Ultra-selective ligand-driven separation of strategic actinides

Abstract

Metal ion separations are critical to numerous fields, including nuclear medicine, waste recycling, space exploration, and fundamental research. Nonetheless, operational conditions and performance are limited, imposing compromises between recovery, purity, and cost. Siderophore-inspired ligands show unprecedented charge-based selectivity and compatibility with harsh industry conditions, affording excellent separation efficiency, robustness and process control. Here, we successfully demonstrate a general separation strategy on three distinct systems, for Ac, Pu, and Bk purification. Separation factors (SF) obtained with model compound 3,4,3-LI(1,2-HOPO) are orders of magnitude higher than with any other ligand currently employed: 106 between Ac and relevant metal impurities, and over 108 for redox-free Pu purification against uranyl ions and trivalent actinides or fission products. Finally, a one-step separation method (SF > 3 × 106 and radiopurity > 99.999%) enables the isolation of Bk from adjacent actinides and fission products. The proposed approach offers a paradigm change for the production of strategic elements.

Introduction

Isotope production has been the cornerstone of many research fields and applications throughout the last century1 and relies largely on separation science. Contemporary examples illustrating the primary importance of separations include radionuclide purification for use in radiopharmaceuticals2 or in radioactive thermoelectric generators that are vital to space exploration3. The development of efficient separation methods is also critical for forensics analysis, recycling of ageing weapon materials, fabrication of nuclear fuels4, production of radiotracers for research5, as well as manufacturing of high-purity actinide targets for the discovery of new elements6. Regardless of the application, product purity must be as high as possible, which requires highly efficient and cost-effective separation methods. Radionuclide production through either target irradiation (225Ac, 177Lu, 90/86Y, 89Zr, 47/44Sc, 238Pu, 248Cm, 249Bk, 249/252Cf, etc.) or milking from long-lived sources (227Ac → 227Th → 223Ra, 241Pu → 241Am, 233U → 229Th → 225Ra → 225Ac, 232Th → 212Pb, etc.) involves the handling of mixtures of metal ions where major impurities are often neighboring elements in the periodic table. In most cases, the ratio between the valuable element and impurities is extremely high (a few μg diluted in multi-g targets), rendering purification very challenging, albeit critical for the availability of the coveted isotope.

Recent reports have highlighted the creative use of solid matrices, such as crystalline selenites7 or borates8, to quantitatively separate f-elements. However, most at-scale chemical purifications rely on chromatographic separations or liquid-liquid extraction methods or both, depending on the process scale and the desired specifications. These bi-phasic techniques are based on intrinsic interactions between metal ions and organic molecules dissolved in an organic diluent (liquid-liquid extraction) or grafted onto a solid matrix (chromatography). Ideally, these organic molecules (hereafter referred to as extractants) are amenable to transfer ions of interest from one phase to another in a selective manner relative to impurities. Extractant performance is typically not predictable and not always transposable from one separation system to another. In fact, predicting the efficiency and metal selectivity of a given process formulation (aqueous phase, diluent, and extractant) is a scientific challenge with numerous correlated variables9,10, such as metal speciation in the aqueous phase, metal-extractant compound speciation in the organic phase, free extractant speciation, influence of the diluent, loading capacity of the organic phase, etc. Most extractants currently used in hydrometallurgy can potentially co-extract multiple elements depending on chemical conditions (acidity, extractant concentration, phase ratio etc.)11,12,13. Separation selectivity is only achieved by finely tuning those chemical conditions and operational conditions for these processes are generally highly constrained, with many required steps to reach desired purities.

To overcome these challenges, a class of hydroxypyridinone (HOPO) chelators was investigated for its high metal-binding selectivity and applicability to separation needs. These molecules exhibit a unique combination of properties long sought in separation science: (i) water-solubility, (ii) structures consisting of solely H, C, N, and O atoms, (iii) ability to control metal oxidation states without additional redox-active species, (iv) extremely high charge-based selectivity, and (v) high metal-ligand complex stability even in strong acid (up to 10 M H+). Using the model octadentate HOPO chelator, 3,4,3-LI(1,2-HOPO) (hereafter referred to as 343HOPO), and taking advantage of these unprecedented characteristics, highly efficient and robust chemical separation processes were developed for three strategic examples: the purification of 225Ac, Pu-isotopes, and 249Bk.

