Next Article in Journal
Summary of Research Progress on Metallurgical Utilization Technology of Red Mud
Next Article in Special Issue
Recent Work on the Recovery of Rare Earths Using Ionic Liquids and Deep Eutectic Solvents
Previous Article in Journal
Ce and Nd Extraction by Cationic Exchange, Using Bentonite, Diatomite, and Eggshell—Preliminary Study
Previous Article in Special Issue
Simulation of Solvent Extraction Circuits for the Separation of Rare Earth Elements
 
 
Search for Articles:
Title / Keyword
Author / Affiliation / Email
Journal
Article Type
 
 
Advanced Search
 
Section
Special Issue
Volume
Issue
Number
Page
 
Journals
Minerals
Volume 13
Issue 6
10.3390/min13060736
minerals-logo
Submit to this Journal Review for this Journal Propose a Special Issue
► Article Menu

Article Menu

share Share announcement Help format_quote Cite question_answer Discuss in SciProfiles thumb_up
...
Endorse textsms
...
Comment
first_page
settings
Order Article Reprints
Font Type:
Arial Georgia Verdana
Font Size:
Aa Aa Aa
Line Spacing:
Column Width:
Background:
Article

Extraction of Lanthanides(III) from Aqueous Nitric Acid Solutions with Tetra(n-octyl)diglycolamide into Methyltrioctylammonium Bis(trifluoromethanesulfonul)imide Ionic Liquid and Its Mixtures with Molecular Organic Diluents

by
Alexander N. Turanov
1,*,
Vasilii K. Karandashev
2 and
Vladimir E. Baulin
3
1
Osipyan Institute of Solid State Physics, Russian Academy of Sciences, Chernogolovka, Moscow 142432, Russia
2
Institute of Microelectronics Technology and High Purity Materials, Russian Academy of Sciences, Chernogolovka, Moscow 142432, Russia
3
Institute of Physiologically Active Substances, Russian Academy of Sciences, Chernogolovka, Moscow 142432, Russia
*
Author to whom correspondence should be addressed.
Minerals 2023, 13(6), 736; https://doi.org/10.3390/min13060736
Submission received: 11 April 2023 / Revised: 25 May 2023 / Accepted: 27 May 2023 / Published: 29 May 2023
(This article belongs to the Special Issue Solvent Extraction of Rare-Earth Elements with Ionic Liquids and Deep Eutectic Solvents)
Browse Figures
Versions Notes

Abstract

:
The extraction of lanthanides(III) from aqueous nitric acid solutions with tetra(n-octyl)diglycolamide into methyltrioctylammonium bis(trifluoromethanesulfonul)imide ([N1888][Tf2N]) ionic liquid and its mixtures with molecular organic diluents is investigated in this study. This study also investigates the effect of HNO3 concentration in the aqueous phase on the extraction of Ln(III) ions. Subsequently, the stoichiometry of the extracted complexes is determined, and the mechanism of Ln(III) extraction in a system with [N1888][Tf2N] is discussed. It is shown that the intragroup selectivity of the extraction of Ln(III) ions is significantly higher when using [N1888][Tf2N] than when using the imidazolium-based ionic liquid [C4mim][Tf2N].

1. Introduction

Individual rare earth elements (REEs) and their compounds are widely used in various modern industries, as well as for the production of radiopharmaceuticals. The growing consumption of rare earth elements and their compounds necessitates the processing of mineral raw materials with a low content of rare earth elements, as well as industrial end-of-life wastes [1,2,3]. The separation of REEs is a difficult task because of the closeness of the physicochemical properties of these elements. In the hydrometallurgy of REEs, various methods are used for their extraction, separation, and purification from impurities, such as fractional precipitation and crystallization, selective redox, adsorption, ion exchange, membrane processes, solvent extraction, and others. Compared to other methods, solvent extraction has a number of advantages, such as the ability to carry out the extraction process in a continuous, multi-step mode, which is easy to automate and has high productivity. Extraction methods with the use of organophosphorus and carboxylic acids, neutral mono- and polydentate organophosphorus compounds, are widely used to extract, concentrate, and separate REEs [4,5,6,7]. Nevertheless, the search for new effective and selective extractants continues.
In recent decades, interest in the use of alkylsubstituted diglycol-amides (DGA) as extractants has increased. These compounds exhibit high extraction ability with respect to lanthanide and actinide ions in nitric acid medium [8,9,10,11,12,13,14,15,16]. They act as tridentate ligands since they contain three oxygen atoms. The advantages of DGA as compared to bidentate-neutral organophosphorus compounds are ease of synthesis, milder requirements for stripping, and the harmless chemical composition of completely incinerable elements. The hydrophobicity of DGA extractants is controlled by the length of the alkyl radicals linked to the amidic N atoms. The octyl chains of N,N,N,N′,N′-tetraoctyldiglycolamide (TODGA) give the molecule sufficient lipophilicity to dissolve in various organic diluents. The efficiency of Ln(III) extraction with TODGA largely depends on the nature of the organic diluent [11]. A significant disadvantage of DGA is its tendency to aggregate in solutions of non-polar organic solvents, which leads to the formation of a third phase during the extraction of metal ions from nitric acid solutions. This seriously complicates the process of REE extraction. To eliminate this phenomenon, various modifiers such as high-molecular-weight alcohols, tributyl phosphate, and others are added to the organic phase [14].
In recent years, ionic liquids (ILs), due to their extremely low volatility, noncombustibility, and excellent solvating properties, have been considered a possible replacement for conventional molecular organic diluents in various extraction areas, including spent nuclear fuel reprocessing [17,18,19,20,21,22,23,24,25,26,27,28,29,30,31]. In addition, it has been found that the simple replacement of traditional molecular solvents with IL increases the extraction efficiency of many known neutral extractants. Nakashima et al. [19] showed that the extractability and selectivity of the lanthanide cations with octylphenyl-N,N-diisobutylcarbamoylmethyl-phosphine oxide (CMPO) dissolved in [C4mim][PF6] or [C4mim][Tf2N] significantly increased compared to CMPO solutions in conventional organic diluents. The undoubted advantage of using IL as a solvent is the absence of the formation of a third phase in the extraction of actinides and REEs from nitric acid solutions with TODGA [14].
A number of studies have studied the extraction behavior of actinides and lanthanides in DGA-IL systems [32,33,34,35,36]. DGA extractant solutions in [Cnmim][PF6] and ([Cnmim][Tf2N] (n = 4, 6, 8, and 10) efficiently extract lanthanides and actinides from aqueous solutions under reduced acidity, while traditional organic solvents such as chloroform show insignificant extraction. However, in DGA-[Cnmim][Tf2N] systems, low intragroup selectivity was observed, which greatly hindered their application for the separation of rare earth elements in nitric acid media [33].
The addition of even small amounts of ILs to a solution of neutral extractants in conventional molecular diluents leads to a significant increase in the extraction efficiency of metal ions. In the extraction of alkaline earth cations, actinides, and lanthanides from aqueous nitric acid solutions in the presence of a small amount of IL in the organic phase containing DGA ligands [37,38,39], CMPO-type ligands [40], and a pillar[5]arene-based phosphine oxide [41], a significant synergetic effect was observed. A large number of possible “extractant—IL—molecular diluent” mixtures enable the development of new extraction systems for separating and preconcentrating metal ions. This allows for maintaining the high efficiency and selectivity of extraction processes with IL and eliminates significant cost increases.
In a number of studies, the effect of the nature of the cation and anion of ILs on the efficiency of the extraction of metal ions was studied. It was established that an increase in the hydrophobicity of the IL anion enables an increase in the extraction efficiency [20]. On the contrary, an increase in the hydrophobicity of the IL cation is accompanied by a decrease in the extraction of metal ions. It was shown that an increase in the length of the alkyl substituent in the [Cnmim]+ cation leads to a sharp decrease in the extraction of Am(III) and Eu(III) by CMPO solutions in IL [42]. Hence, only when using IL diluents with relatively short alkyl chain radicals attached to the cationic part of the ILs, a significant increase in the extraction efficiency of neutral donor ligands with respect to metal ions is observed. However, because of their appreciable solubility in aqueous solutions, IL ions contaminate the aqueous phase. This disadvantage, as well as the high cost and viscosity of ILs, significantly complicates their wide-scale use as diluents. Therefore, a very urgent task is to find ways to minimize the loss of IL to the aqueous phase.
Recently, the use of alkylammonium ILs for metal ion extraction has attracted increasing attention. These ILs are more hydrophobic than imidazolium-based ILs due to the presence of alkyl radicals that are attached to the cationic N atom [43]. In addition, the alkylammonium ILs are easy to prepare and cheaper than imidazolium-based ILs. The extraction of Eu(III) with N,N,N′,N′-tetra(2-ethylhexyl)diglycolamide (T2EHDGA) into [N1444][Tf2N] was studied [44]. However, there are no data on the selectivity of Ln(III) extraction in systems with alkylammonium ILs. In addition, there are no data on the effect of these ILs on the extraction of Ln(III) with solutions of DGA in molecular organic diluents.
This paper describes the results of our studies on the simultaneous extraction of lanthanides(III) with TODGA into methyltrioctylammonium bis(trifluoromethanesulfonul)imide ([N1888][Tf2N]) ionic liquid and its mixtures with molecular organic diluents. Scheme 1 shows the structures of TODGA and [N1888][Tf2N].

