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Novel DGT Configurations for the Assessment of Bioavailable Plutonium, Americium, and Uranium in Marine and Freshwater Environments

  • Joshua D. Chaplin
    Joshua D. Chaplin
    Institute of Radiation Physics, Lausanne University Hospital and University of Lausanne, 1 Rue du Grand-Pré, CH-1007 Lausanne, Switzerland
  • Phillip E. Warwick
    Phillip E. Warwick
    School of Ocean and Earth Science, University of Southampton, National Oceanography Centre, European Way, Southampton SO14 3ZH, United Kingdom
  • Andrew B. Cundy
    Andrew B. Cundy
    School of Ocean and Earth Science, University of Southampton, National Oceanography Centre, European Way, Southampton SO14 3ZH, United Kingdom
  • François Bochud
    François Bochud
    Institute of Radiation Physics, Lausanne University Hospital and University of Lausanne, 1 Rue du Grand-Pré, CH-1007 Lausanne, Switzerland
  • , and 
  • Pascal Froidevaux*
    Pascal Froidevaux
    Institute of Radiation Physics, Lausanne University Hospital and University of Lausanne, 1 Rue du Grand-Pré, CH-1007 Lausanne, Switzerland
    *Email: [email protected]
Cite this: Anal. Chem. 2021, 93, 35, 11937–11945
Publication Date (Web):August 25, 2021
https://doi.org/10.1021/acs.analchem.1c01342

Copyright © 2021 The Authors. Published by American Chemical Society. This publication is licensed under

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Abstract

Plutonium, americium, and uranium contribute to the radioactive contamination of the environment and are risk factors for elevated radiation exposure via ingestion through food or water. Due to the significant environmental inventory of these radioelements, a sampling method to accurately monitor their bioavailable concentrations in natural waters is necessary, especially since physicochemical factors can cause significant temporal fluctuations in their waterborne concentrations. To this end, we engineered novel diffusive gradients in thin-film (DGT) configurations using resin gels, which are selective for UO22+, Pu(IV + V), and Am(III) among an excess of extraneous cations. In this work, we also report an improved synthesis of our in-house ion-imprinted polymer resin, which we used to manufacture a resin gel to capture Am(III). The effective diffusion coefficients of Pu, Am, and U in agarose cross-linked polyacrylamide were determined in freshwater and seawater simulants and in natural seawater, to calibrate these configurations for environmental deployments.

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Note Added After ASAP Publication

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Due to a production error, the version of this paper that was published ASAP on August 25, 2021, was missing a symbol in eq 1. The corrected version was reposted August 26, 2021.

