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ISSN : 1738-1894(Print)
ISSN : 2288-5471(Online)
Journal of Nuclear Fuel Cycle and Waste Technology Vol.19 No.1 pp.39-49
DOI : https://doi.org/10.7733/jnfcwt.2021.19.1.39

Behaviors of Desorption Agents During Removal of Cs From Clay Minerals and Actual Soil

Chan Woo Park*, Ilgook Kim, In-Ho Yoon, Hee-Man Yang, Bum-Kyung Seo
Korea Atomic Energy Research Institute, 111, Daedeok-daero 989beon-gil, Yuseong-gu, Daejeon, Republic of Korea
* Corresponding Author. Chan Woo Park, Korea Atomic Energy Research Institute, E-mail: chanwoo@kaeri.re.kr, Tel: +82-42-866-6160

October 25, 2020 ; December 11, 2020 ; December 19, 2020

Abstract


The behaviors of various desorption agents were investigated during the desorption of cesium (Cs) from samples of clay minerals and actual soil. Results showed that polymeric cation exchange agents (polyethyleneimine (PEI)) efficiently desorbed Cs from expandable montmorillonite, whereas acidic desorption solutions containing HCl or PEI removed considerable Cs from hydrobiotite. However, most desorption agents could desorb only 54% of Cs from illite because of Cs’s specific adsorption to selective adsorption sites. Cs desorption from an actual soil sample containing Cs-selective clay mineral illite (< 200 μm) and extracted from near South Korea’s Kori Nuclear Power Plant was also investigated. Considerable adsorbed 137Cs was expected to be located at Cs-selective sites when the 137Cs loading was much lower than the sample’s cation exchange capacity. At this low 137Cs loading, the total Cs amount desorbed by repeated washing varied by desorption agent in the order HCl > PEI > NH4+, and the highest Cs desorption amount achieved using HCl was 83%. Unlike other desorption agents with only cation exchange capabilities, HCl can attack minerals and induce dissolution of metallic elements. HCl’s ability to both alter minerals and induce H+/Cs+ ion exchange is expected to promote Cs desorption from actual soil samples.



초록


    National Research Foundation of Korea(NRF)
    2017M2A8A5015148

    1. Introduction

    Inadvertent and accidental release of radiocesium from nuclear facilities into the environment produces problematic Cs-contaminated soil wastes [1, 2]. Among various soil components, the 2:1 clay minerals strongly and specifically bind radiocesium [3, 4], and thus remediation of Cs-contaminated soil generally faces technical challenges.

    A variety of clay minerals (including such as kaolinite, illite, smectite, and vermiculite), can be present in soil depending on parent minerals and weathering conditions. Each type of clay mineral has distinguishable mineralogical characteristics including expansion properties and cation exchange capacity (CEC), among many others [5]. Consequently, individual clay minerals display different Cs adsorption and desorption behaviors [3, 6, 7]. For example, Cs adsorption on kaolinite (1:1 clay mineral) mainly takes place on the external surface of a particle through formation of an outer-sphere complex. Moreover, the Cs adsorbed to kaolinite is readily exchangeable [8, 9].

    On the other hand, 2:1 clay minerals contain additional Cs adsorption sites, such as hydrated or dehydrated interlayer sites, as well as frayed edge sites (FES), in addition to the external planar sites [7]. In particular, FES can be formed as a result of weathering at the edges of potassiumbearing micaceous clay minerals. It has been experimentally and theoretically proven that the highly Cs-selective FES can adsorb Cs in stable form [10-13], and that the bound Cs is stabilized by consequent shrinkage of the weathered interlayers [14-16]. For this reason, the adsorbed Cs ions on non-expandable illite, and on micas containing FES, are hardly removable [17, 18]. On the other hand, highly expandable montmorillonite has Cs adsorption sites in negatively charged interlayers. Moreover, it was reported that a small fraction of Cs could be adsorbed via strong inner-sphere complexations on the mineral when the Cs loading was low [19, 20]. Meanwhile, partially expandable vermiculite interlayers sometimes undergo dehydration and shrinkage after Cs adsorption, and the desorption of such stabilized Cs has been reported to be inefficient [5].