2. Materials and Methods

All starting materials for the synthesis of the extractants TODGA and methyltrioctylammonium bis(trifluoromethanesulfonul)imide ionic liquid were purchased from Sigma-Aldrich (St. Louis, MO, USA) and were used without further purification. Chemical and analytical grade nitrobenzene, 1-octanol, chloroform, n-nonane, tri-n-butyl phosphate, and 1,2-dichloroethane were purchased from Vekton (Saint Petersburg, Russian Federation). Stock aqueous solutions of lanthanides(III) were prepared from single-element standard solutions (High Purity Standards, North Charleston, SC, USA). High-purity nitric acid (65%) was purchased from Merck, Germany. Deionized water after the NANOPURE purification system (Thermo Scientific, North Charleston, SC, USA) with a specific resistivity of 18 MΩ was used to prepare all aqueous solutions.
N,N,N′,N′-tetra(n-octyl)diglycolamide (TODGA) N,N,N,N′,N′-tetra(n-octyl)diglycolamide (TODGA) was synthesized and then purified according to the method described in [45]. Trioctylmethylammonium bis(trifluoromethylsulfonyl)imide was obtained by the procedure given in [46].
The Ln(III) concentration in the initial and equilibrium aqueous solutions was determined by inductively coupled plasma mass spectrometry (ICP-MS) on an XSeries II mass spectrometer (Thermo Scientific, Waltham, MA, USA). The Tf2N− anion concentration in equilibrium aqueous solutions was determined by inductively coupled plasma atomic emission spectrometry (ICP-AES) on an iCAP-6500 spectrometer (Thermo Scientific, Waltham, MA, USA). The concentration of HNO3 in the equilibrium aqueous phase was determined by potentiometric titration of H+ with a standard NaOH solution.

Extraction Procedure

Extractant solutions were prepared using precisely weighed portions. Initial aqueous solutions of Ln(III) were prepared by diluting stock aqueous solutions with water and adding HNO3 to the desired concentration. All lanthanides(III) (except for Pm) were presented in the initial aqueous phase. The initial concentration of each Ln(III) was 2 μM.
Metal ion extraction experiments were performed in plastic tubes at room temperature (21 ± 2 °C) and a volume ratio of aqueous vs. organic phases of 1:1. The organic and aqueous phases were mixed on a rotary mixer at 60 rpm for 1 h. To separate the phases, the tubes with the extract were centrifuged, and then aliquots of each phase were sampled for further analysis.
The Ln(III) concentration in the initial and equilibrium aqueous solutions was determined by ICP-MS. The content of lanthanides(III) in the organic phase was determined as the difference between the initial ([Ln]init) and equilibrium ([Ln]aq) concentrations of metal ions in the aqueous phase. Since this difference was very small in some cases, the concentration of metal ions in the organic phase ([Ln]org) was determined by ICP-MS after the stripping of Ln(III). In this work, an aqueous solution of 0.1 M of 1-hydroxyethane-1,1-diphosphonic acid was used as a stripping agent. It is known that this reagent forms very stable complexes with Ln(III) ions in aqueous solutions [47]. The Ln(III) stripping was carried out at a volume ratio of organic and aqueous phases of 1:1. It was found that the sum of the metal ion concentrations in the aqueous phases after extraction and back-extraction was well in agreement with the initial concentration of metal ions. Consequently, virtually total Ln(III) stripping has been achieved. The values of the distribution coefficient (DLn) were calculated as [Ln]org/[Ln]aq. At least three replicate measurements were carried out. The measurement error of D usually does not exceed 10%.

