Next Article in Journal
An ATM/CHK2 Signaling Pathway Induces Nuclear Translocation of SRPK2 in Cisplatin-Treated HeLa Cells
Previous Article in Journal
In Silico Analysis and Experimental Evaluation of Ester Prodrugs of Ketoprofen for Oral Delivery: With a View to Reduce Toxicity
 
 
Search for Articles:
Title / Keyword
Author / Affiliation / Email
Journal
Article Type
 
 
Advanced Search
 
Section
Special Issue
Volume
Issue
Number
Page
 
Journals
Processes
Volume 9
Issue 12
10.3390/pr9122222
processes-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

Solvent Extraction of Lanthanides(III) in the Presence of the Acetate Ion Acting as a Complexing Agent Using Mixtures of Cyanex 272 and Caprylic Acid in Hexane

by
Vera V. Belova
,
Yulia V. Tsareva
,
Yulia A. Zakhodyaeva
,
Vladimir K. Ivanov
and
Andrey A. Voshkin
*
Kurnakov Institute of General and Inorganic Chemistry, Russian Academy of Sciences, 31 Leninsky Prospect, 119991 Moscow, Russia
*
Author to whom correspondence should be addressed.
Processes 2021, 9(12), 2222; https://doi.org/10.3390/pr9122222
Submission received: 4 November 2021 / Revised: 3 December 2021 / Accepted: 7 December 2021 / Published: 9 December 2021
(This article belongs to the Section Chemical Processes and Systems)
Browse Figures
Versions Notes

Abstract

:
A new extraction system containing a mixture of Cyanex 272 and caprylic acid is proposed for the extraction and separation of lanthanides(III). It was shown that this system possesses a high level of extraction ability and capacity. The extraction of lanthanides(III) from chloride-acetate and nitrate-acetate media was investigated on an example of La(III). The composition of the extracted species was confirmed, based on the analysis of lanthanum(III) extraction isotherms. In the case of acetic-acetate aqueous solutions, a decrease in lanthanum(III) extraction efficiency was observed, due to the decreasing equilibrium pH of the aqueous phase in accordance with the cation-exchange mechanism. The composition of the synergistic mixture of Cyanex 272-caprylic acid established demonstrates highly efficient separation of rare-earth metal ions.