Plutonium, americium, and uranium are radioactive and biotoxic actinides whose most abundant isotopes emit mutagenic α(24He) particles. These radionuclides persist in the environment due to their long half-lives, therefore presenting particular concern when they contaminate land and water. Following significant environmental releases due to nuclear weapon fallout, reactor-core breaches, authorized releases from fuel reprocessing, and other miscellaneous sources, it is critical to monitor and fully understand the behavior of Pu, Am, and U in natural waters.
The oceans in particular have accumulated a significant actinide inventory, presenting concern to marine ecosystems and radionuclide transfer into the human food chain. For example, 717 TBq of 239+240Pu was released into the Irish Sea from the Sellafield fuel reprocessing facility (U.K.) between 1952 and 1995. (1) Furthermore, radionuclides often concentrate within marine life and sediments. (2−4) Spot sampling techniques, whereby water samples are retrieved and analyzed ex situ, are widely used to calculate waterborne radionuclide concentrations. Given that these concentrations continuously fluctuate throughout time due to a range of factors, including complexation effects as a function of variable physicochemical parameters, seawater actinide concentrations are not generalizable but rather are time- and site-specific. This, in addition to phylogenetic effects, (5,6) likely explains why concentration factors (CFs) in marine life vary widely between studies for the same organism and radionuclide. (7−15)
We suggest that the diffusive gradients in thin-film (DGT) sampling technique may be a more valid alternative to spot sampling and therefore provide a better predictor of the toxic effects of actinides to marine and other aquatic life. DGT samplers can be deployed in situ for extended periods (>14 days), producing time-weighted-average concentrations, which account for concentration fluctuations throughout the deployment period. Furthermore, DGT selectively analyzes the labile fraction of the target contaminant(s), which consists of soluble free (cationic) and metal-complex species, (16−19) which are therefore fully bioavailable. Since accumulations in the resin gel are speciation-dependent, this means that DGT analyzes the chemical toxicity in addition to the radiological toxicity for radionuclides. Moreover, radionuclide speciation is fundamentally important for environmental mobility and biokinetics, which will impact on the dose committed to organisms.
A DGT sampler consists of a plastic acrylonitrile butadiene styrene (ABS) housing, which hosts three interior layers: an exposed 0.45 μm polysulfone membrane filter, an intermediary diffusive gel, and an innermost resin gel. Polyacrylamide, cross-linked with an agarose derivative (APA), is used in most DGT configurations and in this work as the diffusive layer. This controls the rate at which the target analyte(s) are delivered to the resin gel (their diffusion coefficient through APA, D, cm2·s–1). The analyte is adhered to a suitable adsorbent embedded within the resin gel. The labile waterborne concentration of the analyte according to DGT (cDGT) can be calculated with eq 1, following measurement of the mass or activity (A) of the analyte in the eluate of the binding gel. The other components of eq 1 are described in the Experimental Section.
(1)
The analysis of radionuclides by DGT presents unique challenges, as certain radioisotopes are short-lived and therefore require an extended deployment period to accumulate sufficient masses in the DGT resin gel for analysis by suitable techniques. The resin which is used in the DGT resin gel therefore needs to be selective for its target analyte(s) among spectator ions so that it demonstrates linear temporal uptake of its target analyte(s), especially in seawater where these extraneous ions could quickly saturate the binding sites in the resin if it is not selective. Previous studies have dealt with the analysis of radionuclides (and more specifically the actinides) by DGT, including for U in natural waters (20−22) and for Pu in freshwater systems (23−26) in previous work in our laboratories. However, to our knowledge, DGT has never been applied to Am in any context, while U is the only actinide to have been studied with DGT in seawater. (22,27) Therefore, there remains a scope to develop DGT for Pu and Am measures in seawater and also for Am measures in freshwater. Furthermore, current DGT configurations for marine U suffer from considerable limitations, which would be solved using a more selective and robust resin. In this work, we therefore aimed to develop and characterize DGT configurations with novel resin gels, which are selective for the target radionuclides in seawater and which have high uptake capacities for their target radionuclide(s). This advance would facilitate the capture of sufficient masses of low-abundance-sensitivity isotopes for detection by techniques such as accelerator mass spectrometry. (28)
First, we developed a novel DGT configuration for the uranyl (UO22+) oxycation. U exists in nature between U(IV) and U(VI), of which only U(VI) is soluble as (UO22+) and complexes thereof. In seawater, UO22+ is primarily speciated as ternary U–carbonate complexes, where the dominant species is [Ca2UO2(CO3)3](aq). (29) Previous work by Turner et al. successfully used Metsorb, Chelex-100, and MnO2 resin gels for short-term (>24 h) marine UO22+ analyses by DGT. (21,22) The maximum marine deployment time during which linear uptake by the DGT sampler was observed in this work was 4 days (with MnO2). (22) Owing to the redox sensitivity of MnO2, we sought to develop an alternative solution that is Eh-robust, to support DGT sampler deployments in anoxic conditions in sediment and throughout the water column. To this end, we manufactured polyacrylamide (PAM) resin gels hosting the KMS-1 extractant (30−32)—a layered chalcogenide with a high kd of 104–106 for UO22+ across the pH range 2–9. (32) We also applied the KMS-1 configuration for Pu(IV + V) measure in freshwater and seawater, while also calibrating the existing Chelex-100 DGT configuration for marine Pu capture. We performed further testing for marine UO22+ and Pu(IV + V) using the organic–inorganic thiostannate FJSM-SnS (33,34) in a DGT configuration.
The need to effectively monitor bioavailable aquatic Am(III) is highlighted by the fact that CFs for Am have been reported to be higher than for Pu, (8) while ingrowth of 241Am (from β decay of 241Pu) has been estimated to add 8 TBq·yr–1 to the 241Am inventory of the Irish Sea. (35) Furthermore, there is currently little knowledge on the environmental speciation of Am, save for its identification as a ternary biscarbonato complex in seawater [NaAm(CO3)2.nH2O]. (36) To develop a suitable DGT configuration for freshwater and marine Am(III), we developed a novel resin gel by embedding our in-house ion-imprinted polymer resin (denoted herein as IIP-Y3+) into polyacrylamide. IIP-Y3+ is selective for trivalent cations and excludes other cations such as Ca2+, even when present in g·L–1 concentrations, as is the case in seawater. Furthermore, its extraction capacity for Y(III) is >2 mg·g–1, (37) meaning that it is largely sufficient for Am(III) extraction because of the much lower number of Am atoms involved in the extraction procedure compared to Y. We have recently developed an improved and more scalable synthesis of IIP-Y3+, which we report herein.
To calibrate the novel DGT configurations developed in this work, we used a diffusion cell to calculate the effective diffusion coefficients of Pu(IV), Pu(V), Am(III), and UO22+ through agarose cross-linked polyacrylamide (D) in solutions of buffered 10 mM NaNO3 nitrate-MOPS solution (“NMS”, a reference solution and approximation for freshwater conditions), seawater simulant (SWS), commercial aquarium seawater (CASW), and natural seawater directly retrieved from the environment (NSW-RE). We then validated the configurations by manufacturing DGT samplers for exposure in the same solutions.

Experimental Section

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Materials

All reagents used were of analytical grade. The KMS-1 extractant (K2xMnxSn3–xS6, x = 0.5–0.95) was synthesized by the hydrothermal method reported in point C in the Supporting Information of Manos et al. (30) The FJSM-SnS extractant ([Me2NH2]1.33[MeNH]0.67Sn3S7·1.25H2O) was synthesized by the gram-scale hydrothermal method reported by Qi et al. (34) Plastic housings, Chelex-100 resin gel, and all APA diffusive gels were purchased from DGT Research Ltd., Lancaster, U.K. A depleted-uranium(+VI) source was prepared by dissolving UO2(NO3)2·6H2O (Merck) in 0.1 M HCl. Other sources (233U, 238Pu, 239Pu, and 241Am) and yield tracers (232U, 242Pu, and 243Am) were prepared by the Radiometrology Unit at Lausanne University Hospital’s Institute of Radiation Physics, traceable to NIST sources.

