EP2851454A1 - Procédé de récupération de métal depuis une solution, système de récupération de métal depuis une solution, et système de récupération de lithium depuis de l'eau salée - Google Patents

Procédé de récupération de métal depuis une solution, système de récupération de métal depuis une solution, et système de récupération de lithium depuis de l'eau salée Download PDF

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Publication number
EP2851454A1
EP2851454A1 EP13790312.6A EP13790312A EP2851454A1 EP 2851454 A1 EP2851454 A1 EP 2851454A1 EP 13790312 A EP13790312 A EP 13790312A EP 2851454 A1 EP2851454 A1 EP 2851454A1
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EP
European Patent Office
Prior art keywords
electrode
solution
metal
lithium
recovery
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Withdrawn
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EP13790312.6A
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German (de)
English (en)
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EP2851454A4 (fr
Inventor
Je-Yong Yoon
Jae-Han Lee
Choon-Soo Kim
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Cellgen Co Ltd
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SNU R&DB Foundation
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Publication of EP2851454A1 publication Critical patent/EP2851454A1/fr
Publication of EP2851454A4 publication Critical patent/EP2851454A4/fr
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    • C—CHEMISTRY; METALLURGY
    • C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
    • C25C—PROCESSES FOR THE ELECTROLYTIC PRODUCTION, RECOVERY OR REFINING OF METALS; APPARATUS THEREFOR
    • C25C1/00—Electrolytic production, recovery or refining of metals by electrolysis of solutions
    • C25C1/22—Electrolytic production, recovery or refining of metals by electrolysis of solutions of metals not provided for in groups C25C1/02 - C25C1/20
    • C—CHEMISTRY; METALLURGY
    • C22—METALLURGY; FERROUS OR NON-FERROUS ALLOYS; TREATMENT OF ALLOYS OR NON-FERROUS METALS
    • C22B—PRODUCTION AND REFINING OF METALS; PRETREATMENT OF RAW MATERIALS
    • C22B26/00—Obtaining alkali, alkaline earth metals or magnesium
    • C22B26/10—Obtaining alkali metals
    • C22B26/12—Obtaining lithium
    • C—CHEMISTRY; METALLURGY
    • C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
    • C25C—PROCESSES FOR THE ELECTROLYTIC PRODUCTION, RECOVERY OR REFINING OF METALS; APPARATUS THEREFOR
    • C25C1/00—Electrolytic production, recovery or refining of metals by electrolysis of solutions
    • C25C1/02—Electrolytic production, recovery or refining of metals by electrolysis of solutions of light metals
    • C—CHEMISTRY; METALLURGY
    • C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
    • C25C—PROCESSES FOR THE ELECTROLYTIC PRODUCTION, RECOVERY OR REFINING OF METALS; APPARATUS THEREFOR
    • C25C3/00—Electrolytic production, recovery or refining of metals by electrolysis of melts
    • C25C3/02—Electrolytic production, recovery or refining of metals by electrolysis of melts of alkali or alkaline earth metals
    • C—CHEMISTRY; METALLURGY
    • C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
    • C25C—PROCESSES FOR THE ELECTROLYTIC PRODUCTION, RECOVERY OR REFINING OF METALS; APPARATUS THEREFOR
    • C25C7/00—Constructional parts, or assemblies thereof, of cells; Servicing or operating of cells
    • C25C7/02—Electrodes; Connections thereof