1. Introduction

Rare earth elements (REE) find their application in many fields of advanced materials science and industry as they demonstrate a variety of promising and unique properties (for example, luminescent, electronic, magnetic, and catalytic properties) [1,2,3,4,5].
The separation of lanthanides is a challenging goal, due to their similar chemical and physical behavior. In recent years, there have been a growing number of studies on the recovery and separation of lanthanides using a variety of methods, among which special attention has been paid to liquid-liquid extraction [6,7,8,9,10,11]. Liquid-liquid extraction is the most common large-scale separation method, which is usually carried out as a continuous, multi-stage process of extraction and separation of REE from aqueous solutions using an organic solvation agent (extractant) that forms complexes with REE ions. Rare earth metals are then stripped from the REE-enriched organic phase by putting it in contact with an aqueous solution with which ions have a greater affinity. Due to the very small behavioral difference between lanthanides, the extraction-stripping process should be repeated multiple times to achieve satisfactory separation. Usually, solvent extraction is followed by precipitation of REE as a salt (e.g., carbonate, oxalate) or hydroxide, filtering, washing, drying (or calcination) and grinding. Extractants of various classes have recently been used for REE extraction and separation, for example, organophosphorus cation-exchange extractants [12,13,14,15], neutral extractants (e.g., TBP, trialkylphosphine oxides) [16,17,18,19], binary extractants and ionic liquids [20,21,22,23,24,25,26].
The most widely used acidic organophosphorus extractants for REE are 2-ethylhexylphosphonic acid mono-2-ethylhexyl ester (EHEHPA), di(2,4,4-trimethylpentyl)phosphinic acid (Cyanex 272) and di(2-ethylhexyl)phosphoric acid (DEHPA) [27,28,29,30]. Previously, the extraction of REE from chloride solutions was studied using organophosphorus acids 2-ethylhexylphosphonic acid mono-(2-ethylhexyl) ester (HEHEHP) combined with DEHPA, isopropylphosphonic acid 1-hexyl-4-ethyloctyl ester, Cyanex 272, bis(2,4,4-trimethypentyl)-monothiophosphinic acid (Cyanex 302) or bis(2,4,4-trimethypentyl)dithiophosphinic acid (Cyanex 301) as extractants. It was found that HEHEHP and Cyanex 272 could be used for the separation of Tm(III), Yb(III) and Lu(III) from the other rare earth elements [27]. Acidic extractants are usually saponified in the organic phase by the addition of bases, in order to speed up the extraction, and then REE are stripped from the organic phase using acidic aqueous solutions during the subsequent step. Synergistic extraction of heavy REE was observed in chloride media when mixing (2-ethylhexylamino)methylphosphonic acid mono-2-ethylhexyl ester (HEHAMP) and EHEHPA. The maximum synergistic enhancement factors of Lu(III), Yb(III), Tm(III), Er(III), Y(III) and Ho(III) were 2.89, 2.76, 2.54, 2.14, 2.14 and 2.06, respectively, at a mole fraction of HEHAMP equal to 0.5 [28]. Different extractants and their mixtures were investigated for Pr(III) extraction from chloride media [29]. Among all the combinations, mixtures of Cyanex 301 with Cyanex 921 or Cyanex-923 demonstrated a synergistic effect on the extraction of praseodymium. Different extractants (Cyanex 272, DEHPA, EHEHPA and Cyanex 301) were tested for the separation of La from Pr and Nd from synthetic chloride leach liquor [30]. Cyanex 272 demonstrated a better extraction affinity toward Pr and Nd than La. Saponification of Cyanex 272 favored the separation of La from Pr and Nd.
The practical application of Cyanex 272 is restricted by its low loading capacity, because of its high pKa value [31], and the low lipophilicity of the extracted species. In this regard, a number of synergistic extractant systems have been suggested for overcoming the low extractability of Cyanex 272 and much attention has been paid to systems containing several extractants. Thus, the synergistic extraction of Pr and Nd was achieved with the binary mixtures of Cyanex 272 and tertiary amines [31,32,33]. Among the extractant mixtures studied, the combination of Cyanex 272 and Alamine 336 showed the best extraction ability, and the highest synergistic enhancement factors were observed at a Cyanex 272 mole fraction of 0.5. The quantitative stripping of REE from the organic phase was found to be possible by using solutions of mineral acids. A binary extractant based on Cyanex 272 and methyltrioctylammonium showed a high extraction ability for REE recovery from nitrate media [24]. In the extraction of light REE, a synergistic effect was found in the case of a Cyanex 272-EHEHPA system with a low acid concentration [34]. Synergistic extraction of REE was observed while using mixtures of bis(2,4,4-trimethylpentyl)phosphinic acid with 8-hydroxyquinoline [35] and with sec-nonylphenoxy acetic acid [36]. The mixture of DEHPA and Cyanex 272 was found to be synergistic for Eu(III) extraction. In the extraction studies, the maximum synergistic enhancement factor was obtained for the DEHPA-Cyanex 272 mixture with a 1:1 molar ratio [37].
As well as using synergistic systems, the extraction and separation of REE can be significantly improved by the addition of complexing agents to the aqueous phase. For example, the extraction and separation of Pr(III) and Ce(III) in the EHEHPA-containing system was found to become more efficient in the presence of complexing agents, such as lactic or citric acid [38]. The addition of lactic acid to the DEHPA-containing system was accompanied by an increase in DEHPA extraction capacity [39]. It was found that the use of acetic acid, along with lactic acid, promoted the extraction of REE by Cyanex 272 in kerosene [40]. The extraction of La(III) from acidic nitrate-acetate media by Cyanex 272 (H2A2) alone, or in combination with trioctylphospine oxide (TOPO) (B) in toluene, was investigated [41]. It was found that [La(OAc)2A·3HA] and [La(OAc)A2·B] are extracted in systems without and with TOPO, respectively.
In the case of Nd3+, Zanonato [42] demonstrated that lanthanide ions form various acetate complexes according to the following equilibrium:
Ln3+ + j(OAc)− ⇆ Ln(OAc)j(3−j)+, j = 1, 2, 3
It has been reported that the extraction of REEs by the binary extractants is improved in the presence of carboxylates due to the solvation of extracted species in the organic phase [43,44]. Thus, the mixture of Cyanex 272 with caprylic acid was examined to improve the solubility of lanthanum extracted complexes. The availability of acetic acid, in combination with its low price, makes it suitable for extraction purposes. Thus, the acetate ion was used as a complexing agent in the experimental study described below. This paper describes a new Cyanex 272-caprylic acid system for the extraction of lanthanides(III) from chloride-acetate and nitrate-acetate solutions. La(III) was chosen as a model object.

