Contribution of Ternary Reaction to Pd Sorption on MX-80 in Na-Ca-Cl Solution at High Ionic Strength

Nagasaki, Shinya; Riddoch, Justin; Racette, Joshua

doi:https://doi.org/10.1155/2019/6572606

Science and Technology of Nuclear Installations

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Abstract Introduction Materials and Methods Results and Discussion Conclusions Data Availability Conflicts of Interest Acknowledgments Supplementary Materials References Copyright Related Articles

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Advanced Technologies in Nuclear Waste Management Process Design and Materials

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Research Article | Open Access

Volume 2019 | Article ID 6572606 | https://doi.org/10.1155/2019/6572606

Contribution of Ternary Reaction to Pd Sorption on MX-80 in Na-Ca-Cl Solution at High Ionic Strength

Shinya Nagasaki,¹Justin Riddoch,¹and Joshua Racette¹

Guest Editor: Rema Abdulaziz

Received01 Apr 2019

Revised23 May 2019

Accepted10 Jun 2019

Published24 Jun 2019

Abstract

In this study, we first examined the sorption of Pd on MX-80 in Na-Ca-ClO₄ solution as a function of (3–9) and ionic strength (0.1 M–4 M) and confirmed that the experimentally derived values could be fitted by a 2-site protolysis nonelectrostatic surface complexation and cation exchange (2SPNE SC/CE) model using three binary surface complexation constants previously estimated. Then, we investigated the sorption of Pd on MX-80 in Na-Ca-Cl-ClO₄ solution as a function of (3–9) and molar concentration ratio (0–∞) at the ionic strength = 4 M. We found that the sorption of Pd on MX-80 in Na-Ca-Cl-ClO₄ solution could be simulated only by the three binary and one ternary surface complexations (). This suggests that the contribution of other ternary surface complexations such as ≡S-OH ≡ ( = 1, 2 and 3) to Pd sorption in Na-Ca-Cl-ClO₄ solution with ionic strength = 4 M was negligibly small.

1. Introduction

Canadian sedimentary rocks are being considered as potential host rocks for a deep geologic repository (DGR) for used nuclear fuel. Some of these rocks in Canada (for example, Southern Ontario, Michigan Basin [1]) contain Na-Ca-Cl type brine solutions with total dissolved solids (TDS) concentration up to 350 g/L or with the ionic strength (I) as high as 7.2 M. Sorption of radionuclides onto host rocks surrounding a DGR and onto materials comprising the engineered barrier system is considered an important mechanism for retarding their subsurface transport from the repository to the biosphere [2–6]. Therefore, it is important to elucidate the sorption behaviour of radionuclides not only on host rocks, but also on engineered barrier materials such as bentonite.

The Nuclear Waste Management Organization of Canada (NWMO) has been maintaining a database of sorption distribution coefficients, , for Canadian sedimentary rocks and bentonite [2]. Palladium is selected as an element of interest by the NWMO, but the only existing relevant sorption data for Pd on bentonite had been measured in 0.01 and 0.1 M NaCl solutions [7]. Hence, sorption of Pd onto Queenston shale, illite (the major mineral constituent of Queenston shale), and MX-80 bentonite (the candidate material for engineered barrier in Canada) in Na-Ca-Cl solutions with ranging from 3 to 9 and I ranging from 0.01 M to 6 M was studied in our previous paper [8]. The 2-site protolysis nonelectrostatic surface complexation and cation exchange (2SPNE SC/CE) model [9, 10] with SIT parameters was applied to the dependence of values for illite and MX-80 (I ≤ 4 M), and the optimized surface complexation and cation exchange constants were estimated [8]. Since Pitzer parameters for Pd in Na-Ca-Cl solution are not completely compiled, we did not apply the 2SPNE SC/CE model to the values at I = 6 M. We found that Pd sorption could largely be accounted for with the formation of the ≡S-OPdOH, ≡S-, ≡S- surface species, and the ≡S-O₂Pd exchange species with 2Na⁺ for both sorbents, with the additional ≡S-OPd⁺ surface species for MX-80. We included four possible ternary surface complexations (≡S-OH + Pd²⁺ + xCl^-↔ ≡S- + H⁺; x = 1 – 4) in the fitting by 2SPNE SC/CE model, but only one reaction (≡S-OH + Pd²⁺ + 4Cl^-↔ ≡S- + H⁺) was found to contribute to the sorption in Na-Ca-Cl solutions with high I.

