Process for recovering lithium chloride from industrial solid waste

Abstract

Process for recovering lithium as lithium chloride, which is present in the industrial solid waste generated in the production of lithium carbonate. The process involves leaching the industrial solid waste by means of leaching in which an ion exchange is generated using calcium and / or magnesium. The leaching process can be carried out in different types of operations: reactors, pans and leaching heaps.

Description

[0001] PROCESS FOR RECOVERING LITHIUM-RICH BRINES FROM INDUSTRIAL SOLID WASTE PREVIOUS ARTWORK

[0002] The production process for obtaining lithium begins with lithium chloride (LiCl) brine obtained from the salt flat as a byproduct of potassium chloride production.

[0003] The L1 in brine concentrates inside the ponds, where different salts precipitate. The main solids precipitated in this system are: balite (NaCl), sylvinite (NaCl-KCl), sylvite (KCl), potassium carnallite (KClMgCl2-6H2O), and bischofite (MgCl2-6H2O).

[0004] As a result of the salting process, a shipping brine is obtained, which is concentrated at approximately 3-7% LiCl or 25-38% LiCl. This is subsequently sent for purification and conversion to lithium carbonate (Li2CO3), involving solvent extraction (SX), impurity precipitation, carbonation, drying, and Li2CO3 packaging.

[0005] The chemical plant generates various solid industrial wastes (SIWW), some of which have the potential to be treated through a leaching process to recover lithium.

[0006] Document WO2010006366 describes a process for recovering lithium from an impure natural or industrial brine. The process comprises:

[0007] (i) adjust the pH of a lithium-containing feed brine to a value not less than 11.3; (ii) separate the solid waste and a solution containing lithium values.

[0008] The solution can be concentrated and treated to obtain lithium carbonate and a lithium chloride solution, which is suitable for obtaining electrolytic grade lithium chloride.

[0009] The method also includes:

[0010] (i) obtaining crude lithium carbonate from brine by precipitating the solid by adding a soluble carbonate and separating the solid, and redissolving and precipitating the crude lithium carbonate to produce high-purity lithium carbonate and separating the solid.

[0011] (i) prepare a lithium chloride solution from lithium carbonate.

[0012] While this document describes the production of lithium chloride, it fails to mention that it is generated from a solid waste product derived from lithium carbonate production, nor that magnesium chloride is added to the solution. This omission fails to account for the generation of a solid waste product from which lithium can be recovered through a leaching process. Furthermore, neither CaCl2 nor MgCl2 is used in the process in any of its technical grades.

[0013] Document EP3800163 (equivalent to document CL202002454) describes a method for producing lithium hydroxide monohydrate from lithium-containing brines and is characterized in that the method includes: (i) filtering impurities from the lithium-containing brine components to form a brine with an abundant lithium content,

[0014] (i) sorption separation of the primary lithium concentrate and lithium-rich brine in sorption-desorption columns with a fixed bed of a granular sorbent selective for LiCl in the form of an aqueous solution,

[0015] (iii) decarbonization of the primary lithium concentrate through acidification,

[0016] (iv) nanofiltration of the decarbonized primary lithium concentrate for the non-reactive purification of magnesium, calcium and sulfate ions, (v) reverse osmosis concentration of the primary lithium concentrate purified by nanofiltration to obtain a permeate stream in the form of a demineralized aqueous solution and a reverse osmosis lithium chloride concentrate stream,

[0017] (vi) Concentration of the lithium chloride concentrate by reverse osmosis using electrodialysis to obtain a flow of the dialyzed product containing lithium and a flow of lithium chloride concentrate subjected to electrodialysis,

[0018] (vii) chemical purification of calcium, magnesium and sulfate ions from the lithium chloride concentrate subjected to electrodialysis,

[0019] (viii) ion exchange purification of chemically purified electrodialytic lithium chloride concentrate, (ix) boiling of electrodialytic lithium chloride concentrate purified by ion exchange with salt and separation of sodium chloride and potassium chloride crystals, (x) production of a solution with abundant lithium chloride content by diluting the boiling lithium chloride concentrate with demineralized water,

[0020] (x¡) electrochemical conversion by membrane electrolysis of the solution with an abundant lithium chloride content to produce cathodic hydrogen, anodic chlorine and an aqueous solution of lithium hydroxide as the catholyte,

[0021] (xii) boiling of the LiOH solution,

[0022] (xiii) crystallization of LiOH H2O from the boiled LiOH solution. The method also comprises mixing the residual stream obtained in step (iv) of the reverse osmosis concentration, enriched with magnesium and calcium, with brine containing abundant lithium.