    Various attempts have been made to desorb Cs from clay minerals using organic and inorganic cations based on ion-exchange reactions between cations and Cs [21]. Even though the excess Mg2+ ions could extract significant (~90%) amounts of Cs from vermiculite, Cs removal by ammonium or metal ions from montmorillonite and illite were relatively inefficient (50–60%) [22, 23]. It was also reported that the highest achievable Cs desorption from illite by NH4+ (1 M) was only 54%, even after 8 weeks of reaction [18]. In contrast, cationic surfactant and polymers have been reported to be efficient Cs desorption agents for fully and partially expandable clay minerals such as montmorillonite (~95%, 137Cs) and hydrobiotite (~87%, 133Cs). The expansion of interlayers induced by polymer or surfactant intercalation in the interlayers enhanced ion-exchange reactions between cations and Cs [16, 20, 24, 25]. Meanwhile, a hydrogen peroxide solution promoted expansion of the interlayers of hydrobiotite, which is a mixed-layer clay mineral of expandable vermiculite and non-expandable mica. Moreover, hydrogen peroxide also potentiated the ion-exchange capability when a complementary cation exchange agent (Mg2+) was added with the Cs [26].

    Organic and inorganic acids have also been investigated as Cs desorption agents. The acids are capable of dissolving mineral components and elements, and thus desorption of Cs can be enhanced with the help of the H+/Cs+ exchange reaction [27-30]. Even though various acids have shown promising Cs-desorption performance against single clay minerals, the reported Cs-desorption efficiency of oxalate from the actual soil was less than 63%, even after the 68- day treatment [31].

    Although various Cs-desorption agents have been investigated for use against single clay minerals, comparisons of the effectiveness of Cs-desorption agents against different kinds of clay minerals are also important subjects to investigate. Moreover, the trend of Cs desorption from actual soil samples is frequently different from that involving single clay minerals. For this reason, the Cs desorption properties of the agents must be evaluated by considering the mineral components in the actual soil.

    In the work reported in this paper, we investigated the behavior of various desorption agents (including polymeric cation exchange agents, single molecular cations, and acid) for desorption of Cs from clay minerals and actual soil samples. The clay minerals investigated included expandable montmorillonite, non-expandable illite, and mixed-layer clay of expandable vermiculite and non-expandable biotite (hydrobiotite). To investigate the behavior of Cs-desorption from actual soil samples containing various soil constituents, soil samples were collected from near the Kori Nuclear Power Plant (NPP). In addition, the correlations between the mineral components and Cs-desorption behaviors were investigated.

    2. Experimental

    2.1 Materials

    Montmorillonite (MT, SAz-1 from The Clay Minerals Society, USA) and illite (IL, 2,500 mesh, Youngkoong Illite Co., Ltd.) were used as received. A hydrobiotite (HB, < 38 μm) sample was prepared by sequential treatment of vermiculite (Sigam-Aldrich) by mechanical milling (M 20 universal mill, IKA) and mechanical sieving using a standard test sieve (400 mesh) [16].

    Cesium chloride, tetramethyl ammonium chloride (TMA), hydrochloric acid, poly(diallyldimethylammonium chloride) (PDDA, Mw < 100 kDa), hydrochloric acid, ammonium nitrate, and poly(ethyleneimine) with Mw = ~2 kDa (PEI2k) and ~25 kDa (PEI25k), were purchased from Sigma-Aldrich and used as received.

    2.2 Sampling and fractionation of soil

    The soil samples were taken at depths of 0 to 15 cm from the soil surface within 2 km of the Kori NPP (35° 20′ 33″ N, 129° 17′ 33″ E). The soil fraction under 200 μm (SF200) was obtained by dry-sieving the soil using a vibratory sieve shaker (Retsch AS 200) with a standard sieve (Retsch, ISO 3310/1). The soil weight fraction < 200 μm was 36.5%.