IIP-Y3+ Synthesis

IIP-Y3+ was synthesized using the ion-imprinted polymer principle. (37−41) Briefly, the complex Y(L1)3(NO3)3 is imprinted in a styrene/divinylbenzene network using a polymer emulsion synthesis. After removal of the template Y(III) cation, the resin is suitable for the extraction of trivalent cations including lanthanides, lanthanoids, and certain actinides such as Am(III). In this work, we used a modified procedure to obtain the ligand L1 in a one-pot synthesis, as described by Devi et al. for amide synthesis from picolinic acid. (42) This is quicker and more scalable than previously reported (Scheme 1). (37)

Scheme 1

Scheme 1. Synthesis of Ligand L1a

aDipicolinic acid is refluxed with SOCl2 overnight. After excess SOCl2 removal by vacuum distillation, the residue is dissolved in dry CH2Cl2. K3PO4 is added as a H+ acceptor and vinylaniline dissolved in CH2Cl2 is added dropwise. The CH2Cl2 is then evaporated, and a basic water solution is added to extract the anion of ligand L1 in the water phase. The di-substituted amide present as an impurity is filtered off and addition of HCl precipitates L1, which is then filtered and dried in a desiccator (η ≃ 65% mass).

Resin Gel Syntheses

Resin gels of thickness 0.5 mm were manufactured in 9 × 9 or 23 × 6 cm2 sheets using our custom injection apparatus (Figure 1). To manufacture the IIP-Y3+ resin gel, 5.0 mL of 29:1 N,N′-methylene-bis-acrylamide (Bio-Rad) was diluted with 4.8 mL of deionized H2O. N,N,N′,N′-Tetramethylethane-1,2-diamine (TEMED, 40 μL, Bio-Rad) and IIP-Y3+ resin (200 mg) were added to the solution. 100 μL 13% aqueous ammonium persulfate (APS, Bio-Rad) solution was added to initiate polymerization while thoroughly mixing to homogenize the resin particle distribution. Five seconds after the APS was added, the solution was collected in a syringe and injected into the apparatus. Polymerization occurred within minutes, allowing the resin particles to settle toward the lower surface of the resin gel.

Figure 1

Figure 1. Injection apparatus used to manufacture resin gels.

To synthesize the KMS-1 and FJSM-SnS resin gels, a solution of 5.0 mL of 29:1 N,N′-methylene-bis-acrylamide, 4.05 mL of deionized H2O, 0.75 mL of agarose cross-linker solution (2% aqueous, DGT Research), and 200 μL of TEMED was added into a pestle containing 450 mg of the mortar-ground resin. 20% Aqueous APS (250 μL) was added to initiate polymerization.
After allowing 15–30 min for polymerization, resin gels were hydrated with dropwise addition of 10 mM NaNO3 or 0.3 M NaCl as necessary to ease retrieval from the glass; this depended on whether the gels were destined for experiments in NMS (in which case, 10 mM NaNO3 was used) or SWS/CASW/NSW-RE (in which case, 0.3 M NaCl was used). The gels were then stored in the same solution in a fridge at 4 °C. This was done to remove any unreacted acrylamide groups from the polymer structure while establishing ionic equilibrium prior to experimentation. The KMS-1 resin gel was additionally washed in 0.1 M KCl overnight before storage in 10 mM NaNO3 or 0.3 M NaCl.

Solutions

A reference solution containing an electrolyte (10 mM NaNO3, Sigma-Aldrich) was buffered with 10 mM 3-(N-morpholino)propanesulfonic acid (MOPS, Sigma-Aldrich) and used at between pH 5–6.5, the “nitrate-MOPS solution” (NMS). A seawater simulant (“SWS”) was prepared per Kester et al. (43) at pH 7.75. To prepare the commercial aquarium seawater (CASW) solution, 16 L of Two Little Fishies Accurasea Natural Seawater at pH 8.1 was poured into a 20 L plastic tub. A live rock was retrieved from an aquarium hosting fish and marine flora and placed in the tub, and the water was exposed to the atmosphere for 1 week to cultivate a microbiome. Oxidation and flow were maintained throughout with a Jecod SW-2 Propeller Pump Wavemaker set at 50% flow rate (2250 L·h–1). After 1 week, the CASW was spiked with 20 Bq of the analyte isotopes and left for a further 48 h to ensure the analytes were at complexation equilibrium before deploying samplers in the solution. The oxidation state of the 239Pu source was not manipulated before addition to the CASW, to allow the Pu to reach a natural equilibrium between its oxidation states with the objective of this being representative of its equilibrium in the natural marine environment. Pu(IV)/Pu(V) ratios at equilibrium in the SWS, and CASW solutions were determined by taking two identical samples of 2–3 mL, diluting to 20 mL and selectively adsorbing Pu(IV) onto 100 mg silica gel (Merck, 70–230 mesh). The solution was magnetically stirred at 250 rpm for at least 2 h, and the silica gel was separated with a 0.45 μM borosilicate syringe filter. The filtrate was considered as the Pu(V) fraction. Natural estuarine seawater from the Ravenglass Estuary, U.K., (NSW-RE) was retrieved on site on 24 August 2020 and stored in an airtight carboy. The NSW-RE was re-exposed to the atmosphere on 27 January 2021 and filtered through a 0.45 μm filter paper before use.
The analytes added to these solutions were 238U (with accompanying U-isotopes at depleted-uranium ratios) or 233U, 238Pu or 239Pu, and 241Am. We do not consider the mass difference between 10 Bq of 238Pu and 239Pu to have affected any results at the concentrations we used, as similarly demonstrated in previous work concerning DGT and Pu. (25) Pu sources were prepared at oxidation state +IV or +V according to previously described methods, using a sulfate buffer for Pu(IV) (44) and KMnO2 oxidation followed by photoreduction and back extraction for Pu(V). (45)