2. Materials and Methods

Stock solutions of lanthanum(III) chloride and nitrate were prepared by dissolving LaCl3·7H2O and La(NO3)3·6H2O in distilled water. Stock solutions of Nd, Eu, Dy, Er and Yb chlorides were prepared from their oxide (>99.9%) by dissolving them in HCl (conc.) and diluting to the required volume with distilled water. The initial aqueous solutions were diluted to the desired lanthanide concentration. Selected concentrations of acetate ions in aqueous solutions were maintained by adding NaOAc or AcOH.
A mixture of di(2,4,4-trimethylpentyl)phosphinic acid (Cyanex 272, CYTEC, Canada) and caprylic acid (Acros) was used as an extractant (solution in hexane). Commercial extractants were used without any further purification.
The concentrations of lanthanide in the initial solution and in the aqueous phase after extraction were determined via titration with a standard solution of EDTA at pH 5.5, using xylenol orange as an indicator. The concentration of lanthanide in the organic phase was calculated as the difference between the concentrations in the initial solution, and the aqueous phase, after extraction. The concentrations of lanthanide in the organic phase were also determined after its stripping with 0.5 mol/L HCl solution. Reagent grade chemicals were used. The distribution ratio (D) was determined as the ratio of the concentration of lanthanide(III) in the organic phase to that in the aqueous phase, and was calculated according to the following equation:
D = [Ln]o/[Ln]aq,
where [Ln]o and [Ln]aq are the equilibrium concentrations of the lanthanide in the organic and aqueous phase, respectively. The separation factor characterizes the separation degree between two lanthanides (Ln1–Ln2) in the extraction system and was calculated according to the following equation:
β = D(Ln2)/D(Ln1)
Extraction was performed at 20 °C in test tubes with ground-in stoppers, with equal volumes of the aqueous and the organic phases. Phases were mixed for 15 min, which was sufficient to establish the permanent values of the distribution ratios of lanthanides. pH measurements were performed using a SevenExcellence s470-k pH meter.
Three replicate experiments showed that the standard deviation of the measurements was less than 5%.

3. Results and Discussion

Preliminary experiments indicated that the extraction of La(III) from chloride-acetate solutions with a 0.015 mol/L Cyanex 272 solution in hexane was accompanied by the formation of insoluble products. To increase the solubility of lanthanum extracted species, hexane solutions of Cyanex 272 were supplemented with caprylic acid in different concentrations (vide infra). The introduction of the latter resulted in complete precipitation suppression. The structure of the extractants is shown in Figure 1.

3.1. Effect of Caprylic Acid Concentration

Figure 2 shows evidence, from experimental data, for the effect of caprylic acid concentration on La(III) extraction from chloride-acetate solution (0.1 mol/L NaOAc; CLa(init) = 0.02 mol/L), both for pure acid and its mixture with Cyanex 272. In the first case (curve 1, pure acid), the distribution ratios of La(III) did not exceed 0.6, despite the increase of the concentration of caprylic acid to 0.05 mol/L. The use of caprylic acid in combination with Cyanex 272 led to a significant growth in the La(III) distribution ratios (curve 2). In this case, extraction efficiency improved noticeably with an increase in the caprylic acid concentration. It can be assumed that extractable compounds with a different composition were formed in the system, involving a mixture of Cyanex 272 and caprylic acid, compared to extraction with pure extractants.

3.2. Effect of Sodium Acetate Concentration

Sodium acetate concentration was found to affect, to some extent, La(III) extraction from chloride-acetate and nitrate-acetate solutions (CLa(init) = 0.02 mol/L) with a mixture of Cyanex 272 (0.015 mol/L) and caprylic acid (0.02 mol/L) in hexane (Figure 3). In particular, an increase in NaOAc concentration caused a substantial increase in the distribution ratio of lanthanum until reaching a NaOAc:La ratio of about 10:1, after which no significant changes were observed. It is also noteworthy that the equilibrium pH value of the aqueous phase grew together with the efficiency of the La(III) transfer to the organic phase.
When studying the complexation of Nd(III) with the acetate ion in aqueous solutions, Zanonato [42] observed the formation of stable complex cations Nd(OAc)2+ when the ratio of acetate to metal was equal to 10 or more at 25 °C. It can be inferred that under corresponding experimental conditions complex cations such as La(OAc)2+ are also the most stable species; thus, an increase in the sodium acetate concentration to more than 0.2 mol/L (when the ratio of sodium acetate to lanthanum reached 10) did not lead to the further DLa increase (Figure 3).
To establish a synergistic effect in the system containing mixtures of Cyanex 272 and caprylic acid, a study of La(III) distribution was carried out in the case of chloride-acetate solutions (0.1 mol/L NaOAc; CLa(init) = 0.02 mol/L) using isomolar mixtures of Cyanex 272 and caprylic acid, depending on the molar fraction of Cyanex 272 in the organic phase (Figure 4). It can be noted that an increase in the molar fraction of Cyanex 272 in the mixture of extractants led to a monotonous increase in the lanthanum distribution ratios, indicating the predominant formation of lanthanum complexes with this extractant.

