CROSS-REFERENCE TO RELATED APPLICATIONS

[0001] This application claims the benefit of Provisional Appl. No. 63/209,807, filed June 11, 2021. The content of the aforesaid application is relied upon and is incorporated by reference herein in its entirety.

FIELD OF THE INVENTION

[0002] The field of the invention relates generally to extraction of metal from metal-containing materials. More particularly, the invention relates to extraction of metal from spent lithium- ion batteries.

BACKGROUND

[0003] The demand for lithium-ion batteries (LIBs) for consumer electronics and automotive applications is expected to increase during the next 15-20 years (Steward et al., 2019). Despite the development of high-performance electrode materials to meet the increasing demand for energy storage, lithium cobalt (III) oxide (LiCoC^) remains the most common cathode material in LIBs for high specific energy, low rate of self-discharge, and simple manufacturing (Deng, 2015; Golmohammadzadeh et al., 2018). After a short life span of 3-8 years, the disposal of end-of-life LIBs should be carefully managed, to avoid contamination of soil, air, and groundwater (Liu et al., 2017). In addition, spent LIBs contain metals such as cobalt and lithium, and it is desirable to recover these metals. Thus, the recycling of spent LIBs is urgent in terms of environmental restriction, resource utilization and economic benefits.

[0004] Compared with the pyrometallurgy, a hydrometallurgical process is reported to provide an environmentally friendly and efficient method to recover valuable metals from the cathode of spent LIBs (Li et al., 2016). Inorganic acid, especially sulfuric acid, is widely used in the recycling process, but the high acid concentration needed can require expensive downstream processing. Environmentally benign and biodegradable chemicals, including organic acids such as citric acid, tartaric acid, malic acid, succinic acid, ascorbic acid have been explored as lixiviants in the treatment of spent LIBs (Dos Santos et al., 2019; Li et al., 2015; Musariri et al., 2019; Nayaka et al., 2016b). The leaching kinetics of organic acids are usually slower than those of inorganic acids due to higher pKa values. However, a potential advantage of using organic acids is their selectivity. According to Gao et al., cobalt and lithium can be selectively leached using organic acid, for separating valuable metals and Al foil (Gao et al., 2018).

[0005] Recently, glycine has been reported as a lixiviant in copper and gold leaching, with the assistance of hydrogen peroxide in an alkaline environment (Eksteen et al., 2017; Perea and Restrepo, 2018; Shin et al., 2019).

[0006] This background information is provided for the purpose of making information believed by the applicant to be of possible relevance to the present invention. No admission is necessarily intended, nor should it be construed, that any of the preceding information constitutes prior art against the present invention.

SUMMARY

[0007] There is an urgent and increasing need for methods of recovering metals from lithium- ion batteries. The proliferation of consumer electronic devices and electronic vehicle lithium-ion batteries (LIBs) can be expected to accelerate rapidly. Improved and cost- effective methods are necessary for enabling the recycling of spent LIBs and reducing the environmental and economic impact of these materials critical to LIB chemistry.

[0008] In some embodiments, the invention provides method of leaching a metal-containing material (e.g., ore, concentrate, etc.), the method comprising: a) forming a leach solution by dissolving at least one amino acid (e.g., glycine, histidine and/or lysine) and a reducing agent (e.g. sodium metabisulfite (SMB)) in water; b) forming a mixture of the leach solution of step (a) and a metal-containing material; c) leaching at least one metal from the metal-containing material by heating the mixture of step (b) in a temperature range from about 20°C to about 100°C.

[0009] In some embodiments, the invention provides a method of recovering metal from a spent lithium-ion battery cathode, the method comprising: a) separating the cathode components by one or more steps of removing adhesive used to adhere LiCo02 to an aluminum foil in the cathode (or in other words step (a) comprises separating the aluminum foil from LiCo02 to recover said LiCo02); b) forming a leach solution by dissolving glycine and sodium metabisulfite in water; c) forming a mixture of the leach solution of step (b) and LiCo02 from step (a); d) leaching at least one metal from the metal-containing material by heating the mixture of step (c) in a temperature range from about 20°C to about 100°C.

BRIEF DESCRIPTION OF THE DRAWINGS

[0010] FIG. 1 is a graph showing speciation of glycine in water at various pH values.

[0011] FIG. 2 is a chart showing and XRD pattern of LiCoCh powder.

[0012] FIGS. 3 A and 3B are graphs showing an effect of Na ₂ S ₂ 0s on L1C0O2 dissolution using 0.5 M glycine at 80°C; FIG. 3 A shows the percentage (%) of Co recovery, and FIG. 3B shows Li recovery (%).

[0013] FIGS. 4A and 4B are graphs showing an effect of glycine concentration on L1C0O2 dissolution using 0.5 M Na ₂ S ₂ 0s at 80°C; FIG. 4A shows Co recovery (%); FIG. 4B shows Li recovery (%).

[0014] FIGS. 5A and 5B are graphs showing an effect of solid/liquid ratio on L1C0O2 dissolution using 0.5 M glycine and 0.5 MNa ₂ S ₂ C> ₅ at 80°C; FIG. 5 A shows metal recovery (%), and FIG. 5B shows metal concentration as molarity (M).

[0015] FIGS. 6A and 6B are graphs showing an effect of temperature on L1C0O2 dissolution using 0.5 M glycine and 0.5 M Na ₂ S ₂ 0s; FIG. 6A shows Co recovery (%), and FIG. 6B shows Li recovery (%).