    2.3 Characterization of clay minerals and soil samples

    The compositions of the clay minerals and SF200 were determined by X-ray diffraction (XRD) analysis using a Rigaku SmartLab diffractometer (Japan). The elemental contents in the samples were determined by energy dispersive X-ray fluorescence (XRF) spectrometry analysis using an S2 RANGER (Bruker). For the XRF analysis, a doublelayer pellet (sample and boric acid) was prepared by pressing the clay or soil (200 mg) on an as-prepared boric acid pellet (6 g) using a hydraulic press at 20 t [20]. The cation exchange capacity (CEC) of clay minerals and soil samples were determined by following the SW-846 Test Method 9081 (U.S. Environmental Protection Agency).

    2.4 Preparation of Cs-adsorbed clay minerals and soil samples

    A portion (35 g) of each sample (MT, IL, HB, and SF200) was mixed with 3 mM CsCl solution in deionized water (350 mL). Then, the Cs adsorption was allowed to reach equilibration by shaking the mixture for 7 days at 25°C in a shaking incubator. The Cs-adsorbed clay minerals and SF200 sample were collected by centrifugation, followed by washing with deionized water. To estimate the amounts of adsorbed Cs on the clay minerals and SF200, unbound Cs in the liquid was quantified using inductively coupled plasma mass spectroscopy (ICP-MS, ELAN DRC II, PerkinElmer, USA). The aqueous phase was filtered using a polyvinylidene fluoride (PVDF) syringe filter (pore size = 0.2 μm) prior to the measurements. The Cs-adsorbed MT, IL, HB, and SF200 samples were denoted as Cs-MT, Cs-IL, Cs-HB, and Cs-SF200, respectively.

    2.5 Desorption of Cs from clay minerals and soil samples

    The Cs-adsorbed clay minerals and SF200 (300 mg) were each mixed with (30 mL) solutions containing various desorption agents (PEI2k, PEI25k, TMA, PDDA, HCl, or NH4+), and the concentration of desorption agent was 20 mmol per gram of clay minerals or SF200. In the cases of the PEI2k, PEI25k, and NH4+ solutions, the solution pH was adjusted to pH 3 using 1 M HCl solution [32]. The mixture was placed in a horizontal shaker for 1 day at 20°C or 80°C. The clay minerals and soil samples were removed by centrifugation, and supernatants were filtered with an Amicon Ultra centrifugal filter (Millipore, molecular weight cut-off (MWCO) = 10 kDa). The total amount of desorbed Cs in the supernatant was quantified by ICP-MS.

    2.6 Adsorption and desorption of radiocesium

    The SF200 (35 g) was added to a 137Cs solution (68.8 Bq·mL−1, 175 mL) and the resulting mixture was shaken at 25°C for 7 days. The 137Cs-adsorbed SF200 (137Cs-SF200) was separated from aqueous phase by centrifugation for 1 hr. The 137Cs-SF200 was air-dried at room temperature, and the aqueous phase was filtered using a PVDF syringe filter (pore size = 0.2 μm). The radioactivity of the filtrate (C, Bq·mL−1) and the dried 137Cs-SF200 (q, Bq·mL−1) were measured using a high-purity germanium detector (HPGe) equipped with a multi-channel analyzer (MCA, CANBERRA Ind.). The minimum detectable activity was maintained below 0.02 Bq·g−1. The radiocesium distribution coefficient (Kd) of the SF200 was calculated using.

    K d = q / C
    (1)

    The desorption of radiocesium from the 137Cs-SF200 (300 mg) was carried out by following the experimental method described above. Solutions (30 mL) containing 20 mmol·g−1 soil were mixed with desorption agents (PEI2k, PEI25k, TMA, PDDA, HCl, or NH4+) at 20°C for 1 day. For repeated radiocesium desorption experiments, the 137Cs- SF200 (300 mg) was reacted with solutions (30 mL) containing 20 or 50 mmol·g−1 soil of PEI2k, HCl, or NH4+ at 20°C for 1 day. Then, the aqueous phase was replaced with a fresh solution containing the desorption agent every 24 hr, after separating the solids by centrifugation. The radioactivity of the liquid phase was determined using a HPGe equipped with a MCA. This was done after filtration using an Amicon Ultra centrifugal filter (MWCO = 10 kDa).