3.3. Extraction Isotherms for La(III)

Figure 5 shows the extraction isotherms of La(III) from chloride-acetate (1, 2) and nitrate-acetate (3) solutions obtained at various initial concentrations of Cyanex 272 (mol/L: 0.01 (1), 0.015 (2), 0.012 (3)) and caprylic acid (mol/L: 0.015 (1, 3), 0.03 (2)) under conditions of caprylic acid excess. The extraction isotherms obtained were characterised by high distribution ratios of La(III) in the initial regions (Figure 5), indicating the high extraction ability of the proposed mixtures. Under saturation conditions, the concentration of La in the organic phase was close to the initial concentration of Cyanex 272, during extraction from both chloride-acetate and nitrate-acetate solutions (Figure 5), i.e., the ratio of CLa(o):CCyanex (init.)~1. A double increase in the caprylic acid concentration (from 0.015 to 0.03 mol/L) at an initial Cyanex 272 concentration of 0.01 mol/L (Figure 5, curves 1, 2) did not lead to an increase in the La concentration in the organic phase. Thus, the data obtained from the extraction isotherms (Figure 5) and the isomolar series (Figure 4) confirm the formation of La(III) extracted species in the organic phase, mainly with Cyanex 272. It can be assumed that caprylic acid molecules solvated the extracted species, increasing their solubility in the organic phase as, in the absence of caprylic acid, the extraction of La(III) with Cyanex 272 was accompanied by precipitation. The solvate formation in the organic phase not only improved the solubility of the extracted complexes but also increased their thermodynamic stability, since the La(III) distribution ratios increased with caprylic acid concentration (Figure 2).
Based on the literature data on the composition of La(III) complexes in acetate solutions [42], these experimental results allow us to suggest that the extraction of La(III) from chloride-acetate and nitrate-acetate solutions in the presence of Cyanex 272 (H2A2) and caprylic acid (H2B2) (which are usually dimeric in nonpolar solvents) mixtures proceeded according to the cation-exchange mechanism and can be described by the equilibrium below:
La(OAc)2+(aq) + 0.5 H2A2(o) + s H2B2(o) ⇆ La(OAc)2A·sH2B2(o) + H+(aq),
where aq and o stand for the aqueous and the organic phases, respectively, and s is the number of caprylic acid dimers in solvates. Thus, an increase in DLa values, with an increase in the concentration of NaOAc (Figure 3), is associated both with increasing the acetate ion concentration in the aqueous phase, and with the growth of equilibrium pH in accordance with the above equation.

3.4. Extraction in the Presence of NaOAc/AcOH Mixtures

High distribution ratios of La(III) for chloride-acetate and nitrate-acetate solutions in systems containing Cyanex 272–caprylic acid mixtures complicate the separation of lanthanides; therefore, the extraction of lanthanum and neodymium from aqueous solutions in the presence of mixtures of sodium acetate and acetic acid were examined. The experimental conditions were as follows: aqueous phase—NaOAc + AcOH = 0.2 mol/L; CLn(init) = 0.01 mol/L; organic phase—0.01 mol/L Cyanex 272 (a, b); 0.02 mol/L (a), 0.15 mol/L (b) caprylic acid. The equilibrium pH values are given in Figure 6. The data for isomolar series (Figure 6) showed that the distribution ratios of lanthanides decreased with a reduction in the molar fraction of NaOAc in a mixture because of the equilibrium pH of the aqueous phase decreasing with the addition of acetic acid in accordance with the cation-exchange mechanism of the extraction. Experimental data (Figure 6) show that for extraction from nitrate acetic-acetate solutions distribution ratios for Nd(III) were higher than for lanthanum.
The distribution ratios of lanthanides(III) for chloride acetic-acetate solutions at CCH3COOH + CCH3COOH = 0.2 mol/L in the aqueous phase, during extraction with a mixture containing 0.01 mol/L Cyanex 272 and 0.15 mol/L caprylic acid in hexane, are presented in Table 1. These results show a decrease in the distribution ratios of lanthanides(III) with an increase in the molar fraction of acetic acid in the mixture, as do the data in Figure 6.
It is possible to affect the distribution and separation of REE by changing the composition of the aqueous phase, for example, by varying the ratio of NaOAc and AcOH. Thus, the system containing a mixture of Cyanex 272 and caprylic acid can be used for the efficient extraction of the sum of lanthanides(III) from acetate solutions.

3.5. Extraction of Lanthanides(III) from Chloride and Nitrate Acetic-Acetate Solutions

Since the distribution ratios of lanthanides are reduced for acetic acid solutions, the extraction of these metals from chloride and nitrate acetic-acetate solutions was studied, in order to determine the possibility of their separation. The distribution ratios of lanthanides(III) during extraction from chloride and nitrate acetic-acetate solutions with a mixture of Cyanex 272 and caprylic acid at 1/3 and 1/2 in hexane are given in Figure 7 and Table 2, respectively.
Experimental conditions were as follows: aqueous phase—0.2 mol/L mixture of NaOAc and AcOH (2:1); CLn(init) = 0.01 mol/L; pHeq. = 5.8. Experimental results indicated that, in this system, the separation of heavy lanthanides from light REE was possible.