[0016] FIG. 7 is a graph showing an Arrhenius plot of Co and Li.

[0017] FIGS. 8A and 8B are graphs of XPS spectra; FIG. 8A shows Co 2p core peaks for three samples (SI, S2, S3); FIG. 8B shows O ls core peaks for the three samples (SI, S2, S3).

[0018] FIGS. 9A and 9B are SEM (scanning electron microscopy) images of original L1C0O2 powder (FIG. 9A) and leaching residue (FIG. 9B), respectively.

[0019] FIG. 10 is an SEM image of a leaching residue from after leaching L1C0O2 powder with 0.5 M glycine and 1.0 M Na ₂ S ₂ 0s.

[0020] FIGS. 11 A to 1 IF are SEM and EDS (electron dispersive X-ray microanalysis) images of a leaching residue from after leaching L1C0O2 powder with 0.5 M glycine and 1.0 M Na ₂ S ₂ C> ₅ . FIG. 11A is an SEM image of the residue. The images in FIGS. 11B to 1 IF show EDS analyses of the residue for the elements Co, O, S, Na and C, respectively.

[0021] FIGS. 12A and 12B show an SEM image (FIG. 12A) of a cubic particle of residue from after leaching LiCoCh powder with 0.5 M glycine and 1.0 M Na ₂ S ₂ 0s, and EDS analysis results (FIG. 12B) of the inset region in FIG. 12 A.

[0022] FIG. 13 is a graph showing solution pH and potential during a leaching using optimized concentrations of glycine and Na ₂ S ₂ 0s, at 80°C.

[0023] FIGS. 14A and 14B are graphs showing Eh-pH diagrams for Co (FIG.14A) and Li (FIG. 14B) in glycine-sodium metabisulfite leaching system at 25°C (solid line) and 80°C (dashed line), [Co]=[Li]=0.2 M, [glycine]=[ Na2S2O5]=0.5 M.

DETAILED DESCRIPTION

[0024] Definitions

[0025] For the purposes of promoting an understanding of the principles of the invention, reference will now be made to certain embodiments and specific language will be used to describe the same. It will nevertheless be understood that no limitation of the scope of the invention is thereby intended, and alterations and modifications in the illustrated invention, and further applications of the principles of the invention as illustrated therein are herein contemplated as would normally occur to one skilled in the art to which the invention relates.

[0026] Unless defined otherwise, all technical and scientific terms used herein have the same meaning as commonly understood by one of ordinary skill in the art to which this invention pertains.

[0027] For the purpose of interpreting this specification, the following definitions will apply and whenever appropriate, terms used in the singular will also include the plural and vice versa. In the event that any definition set forth below conflicts with the usage of that word in any other document, including any document incorporated herein by reference, the definition set forth below shall always control for purposes of interpreting this specification and its associated claims unless a contrary meaning is clearly intended (for example in the document where the term is originally used).

[0028] The use of “or” means “and/or” unless stated otherwise. [0029] The use of “a” or “an” herein means “one or more” unless stated otherwise or where the use of “one or more” is clearly inappropriate.

[0030] The use of “comprise,” “comprises,” “comprising,” “include,” “includes,” and “including” are interchangeable and not intended to be limiting. Furthermore, where the description of one or more embodiments uses the term “comprising,” those skilled in the art would understand that, in some specific instances, the embodiment or embodiments can be alternatively described using the language “consisting essentially of’ and/or “consisting of.”

[0031] As used herein, the term “about” refers to a ±10% variation from the nominal value. It is to be understood that such a variation is always included in any given value provided herein, whether or not specifically referred to.

[0032] As used herein, the term “Eh” refers to a measure of the redox (oxidation-reduction) state of a solution or, more exactly, its solutes.

[0033] One aspect of the invention pertains to a solution for leaching a metal-containing material. In some embodiments, the leach solution comprises glycine and a reducing agent.

[0034] Glycine (NH2CH2COOH) has two pKa values, 2.34 and 9.60, because of the presence of an amino group and a carboxyl group (Smith and Martell, 1989). Protonation of the amino group in glycine happens under acidic conditions, forming a cationic species ^NF^CF^COOFl). A zwitterionic species ^NF^CF^COO ) dominates in the pH region from 4 to 8 with the deprotonation in the carboxyl group. At alkaline pH, deprotonation of glycine forms an anionic species (NH2CH2COO ). Speciation of glycine in an aqueous solution as a function of pH is shown in FIG. 1.

[0035] Glycine can form coordination compounds with some metal ions over a pH range of 2- 11. The speciation of metal-glycinate is dependent on solution pH, oxidation status of metal ion, and metal ion concentration (Borsook and Thimann, 1932; Keefer, 1948; Prasad and Prasad, 2009).

[0036] Stability constants of some metal-glycinate complexes are listed in Table 1 (Angkawijaya et ak, 2012; Azadi et al., 2019; Lotfi et ah, 2009). Stability constant can be calculated by thermodynamic data indicating potentials of metal dissolution. These metals listed here can be complexed with glycine in the solution so it can be used to metal extraction/recovery process.