Results and Discussion

Choice of aqueous chelator as hold-back reagent

Numerous drug development studies14,15,16 have focused on synthetic siderophore-inspired compounds because of their ability to form stable, and sometimes luminescent, complexes with metal ions of interest for medical imaging, radionuclide decontamination, and cancer treatments. While this class of ligands, encompassing HOPO and catecholamide (CAM) derivatives, has been known for decades, it had never been studied in details for separation applications. In fact, a few exceptions aside, most of these chelators have only been studied with a single cation, such as Gd3+, Th4+, or Pu4+, impairing broader evaluation of their metal-metal selectivity. The chemistry of some HOPO ligands was recently extended across the periodic table, highlighting their outstanding selectivity, and large superiority over polyaminocarboxylate chelators (IDA, EDTA, DTPA, etc.), typically encountered in separations (Fig. 1). A comparison of metal complex formation constants for the octadentate 343HOPO shows striking differences between tetravalent species and corresponding divalent or trivalent ones. The observed selectivity seems mainly charge-based and only slightly dependent on the ionic radius of the cations (Supplementary Fig. 1), although some selectivity is noted across the trivalent lanthanide and actinide series. 343HOPO outperforms any known chelator in terms of charge-specific selectivity and, in particular, for the binding of tetravalent ions. As such, the Ce4+/Ce3+ selectivity of 343HOPO is about 15 orders of magnitude higher than what could be expected from a carboxylate ligand. Extreme selectivity is also observed even for ions of similar size, such as in the Th4+/Am3+, Th4+/Gd3+, Ce4+/Lu3+, or Th4+/Cd2+ pairs (Fig. 1 and Supplementary Fig. 2). As shown in Fig. 1, a handful of other molecules from the same family (octadentate 3,4,3-LI-CAM, Bis-TREN-Me-3,2-HOPO, and TAM-macrocycle; tetradentate 5LI-Me-3,2-HOPO, 5LIO-Me-3,2-HOPO; and bidentate PR-Me-3,2-HOPO)17,18,19,20 exhibit known solution thermodynamic properties that match those of 343HOPO but none of the chelators typically used for separation methods is nearly as selective. Many additional HOPO and CAM ligands have been designed15 and previously reported octadentate 1,2-HOPO21, mixed 3,4,3-LI(1,2-HOPO/Me-3,2-HOPO)22, and DFO/1,2-HOPO23 structures would certainly make excellent candidates for charge-based selectivity; however, their chelation properties have so far only been investigated with either Eu3+, Zr4+, or Pu4+. Due to its current kg-scale availability and established solution thermodynamics, 343HOPO was used here as a model case. It was not initially designed for separation applications and its performance should not be considered as the upper limit for a separation strategy that could be extended to an entire molecular family.

Fig. 1
figure1

Relative thermodynamic stabilities of metal-ligand complexes discussed in this work. a Stability constants (log βML)24,25,46,48,49,50 of 343HOPO complexes with tetravalent cations (red), divalent ions (yellow), trivalent actinides (green), and trivalent lanthanides (blue). The value plotted for Ac3+ is an estimate based on its ionic radius. Selectivity comparisons for Ce4+/Ce3+ (b), Th4+/Eu3+ (d), and Th4+/Cd2+ (f), with HOPO and CAM ligands and classical chelators used in separations. For tetradentate ligands 5-LIO-Me-3,2-HOPO and 5-LI-Me-3,2-HOPO, the βML2 value is used. For bidentate PR-Me-3,2-HOPO, the βML4 value is used. The line y = x corresponds to no selectivity. Additional selectivity comparisons are given in Supplementary Fig. 2. Full ligand names and structures are given in Supplementary Table 1. Metal speciation diagrams for 343HOPO solutions containing Ac3+ or Eu3+ (c) and UO22+ or Th4+ (e). [Chelator]/[Metal] = 1 mol/mol. L = Ligand. Solid lines: free metal. Dotted lines: 343HOPO complexes

The selectivity of 343HOPO for tetravalent ions is so high that it is expected to form complexes even under very acidic conditions (experimentally observed24 in 3 M HCl for Sn4+), whereas it should release trivalent25 and divalent24,26 ions completely below pH~2 (Fig. 1). To our knowledge, no other reported class of ligands exhibits such behavior. The clear metal discrimination afforded by 343HOPO (bound M4+ versus free M3+/2+/1+) can therefore be leveraged as a chemical switch to isolate charged ions, a needed tool when separating Ac3+/Th4+ or Pu4+/Am3+ mixtures. If such an ultra-selective complexant is present in the aqueous phase, overall process selectivity is expected to be decoupled from extractant selectivity, since a system containing 343HOPO in the aqueous phase and a completely non-selective extractant in the organic phase will still result in highly efficient separation. Such ligand-driven performance enables more flexible solvent formulation and operational process conditions. It will also spare the cumbersome development of new extractants and can be applied to a variety of Mx+/My+ pairs, as demonstrated below.