4. Conclusions

This paper has described how a new extraction system containing mixtures of Cyanex 272 and caprylic acid in hexane was examined for La(III) extraction from chloride-acetate and nitrate-acetate media, as well as from acetic-acetate aqueous solutions. This system has the advantage of using commercially available extractants. The mixtures of Cyanex 272 and caprylic acid exhibited a high extraction ability and capacity. The extraction isotherms and the isomolar series data indicated that the La(III) extraction from chloride-acetate and nitrate-acetate solutions in this system proceeded through a cation-exchange mechanism, with the formation of lanthanum extracted species of the form La(OAc)2A.sH2B2 in the organic phase. The extraction of La(III) from acetic-acetate aqueous solutions proceeded with lower distribution ratios because of the decreasing equilibrium pH of the aqueous phase. It has been shown that the separation of lanthanides(III) can be achieved by extraction with synergistic Cyanex 272-caprylic acid mixtures in hexane from chloride acetic-acetate solutions. It was concluded that the extraction capacity of the investigated synergistic Cyanex 272-caprylic acid mixtures correlated with methods previously proposed. The usage of organic acidic agent mixtures, in particular a mixture of Cyanex 272 and caprylic acid in hexane, for the extraction and separation of rare earth metals from acetate and acetic-acetate solutions, is quite promising and may be of practical importance, for example, when carrying out processes in the multistage dynamic extraction mode.

Author Contributions

Conceptualisation, V.V.B. and Y.V.T.; methodology, V.V.B.; software, Y.V.T.; validation, V.K.I. and A.A.V.; formal analysis, Y.A.Z.; investigation, Y.V.T.; resources, V.V.B.; data curation, V.V.B.; writing—original draft preparation, V.V.B. and Y.V.T.; writing—review and editing, Y.A.Z. and A.A.V.; visualisation, V.V.B.; supervision, V.K.I.; project administration, A.A.V.; funding acquisition, V.K.I. All authors have read and agreed to the published version of the manuscript.

Funding

This work was supported by the Ministry of Science and Higher Education of the Russian Federation as part of the State Assignment of the Kurnakov Institute of General and Inorganic Chemistry of the Russian Academy of Sciences.

Conflicts of Interest

The authors declare no conflict of interest.