Definitions

  • Example embodiments of the present invention relate to methods and systems for recovering a metal. More particularly, example embodiments of the present invention relate to methods for recovering a metal from solution, systems for recovering a metal from solution, and systems for recovering lithium from salt water.
  • Lithium (Li) is widely utilized in various industries such as glasses, ceramics, alloys, lubricating oils, pharmaceutics, etc. Particularly, a lithium secondary battery has been recently highlighted and developed for a power supply of a hybrid vehicle and an electric vehicle. A demand for the lithium secondary battery is expected to surge up to about 100 times a demand in a compact battery market for, e.g., a cell phone, a laptop computer, etc.
  • lithium lithium
  • a demand for lithium may be increased drastically as global environmental restrictions are becoming strengthened, and an application of lithium may be expanded to various industries of 21 st century including electronic, chemical and energy industries as well as the hybrid and electric vehicles industry.
  • a source of lithium may include a mineral, a brine or a sea water.
  • the mineral may include spodumene, petalite and lepidolite which contain a relatively large amount of lithium in a range of about 1 % to about 1.5 %.
  • an extraction of lithium from the mineral may require many complex processes such as a floatation, an annealing, a grinding, an acid mixing, an extraction, a purification, an concentration, a precipitation, etc., and thus large cost and energy may be spent during the processes.
  • an environmental pollution may be caused by an acid used in the extraction of lithium.
  • a recovery device including an adsorbent When lithium is recovered from the sea water, a recovery device including an adsorbent may be introduced into the sea water so that lithium may be selectively adsorbed, and then lithium may be recovered by an acid treatment.
  • a concentration of lithium in the sea water is as small as about 0.17 ppm, and thus the recovery from the sea water may be limited from an economical aspect.
  • lithium is mainly recovered from the brine.
  • a salt lake is used as a crude source of lithium, and other salts including Mg, Ca, B, Na or K co-exist therein together with lithium.
  • a concentration of lithium in the brine may range from about 0.3 g/L to about 1.5 g/L, and lithium in the brine may be extracted as a form of lithium carbonate.
  • a solubility of lithium carbonate may be about 13 g/L.
  • a concentration of lithium carbonate in the brine may range from about 1.59 g/L to about 7.95 g/L which is smaller than the solubility of lithium carbonate.
  • precipitated lithium carbonate may be re-dissolved thereby to reduce a recovery ratio of lithium.
  • a conventional method for recovering lithium in the brine as the form of lithium carbonate includes pumping the brine from a natural salt lake and storing in an evaporation pond, naturally vaporizing the brine for a long period more than a year to concentrate lithium as great as several ten times, and removing impurities such as Mg, Ca or B by a precipitation so that lithium may be recovered at an amount greater than the solubility of lithium carbonate.
  • the conventional method requires much time for the vaporization and the concentration of the brine to reduce an overall productivity. Further, lithium may be precipitated together with the impurities during the vaporization and the concentration steps to cause a loss of lithium, and the method is limited in a rainy season.
  • Example embodiments of the present invention provide a method for efficiently recovering various metals from a solution.
  • Example embodiments of the present invention provide a system for recovering various metals from a solution.
  • Example embodiments of the present invention provide a system for recovering various metals such as lithium from a salt water.
  • a method for recovering a metal from a solution In the method, a first electrode that includes a metal for recovery and a second electrode that includes a metal different from the metal for recovery are prepared. The first electrode and the second electrode are immersed in a first solution that includes a metal ion for recovery. The metal ion for recovery in the first solution is combined with the first electrode. The first electrode and the second electrode are charged while immersing the first and second electrodes in a second solution different from the first solution so that the metal ion for recovery is separated from the first electrode. The metal for recovery is recovered from the second solution.
  • the first electrode and the second electrode which are positively and negatively charged, respectively may be electrically connected to induce a discharge.
  • the metal for recovery may include lithium
  • the first electrode may include a lithium manganese oxide
  • the second electrode may include silver, zinc, copper and/or mercury.
  • a system for recovering a metal from a solution includes a first electrode including a first metal, a second electrode including a second metal different from the first metal, and a power source for charging the first and second electrodes.
  • the first electrode is discharged in a first solution that includes a first metal ion to be combined with the first metal ion and is charged in a second solution different from the first solution to release the first metal ion.
  • the second electrode is discharged in the first solution to be combined with a first anion of the first solution and is charged in the second solution to release the first anion.
  • the first electrode may include a lithium manganese oxide
