interspersed and/or intergrown with the hydromagnesite (Fig. 1f). The distribution of chromium in hydromagnesite–dypingite (60°C) is notably different and comprises a more even dispersion of the element across a whole spherulite, with the highest concentration observed consistently in the marginal zones of increased microporosity (Fig. 1g). The amount of chromium associated with the spherulites formed at 60°C is an order of magnitude lower than in the precipitates from the 20°C experiment.
X-ray absorption near-edge structure (XANES) at the Cr K-edge collected from the hydromagnesite spherulites (20°C) shows a prominent pre-edge peak at 5995.5 eV, indicating the presence of Cr6+, whereas the Cr K XANES pre-edge of hydromagnesite/dypingite formed at 60°C contains only two weak peaks at 6010 eV and 6025 eV, which are indicative of Cr3+ (Fig. 2b). The presence of Cr3+ is probably the result of chromium reduction during or after the precipitation. The exact molecular-level mechanism for this reduction and its timing are currently unclear. One possible mechanism might involve the ubiquitous chlorine present in the experiment, the redox reactions accompanying the oxidation of the chloride ion and the reduction of chromium to Cr3+ in the solution. The processes are complex and proceed via several intermediates, however they could lead to the formation of chlorine gas (and temperature driven evaporation) and/or chlorate (ClO3–) catalysed by the presence of chromate (CrO42–) (Busch et al., Reference Busch, Simic and Ahlberg2022). As no reduction occurred during the 20°C experiment, we can exclude radiolytic reduction by the X-ray beam. The increase of temperature to 60°C appears to be the trigger of the reactions. Indeed, previous in situ XANES of Cr(OH)3 revealed strongly temperature-dependent interconversions between Cr3+ and Cr6+ (Schroeder et al., Reference Schroeder, Moggridge, Lambert and Rayment1997). This dependence of speciation on the process conditions may be potentially important in the long-term design of industrial crystallographic trapping of Cr in the carbonate structure and deserves further investigation.
(a) Cr K-edge XANES spectra, with the 5995.5 eV Cr6+ pre-edge peak, collected from isolated spherulites of hydromagnesite formed at 20°C (in red – this study), K2Cr2O7, CaCrO4 (Tang et al., Reference Tang, Elzinga, Lee and Reeder2007) and Cr-doped calcite (c25-1hr from Tang et al., Reference Tang, Elzinga, Lee and Reeder2007). (b) XANES of hydromagnesite/dypingite spherulites formed at 60°C (in red – this study), compared to Cr3+-bearing reference materials, including Cr in nesquehonite (Nes) (Hamilton et al., Reference Hamilton, Wilson, Morgan, Turvey, Paterson, MacRae, McCutcheon and Southam2016) and K2Cr2O7, i.e. the initial host of chromium.
However, if chloride–chromate redox reactions have occurred, then we speculate the following set of events resulted in the lower concentration and a more even distribution of chromium as Cr3+ in the spherulites that formed at 60°C: (1) rapid trapping of Cr6+ in amorphous magnesium carbonate (AMC); (2) reduction of the residual Cr6+ in the solution to Cr3+, driven by reactions involving chloride and/or temperature-dependent interconversion between chromium species, and precipitation as Cr(OH)3; which (3) creates a chromium concentration gradient between the solid and the solution, which in turn drives the diffusion of Cr6+ trapped in the solid out to the solution phase. Diffused chromium undergoes reduction and precipitation, as per (2), until the cessation of the 6 hours experiment.
The higher concentration of chromium in the outer zones of the spherulites (Fig. 1g) might have resulted from a combination of: (1) diffusion of core zone chromium towards the margin and reduction upon contact with solution; and (2) reduction of in situ chromium, with the width of the chromium-rich rim representing the depth of chloride-bearing solution penetration into the solid. Regardless, it is apparent that the diffused and in situ chromium have been mostly expelled from the solid upon the crystallisation of AMC into hydromagnesite/dypingite. Further trace-element investigations are needed to establish if any chromium was captured crystallographically, and if so, what the effect of such structural substitution is on the stability of the carbonate mineral.
Discussion and outlook
On the basis of the rapid precipitation of carbonate (seconds) in the static experiment and the spherical morphology and texture of hydromagnesite and dypingite, we infer that the initial material formed was amorphous and attained crystalline structure over time. Nesquehonite was the predominant phase identified in the stirred experiments. Such dynamic systems are known to promote the transformation of amorphous magnesium carbonate in aqueous solution to long-range ordered minerals, such as nesquehonite (Yamamoto et al., Reference Yamamoto, Kyono and Okada2021).