In this work, we first measured the sorption of Pd on MX-80 in Na-Ca-ClO₄ solutions as a function of and I and studied whether the experimentally derived values in the absence of Cl^- can be simulated by using our previously optimized constants. Then, we measured the sorption of Pd on MX-80 in Na-Ca-Cl-ClO₄ solutions as a function of and Cl^-/ molar concentration ratio (0–∞) at I = 4 M and investigated the contribution of ternary surface complexation to the Pd sorption on MX-80 at I = 4 M.

2. Materials and Methods

2.1. Chemicals, Solids, and Solutions

All chemicals used were reagent grade and were supplied from Fisher Scientific. Deionized water was prepared using a Milli-Q Direct 8 (18.2 MΩ·cm). The MX-80 bentonite sample was supplied by the American Colloid Company and was used as received. Pd used in experiments was derived from a 1000 ± 1 μg/mL standard solution with a natural isotopic abundance supplied by Agilent Technology. A Precise Controlled Atmosphere Glove Box (GB) supplied by Labconco was filled with N₂ gas (>99.999 %). The concentration of O₂ in the GB was smaller than 2 ppm.

The reference brine solution in Southern Ontario, SR-270-PW, is proposed by the NWMO [2]. It has a Na/Ca molar concentration ratio of 2.7. In this study, Na-Ca-ClO₄ solutions (Na/Ca molar concentration ratio = 2.7) with I = 0.1, 1, 2, 4 M were prepared by NaClO₄·H₂O and Ca(ClO₄)₂·4H₂O, and Na-Ca-Cl-ClO₄ solutions (Na/Ca ratio = 2.7; Cl^-/ ratio = 0.01, 0.1, 1, 10, 100, ∞) with I = 4 M were prepared by NaCl, CaCl₂·2H₂O, and NaClO₄·H₂O. Na-Ca-ClO₄ solution with I = 4 M was considered a case of Cl^-/ ratio = 0.

The pH values indicated on the pH meter () should be considered as operational values at high ionic strength (I ≥ 0.1 M) [11]. The relationships between the operational and the molar H⁺ concentrations () or the molal H⁺ concentration () were discussed in detail by Altmaier et al. [12, 13]. In this study, the relationships between (Fisher Scientific Accumet AB 150/micro accupHast pH combination electrode) and in solutions were determined by titration (Metrohm Ti-Touch 916), and the values were converted to the values.

2.2. Sorption Experiments

All sorption experiments were carried out in triplicate at 25°C. In preliminary tests, the sorption of Pd on the wall of a polycarbonate reaction vessel was found to be negligible. Initial concentration of Pd for all sorption tests was 1.0 × 10⁻⁷ M and was confirmed to be smaller than solubility of Pd [8]. The liquid/solid ratio was set to be 0.5 m³/kg.

We followed the sorption experimental procedure we conducted in Np(V) and Np(IV) sorption previously [14–16]. In the GB, MX-80 was added into a polycarbonate reaction vessel and Na-Ca-ClO₄ or Na-Ca-Cl-ClO₄ solution was added into the reaction vessel. The suspensions were kept in the GB for 3 to 4 days for preequilibration (the of solutions in contact with MX-80 was confirmed to be stabilized within 1 day in the preliminary tests). The reaction vessels were removed from the GB and the liquid and solid were separated by centrifugation for 120 min at 18,000 rpm (Beckman Coulter, Allegra X-30R). The reactions vessels were then transferred back into the GB and the liquid was removed by pipette. Na-Ca-ClO₄ or Na-Ca-Cl-ClO₄ solution was then added into the reaction vessel again, and a portion of the Pd standard solution was spiked into the reaction vessel. The of the solution was adjusted to the predecided values at 3 ≤ ≤ 9 by addition of 0.01 M HClO₄, 0.01 M HCl, or 0.01 M NaOH solution in the GB, and the reaction vessel was tightly sealed. Change in I and Cl^-/ ratio by addition of HClO₄, HCl, or NaOH could be neglected.

