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    • 专利摘要:
    Material in the form of an alveolar monolith consisting of a matrix of an inorganic oxide with open hierarchical porosity comprising macropores, mesopores, and micropores, said macropores, mesopores, and micropores, being interconnected, and nanoparticles at least one inorganic solid material exchanger of a metal cation being distributed in said porosity. Process for the preparation of this material and method for separating a metal cation, in particular a cation of a radioactive isotope of a metal such as cesium using this material.
    公开号:FR3015476A1
    申请号:FR1363329
    申请日:2013-12-20
    公开日:2015-06-26
    发明作者:Jeremy Causse；Agnes Grandjean；Alexei Tokarev；Yves Barre
    申请人:Commissariat a lEnergie Atomique CEA；Commissariat a lEnergie Atomique et aux Energies Alternatives CEA；
    IPC主号:
    专利说明:

    [0001] INVERGANIC MONOLITHIC MATERIALS ALVEOLAR CATIONIC EXCHANGERS, PROCESS FOR PREPARING THE SAME, AND SEPARATION METHOD USING SAME. TECHNICAL FIELD The invention relates to an inorganic alveolar cationic exchanger monolithic material. More specifically, the invention relates to a material in the form of an alveolar monolith constituted by a matrix of an inorganic oxide with hierarchical porosity, open and interconnected, and nanoparticles of at least one inorganic solid material exchanger a metal cation such as a metal hexa- or octacyanometallate being distributed in said porosity. The invention also relates to the process for preparing said material. The present invention also relates to a process for separating metal cations, in particular radioactive cations, contained in a liquid using said material. The technical field of the invention may, in general, be defined as that of a treatment of liquid effluents and in particular such as that of the treatment of radioactive liquid effluents, in particular with a view to removing metal cations, such as cations. cesium. STATE OF THE PRIOR ART Nuclear installations such as power reactors, spent nuclear fuel reprocessing plants, laboratories, research centers, and liquid effluent treatment plants generate radioactive liquid effluents. These effluents, whose volumes are considerable, must be treated and decontaminated before being released into the environment.
    [0002] The pollutants contained in these effluents and which must therefore be eliminated are mainly solid particles and radio-elements essentially present in the form of metal cations in solution. Industrial processes for the decontamination of liquid effluents, and in particular radioactive liquid effluents, are, however, few in number because of the complex composition of said effluents, their high ionic strength, and also the wide variety of pH values that they can present. . The most common treatments currently used for the decontamination of liquid effluents are evaporation and chemical treatment by coprecipitation.
    [0003] Thus, the first step of a process for decontaminating liquid solutions, in particular low-concentration radioactive liquid solutions, on an industrial scale, generally consists in carrying out the evaporation of these solutions in order to concentrate all the ions present in those in the form of a solid waste, which thus becomes a residue of the decontamination process.
    [0004] However, this evaporation treatment is not possible for saline effluents because it then occurs scaling of the installation. In addition, the presence of certain ions in the liquid effluents causes hot corrosion during the evaporation treatment. In the case of highly saline radioactive effluents, another possible treatment is chemical treatment by coprecipitation or entrainment which is a phase change treatment. It involves transferring the radio-elements present from a liquid phase to a solid phase either by coprecipitation or by entrainment from solid particles. These solid particles are then rich in radioactive elements and are then recovered by filtration or decantation before being confined in a suitable matrix. These methods of coprecipitation (for example by barium sulfate for the extraction of 90Sr) or entrainment (from particles of nickel-potassium hexacyanoferrate for 137Cs) have a number of disadvantages. Firstly, the volumes of sludge formed are substantial and may pose problems of compatibility with the materials currently used for confining industrial waste, such as glasses or cementitious matrices. In addition, the coprecipitation agents are often sensitive to the chemical composition and the ionic strength of the effluent, which causes a significant drop in the selectivity and therefore an increase in the volume of waste.
    [0005] In order to overcome the drawbacks enumerated above of treatment processes, decontamination of liquid effluents, many researchers and industrialists, particularly in the nuclear industry, are currently looking for other ways of treating these effluents. One of the solutions studied is the use of inorganic ion exchange materials, or more precisely inorganic cation exchange materials which have a high selectivity for the ions to be extracted. Although there is a very large literature on the different ionic ion exchanger materials that are selective for 905r, 137Cs, or 60Co, the majority of the studies concern discontinuous tests involving powder-type exchanger materials. In fact, the inorganic ion exchange materials currently used to sorb the elements to be decontaminated are essentially in the form of relatively fine powders, having grain sizes of the order of one micrometer, which are not compatible with a method used. continuously. These powders, when used in a process carried out continuously, in particular in columns, can cause a high pressure drop in these columns, which can go as far as clogging them, clogging them, and stopping them. installation. If the inorganic ion exchange materials are no longer used in the form of loose powders but solid, compact powders, clogging problems are certainly avoided, but the micron size implies a low adsorption capacity because the adsorption occurs in area. There is therefore, in the light of the foregoing, a need for an inorganic solid ion exchange material, more exactly for an inorganic cation exchange material that is compatible with a continuous implementation in a process for separating a metal cation. from a liquid medium, and which has a high adsorption capacity.
    [0006] In particular, this inorganic solid material ionic exchangers must be chemically and mechanically stable so as to be thus packaged in a column allowing a continuous operation without the occurrence of clogging phenomena, clogging.
    [0007] This inorganic solid ion exchanger material must also have excellent fixing properties, in particular decontamination, that is to say similar, or even superior in particular to that of an inorganic ion exchange material in the form of loose powders. The inorganic ion exchange material must also combine good mechanical stability with a high reaction rate as opposed to products in compact form whose low specific surface area leads to slow reaction rates. In other words, this inorganic solid ion exchange material must have among others excellent mechanical and chemical stability, a high coefficient of affinity or decontamination, a high reactivity, as well as good selectivity.
    [0008] These properties must be obtained with a minimum amount of inorganic solid ion exchange material. In addition, particularly in the case of the attachment of radioactive elements, it is necessary that the inorganic solid ion exchange material can be easily stored and / or vitrified without risk by known methods.
    [0009] Finally, the material must have a composition and properties perfectly reproducible and controlled, and must be prepared by a reliable method. The object of the present invention is to provide an inorganic solid ion exchange material that meets these needs, among others. The object of the present invention is still to provide an inorganic solid ion exchange material, which does not have the drawbacks, defects, disadvantages, and limitations of the ionic solid ion exchange material of the prior art, especially in the form of loose or compact powders. , and which overcomes the problems of the materials of the prior art.