Our current understanding of the striking, albeit inconsistent association of Cr6+ with the cores of hydromagnesite spherulites does not support a structural incorporation mechanism, instead it suggests a physical trapping of Cr-bearing material in the intercrystalline microporosity of the aggregates (Fig. 3). The coexistence of and, the notably more even distribution of Cr3+ within hydromagnesite–dypingite spherical aggregates formed at 60°C, in addition to the similarity of our XANES data with that of Cr(OH)3, are intriguing (Fig. 2) and suggest the potential incorporation of hydroxide. Trivalent chromium might be incorporated into carbonate as shown by previous investigations (Hamilton et al., Reference Hamilton, Wilson, Morgan, Turvey, Paterson, MacRae, McCutcheon and Southam2016; Boschi et al., Reference Boschi, Bedini, Baneschi, Rielli, Baumgartner, Perchiazzi, Ulyanov, Zanchetta and Dini2020) although not necessarily by a direct Cr3+ to Mg2+ substitution. In calcium carbonate, Cr3+ cannot substitute directly for Ca2+, however as hydroxide, it may be adsorbed to crystal surfaces or occupy interstitial voids in the crystals (Fang et al., Reference Fang, Liu, Yao, Zhou, Wei and Qin2022). A similar phenomenon might be true for magnesium carbonates (Fig. 3), and in such cases, chromium would have been expelled from the carbonate structure during the crystallisation of AMC. The crystallisation of AMC and the degree to which incompatible elements are incorporated structurally or physically, and/or expelled from the crystalline material might depend on the mechanism of crystallisation, i.e. dissolution–reprecipitation versus solid-state crystallisation. In the latter, a cascade of fast exchanges of hydrogen between the AMC and H2O molecules from the hydration shell and the surrounding solution, enhances mobility of ions/molecules that compose the AMC (Von Euw et al, Reference Von Euw, Azais, Manichev, Laurent, Pehau-Arnaudet, Rivers, Murali, Kelly and Falkowski2020). This allows for the rearrangement of AMC into crystalline domains via solid-state transformation (idem), possibly promoting the expulsion of incompatible elements and their physical entrapment in the local microporosity, as observed in the spherulites formed in this investigation. Although the spherulite morphology of hydromagnesite–dypingite precipitates is consistent with solid-state crystallisation, the dissolution–reprecipitation mechanism or a combination of both crystallisation pathways can not be ignored. Dissolution–reprecipitation would probably remove incompatible elements from the vicinity of the crystallising solid into the solution, decreasing the degree of entrapment and ultimately leading to the release of these elements. The phase-transformation mechanisms, including both the AMC to crystalline and subsequent changes to crystal structure within the hydrated–anhydrous magnesium carbonate system, are highly relevant to the cycling of potential contaminants such as chromium (Harison et al, Reference Harrison, Mavromatis, Oelkers and Bénézeth2019). Further experimental and nanoscale investigations are required to appraise the incorporation mechanism in detail. One potential avenue to explore is pressure-induced crystallisation that has been shown as an efficient pathway to dope incompatible elements into crystals of calcium carbonates (Matsunuma et al., Reference Matsunuma, Kaqi, Komatsu, Maruyama and Yoshino2014).
Possible incorporation mechanisms of chromium in Mg carbonates, including physical trapping and adsorption.
In our opinion, experimental efforts should also focus on such Cr3+-bearing materials that have a natural long-term capacity to retain chromium, rather than forcing structure-modifying incompatible chromate ions into an otherwise stable structure of magnesium carbonates. Accordingly, we recognise that minerals belonging to the layered double hydroxides (LDHs), specifically the CO2-bearing hydrotalcite supergroup with pyroaurite–hydrotalcite–stichtite end-members might present a viable matrix for chromium. These minerals comprise positively charged brucite-like layers (A6–xB2+x)(OH)2, where A is a divalent cation (e.g. Mg or Fe) and B is a trivalent cation (e.g. Al, Fe or Cr). Interlayer regions typically contain a monovalent or divalent anion X, such as CO32–, SO42–, Cl– and OH–. The well-defined structural site for trivalent elements and the wide range of possible cation–anion substitutions suggest that hydrotalcites represent a potentially suitable matrix for chromium or other PTE and CO2 (Aschenbrenner et al., Reference Aschenbrenner, McGuire, Alsamaq, Wang, Supasitmongkol, Al-Duri, Styring and Wood2011). Although the incorporation of trivalent chromium in hydrotalcite is relatively straightforward, albeit requiring metal reduction, the substitution of chromate for carbonate is challenging because of structural affinity of the CO32– ion to the local symmetry of the interlayer site in hydrotalcite and the strong hydrogen bonding between the hydroxyl ions of the layer with the carbonate ions (Prasanna and Kamath, Reference Prasanna and Kamath2008). This makes the CO2-bearing hydrotalcite very stable and thus it has a wide range of applications, including the cement industry (Bernard et al., Reference Bernard, Zucha, Lothenbach and Mader2022). The hydrotalcite supergroup with pyroaurite–hydrotalcite–stichtite end-members represents a potential stable host for chromium and the CO2 formed through integrated CCSM.
We, thus hypothesise that a disruptive innovation in the design of Ni laterite ore processing to include CO2 and chromium sequestration through the precipitation of hydrotalcite will lead to more sustainable utilisation and management of the Earth's resources. Such process integration necessitates knowledge cross-fertilisation and a shared vision between industry and academia to timely assess its potential and drive the theory of change in the ore processing industry.
Acknowledgements
The research was part of the BGS International NC programme ‘Geoscience to tackle Global Environmental Challenges’, NERC reference NE/X006255/1. The authors publish with the permission of the Executive Director of the British Geological Survey (UKRI). Dr Michael Styles and Dr Kathryn Goodenough are acknowledged for providing an internal review of the manuscript. DS and SLMS acknowledge financial support by EPSRC through the Future Continuous Manufacturing and Advanced Crystallisation (CMAC) Hub (EP/P006965/1). DS was financially supported by Innovate UK under a Knowledge Transfer Partnership. We acknowledge the allocation of B18 beamtime by Diamond Light Source under the reference SP28772-1 and thank the beamline scientists Diego Gianolio and Veronica Cellorio for their support. John Fletcher (BGS) is thanked for the preparation of polished blocks for microanalysis. The authors thank anonymous reviewers and the editors of the journals for their valuable comments that improved the quality of the paper. All data supporting this study are provided either in the results section of this paper or in the electronic supplementary information accompanying it.
Supplementary material
The supplementary material for this article can be found at https://doi.org/10.1180/mgm.2023.91.
Competing interests
The authors declare none.
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