Actinium purification

While there is great interest in using 225Ac for targeted alpha therapy27,28, the development of 225Ac-based pharmaceuticals is still hindered by low isotope availability relative to potential market needs1. Furthermore, Ac chemistry is largely unexplored since (i) Ac3+ being the biggest trivalent ion of the periodic table28,29, there is no adequate surrogate to study its chemistry, and (ii) its highly-radioactive longest-lived isotope (227Ac, t1/2 = 21.8 year) is available in only μg amounts. Both 227Ac decay and 225Ac production yield mixtures of Ac3+, Th4+, Ra2+, and trivalent lanthanides. The ratio between unwanted elements and Ac is typically very high and purification options are limited30. 343HOPO exhibits very low affinity toward Ac3+ compared with other trivalent ions and has extremely high affinity for tetravalent ions, providing a straightforward tool to selectively isolate Ac. Figure 2 shows the Ac3+ and Pu4+ extraction yields by HDEHP (extractant widely used in hydrometallurgy, also known as D2EHPA)31,32 in the presence of 343HOPO at different pH values. Full Ac3+ extraction in the organic layer was achieved, while scavenging Pu4+ (a surrogate for Th4+) in the aqueous layer. Similar experiments in the presence of reference aqueous chelator DTPA, also used in the so-called TALSPEAK process31, showed partial extraction of both isotopes and no practical separation or recovery. After only a single step and despite a large initial Pu/Ac ratio (~10,000 mol/mol), SFAc/Pu values reached at least 1,000,000 in the presence of 343HOPO, combined with recovery yields of up to 99.70% for Ac in the organic phase and higher than 99.97% for Pu in the aqueous phase. In comparison, DTPA SFAc/Pu values were between 1 and 100, the typical selectivity range observed in hydrometallurgical processes, with less than 50% Ac recovery. Separation of Ac from trivalent impurities was also investigated. Figure 3 displays Ac3+, Am3+, and Gd3+ extraction profiles in both HDEHP/343HOPO-HNO3 and HDEHP/DTPA-HNO3 systems. Significant discrimination was observed for Ac3+ against Am3+ and Gd3+, with SFAc/Am and SFAc/Gd reaching 130,000 and 1,300,000, respectively. In the DTPA case, SFAm/Ac and SFGd/Ac values were below 10 and 5300, respectively, and Ac recovery was low. A process flowsheet for 225Ac purification using the 343HOPO-HDEHP combination is proposed in Supplementary Fig. 3.

Fig. 2
figure2

Separation of Ac from Pu. a Extraction yield of Ac3+ (stars) and Pu4+ (triangles) by 0.5 M HDEHP as a function of pH, in the presence of DTPA (dotted lines) or 343HOPO (solid lines). A logarithmic scale is used due to the low extraction yields of Pu4+. b Corresponding separation factors. Aqueous phase: 40 mM of chelator in sodium lactate/sodium nitrate buffer (I = 2 M). Vorg/Vaq = 1. T = 25 °C. LoD = Limit of detection. Data points with arrows are lower limits

Fig. 3
figure3

Separation of Ac from Gd and Am. Extraction yield of trivalent Ac (stars), Gd (squares), and Am (circles) by 0.5 M HDEHP as a function of pH, in the presence of DTPA (a) or 343HOPO (c). A logarithmic scale is used due to the low extraction yields of Pu4+. The corresponding separation factors in the presence of DTPA or 343HOPO are given in b and d, respectively. Aqueous phase: 40 mM of chelator in sodium lactate/sodium nitrate buffer (I = 2 M). Vorg/Vaq = 1, one contact. T = 25 °C. Data points with arrows are lower limits