[0023] This document does not teach the dissolution of magnesium chloride in the solid residue from the lithium carbonate production process, considers the use of reverse osmosis and electrodialysis processes to purify brine and obtain lithium hydroxide as a product, and does not use waste streams to recover Li by means of exchange with Ca / Mg. Document WO2018190754 (equivalent to document CL201800938) describes an industrial method for preparing lithium concentrate from natural brines containing lithium.

[0024] The brine is first subjected to purification of suspended solids, then filtered through a static layer of granulated solvent based on the compound LiCl 2Al(OH)3 mH2O (DGAL-Cl) to obtain a primary lithium concentrate.

[0025] The process is carried out in sorption-desorption units consisting of four columns. Two columns are constantly sorbing lithium chloride from the brine. Another column is washing the adsorbent from the brine, and the other column is constantly desorbing LiCl.

[0026] The operating sequence of the columns is automatically determined following the developed cycle diagram. The primary lithium concentrate obtained is converted into secondary lithium concentrate when one of the alternatives is followed. According to the first alternative, the primary lithium concentrate is transported to the evaporation tanks, where the calcium and magnesium mixtures are also purified. This is done using lithium carbonate pulp after its carbonization, yielding a precipitate composed of CaCO3 + 3MgCO3 → Mg(OH)2·3H2O. After the separation of the calcium and magnesium salt precipitate, the secondary lithium concentrate is brought to a LiCl concentration of 190–200 kg / m³ 3 The method comprises:

[0027] (i) that the amount of lithium carbonate by weight is repulped, the pulp is carbonized with carbon dioxide or CO2 comprising the gas mixture in the pulp circulation mode until all the lithium carbonate is dissolved, then this stream is mixed with the other primary lithium concentrate stream, the mixed solution is directed to the evaporation tank to concentrate the liquid phase with respect to LiCl, decarbonization and gradual conversion of the soluble calcium and magnesium chlorides into sparingly soluble compounds CaCO3 and Mg(OH)2*3MgCO3*3H2O, which are separated from the concentrated LiCl solution containing NaCl and KCl as main additives - secondary lithium concentrate which is then used to obtain lithium chloride or lithium carbonate.

[0028] In the second alternative, the predetermined amount of Li2CO3 by weight is repulped into the primary lithium concentrate stream obtained by reverse osmosis concentration-desalination. The pulp is carbonized with carbon dioxide (CO2) comprising a gas mixture in the pulp circulation mode until all the lithium carbonate is dissolved. The solution is heated to a temperature of 80-85°C under vacuum treatment and decarbonized. The released carbon dioxide is directed to the carbonization stage of the pulp prepared from lithium carbonate and lithium concentrate obtained by reverse osmosis. Simultaneously, CaCl and MgCl are converted into precipitates of CaCl and Mg(OH)2*3MgCO3*3H2O, which are separated from the liquid phase. This liquid phase is an aqueous solution of LiCl with NaCl and KCl mixed in. This solution is concentrated with respect to lithium chloride by electrodialysis or a heating process, or a combination of both.until a LiCl solution with a concentration of 190-200 kg / m³ is obtained, 3 corresponding to the composition of the secondary lithium concentrate, which is then used to obtain lithium chloride or lithium carbonate.

[0029] This document describes the purification of brine using sorption-desorption columns, without treating any solid residue for leaching with Ca / Mg. Carbonation of the system is performed to precipitate Ca / Mg, but the lithium carbonate solution is not mentioned, which is derived from the waste generated during lithium chloride formation. Carbonization and reverse osmosis stages are described for purifying the lithium chloride-rich brine.

[0030] Document WO2021231597 (equivalent to document CL202102989) describes a system for efficiently extracting lithium from brines by reducing lithium losses due to coprecipitation and allowing for a significantly higher lithium concentration. The system comprises:

[0031] (i) a sequence of two or more solar evaporation ponds configured to allow brine evaporation to occur in each pond and for the brine to flow from a first pond to one or more different ponds in the sequence; (ii) a conduit configured to remove at least a portion of the brine at a brine removal location and to transfer the removed brine to a separator whereby one or more impurities are separated from the lithium to form a high-impurity stream and a low-impurity stream;

[0032] (iii) wherein the high impurity stream is optionally recycled to the evaporation pond sequence at a location equal to, upstream of the brine removal location, or placed in a separate pond or reinjected underground and the low impurity stream is fed to one or more brine removal locations, to a later pond in the sequence, or to a lithium plant or concentration facility;

[0033] (iv) the location of the brine removal being positioned so that the coprecipitation of lithium together with one or more impurities is reduced compared to an amount of lithium coprecipitation that would occur in the upstream or downstream ponds in the absence of the separation system;

[0034] (v) in which the loss of lithium due to coprecipitation is reduced or eliminated.