TABLE 1. Equilibrium stability constants of metal ions with glycine at standard state. Metal logPi logP2 logP3

Cu ²⁺ 8.26 15.15 17.24

Cu ⁺ 6.75 10.00

M ²⁺ 5.83 10.70 13.92

Co ²⁺ 4.82 8.74 11.63

Mn ²⁺ 3.01 5.00 5.70

Zn ²⁺ 5.10 9.40 11.59

Cd ²⁺ 4.40 7.84 10.31 p _b ² + 5.18 8.44 p _d ² + 9.12 17.55

Fe ²⁺ 4.02 6.65

Ag ⁺ 3.43 6.71

Au ³⁺ 7.05 10.57

Au ⁺ 16.70

[0037] In some embodiments of the present invention, the leach solution includes a reducing agent. Inclusion of a reducing agent can enhance the ability to leach metal(s) from a metal- containing material. A variety of reducing agents have been investigated, paired with different acids to leach cathode materials of LIBs. For example, the utilization of H ₂ 0 ₂ can improve leaching efficiency without introducing extra ions into leaching systems. However, at elevated temperatures the decomposition of H ₂ 0 ₂ increases, leading to higher reagent consumption. Moreover, the oxidative degradation of some organic acids (e.g., ascorbic acid) by ¾(¾ was reportedly detrimental for metal extraction (Deutsch, 1998). [0038] In some embodiments of the present invention, the reducing agent is included to enhance the leaching of metal-containing materials, including the L1C0O2 commonly used in cathodes of LIBs. Cobalt exists as Co(III) in the L1C0O2 crystal structure, which has been difficult to leach. In a leaching process without a reducing agent, C03O4 may be formed as an intermediate oxide, which is not readily soluble (Musariri et al., 2019). The chemical bonds in the L1C0O2 crystal become weaker after Co (III) is reduced, and Co (II) can then be dissolved in an aqueous solution more readily. [0039] Sodium metabisulfite (SMB, Na2S2C>5) exhibits a reducing ability, and it is commonly used as a preservative in food and pharmaceutical industries (Ahmadi et al., 2018). In gold leaching, it is also used as an inhibitor for thiosulfate oxidation to minimize reagent loss (Fleming et al., 2000). SMB is also available commercially in industrial scale. The present disclosure describes a valuable metal extraction from L1C0O2 powder in a leaching system of glycine and sodium metabisulfite (glycine-SMB), where glycine serves as a lixiviant and SMB is a reducing agent. Preferred conditions were studied, and a leaching mechanism was also proposed.

[0040] One aspect of the invention pertains to a method of leaching a metal-containing material (e.g., ore, concentrate, etc.), the method comprising: a) forming a leach solution by dissolving at least one amino acid (e.g., glycine, histidine and/or lysine)-and a reducing agent (e.g. sodium metabisulfite (SMB)) in water; b) forming a mixture of the leach solution of step (a) and a metal-containing material; c) leaching at least one metal from the metal-containing material by heating the mixture of step (b) in a temperature range from about 20 °C to about 100 °C or about 10 °C to about 95 °C.

[0041] In some embodiments, the metal-containing material comprises LiCoC^.

[0042] In some embodiments, the metal-containing material comprises one or more lithium compounds.

[0043] In some embodiments, the at least one metal leached from the metal-containing material comprises lithium, cobalt, manganese or nickel (e.g., for battery recycling, using the present invention the metals leached may be manganese and/or nickel).

[0044] In some embodiments, wherein the at least one amino acid is chosen from glycine, histidine and lysine.

[0045] In some embodiments, the concentration of the glycine in the leach solution is in a range from about 0.01M to about 2.0M, or from about 0.3 M to about 1.5 M, or even about 0.5 M.

[0046] In some embodiments, the reducing agent is sodium metabisulfite.

[0047] In some embodiments, the concentration of the sodium metabisulfite in the leach solution is in a range from about 0.1M to about 2.0 M, or from about 0.1 M to about 1.0 M, or even about 0.5 M. [0048] In some embodiments, said method further comprises adjusting the pH of the leach solution to a pH from about 1 to about 14, or from about 3 to about 7, or even from about 4.5 to 5.5.

[0049] In some embodiments, the metal-containing material is leached for a duration of about 10 minutes to about 180 minutes, or about 1 hour to about 96 hours.

[0050] In some embodiments, the said metal-containing material is an ore or concentrate. [0051] Another aspect of the invention is a method of recovering metal from a spent lithium- ion battery cathode, the method comprising: a) separating the cathode components comprising separating an aluminum foil in the cathode from a lithium containing material (e.g. material containing LiCoC ) to recover said one or more lithium containing material (such as a material comprising L1C0O2); b) forming a leach solution by dissolving an amino acid (e.g. glycine) and a reducing agent (e.g. sodium metabi sulfite) in water; c) forming a mixture of the leach solution of step (b) and lithium containing material (such as L1C0O2) from step (a); d) leaching lithium and/or cobalt from the lithium containing material by heating the mixture of step (c) in a temperature range from about 20°C to about 100°C.

[0052] In some embodiments, the separating in step (a) comprises physical separating using a method comprising crushing, milling, and/or air/gravity separation and collecting the resulting or separated lithium containing material (e.g. L1C0O2).

[0053] In some embodiments, said temperature range is from about 10°C to about 95 °C. [0054] A further aspect the invention, a method for leaching nickel and/or manganese from used batteries, the method comprising: a) separating a nickel and/or manganese containing material from one or more used batteries; b) forming a leach solution by dissolving at least one amino acid and a reducing agent in water; c) forming a mixture of the leach solution of step (b) and a metal-containing material; d) leaching at least nickel and/or manganese from the metal-containing material by heating the mixture of step (c) in a temperature range from about 20 °C to about 100 °C or about 10 °C to about 95 °C. wherein said at least one amino acid is chosen from glycine, histidine and lysine.