Plutonium purification

Since the 1940’s, worldwide Pu inventory has evolved from almost 0 to ~2,500,000 kg due to anthropogenic activities33,34, and is estimated to increase by 70,000 kg/year35 based on civilian nuclear power generation forecasts. Pu materials must be properly safeguarded throughout their lifespan, which necessitates advanced nuclear forensic controls and reprocessing activities. In this context, isolation of Pu from minor actinide and fission product impurities is essential. The standard PUREX (Plutonium Uranium Redox EXtraction) liquid-liquid extraction process36 allows recovering and separating Pu and U from minor actinides and fission products. PUREX operates in concentrated HNO3 media and includes two critical steps: (i) UO22+ and Pu4+ co-extraction into the organic phase (30 % TBP in diluent) while leaving trivalent ions in the aqueous phase, and (ii) reductive back-extraction of Pu as Pu3+ while leaving UO22+ in the organic phase. The latter is indispensable for U/Pu separation because of TBP’s lack of selectivity between tetravalent and actinyl species. While reduction of Pu4+ to Pu3+ is achieved by addition of strong reducing agents into the liquid-liquid extraction batteries37, Pu3+ is inherently unstable, and this redox component creates constraints in the reactive TBP-nitric medium (reduction of HNO3 to HNO2 and formation of potentially explosive compounds such as HN3).

A simple but effective modification of PUREX was investigated for non-reductive separation of Pu and U (Supplementary Fig. 4). Figure 4 shows that Pu4+ and UO22+ extraction behaviors under typical PUREX conditions are expectedly very similar, with quantitative extraction of both elements and SFU/Pu values below 3. After co-extraction of U and Pu by TBP, the unprecedented chelation properties of 343HOPO at high acidity and its charge-based selectivity can be leveraged to selectively strip Pu4+ from the organic phase. Efficient U/Pu separation was observed in the presence of 343HOPO (Fig. 4) by selective chelation of Pu4+, without significant interactions with UO22+ over a broad range of acidity (up to 8 M HNO3) and SFU/Pu values as high as 5800. The use of 343HOPO-type chelators could afford straightforward and efficient separation methods for the purification of U and Pu, and so, without using any redox-active chemical or non-volatile contaminant. This method also leads to very flexible process control, as demonstrated by the broad acidity range under which 343HOPO selectively scavenges Pu4+.

Fig. 4
figure4

Separation of Pu from U, Gd, Lu, and Cf. Extraction of Pu4+ (triangles) and UO22+ (diamonds) under typical PUREX conditions (a) and back-extraction in the presence of 1 mM 343HOPO (b). Dotted lines: separation factor U/Pu. Organic phase: 30 % TBP in kerosene. c and d show the extraction yields of Gd3+ (squares), Lu3+ (crosses), Cf3+ (circles), UO22+, and Pu4+ by TODGA in the absence or presence of 1 mM 343HOPO, respectively. Corresponding separation factors are given in e and f. Organic phase: 0.1 M TODGA in kerosene. Aqueous solvent: HNO3. T = 25 °C. O/A = 1, one contact. Points with arrows are lower limits

Another route, using TODGA as extractant, was explored for the purification of Pu not only from divalent ions but also from trivalent metals. TODGA is from the diglycolamide family used for resins separations38,39, and is currently investigated for next-generation nuclear waste treatment processes, such as EURO-GANEX11,40,41. TODGA is effective at extracting trivalent lanthanides and actinides from concentrated nitric media but its selectivity toward other ions, such as Pu4+, is very low. Very high yields were observed for the extraction of Gd3+, Lu3+, UO22+, Pu4+, and Cf3+ from HNO3 (>99.5% if HNO3 > 1 M), emphasizing the lack of potential for practical separation (Fig. 4). In the presence of 343HOPO, Pu4+ is selectively held-back in the aqueous phase whereas the extraction behaviors of trivalent actinides, lanthanides, and uranyl are not impacted, offering a direct avenue for Pu recovery. SF values between the trivalent ions and Pu4+ are above 450,000,000 (LoD reached) whereas SFU/Pu values are around 50,000. SFU/Pu values are limited by the relatively low distribution factors of uranyl (DU < 30) when using TODGA, as observed here and elsewhere11. Combining the high affinity of TODGA for trivalent lanthanides and actinides with the high affinity of TBP for uranyl and the selectivity of 343HOPO for Pu, a redox-free process was devised for the flash-recovery and purification of Pu from materials containing Pu, uranyl, minor actinides, and fission products (Supplementary Fig. 5).