[0035] (vi) the feed to a first pond in the pond sequence is a Chilean-type brine.

[0036] (vii) the high impurity stream is recycled to a pond that precipitates a salt selected from the group that is composed of bischofite, calcium borate, anhydrite, gypsum and carnallite or others. (viii) the low impurity stream is fed to a pond that is substantially free of L1 co-precipitated in the form of lithium carnallite and lithium metaborate or others.

[0037] (ix) The high impurity stream is recycled to a pond that precipitates a selected salt from the group consisting of bischofite, carnallite, epsomite, kainite, polyhalite, calcium borate, anhydrite, gypsum, hexahydrite, and kieserite or others.

[0038] This document does not specifically mention obtaining lithium chloride; it considers stages of lithium brine concentration through evaporation ponds with recirculation of high impurity streams to precipitate the greatest amount of unwanted species and does not consider the treatment of waste salts to dissolve present lithium and reintegrate it into a low impurity stream.

[0039] Document W02016119003 (equivalent to document CL201701910) describes a process for treating a lithium-containing material, the process comprising the following steps:

[0040] (i) prepare a process solution from the lithium-containing material;

[0041] (i) passing the process solution from step (i) through a series of impurity removal stages, one of which is an HCl bubbling step, thereby providing a substantially purified lithium chloride solution; and (iii) passing the purified lithium chloride solution from step (i) through an electrolysis stage, thereby producing a lithium hydroxide solution.

[0042] The lithium hydroxide solution produced in step (iii) is subjected to carbonation by passing compressed carbon dioxide through the solution, thereby producing a precipitate of lithium carbonate.

[0043] On the other hand, the process solution of step (i) is prepared in the form of a loaded leach solution. Preferably, the loaded leach solution is formed by passing a lithium-containing material to a leaching step in which the material is leached with hydrochloric acid.

[0044] This document does not mention the use of CaCl2 or MgCl2. It describes the purification of lithium-containing material by bubbling hydrochloric acid through it and electrolysis to obtain lithium hydroxide solution and subsequently lithium carbonate. It considers reaction steps of a material with hydrochloric acid, without specifying the use of calcium or magnesium chloride to dissolve lithium carbonate present in waste from lithium brine purification processes. The raw material for the process is not RISES but spodumene. Furthermore, the products generated are battery-grade lithium carbonate and lithium hydroxide, not LiCl brine. Document EP3589763 describes a method for producing lithium hydroxide, in particular high-purity lithium hydroxide for use in batteries and / or accumulators, from lithium-containing ores and / or minerals and / or earths using a chlor-alkali process, in which:

[0045] (i) a lithium chloride solution is produced in a calcination and leaching stage (A), wherein the lithium-containing ores and / or minerals and / or earths are initially calcined using one or more metal chloride vapors and / or a mixture of metal chlorides and are subsequently leached, in particular using water, wherein the one or more metal chlorides used or the mixture of metal chlorides used comprises at least sodium chloride;

[0046] (i) In the subsequent purification stage, a high-purity lithium chloride solution is produced, wherein the lithium chloride solution is purified in particular by the removal of cations such as sodium, potassium, calcium, magnesium and / or iron from the lithium chloride solution and

[0047] (iii) In the purification stage, sodium chloride, particularly obtained by fractional crystallization or solvent extraction, is used to calcine the lithium-containing ores and / or minerals and / or soils and is fed to the calcination and leaching stage. The method comprises one or more metal chlorides or the mixture of metal chlorides used in the calcination and leaching stage comprises at least potassium chloride and / or lithium chloride and / or magnesium chloride and / or calcium chloride. This document describes calcination and leaching stages of lithium-containing minerals, using metal chlorides and water, and does not include leaching stages from solid waste using magnesium chloride to enrich a liquid industrial residue with lithium.

[0048] Unlike previous art documents, the lithium recovery process by RISES leaching, where L2CO3 is extracted by performing an ion exchange using calcium and / or magnesium.