Diffusion Cell Experiments

Diffusion experiments were performed in our purpose-built Teflon diffusion cell (see previous work by Cusnir et al. (23) for full methodology) to calculate D of each analyte. Briefly, the Section A solution contains NMS, SWS, or CASW, which is spiked with 10 Bq of the analyte isotope, and the Section B solution contains the equivalent nonradioactive NMS, SWS, or CASW. These solutions were prepared prior to experimentation by magnetic stirring at 250 rpm overnight while exposed to the atmosphere, ensuring equilibration with natural CO2 and complexation equilibrium of the actinides in the solution under these conditions. The solutions were added to their respective sections, which were interconnected through a 0.39 mm DGT Research APA diaphragm. The diffusion of the actinide species through the gel was observed as a function of time by measuring the Section B activity concentration. This was carried out at short timescales of up to 5 h so that back-diffusion of the radionuclides into Section A would not affect a linear diffusion trend.

Actinide Analyses

Samples were traced with 25 mBq of 232U, 242Pu, or 243Am as appropriate prior to solid-phase extraction. Pu samples were dissolved in several milliliters of 8 M HNO3. Fe(III) (50 μg) was added before 100 mg of ascorbic acid was added to reduce Fe(III) to Fe(II), consequently co-reducing all Pu to Pu(III). Pu(III) was then fixed to Pu(IV) by adding 40–60 mg of NaNO2 while heating on a hot plate at 150 °C for 10 min. This prepared the sample for extraction on a Bio-Rad Poly-Prep column containing 2 mL of Bio-Rad AG 1-X4 resin. These columns were washed with 3 × 5 mL of 8 M HNO3 beaker washouts and subsequently with 15 mL of 9 M HCl to elute Th. Pu was eluted with 15 mL of H3NO·HCl (5% aq.).
U samples were dissolved in 3 mL of 8 M HNO3 for extraction on 100 mg of UTEVA (Triskem, France) resin, within a 1 mL micropipette cartridge column. Three 1.5 mL 8 M HNO3 beaker washouts were transferred through the column. The columns were washed with 6 M HCl to remove residual Th, and U was eluted with 5 mL of 0.01M HCl.
Am samples were evaporated to dryness and were then dissolved in Milli-Q H2O, which had been adjusted to pH 3 with dropwise addition of 0.1 M HCl. This solution was loaded onto a 2 mL cartridge packed with IIP-Y3+ resin. IIP-Y3+ was prewashed by passing 10 mL of 3 M HCl through the cartridge at 1 mL·min–1 using a syringe pusher. The column was conditioned with 20 mL of H2O (pH 3), and the samples were dissolved in H2O (pH 3) and loaded on IIP-Y3+. The column was washed with 3 × 5 mL H2O (pH 3) beaker washouts, and Am(III) was eluted with 20 mL of 3 M HCl. IIP-Y3+ columns were cleaned after elution with 5 mL of 0.1 M C2H2O4 before regeneration for reuse with 40 mL of Milli-Q H2O (pH 3).
Pu, U, and Am fractions were treated for electrodeposition on stainless steel disks as reported by Bajo et al. (44) Disks were counted using 450 mm2 passivated implanted planar silicon detectors in α-spectrometers (α Analyst, Canberra, France) with Apex software.