3. Results and Discussion

3.1. Solubility of [N1888][Tf2N] in Aqueous HNO3 Solutions

In order to evaluate the transfer of [N1888][Tf2N] components into an aqueous phase during the extraction of metal ions, the distribution of Tf2N− ions between IL and aqueous solutions of nitric acid was considered. An increase in the HNO3 concentration in the aqueous phase leads to an increase in the Tf2N− concentration in the aqueous phase, meaning an increase in the IL transition into the aqueous phase (Figure 1, Table S1). This may be due to the formation of IL with nitrate ions, which have a significantly lower hydrophobicity than Tf2N− ions. In the case of IL [N1888][Tf2N], the process of equilibrium can be described by the equation
H+ + NO3− + [N1888][Tf2N](org) ⇌ [N1888][NO3](org) + Tf2N− + H+
where components with the index (org) and those without an index refer to the organic and aqueous phases, respectively.
It should be noted that in the system with [N1888][Tf2N], the transfer of Tf2N− ions into the aqueous phase occurs to a much lesser extent than in systems with imidazolium ILs used in the solvent extraction of metal ions. Thus, during extraction from the 3 M HNO3 solution, the concentration of the Tf2N− ion in the aqueous phase when using [N1888][Tf2N] is 0.0009 M, and when using IL [C4mim][Tf2N], it is 0.047 M [48].

3.2. Effect of the Composition of the Aqueous Phase on the Ln(III) Extraction with TODGA into [N1888][Tf2N]

The composition of the aqueous phase has a significant effect on the extraction of metal ions with neutral donor extractants. At the extraction of Ln(III) with TODGA solutions in low-polarity organic solvents, an increase in DLn is observed with an increase in the concentration of HNO3 in the aqueous phase [8]. It was found that both the unbound TODGA (L) and its complex HNO3L take part in the complexation with Ln(III) ions when polar organic diluents are used [40]. In this case, the extraction of Ln(III) with TODGA into the organic phase from the nitric acid solution through the solvation mechanism can be described using the following equation:
Ln3+ + 3NO3− + (s-n)L(org) + nHNO3L(org) ⇌ LnLs-n(HNO3L)n(NO3)3(org)
where s is a solvation number equal to 2 or 3.
The nature of the logDLn-log[HNO3] dependence changes sharply upon extraction with DGA solutions in ILs. The effect of the HNO3 concentration in the equilibrium aqueous phase on the extraction of Ln(III) ions with TODGA into [N1888][Tf2N] is shown in Figure 2 (Table S2). An increase in the concentration of HNO3 in the aqueous phase is accompanied by a decrease in the distribution ratios of Ln(III). A similar dependence of D on the acidity of the aqueous phase was previously observed during the extraction of Ln(III), alkaline earth metals, and U(VI) with neutral DGA extractants [32,33,34,35] dissolved in imidazolium ILs, as well as the extraction of Eu(III) with T2EHDGA into [N1444][Tf2N] [44].
The extraction of Ln(III) ions into the organic phase containing the neutral ligand TODGA into [N1888][Tf2N], according to the cation exchange mechanism, can be described by the following equilibrium:
Ln3+ + sL(org) + 3[N1888][Tf2N](org) ⇌ LnLs(Tf2N)3(org) + 3N1888+
It follows from this equation that, formally, the efficiency of the Ln(III) extraction does not depend on the concentration of HNO3 in the aqueous phase. However, the effect of the concentration of H+ and NO3− ions in the aqueous phase is significantly different. As can be seen from the data in Figure 3 (Table S3), at a constant acidity of the aqueous phase, an increase in the concentration of NO3− ions in the aqueous phase does not lead to a significant change in the Ln(III) distribution ratios. Some decrease in DLn with an increase in the concentration of nitrate ions can be due to a shift in equilibrium (1) to the right, leading to an increase in the concentration of [N1888][NO3] in the organic phase. Consequently, there will be an increase in the concentration of N1888+ ions in the aqueous phase, leading to a shift in equilibrium (3) to the left and, consequently, a decrease in DLn.
On the other hand, an increase in the acidity of the aqueous phase at a constant concentration of NO3− ions is accompanied by a sharp decrease in the Ln(III) distribution ratios (Figure 4, Table S4). This may be due to the protonation of the TODGA molecule and the formation of TODGA complexes with NO3− and Tf2N− ions. Moreover, the molar fraction of the latter in the ionic liquid phase is significantly higher since TODGA interacts more actively with HTf2N than with HNO3. This is indicated by the difference in the values of the extraction constants of these acids with TODGA into dichloroethane (KHNO3 = 0.625 [39], KHTf2N = 14,100 [37]). Therefore, the process of extraction of Ln(III) ions by the cation exchange mechanism can be described by the following equilibrium:
Ln3+ + sLHTf2N(org) ⇌ LnLs(Tf2N)3(org) + sH+

3.3. Effect of TODGA Concentration in the IL Phase on the Extraction of Ln(III)

In order to determine the stoichiometric ratio of Ln(III): TODGA in the extracted complexes, the dependence of the distribution ratios of Ln(III) on the concentration of TODGA in IL during extraction from aqueous solutions with a constant concentration of nitric acid was studied. The plot of logDLn vs. log[L] shows straight lines with a slope close to 3 (Figure 5, Table S5). This indicates that three TODGA molecules are coordinated to Ln(III) ions in the IL phase. Similar results were obtained for the extraction of Eu(III) with T2EHDGA into [N1444][Tf2N] ionic liquid [44].
Since [N1888][Tf2N] itself does not extract Ln(III) from nitric acid solutions (log D < −2), and increasing the concentration of nitrate ions in the aqueous phase has almost no effect on the efficiency of the Ln(III) extraction with TODGA into the IL phase, it can be assumed that Ln(III) are extracted in the Ln(III)-HNO3-TODGA-IL system in the form of LnL3(Tf2N)3 complexes. The inclusion of Tf2N− anions into such complexes leads to the formation of extractable complexes of a more hydrophobic nature in comparison with the complexes formed with nitrate ions. Previously, Rao et al. based on luminescence spectroscopy studies, confirmed the coordination of T2EHDGA in the first coordination sphere of Eu(III) and the expulsion of water molecules from the coordination sphere [44]. We assume that the Tf2N− anions, which have weak coordination ability [49], are located in the outer coordination sphere of the extracted complexes. Large Tf2N− anions are incompatible with the strongly hydrogen-bonded structure of water in the aqueous phase, which makes their transfer to the organic phase more energetically favorable compared to smaller nitrate anions. However, the experimental extraction data in the present study do not allow us to characterize the exact structure of the extracted species. Further spectroscopic study would provide helpful information about the postulated extracted metal complexes.