[0049] BRIEF DESCRIPTION OF THE FIGURES

[0050] Figure 1: represents the lithium recovery diagram from brines using the lithium carbonate plant RISES.

[0051] Figure 2: represents a process of leaching the pulp in suspension by means of mechanical agitation.

[0052] Figure 3: represents a process of leaching the pulp in suspension by means of pneumatic agitation.

[0053] Figure 4: represents a graph illustrating the leaching yields of RISES. Figure 5: represents a graph illustrating the leaching yields of RISES with Ca vs. Mg.

[0054] Figure 6: represents a graph that illustrates a study of the percentage effect of solids.

[0055] Figure 7: represents a graph illustrating the process yield by carrying out the leaching, accumulated in 4 stages. Figure 8: represents a graph illustrating the yields in stockpiling.

[0056] Figure 9: corresponds to a LiCl-NaCl-CaCl2 ternary diagram

[0057] Figure 10: corresponds to a LiCl-NaCl-MgCl2 ternary diagram

[0058] DESCRIPTION OF THE INVENTION

[0059] The invention consists of a process for recovering lithium from industrial solid waste (ISWW) by leaching with a solution with a high concentration of calcium and / or magnesium. Leaching is a solid-liquid transfer process, where the objective is the selective dissolution of one or more elements of interest, in order to obtain from a solid matrix, using an aqueous solution, an aqueous outlet solution (PLS), containing the species of interest, and a solid waste residue.

[0060] In the case of RISES (Recycled Lithium Energy Sources), the lithium present is in the form of lithium carbonate (Li₂CO₃), which is extracted by ion exchange using calcium and / or magnesium. This process involves contacting the RIS with a solution called mother liquor, which can be high or low in boron (LMAB and LMBB, respectively). This mother liquor comprises an industrial liquid waste (ILW). The mixture of RIS with LMBB or LMAB is adjusted using calcium chloride (CaCl₂) and / or magnesium chloride (MgCl₂), generating an incoming mother liquor in its different technical grades and hydration levels. This adjustment reduces the CO₃ content of the mother liquors (LMBB and LMAB) and also provides the necessary Ca and Mg for exchange with the Li₂.The adjusted liquid is subjected to a filtration stage, from which a stream of industrial solid waste originates that goes to collection and a mother liquor (ML) stream with a high content of Ca or Mg that is contacted with the RISES of the purification stage, obtaining a charged solution (PLS) with a high content of lithium and lithium-depleted RISES.

[0061] The process is based on the following dissolution reactions of Li2CO3 in the presence of CaCI2 and MgCI2:

[0062] CaCl 2(ac) + Li2CO 3(ac) → 2LiCl (ac) + CaCO 3(s) (Reaction 1)

[0063]

[0064] MgCl 2(ac) + Li2CO 3(ac) → 2LiCl (ac) + MgCO 3(s) (Reaction 2) These reactions demonstrate that Li2CO3 is more soluble than CaCO3 and MgCO3, which facilitates the dissolution of lithium, while calcium and magnesium precipitate as carbonates (CaCO3 and MgCO3, respectively).

[0065] The leaching process can be carried out in different types of equipment, such as reactors, vats, and heap leaching pads. Figures 1, 2, and 3 illustrate examples of leaching in reactors and the stages of the process. Leaching can be performed by agitation, using a mechanical impeller, or by air injection, which keeps the RISES in suspension within the leaching solution.

[0066] The agitation leaching method is used for high-grade minerals with a low particle size and low porosity.

[0067] The mineral in solution (7) is agitated by an impeller (4) as mechanical agitation or by air injection (6) as pneumatic agitation, which keeps the solid (8) (RIS) in suspension with the leaching solution (LM), as shown in Figure 3. Several leaching tests were performed to evaluate the lithium extraction performance from the RISES, using mother liquor with different concentrations of calcium and magnesium. The test conditions, results, and observations from these tests are presented below. Test conditions 1 (Table 1): Leaching of RISES using low-boron mother liquor (LMBB) adjusted with CaCl2.

[0068] • Test conditions 2 (Table 2): Comparison of RISES leaching using low boron mother liquor with CaCI2 versus mother liquor with MgCI2.

[0069] • Test conditions 3 (Table 3): Effect of solids ratio on leaching performance.