  • the second electrode may include silver, zinc, copper and/or mercury.
  • the first electrode may include LiMn 2 O 4 having a spinel phase.
  • the first electrode may further include a carbon electrode, and the lithium manganese oxide may be coated on a surface of the carbon electrode.
  • the system may further include a battery capable of repeating charge and discharge processes.
  • An electric energy generated when the first and second electrodes are discharged may be stored in the battery, and the battery may be connected to the power source to provide the stored electric energy.
  • a system for recovering lithium from a salt water includes a first electrode including a lithium manganese oxide, a second electrode including silver, a power source for charging the first and second electrodes, and a battery capable of repeating charge and discharge processes.
  • the first electrode is discharged in a salt water that includes a lithium ion and a chlorine ion to be combined with the lithium ion and is charged in a charging solution different from the salt water to release the lithium ion.
  • the second electrode is discharged in the salt water to be combined with the chlorine ion and is charged in the charging solution to release the chlorine ion.
  • the battery stores an electric energy generated when the first electrode is discharged and is connected to the power source to provide the stored electric energy.
  • the first electrode may include LiMn 2 O 4 having a spinel phase.
  • Example embodiments are described herein with reference to cross-sectional illustrations that are schematic illustrations of idealized example embodiments (and intermediate structures). As such, variations from the shapes of the illustrations as a result, for example, of manufacturing techniques and/or tolerances, are to be expected. Thus, example embodiments should not be construed as limited to the particular shapes of regions illustrated herein but are to include deviations in shapes that result, for example, from manufacturing. For example, an implanted region illustrated as a rectangle will, typically, have rounded or curved features and/or a gradient of implant concentration at its edges rather than a binary change from implanted to non-implanted region.
  • a buried region formed by implantation may result in some implantation in the region between the buried region and the surface through which the implantation takes place.
  • the regions illustrated in the figures are schematic in nature and their shapes are not intended to illustrate the actual shape of a region of a device and are not intended to limit the scope of the present inventive concept.
  • FIG. 1 is a flow chart illustrating a method for recovering a metal from a solution in accordance with example embodiments.
  • a first electrode and a second electrode may be immersed in a first solution containing a metal ion for recovery, and the metal ion in the first solution may be combined with the first electrode.
  • the first electrode and the second electrode may be positively and negatively charged, respectively, and the first and second electrodes may be electrically connected to cause a discharge so that the metal ion for recovery in the first solution may be combined with the first electrode.
  • the first electrode may be positively charged and the second electrode may be negatively charged.
  • a metal for recovery may not be specifically limited, however, may include, e.g., lithium, sodium, potassium, magnesium, calcium, strontium, manganese, etc.
  • the first solution may be obtained, e.g., a sea water or a highly concentrated brine (or a salt water).
  • the first solution may further include other metal ions and anions in addition to the metal ion for recovery.
  • the metal for recovery is lithium
  • the first solution may include cations of lithium, sodium, potassium, magnesium, calcium, strontium, manganese, etc., and a chlorine anion (Cl - ).
  • the first electrode may include the metal for recovery.
  • the first electrode may also include lithium.
  • the first electrode may have a selectivity for the metal for recovery.
  • the first electrode may include a lithium manganese oxide (LMO).
  • the LMO may include LiMn 2 O 4 , LiMnO 6 , etc., and these may be used alone or in a combination thereof.
  • the selectivity for a lithium ion of the LMO may vary according to a phase of the LMO.
  • the LMO may have a spinel phase.
  • the second electrode may include a metal different from the metal for recovery.
  • the metal of the second electrode may have an ionization tendency greater than that of the metal for recovery.
  • the first electrode may serve as an anode (positive electrode) and the second electrode may serve as a cathode (negative electrode).
  • the metal of the second electrode may be selected in consideration of the ionization tendency of the metal for recovery, for example, may include silver, zinc, copper, mercury, etc.
  • the second electrode may preferably include the metal that may be combined with and separated from an anion reversibly and repeatedly in charge and discharge processes.
  • silver may be used as the metal of the second electrode in consideration of the reversibility and an environmental aspect.
  • the discharge may occur.
  • electrons may be moved from the first electrode to the second electrode.
  • the metal ion for recovery in the first solution may accept the electron to be combined with the first electrode, and the metal of the second electrode may lose the electron to be combined with an anion in the first solution.
  • the first electrode may include LiMn 2 O 4
  • the second electrode may include silver
  • the first solution may include the lithium cation and the chlorine anion.