Berkelium purification

Bk and Cf are of particular interest due to their use as targets for the production of super-heavy elements, such as elements 117 (tennessine, named after a 249Bk target manufactured at Oak Ridge National Laboratory - ORNL, Tennessee)42 and 118 (oganesson, produced from 249Cf)43. 252Cf is also a strategic isotope for oil and gas exploration as well as quality control of nuclear reactors1. Bk and Cf are produced via prolonged neutron irradiation of Am/Cm targets, yielding mixtures of actinides from Am to Fm and some fission products5. These transplutonium elements have traditionally displayed very similar chemistries as they exhibit the +III oxidation state in solution and have almost identical ionic radii44. To separate Cf3+ from Bk3+, Bk3+ can eventually be oxidized to Bk4+ under harsh conditions (heating combined with excess NaBrO3 in 8 M HNO3) but it is unstable, which adds another level of complications to the eventual separation scheme. Campaigns conducted at ORNL for the purification of mg amounts of 249Bk take several months5,45 and result in relatively limited purification factors. The Bk isolation process5 comprises about 25 steps, with a purification factor for the entire procedure (product of SF values from all steps) of ~107.

343HOPO was recently shown46 to oxidize Bk3+ and stabilize Bk4+ in aqueous solution without addition of any redox-active species; a direct consequence of the ligand’s thermodynamic preference for tetravalent cations (vide supra). The separation strategy detailed above can therefore be applied to the isolation of Bk from all trivalent ions. Preliminary tests with extractant HDEHP at high acidity (0.1–6 M HNO3) show a drastic influence of 343HOPO on the Bk extraction by HDEHP (Supplementary Fig. 6). Comparisons with Pu4+, Gd3+, and Cf3+ confirm that Bk exists as Bk3+ in nitric media without chelator but forms a Bk4+ complex with 343HOPO even under very acidic conditions (Supplementary Fig. 7). Thus, isolation of Bk from its trivalent neighbors and lanthanides was studied in the HDEHP-HNO3−343HOPO system (Fig. 5). After a single step at room temperature, high extraction yields were observed for all tested trivalent ions, whereas Bk was selectively sequestered in the aqueous phase. SFBk/Lu values as high as 320,000 were obtained, and SF values between 3000 and 10,000 were reached between Bk and adjacent actinides Am3+, Cf3+, and Es3+. Similar tests in the presence of NTA, EDTA, CDTA, and DTPA showed no separation at all between Bk and Cf, (similar to what is observed without chelator) since this type of ligands is not strong enough to bind metal ions under acidic conditions and is not selective enough to oxidize Bk3+ to Bk4+. Importantly (Fig. 5 and Supplementary Fig. 8), the behavior of Bk in the presence of 343HOPO is completely decoupled from classic extraction parameters (extractant concentration, phase ratio), resulting in stable separation performance and robustness over a wide range of conditions. Given the system SF values, two consecutive steps would yield purification factors similar or higher than the current state-of-the-art process5.

Fig. 5
figure5

Separation of Bk, from Gd, Lu, Am, Cf, and Es. a Extraction of 177Lu (crosses), 153Gd (squares), 243Am (diamonds), 249Bk (triangles), 249Cf (circles) and 253Es (vertical crosses) by HDEHP as a function of the extractant concentration. Aqueous phase: 1 mM 343HOPO in 0.1 M HNO3 and 1.9 M NaNO3. Organic phase: HDEHP in kerosene. b Corresponding separation factors. A log scale is used for clarity. See Supplementary Fig. 8 for results as a function of the phase ratio. c and d show the extraction yields of 249Bk and 249Cf by TODGA (solid lines) and separation factors Cf/Bk (dotted lines) as a function of the acidity and in the absence or presence of 1 mM 343HOPO, respectively. Aqueous phase: 0 or 1 mM 343HOPO in HNO3. Organic phase: 0.1 M TODGA in kerosene. T = 25 °C. O/A = 1, one contact. Points with arrows are lower limits