[0070] Test conditions

[0071] % Li RIS 1.58

[0072] % Li LM 0.12

[0073] % Ca in LM 0.65

[0074] % solids 20

[0075] RIS of

[0076] RIS type

[0077] plant

[0078] LM type AB

[0079] Time

[0080] 60 min

[0081] agitation

[0082]

[0083] Table 1: Test conditions for RISES leaching. Test conditions

[0084] LMBB Ca LMBB Mg Variables

[0085] 1.41 1.24

[0086] %L¡ RIS

[0087] 0.11 0.11

[0088] % Li LM

[0089] 0.83 0

[0090] % Ca in LM

[0091] 0 3.42

[0092] % Mg in LM

[0093] 40 40

[0094] % solids

[0095] RIS of RIS of

[0096] RIS type

[0097] plant plant

[0098] BB BB

[0099] LM type

[0100] Time

[0101] 60 min 180 min

[0102]

[0103] agitation

[0104] Table 2: Test conditions for leaching RISES with Ca vs Mg

[0105] Variables 30% solids 70% solids %L¡ RIS 1.24 1.24

[0106] %L¡ LM 0.11 0.11

[0107] %Ca in LM 0 0

[0108] %Mg in LM 3.42 3.42

[0109] % solids 30 70

[0110] RIS type Plant RIS Plant RIS type LM BB BB

[0111] Agitation time 60 min 60 min

[0112]

[0113] Table 3: Test Conditions Study of % solids effect. The results obtained show that calcium acts more effectively than magnesium as a leaching agent, which is due to a greater difference in solubility between Li2CO3 and calcium and magnesium carbonates.

[0114] The multi-stage leaching process was evaluated to maximize lithium extraction yield. The results (Table 4 and Figure 7) show a sustained increase in yield at each stage, reaching over 90% after four leaching stages.

[0115] Test conditions

[0116] Variables 1st Stage 2 o Stage 3 o Stage 4 o Stage % Li RIS 1.25 0.86 0.67 0.61

[0117] % Li LM 0.12 0.12 0.12 0.12

[0118] % Ca in LM 0 0 0 0

[0119] % Mg in LM 1.08 1.08 1.08 1.08

[0120] % solids 30 30 30 30

[0121] RIS of RIS of RIS of RIS of RIS Type

[0122] plant plant plant plant Type of LM BB BB BB BB Time

[0123] 60 min 60 min 60 min 60 min agitation

[0124]

[0125] Table 4: Multi-stage performance test conditions.

[0126] A study was also conducted on the leaching of stockpiled industrial waste to determine the feasibility of recovering lithium from this waste. The results showed that efficient lithium extraction is achieved even with stockpiled waste, demonstrating the viability of the process for this discarded waste.

[0127] Test conditions

[0128] %L¡ RIS 0.58

[0129] %L¡ LM 0.13

[0130] %Mg in LM 1.17

[0131] % solids 30

[0132] Type of RIS Collection

[0133] LM type AB

[0134] Time

[0135] 60 min

[0136]

[0137] agitation

[0138] Table 5: Performance test conditions in storage.

[0139] To determine the chemical equilibrium between the species present in the brine, tests were performed with different doses of CaCl2 and MgCl2. The results (Tables 6, 7 and 8) showed that equilibrium is reached similarly with both ions, with lithium concentrations in the resulting brine up to 1.3%.

[0140] Equilibrium conditions with Mg Equilibrium with Ca

[0141] proof

[0142] %Li RIS 0.84 2.06 %Li LM 0.10 0.21 %Ca in LM 9.90 3.20 %solids 30 30 No. stages 7 9

[0143] RIS type FP FT

[0144] Type LM AB BB

[0145]

[0146] Agitation time 60 min 60 min

[0147] Table 6. Equilibrium study test conditions Evolution LM c / Ca %K %Na %Mg %Ca %SO4 %Li %Cl %B %CO3 LMBB 9.9% Ca 0.20 1.32 0.12 9.94 0.02 0.10 20.90 0.45 0.57

[0148]

[0149] LM High Li w / Ca 0.23 5.25 0.04 0.59 0.00 1.23 17.30 0.01 0.01

[0150] Table 7. LM evolution in RIS leaching with Ca (fresh LM - stage 7)

[0151] Evolution LM c / Ca %K %Na %Mg %Ca %SO4 %L¡ %CI %B %CO3 LMBB 3.2% Mg 0.18 4.62 3.17 0.001 0.12 0.21 15.9 0.001 0.30 LM Alto Li c / Mg 0.18 5.38 0.13 0.001 0.04 1.10 16.21 0.02 0.05

[0152]