    3. Results and discussion

    3.1 Characterization of clay minerals and soil samples

    XRD analysis of the clay minerals and SF200 was carried out to identify minerals present in the samples (Fig. 1). Each clay mineral sample showed its own typical XRD pattern [5], and characteristic peaks of montmorillonite and illite were observed at 2θ = ~6.1° and ~8.8°, respectively. The HB sample showed an XRD pattern of a mixed-layer clay mineral containing expandable vermiculite and nonexpandable mica. The peak characteristic of hydrobiotite was observed at 2θ = 7.4°, and peaks of mica and vermiculite were also observed at 2θ = 8.8° and 6.1° [16]. From the XRD pattern of the SF200, illite and kaolinite peaks were found at 2θ = ~8.8° and ~12°, respectively, and strong peaks characteristics of quartz were also observed at 2θ = ~21.2° and ~26.3° [33, 34]. Finally, it was determined that the SF200 contains quartz as well as clay minerals that included illite and kaolinite.

    For analysis of the elemental contents in the samples, XRF measurements of the clay minerals and the SF200 were carried out (Table 1). As expected, the element contained in nearly all the samples was Si because it is a major component of phyllosilicate clay minerals and quartz. The mineral montmorillonite (SAz-1), which contains Ca as an exchangeable interlayer cation, showed high Ca content (CaO = 6.8%). Similarly, the IL sample showed high K content (K2O = 5.9%) because its interlayer cation is K. In the case of HB, which is composed of mixed layers of vermiculite and biotite, both Mg and K were abundant in the sample because they are interlayer cations of vermiculite and biotite, respectively. Because trioctahedral layers of biotite is composed of Mg and Fe, the HB sample also showed high Fe content. The SF200 sample contained relatively high amounts of K compared to other available interlayer cations, such as Na or Ca. This supports the presence of micaceous clay minerals, such as illite, in the SF200 sample.

    3.2 Desorption of Cs from clay minerals and soil sample

    The Cs-adsorbed clay minerals and the soil sample were prepared by reacting the samples with 133CsCl solutions for 7 days, and the initial Cs/solid ratio was 30 μmol·g−1 (Table 2). Because each clay mineral and soil sample has a different CEC value, the fraction of adsorbed Cs to total CEC varied from 2.2% (Cs-MT) to 11.5% (Cs-IL). In the case of Cs-SF200, the adsorbed amount of Cs was 26.5 μmol·g−1 of Cs, equivalent to 9.3% of CEC.

    The efficiency of Cs desorption from clay minerals and soil samples by various desorption agents was analyzed. Polymeric cations (PEI2k, PEI25k, and PDDA), single molecular cations (TMA and NH4+), and strong acid (HCl) were tested as desorption agents. The PDDA and TMA contain permanently charged quaternary ammonium cations. In contrast, PEI and ammonium nitrate can have different protonation states depending on the pH of solutions [16, 32]; thus, the pH of those solutions were maintained at pH 3. Even though both TMA and NH4+ are single molecular cations, TMA has a slightly bulkier structure compared to NH4+ because of the four methyl groups in TMA. Unlike the other desorption agents, which have only ion-exchange ability, HCl is not only able to decompose mineral structures and to dissolve metallic elements from clay minerals but also can induce ion-exchange with Cs [28, 35, 36]. The added amount of desorption agents was 20 mmol·g−1 based on the cations contained in the desorption agents. This amount is at least ~7 times higher than the amount of Cs adsorbed on the clay minerals and soil samples.

    Fig. 2(a) shows the amount of Cs desorbed from the Cs-MT. The large molecular polymeric cations (such as PEI and PDDA) showed higher Cs desorption efficiency compared to smaller molecular cations such as TMA, H+, or NH4+. The amount of Cs desorbed by PEI25k solution at pH 3 was 84.7 ± 5.5% while that achieved by NH4+ solution at pH 3 was only 34.7 ± 3.5%. It was reported that the cationic polymers can be intercalated into the interlayers of montmorillonite, and that this results in expansion of the interlayers [15]. Once the cation polymer is adsorbed to the interlayers, the locally increased cation concentration enhances desorption of Cs from the montmorillonite [15]. Although both TMA and PDDA contain permanently charged quaternary ammonium ions, the polymeric PDDA showed better Cs desorption than monomolecular TMA did. This indicates the beneficial effect of a polymeric desorption agent for Cs desorption from montmorillonite.