Determination of the Diffusion Coefficient

D (cm2·s–1) is the diffusion coefficient. For diffusion cell experiments, D at the temperature of experimentation, DTEX, can be calculated using eq 2
(2)
where Δg is the material diffusive layer (cm), S is the area of the diffusive window (cm2), c0soln is the concentration of the analyte in solution (taken at the beginning of the experiment, mBq·mL–1), and slope is the activity (A, mBq) diffused into section B of the cell against time (t, seconds). For note:
(3)
where δg is the diffusive APA gel thickness and δf is the thickness of the membrane filter (140 μm). The filter membrane was only present in deployments of the fully assembled DGT samplers, whereas no membrane filter was used in the diffusion cell; thus, for diffusion cell experiments, Δg = δg. No δdbl was included in diffusion cell experiments due to the thorough mixing of the solutions by the stirrers, which were in close proximity (2.5 cm) to the gel diaphragm, which we consider would have minimized any δdbl to a negligible thickness. DTEX was normalized to 25 °C (DT25) using the Stokes–Einstein equation to combine temperature and viscosity corrections using eq 4. D is always reported in this work as DT25.
(4)

Laboratory Sampler Deployments

Several DGT samplers were deployed in NMS and SWS solutions of known c0soln, within 1 L plastic beakers for periods of up to 3 weeks. Samplers were individually retrieved at various intervals, to observe if they captured the analyte in a linear manner as a function of time. The samplers were secured in plastic supports with each sampler facing the same direction, tangential to the revolving current produced by a magnetic stirrer at the base of the beaker. Experiments involving Pu in NMS or SWS were performed inside a N2-saturated glovebox to preserve the oxidation state at which the Pu had been prepared as best as possible. After sampler retrieval, the housings were disassembled, and the membrane filters and diffusive gels were discarded. The resin gel was placed in 20 mL of a tracer-spiked eluent (8 M HNO3 for Chelex-100, 8 M HNO3 plus three droplets of H2O2 (30% aq.) for KMS-1 and FJSM-SnS, and 3 M HCl for IIP-Y3+). Eluents were left overnight, before the resin gel was filtered off with a 0.45 μM borosilicate syringe filter. The filtered eluent was prepared for chemical separation(s) and measurement. For experiments where Pu and U were eluted from the same resin gel disk, the Pu was separated first on Bio-Rad AG 1-X4 resin as described earlier. The waste from the loading solution was retained and evaporated to dryness; then, the residue was redissolved in 8 M HNO3 for U separation on UTEVA resin as also described earlier. As c0soln of these solutions was known, the activity captured in each sampler (A) was fed into eqs 2 and 3 to derive D. Uncertainties on D were calculated using combined uncertainty summation, including slope uncertainty calculations with Python script (provided in the Supporting Information), using estimates of σ for volume (2%), Δg (5%), and S (5%). IIP-Y3+ samplers with δg of 1.96 mm were deployed in Am(III)-spiked NMS to derive δdbl from the relationship described in eq 4 of Warnken et al. (46) An average δdbl of 490 μm was calculated (n = 5), which corresponds to that obtained in previous work with actinides and DGT (14) (480 μm).

Results and Discussion

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Resin and Resin Gel Syntheses

The synthesis of the KMS-1 extractant was replicated according to the reported procedure. (30) We also recovered a similar yield for KMS-1 (≃76% total mass) to Manos et al. (30) (81%). We favor the use of KMS-1 for a DGT configuration to target U and Pu, as its synthesis is quicker and more scalable than other layered sulfide resins.
Our streamlined ligand L1 synthesis for the manufacture of the IIP-Y3+ resin is replicable and can produce tens of grams of IIP-Y3+ per pot within 4 days.
The recipe for the KMS-1 resin gel required further development, as when initially using the same reagent proportions as for IIP-Y3+, the KMS-1 remained in a separate liquid phase below a blank PAM gel which polymerized above. Increasing the TEMED and APS constituents consistently produced an inhomogeneous gel if polymerization was successful. The addition of the DGT Research agarose cross-linker (2% aq.) solution in combination with the reported reagent proportions produced a replicable and homogeneous KMS-1 resin gel. This and the IIP-Y3+ resin gel recipe scale between both sizes of our injection apparatus.

D Determinations for UO22+

Diffusion coefficient data for all elements is presented in Table 1. Data from diffusion cell experiments are presented in Figure 2, whilst data from DGT expositions are presented in Figure 3.
Table 1. Diffusion Coefficients, Solution Concentrations, and cDGT Produced in Diffusion Cell Experiments and DGT Expositionsh
analytehost solutionpHD (diffusion cell-derived) (×10–6 cm2·s–1)diffusion R2resin used in resin gelresin gel uptake R2cDGT (mBq·mL–1)c0soln (mBq·mL–1)deployment period (days)g
U(VI) (UO22+)NMS5.005.02 ± 0.290.982KMS-10.9974.70 ± 0.514.77 ± 0.444.22
SWS7.751.35 ± 0.240.942KMS-10.96616.7 ± 1.6715.6 ± 1.185.13
CASW8.101.73 ± 0.250.959KMS-1no significant uptake observed1.04 ± 0.1120.7
IIP-Y3+no significant uptake observed7.79 ± 0.687.00
FJSM-SnSno significant uptake observed1.70 ± 0.1919.7
Chelex-100no significant uptake observed1.70 ± 0.1919.7
CASWa7.00not measured in diffusion cellKMS-1no significant uptake observed1.44 ± 0.1421.0
FJSM-SnSno significant uptake observed1.44 ± 0.1421.0
NSW-RE8.05not measured in diffusion cellKMS-10.9270.0663 ± 0.0109e0.0566 ± 0.001414.6
Pu(IV)NMS6.502.38 ± 0.470.979Chelex-1000.9984.07 ± 0.445.20 ± 0.301.26
SWSb7.75not measured in diffusion cellChelex-1000.9691.21 ± 0.28f1.04 ± 0.262.54
KMS-10.9901.56 ± 0.29f1.04 ± 0.262.54
Pu(IV) + Pu(V)CASWd8.102.59 ± 0.210.991Chelex-1000.9570.340 ± 0.0830.405 ± 0.0766.02
KMS-10.9851.49 ± 0.261.28 ± 0.4215.1
IIP-Y3+no significant uptake observed1.28 ± 0.4215.1
Pu(V)SWSc7.75not measured in diffusion cellChelex-1000.9990.425 ± 0.045f0.358 ± 0.0422.54
KMS-10.9580.434 ± 0.014f0.358 ± 0.0422.54
Am(III)NMS5–6.54.12 ± 0.29 (pH 6.5)0.991IIP-Y3+0.9959.05 ± 1.07 (pH 5)7.91 ± 1.593.05
SWS7.751.10 ± 0.110.996IIP-Y3+0.986328 ± 62.7207 ± 11.65.00
CASW8.101.56 ± 0.280.972IIP-Y3+0.9910.173 ± 0.0320.230 ± 0.0515.02
a