References

  1. Zhou, J.; Leaño, J.L.; Liu, Z.; Jin, D.; Wong, K.; Liu, R.; Bünzli, J.G. Impact of Lanthanide Nanomaterials on Photonic Devices and Smart Applications. Small 2018, 14, 1801882. [Google Scholar] [CrossRef]
  2. Binnemans, K.; Jones, P.T.; Blanpain, B.; Van Gerven, T.; Yang, Y.; Walton, A.; Buchert, M. Recycling of rare earths: A critical review. J. Clean. Prod. 2013, 51, 1–22. [Google Scholar] [CrossRef]
  3. Shcherbakov, A.B.; Reukov, V.V.; Yakimansky, A.V.; Krasnopeeva, E.L.; Ivanova, O.S.; Popov, A.L.; Ivanov, V.K. CeO2 Nanoparticle-Containing Polymers for Biomedical Applications: A Review. Polymers 2021, 13, 924. [Google Scholar] [CrossRef]
  4. Yapryntsev, A.D.; Baranchikov, A.E.; Ivanov, V.K. Layered rare-earth hydroxides: A new family of anion-exchangeable layered inorganic materials. Russ. Chem. Rev. 2020, 89, 629–666. [Google Scholar] [CrossRef]
  5. Shcherbakov, A.B.; Zholobak, N.M.; Spivak, N.Y.; Ivanov, V.K. Advances and prospects of using nanocrystalline ceria in cancer theranostics. Russ. J. Inorg. Chem. 2014, 59, 1556–1575. [Google Scholar] [CrossRef]
  6. Belova, V.V.; Voshkin, A.A.; Egorova, N.S.; Khol’kin, A.I. Extraction of rare earth metals from nitrate solutions with a binary extractant based on Cyanex 272. Russ. J. Inorg. Chem. 2010, 55, 629–633. [Google Scholar] [CrossRef]
  7. Xie, F.; Zhang, T.A.; Dreisinger, D.; Doyle, F. A critical review on solvent extraction of rare earths from aqueous solutions. Min. Eng. 2014, 56, 10–28. [Google Scholar] [CrossRef]
  8. Fedorova, M.I.; Zakhodyaeva, Y.A.; Zinov’eva, I.V.; Voshkin, A.A. Recovery of rare-earth elements from nitrate solutions using polyethylene glycol 1500. Russ. Chem. Bull. 2020, 69, 1344–1348. [Google Scholar] [CrossRef]
  9. Belova, V.V.; Egorova, N.S.; Voshkin, A.A.; Khol’kin, A.I. Extraction of rare earth metals, uranium, and thorium from nitrate solutions by binary extractants. Theor. Found. Chem. Eng. 2015, 49, 545–549. [Google Scholar] [CrossRef]
  10. Chang, H.; Li, M.; Liu, Z.; Hu, Y.; Zhang, F. Study on separation of rare earth elements in complex system. J. Rare Earths. 2010, 28, 116–119. [Google Scholar] [CrossRef]
  11. Belova, V.V.; Voshkin, A.A.; Kholkin, A.I.; Payrtman, A.K. Solvent extraction of some lanthanides from chloride and nitrate solutions by binary extractants. Hydrometallurgy 2009, 97, 198–203. [Google Scholar] [CrossRef]
  12. Sato, A.T. Liquid-liquid extraction of rare-earth elements from aqueous acid solutions by acid organophosphorus compounds. Hydrometallurgy 1989, 22, 121–140. [Google Scholar] [CrossRef]
  13. Zhang, C.; Wang, L.; Huang, X.; Donga, J.; Long, Z.; Zhang, Y. Yttrium extraction from chloride solution with a synergistic system of 2-ethylhexylphosphonic acid mono-(2-ethylhexyl)ester and bis(2,4,4-trimethylpentyl)phosphinic acid. Hydrometallurgy 2014, 147-148, 7–12. [Google Scholar] [CrossRef]
  14. Radhika, S.; Kumar, B.N.; Kantam, M.L.; Reddy, B.R. Liquid-liquid extraction and separation possibilities of heavy and light rare-earths from phosphoric acid solutions with acidic organophosphorus reagents. Sep. Purif. Technol. 2010, 75, 295–302. [Google Scholar] [CrossRef]
  15. Pusparini, W.R.; Silfi, A.N.; Handini, T. Synergistic extraction of yttrium using mixtures of organophosphorus extractants. AIP Conf. Proc. 2021, 2381, 020065. [Google Scholar]
  16. Jorjani, E.; Shahbazi, M. The production of rare earth elements group via tributyl phosphate extraction and precipitation stripping using oxalic acid. Arab. J. Chem. 2016, 9, S1532–S1539. [Google Scholar] [CrossRef]
  17. Panda, N.; Devi, N.; Mishra, S. Solvent extraction of neodymium(III) from acidic nitrate medium using Cyanex 921 in kerosene. J. Rare Earths 2012, 30, 794–797. [Google Scholar] [CrossRef]
  18. Tong, H.; Wang, Y.; Liao, W.; Li, D. Synergistic extraction of Ce(IV) and Th(IV) with mixtures of Cyanex 923 and organophosphorus acids in sulfuric acid media. Sep. Purif. Technol. 2013, 118, 487–491. [Google Scholar] [CrossRef]
  19. Turanov, A.N.; Karandashev, V.K.; Boltoeva, M. Solvent extraction of intra-lanthanides using a mixture of TBP and TODGA in ionic liquid. Hydrometallurgy. 2020, 195, 105367. [Google Scholar] [CrossRef]
  20. Kalyakin, S.N.; Kuzmin, V.I.; Mulagaleeva, M.A. Binary extraction of neodymium nitrate using 2-ethylhexylphosphonic acid 2-ethylhexyl mono ester and tri-n-octylamine. J. Mol. Liq. 2019, 273, 45–49. [Google Scholar] [CrossRef]
  21. Belova, V.V.; Voshkin, A.A.; Egorova, N.S.; Kholkin, A.I. Solvent extraction of rare earth metals from nitrate solutions with di(2,4,4-trimethylpentyl)phosphinate of methyltrioctylammonium. J. Mol. Liq. 2012, 172, 144–146. [Google Scholar] [CrossRef]
  22. Rout, A.; Binnemans, K. Solvent extraction of neodymium(III) by functionalized ionic liquid trioctylmethylammonium dioctyl diglycolamate in fluorine-free ionic liquid diluents. Ind. Eng. Chem. Res. 2014, 53, 6500–6508. [Google Scholar] [CrossRef]
  23. Belova, V.V.; Martynova, M.M.; Tsareva, Y.V.; Baulin, V.E.; Baulin, D.V. Solvent extraction of lanthanum(III) from chloride and nitrate aqueous solutions with dioctyldiglycolamates of dioctylammonium and trioctylammonium. J. Mol. Liq. 2019, 293, 111568. [Google Scholar] [CrossRef]
  24. Belova, V.V.; Tsareva, Y.V. Extraction and separation of lanthanides from aqueous chloride and nitrate media using mixtures of binary extractants based on secondary and tertiary amines. Mendeleev Commun. 2021, 31, 116–118. [Google Scholar] [CrossRef]
  25. Quintriqueo, A.; Romero, J.; Quijada-Maldonado, E.; Bringas, E.; Olea, F.; Hernández, J. Extraction and separation factor for lanthanum(III) and cerium(III) complexes from aqueous medium using ionic liquid and kerosene. Adv. Chem. Eng. Sci. 2020, 10, 343–357. [Google Scholar] [CrossRef]
  26. Pospiech, B.; Gega, J. Solvent extraction of metal ions from sulfate solutions obtained in leaching of spent Ni-MH batteries. New Trends Prod. Eng. 2019, 2, 214–221. [Google Scholar] [CrossRef] [Green Version]
  27. Wang, X.; Li, W.; Li, D. Extraction and stripping of rare earths using mixtures of acidic phosphorus based reagents. J. Rare Earths 2011, 29, 413–415. [Google Scholar] [CrossRef]
  28. Zhao, Q.; Li, Y.; Kuang, S.; Zhang, Z.; Bian, X.; Liao, W. Synergistic extraction of heavy rare earths by mixture of α-aminophosphonic acid HEHAMP and HEHEHP. J. Rare Earths 2019, 37, 422–428. [Google Scholar] [CrossRef]