    In the case of Cs-IL, the tested desorption agents showed similar Cs removal efficiencies (less than ~54%, Fig. 2(b)). It is well known that illitic clay minerals possess highly Cs-selective adsorption sites, such as FES and Type II sites [11]. Thus, the Cs ions adsorbed to such adsorption sites are hardly exchangeable with cations [17, 18]. The content of the most Cs-selective Type I sites (FES) and the second highest Cs-selective Type II sites in illite are generally less than 0.25% and 20% of the CEC, respectively [11]. Based on our experimental results, it is expected that the adsorption sites that correspond to ~5.3% of the CEC can strongly bind Cs ions, and such Cs ions are not readily exchangeable with any desorption agents.

    In the case of Cs-HB, the amount of Cs desorbed by both HCl and PEI2k (pH 3) solutions was ~73% (Fig. 2(c)). Moreover, the acidic solution containing PEI25k and NH4+ at pH 3 also showed higher Cs removal efficiency than did quaternary ammonium ions dissolved in deionized water (PDDA = 23%). Similar to these results, it was previously reported that Cs desorption from hydrobiotite by PEI or NH4+ increased as the solution pH was decreased, and only pH adjustment of the hydrobiotite dispersion to pH 3 could induce ~30% of Cs desorption [16]. In this regard, it is predicted that acidic solutions could potentiate desorption of Cs from hydrobiotite.

    Finally, the Cs removal capabilities of the desorption agents against Cs-SF200 were observed. At 20°C, the average Cs desorption efficiency of NH4+ and HCl was 73% and 70%, respectively, and these desorption agents showed slightly higher Cs desorption efficiencies than the other desorption agents did (50–60%). The amount of desorbed Cs at higher temperature (80°C) was similar to that obtained at 20°C. However, the Cs desorption efficiency of HCl was increased by ~9% after raising the temperature from 20°C to 80°C, and the highest Cs desorption from Cs-SF200 (79%) was achieved using HCl solution at 80°C. Unlike clay mineral samples, the actual soil fraction sample (Cs-SF200) contained various soil components such as primary minerals, clay minerals, and soil organic materials. More specifically, SF200 contained quartz, illite, and kaolinite. The content of Cs-selective FES sites in illite is generally less than 0.25% of the CEC [11, 37, 38], and the illite content in the SF200 sample was also expected to be low. Because the amount of Cs adsorbed on Cs-SF200 was 9.3% of the CEC (Table 2), it was predicted that most of the adsorbed Cs ions would be present at non-selective adsorption sites.

    3.3 Desorption of 137Cs from the soil samples

    The adsorption of 137Cs on the actual soil sample (SF200) was analyzed. After equilibration of the adsorption reaction, the measured radioactivity of 137Cs-SF200 was 343.45 Bq·g−1, and the calculated Cs distribution coefficient (Kd) of SF200 was 4347 mL·g−1. This adsorbed amount of 137Cs was equivalent to 0.78 pmol·g−1, and only 2.8 × 10−7% of CEC was occupied by the adsorbed 137Cs. In low-concentration 137Cs solutions, Cs ions tend to be sequestered by Cs-selective adsorption sites among the various adsorption sites in soil [6]. For this reason, it is expected that many of the 137Cs ions were bound to the Cs-selective sites, unlike in the previous experimental condition that the amount of the adsorbed Cs exceeded the quantity of expected Csselective sites in soil.

    Fig. 3 shows the amount of 137Cs desorbed from 137Cs- SF200 by various desorption agents at 20°C. Similar to the previously described experimental result (non-radioactive Cs desorption), NH4+ could desorb a large amount of 137Cs (~27%) from 137Cs-SF200 at pH 3. The PEI2k (~18%), PEI25k (~14%), and HCl (13%) also could desorb significant amounts of 137Cs from the soil. In contrast, the desorption agents containing quaternary ammonium ions were not efficient at desorbing stably bound 137Cs from the soil samples. Furthermore, none of the 137Cs could be desorbed from the soil when 137Cs-SF200 was reacted with deionized water.