  • a reaction represented by Chemical Equation 1 may occur in the first electrode
  • a reaction represented by Chemical Equation 2 may occur in the second electrode.
  • the lithium ion in the first solution may be combined with the LMO of the first electrode, and the chlorine ion in the first solution may be combined with silver of the second electrode to generate silver chloride. As a result, concentrations of the lithium and chlorine ions in the first solution may be reduced.
  • the LMO included in the first electrode may have the selectivity for lithium, and thus lithium may be selectively separated from the first solution containing the different metal ions.
  • the positively charged first electrode and the negatively charged second electrode may be electrically connected to each other for discharging the first and second electrodes.
  • a power source may be connected to the first and second electrodes, the first electrode may be negatively charged (electrons may be provided), and the second electrode may be positively charged so that the lithium ion in the first solution may be combined with the first electrode.
  • the first and second electrodes may be immersed in a second solution different from the first solution and may be charged so that the metal ion for recovery may be separated from the first electrode.
  • the second solution may be an aqueous solution including suitable electrolytes.
  • the first and second electrodes may be charged such that the first electrode may be positively charged and the second electrode may be negatively charged to cause a reaction represented by Chemical Equation 3 in the first electrode and a reaction represented by Chemical Equation 4 in the second electrode.
  • Chemical Equation 3 LiMn 2 O 4 ⁇ Li 1-x Mn 2 O 4 + xLi+ + xe -
  • Chemical Equation 4 xAgCl + xe - ⁇ xAg + xCl -
  • the LMO of the first electrode may lose the lithium ion
  • silver chloride of the second electrode may lose the chlorine ion to be reduced into silver.
  • the second solution may include the lithium cation and the chlorine anion.
  • step S30 the metal for recovery may be recovered from the second solution.
  • Various conventional methods may be implemented for recovering the metal.
  • the second solution when the second solution includes the lithium cation and the chlorine anion, the second solution may be heated to obtain a solid-state lithium chloride.
  • Lithium chloride may be non-toxic and chemically stable, and thus easily stored and managed. Additionally, lithium chloride may be directly used as an electrolyte of a lithium secondary battery.
  • the second solution including the lithium cation and the chlorine anion may be treated by an electrolysis to collect lithium.
  • the discharge process in the first solution and the charge process in the second solution described above may be repeated so that a concentration of the metal for recovery in the second solution may be increased.
  • the first electrode may be positively charged and the second electrode may be negatively charged by the charge process in the second solution.
  • the first and second electrodes may be taken out from the second solution, and immersed and electrically connected to each other again in the first solution so that the lithium ion in the first solution may be combined again with the first electrode by the discharge process. If the concentration of the metal for recovery in the second direction becomes increased, a recovery efficiency of the metal may be improved.
  • a metal may be efficiently recovered from a solution.
  • highly concentrated lithium may be obtained in a short time compared to conventional methods using vaporization/concentration of brine and adsorption from a sea water.
  • the method in accordance with example embodiments may include simple processes and may be relatively free from an environmental pollution. Additionally, an electric energy generated from the discharge process may be stored and reused to minimize an energy consumption.
  • the method in accordance with example embodiments may be used for recovering a metal from a sea water or a highly concentrated brine, and may be also used for recovering a metal from an industrial wastewater.
  • a system for recovering a metal from a solution may comprise a first electrode including a first metal and a second electrode including a second metal different from the first metal.
  • the first and second electrodes may be electrically connected to each other.
  • the first electrode may be discharged in a first solution including a first metal ion to be combined with the first metal ion, and may be charged in a second solution different from the first solution to release the first metal ion.
  • the second electrode may be discharged in the first solution to be combined with a first anion of the first solution, and may be charged in the second solution to release the first anion.
  • the system may include a power source for charging the first and second electrodes.
  • FIGS. 2 and 3 are schematic views illustrating a system for recovering a metal from a solution in accordance with example embodiments.
  • a first solution 30 may be accommodated in a first bath 40.
  • a first electrode 10 and a second electrode 20 may be immersed in the first solution 30.
  • the first electrode 10 and the second electrode 20 may be partially immersed in the first solution 30 such that upper portions thereof may be exposed from the first solution 30.
  • the first and second electrodes 10 and 20 may be entirely immersed in the first solution 30.
  • the first solution 30 may include a metal ion for recovery.
  • a metal for recovery may be lithium.