    [0010] SUMMARY OF THE INVENTION This and other objects are achieved according to the invention by a solid material in the form of an alveolar monolith consisting of a matrix of an inorganic oxide with hierarchical and open porosity. comprising macropores, mesopores, and micropores, said macropores, mesopores, and micropores being interconnected, and nanoparticles of at least one inorganic solid material exchanging a metal cation being distributed in said porosity. The material according to the invention is fundamentally different from the materials of the prior art in that it is in the specific form of an alveolar monolith, in that this monolith has a hierarchized porosity associating three types of pores, namely macropores, mesopores, and micropores, and finally in that nanoparticles of a specific material which is an inorganic solid material exchanger of a metal cation are distributed in this porosity. The material according to the invention meets the needs listed above, it does not have the disadvantages of the materials of the prior art and it provides a solution to the problems posed by the materials of the prior art. Thus, in the case of a column effluent treatment method, the material according to the invention, which is in the specific form of a hierarchized porous alveolar monolith, has the advantage of greatly reducing the pressure drop. relative to a material consisting of a compact stack of particles. The material according to the invention thus makes it possible to limit the risk of clogging of the treatment system, such as a column, due to the production of fine particles within the bed of particles. The fact that the material according to the invention is in the form of a monolith gives it high mechanical strength and stability, while the fact that the monolith is mainly constituted by an inorganic oxide gives it a high chemical resistance and ensures hence the treatment of a wide variety of effluents. In addition, the presence of the inorganic metal cation exchanger solid material in the form of nanoparticles distributed in the porosity of the monolith greatly increases the amount of metal cations that can be absorbed relative to an inorganic solid cation exchange material which is a massive form. This is explained by the fact that when the cation exchanger is in nanometric form, the specific surface area available for metal cations, such as cesium cations, is higher. Monoliths with hierarchical porosity are commercially available. It is only silica monoliths. The incorporation of cation exchanger nanoparticles into such monoliths, however, has neither been described nor suggested, it is the same for their use for removing cations from a liquid effluent, in particular for decontaminating complex effluents containing different radio elements. Numerous documents report on the functionalization of inorganic monoliths by chemical functions covalently bonded to the material. It is therefore not about the incorporation of nanoparticles and even fewer nanoparticles of a cation exchanger into the porosity of monoliths. For example, WO-A1-2001 / 47855 [1] discloses the functionalization of a silica monolith with a silane in order to more efficiently produce ketene molecules. In this case, the silane is thus bonded to the silica network by post-functionalization. Similarly, the document WO-A2-2008 / 031108 [2] presents a list of silane precursors intended for the functionalization of pre-synthesized porous silicas. The targeted applications are diverse and depend on the type of silane considered. Moreover, we know a method of monolith synthesis which was developed by R. BACKOV group of the Paul Pascal Research Center in Bordeaux. This process consists of preparing a direct oil-in-water emulsion containing a majority of oil by volume. A silica precursor previously dissolved in the aqueous phase reacts to form an inorganic network surrounding the drops of oil. The oil phase is then removed by rinsing, which releases the macroporosity of the material. In order to stabilize the water / oil interface, surfactants are required.
    [0011] These surfactants can be either molecular organic surfactants or colloidal particles. The process using molecular organic surfactants has been the subject of the application WO-A2-2008129151 [3]. It makes it possible to obtain a material in the form of a solid alveolar monolith consisting of a polymer of an inorganic oxide bearing organic groups, which has a hierarchical porosity with macropores, mesopores and interconnected micropores. More specifically, this process consists in preparing an emulsion by adding an oily phase to an aqueous surfactant solution, adding to the aqueous surfactant solution at least one precursor tetraalkoxide of the inorganic oxide polymer, before or after the preparation of the emulsion, the reaction mixture is allowed to stand until the precursor is condensed, then the mixture is dried to obtain a monolith. At least one alkoxide carries an organic group. There is no mention or suggestion in this document of the incorporation of nanoparticles, let alone nanoparticles of cation exchangers, in such monoliths. In the same way, the use of these monoliths to remove cations from a liquid effluent, in particular to remove cations of radioactive effluent radioactive elements, is not described or suggested in this document. The process employing colloidal solid particles has been the subject of the application WO-A2-2012 / 049412 [4]. It makes it possible to obtain a purely macroporous, monodisperse material and not a hierarchically porous material. More specifically, this process comprises at least one step of mineralization of an oil-in-water emulsion, formed by droplets of an oily phase dispersed in a continuous aqueous phase, and in which colloidal solid particles are present at the interface. formed between the continuous aqueous phase and the droplets of the oily phase. The colloidal solid particles may be inorganic or organic. There is no mention or suggestion in this document that the colloidal solid particles may be cation exchange nanoparticles. Similarly, the use of the monoliths of this document for removing cations from a liquid effluent, particularly for removing cations from radioactive effluent radioactive elements, is neither described nor suggested. The role of the colloidal particles in this document is exclusively to stabilize the emulsion, more precisely the water-oil interface of the emulsion, to induce a monodisperse macroporosity of the material. Indeed, the macroporosity of the material, directly derives from the size of the drops of the emulsion. The size of the drops of the emulsion being monodisperse, the macroporosity of the material is consequently also very monodisperse. The role of the particles in this document is in no way to functionalize the monolith in order to confer cation exchange properties, including selective adsorbent certain cations. The objective of the material according to the invention which is to functionalize the monoliths with these nanoparticles, is neither mentioned nor suggested in this document or the role of the colloidal particles is only to stabilize the emulsion, and in no way to make the monolith reactive for use in removing cations from a solution. According to the invention, the only role of the nanoparticles used is to functionalize the monolith, and not to stabilize the emulsion used during the preparation of the material, as will be seen below in the description of the process for preparing the material according to the invention. In fact, the nanoparticles of cation exchangers, in particular of ferrocyanides used alone, do not make it possible to stabilize the emulsion and to prepare the monolith. This is why in the process according to the invention, a surfactant, in addition to the nanoparticles, is needed to stabilize the emulsion.
    [0012] For the purposes of the present invention, the term monolith means a solid object whose average dimension is at least 1 mm. Within the meaning of the present invention, macropores are understood to mean pores whose average size, generally defined by the diameter of their cross section -because the pores generally have a circular cross-section, from 4 μm to 50 μm; by mesopores are meant pores with an average size of 20 to 500 Å, preferably 20 to 300 Å; and by micropores means pores whose mean dimension is less than 20 Å, for example is 5 to 10 Å. Advantageously, the inorganic oxide is selected from oxides of at least one metal or metalloid selected from Si, Ti, Zr, Th, Nb, Ta, V, W, Y, Ca, Mg and Al.