No organic content added to the commercial product, and pH reduced to 7.

b

Pu(V) fraction: 6.8 ± 2.4%.

c

Pu(V) fraction: 100%.

d

Pu(V) fraction: 80 ± 14%.

e

Based on D of 1.73 × 10–6 cm2·s–1 for UO22+ in CASW.

f

Based on D of 2.59 × 10–6 cm2·s–1 for Pu(IV + V) in CASW.

g

The period between the initial exposition of the samplers and the retrieval of the final DGT sampler probe.

h

2σ uncertainties.

Figure 2

Figure 2. (a–c) Diffusion of (a), UO22+, (b) Am(III), and (c) Pu(IV) and Pu(V) through 0.39 mm APA gel diaphragm within diffusion cell containing NMS, SWS, CASW, and NSW-RE solutions. 2σ uncertainties on points. Y-intercepts normalized to 0 to emphasize slope comparisons. Refer to Table 1 footnote for Pu(IV) and Pu(V) constituents of solutions.

Figure 3

Figure 3. (a–c) Accumulation of (a), UO22+, (b) Am(III), and (c) Pu(IV) and Pu(V) in DGT resin gels deployed in NMS, SWS, CASW, and NSW-RE solutions. 2σ uncertainties on points. Y-intercepts normalized to 0 and total deployment times normalized to 24 h to emphasize slope comparisons. Refer to Table 1 footnotes for Pu(IV) and Pu(V) constituents of solutions.

D for UO22+ in NMS ((5.02 ± 0.26) × 10–6 cm2·s–1) closely corresponded to previous work under similar experimental conditions by Garmo et al. (5.60 × 10–6 cm2·s–1 for UO22+ in 10 mM NaNO3 at pH 5 (47)). DGTKMS-1 sampler deployments in NMS captured U in a linear manner as a function of time, with a cDGT of 4.70 ± 0.51 mBq·mL–1 compared to a c0soln of 4.77 ± 0.44 mBq·mL–1. This demonstrates the validity of the DGTKMS-1 configuration for measurements in NMS and also demonstrates that UO22+ is fully labile under these conditions at pH 5.
Effective D for UO22+ in SWS and CASW were 3 times lower than in NMS. This is most likely due to the difference in pH of the solutions; Li et al. found a similar dependence with U in alkaline waters. (48)D for UO22+ was similar in both SWS ((1.35 ± 0.23) × 10–6 cm2·s–1) and CASW ((1.73 ± 0.24) × 10–6 cm2·s–1), indicating that the presence of organic content does not seem to have a significant effect on UO22+ diffusion through the polyacrylamide diaphragm and that U–organic matter complexes do not adsorb to sites in the APA gel. However, the DGTKMS-1 configuration captured UO22+ in a linear manner in SWS but did not capture any significant activity in CASW at pH 8.1. This is despite the eluates of the same KMS-1 resin gel disks demonstrating linear Pu(IV + V) uptake throughout 15 days. These deployments were repeated several times with the same results. Having seen these data, we then manufactured the DGTFJSM-SnS configuration using the same reagent proportions that we optimized for the KMS-1 resin gel. DGTFJSM-SnS once more captured Pu in a linear manner as a function of time from CASW but did not capture any U. This confirmed that the sorption of UO22+ onto the resin under these conditions was not a phenomenon solely due to K+-exchange in the KMS-1 lattice, but also with organic amine [Me2NH2+]-exchange. We subsequently set up an aquarium with the Two Little Fishies Accurasea Natural Seawater, without adding the live rock and lowering the pH of the solution to 7 through dropwise addition of 0.1 M HCl. We redeployed KMS-1 samplers and FJSM-SnS samplers but still observed no U uptake under these conditions. Linear uptake of U could not be proven from eluates of DGTChelex-100 samplers in CASW, which is consistent with previous work with U in natural seawater by Hutchins et al. (27) Turner et al. (22) reported that DGTChelex-100 does show some degree of U uptake from seawater (albeit not linear after 8 h). This confirmed that the noncapture of U on DGTKMS-1 under these conditions is a solution phenomenon, which may be due to how the commercial seawater is treated prior to sale (UV irradiation); however, we do not know the full treatment process. We demonstrated with the diffusion cell that U diffuses linearly as a function of time through the APA gel and thus does not adsorb within this layer; therefore, we can infer from these results that the U in CASW likely formed kinetically inert complexes with organic matter at pH 7.0–8.1 that did not react with the active sites in the KMS-1 and FJSM-SnS resin lattices. However, U uptake was observed in NSW-RE with R2 for of 0.927 over 14 days (Table 1). If deriving D from the sampler exposition experiments by eq 2, using A as the activity eluted from the resin gel rather than the activity diffused into section B of the diffusion cell, D of UO22+ in NSW-RE is (1.83 ± 0.16) × 10–6 cm2·s–1, which closely corresponds to the D of UO22+ calculated in the diffusion cell hosting CASW of (1.73 ± 0.25) × 10–6 cm2·s–1. As NSW-RE was directly retrieved from the environment and untreated prior to use, we endorse the use of the DGTKMS-1 configuration for use in estuarine waters under these conditions. There also remains further scope for DGTKMS-1 to be used for other radionuclide analyses by DGT, especially for radiocaesium and radiostrontium, as Manos et al. have demonstrated efficient and rapid uptake of Cs+ (31) and Sr2+ (30) by KMS-1.