    Because PEI2k, HCl, and NH4+ showed promising results for the desorption of 137Cs from the soil sample, the cumulative amounts of desorbed 137Cs were measured after repeated treatment of the soil samples with desorption agents by replacing the solution every 24 hr (Fig. 4). The amount of desorption agent relative to the amount of soil was 20 mmol·g−1 or 50 mmol·g−1. In the case of the NH4+ at pH 3, most exchangeable 137Cs ions were desorbed during the first washing step, and a very small amount of 137Cs was additionally desorbed during the second and third washing steps. Furthermore, the total amount of 137Cs desorbed by two different concentrations of NH4+ were almost identical (~32%). In these regards, it is concluded that NH4+ is efficient for removing weakly bound Cs in actual soil in a single washing step, but that additional extraction of stably bound 137Cs is inefficient.

    In contrast, a significant amount of additional 137Cs could be desorbed from the soil by repetitive treatment with HCl solutions. Moreover, higher concentrations of HCl desorbed much larger amounts of 137Cs from 137Cs- SF200. When 137Cs-SF200 was washed three times with HCl solutions at 20 and 50 mmol·g−1 soil, the total amount of desorbed 137Cs was 35% and 83%, respectively. Unlike the other desorption agents, HCl is known to initiate disintegration of clay minerals [28, 35], and it was reported that Al and Fe elements can be partially dissolved from illite and kaolinite by an HCl solution [36]. It is predicted that the additional desorption of 137Cs by repetitive HCl treatment is related to weakening of the structural integrity of the soil components; thus, more comprehensive study will be required.

    In the case of PEI, 40% of 137Cs was desorbed after treatment repeated three times with 50 mmol·g−1 soil. Even though the total desorbed 137Cs from the soil sample by PEI was higher than that achieved by repetitive treatment with NH4+, PEI also showed limited 137Cs desorption because the SF200 sample contained only non-expandable clay minerals of which the interlayers were not accessible using cationic polymers.

    4. Conclusions

    The behaviors of Cs desorption from clay minerals and actual soil samples were investigated using various Csdesorption agents, including polymeric cation exchange agents, single molecular cations, and HCl.

    First, the desorption of Cs from pure clay minerals, including montmorillonite and illite, and mixed-layer clays of hydrobiotite, vermiculite, and biotite were investigated. The polymeric cation exchange agents (such as PEI and PDDA) could efficiently remove Cs from expandable montmorillonite. The acidic desorption solutions containing HCl or PEI could remove a large amount of Cs from hydrobiotite. However, most desorption agents could desorb only ~54% of Cs from illite because of the specific adsorption of Cs to selective adsorption sites.

    The actual soil samples were collected from near a NPP in South Korea and the major minerals in the soil were identified as illite, kaolinite, and quartz. Because a small amount of Cs-selective illite was contained in the soil sample, the total amount of adsorbed 133Cs was larger than the amount at the Cs-selective sites in soil. Thus, desorption of non-selectively bound Cs from the soil seemed to take place mostly during the reaction. Nevertheless, NH4+ and HCl showed high Cs desorption efficiency in the actual soil samples. In contrast, the 137Cs-adsorbed soil sample had extremely low Cs loading compared to the CEC (2.8 × 10−7%), and thus most of the adsorbed 137Cs is expected to be located at Cs-selective sites. The total amount of 137Cs desorbed by repeated washing was related to the desorption agents in the order: HCl > PEI > NH4+, and HCl efficiently removed ~83% of the radiocesium. It is expected that a synergetic effect between the alteration of minerals by acidic attack and the H+/Cs+ ion exchange reaction promoted desorption of 137Cs. In this regard, mineral alteration agents used in cooperation with a cation exchanger offers a promising washing solution for the remediation of radiocesium-contaminated soils.

    Although individual clay minerals exhibited distinguishable behaviors during the desorption of Cs, it was difficult to clearly reveal correlations between the Cs desorption from single clay minerals and that from the example soil samples. Because actual soils display complex behaviors according to their soil compositions and weathering conditions, comprehensive characterizations of actual soil wastes and adsorption/desorption behaviors will be crucial to design successful soil remediation plans.