    [0013] Preferably, the inorganic oxide is silica. The inorganic solid material exchanger of a metal cation may be chosen from all the inorganic solid materials exchangers of a metal cation known to those skilled in the art. This exchanger material is chosen according to the intended application, the nature of the liquid effluent to be treated, and in particular as a function of the metal cation or cations that it is desired to separate. Advantageously, the inorganic solid material exchanger of a metal cation is chosen from metal hexa- and octacyanometallate of formula [Alk + x] Mn + y [M '(CN),] tz-, where Alk is a monovalent cation selected of the alkali metal cations and the ammonium cation NH4 +, x is 0, 1 or 2, M is a transition metal, n is 2 or 3, y is 1, 2 or 3, M 'is a transition metal, m is 6 or 8, z is 3 or 4, and t is 1, or 2. Advantageously, Mn + is Fe 2+, Ni 2+, Fe 3+, Co 2+, Cu 2+, or Zn 2+. Advantageously, M 'is Fe2 + or Fe3 + or Co3 + and m is 6; or M 'is Mo5 + and m is 8. Advantageously, [M' (CN),] z- is [Fe (CN) 6] 3-, [Fe (CN) 6] 4-, [Co (CN) 6 ] 3-or [Mo (CN) 8] 3-. Preferably, the inorganic solid material exchanger of a metal cation has the formula [K + x] Cu 2 + y [Fe (CN) 6] Z-, for example K 2 Cu Fe (CN) 6.
    [0014] Indeed, one of the main applications targeted for the materials according to the invention is that of radioactive cesium sorbents for nuclear decontamination purposes. Ferrocyanide (and ferricyanide) nanoparticles of copper (FCCu) of general formula [K + x] Cu 2 + y [Fe (CN) 6] Z-, for example K 2 Cu Fe (CN) 6, are very selective for cesium. Their crystalline structure is cubic face-centered, and has the advantage of being able to selectively exchange a cesium atom with an unbound potassium atom present in the cell. Generally, nanoparticles have a sphere or spheroidal shape. Generally, the nanoparticles have an average size of 2 to 300 nm, preferably 2 to 100 nm, more preferably 2 to 50 nm. Generally, the nanoparticle content of the at least one inorganic metal cation exchanger solid material is 0.5 to 15% by weight, preferably 0.5 to 5% by weight. The invention furthermore relates to a method for preparing the material according to the invention which comprises at least the following steps: a) a colloidal aqueous suspension of nanoparticles of at least one inorganic solid material exchanger of a metal cation is prepared ; b) preparing an aqueous solution containing an organic surfactant and a precursor of the inorganic oxide; c) mixing the aqueous colloidal suspension prepared in step a) with the aqueous solution prepared in step b); d) an oil phase, with mechanical stirring with shear, is added to the aqueous solution prepared in stage c), whereby an oil-in-water emulsion is obtained which is formed from droplets of the oily phase dispersed in a continuous aqueous phase. and wherein the nanoparticles of the at least one inorganic solid metal cation exchanger material are present at the interface formed between the continuous aqueous phase and the droplets of the dispersed oily phase. e) the mineralization of the emulsion obtained in step d) is carried out, whereby the monolith is formed and the material according to the invention is obtained. As has already been explained above, according to the invention the sole and only role of the nanoparticles used is to functionalize the monolith and not to stabilize the emulsion used during the preparation of the material, as it is the case in the process described in document [4]. In fact, the nanoparticles of cation exchangers, especially ferrocyanides used alone, do not make it possible to stabilize the emulsion and to prepare the monolith. Therefore, in the process for preparing the material according to the invention, unlike the process described in document [4], an organic, molecular surfactant, in addition to the nanoparticles, is needed to stabilize the 'emulsion. Generally, the colloidal aqueous suspension of nanoparticles prepared in step a), has a nanoparticle concentration of 1 g / l to 50 g / l, preferably 9 g / l to 32 g / l, and its pH is generally from 5 to 6. The concentration of nanoparticles in the aqueous colloidal suspension is chosen as a function of the final concentration of nanoparticles in the solid, monolithic material.
    [0015] In the case where the inorganic solid material exchanger of a metal cation is a ferrocyanide of formula [rx] Cu2 + y [Fe (CN) 6] Z-, for example K2Cu Fe (CN) 6, the colloidal solutions of these compounds can be prepared by mixing an aqueous solution of K4Fe (CN) 6 with an aqueous solution of a copper salt such as copper nitrate. This preparation technique is advantageous because it promotes the synthesis of nanoparticles of ferrocyanides little monodisperse with average sizes generally between 10 nm and 20 nm. This technique of preparation, by mixing two aqueous solutions, of the colloidal aqueous suspension of the inorganic solid material exchanger of a metal cation, is not limited to ferrocyanides of formula [ex] Cu 2 + y [Fe (CN) 6] Z-, for example K2Cu Fe (CN) 6, and can be applied to all kinds of cation exchange materials and in particular to metal hexa- and octacyanometallate of formula [Alk + x] Ney [M '(CN),] tz-, as explained above. The aqueous solution containing an organic surfactant and a precursor of the inorganic oxide is generally prepared by adding the precursor, usually liquid, to a solution of the organic surfactant. The solution of the organic surfactant may generally have a concentration of 10 to 30% by weight, for example 20% by weight. This solution may have a pH in the region of 2, for example from 1.5 to 2.5, in particular from 1.8 to 2.2, when the inorganic solid material exchanger of a metal cation is a metal hexa- or octacyanometallate. of the above formula [Alk + x] Mn + y [W (CN) m] tz, such as a ferrocyanide of the formula [K + x] Cu2 + y [Fe (CN) 6] Z- such as K2Cu Fe (CN) 6. The pH can be adjusted to the desired value with the aid of a mineral or organic acid, preferably selected from hydrochloric acid, nitric acid, or sulfuric acid. The organic surfactant is preferably chosen from cationic and nonionic surfactants, such as Pluronics such as Pluronic P 123 marketed by BASF or SIGMA-ALDRICH. The inorganic oxide is generally chosen from oxides of metals and metalloids, and the precursor of this oxide is generally chosen from alkoxides of metals or metalloids, and salts of metals or metalloids, such as chlorides and nitrates. metals and metalloids. In the case where the inorganic oxide is silica, the precursor (s) of the silica may be chosen from tetramethoxyorthosilane (TMOS), tetraethoxyorthosilane (TEOS) and dimethyldiethoxysilane (DMDES), and mixtures thereof. The concentration of the surfactant in the aqueous solution prepared in step b) is generally 10% to 30% by weight, and the concentration of the precursor is generally 1 to 500 g / L. The pH of the aqueous solution prepared in step b) may be close to 2, for example from 1.5 to 2.5, in particular from 1.8 to 2.2. In step c), a volume of the aqueous suspension (it may also be called the aqueous solution) prepared in step a) (that is to say the aqueous colloidal suspension of nanoparticles of at least minus an inorganic solid metal cation exchanger), with a volume of the aqueous solution prepared in step b) (i.e., the aqueous solution containing an organic surfactant and a precursor of the inorganic oxide). This mixture is produced in a ratio R by volume, defined by the following relationship: R = Volume of the aqueous suspension prepared in step a) / volume of the aqueous solution prepared in step b).