D Determinations for Pu(IV) and Pu(V)

We characterized the Pu(IV) and Pu(V) constituents of the SWS and CASW solutions as described in the methodology; we consider that Pu(III) or Pu(VI) would not be present in significant quantities in these solutions at natural physicochemical parameters. After preparing the Pu(IV) sulfate residue, dissolving it in SWS and stirring overnight, <7% of the total Pu was detected in the filtrate from the silica gel. Similarly, Pu(V) was also stable in SWS following its preparation with the back-extraction procedure, with 100% total Pu found in the Pu(V) fraction. The proportion of Pu(V) in the CASW was 80 ± 14%. This corresponds to previously reported marine Pu oxidation state data (87 ± 6% Pu(V) with little or no spatial or temporal variation (49)); therefore, we consider the Pu speciation in our CASW solution to be valid.
D for Pu(IV) in NMS ((2.38 ± 0.47) × 10–6 cm2·s–1) reaffirms the work of Cusnir et al., (25) who reported a D of (2.29 ± 0.15) × 10–6 cm2·s–1 under the same conditions. Unlike with UO22+, the D of Pu(IV + V) in CASW was similar to that in NMS, at (2.59 ± 0.21) × 10–6 cm2·s–1. This suggests that any diminishing effect on D between NMS and CASW by the pH (as was seen between D in NMS and SWS/CASW for UO22+) is offset by other factors. This demonstrates that Pu complexes, likely in a carbonated [Pu(V)-(CO3)n]+ form, are relatively mobile in CASW. Their transport is likely mainly colloid-facilitated, as demonstrated in previous work; (50−52) Pu(IV) has shown to be speciated as {PuO2}-type colloids in natural seawater. (53)
Both the DGTKMS-1 and DGTChelex-100 configurations captured Pu(IV) linearly as a function of time from SWS and CASW. Additionally, we demonstrated linear Pu(IV) uptake by DGTKMS-1 throughout a 15-day period in CASW with a close reproduction between cDGT and c0soln, endorsing DGTKMS-1 for marine Pu(IV + V) measures over this timescale.

D Determinations for Am(III)