[0055] In some embodiments, said a reducing agent is sodium metabisulfite (SMB).

[0056] In some embodiments, said temperature range is from about 10 °C to about 95 °C.

[0057] In some embodiments, the metal-containing material comprises one or more nickel compounds and/or one or more manganese compounds.

LIST OF EMBODIMENTS

[0058] The following is a non-limiting list of embodiments of the present invention:

[0059] Embodiment 1. A method of leaching a metal-containing material (e.g., ore, concentrate, etc.), the method comprising:

(a) forming a leach solution by dissolving at least one amino acid (e.g., glycine, histidine and/or lysine) and a reducing agent (e.g., sodium metabisulfite (SMB)) in water;

(b) forming a mixture of the leach solution of step (a) and a metal-containing material;

(c) leaching at least one metal from the metal-containing material by heating the mixture of step (b) in a temperature range from about 20 °C to about 100 °C or about 10 °C to about 95 °C.

[0060] Embodiment 2. The method of embodiment 1, wherein the metal-containing material comprises LiCoCh.

[0061] Embodiment 3. The method of embodiment 1, wherein the at least one metal leached from the metal-containing material comprises lithium, cobalt, manganese or nickel (e.g, for battery recycling, using the present invention the metals leached may be manganese and/or nickel).

[0062] Embodiment 4. The method of embodiment 1, wherein a concentration of the glycine in the leach solution is in a range from about 0.01M to about 2.0M or from about 0.3 M to about 1.5 M.

[0063] Embodiment 5. The method of embodiment 1, wherein a concentration of the sodium metabisulfite in the leach solution is in a range from about 0.1M to about 2.0M or from about 0.1 M to about 1.0 M.

[0064] Embodiment 6. The method of embodiment 1, further comprising adjusting the pH of the leach solution to a pH from about 1 to about 14 (e.g., a pH of about 5). [0065] Embodiment 7. The method of embodiment 1, wherein the metal-containing material is leached for a duration of about 10 minutes to about 180 minutes, or about 1 hour to about 96 hours.

[0066] Embodiment 8. A method of recovering metal from a spent lithium-ion battery cathode, the method comprising:

(a) separating the cathode components by one or more steps of removing adhesive used to adhere LiCoCE to an aluminum foil in the cathode (or in other words step (a) comprises separating the aluminum foil from LiCoCE to recover said LiCoCE);

(b) forming a leach solution by dissolving glycine and sodium metabisulfite in water;

(c) forming a mixture of the leach solution of step (b) and LiCoCE from step

(a);

(d) leaching at least one metal from the metal-containing material by heating the mixture of step (c) in a temperature range from about 20 °C to about 100 °C.

[0067] Embodiment 9. The method of embodiment 8, wherein the separating in step (a) comprises physical separating using a method comprising crushing, milling, and/or air/gravity separation and collecting resulting or separated LiCoCE.

[0068] In some embodiments of the present disclosure, the temperature of the leaching is in a range of from about 20 °C to about 100 °C, or from about 10 °C to about 95 °C, or even about 80 °C.

[0069] In some embodiments of the present disclosure, the pH of the leaching solution is at least about 2, at least about 3, at least about 4, at least, about 5, at least about 6, and even at least about 7. In some embodiments, the pH of the leaching solution is in a range of from about 3 to about 7, from about 4 to about 6, and even from about 4.5 to about 5.5. In some embodiments, the pH of the leaching solution is about 5.

[0070] In some embodiments of the present disclosure, the concentration of glycine is in a range from about 0.01M to about 2.0M.

[0071] In some embodiments of the present disclosure, the concentration of reducing agent is from about 0.1M to about 2.0M.

[0072] In some embodiments of the present disclosure, the duration of leching the metal- containing material is in a range from about 1 hour to 96 hours. [0073] It is to be understood that both the foregoing general description of the invention and the following detailed description are exemplary, and thus do not restrict the scope of the invention.

EXAMPLES

[0074] Materials

[0075] The reagent grade lithium cobalt(III) oxide powder (LiCo0 ₂ , 97% purity, Alfa Aesar,

USA) was used as a raw material for the study. The composition was analyzed by X-ray powder diffraction (XRD), and the result can be seen in FIG. 2. The XRD pattern was in good agreement with the JCPDS card (No. 01-075-0532) of LiCo0 _2.

[0076] Leaching experiments were conducted in a beaker with a watch glass cover to prevent the evaporative loss of solution. First, the leaching solution was made by adding specific amounts of chemical reagents to deionized water, and heating to 80°C using a hot plate. When the temperature reached a set point, 2.0 g L1C0O2 powder sample was added into the solution, along with additional deionized water to bring the solution volume to 100 mL. During the test, 5 mL kinetic samples at 45, 90, and 180 minutes were taken using a syringe filter with 0.45 micrometer pore size. Meanwhile, pH and oxidation-reduction potential (ORP) value were recorded. The kinetic samples were assayed by Atomic Absorption Spectrophotometer (AAS, PinAAcle 500, Perkin-Elmer, USA) for cobalt and lithium concentrations. After leaching tests, residues were filtered, washed three times using deionized water, and dried at the ambient atmosphere for further analysis. Co and Li recoveries were calculated using Equation (1): where R is the recovery of Co or Li (%); c is the concentration of metal ions in solution (g/L); V is the volume of leaching solution (L); m is the weight of L1C0O2 used in the test (g); w is Co or Li content in L1C0O2 powder. The cumulative recovery was calculated at leaching times of 90 minutes and 180 minutes.