    [0016] The ratio R may vary from 0 to 2, preferably from 0.1 to 2, more preferably from 0 to 1, better still from 0.1 to 1. At the end of step c), and before the step d), when the inorganic solid material exchanger of a metal cation is a metal hexa- or octacyanometallate of the formula [Alk + x] Mn + y [NA '(CN) rn] tz- exposed above, such as a ferrocyanide of formula [ex] Cu 2 + 1, [Fe (CN) 6] z, such as K 2 Cu Fe (CN) 6, the pH of the solution obtained in step c) is adjusted to around 2 (for example from 1.5 to 2.5, in particular from 1.8 to 2.2), and a step c1) is also carried out during which an aqueous solution of at least one metal fluoride, preferably dichloromethane, is added. at least one alkali metal fluoride such as KF, LiF, or NaF to the solution obtained in step c). Sodium fluoride is generally used. Step c1) is carried out when the inorganic solid material exchanger of a metal cation is a metal hexa- or octacyanometallate of the formula [Alk + x] Mn + y [M '(CN) At 2 - exposed above, such as a ferrocyanide of formula [K + x] Cu 2 + y [Fe (CN) 6] z - as K 2 Cu Fe (CN) 6. Indeed, in the applications [3] and [4] mentioned above, the pH of the preparation of the materials, or rather the pH of the aqueous phases used, and in particular of the aqueous phase of the emulsion, is close to 0. However, at such a pH, the nanoparticles of hexa- or octacyanometalate of metal of formula [Alk + x] Mn + y [M '(CN)], described above, are not stable. When using such nanoparticles, it is therefore necessary to place at a pH of the aqueous phase of the emulsion, that is to say of the solution prepared in step c) higher, generally close to 2 (for example from 1.5 to 2.5, in particular from 1.8 to 2.2), and under these conditions, the addition of at least one metal fluoride, such as NaF, is essential, otherwise during in step d) the emulsion remains liquid, the sol-gel reaction never changes to the solid, and no monolith is obtained. The solution of at least one metal fluoride, such as NaF, generally has a concentration of 1 to 40 g / l, for example 8 g / l.
    [0017] The oily phase added in step d) is generally constituted by one or more linear or branched alkanes having from 7 to 22 carbon atoms such as dodecane and hexadecane. The mechanical stirring carried out in step d) is generally carried out using an apparatus for emulsifying an Ultraturrax® disperser-homogenizer apparatus. Step d) can be described as an emulsification step of the system consisting of the solution obtained in step c) or step c1). Mechanical agitation is mechanical stirring with shear. The shear rate can range from 1 to 20000 rpm, preferably from 2000 to 15000 rpm, more preferably the shear rate is 3200 rpm. As shown in Example 2 (Figure 3), it is possible to control the size of the macroporosity of the monoliths by acting on the shear rate of the emulsion. The size of the macroporosity decreases as the shear rate increases.
    [0018] The volume fraction of the oily phase of the emulsion obtained in step d) is generally from 50% to 74%, preferably from 55% to 65% of the volume of the emulsion. In step e), the maturation, mineralization of the emulsion obtained in step d) is carried out, whereby the monolith is formed and the material according to the invention is obtained.
    [0019] This step can be carried out by leaving the emulsion obtained in step d) at rest at a temperature of 10 to 60 ° C., for example at a temperature of 40 ° C. for a time sufficient for the monolith with hierarchical porosity to become form. This duration can be for example from 2 hours to 3 weeks, for example 7 days. Generally at the end of step e), the material is washed and then dried.
    [0020] The washing makes it possible to eliminate the organic residues originating from the oily phase and which are essentially in the macropores. This washing can be carried out with an organic solvent such as THF, acetone and their mixtures. This washing can be carried out for a period of 12 to 36 hours, for example 24 hours.
    [0021] Preferably, this rinsing is carried out by bringing the organic solvent to reflux. Drying can be carried out by allowing the organic solvent used for washing at room temperature to evaporate for a period generally of 5 to 10 days, for example 7 days.
    [0022] Drying can also be performed using a supercritical fluid, such as supercritical CO2. The material according to the invention can be used in particular, but not exclusively, in a process for separating at least one metal cation from a liquid medium containing it, wherein said liquid medium is brought into contact with the material according to the invention. The materials according to the invention, because of their excellent properties such as excellent exchange capacity, excellent selectivity, high reaction rate, are particularly suitable for such use. This excellent efficiency is obtained with reduced amounts of inorganic solid material exchanger of a metal cation such as an insoluble hexacyanoferrate. In addition, the excellent properties of strength and mechanical stability of the material according to the invention, resulting from its specific structure allow its packaging in column and the continuous implementation of the separation process, which can thus be easily integrated into an installation existing, for example in a chain or processing line comprising several steps. Advantageously, said liquid medium may be an aqueous liquid medium, such as an aqueous solution. Said liquid medium may be a process liquid or an industrial effluent.
    [0023] Advantageously, said liquid medium can be selected from liquids and effluents from industry and nuclear facilities and activities using radionuclides. Generally, said cation may be present at a concentration of 0.1 picogram to 100 mg / L, preferably from 0.1 picogram to 10 mg / L.
    [0024] The term "metal" also covers the isotopes and in particular the radioactive isotopes of said metal. Preferably, the cation is a cation of an element selected from Cs, Co, Ag, Ru, Fe and Ti and the isotopes, especially radioactive thereof.
    [0025] More preferably, the cation is a cation of 134Cs, or 137Cs. This process has all the advantages intrinsically related to the material according to the invention, implemented in this process, and which have already been described above. BRIEF DESCRIPTION OF THE DRAWINGS FIG. 1 is a transmission electron microscope (TEM) photograph of the copper ferrocyanide nanoparticles which are in a colloidal solution prepared as in step 1 of the nanoparticle-containing monolith preparation protocol. The scale shown in FIG. 1 represents 20 nm. FIG. 2 is a photograph taken by transmission electron microscope (TEM) of copper ferrocyanide nanoparticles which are in a colloidal solution prepared as in step 1 of the preparation protocol for the monoliths containing nanoparticles. The scale shown in FIG. 2 represents 50 nm. FIG. 3 (A, B, C) shows photographs taken by scanning electron microscope (SEM) of silica monoliths prepared from emulsions prepared using a shear rate of 13000 rpm respectively. (A), a shear rate of 6500 rpm. (B), and a shear rate of 3200 rpm (C).