  • the first solution 30 may be a sea water or a highly concentrated brine (or salt water), and may further include sodium, potassium, magnesium, calcium, strontium, manganese, etc., in addition to lithium.
  • the first solution 30 may also include an anion. If the first solution 30 is the sea water or the highly concentrated brine, the first solution may mainly include a chlorine anion (Cl - ).
  • the first electrode 10 may include the metal for recovery.
  • the first electrode 10 may also include lithium.
  • the first electrode 10 may have a selectivity for the metal for recovery.
  • the first electrode 10 may include a lithium manganese oxide (LMO).
  • the LMO may include LiMn 2 O 4 , LiMnO 6 , etc., and these may be used alone or in a combination thereof.
  • the selectivity for a lithium ion of the LMO may vary according to a phase of the LMO.
  • the LMO may have a spinel phase.
  • the LMO may have a relatively low conductivity.
  • the first electrode 10 may further include an additional material having a relatively strong conductivity.
  • the first electrode 10 may include a carbon electrode containing graphite, carbon nanotube, graphene, etc., and the LMO may be at least partially coated on a surface of the carbon electrode.
  • a wire for electrically connecting the first electrode 10 and the second electrode 20 may be connected to the carbon electrode.
  • the first electrode 10 may include a mixture of powders of the LMO and graphite, and the mixture may be at least partially coated on the surface of the carbon electrode.
  • a positive electrode material composition including the LMO, the powder of graphite, a binding agent and a solvent may be coated on the carbon electrode, and dried to obtain the first electrode 10.
  • the binding agent may include polyvinyliden fluoride (PVDF), polyvinyl alcohol (PVA), polyurethane (PU), etc. These may be used alone or in a combination thereof.
  • the solvent may include an alcohol such as methanol, ethanol, propanol, butanol, etc. These may be used alone or in a combination thereof.
  • the second electrode 20 may include a metal different from the metal for recovery. Further, the metal of the second electrode 20 may have an ionization tendency greater than that of the metal for recovery. Thus, when the first and second electrodes 10 and 20 are electrically connected to each other, the first electrode 10 and the second electrode 20 may serve as an anode and a cathode, respectively.
  • the metal of the second electrode 20 may include silver, zinc, copper, mercury, etc. In example embodiments, the second electrode 20 may include silver.
  • the first and second electrodes 10 and 20 may be electrically connected to each other through the wire for a discharge process.
  • the first electrode 10 may be positively charged, and the second electrode 20 may be negatively charged to result in the discharge process of the first and second electrodes 10 and 20.
  • the first electrode 10 may include LiMn 2 O 4
  • the second electrode 20 may include silver
  • the first solution 30 may include the lithium cation and the chlorine anion. Therefore, when the first and second electrodes 10 and 20 are electrically connected to each other, the lithium cation of the first solution 30 may be combined with the LMO of the first electrode 10, and the chlorine anion of the first solution 30 may be combined with silver of the second electrode 20 to generate silver chloride. As a result, concentrations of the lithium and chorine ions may be reduced in the first solution 30.
  • the first and second electrodes 10 and 20 may be connected to a battery 50.
  • An electric energy generated from the discharge process may be stored in the battery 50.
  • the battery 50 may be also used as a power source in a charge process described below.
  • the battery 50 may include any conventional battery capable of repeating charge and discharge processes of an electric energy.
  • a lead storage battery, a mercury battery, a lithium ion battery, a lithium polymer battery, etc. may be used as the battery 50.
  • the first and second electrodes 10 and 20 after the discharge process may be immersed in a second solution 60 accommodated in a second bath 70.
  • the LMO of the first electrode 10 may lose the lithium ion and silver chloride of the second electrode 20 may lose the chlorine ion to be reduced into silver.
  • the second solution 60 may include the lithium cation and the chlorine anion.
  • the first and second electrodes 10 and 20 may be connected to a suitable power source for charging the first and second electrode 10 and 20.
  • the power source may be connected to the battery 50, and the electric energy stored in the battery may be utilized so that an energy efficiency may be improved.
  • lithium may be recovered as a form of, e.g., a lithium salt from the lithium ion solution.
  • the first and second bath 40 and 70 may be separated from each other. However, the discharge process may be performed in the first solution, and then the first solution may be replaced with the second solution to perform the charge process continuously in a single container.
  • highly concentrated lithium may be obtained in a short time compared to conventional methods using vaporization/concentration of brine and adsorption from a sea water.
  • the method or the system in accordance with example embodiments may include simple processes and may be relatively free from an environmental pollution. Additionally, an electric energy generated from the discharge process may be stored and reused to minimize an energy consumption.
  • a silver electrode of 3x3 cm 2 , and a graphite electrode of the same size were prepared.
  • a powder of LiMn 2 O 4 , Super-P (manufactured by Timcal, Swiss) as a graphite powder, and PVDF as a binder resin were mixed in a mixing ratio of about 80:10:8 to form a mixture.