The reaction vessels were transferred from the GB to an incubator at 25°C (Infors HT Ectron) and were shaken for 14 days. Fourteen days were enough to reach to the sorption equilibrium [8]. The of the solution was measured once a day in the GB and readjusted to the original value if the changed by more than ± 0.3 from the original value. After 14 days, the liquid was separated from the solid by centrifugation for 120 minutes at 18,000 rpm at 25°C. We previously confirmed that the liquid phase was sufficiently separated from the solid phase by this method [14]. The of the liquid was measured in the GB, and an aliquot was sampled from the liquid phase of each reaction vessel. The concentration of Pd in the aliquot was measured by ICP-MS (Agilent ICP-MS 8800).

The value (m³/kg) is calculated according to Equation (1), where C_i is the initial concentration of Pd in solution (1.0 × 10⁻⁷ M), C_eq the concentration at sorption equilibrium (M), L the volume of liquid used in the sample (m³), and M the mass of solid used (kg). In this paper, the sorption of Pd on MX-80 is described by values.

2.3. Sorption Modelling

The , I, and Cl^-/ ratio dependence of values for MX-80 was fitted using the 2SPNE SC/CE model with the program PHREEQC [17]. The specific-ion interaction theory (SIT) was used for the computational method, as it accounts for the electrostatic interactions of all other ions in solution with the one ion of interest. This is necessary for accuracy when computing activity coefficients in solutions of high I. The Pitzer computational method can be more accurate in higher I solutions; however, Pitzer parameters for Pd were not completely known at the present. SIT is known to be inaccurate at I > 4.0 M and, therefore, sorption was modelled at I ≤ 4.0 M in this study [18].

The Japan Atomic Energy Agency (JAEA) thermodynamic database (TDB) was chosen as the reference database since it contains the necessary thermodynamic data for Pd [19]. However, no thermodynamic data for PdOH⁺ and are available in JAEA TDB, so the values contained in the SIT database (v9a) included in the PHREEQC [20] were added to the JAEA TDB. The hydrolysis and complexation constants used in this work are summarized in Table 1.

The specific surface area and the cation exchange capacity of MX-80 were 26.2 m²/g [21] and 102.1 meq/100g [22], respectively. However, the sorption site capacity was not measured. Hence, we assumed that the sorption site capacity is proportional to the specific surface area [14]. As shown in Supplementary Materials, the contribution of cation exchange reaction to the sorption of Pd on MX-80 was negligibly small. Therefore, the slight difference in the value of the cation exchange capacity did not affect the calculation results. Since the concentration of Pd in the solution was much smaller than the total sorption site number in the MX-80 used, the slight difference in the value of the specific surface area also did not influence the calculation results.

In the 2SPNE SC/CE model, Bradbury and Baeyens considered both strong and weak surface sites [9, 10]. In our previous work [8], we could simulate the Pd sorption on MX-80 in Na-Ca-Cl solution by considering the strong site only and estimate the optimized surface complexation and cation exchange constants at I = 0 M, as shown in Table 2.

For the Pd sorption in Na-Ca-ClO₄ solutions, the 2SPNE SC/CE model calculation was conducted using the binary surface complexation and cation exchange constants illustrated in Table 2.

For the Pd sorption in Na-Ca-Cl-ClO₄ solutions, we included the additional three ternary surface complexations (≡S-OH + Pd²⁺ + xCl^-↔ ≡S- + H⁺; x = 1 – 3) in the modelling. Bradbury and Baeyens proposed the linear free energy relationships (LFER) between the surface complexation constants for montmorillonite and the hydrolysis constants [9]. In the fitting of the 2SPNE SC/CE model to the values experimentally derived, we set the initial values for additional ternary surface complexation constants, by assuming that the proposed LFER equation for montmorillonite can be used for the surface complexation constants and the complexation constants (x = 1 – 3). The initial value of ternary surface complexation constant for ≡S-OH + Pd²⁺ + 4Cl^-↔ ≡S- + H⁺ was set as 13.05. In the fitting, the values of four ternary sorption reaction constants were used as the fitting parameters to obtain the best optimized fitting, and other values were fixed.

3. Results and Discussion

3.1. Sorption in Na-Ca-ClO₄ Solution

The and I dependence of values for MX-80 is plotted in Figure 1. It was found that the values decreased with (3–7) and then became constant against (7–10). Little dependence of values on I was also observed. These tendencies are consistent with the previous study by Tachi et al. [7].