    [0026] The scales shown in Figure 3 represent 10 μm. FIG. 4 is a graph which gives the average diameter D of the macropores of monoliths (in μm), as a function of the shear rate (in min -1) used during the preparation of the emulsion used to prepare these monoliths . - Figure 5 is a photograph of a silica monolith that does not contain nanoparticles.
    [0027] Figure 6 is a photograph of a silica monolith containing 1.83 wt% nanoparticles (designated 1.83 @ 3200). Figure 7 is a graph which gives the X-ray diffraction (XRD) spectra of a massive block of particles of K2,07Cu1,08Fe (CN) 6 (CuHCF) (curve A), and of monoliths containing these nanoparticles. different concentrations, namely monolines 2,86 @ 3200 (curve B); and 5.10 @ 3200 (curve C). In ordinate is carried I (in arbitrary units) and in abscissa is carried 20 (in °). - Figure 8 is a graph that gives the total amount of adsorbed Cs (QADs) (in the left ordinate, points O and ^), and the amount of normalized adsorbed Cs (in ordinate on the right, points - and ^) which is the total amount of adsorbed Cs divided by the adsorbent mass (QADs / mADs), as a function of the mass fraction of nanoparticles in the monoliths. The (O and -) relate to the monoliths prepared from a colloidal solution whose concentration of nanoparticles, [NP], in the colloidal suspension is 9.0 g / L., And the (^ and ^) concern the monoliths prepared from a colloidal solution whose concentration of nanoparticles, [NP], in the colloidal suspension is 32.2 g / L. Figure 8 also shows the results obtained with massive ferrocyanides (-and ^).
    [0028] DETAILED DESCRIPTION OF PARTICULAR EMBODIMENTS The invention will now be described with reference to the following examples given for illustrative and non-limiting.
    [0029] EXAMPLES. In the following examples, silica monoliths containing nanoparticles of ferrocyanides are prepared and these silica monoliths containing ferrocyanides are used as ionic cesium (Cs +) sorbents.
    [0030] Example 1
    [0031] In this example, the protocol for the preparation of silica monoliths containing nanoparticles of ferrocyanides is described. The protocol for the preparation of silica monoliths containing ferrocyanide nanoparticles comprises the following successive steps: 1. Preparation of colloidal aqueous suspensions of [Kx] CuyFe (CN) nanoparticles (NP) 6. During this step, solutions are prepared, colloidal suspensions of nanoparticles (NP) of [Kx] CuyFe (CN) 6 where x is from 0.5 to 2.5 and y is from 0.5 to 2.
    [0032] The nanoparticle concentration of these solutions, suspensions can be up to 50 g / l preferably up to 32 g / l. Specifically, two solutions, colloidal suspensions were prepared for use in the following examples, namely a 9 g / L suspension. of [K1.22] Cu1, 16Fe (CN) 6 and a suspension of 32 g / L. of [<2.07] Cu1,08Fe (CN) 6.
    [0033] For this, a solution of K4Fe (CN) 6 and a solution of Cu (NO3) 2 are rapidly mixed. The respective concentrations of K4Fe (CN) 6 and Cu (NO3) 2 in each of the solutions are 5.10-3M and 3.9.10-3M to obtain a suspension at 9 g / L of [K1, 22] Cu1, 16Fe. (CN) 6 and 1,510-2M and 1,1.10-2M to obtain a suspension at 32 g / L. of [K2.02] Cu1, o8Fe (CN) 6. The stoichiometry of ferrocyanides was determined on the basis of ICP (Inductively Coupled Plasma) results. The colloidal suspensions of ferrocyanide nanoparticles obtained are stained red and are stable for months.
    [0034] These suspensions are then used as a precursor of the final material, that is to say of the silica monolith containing nanoparticles of ferrocyanide. The suspension used depends on the desired final nanoparticle concentration (NP) in the final material. The size of the NPs was determined by transmission electron microscopy (TEM).
    [0035] FIGS. 1 and 2 show images taken in transmission electron microscopy (TEM) of copper ferrocyanide nanoparticles prepared during this step: they are nanoparticles of [K1,77] Cu1,16Fe (CN) 6. This preparation technique favors the synthesis of slightly monodisperse NPs with mean sizes of between 10 and 20 nm. The colloidal solution prepared in this step is called solution A. 2. Preparation of an aqueous solution of surfactant. During this step, an aqueous solution containing 20% by weight of Pluronic® P123 (surfactant marketed by BASF® or Sigma-Aldrich®) is prepared at pH = 2. The surfactant solution prepared in this step is called solution B. 3. Preparation of a solution of a silica precursor containing a surfactant. During this step, a given volume of solution B is taken and a given volume of tetraethylorthosilicate (TEOS) is slowly added thereto. Wait 30 minutes until the solution becomes clear again. Solution C is obtained. 4. Preparation of an aqueous solution containing ferrocyanide nanoparticles, a silica precursor, and a surfactant. During this step, a given volume of solution A is mixed with a given volume of solution C. This mixing is carried out according to a ratio, volume ratio R defined by the following relationship: R = V colloidal suspension of nanoparticles / V solution P123 at 20% by weight and pH 2 (V solution A / V solution C) This ratio, R ratio can vary between 0 and 2, preferably between 0 and 1. This mixture is called solution D.30 5. During this step, add a given volume of a solution of sodium fluoride (NaF) at 8 g / I in solution D. This gives the solution E. 6. Preparation of an emulsion from the solution E. Quickly that is to say, within 15 minutes after the addition of the sodium fluoride solution which made it possible to prepare the solution E, the solution is emulsified with a given volume of dodecane (C12H26). For this purpose, an Ultraturrax® type disperser-homogenizer apparatus is used and the dodecane is slowly added to the solution E under shear. The shear rate can vary from 0 to 20000 rpm, and is preferably 3200 rpm. The volume ratios of each constituent used to prepare the emulsion are as follows: V colloidal suspension of nanoparticles (solution / suspension A) + V solution P123 at 20% by weight and pH 2 (solution B) / V TEOS / V Solution of NaF at 8g / I / V dodecane = 1.94 / 1 / 9.3.10-3 / 4.75. The emulsion F. is thus obtained. 7. Preparation of the monolith. During this so-called maturation step, the monolith containing ferrocyanide nanoparticles is prepared. For this, the solution F is placed in an oven at 40 ° C for 7 days. At the end of this stage of maturation, the monolith is formed.
    [0036] All that remains is the washing, rinsing / drying steps to be performed. 8. Washing the monolith. During this step, the monolith is placed in a cartridge of a soxhlet extractor, and rinsed for 24 hours with refluxing tetrahydrofuran (THF). 9. Drying of the monolith. During this step, the THF is slowly evaporated at room temperature for 7 days. This drying step can also be carried out using supercritical CO2.