  29. Padhan, E.; Sarangi, K. Solvent extraction of praseodymium using different extractants—A synergistic study. Sep. Purif. Technol. 2018, 53, 295–302. [Google Scholar] [CrossRef]
  30. Banda, R.; Jeon, H.S.; Lee, M.S. Solvent extraction separation of La from chloride solution containing Pr and Nd with Cyanex 272. Hydrometallurgy 2012, 121–124, 74–80. [Google Scholar] [CrossRef]
  31. Wang, Y.L.; Liao, W.P.; Li, D.Q. A solvent extraction process with mixture of CA12 and Cyanex 272 for the preparation of high purity yttrium oxide from rare earth ores. Sep. Purif. Technol. 2011, 82, 197–201. [Google Scholar] [CrossRef]
  32. Liu, Y.; Jeon, H.S.; Lee, M.S. Solvent extraction of Pr and Nd from chloride solution by the mixtures of Cyanex 272 and amine extractants. Hydrometallurgy 2014, 150, 61–67. [Google Scholar] [CrossRef]
  33. Liu, Y.; Jeon, H.S.; Lee, M.S. Separation of Pr and Nd from La in chloride solution by extraction with a mixture of Cyanex 272 and Alamine 336. Met. Mater. Int. 2015, 21, 944–949. [Google Scholar] [CrossRef]
  34. Quinn, J.E.; Soldenhoff, K.H.; Stevens, G.W.; Lengkeek, N.A. Solvent extraction of rare earth elements using phosphonic/phosphinic acid mixtures. Hydrometallurgy 2015, 157, 298–305. [Google Scholar] [CrossRef]
  35. Wang, X.L.; Du, M.; Liu, H. Synergistic extraction study of samarium(III) from chloride medium by mixtures of bis(2,4,4-trimethylpentyl)phosphinic acid and 8-hydroxyquinoline mixtures. Sep. Purif. Technol. 2012, 93, 48–51. [Google Scholar] [CrossRef]
  36. Sun, X.; Wang, J.; Li, D.; Li, H. Synergistic extraction of rare earths by mixture of bis(2,4,4-trimethylpentyl)phosphinic acid and sec-nonylphenoxy acetic acid. Sep. Purif. Technol. 2006, 50, 30–34. [Google Scholar] [CrossRef]
  37. Zaheri, P.; Abolghasemi, H.; Maraghe, M.G.; Mohammadi, T. Intensification of europium extraction through a supported liquid membrane using mixture of D2EHPA and Cyanex 272 as carrier. Chem. Eng. Process. 2015, 92, 18–24. [Google Scholar] [CrossRef]
  38. Zhang, F.; Wu, W.; Dai, J.; Bian, X. Extraction and separation of Pr(III)/Ce(III) from chloride medium by 2-ethylhexylphosphonic acid mono-(2-ethylhexyl) ester in the presence of two complexing agents. Sep. Purif. Technol. 2016, 51, 778–783. [Google Scholar] [CrossRef]
  39. Yin, S.; Wu, W.; Bian, X.; Zhang, F. Effect of complexing agent lactic acid on the extraction and separation of Pr(III)/Ce(III) with di-(2-ethylhexyl) phosphoric acid. Hydrometallurgy 2013, 131–132, 133–137. [Google Scholar] [CrossRef]
  40. Kashi, E.; Habibpour, R.; Gorzin, H.; Maleki, A. Solvent extraction and separation of light rare earth elements (La, Pr and Nd) in the presence of lactic acid as a complexing agent by Cyanex 272 in kerosene and the effect of citric acid, acetic acid and Titriplex III as auxiliary agents. J. Rare Earths 2018, 36, 317–323. [Google Scholar] [CrossRef]
  41. Saleh, M.I.; Bari, M.F.; Saad, B. Solvent extraction of lanthanum(III) from acidic nitrate-acetato medium by Cyanex 272 in toluene. Hydrometallurgy 2002, 63, 75–84. [Google Scholar] [CrossRef]
  42. Zanonato, P.L.; Bernardo, P.; Bismondo, A.; Rao, L.; Choppin, G.R. Thermodynamic studies of the complexation between neodymium and acetate at elevated temperatures. J. Sol. Chem. 2001, 30, 1–18. [Google Scholar] [CrossRef]
  43. Kalyakin, S.N.; Kuz’min, V.I.; Mulagaleeva, M.A. Binary extraction of lanthanide (III) chlorides using carboxylates and dialkylphosphates of secondary and tertiary amines. Hydrometallurgy 2015, 151, 116–121. [Google Scholar] [CrossRef]
  44. Kalyakin, S.N.; Kuzmin, V.I.; Mulagaleeva, M.A. Binary extraction of lanthanides (III) nitrates with carboxylates and dialkylphosphates of secondary and tertiary amines. Theor. Found. Chem. Eng. 2016, 50, 878–883. [Google Scholar] [CrossRef]
Processes 09 02222 g001 550
Figure 1. Commercial extractants Cyanex 272 and caprylic acid.
Figure 1. Commercial extractants Cyanex 272 and caprylic acid.
Processes 09 02222 g001
Processes 09 02222 g002 550
Figure 2. Effect of caprylic acid concentration on the La(III) extraction.
Figure 2. Effect of caprylic acid concentration on the La(III) extraction.
Processes 09 02222 g002
Processes 09 02222 g003 550
Figure 3. Effect of NaOAc concentration on the La(III) extraction.
Figure 3. Effect of NaOAc concentration on the La(III) extraction.
Processes 09 02222 g003
Processes 09 02222 g004 550
Figure 4. Effect of molar fraction of Cyanex 272 on the La(III) extraction.
Figure 4. Effect of molar fraction of Cyanex 272 on the La(III) extraction.
Processes 09 02222 g004
Processes 09 02222 g005 550
Figure 5. Isotherms of La(III) extraction with Cyanex 272-caprylic acid mixtures.
Figure 5. Isotherms of La(III) extraction with Cyanex 272-caprylic acid mixtures.
Processes 09 02222 g005
Processes 09 02222 g006 550
Figure 6. Effect of the molar fraction of NaOAc on the extraction of La(III) (a) and Nd(III) (b).
Figure 6. Effect of the molar fraction of NaOAc on the extraction of La(III) (a) and Nd(III) (b).
Processes 09 02222 g006
Processes 09 02222 g007 550
Figure 7. Extraction of lanthanides(III) with a mixture of 0.01 mol/L Cyanex 272 and 0.03 mol/L caprylic acid.
Figure 7. Extraction of lanthanides(III) with a mixture of 0.01 mol/L Cyanex 272 and 0.03 mol/L caprylic acid.
Processes 09 02222 g007
Table
Table 1. Distribution ratios of lanthanides(III) for chloride acetic-acetate solutions (eq.—equal).
Table 1. Distribution ratios of lanthanides(III) for chloride acetic-acetate solutions (eq.—equal).
LnNaOAc:AcOH
1:11:1.41:2
DLnpH eq.DLnpH eq.DLnpH eq.
Nd4.465.552.335.301.355.15
Sm4.985.553.355.301.865.15
Dy5.675.554.05.302.105.15
Table
Table 2. Distribution ratios (DLn) and separation factors (βLn/La) of lanthanides(III) with a mixture of 0.01 mol/L Cyanex 272 and 0.02 mol/L caprylic acid.
Table 2. Distribution ratios (DLn) and separation factors (βLn/La) of lanthanides(III) with a mixture of 0.01 mol/L Cyanex 272 and 0.02 mol/L caprylic acid.
Chloride Acetic-Acetate MediaNitrate Acetic-Acetate Media
LnDLnβLn/LaLnDLnβLn/La
La1.14-La0.818-
Eu2.752.41Nd1.01.22
Dy13.912.2Eu2.332.85
Er37.532.9Dy2.332.85
Yb8.109.9
Publisher’s Note: MDPI stays neutral with regard to jurisdictional claims in published maps and institutional affiliations.