The 2SPNE SC/CE model with the binary surface complexation and cation exchange constants previously estimated in the Na-Ca-Cl solutions [8] was applied to the and I dependence of values in the Na-Ca-ClO₄ solutions. The model calculation results are also illustrated in Figure 1. We could find the consistency between the experimental and calculation results.

In the pH region of 3 – 10, Pd(OH)₂ is a dominant species in the solution (Pd speciation in Na-Ca-ClO₄ solution at I = 4 M is shown in Figure S-1. Pd speciation at I < 4 M is not shown here). As shown in Figure S-8, the binary surface complexations ≡S-OH + Pd²⁺↔ ≡S-OPd⁺ + H⁺, ≡S-OH + Pd²⁺ + H₂O ↔ ≡S-OPdOH + 2H⁺, and ≡S-OH + Pd²⁺ + 2H₂O ↔ ≡S- + 3H⁺ dominate the sorption at pH = 3–6, 6–8, and 8–10, respectively. This indicates that Pd sorbs on MX-80 markedly in the acidic pH region through the ≡S-OH + Pd²⁺↔ ≡S-OPd⁺ + H⁺ surface complexation in the absence of Cl^-. From Figure S-8, the contribution of cation exchange reaction was also found to be negligibly small. These demonstrate that the binary surface complexation constants we previously estimated [8] can be used to simulate the sorption of Pd on MX-80 in the Na-Ca-ClO₄ solutions quantitatively.

3.2. Sorption in Na-Ca-Cl-ClO₄ Solutions

Figure 2 illustrates the and Cl^-/ ratio dependence of values for MX-80. We found that the values at < 7 decreased as the Cl^-/ ratio increased. Particularly, the values at < 6 for MX-80 were drastically suppressed in the presence of Cl^- even at Cl^-/ ratio = 0.01, compared to the values in the absence of Cl^- (Figure 1). On the other hand, the values at = 7 – 9 slightly increased with Cl^-/ ratio up to 1 and did not change any more at Cl^-/ ratio ≥ 10.

The Pd speciation in Na-Ca-Cl-ClO₄ solutions at I = 4 M at Cl^-/ ratio = 0.01, 0.1, 1, 10, 100 and infinity are shown in Figures S-2–S-7, respectively. It was found that the pH region of dominance expanded with Cl^-/ ratio, while that of Pd(OH)₂ dominance shrank. Figure 2 suggests that the formation of complex strongly suppressed the Pd sorption, especially the surface complexation ≡S-OH + Pd²⁺↔ ≡S-OPd⁺ + H⁺, on MX-80 at < 7.

The fitting results of the 2SPNE SC/CE model to the experimentally measured values using three binary and four ternary surface complexations and cation exchange reaction are also drawn in Figure 2. It was shown that the dependence of values in the wide range of Cl^-/ ratio could be also quantitatively fitted by the 2SPNE SC/CE model. It was found that the fitting results could be obtained only with three binary and one ternary surface complexations as we studied in Na-Ca-Cl solutions [8]. Namely, only the ternary surface complexation, ≡S-OH + Pd²⁺ + 4Cl^-↔ ≡S- + H⁺, among the four complexations considered in the modelling contributed to the Pd sorption on MX-80 in Na-Ca-Cl-ClO₄ solutions. The contribution of other three ternary surface complexations was negligible. The surface complexation constant for this ternary sorption reaction was estimated as 13.3 ± 0.3. This value is consistent with 13.05 ± 0.2 which was previously estimated [8].

The pH dependence of surface complexation and cation exchange reaction at Cl^-/ ratio = 0, 0.01, 0.1, 1, 10, 100 and infinity is shown in Figures S-8–S-14, respectively. Three binary surface complexations dominated the sorption at Cl^-/ ratio = 0. In the presence of Cl^-, the surface complexation, ≡S-OH + Pd²⁺↔ ≡S-OPd⁺ + H⁺, was drastically suppressed even at Cl^-/ ratio = 0.01. As the Cl^-/ ratio increased, the contribution of surface complexations, ≡S-OH + Pd²⁺↔ ≡S-OPd⁺ + H⁺ and ≡S-OH + Pd²⁺ + H₂O ↔ ≡S-OPdOH + 2H⁺, became small and was finally zero. This led to the decrease in the measured values at < 7. On the other hand, the contribution of ternary surface complexation, ≡S-OH + Pd²⁺ + 4Cl^-↔ ≡S- + H⁺, became large at Cl^-/ ratio = 0.1 and was significant and dominated the sorption at Cl^-/ ratio ≥ 1. The increase in the measured values at 7–9 was attributed to this ternary surface complexation.