To verify δdbl in our solutions, DGTIIP-Y3+ samplers with δg = 0.198 cm were deployed in SWS for 1, 2, 4, and 5 days exactly. The activities captured in the binding layers were compared with that of concurrent DGTIIP-Y3+ samplers of δg = 0.039 cm. δdbl was derived and ranged between 0.042 and 0.053 cm with a mean of 0.049 cm. This corresponds closely to previously determined δdbl under these conditions in previous work with DGT and Pu (0.048 cm); (26) therefore, we considered δdbl = 0.049 cm for all DGT sampler deployments. We considered that due to the thorough stirring of the solutions, δdbl would not cause significant variations in the D calculated from DGT sampler deployments.
D for Am(III) in NMS is comparable to that for other trivalent lanthanides, such as demonstrated by Garmo et al. for Eu(III) (5.1 × 10–6) in 10 mM NaNO3. (47)cDGT for Am(III) in NMS was also within the error range of c0soln that we calculated, despite the difference in pH between the experiments. We observed that the 241Am concentration was stable in the diffusion cell at pH 6.5 for 75 min; however, the Am hydrolyzed throughout a 3-day deployment period under the same conditions. Lowering the NMS pH to 5 maintained the stability of the Am(III) concentration for 3 days. We nevertheless consider that this reasonably represents that DGTIIP-Y3+ is valid for measures under freshwater conditions, with high temporal linearity of Am(III) capture in the IIP-Y3+ resin gel. We did not find significant activities of U or Pu in the IIP-Y3+ resin gel eluate, confirming the selectivity of IIP-Y3+ for trivalent cations. This is an especially beneficial trait for Am analysis under environmental conditions, as neighboring isobaric Pu masses will not be present in these samples if analyzing the gel eluates by mass spectrometric techniques. Additionally, given that we have successfully extracted Pu(III) on IIP-Y3+ in our laboratory (unpublished results), this further confirms the absence of any significant activity of reduced Pu(III) in our CASW solution.
A similar effect on D was observed between NMS and SWS/SW for Am(III) as for with UO22+, with D roughly 3 times lower in the seawater solutions; we attribute this predominantly to the pH of the solutions. Variation was observed between D between the diffusion cell experiments and sampler expositions in SWS and CASW, despite linear temporal Am(III) capture (R2 for of 0.986 and 0.991 for SWS and CASW, respectively). Having demonstrated that Am(III) is not adsorbed to the diffusive APA gel during diffusion experiments, the results in CASW likely demonstrate that a proportion of Am(III) forms complexes in the presence of organic matter, perhaps as might be the case with U in CASW at pH 8.1. However, log β3 values of 19.7–19.9 have previously been determined for Ln3+(L1)3 complexes with Eu and Tb. (37) Similar values can be expected for Am3+(L1)3 complexes, rendering IIP-Y3+ very competitive for Am3+ capture compared to other Am3+–organic matter complexes. In this respect, lower D in CASW likely demonstrates the lower diffusion capability of Mz+–organic matter complexes compared to mineral complexes (e.g., mostly carbonates and sulfates, which are present in SWS containing no organic matter). There remains clear further potential for the analysis of rare earth elements and other trivalent cations by DGTIIP-Y3+, especially as the widely used Chelex-100 DGT configuration may possibly be affected by strong carbonate complexation of the lanthanides.
The highly linear capture of the target analytes by the DGTKMS-1 and DGTIIP-Y3+ configurations has demonstrated that adhesion and elution factors of 1 can be assumed. Furthermore, this demonstrates that the resins do not saturate with extraneous cations, which might hinder linear temporal uptake of their target analytes. The calibration of these DGT configurations for freshwater and seawater has also been constrained, with high temporal linearity of diffusion for the effective D values in NMS and CASW. Having observed this, we endorse the DGTKMS-1 configuration for passive monitoring of UO22+ and Pu(IV + V), and the DGTIIP-Y3+ configuration for Am(III) in natural waters. Further work with these DGT configurations in marine aquatic systems is already underway in our laboratories, following field deployments of the samplers at a contaminated marine site.

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  • Corresponding Author
  • Authors
    • Joshua D. Chaplin - Institute of Radiation Physics, Lausanne University Hospital and University of Lausanne, 1 Rue du Grand-Pré, CH-1007 Lausanne, SwitzerlandOrcidhttps://orcid.org/0000-0002-6151-1942
    • Phillip E. Warwick - School of Ocean and Earth Science, University of Southampton, National Oceanography Centre, European Way, Southampton SO14 3ZH, United Kingdom
    • Andrew B. Cundy - School of Ocean and Earth Science, University of Southampton, National Oceanography Centre, European Way, Southampton SO14 3ZH, United Kingdom
    • François Bochud - Institute of Radiation Physics, Lausanne University Hospital and University of Lausanne, 1 Rue du Grand-Pré, CH-1007 Lausanne, Switzerland
  • Notes
    The authors declare no competing financial interest.

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The authors gratefully acknowledge funding under the Swiss National Science Foundation Fund No. 175492, which supported the PhD studentship associated with this project and the open access publishing of this work.

References

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  • Abstract

    Scheme 1

    Scheme 1. Synthesis of Ligand L1a

    aDipicolinic acid is refluxed with SOCl2 overnight. After excess SOCl2 removal by vacuum distillation, the residue is dissolved in dry CH2Cl2. K3PO4 is added as a H+ acceptor and vinylaniline dissolved in CH2Cl2 is added dropwise. The CH2Cl2 is then evaporated, and a basic water solution is added to extract the anion of ligand L1 in the water phase. The di-substituted amide present as an impurity is filtered off and addition of HCl precipitates L1, which is then filtered and dried in a desiccator (η ≃ 65% mass).

    Figure 1

    Figure 1. Injection apparatus used to manufacture resin gels.

    Figure 2

    Figure 2. (a–c) Diffusion of (a), UO22+, (b) Am(III), and (c) Pu(IV) and Pu(V) through 0.39 mm APA gel diaphragm within diffusion cell containing NMS, SWS, CASW, and NSW-RE solutions. 2σ uncertainties on points. Y-intercepts normalized to 0 to emphasize slope comparisons. Refer to Table 1 footnote for Pu(IV) and Pu(V) constituents of solutions.

    Figure 3

    Figure 3. (a–c) Accumulation of (a), UO22+, (b) Am(III), and (c) Pu(IV) and Pu(V) in DGT resin gels deployed in NMS, SWS, CASW, and NSW-RE solutions. 2σ uncertainties on points. Y-intercepts normalized to 0 and total deployment times normalized to 24 h to emphasize slope comparisons. Refer to Table 1 footnotes for Pu(IV) and Pu(V) constituents of solutions.

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