Share and Cite

MDPI and ACS Style

Belova, V.V.; Tsareva, Y.V.; Zakhodyaeva, Y.A.; Ivanov, V.K.; Voshkin, A.A. Solvent Extraction of Lanthanides(III) in the Presence of the Acetate Ion Acting as a Complexing Agent Using Mixtures of Cyanex 272 and Caprylic Acid in Hexane. Processes 2021, 9, 2222. https://doi.org/10.3390/pr9122222

AMA Style

Belova VV, Tsareva YV, Zakhodyaeva YA, Ivanov VK, Voshkin AA. Solvent Extraction of Lanthanides(III) in the Presence of the Acetate Ion Acting as a Complexing Agent Using Mixtures of Cyanex 272 and Caprylic Acid in Hexane. Processes. 2021; 9(12):2222. https://doi.org/10.3390/pr9122222

Chicago/Turabian Style

Belova, Vera V., Yulia V. Tsareva, Yulia A. Zakhodyaeva, Vladimir K. Ivanov, and Andrey A. Voshkin. 2021. "Solvent Extraction of Lanthanides(III) in the Presence of the Acetate Ion Acting as a Complexing Agent Using Mixtures of Cyanex 272 and Caprylic Acid in Hexane" Processes 9, no. 12: 2222. https://doi.org/10.3390/pr9122222

APA Style

Belova, V. V., Tsareva, Y. V., Zakhodyaeva, Y. A., Ivanov, V. K., & Voshkin, A. A. (2021). Solvent Extraction of Lanthanides(III) in the Presence of the Acetate Ion Acting as a Complexing Agent Using Mixtures of Cyanex 272 and Caprylic Acid in Hexane. Processes, 9(12), 2222. https://doi.org/10.3390/pr9122222

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