[0077] Material characterization [0078] L1C0O2 powders were characterized before and after leaching in the glycine-SMB system, using X-ray photoelectron spectroscopy (XPS) and scanning electron microscope (SEM) techniques. XPS measurements were carried out with a Kratos Axis 165 Ultra spectrometer using a focused monochromatized A1 Ka radiation (1486.6 eV). All spectra were calibrated using the C Is peak at 284.8 eV. Core peaks were analyzed using a nonlinear Shirley-type background. The high-resolution XPS spectra were analyzed using a peak-fit program with Gaussian-Lorentzian sum function. The morphology analysis was conducted by SEM with energy dispersive X-ray microanalysis (SEM-EDS, Hitachi S- 4800).

[0079] Leaching Study

[0080] Effect of Reductant Concentration

[0081] The effect of Na2S2C>5 concentration was studied at a glycine concentration of 0.5 M.

The results Co and Li recovery are shown in FIGS. 3A and 3B, respectively.

[0082] Co and Li recovery were strongly affected by the concentration of Na2S205 at 80°C.

When Na2S205 concentration increased from 0.1 M to 0.5 M, Co extraction increased from 46.3% to 99.2% and Li recovery grew from 29.0% to 95.7% after 180 min. However, a further increase of Na2S2C>5 concentration to 1.0 M did not improve the L1C0O2 dissolution. Although faster kinetics were observed, Co extraction decreased by 1.6% from 90 min to 180 min. Similarly, an apparent drop of Li concentration in leachate was also observed from 90 min to 180 min. After the leaching test, a brown precipitate was found, which was analyzed and discussed in the following sections. From this study, a preferred Na2S205 concentration was found to be 0.5 M.

[0083] Li recovery and leaching kinetics were lower than those of Co with 0.1 M Na2S205, but improvement was observed with higher Na2S205 concentration. For example, when using 0.5 M Na2S2C>5, similar leaching kinetics of Co and Li were obtained. The results were consistent with needing the reduction of Co (III) and release of Co from L1C0O2 crystal structure in order to obtain Li dissolution, while Li did not need to be reduced. The slow leaching kinetics of Li in organic acid leaching systems can also be found in published literature, implying that the leaching of Li may be affected by solution chemistry (Fu et ak, 2019; Li et ak, 2015; Nayaka et ak, 2016a).

[0084] Effect of Glycine Concentration [0085] FIGS. 4A and 4B illustrate the leaching behavior of L1C0O2 using 0.5 M Na2S2C>5 with various glycine concentrations, with FIG. 4A showing the results for Co and FIG. 4B showing the results for Li. Cobalt leaching kinetics and overall recovery improved when glycine concentration increased from 0.3 M to 0.5 M. Meanwhile, lithium leaching kinetics were faster with 0.5 M glycine, but the ultimate Li recoveries were about the same after 180 min, around 95%. Higher levels of glycine (e.g.,1.0 M and 1.5 M) resulted in decreased Co and Li leaching kinetics and the recovery to different extents. This is possibly due to high ionic strength of the leaching solution. In theory, higher ionic strengths resulted in not only lowering the ionic mobility and thus hindered mass transfer but also possibly the precipitation formation in the leaching solution (Bahga et ak, 2010). On the other hand, higher glycine dosages than stoichiometric amount were observed to only contributed to a product with a higher glycine/metal ratio, rather than accelerating the leaching speed. A glycine concentration of 0.5 M was therefore selected for leaching studies.

[0086] Effect of Solid/Liquid Ratio

[0087] The effect of solid/liquid ratio was tested with the following conditions: 0.5 M glycine, 0.5 M Na2S2C>5, 180 min leaching time, and a temperature of 80°C. Co and Li leaching recovery and concentration in leachate with various S/L ratios were as shown in FIGS. 5A and 5B. At higher S/L ratios, there was a decrease in metal recovery. Co and Li leaching recoveries were above 95% when S/L ratio was less than 30 g/L. The highest Co and Li leaching recovery was observed with the S/L ratio of 20 g/L.

[0088] The molar (M) concentrations of Co and Li in leachate were almost equivalent under the same conditions, (i.e, 0.5M glycine and 0.5M SMB) indicating that they were dissolved from L1C0O2 in the atomic ratio of about 1:1. The soluble Co and Li species increased with

S/L ratio and reached a plateau of 0.36 M with an S/L ratio of 50 g/L. Under these conditions, the cobalt-glycinate complex was possibly Co2( H2CH2COO)3 (Borsook and

Thimann, 1932). Accordingly, the decrease of metal extraction at high S/L ratios was possibly due to a depleted level of leaching reagents.