[0153] Table 8. LM evolution in RIS leaching with Mg (fresh LM - stage 9)

[0154] The operating ranges of the process were determined, including the amount of solids, leaching time, and concentrations of lithium, calcium, and magnesium in the different process streams. The ranges obtained are as follows (Table 9):

[0155] Working ranges and results

[0156] MgCl2 - CaCl2 dosing type

[0157] RIS Type FT- Collection

[0158] Type of LM LMBB - LMAB

[0159] %Solid 20 - 70

[0160] Leaching time 60 - 180 min

[0161] %L¡ RIS input 0.58 - 1.60

[0162] %L¡ LM input 0.11 - 0.13

[0163] %Ca LM input 0.001 - 2.05

[0164] %Mg LM input 0.02 - 3.42

[0165]

[0166] %L¡ RIS output 0.37 - 1.10

[0167] %L¡ LM output 0.16 - 1.13 Extraction performance

[0168] 22 - 56

[0169] RIS

[0170] Extraction performance

[0171] 25 - 54

[0172] LM

[0173]

[0174] Table 9: Ranges of results of 1-stage leaching.

Claims

RECLIN DICATION IS 1. A process for recovering lithium from industrial solid waste (ISWW) from a lithium carbonate production process in order to increase the overall efficiency of the lithium production process, CHARACTERIZED in that it comprises leaching lithium carbonate (Li₂CO₃) industrial solid waste (ISWW) by performing an ion exchange using calcium and / or magnesium in the leaching; wherein the process comprises subjecting the industrial solid waste to contact with industrial liquid waste adjusted with calcium and / or magnesium; wherein the adjustment is made with a solution comprising calcium chloride (CaCk) and / or magnesium chloride (MgCk) to generate an inlet mother liquor, in its different technical and hydration grades, so as to reduce the CO3 content of the mother liquor and incorporate the calcium (Ca) and magnesium (Mg) necessary to exchange with the lithium;where said adjusted liquid is subjected to a filtration stage, from which a stream of industrial solid waste originates that goes to collection and the incoming mother liquor stream (LM) with a high calcium or magnesium content is fed to the RISES leaching of the lithium carbonate process, from which a loaded solution (PLS) with a high lithium content and an outlet stream of lithium-depleted industrial solid waste are obtained.

2. Process for recovering lithium-rich brines from industrial solid waste according to claim 1, CHARACTERIZED in that said mother liquor has a high concentration in boron (LMAB).; 3. Process for recovering lithium-rich brines from industrial solid waste according to claim 1, CHARACTERIZED in that said mother liquor has a low concentration of boron (LMBB).

4. Process for recovering lithium-rich brines from industrial solid waste according to claim 1, CHARACTERIZED in that said leaching is carried out in reactors, vats or leaching heaps.

5. Process for recovering lithium-rich brines from industrial solid waste according to claim 1, CHARACTERIZED in that the percentage of solids in said RISES is in a range of 20 to 70%.

6. Process for recovering lithium-rich brines from industrial solid waste according to claim 1, CHARACTERIZED in that said leaching is carried out for a time between 60 and 180 minutes.

7. Process for recovering lithium-rich brines from industrial solid waste according to claim 1, CHARACTERIZED in that the percentage of lithium in the input solid waste is in a range between 0.58 and 2.50%.

8. Process for recovering lithium-rich brines from industrial solid waste according to claim 1, CHARACTERIZED in that the percentage of lithium in said input mother liquor is between 0 and 0.18%.

9. Process for recovering lithium-rich brines from industrial solid waste according to claim 1, CHARACTERIZED in that the percentage of calcium in said input mother liquor is in a range between 0.001 and 2.05%.

10. Process for recovering lithium-rich brines from industrial solid waste according to claim 1, CHARACTERIZED in that the percentage of magnesium in said input mother liquor is in a range between 0.02 and 3.42%.

11. Process for recovering lithium-rich brines from industrial solid waste according to claim 1, CHARACTERIZED in that the percentage of lithium in the output industrial solid waste is in a range between 0.01 and 1.10%.

12. Process for recovering lithium-rich brines from industrial solid waste according to claim 1, CHARACTERIZED in that the percentage of lithium in the loaded solution (PLS) is in a range between 0.16 and 1.3%.

13. Process for recovering lithium-rich brines from industrial solid waste according to claim 1, CHARACTERIZED in that it uses an inlet solution adjusted with calcium chloride and / or magnesium chloride to perform lithium leaching.

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