3.4. Selectivity of Ln(III) Extraction with TODGA into [N1888][Tf2N]

At a moderate concentration of HNO3 in the equilibrium aqueous phase, the extraction of Ln(III) with TODGA into [N1888][Tf2N] increases as the atomic number (Z) of lanthanides increases (Figure 6, Table S6). On the whole, this order of extractability in the series of lanthanides is typical for ligands of the DGA type [15] in nitric acid systems. The dependence of logDLn on Z trend was explained by an increase in the positive charge density of Ln3+ ions as their ionic radii decreased with increasing Z.
The selectivity of Ln(III) extraction with TODGA solutions can be characterized by the separation factor of Lu over La (SFLu/La = DLu/DLa). From the data on the Ln(III) extraction from 3 M HNO3 solution with TODGA into ionic liquids [N1888][Tf2N] and [C4mim][Tf2N], as well as the molecular organic solvent 1,2-dichloroethane (DCE), it follows that the systems with imidazolium IL are characterized by low selectivity. The SFLu/La value in systems with [C4mim][Tf2N] is 0.76, while in the DCE system the SFLu/La is 275. Previously, it was shown that the selectivity of Ln(III) extraction from HNO3 solutions with N,N,N′,N′-tetrabutyldiglycolamide into [C4mim][Tf2N] is significantly lower than when using octanol as a diluent [33].
The use of alkylammonium IL [N1888][Tf2N] as a diluent leads not only to an increase in the efficiency of Ln(III) extraction but also to an increase in the selectivity of their separation. The SFLu/La value in the system with [N1888][Tf2N] is 144. Therefore, the use of alkylammonium IL [N1888][Tf2N] as a diluent not only leads to a significant decrease in the transfer of IL components to the aqueous phase but also to an increase in the efficiency and selectivity of Ln(III) extraction compared to imidazolium ILs.

3.5. Extraction of Lanthanides(III) from Aqueous Nitric Acid Solutions with Mixtures of TODGA and [N1888][Tf2N] in Molecular Organic Diluents

It was previously established that the addition of even small amounts of [C4mim][Tf2N] to a solution of DGA ligands [37,38,39] in conventional molecular diluents leads to a significant increase in the efficiency of the extraction of Ln(III) ions. This effect was associated with the high hydrophobicity of the IL anions, Tf2N−, which are involved in the formation of extractable complexes as counterions. Therefore, in this work, we consider the effect of [N1888][Tf2N] on the extraction of Ln(III) ions with solutions of TODGA in molecular organic diluents.
It can be seen from Figure 7 (Table S7) that the addition of [N1888][Tf2N] to the organic phase leads to a significant increase in the extraction of Ln(III) with solutions of TODGA in DCE. Since the IL itself does not extract Ln(III) under these conditions, it can be said that this system exhibits a synergistic effect—a non-additive increase in the distribution ratios of metal ions, which is often used to increase the efficiency of the metal ion extraction [50,51]. The synergistic enhancement of the Ln(III) extraction produced by TODGA—[N1888][Tf2N] mixtures can be determined using synergistic coefficients (SC) calculated as
SC = D(L+IL)/(D(L) + D(IL))+
where D(L), D(IL), and D(L+IL) are the distribution ratios of the metal ion with TODGA and [N1888][Tf2N] taken separately and with their mixtures, respectively.
The SC values in the system with [N1888][Tf2N] increase from 9.5 for La(III) to 52.5 for Lu(III). It is obvious that the extraction of more hydrated heavy Ln(III) ions is most sensitive to the participation of hydrophobic Tf2N− anions in the formation of the extracted Ln(III) complexes. In addition, the intragroup selectivity of Ln(III) extraction in the presence of IL increases significantly. The SFLu/La values during extraction from the 4 M NH4NO3 solution with TODGA solutions in DCE without and with [N1888][Tf2N] are 31.6 and 174, respectively.
The effect of the nature of the organic diluent on the extraction of Ln(III) is considered. As can be seen from the data in Figure 8 (Table S8), the efficiency of Ln(III) extraction increases in the series chloroform < nonane–1.1 M TBP < DCE < octanol < nitrobenzene. The addition of TBP to nonane was carried out to prevent the formation of a third phase.
The effect of the HNO3 concentration in the equilibrium aqueous phase on the extraction of Ln(III) ions with TODGA solutions in DCE and in the 1.1 M TBP solution in nonane containing the [N1888][Tf2N] additive, as well as in these solvents without IL, is shown in Figure 9 (Table S9). The addition of [N1888][Tf2N] to the organic phase leads to a significant increase in the extraction of Ln(III) with solutions of TODGA in DCE. In the case of using the 1.1 M TBP solution in nonane, the synergistic effect is less pronounced. An increase in the concentration of HNO3 in the aqueous phase is accompanied by a decrease in the SC value. The same nature of the SC—[HNO3] dependence was observed earlier in the extraction of Ln(III) ions with TODGA in DCE in the presence of an [C4mim][Tf2N] additive [38].
The data on the Ln(III) extraction from a 3 M acid solution with solutions of TODGA in DCE and nonane containing 1.1 M TBP in the presence of 0.1 M [N1888][Tf2N] are shown in Figure 10 (Table S10). It can be seen from these data that the distribution ratios of Ln(III) in these systems are higher than in the extraction of Ln(III) with TODGA in undiluted [N1888][Tf2N] (Figure 6). In addition, the selectivity of Ln(III) extraction with TODGA solutions in molecular solvents containing IL is higher than that of Ln(III) extraction with TODGA in undiluted [N1888][Tf2N] IL. The SFLu/La values in the systems TODGA—DCE—IL, TODGA—nonane—TBP—IL, and TODGA—IL are 2630, 320, and 144, respectively.

4. Conclusions

The Ln(III) extraction from aqueous nitric acid solutions with tetra(n-octyl)diglycolamide (TODGA) into methyltrioctylammonium bis(trifluoromethanesulfonul)imide ([N1888][Tf2N]) ionic liquid is studied. The high hydrophobicity of this IL leads to a significant decrease in the transfer of IL components into the aqueous phase compared to imidazolium-based ILs. The use of [N1888][Tf2N] as a diluent leads to a significant increase in the efficiency of lanthanides(III) extraction with TODGA compared to conventional organic solvents. This is due to the high hydrophobicity of IL anions, Tf2N−, which are involved in the formation of the extracted complexes as counter ions. The stoichiometry of the extracted complexes is determined, and the effect of the composition of the aqueous phase is studied. The use of alkylammonium IL [N1888][Tf2N] as a diluent leads not only to an increase in the efficiency of Ln(III) extraction but also to an increase in the selectivity of their separation. This study demonstrates a significant synergistic effect in the extraction of lanthanides(III) from aqueous HNO3 solutions with TODGA dissolved in molecular organic diluents in the presence of [N1888][Tf2N]. In these systems, the distribution ratios of Ln(III) are higher than in the case of extraction of Ln(III) with TODGA into undiluted [N1888][Tf2N]. The results of this work can be used to develop technologies for the recovery and separation of rare earth elements from various objects, for example, industrial end-of-life wastes. This requires additional studies, including the determination of the capacity of the extractant solution, the study of the influence of accompanying metal ions, and a detailed study of the stripping stage and reuse of the extractant. We believe that solutions containing water-soluble complexing agents, such as ethylenediaminetetraacetic acid (EDTA) or diethylenetriamine pentaacetate (DTPA), can be used for the REEs stripping.