Bk purification using TODGA as extractant was also investigated. TODGA is more relevant than HDEHP for the production of heavy actinides since it is effective at high acidity and is therefore compatible with the post-irradiation metallic target dissolution step. The extraction behavior of Bk in a TODGA-based system has never been reported11, but high extraction yields for Bk3+ could be expected based on the behavior of Cf3+. In nitric solutions without chelator, quantitative co-extraction of 249Bk3+ and 249Cf3+ by TODGA was observed, leading to no practical separation between the metals (Fig. 5). In stark contrast, addition of 343HOPO drastically changes the Bk extraction profile: less than 1% Bk is extracted throughout the acidity range whereas Cf extraction remains undisturbed, due to the non-interaction between trivalent ions and the aqueous chelator at high acidity. The two adjacent actinides can be separated over a very broad acidity range (0.5–10 M HNO3). Even if an unfavorable initial ratio Cf/Bk was used in those experiments (Cf/Bk~12,000), 249Bk samples completely exempt of 249Cf were obtained, notably so after only a single extraction. Experiments at various concentrations of extractant further confirmed the reliability of the TODGA-HNO3−343HOPO separation formulation (Supplementary Fig. 9) with SFCf/Bk > 1,000,000, regardless of the TODGA and HNO3 concentrations. Additional separation experiments with Gd3+ and Lu3+ further evidenced the reliability of this system for purifying Bk (Supplementary Fig. 10). Finally, the separation method was tested at the mCi level. Legacy samples of 249Bk/249Cf used in previous studies44,47 were gathered, evaporated, incinerated and reconstituted in 3 M HNO3 solutions containing multiple mCi of 249Bk with a Cf/Bk ratio of ~3.4 mol/mol. The solution was split in five, 343HOPO was added, and an extraction step was performed using TODGA. As detailed in Table 1, after only a single step and regardless of the conditions used, very efficient separation was observed with the recovery of essentially pure 249Bk in the aqueous phase (radiopurity > 99.999%, chemical purity > 99.8%) and high-purity 249Cf in the organic phase (chemical purity > 99.5%). These results further confirm the proposed strategy could be used with high-activity samples, and scaled up to either produce high-purity Bk isotopes or to remove Bk traces during Cm, Cf, Es, or Fm production. Subsequent recovery of all isotopes would be facilitated by incineration and reconstitution in the desired matrix.

Table 1 Separation of 249Bk and 249Cf at the mCi level using TODGA and 343HOPOa

Noteworthy, the results presented above, although already providing better Cf/Bk separation than with any published method, do not represent optimum system performance since 343HOPO was not initially developed for separation applications and molecules with even higher selectivity could be designed. In addition, the three isotope purification examples examined in this work demonstrate the versatility of the proposed separation strategy, which could undoubtedly be transposed to other critical challenges1, such as those encountered with 89Zr4+/Y3+, 177Lu3+/Hf4+, 134La3+/134Ce4+, or 117mSn4+/116Cd2+ purifications. We anticipate that the use of HOPO ligand derivatives as aqueous chelating hold-back reagents could pave the way to more reliable, flexible and efficient methodologies for metal cation separations.

Methods

Caution

The following isotopes were used in this work: 153Gd (ε, t1/2 = 240 days, 130 TBq/g), 177Lu (β, t1/2 = 6.6 days, 4,100 TBq/g), 225Ac (α, t1/2 = 9.95 days, 2,100 TBq/g), 233U (α, t1/2 = 159200 years, 0.36 GBq/g), 241Pu (β, t1/2 = 14.3 years, 3.8 TBq/g), 242Pu (α, t1/2 = 3.74 × 105 years, 0.15 GBq/g), 243Am (α, t1/2 = 7388 year, 7.4 GBq/g), 249Bk (β, t1/2 = 0.9 year, 61 TBq/g), 249Cf (α, t1/2 = 352 year, 0.15 TBq/g), and 253Es (α, t1/2 = 20.5 days, 932 TBq/g). All are highly radioactive, presenting serious health risks, and were manipulated in facilities specially designed for safe handling of long-lived radioactive materials at the Lawrence Berkeley National Laboratory (LBNL).

Materials

153Gd(III) chloride and 233U(VI) nitrate were purchased from Eckert & Ziegler Isotope Products (Valencia, CA). 177Lu(III) chloride was purchased from Perkin Elmer Health Sciences (Shelton, CT). A Pu(IV) chloride stock solution containing a 50/50 mixture (Bq/Bq) of 241Pu and 242Pu and a stock solution of 243Am(III), prepared by dissolution of 243Am2O3 in 1 M HNO3, were from LBNL inventory. 225Ac(III), 249Bk(III), and 249Cf(III) were obtained as chlorides from ORNL. A 253Es(III) perchlorate solid sample was provided by Prof. J. Shafer (Colorado School of Mines). 343HOPO was from LBNL inventory14. Standard solutions of 0.1 M and 6.0 M HNO3 (BDH VWR Analytical), 70% HNO3 (Sigma Aldrich), NaNO3 (>99%, ACS grade, VWR), sodium lactate (Sigma Aldrich), TODGA (>99%, Technocomm Ltd.), HDEHP (>95%, Merck), tributyl phosphate (TBP, >98%, Alpha Aesar), kerosene low odor (Alpha Aesar), DTPA (>98%, TCI), and Ultima Gold LLT (Perkin Elmer) were used as received. All solutions were prepared using deionized water purified by a Millipore Milli-Q reverse osmosis cartridge system. Stocks were stored at 8 °C in the dark between experiments.