The complexation constant for Pd²⁺ + 3Cl^- + H₂O - H⁺↔ PdCl₃OH^2- is compiled in the JAEA TDB (Table 1). Although PdCl₃OH^2- did not appear in Na-Ca-Cl-ClO₄ solutions at I = 4 M (Figures S-1–S-7), the 2SPNE SC/CE model including the ternary surface complexation ≡S-OH + Pd²⁺ + 3Cl^- + H₂O ↔ ≡S-OPdCl₃OH^3- + 2H⁺ was also applied to the measured values to make sure of the contribution of ternary surface complexation in the Pd sorption on MX-80. However, it was found that this ternary surface complexation could be negligible.

4. Conclusions

The values of Pd for MX-80 were systematically measured as a function of , I, and Cl^-/ molar concentration ratio in Na-Ca-ClO₄ (3 ≤ ≤ 9 and 0.1 M ≤ I ≤ 4M) and Na-Ca-Cl-ClO₄ (3 ≤ ≤ 9 and 0 ≤ Cl^-/ ratio ≤ ∞; I = 4 M) solutions.

It was found that the , I, and Cl^-/ ratio dependence of values was quantitatively fitted by the 2SPNE SC/CE model. The model calculation indicated that, in the presence of Cl^-, the contributions of binary surface complexations were suppressed while that of the ternary surface complexation dominated the sorption as the Cl^-/ ratio increased.

It was also found that the dependence of values for MX-80 in the Na-Ca-Cl-ClO₄ solutions at I = 4 M could be simulated by considering only one ternary surface complexation reaction (≡S-OH + Pd²⁺ + 4Cl^-↔ ≡S- + H⁺) besides the binary surface complexation reactions in all range of Cl^-/ ratio (0–∞).

Data Availability

The sorption data used to support the findings of this study are available from the corresponding author upon request.

Conflicts of Interest

The authors declare that there are no conflicts of interest regarding the publication of this paper.

Acknowledgments

The authors would like to show their gratitude to Dr. Takumi Saito (the University of Tokyo), Drs. Tetsuji Yamaguchi, Yoshihisa Iida, Yukio Tachi, and Akira Kitamura (Japan Atomic Energy Agency), Dr. Tammy Yang (Nuclear Waste Management Organization of Canada), and Dr. Peter Vilks (Canadian Nuclear Laboratories) for their fruitful and valuable comments throughout this work and would like to thank Dr. Naoki Sugiyama and Mr. Wijdan Malik of Agilent Technologies for helpful discussion on the Pd measurement and improvement of detection limit of Pd by ICP-MS. This research was supported by NSERC Discovery Grant (RGPIN-2014-05732).