Supplementary Materials

The following supporting information can be downloaded at: https://www.mdpi.com/article/10.3390/min13060736/s1, Table S1: The effect of HNO3 concentration in the aqueous phase on the transfer of Tf2N− ions into the aqueous phase; Table S2: The effect of HNO3 concentrations in the aqueous phase on the extraction of Ln(III) with 0.01 M solutions of TODGA in [N1888][Tf2N]; Table S3: The effect of NO3− concentrations in the aqueous phase on the extraction of Ln(III) with 0.01 M solutions of TODGA in [N1888][Tf2N]. [H+] = 2 M; Table S4: The effect of H+ concentrations in the aqueous phase on the extraction of Ln(III) with 0.01 M solutions of TODGA in [N1888][Tf2N]. [NO3−] = 4 M; Table S5: The effect of TODGA concentration in [N1888][Tf2N] on the extraction of lanthanides(III) from 3 M HNO3 solutions; Table S6: The extraction of lanthanides(III) from 3 M HNO3 solutions with 0.01 M TODGA solutions in [N1888][Tf2N], [C4mim][Tf2N], and dichloroethane (DCE); Table S7: The extraction of lanthanides(III) from 4 M NH4NO3 solutions with 0.01 M TODGA solutions in DCE and DCE containing 0.01 M [N1888][Tf2N]; Table S8: The extraction of lanthanides(III) from 1 M HNO3 solutions with 0.01 M TODGA solutions in nitrobenzene (NB), octanol (OC), dichloroethane (DCE), nonane containing 1.1 M TBP (N/TBP), and chloroform (CL) in the presence of 0.01 M [N1888][Tf2N]; Table S9: The effect of HNO3 concentrations in the aqueous phase on the extraction of Eu(III) with 0.01 M solutions of TODGA (L) in DCE, nonane containing 1.1 M TBP, and DCE in the presence of 0.1 M [N1888][Tf2N]; Table S10: The extraction of lanthanides(III) from 3 M HNO3 solutions with 0.01 M TODGA solutions in DCE, nonane containing 1.1 M TBP, and DCE in the presence of 0.1 M [N1888][Tf2N].

Author Contributions

Conceptualization, A.N.T.; methodology, A.N.T., V.K.K. and V.E.B.; formal analysis, A.N.T., V.K.K. and V.E.B.; writing—original draft preparation, A.N.T., V.K.K. and V.E.B.; writing—review and editing, A.N.T., V.K.K. and V.E.B.; supervision A.N.T., V.K.K. and V.E.B. All authors have read and agreed to the published version of the manuscript.

Funding

This work was performed within the framework of the government assignment for the ISSP RAS, IMTHPM RAS, and IPAC RAS and was financially supported by the Ministry of Science and Higher Education of the Russian Federation.

Data Availability Statement

Not applicable.

Conflicts of Interest

The authors declare no conflict of interest.