Methods

pH measurements were performed with a glass electrode (Metrohm - Micro Combi - response to [H+]) calibrated at 25.0 °C using three NIST standards. Extraction samples were analyzed by liquid scintillation counting (LSC). The distribution coefficient, D(M), of a given metal, M, is defined in Eq. (1), where [M]organic and [M]aqueous are the respective total concentrations of M in the organic and aqueous layers, after extraction. Both concentrations are proportional to the volumetric activity (in Bq L−1) determined by LSC. The separation factor, SFM1/M2, between two metals, M1 and M2, and extraction yield were calculated according to Eq. (2) and Eq. (3), respectively.

$$D\left( {\mathrm{M}} \right) = \frac{{\left[ {\mathrm{M}} \right]_{{\mathrm{organic}}}}}{{\left[ {\mathrm{M}} \right]_{{\mathrm{aqueous}}}}} = \frac{{[{\mathrm{Activity}}]_{{\mathrm{organic}}}}}{{[{\mathrm{Activity}}]_{{\mathrm{aqueous}}}}}$$
(1)
$${\mathrm{SF}}_{{\mathrm{M}}1/{\mathrm{M}}2} = \frac{{D({\mathrm{M}}_1)}}{{D({\mathrm{M}}_2)}}$$
(2)
$$\% {\mathrm{Extraction}} = \frac{{[{\mathrm{Activity}}]_{{\mathrm{organic}}} \times V_{{\mathrm{organic}}}}}{{[{\mathrm{Activity}}]_{{\mathrm{organic}}} \times V_{{\mathrm{organic}}} + [{\mathrm{Activity}}]_{{\mathrm{aqueous}}} \times V_{{\mathrm{aqueous}}}}} \times 100$$
(3)

In a typical experiment, the solvent (extractant diluted in kerosene) was pre-conditioned by shaking one volume of solvent with three volumes of aqueous phase (typically HNO3) at room temperature for 1 h, thrice. For radioisotope extractions, at least 400 µL aqueous phase (typically containing HNO3, a chelator and a radioisotope) and solvent were placed in air-tight screw-capped plastic tubes, triply-contained, and shaken in a thermoshaker at 300 rpm, 25 °C, for at least 30 min. Samples were then centrifuged for 5 min at 3000 rpm and phases separated before analysis. LSC analyses were performed on a Packard Tri-Carb B4430 instrument (Perkin Elmer) after mixing sample aliquots or sample dilution aliquots (10–200 µL) with 10 mL of scintillation cocktail (UltimaGold LLT). Samples were counted for at least 6 min and results were background subtracted. The analytical samples contained between 0 and 800,000 CPM. Mixtures of 249Bk and 249Cf were analyzed using α/β discrimination and energy windows were set to 0–50 keV for low-energy β particles of 249Bk and 50–1000 keV for α particles of 249Cf. 243Am and 225Ac samples were counted at secular equilibrium.

Data availability

All data generated or analysed during this study are included in this published article (and its supplementary information files).

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Acknowledgements

This work was supported by the U.S. Department of Energy, Office of Science, Office of Basic Energy Sciences, Chemical Sciences, Geosciences, and Biosciences Division at LBNL under Contract DE-AC02–05CH11231. The Radiochemical Engineering and Development Center at ORNL is supported by the U.S. Department of Energy, Isotope Development and Production for Research and Applications Program. We thank Dr. Wayne Lukens Jr. (LBNL) for preparation of the Pu starting material, and Prof. Jenifer Shafer (Colorado School of Mines) for providing the Es starting material.

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G.J-P.D. and R.J.A. designed the research. G-J.P.D. and A.R. collected experimental data. All of the authors discussed the results and commented on the manuscript.

Correspondence to Rebecca J. Abergel.

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R.J.A. and G-J.P.D. are listed as inventors on patent applications filed by LBNL and describing inventions related to the research results presented here. The remaining authors declare no competing interests.

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