[0089] Effect of Temperature

[0090] To gain further insights into the L1C0O2 dissolution behavior at different temperatures in the glycine-SMB system, tests were conducted using 0.5 M glycine and 0.5 MNa2S2C>5 at temperatures in of range from 20°C to 80°C. The resulting Co and Li leaching behavior at different temperatures is illustrated in FIGS. 6 A and 6B. [0091] As shown in FIGS. 6 A and 6B, an increase in temperature accelerated L1C0O2 dissolution in the glycine-SMB leaching system, which can be seen from the increased leaching kinetics and recovery for Co (FIG. 6A) and Li (FIG. 6B). At temperatures below 65°C, Co and Li recovery increased steadily with leaching time. Co and Li extraction still showed an upward trend after 180 min. It is believed that the dissolution of L1C0O2 at low temperatures was a slow process (not ceased within 3 hours). The highest leaching kinetics and recovery were observed at 80°C.

[0092] Leaching Kinetics

[0093] Making an assuming that L1C0O2 powders are spherical particles and the unreacted core shrinks during leaching, a shrinking core model was applied to explain the leaching mechanism, as shown in Eqs. (2)-(4) (Levenspiel, 1999). Equation (2) represents a surface chemical reaction-controlled model, Eqs. (3) and (4) are expressions for product layer diffusion and boundary layer diffusion limited models, respectively.

1 — (1 — x)7 = kt (2)

1 — (1 — x)3 = kt (4) where: x is fraction reacted (metal recovery), A: is rate constant (min ¹ ), t is leaching time (min). The leaching rate constants and the coefficients of determination from these three models for Co and Li leaching are shown in Tables 2 and 3, respectively.

TABLE 2. Fitting parameters of shrinking core model for Co leaching Surface chemical reaction Diffusion through Diffusion through t/° control product layer boundary layer

20 0.349 0.987 0.021 0.963 0.675 0.985

35 0.779 0.998 0.101 0.926 1.447 0.997

50 1.948 0.998 0.523 0.962 3.226 0.990

65 4.167 0.982 1.415 0.980 6.297 0.952

80 10.452 0.994 2.569 0.901 17.684 0.999

TABLE 3. Fitting parameters of shrinking core model for Li leaching Surface chemical reaction Diffusion through Diffusion through

T/° control product layer boundary layer

20 0.317 0.950 0.017 0.983 0.616 0.947

35 0.658 0.981 0.072 0.982 1.239 0.976

50 1.274 0.968 0.198 0.938 2.327 0.964

65 3.204 0.980 0.775 0.986 5.457 0.970

80 5.379 0.978 0.835 0.988 9.816 0.970

[0094] By comparing these three models, the chemical reaction control model fitted the Co leaching results well, with high coefficients of determination, suggesting the surface chemical reaction of Co (III) reduction by Na2S2C>5 may govern the cobalt dissolution. For

Li leaching, higher correlation coefficients were found in models of the surface chemical reaction control and the diffusion through the product layer. In the present study, there was no presence of impurities such as organic binders accumulating on the L1C0O2 surface to limit diffusion, since high purity synthetic L1C0O2 powder was used as raw material

(Musariri et al., 2019). Also, Co-glycinate diffusion from particle surface to solution bulk was a rapid step. Therefore, a product layer was not likely to be formed, and the Li leaching was mainly limited by surface chemical reaction, consistent with a reductive dissolution of Co facilitating Li dissolution from L1C0O2 crystal.

[0095] The relationship between reaction rate constant and temperature can be described by Arrhenius law, shown as Equation (5). Equation (6) is the logarithm form. k = Ae ^Ea / ^RT (5)

Ink (6) ⁷ where k is the reaction constant (h ¹ ), A is the frequency factor, 77, i s the apparent activation energy (kJ/mol), R is the universal gas constant (8.314 J/K/mol), and T is the absolute temperature (K).

[0096] Using the rate constants calculated from the surface chemical reaction-controlled model listed in Tables 2 and 3, the Arrhenius plots of Co and Li were constructed, with results as shown in FIG. 7. A good linear relationship (i.e., a good linear relationship with R-square values of 0.9931 and 0.9937 for Co and Li, respectively) was found between In k and 1/T. The apparent activation energies of Co and Li dissolution from L1C0O2 were determined to be 48.05 kJ/mol and 41.51 kJ/mol, respectively. The high activation energy confirmed the metal ion extraction from L1C0O2 using glycine and SMB was controlled by surface chemical reaction.

[0097] Microanalytical Characterization

[0098] To confirm the leaching results and determine the composition of the precipitates formed during the leaching experiments, microanalysis using XPS and SEM were performed on the LiCo02 pristine sample and two selected experimental residues. The sample information is listed in Table 4. LiCo02 powder without any treatment is labeled as SI; residues of leaching tests using 0.5 M glycine and 0.3 and 1.0 M Na2S2C>5 were S2 and S3, respectively. It should be noted that there was no detectable leaching residue using 0.5 glycine and 0.5 M Na2S205 since L1C0O2 was fully dissolved into leaching solution.

Sample S2 is a black residue while sample S3 is a brownish powder; their compositions and morphologies were as determined here.

TABLE 4. Sample information for XPS analysis

No. Sample Condition

SI L1C0O2 powder Without treatment

S2 residue 0.5 M glycine and 0.3 M Na2S2C>5

S3 residue 0.5 M glycine and 1.0 M Na2S2C>5

[0099] XPS analysis

[0100] FIG. 8 A display the Co 2p and O ls core peaks of the three samples SI -S3. Due to the spin-orbit coupling, the Co 2p spectrum is split into two parts (2p _3/2 and 2pi _/2 ) with an intensity ratio close to 2: 1. Similar Co 2p spectra were observed in sample S 1 and S2 with binding energies of Co 2p _3/2 and 2pi _/2 near 780 and 795 eV, respectively, indicating the existence of cobalt in the two samples was the same, from L1C0O2 crystal structure (cf.