    [0037] At the end of the drying step, a monolith loaded with ready-to-use nanoparticles is obtained. Example 2 In this example, it is shown that it is possible to control the size of the macroporosity of silica monoliths by acting on the shear rate of the emulsion during step 6 of preparing the emulsion which precedes step 7 of preparing the monoliths. This preliminary study focused on emulsions and materials that do not contain nanoparticles.
    [0038] The objective was to show that it was possible to synthesize silica monoliths whose size of the macroporosity is controlled, by acting on the shear rate of the emulsion. For this, several emulsions are prepared from the same solution E, according to step 6, by carrying out the emulsification of this solution with a given volume of dodecane (C12H26). The volume ratios of each constituent used to prepare the emulsion are as follows: 20% by weight P123 solution and pH 2 / V TE05 / VNaF_8g / 1 / V dodecane = 1.94 / 1 / 9.3 × 3/3 4.75. To prepare the emulsions, an Ultraturrax® type disperser-homogenizer apparatus is used and the dodecane is slowly added to the solution E under shear. A first emulsion is prepared using a shear rate of 13000 rpm, a second emulsion is prepared using a shear rate of 6500 rpm, and a third emulsion is prepared using a shear rate of 3200. rev / min.
    [0039] A monolith is then prepared from each of the emulsions and then washed and dried in accordance with steps 7, 8, and 9. Each monolith thus prepared is observed by scanning electron microscope (SEM).
    [0040] Scanning electron microscopy makes it possible to determine the statistical size of the macropores of the monolith, the final material. Figure 3 (A, B, C) clearly shows the effect of the shear rate of the emulsion on the size of the macroporosity of the prepared monoliths. The size of the macroporosity decreases as the shear rate increases.
    [0041] It is therefore possible to draw a kind of abacus for predicting the size of the macropores of the monolith according to the shear rate used during the preparation of the emulsion. FIG. 4 thus represents the average diameter of the macropores of the monolith as a function of the shear rate.
    [0042] Example 3. In this example, silica monoliths containing nanoparticles (NP) of ferrocyanides [Kx] CuyFe (CN) 6 where x is from 0.5 to 2.5 and y is from 0.5 to 2 are prepared.
    [0043] To prepare these monoliths, the protocol described above is used, with nanoparticle concentrations of the colloidal solution A (step 1 of the protocol) of 9 g / L. or 32 g / L., various volume ratios R (step 4 of the protocol) and a shear rate of 3200 rpm during the preparation of the emulsion (step 6 of the protocol). Table I below gives the concentrations of NP of the colloidal solutions, the values of the volume ratios R, the theoretical and measured monolith n NP concentrations (by weight), for the six monoliths containing prepared nanoparticles. 0.07 0.3 0.21 9 0.11 0.6 0.43 23 1 0.64 0 C 2.5 TABLE I NP concentrations by weight were determined by ICP / AES measurements after dissolving the monoliths. These measured NP concentration values are found to differ from the theoretical NP concentration values. This is due to the loss of part of the NP during the rinsing steps of the monoliths. The monoliths prepared all have a hierarchical porosity with both a microporosity, a mesoporosity and a macroporosity. As a result, the monoliths were also characterized by nitrogen adsorption-desorption measurements to determine their BET specific surface area (S BET) as well as the size of the mesopores and macropores. The results of these measurements are presented in Table II below. 218 383 479 547 643 2.6 2.7 2.7 2.7 3.1 6.2 4.2 4.1 4.3 8.6 5, T 5.1 TABLE II A silica monolith containing no nanoparticles (0% NP).
    [0044] Photographs of this monolith without nanoparticles and the monolith named 1.83 @ 3200 are shown respectively in Figures 5 and 6. X-ray diffraction (XRD) analyzes are then carried out on a massive block of K2, 07Cu1 particles. , o8Fe (CN) 6 (CuHCF), and monoliths containing these nanoparticles at different concentrations, namely the 2.86 @ 3200 and 5.10 @ 3200 monoliths, the results of the XRD analysis are shown in Figure 7.
    [0045] The XRD analysis confirms that the NP structure is that of a tetragonal structure of K2CuFe (CN) 6. The diffractograms relating to monoliths show that the nanoparticles are inserted in the silica network and that the structure is little modified.
    [0046] EXAMPLE 4 In this example, Cs + sorption tests were carried out on the silica monoliths containing ferrocyanide nanoparticles prepared in Example 3 or on solid copper ferrocyanide.
    [0047] The purpose of these tests is therefore to compare the exchange capacity of the monoliths charged with NP with that of the corresponding solid copper ferrocyanide. In these tests, ferrocyanides are used as specific sorbents for ionic cesium (Cs +). Indeed, they contain a potassium ion in the crystal mesh which is specifically exchanged with a cesium ion.
    [0048] The sorption tests summarized below are carried out according to a standardized protocol. This protocol comprises the following successive steps: 1. A solution containing 1.10-3M of CH3COONa and 1.10-4M of CsNO3 is prepared. This solution is called solution G. 2. 10 mg of monolith, or 10 mg of solid copper ferrocyanide, are taken and immersed in 20 ml of the preceding solution G. 3. Shake for 24 hours. 4. The supernatant is removed, filtered, and the Cs content is measured by ion chromatography.
    [0049] This protocol makes it possible to quantify the exchange capacity of the monoliths while ensuring the selectivity of materials for cesium vis-à-vis sodium. In all the experiments whose results are grouped together, in Figure 8, the sodium concentration was identical before and after immersion of the material in solution G.
    [0050] After stirring for 24 hours, the adsorption equilibrium is reached, which makes it possible to compare the experiments with each other. Figure 8 also shows the advantage of using NPs rather than a massive adsorbent. If the amount of Cs extracted is normalized by the mass of adsorbent present in the material, it appears that the materials with the lowest concentration of NP are the most effective. This is explained by the fact that when the adsorbent is in nanometric form, the specific surface area available for cesium is higher. The increase in the mass fraction in NP must promote their aggregation and the adsorption mechanism in the monolith then becomes more and more similar to that observed in the case of massive copper ferrocyanides. The shift observed for the two solid ferrocyanides is due to the different elemental potassium proportions in both cases. In the case of solid ferrocyanide originating from the 32.2 g / L colloidal solution, there is on average 2.07 potassium atoms per mole whereas in the case of that resulting from the 9.0 g / L solution, L., there is only 1.77. The number of potassium atoms exchangeable with cesium is therefore different, which explains this shift. Example 5 In this example, 137Cs + sorption tests were carried out on the silica monoliths containing ferrocyanide nanoparticles prepared in Example 3, or on solid copper ferrocyanide. In the case of experiments on radioactive Cs, the concentrations are much lower than in the case of non-radioactive Cs. The parameter making it possible to estimate the level of decontamination of a radioactive solution by a sorbent material is then the distribution coefficient Kd. It is expressed as follows: Ao Aeg V Kd = Aeq mmat With Kd distribution coefficient (ml / g); Ao, initial activity of the solution to be decontaminated; Aeq activity at equilibrium after 24 hours of contact time; V volume of decontaminant solution used (ml); and mmat mass of sorbent material used (in g).