  • the mixture was dispersed in ethanol, coated on the graphite electrode and dried to prepare an electrode for lithium recovery.
  • the electrode for lithium recovery and the silver electrode were immersed with a distance of about 1 cm therebetween in a charging solution of about 90 ml including lithium chloride of about 25 mM.
  • a power source was connected to the electrodes to provide a charging voltage of about 1.2 V for about 20 minutes. Accordingly, the electrode for lithium recovery was positively charged, and the silver electrode was negatively charged.
  • the electrode for lithium recovery and the silver electrode were immersed in a discharging solution of about 90 ml including lithium chloride of about 25 mM and sodium chloride of about 25 mM.
  • the electrode for lithium recovery and the silver electrode were connected through a wire to be discharged for about 30 minutes.
  • the charge and discharge processes were repeatedly performed three times. On completion of each cycle (including one charge process and one discharge process), a sample of about 1 ml was extracted from the discharging solution, and concentration changes of lithium and sodium ions were measured using a ion-chromatography apparatus, DX-120 (manufactured by DIONEX). The results are shown in FIG. 4 .
  • a silver electrode of 3x3 cm 2 , and a graphite electrode of the same size were prepared.
  • a powder of LiMn 2 O 4 , Super-P (manufactured by Timcal, Swiss) as a graphite powder, and PVDF (weight average molecular weight: ⁇ 534,000, glass transition temperature: -38 °C, density at 25 °C: 1.74 g/ml, manufactured by Sigma Aldrich, USA) as a binder resin were mixed in a mixing ratio of about 80:10:8 to form a mixture.
  • the mixture was dispersed in ethanol, coated on the graphite electrode and dried to prepare an electrode for lithium recovery.
  • the electrode for lithium recovery and the silver electrode were immersed with a distance of about 1 cm therebetween in a charging solution of about 80 ml including lithium chloride of about 30 mM.
  • a power source was connected to the electrodes to provide a charging voltage of about 1.2 V for about 20 minutes. Accordingly, the electrode for lithium recovery was positively charged, and the silver electrode was negatively charged.
  • the electrode for lithium recovery and the silver electrode were immersed in a discharging solution of about 80 ml including lithium chloride of about 30 mM, sodium chloride of about 30 mM, potassium chloride of about 30 mM and magnesium chloride of about 30 mM.
  • the electrode for lithium recovery and the silver electrode were connected through a wire to be discharged for about 40 minutes.
  • the charge and discharge processes were repeatedly performed four times. On completion of each cycle (including one charge process and one discharge process), a sample of about 1 ml was extracted from the discharging solution, and concentration changes of lithium, potassium, calcium, magnesium and sodium ions were measured using a ion-chromatography apparatus, DX-120 (manufactured by DIONEX). The same amount of a sample was extracted from the charging solution, and a concentration change of a lithium ion was measured. The results are shown in FIGS. 5 and 6 .
  • FIG. 4 is a graph showing concentration changes of the lithium ion and the sodium ion present in the discharging solution while repeating the charge and discharge processes in Example 1.
  • FIG. 5 is a graph showing concentration changes of the lithium ion, the calcium ion, the potassium ion, the magnesium ion and the sodium ion present in the discharging solution while repeating the charge and discharge processes in Example 2.
  • FIG. 6 is a graph showing a concentration change of the lithium ion present in the charging solution while repeating the charge and discharge processes in Example 2.
  • the concentration of the lithium ion was continuously decreased while repeating the charge and discharge processes in Example 1, however, the concentration of the sodium ion was substantially maintained without a reduction. Therefore, it can be acknowledged that the lithium ion may be selectively recovered from a mixture with the sodium ion using the method and the system for recovering a metal from a solution according to example embodiments.
  • the concentration of the lithium ion was continuously decreased while repeating the charge and discharge processes in Example 2, however, the concentrations of the calcium ion, the potassium ion and the sodium ion were substantially maintained without a reduction.
  • the concentration of the magnesium ion was decreased in a first cycle, and then substantially maintained without a reduction in the subsequent cycles.
  • the concentration of the lithium ion was continuously increased in the charging solution while repeating the charge and discharge processes. Therefore, it can be acknowledged that the lithium ion may be selectively recovered from a mixture with the sodium ion, the potassium ion, the calcium ion and the magnesium ion using the method and the system for recovering a metal from a solution according to example embodiments.
  • the sodium and magnesium ions are significantly present in the sea water and the highly concentrated brine which may be sources of lithium.
  • magnesium may have a solubility similar to that of lithium, and thus may not be easily separated by a vaporization method.
  • the presence of these ions may be a main factor reducing an efficiency in a lithium recovery process. Therefore, the method and the system for recovering a metal from a solution according to example embodiments may be implemented to efficiently recover lithium from the sea water and the highly concentrated brine.