Guan et al., 2016; van Elp et al., 1991). The chemical state of cobalt can be determined by satellite peak. The absence of satellite peak at 786 eV showed it is Co (III) in L1C0O2 crystal. A significant decrease of Co 2p intensity was detected in sample S3, suggesting the cobalt content in the residue was lower than sample SI and S2. On the other hand, the Co 2p _3/2 peaked at around 781.5 eV, showing the valence of cobalt in the residue was +2 (Chen et al., 2016).

[0101] The O ls spectra and peak fitting results of the three samples were as shown in FIG. 8B. The binding energy of O Is at 529.5 eV in sample SI and S2 is characteristic of the lattice oxygen from L1C0O2, in good agreement with the literature (van Elp et al., 1991).

Another peak at 531.2 ± 0.1 eV can be attributed to carbonate and hydroxide species, indicating the surface contamination by water, CO2, hydroxide species, or surface defects

(Dahe'ron et al., 2009; Han et al., 2015). Water molecule absorbed on L1C0O2 surface was also found due to the peaks at -533 eV (Weidler et al., 2016). In sample S3, O Is peak at 529.5 eV was disappeared, indicating the metal oxide structure of L1C0O2 was destructed. The three peaks detected were at higher binding energies of 531.0 eV, 532.0 eV, and 535.4 eV. The first two peaks can be assigned as carbonate or hydroxide and organic C=0 bond, respectively (Zhang et al., 2014). The peak at 535.4 eV is caused by the sodium Auger peak considering the high sodium concentration in leaching solution may evolved in the precipitation process. Therefore, it was deduced that sample S2 was mainly undissolved L1C0O2 powder while sample S3 was a precipitate with a complex composition.

[0102] SEM characterization

[0103] SEM images of the original LiCo02 powder (sample SI) and leaching residue of 0.5 M glycine and 0.3 M Na2S205 (sample S2) are shown in FIGS. 9A and 9B, respectively. In FIG. 9A, the raw material of LiCo02 powder showed a larger particle size of 4-6 micrometers with a smooth surface. The LiCo02 crystal structure was damaged by glycine and Na2S2C>5 during leaching, and a significant reduction of size was found in sample S2, as shown in FIG. 9B. Moreover, the smooth semi -spherical surface was reduced, and sharp edges were also observed from the particles. From XPS analysis results, it is undissolved L1C0O2 particles.

[0104] An SEM image and EDS mapping of the residue leached by 0.5 M glycine and 1.0 M Na2S205 (sample S3) was obtained. In contrast to the leaching residue with low concentration, a different morphology of sample S3 was observed. Cubic-shaped particles around 5 micrometers and some smaller irregular particles were seen at the magnification shown in FIG. 10. FIG. 11 A shows a higher magnification SEM of the particles, and FIGS. 1 IB-1 IF show element mapping of the same particles for the elements Co, O, S, Na and C, respectively. The EDS analysis showed that Co (FIG. 1 IB) and S (FIG. 11C) were evenly distributed in the residue. The element maps for O (FIG. 1 ID) and Na (FIG. 1 IE) were overlapped and especially enriched in the areas of irregular particles, indicating the residue consisted of different compositions. The cubic particle was further analyzed by EDS area mapping (inset area of FIG. 12A) and the element composition is summarized in FIG. 12B. The elements Co and S were in an atomic ratio of 1:1, suggesting that the cubic-shaped particle might be C0SO4, given that oxygen was underestimated in EDS analysis.

[0105] It may be worth noting that the detection of lithium may have been unsuccessful because its characteristic radiation is very low. But according to leaching results, the precipitate also contained Li and its recovery dropped from 90 min to 180 min, as was shown in FIG. 3B. Without wishing to limit the invention to a particular theory or mechanism, lithium extraction in FIG. 3B decreased possibly because of the precipitation of lithium in the solution. Thus, the residue was possibly a coprecipitation of sulfate salts of Co, Li, and Na.

[0106] During the leaching process, solution pH and oxidation-reduction potential (ORP) were recorded, with results as shown in FIG. 13. Additionally, the pH-Eh diagrams of Co and Li in the glycine-SMB leaching system at 25°C and 80°C were computed using the EPH MODULE OF HSC CHEMISTRY 9 software, with results displayed in FIG. 14A (for Co) and FIG. 14B (for Li). Glycine and Na2S205 concentrations were both set at 0.5 M, and the Co ²⁺ and Li ⁺ concentrations were 0.2 M, corresponding to an S/L ratio of 20 g/L. [0107] During L1C0O2 leaching using glycine and SMB, the solution pH fluctuated between

4.5 and 5.3 and ORP was between 0.2 V and 0.3 V vs. SHE. In this pH range, the neutral form of glycine ( ⁺ H3CH2COO ) dominates. Zwitterionic glycine is reported to chelate with metal ions, but in very limited conditions (Keefer, 1948). According to a previous study, deprotonation of zwitterion glycine is a rapid step in the presence of high metal ion concentration (Pearlmutter and Stuehr, 1968). Therefore, it is supposed that CO( H2CH2COO)2 complexed by Co (II) and anionic glycine may be the dominant species in the leachate, although various cobalt-glycinate complexes may present.