    [0051] To evaluate the selectivity of the monoliths vis-à-vis other competitive Cs Cs, a complex radioactive solution was prepared with the following composition: Ao = 41.2 kBq / L ([Cs] = 104 ° mol / L) [Na] = 0.652 mol / L [o. 0.0015 mol / L [Mg 2 +] = 0.002 mol / L [NO 3 -] = 0.542 mol / L [SO 4 2-] = 0.008 mol / L [PO 4 -] = 0.105 mol / L The results are shown in Table III below : Sample 0.21 @ 3200 1.83 @ 3200 5.10 @ 3200 Kd (ml / g) 2.4 103 3.0 104 1.1 105 Massive 32g / L 3.1 106 TABLE III The results show that Monoliths capture 137Cs very selectively against other competing cations. Kd are very high irrespective of the NPs concentrations of immobilized ferrocyanides in monoliths. The effectiveness of the monoliths is thus validated on radioactive solutions representative of the solutions that must be treated during a real accidental case, for example the effluents from the Fukushima Daiichi plant that contain seawater.
    权利要求:
    Claims (19)
    [0001]
    REVENDICATIONS1. Solid material in the form of an alveolar monolith consisting of a matrix of an inorganic oxide with open hierarchical porosity comprising macropores, mesopores, and micropores, said macropores, mesopores, and micropores being interconnected, and nanoparticles at least one inorganic solid material exchanger of a metal cation being distributed in said porosity.
    [0002]
    2. Material according to claim 1, wherein the inorganic oxide is chosen from the oxides of at least one metal or metalloid selected from Si, Ti, Zr, Th, Nb, Ta, V, W, Y, Ca, Mg. et al.
    [0003]
    3. The material of claim 2, wherein the inorganic oxide is silica.
    [0004]
    4. Material according to any one of the preceding claims, in which the inorganic solid material exchanger of a metal cation is chosen from metal hexa- and octacyanometallate of formula [Alk + x] Mn + y [M '(CN) where Alk is a monovalent cation selected from the alkali metal cations and the ammonium cation NH4 +, x is 0, 1 or 2, M is a transition metal, n is 2 or 3, y is 1, 2 or 3, M 'is a transition metal, m is 6 or 8, z is 3 or 4, and t is 1, or 2.
    [0005]
    5. The material of claim 4, wherein Mn + is Fe2 +, Ni2 +, Fe3 +, Co2 +, Cu2 +, or ZI12 +.
    [0006]
    6. The material of claim 4 or 5, wherein M 'is Fe2 + or Fe3 + or Co3 + and m is 6; or M 'is Mo5 + and m is 8.
    [0007]
    Material according to any one of claims 4 to 6, wherein [M '(CN),] z- is [Fe (CN) 6] 3-, [Fe (CN) 6] 4-, [Co ( CN) 6] 3-or [Mo (CN) 8] 3-.
    [0008]
    8. The material of claim 4, wherein the inorganic solid material exchanger of a metal cation has the formula [ex] Cu2 + y [Fe (CN) 6] Z-, for example K2Cu Fe (CN) 6.
    [0009]
    9. Material according to any one of claims 1 to 8, wherein the nanoparticles have a sphere or spheroidal shape.
    [0010]
    10. Material according to any one of the preceding claims, wherein the nanoparticles have an average size, such as a diameter, of 2 to 300 nm, preferably 2 to 100 nm, more preferably 2 to 50 nm.
    [0011]
    11. The material as claimed in any one of the preceding claims, in which the nanoparticle content of the at least one inorganic solid material exchanging a metal cation is 0.5 to 15% by weight, preferably 0.5 to 5% by weight. % in weight.
    [0012]
    12. Process for preparing the material according to any one of claims 1 to 11 which comprises at least the following steps: a) a colloidal aqueous suspension of nanoparticles of at least one inorganic solid material exchanger of a metal cation is prepared; b) preparing an aqueous solution containing an organic surfactant and a precursor of the inorganic oxide; c) mixing the aqueous colloidal suspension prepared in step a) with the aqueous solution prepared in step b); d) an oil phase, with mechanical stirring with shear, is added to the aqueous solution prepared in stage c), whereby an oil-in-water emulsion is obtained which is formed from droplets of the oily phase dispersed in a continuous aqueous phase. and wherein the nanoparticles of the at least one inorganic solid metal cation exchanger material are present at the interface formed between the continuous aqueous phase and the droplets of the dispersed oily phase. e) the mineralization of the emulsion obtained in step d) is carried out, whereby the monolith is formed and the material according to the invention is obtained.
    [0013]
    13. The method of claim 12, wherein, after step c) and before step d), when the inorganic solid material exchanger of a metal cation is a hexa- or octacyanometallate metal of formula [Alk +, j1Wy [M '(CN),] tz-, where Alk is a monovalent cation selected from alkali metal cations and the ammonium cation NH4 +, x is 0, 1 or 2, M is a transition metal, n is 2 or 3, y is 1, 2 or 3, M 'is a transition metal, m is 6 or 8, z is 3 or 4, and t is 1, or 2, such as a ferrocyanide of formula [rx ] Cu2 + y [Fe (CN) 6] z-, like K2Cu Fe (CN) 6, the pH of the solution obtained in step c) is adjusted to around 2, and a step ) during which an aqueous solution of at least one metal fluoride such as sodium fluoride is added to the solution obtained in step c).
    [0014]
    14. Process for separating at least one metal cation from a liquid medium containing it, wherein said liquid medium is brought into contact with the material according to any one of claims 1 to 11.
    [0015]
    The method of claim 14, wherein said liquid medium is an aqueous liquid medium, such as an aqueous solution.
    [0016]
    16. The method of claim 14 or 15, wherein said liquid medium is selected from liquids and effluents from industry and nuclear facilities and activities using radionuclides.
    [0017]
    The method of any one of claims 14 to 16, wherein said cation is present at a concentration of 0.1 picogram to 100 mg / L, preferably 0.1 picogram to 10 mg / L.
    [0018]
    18. A process according to any one of claims 14 to 17, wherein the cation is a cation of an element selected from Cs, Co, Ag, Ru, Fe and Tl and isotopes, including radioactive thereof.