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EP13790312.6A 2012-05-16 2013-01-17 Procédé de récupération de métal depuis une solution, système de récupération de métal depuis une solution, et système de récupération de lithium depuis de l'eau salée Withdrawn EP2851454A4 (fr)

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KR1020120051834A KR101361836B1 (ko) 2012-05-16 2012-05-16 용액으로부터 금속을 회수하기 위한 방법, 용액으로부터 금속을 회수하기 위한 시스템 및 염수로부터 리튬을 회수하기 위한 시스템
PCT/KR2013/000353 WO2013172533A1 (fr) 2012-05-16 2013-01-17 Procédé de récupération de métal depuis une solution, système de récupération de métal depuis une solution, et système de récupération de lithium depuis de l'eau salée

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EP2851454A1 true EP2851454A1 (fr) 2015-03-25
EP2851454A4 EP2851454A4 (fr) 2016-01-13

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WO (1) WO2013172533A1 (fr)

Cited By (2)

* Cited by examiner, † Cited by third party
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WO2021160239A1 (fr) * 2020-02-10 2021-08-19 Fraunhofer-Gesellschaft zur Förderung der angewandten Forschung e.V. Procédé et appareil pour l'extraction de lithium à partir de sources de lithium aqueuses
WO2021160240A1 (fr) * 2020-02-10 2021-08-19 Fraunhofer-Gesellschaft zur Förderung der angewandten Forschung e.V. Procédé et appareil d'extraction électrochimique de lithium à partir de sources de lithium aqueuses

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WO2021160240A1 (fr) * 2020-02-10 2021-08-19 Fraunhofer-Gesellschaft zur Förderung der angewandten Forschung e.V. Procédé et appareil d'extraction électrochimique de lithium à partir de sources de lithium aqueuses

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KR20130128079A (ko) 2013-11-26
KR101361836B1 (ko) 2014-02-12

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