Supplementary Materials

Figure S-1: Pd speciation in Na-Ca-Cl-ClO₄ solution (Cl^-/ molar concentration ratio = 0) at I = 4 M. Figure S-2: Pd speciation in Na-Ca-Cl-ClO₄ solution (Cl^-/ molar concentration ratio = 0.01) at I = 4 M. Figure S-3: Pd speciation in Na-Ca-Cl-ClO₄ solution (Cl^-/ molar concentration ratio = 0.1) at I = 4 M. Figure S-4: Pd speciation in Na-Ca-Cl-ClO₄ solution (Cl^-/ molar concentration ratio = 1) at I = 4 M. Figure S-5: Pd speciation in Na-Ca-Cl-ClO₄ solution (Cl^-/ molar concentration ratio = 10) at I = 4 M. Figure S-6: Pd speciation in Na-Ca-Cl-ClO₄ solution (Cl^-/ molar concentration ratio = 100) at I = 4 M. Figure S-7: Pd speciation in Na-Ca-Cl-ClO₄ solution (Cl^-/ molar concentration ratio = ∞) at I = 4 M. Figure S-8: Pd sorption reaction on MX-80 in Na-Ca-Cl-ClO₄ solution (Cl^-/ molar concentration ratio = 0) at I = 4 M. Figure S-9: Pd sorption reaction on MX-80 in Na-Ca-Cl-ClO₄ solution (Cl^-/ molar concentration ratio = 0.01) at I = 4 M. Figure S-10: Pd sorption reaction on MX-80 in Na-Ca-Cl-ClO₄ solution (Cl^-/ molar concentration ratio = 0.1) at I = 4 M. Figure S-11: Pd sorption reaction on MX-80 in Na-Ca-Cl-ClO₄ solution (Cl^-/ molar concentration ratio = 1) at I = 4 M. Figure S-12: Pd sorption reaction on MX-80 in Na-Ca-Cl-ClO₄ solution (Cl^-/ molar concentration ratio = 10) at I = 4 M. Figure S-13: Pd sorption reaction on MX-80 in Na-Ca-Cl-ClO₄ solution (Cl^-/ molar concentration ratio = 100) at I = 4 M. Figure S-14: Pd sorption reaction on MX-80 in Na-Ca-Cl-ClO₄ solution (Cl^-/ molar concentration ratio = ∞) at I = 4 M. (Supplementary Materials)