References

  1. Balaram, V. Rare earth elements: A review of applications, occurrence, exploration, analysis, recycling, and environment impact. Geosci. Front. 2019, 10, 1285–1303. [Google Scholar] [CrossRef]
  2. Rho, B.-J.; Sun, P.-P.; Cho, S.-Y. Recovery of neodymium and praseodymium from nitrate-based leachate of permanent magnet by solvent extraction with trioctylphosphine oxide. Sep. Purif. Technol. 2020, 238, 116429. [Google Scholar] [CrossRef]
  3. Liu, H.; Li, S.; Wang, B.; Wang, K.; Wu, R.; Ekberg, C.; Volinsky, A.A. Multiscale recycling rare earth elements from real waste trichromatic phosphors containing glass. J. Clean. Prod. 2019, 238, 117998. [Google Scholar] [CrossRef]
  4. Liu, T.; Chen, J. Extraction and separation of heavy of rare earth elements: A review. Sep. Purif. Technol. 2021, 276, 119263. [Google Scholar] [CrossRef]
  5. Wei, H.; Li, Y.; Zhang, Z.; Liao, W. Synergistic solvent extraction of heavy rare earth from chloride media using mixture of HEHHAP and Cyanex272. Hydrometallurgy 2020, 191, 105242. [Google Scholar] [CrossRef]
  6. Leonchini, A.; Huskens, J.; Verboom, W. Ligands for f-element extraction used in the nuclear fuel cycle. Chem. Soc. Rev. 2017, 46, 7229–7273. [Google Scholar] [CrossRef]
  7. Hidayah, N.N.; Abidin, S.Z. The evolution of mineral processing in extraction of rare earth elements using liquid-liquid extraction: A review. Miner. Eng. 2018, 121, 146–157. [Google Scholar] [CrossRef]
  8. Sasaki, Y.; Sugo, Y.; Suzuki, S.; Tachimori, S. The novel extractants, diglycolamides, for the extraction of lanthanides and actinides in HNO3–n-dodecane system. Solvent Extr. Ion Exch. 2001, 19, 91–103. [Google Scholar] [CrossRef]
  9. Tachimori, S.; Sasaki, Y.; Suzuki, S. Modification of TODGA–n-dodecane solvent with monoamide for high loading of lanthanides(III) and actinides(III). Solvent Extr. Ion Exch. 2002, 20, 687–699. [Google Scholar] [CrossRef]
  10. Ansari, S.A.; Pathak, P.N.; Manchanda, V.K.; Husain, M.; Prasad, A.K.; Parmar, V.S. N,N,N′,N′-tetraoctyldiglycolamide (TODGA): A promising extractant for actinide-partitioning from high-level waste (HLW). Solvent Extr. Ion Exch. 2005, 23, 463–479. [Google Scholar] [CrossRef]
  11. Sasaki, Y.; Rapold, P.; Arisaka, M.; Hirata, M.; Kimura, T. An additional insight into the correlation between the distribution ratios and the aqueous acidity of the TODGA system. Solvent Extr. Ion Exch. 2007, 25, 187–204. [Google Scholar] [CrossRef]
  12. Sasaki, Y.; Sugo, N.; Morita, Y.; Nash, K.L. The effect of alkyl substituents on actinide and lanthanide extraction by diglycolamide compounds. Solvent Extr. Ion Exch. 2015, 33, 625–641. [Google Scholar] [CrossRef]
  13. Mowafy, E.A.; Mohamed, D. Extraction behavior of trivalent lanthanides from nitric acid medium by selected structurally related diglycolamides as novel extractants. Sep. Purif. Technol. 2014, 128, 18–24. [Google Scholar] [CrossRef]
  14. Ansari, S.A.; Pathak, P.N.; Mohapatra, P.K.; Manchanda, V.K. Chemistry of diglycolamides: Promising extractants for actinide partitioning. Chem. Rev. 2012, 112, 1751–1772. [Google Scholar] [CrossRef]
  15. Chen, Z.; Yang, X.; Song, L.; Wang, X.; Xiao, Q.; Feng, Q.; Ding, S. Extraction and complexation of trivalent rare earth elements with tetralkyl diglycolamides. Inorg. Chim. Acta 2020, 513, 119928. [Google Scholar] [CrossRef]
  16. Mowafy, E.A.; Alshammari, A.; Mohamed, D. Extraction behavior of critical trivalent rare earth elements with novel selected structurally related diglycolamides. Solvent Extr. Ion Exch. 2022, 40, 387–411. [Google Scholar] [CrossRef]
  17. Huddleston, J.G.; Willauer, H.D.; Swatloski, R.P.; Visser, A.E.; Rogers, R.D. Room temperature ionic liquids as novel media for “clean” liquid-liquid extraction. Chem. Commun. 1998, 16, 1765–1766. [Google Scholar] [CrossRef]
  18. Dai, S.; Yu, Y.H.; Barnes, C.E. Solvent extraction of strontium nitrate by a crown ether using room temperature ionic liquids. J. Chem. Soc. Dalton Trans. 1999, 8, 1201–1202. [Google Scholar] [CrossRef]
  19. Nakashima, K.; Kubota, F.; Maruyama, T.; Goto, M. Feasibility of ionic liquids as alternative for industrial solvent extraction processes. Ind. Eng. Chem. Res. 2005, 44, 4368–4372. [Google Scholar] [CrossRef]
  20. Luo, H.; Dai, S.; Bonnesen, P.V.; Haverlock, T.J.; Moyer, B.A.; Buchanan, A.C., III. A striking effect of ionic-liquid anions in the extraction of Sr2+ and Cs+ by dicyclohexano-18-crown-6. Solvent Extr. Ion Exch. 2006, 24, 19–31. [Google Scholar] [CrossRef]
  21. Dietz, M.L. Ionic liquids as extraction solvents: Where do we stand? Sep. Sci. Technol. 2006, 41, 2047–2063. [Google Scholar] [CrossRef]
  22. Billard, I.; Ouadi, A.; Gaillard, C. Liquid-liquid extraction of actinides, lanthanides, and fission products by use of ionic liquids: From discovery to understanding. Anal. Bioanal. Chem. 2011, 400, 1555–1566. [Google Scholar] [CrossRef]
  23. Kolarik, Z. Ionic Liquids: How far do they extend the potential of solvent extraction of f-elements? Solvent Extr. Ion Exch. 2013, 31, 24–60. [Google Scholar] [CrossRef]
  24. Shkrob, I.A.; Marin, T.W.; Jensen, M.P. Ionic liquid based separation of trivalent lanthanide and actinide ions. Ind. Eng. Chem. Res. 2014, 53, 3641–3653. [Google Scholar] [CrossRef]
  25. Atanassova, M. Solvent extraction chemistry in ionic liquids: An overview of f-ions. J. Mol. Liq. 2021, 343, 117530. [Google Scholar] [CrossRef]
  26. Iqbal, M.; Waheed, K.; Rahat, S.B.; Mehmood, T.; Lee, M.S. An overview of molecular extractants in room temperature ionic liquids and task specific ionic liquids for the partitioning of actinides/lanthanides. J. Radioanal. Nucl. Chem. 2020, 325, 1–31. [Google Scholar] [CrossRef]
  27. Wang, K.; Adidharma, H.; Radosz, M.; Wang, P.; Xu, X.; Russell, C.K.; Tian, H.; Fan, M.; Yu, J. Recovery of rare earth elements with ionic liquids. Green Chem. 2017, 19, 4469–4493. [Google Scholar] [CrossRef]
  28. Arrachart, G.; Couturier, J.; Dourdain, S.; Levard, C.; Pellet-Rostaing, S. Recovery of rare earth elements (REEs) using ionic liquids. Processes 2021, 9, 1202. [Google Scholar] [CrossRef]
  29. Prusty, S.; Pradhan, S.; Mishra, S. Ionic liquids as an emerging alternative for the separation and recovery of Nd, Sm and Eu using solvent extraction technique—A review. Sustain. Chem. Pharm. 2021, 21, 100434. [Google Scholar] [CrossRef]
  30. Quijada-Maldonado, E.; Romero, J. Solvent extraction of rare-earth elements with ionic liquids: Toward a selective and sustainable extraction of these valuable elements. Curr. Opin. Green Sustain. Chem. 2021, 27, 100428. [Google Scholar] [CrossRef]
  31. Parmentier, D.; Hoogestraete, T.V.; Metz, S.J.; Binnemans, K.; Kroon, M.C. Selective extraction of metals from chloride solutions with the tetraoctylphosphonium oleate ionic liquid. Ind. Eng. Chem. Res. 2015, 54, 5149–5158. [Google Scholar] [CrossRef]
  32. Shimojo, K.; Kurahashi, K.; Naganawa, H. Extraction behavior of lanthanides using a diglycolamide derivative TODGA in ionic liquids. Dalton Trans. 2008, 37, 5083–5088. [Google Scholar] [CrossRef] [PubMed]
  33. Mincher, M.E.; Quach, D.L.; Liao, Y.J.; Mincher, B.J.; Wai, C.M. The partitioning of americium and lanthanides using tetrabutyldiglycolamide (TBDGA) in octanol and ionic liquid solution. Solvent Extr. Ion Exch. 2012, 30, 735–747. [Google Scholar] [CrossRef]
  34. Panja, S.; Mohapatra, P.K.; Tripathi, S.C.; Gandhi, P.M.; Janardan, P. A highly efficient solvent system containing TODGA in room temperature ionic liquids for actinide extraction. Sep. Purif. Technol. 2012, 96, 289–295. [Google Scholar] [CrossRef]
  35. Chen, Q.; Lu, C.; Hu, Y.; Liu, Y.; Zhou, Y.; Jiao, C.; Zhang, M.; Hou, H. Extraction behavior of several lanthanides from nitric acid with DMDODGA in [C4mim][NTf2] ionic liquid. J. Radioanal. Nucl. Chem. 2021, 327, 565–573. [Google Scholar] [CrossRef]
  36. Mohapatra, P.K. Diglycolamide-based solvent systems in room temperature ionic liquids for actinide ion extraction: A review. Chem. Prod. Process Model. 2015, 10, 135–145. [Google Scholar] [CrossRef]
  37. Turanov, A.N.; Karandashev, V.K.; Baulin, V.E. Extraction of alkaline earth metal ions with TODGA in the presence of ionic liquids. Solvent Extr. Ion Exch. 2010, 28, 367–387. [Google Scholar] [CrossRef]
  38. Turanov, A.N.; Karandashev, V.K.; Khvostikov, V.A. Synergistic extraction of lanthanides(III) with mixtures of TODGA and hydrophobic ionic liquid into molecular diluent. Solvent Extr. Ion Exch. 2017, 35, 461–479. [Google Scholar] [CrossRef]