[0108] In the Co-Li-glycine-SMB system, Co( H2CH2COO)2 was stable at pH 4-9 in a relative wide Eh range. Its stable region moved towards the lower pH direction at a higher temperature. Cobalt sulfate and free Co ion dominate the low pH region, where inorganic acid leaching is typically conducted. Cobalt is known to precipitate as Co(OH)2 in an alkaline environment, which is why cobalt leaching using glycine is not conducted under alkaline solutions of copper and gold. Lithium ion tends not to form a complex with glycine, thus free Li ⁺ is the dominant species in a wide pH and Eh range except strong alkaline conditions. Meanwhile, it has been acknowledged that partially hydrated lithium ion can complex with glycine (Remko and Rode, 2006). Based on the above discussion, the reaction of LiCo0 ₂ dissolution in the glycine-SMB system is proposed as Equation (7).

4 LiCo0 ₂ + 8NH ₂ CH ₂ COOH+ Na ₂ S ₂ 0 ₅

2Li ₂ S0 ₄ + 4CO(NH ₂ CH ₂ COO) ₂ + 2NaOH + 3H ₂ 0 (7)

[0109] Besides the main reaction, a series of reactions may happen after SMB is dissolved in aqueous solution, as illustrated in Equations (8)-(ll) (Irwin, 2011). Sodium bisulfite (NaHSC^) is produced once Na ₂ S ₂ 05 dissolved in solution, and it may be further decomposed to produce S0 ₂ at high temperatures. Meanwhile, Na ₂ S ₂ 05 may also be decomposed to Na ₂ S03 and S0 ₂ when the solution is heated. A portion of S0 ₂ dissolves and reacts with water to form H ₂ S03 and then dissociates to generate HSO3 , which also shows reducing ability. These equations are the reason for high Na ₂ S ₂ 05 demand in the leaching process.

H ₂ O + Na ₂ S ₂ 0 ₅ 2 NaHS0 ₃ (8)

2NaHS0 ₃ Na ₂ S0 ₃ + H ₂ 0 + S0 ₂ (9)

Na ₂ S ₂ 0 ₅ Na ₂ S0 ₃ + S0 ₂ (10)

S0 ₂ + H ₂ 0 H ₂ S0 ₃ HS0 ₃ - + H ⁺ (11)

[0110] Overall, the dissolution of LiCo0 ₂ in the glycine-SMB system can be described as follows. Na ₂ S ₂ 05 attacks the LiCo0 ₂ crystal structure and reduces Co (III) to Co (II).

Crystal defects appear after Co (II) was released to aqueous solution. Meanwhile, Li ion is also dissolved. Co (II) in solution is stabilized by glycine anion to form CO(NH ₂ CH ₂ COO) _2.

[0111] A distinct advantage of the leaching system lies in the mildly acidic leaching pH. The solution pH was near 5, which is higher than other organic acid leaching conditions previous studies using organic acids as lixiviants, a relatively high acid concentration needs to be maintained to achieve high leaching efficiency because organic acid works as both proton provider and complexing agent (Fu et ah, 2019; Li et ah, 2015; Nayaka et ah, 2016b). Glycine has a lower pK _ai (2.34) value compared with organic acids such as acetic acid (4.76), ascorbic acid (4.17), malic acid (3.40), tartaric acid (3.03) and citric acid (2.79). However, in this test, glycine just works as a chelating agent and does not release hydrogen ion to attack L1C0O2 crystal (Golmohammadzadeh et ah, 2018). On the other hand, fast leaching kinetics and high metal recovery can be achieved using a near stoichiometric amount of glycine in the glycine-SMB leaching system. Glycine was fully utilized by dissolved metal ions to form metal-glycinate complex.

[0112] The present disclosure includes embodiments of a method for recovering metal from a spent lithium-ion battery. In many instances, the cathode in spent LIBs includes L1C0O2 adhered to an aluminum foil with an adhesive. It is desirable to separate the L1C0O2 from the aluminum foil prior to leaching the L1C0O2 for recovery of Co and Li. Hence, the method includes removing the removing the adhesive.

[0113] In some embodiments, removal of the adhesive from the LIB cathode includes physical breaking of the adhesive followed by air-separation or gravity separation.

[0114] By way of summary, Cobalt and lithium were extracted from L1C0O2 by glycine with the aid of Na2S205 as a reducing agent at 80°C. Preferred operating conditions were: 0.5 M glycine, 0.5 MNa2S205, 20 g/L S/L ratio, at 80°C for 180 min; the Co and Li recoveries obtained were 99.2% and 95.7% respectively. A shrinking core model was used to describe the dissolution process, and the apparent activation energies of Co and Li were 48.05 kJ/mol and 41.51 kJ/mol. Therefore, the controlling mechanism of the dissolution reaction was possibly a surface chemical reaction. XPS and SEM microanalytical characterizations of L1C0O2 before and after leaching showed that it was not fully dissolved using low Na2S205 concentrations, while higher Na2S205 concentrations caused the precipitation formation, possibly due to high ionic strength of the solution.

[0115] In some embodiments according to the present disclosure, the glycine-SMB leaching system for L1C0O2 dissolution was used under a mildly acidic environment at pH near 5. Glycine was utilized to form a metal-glycinate complex with high efficiency. Thus, the low reagent demands and near-neutral leaching condition in this leaching system as compared with other studies potentially offer an economic alternative to treat cathode material of spent lithium ion batteries. REFERENCES

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