    [0019]
    19. The method of claim 18, wherein the cation is a 134Cs, or 137Cs cation.
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    公开号 | 公开日
    FR3015476B1|2016-02-12|
    EP3083524B1|2018-01-31|
    JP6581986B2|2019-09-25|
    WO2015091677A1|2015-06-25|
    JP2017503741A|2017-02-02|
    EP3083524A1|2016-10-26|
    CA2933984A1|2015-06-25|
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    KR20160102259A|2016-08-29|
    引用文献:
    公开号 | 申请日 | 公开日 | 申请人 | 专利标题
    WO2008129151A2|2007-02-14|2008-10-30|Universite Pierre Et Marie Curie|Hybrid material, and method for the production thereof|
    RU2008125922A|2008-06-25|2009-12-27|Институт химии Дальневосточного отделения Российской академии наук |COLLOID-RESISTANT NANO-SIZED SORBENT FOR DEACTIVATION OF SOLID BULK MATERIALS AND METHOD OF DEACTIVATION OF SOLID BULK MATERIALS WITH ITS USE|
    EP2546841A1|2010-03-08|2013-01-16|Consejo Superior De Investigaciones Científicas |Method for obtaining materials with superparamagnetic properties|FR3106507A1|2020-01-28|2021-07-30|Commissariat A L'energie Atomique Et Aux Energies Alternatives|SOLID MATERIAL WITH MULTIPLE OPEN POROSITY CONSISTING OF A GEOPOLYMER AND SOLID PARTICLES AND ITS PREPARATION PROCESS|JPH022615B2|1982-11-10|1990-01-18|Tokyo Shibaura Electric Co|
    DE69608820T2|1996-03-08|2000-11-16|Minnesota Mining & Mfg|ADSORPTION AGENT FOR CAESUMIONS AND METHOD FOR THEIR PRODUCTION|
    US6232504B1|1998-12-29|2001-05-15|University Of Delaware|Functionalized monolith catalyst and process for production of ketenes|
    WO2008031108A2|2006-09-08|2008-03-13|Cornell Research Foundation, Inc.|Sol-gel precursors and products thereof|
    WO2008057382A2|2006-11-02|2008-05-15|Industrial Science & Technology Network Inc.|Nanopore reactive adsorbents for the high-efficiency removal of waste species|
    KR100864313B1|2007-05-21|2008-10-20|한국화학연구원|Preparation of surface functionalized porous organic-inorganic hybrid materials or mesoporous materials with coordinatively unsaturated metal sites and its catalytic applications|
    FR2929264B1|2008-03-31|2010-03-19|Inst Francais Du Petrole|INORGANIC MATERIAL FORM OF SPHERICAL PARTICLES OF SPECIFIC SIZE AND HAVING METALLIC NANOPARTICLES TRAPPED IN A MESOSTRUCTURED MATRIX|
    FR2945756B1|2009-05-20|2011-08-05|Commissariat Energie Atomique|NANOCOMPOSITE SOLID MATERIAL BASED ON HEXA AND OCTACYANOMETALLATES, PROCESS FOR PREPARING THE SAME, AND METHOD FOR FIXING MINERAL POLLUTANTS USING THE SAME|
    FR2947564B1|2009-07-06|2011-07-22|Univ Paris Curie|HETEROGENEOUS ENZYMATIC CATALYST, PROCESS FOR PREPARATION AND USE|
    FR2965807B1|2010-10-11|2012-12-21|Centre Nat Rech Scient|PROCESS FOR PREPARING ALVEOLAR INORGANIC MONOLITHIC MATERIALS AND USES THEREOF|
    WO2013062989A2|2011-10-24|2013-05-02|Metamateria Technologies, Llc|Porous composite media for removing phosphorus from water|FR3025799B1|2014-09-12|2016-10-14|Commissariat Energie Atomique|PROCESS FOR THE PREPARATION OF A SOLID NANOCOMPOSITE MATERIAL BASED ON HEXA- AND OCTACYANOMETALLATES OF ALKALI METALS|
    FR3033359B1|2015-03-02|2017-04-07|Snecma|MONOBLOC DRAWING DISK HAVING A HUB HAVING AN EVIDENCE FACED BY A BODY COMPRISING SAME|
    FR3038523B1|2015-07-10|2017-07-21|Commissariat Energie Atomique|PROCESS FOR THE SELECTIVE SEPARATION OF A METAL CATION FROM AN AQUEOUS LIQUID MEDIUM|
    FR3055558B1|2016-09-08|2022-01-14|Commissariat Energie Atomique|SOLID NANOCOMPOSITE MATERIAL BASED ON HEXA- OR OCTACYANOMETALLATES OF ALKALINE METALS, METHOD FOR PREPARING IT, AND METHOD FOR EXTRACTION OF METALLIC CATIONS.|
    FR3062126A1|2017-01-24|2018-07-27|Commissariat A L'energie Atomique Et Aux Energies Alternatives|NANOPARTICLES HAVING A HEART STRUCTURE IN A PRESS SHELL BLUE ANALOGUE, METHOD FOR THE PREPARATION THEREOF, MATERIALS COMPRISING SAME, AND PROCESS FOR EXTRACTING METAL CATIONS.|
    FR3084104B1|2018-07-20|2020-10-23|Safran Aircraft Engines|RIGIDIFIED PLATFORM|
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    FR1363329A|FR3015476B1|2013-12-20|2013-12-20|CATIONIC EXCHANGER INORGANIC MONOLITHIC ALTERNATIVES, PROCESS FOR THEIR PREPARATION, AND SEPARATION PROCESS USING SAME.|FR1363329A| FR3015476B1|2013-12-20|2013-12-20|CATIONIC EXCHANGER INORGANIC MONOLITHIC ALTERNATIVES, PROCESS FOR THEIR PREPARATION, AND SEPARATION PROCESS USING SAME.|
    EP14824815.6A| EP3083524B1|2013-12-20|2014-12-17|Inorganic cellular monobloc cation-exchange materials, the preparation method thereof, and separation method using same|
    JP2016539212A| JP6581986B2|2013-12-20|2014-12-17|Inorganic porous monolithic cation exchange material, preparation method thereof, and separation method using the same|
    PCT/EP2014/078275| WO2015091677A1|2013-12-20|2014-12-17|Inorganic cellular monobloc cation-exchange materials, the preparation method thereof, and separation method using same|
    KR1020167019878A| KR20160102259A|2013-12-20|2014-12-17|Inorganic cellular monobloc cation-exchange materials, the preparation method thereof, and separation method using same|
    CA2933984A| CA2933984A1|2013-12-20|2014-12-17|Inorganic cellular monobloc cation-exchange materials, the preparation method thereof, and separation method using same|
    US15/106,089| US10541060B2|2013-12-20|2014-12-17|Inorganic cellular monobloc cation-exchange materials, the preparation method thereof, and separation method using same|
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