References

M. Y. Hobbs, S. K. Frape, O. Shouakar-Stash, and L. R. Kennel, “Regional hydrogeochemistry – Southern Ontario,” NWMO DGR-TR-2011-12, Nuclear Waste Management Organization, 2011.
View at: Google Scholar
P. Vilks, “Sorption of selected radionuclides on sedimentary rocks in saline conditions - Literature review,” NWMO TR-2011-12, Nuclear Waste Management Organization, 2011.
View at: Google Scholar
H. Geckeis, J. Lützenkirchen, R. Polly, T. Rabung, and M. Schmidt, “Mineral–water interface reactions of actinides,” Chemical Reviews, vol. 113, no. 2, pp. 1016–1062, 2012.
View at: Publisher Site | Google Scholar
M. Zavarin, B. A. Powell, M. Bourbin, P. Zhao, and A. B. Kersting, “Np(V) and Pu(V) ion exchange and surface-mediated reduction mechanisms on montmorillonite,” Environmental Science & Technology, vol. 46, no. 5, pp. 2692–2698, 2012.
View at: Publisher Site | Google Scholar
N. Chapman, M. Apted, W. Aspinall et al., “TOPAZ Project long-term tectonic hazard to geological repositories,” NUMO-TR-12-05, Nuclear Waste Management Organization of Japan, 2012.
View at: Google Scholar
National Academy of Science, A Study of The Isolation for Geologic Disposal of Radioactive Wastes, Waste Isolation Systems Panels, Board on Radioactive Waste Management, Washington DC, USA, 1983.
Y. Tachi, T. Shibutani, H. Sato, and M. Shibata, “Sorption and diffusion behavior of palladium in bentonite, granodiorite and tuff,” JNC TN8400 99-088, Japan Nuclear Fuel Cycle Development Institute, 1999.
View at: Google Scholar
J. Goguen, A. Walker, J. Riddoch, and S. Nagasaki, “Sorption of Pd on illite, MX-80 and shale in Na-Ca-Cl solutions,” Nuclear Engineering and Technology (submitted) .
View at: Google Scholar
M. H. Bradbury and B. Baeyens, “Modelling the sorption of Mn(II), Co(II), Ni(II), Zn(II), Cd(II), Eu(III), Am(III), Sn(IV), Th(IV), Np(V) and U(VI) on montmorillonite: Linear free energy relationships and estimates of surface binding constants for some selected heavy metals and actinides,” Geochimica et Cosmochimica Acta, vol. 69, no. 4, pp. 875–892, 2005.
View at: Publisher Site | Google Scholar
M. Bradbury and B. Baeyens, “Sorption modelling on illite. Part II: Actinide sorption and linear free energy relationships,” Geochimica et Cosmochimica Acta, vol. 73, no. 4, pp. 1004–1013, 2009.
View at: Publisher Site | Google Scholar
T. Fanghänel, V. Neck, and J. I. Kim, “The ion product of H2O, dissociation constants of H2CO3 and Pitzer parameters in the system Na+/H+/OH-/HCO-3/CO 2-3/ClO-4/H2O at 25°C,” Journal of Solution Chemistry, vol. 25, no. 4, pp. 327–343, 1996.
View at: Publisher Site | Google Scholar
M. Altmaier, V. Metz, V. Neck, R. Müller, and T. Fanghänel, “Solid-liquid equilibria of Mg(OH)2(cr) and Mg2(OH) 3Cl·4H2O(cr) in the system Mg-Na-H-OH-Cl- H2O at 25°C,” Geochimica et Cosmochimica Acta, vol. 67, no. 19, pp. 3595–3601, 2003.
View at: Publisher Site | Google Scholar
M. Altmaier, V. Neck, and T. Fanghänel, “Solubility of Zr(IV), Th(IV) and Pu(IV) hydrous oxides in CaCl2 solutions and the formation of ternary Ca-M(IV)-OH complexes,” Radiochimica Acta, vol. 96, no. 9-11, pp. 541–550, 2008.
View at: Publisher Site | Google Scholar
S. Nagasaki, “Sorption properties of Np on shale, illite and bentonite under saline, oxidizing and reducing conditions,” NWMO-TR-2018-02, Nuclear Waste Management Organization, 2018.
View at: Google Scholar
S. Nagasaki, T. Saito, and T. T. Yang, “Sorption behavior of Np(V) on illite, shale and MX-80 in high ionic strength solutions,” Journal of Radioanalytical and Nuclear Chemistry, vol. 308, no. 1, pp. 143–153, 2016.
View at: Publisher Site | Google Scholar
S. Nagasaki, J. Riddoch, T. Saito, J. Goguen, A. Walker, and T. T. Yang, “Sorption behaviour of Np(IV) on illite, shale and MX-80 in high ionic strength solutions,” Journal of Radioanalytical and Nuclear Chemistry, vol. 313, pp. 1–11, 2017.
View at: Google Scholar
D. L. Parkhurst and C. A. J. Appelo, “User's Guide to PHREEQC (Version 2) (Equations on which the program is based,” Water-Resources Investigations Report 99-4259, U.S. Department of the Interior, U.S. Geological Survey, 1999.
View at: Google Scholar
I. Grenthe and A. Plyasunov, “On the use of semiempirical electrolyte theories for the modeling of solution chemical data,” Pure and Applied Chemistry, vol. 69, no. 5, pp. 951–958, 1997.
View at: Publisher Site | Google Scholar
Thermodynamic Database, Japan Atomic Energy Agency, TDB Ver. 2014/03, June 2014, https://migrationdb.jaea.go.jp/cgi-bin/db_menu.cgi?title=TDB&ej=1.
PHREEQC (Version 3) – A computer program for speciation, batch-reaction, one-dimensional transport, and inverse geochemical calculations, United States Geological Survey, 2017, https://wwwbrr.cr.usgs.gov/projects/GWC_coupled/phreeqc/.
F. P. Bertetti, “Determination of sorption properties for sedimentary rocks under saline, reducing conditions – Key radionuclides,” NWMO-TR-2016-08, Nuclear Waste Management Organization, 2016.
View at: Google Scholar
E. Galunin, M. D. Alba, M. J. Santos, T. Abrão, and M. Vidal, “Lanthanide sorption on smectitic clays in presence of cement leachates,” Geochimica et Cosmochimica Acta, vol. 74, no. 3, pp. 862–875, 2010.
View at: Publisher Site | Google Scholar

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Copyright © 2019 Shinya Nagasaki et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

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Science and Technology of Nuclear Installations

Advanced Technologies in Nuclear Waste Management Process Design and Materials

Contribution of Ternary Reaction to Pd Sorption on MX-80 in Na-Ca-Cl Solution at High Ionic Strength

Abstract

1. Introduction

2. Materials and Methods

2.1. Chemicals, Solids, and Solutions

2.2. Sorption Experiments

2.3. Sorption Modelling

3. Results and Discussion

3.1. Sorption in Na-Ca-ClO4 Solution

3.2. Sorption in Na-Ca-Cl-ClO4 Solutions

4. Conclusions

Data Availability

Conflicts of Interest

Acknowledgments

Supplementary Materials

References

Copyright

3.1. Sorption in Na-Ca-ClO₄ Solution

3.2. Sorption in Na-Ca-Cl-ClO₄ Solutions