  39. Turanov, A.N.; Karandashev, V.K.; Boltoeva, M.; Gaillard, C.; Mazan, V. Synergistic extraction of uranium(VI) with TODGA and hydrophobic ionic liquid mixtures in molecular diluent. Sep. Purif. Technol. 2016, 164, 97–106. [Google Scholar] [CrossRef]
  40. Turanov, A.N.; Karandashev, V.K.; Sharova, E.V.; Genkina, G.K.; Artyushin, O.I.; Baimukhanova, A. Effect of ionic liquid on the extraction of actinides and lanthanides with 1,2,3-triazole-modified carbamoylmethylphosphine oxide from nitric acid solutions. Radiochim. Acta 2018, 106, 355–362. [Google Scholar] [CrossRef]
  41. Gan, Q.; Cai, Y.; Fu, K.; Yuan, L.; Feng, W. Effect of ionic liquid on the extraction of uranium with pillar[5]arene-based phosphine oxide from nitric acid solutions. Radiochim. Acta 2020, 108, 239–247. [Google Scholar] [CrossRef]
  42. Sun, T.; Zhang, Y.; Wu, Q.; Chen, J.; Xia, L.; Xu, C. Comparative study on the extraction of trivalent americium and europium by CMPO in imidazolium-based ionic liquids and dodecane. Solvent Extr. Ion Exch. 2017, 35, 408–422. [Google Scholar] [CrossRef]
  43. Rout, A.; Ramanathan, N. Liquid-liquid extraction of europium(III) in an alkyl ammonium based ionic liquid containing diglycolamic acid. J. Mol. Liq. 2020, 319, 114016. [Google Scholar] [CrossRef]
  44. Rao, C.V.; Rout, A.; Venkatesan, K.A. Europium(III) complexation behavior in an alkyl ammonium ionic liquid medium containing neutral extractants. Sep. Purif. Technol. 2019, 213, 545–552. [Google Scholar] [CrossRef]
  45. Sasaki, Y.; Choppin, G.R. Solvent extraction of Eu, Th, U, Np and Am with N,N′-dimethyl-N,N′-dihexyl-3-oxapentanediamide and its analogous compounds. Anal. Sci. 1996, 12, 225–230. [Google Scholar] [CrossRef]
  46. Katsuta, S.; Yoshimoto, Y.; Okai, M.; Takeda, Y.; Bessho, K. Selective extraction of palladium and platinum from hydrochloric acid solutions by trioctylammonium-based mixed ionic liquids. Ind. Eng. Chem. Res. 2011, 50, 12735–12740. [Google Scholar] [CrossRef]
  47. Nash, K.L.; Horwitz, E.P. Stability constants for europium(III) complexes with substituted methane diphosphonic acids in acid solutions. Inorg. Chim. Acta 1990, 169, 245–252. [Google Scholar] [CrossRef]
  48. Gaillard, C.; Boltoeva, M.; Billard, I.; Georg, S.; Mazan, V.; Ouadi, A.; Ternova, D.; Henning, C. Insights into the mechanism of extraction of uranium (VI) from nitric acid solution into an ionic liquid by using tri-n-butyl phosphate. ChemPhysChem 2015, 16, 2653–2662. [Google Scholar] [CrossRef]
  49. Binnemans, K. Lanthanides and actinides in ionic liquids. Chem. Rev. 2007, 107, 2592–2614. [Google Scholar] [CrossRef]
  50. Bond, A.H.; Dietz, M.L.; Chiarizia, R. Incorporating size selectivity into synergistic solvent extraction: A review of crown ether-containing system. Ind. Eng. Chem. Res. 2000, 39, 3442–3464. [Google Scholar] [CrossRef]
  51. Atanassova, M.; Kurteva, V. Synergism as a phenomenon in solvent extraction of 4f-elements with calixarenes. RSC Adv. 2016, 6, 11303–11324. [Google Scholar] [CrossRef]
Minerals 13 00736 sch001 550
Scheme 1. The structure of TODGA and [N1888][Tf2N].
Scheme 1. The structure of TODGA and [N1888][Tf2N].
Minerals 13 00736 sch001
Minerals 13 00736 g001 550
Figure 1. The effect of HNO3 concentration in the aqueous phase on the transfer of Tf2N− ions into the aqueous phase.
Figure 1. The effect of HNO3 concentration in the aqueous phase on the transfer of Tf2N− ions into the aqueous phase.
Minerals 13 00736 g001
Minerals 13 00736 g002 550
Figure 2. The effect of HNO3 concentrations in the aqueous phase on the extraction of Ln(III) with 0.01 M solutions of TODGA in [N1888][Tf2N]. The sizes of the points represent error bars.
Figure 2. The effect of HNO3 concentrations in the aqueous phase on the extraction of Ln(III) with 0.01 M solutions of TODGA in [N1888][Tf2N]. The sizes of the points represent error bars.
Minerals 13 00736 g002
Minerals 13 00736 g003 550
Figure 3. The effect of NO3− concentrations in the aqueous phase on the extraction of Ln(III) with 0.01 M solutions of TODGA in [N1888][Tf2N]. [H+] = 2 M. The sizes of the points represent error bars.
Figure 3. The effect of NO3− concentrations in the aqueous phase on the extraction of Ln(III) with 0.01 M solutions of TODGA in [N1888][Tf2N]. [H+] = 2 M. The sizes of the points represent error bars.
Minerals 13 00736 g003
Minerals 13 00736 g004 550
Figure 4. The effect of H+ concentrations in the aqueous phase on the extraction of Ln(III) with 0.01 M solutions of TODGA in [N1888][Tf2N]. [NO3−] = 4 M. The sizes of the points represent error bars.
Figure 4. The effect of H+ concentrations in the aqueous phase on the extraction of Ln(III) with 0.01 M solutions of TODGA in [N1888][Tf2N]. [NO3−] = 4 M. The sizes of the points represent error bars.
Minerals 13 00736 g004
Minerals 13 00736 g005 550
Figure 5. The effect of TODGA concentration in [N1888][Tf2N] on the extraction of lanthanides(III) from 3 M HNO3 solutions. The sizes of the points represent error bars.
Figure 5. The effect of TODGA concentration in [N1888][Tf2N] on the extraction of lanthanides(III) from 3 M HNO3 solutions. The sizes of the points represent error bars.
Minerals 13 00736 g005
Minerals 13 00736 g006 550
Figure 6. The extraction of lanthanides(III) from 3 M HNO3 solutions with 0.01 M TODGA solutions in [N1888][Tf2N], [C4mim][Tf2N] a, and dichloroethane (DCE) a. The sizes of the points represent error bars. a Data from ref. [40].
Figure 6. The extraction of lanthanides(III) from 3 M HNO3 solutions with 0.01 M TODGA solutions in [N1888][Tf2N], [C4mim][Tf2N] a, and dichloroethane (DCE) a. The sizes of the points represent error bars. a Data from ref. [40].
Minerals 13 00736 g006
Minerals 13 00736 g007 550
Figure 7. The extraction of lanthanides(III) from 4 M NH4NO3 solutions with 0.01 M TODGA solutions in DCE and DCE containing 0.01 M [N1888][Tf2N]. The sizes of the points represent error bars.
Figure 7. The extraction of lanthanides(III) from 4 M NH4NO3 solutions with 0.01 M TODGA solutions in DCE and DCE containing 0.01 M [N1888][Tf2N]. The sizes of the points represent error bars.
Minerals 13 00736 g007
Minerals 13 00736 g008 550
Figure 8. The extraction of lanthanides(III) from 1 M HNO3 solutions with 0.01 M TODGA solutions in nitrobenzene, octanol, DCE, nonane, containing 1.1 M TBP, and chloroform in the presence of 0.01 M [N1888][Tf2N]. The sizes of the points represent error bars.
Figure 8. The extraction of lanthanides(III) from 1 M HNO3 solutions with 0.01 M TODGA solutions in nitrobenzene, octanol, DCE, nonane, containing 1.1 M TBP, and chloroform in the presence of 0.01 M [N1888][Tf2N]. The sizes of the points represent error bars.
Minerals 13 00736 g008
Minerals 13 00736 g009 550
Figure 9. The effect of HNO3 concentrations in the aqueous phase on the extraction of Eu(III) with 0.01 M solutions of TODGA in DCE, nonane, containing 1.1 M TBP, and in DCE, nonane, containing 1.1 M TBP in the presence of 0.1 M [N1888][Tf2N]. The sizes of the points represent error bars.
Figure 9. The effect of HNO3 concentrations in the aqueous phase on the extraction of Eu(III) with 0.01 M solutions of TODGA in DCE, nonane, containing 1.1 M TBP, and in DCE, nonane, containing 1.1 M TBP in the presence of 0.1 M [N1888][Tf2N]. The sizes of the points represent error bars.
Minerals 13 00736 g009
Minerals 13 00736 g010 550
Figure 10. The extraction of lanthanides(III) from 3 M HNO3 solutions with 0.01 M TODGA solutions in DCE, nonane, containing 1.1 M TBP, and in DCE, nonane, containing 1.1 M TBP in the presence of 0.1 M [N1888][Tf2N]. The sizes of the points represent error bars.
Figure 10. The extraction of lanthanides(III) from 3 M HNO3 solutions with 0.01 M TODGA solutions in DCE, nonane, containing 1.1 M TBP, and in DCE, nonane, containing 1.1 M TBP in the presence of 0.1 M [N1888][Tf2N]. The sizes of the points represent error bars.
Minerals 13 00736 g010
Disclaimer/Publisher’s Note: The statements, opinions and data contained in all publications are solely those of the individual author(s) and contributor(s) and not of MDPI and/or the editor(s). MDPI and/or the editor(s) disclaim responsibility for any injury to people or property resulting from any ideas, methods, instructions or products referred to in the content.

Share and Cite

MDPI and ACS Style

Turanov, A.N.; Karandashev, V.K.; Baulin, V.E. Extraction of Lanthanides(III) from Aqueous Nitric Acid Solutions with Tetra(n-octyl)diglycolamide into Methyltrioctylammonium Bis(trifluoromethanesulfonul)imide Ionic Liquid and Its Mixtures with Molecular Organic Diluents. Minerals 2023, 13, 736. https://doi.org/10.3390/min13060736

AMA Style

Turanov AN, Karandashev VK, Baulin VE. Extraction of Lanthanides(III) from Aqueous Nitric Acid Solutions with Tetra(n-octyl)diglycolamide into Methyltrioctylammonium Bis(trifluoromethanesulfonul)imide Ionic Liquid and Its Mixtures with Molecular Organic Diluents. Minerals. 2023; 13(6):736. https://doi.org/10.3390/min13060736

Chicago/Turabian Style

Turanov, Alexander N., Vasilii K. Karandashev, and Vladimir E. Baulin. 2023. "Extraction of Lanthanides(III) from Aqueous Nitric Acid Solutions with Tetra(n-octyl)diglycolamide into Methyltrioctylammonium Bis(trifluoromethanesulfonul)imide Ionic Liquid and Its Mixtures with Molecular Organic Diluents" Minerals 13, no. 6: 736. https://doi.org/10.3390/min13060736

APA Style

Turanov, A. N., Karandashev, V. K., & Baulin, V. E. (2023). Extraction of Lanthanides(III) from Aqueous Nitric Acid Solutions with Tetra(n-octyl)diglycolamide into Methyltrioctylammonium Bis(trifluoromethanesulfonul)imide Ionic Liquid and Its Mixtures with Molecular Organic Diluents. Minerals, 13(6), 736. https://doi.org/10.3390/min13060736

Note that from the first issue of 2016, this journal uses article numbers instead of page numbers. See further details here.

Article Metrics

Back to TopTop