    Acknowledgment

    This work was supported by a grant from the National Research Foundation of Korea (NRF), funded by the Korean government via the Ministry of Science, ICT, and Future Planning (No. 2017M2A8A5015148).

    Figures

    JNFCWT-19-1-39_F1.gif

    XRD patterns of montmorillonite (MT), illite (IL), and hydrobiotite (HB); and the fraction of an actual soil sample (< 200 μm).

    JNFCWT-19-1-39_F2.gif

    Cs-desorption efficiency of various desorption agents (20 mmol·g−1) against (a) Cs-MT, (b) Cs-IL, (c) Cs-HB, and (d) Cs-SF200 (24 hr reaction).

    JNFCWT-19-1-39_F3.gif

    Amount of radiocesium desorbed from 137Cs-SF200 after reaction with various desorption agents (20 mmol·g−1) at 20°C for 24 hr.

    JNFCWT-19-1-39_F4.gif

    Cumulative amounts of radiocesium desorption by repeated treatment of 137Cs-SF250 with desorption agents (20 or 50 mmol·g−1) at 20°C (reaction time of each step: 24 hr).

    Tables

    Elemental compositions of the clay minerals and the soil sample

    Amount of Cs adsorbed on the clay minerals and SF2001, and percentage of adsorbed Cs ions to CEC of the samples

    References

    1. T. Yamamoto, “Radioactivity of Fission Product and Heavy Nuclides Deposited on Soil in Fukushima Dai- Ichi Nuclear Power Plant accident”, J. Nucl. Sci. Technol., 49(12), 1116-1133 (2012).
    2. D. Ding, Z. Zhang, Z. Lei, Y. Yang, and T. Cai, “Remediation of Radiocesium-Contaminated Liquid Waste, Soil, and Ash: A Mini Review Since the Fukushima Daiichi Nuclear Power Plant accident”, Environ. Sci. Pollut. Res. Int., 23(3), 2249-2263 (2016).
    3. R.M. Cornell, “Adsorption of Cesium on Minerals: A review”, J. Radioanal. Nucl. Chem. Artic., 171(2), 483- 500 (1993).
    4. N.M. Nagy, J. Kónya, and G.Wazelischen-Kun, “The Adsorption and Desorption of Carrier-Free Radioactive Isotopes on Clay Minerals and Hungarian Soils”, Colloids Surfaces A Physicochem. Eng. Asp., 152(3), 245- 250 (1999).
    5. S.M. Park, J. Lee, E.K. Jeon, S. Kang, M.S. Alam, D.C.W. Tsang, D.S. Alessi, and K. Baek, “Adsorption Characteristics of Cesium on the Clay Minerals: Structural Change Under Wetting and Drying Condition”, Geoderma, 340, 49-54 (2019).
    6. H. Mukai, A. Hirose, S. Motai, R. Kikuchi, K. Tanoi, T.M. Nakanishi, T. Yaita, and T. Kogure, “Cesium Adsorption/Desorption Behavior of Clay Minerals Considering Actual Contamination Conditions in Fukushima”, Sci. Rep., 6, 21543 (2016).
    7. S.M. Park, D.S. Alessi, and K. Baek, “Selective Adsorption and Irreversible Fixation Behavior of Cesium onto 2:1 Layered Clay Mineral: A Mini Review”, J. Hazard. Mater., 569-576 (2019).
    8. J.C. Miranda-Trevino and C.A. Coles, “Kaolinite Properties, Structure and Influence of Metal Retention on pH”, Appl. Clay Sci., 23(1-4), 133-139 (2003).
    9. Y. Kim, R.J. Kirkpatrick, and R.T. Cygan, “133Cs NMR Study of Cesium on the Surfaces of Kaolinite and Illite”, Geochim. Cosmochim. Acta, 60(21), 4059-4074 (1996).
    10. C. Poinssot, B. Baeyens, and M.H. Bradbury, “Experimental and Modelling Studies of Caesium Sorption on Illite”, Geochim. Cosmochim. Acta, 63(19), 3217- 3227 (1999).
    11. M.H. Bradbury and B. Baeyens, “A Generalised Sorption Model for the Soncentration Dependent Uptake of Caesium by Argillaceous Rocks”, J. Contam. Hydrol., 42(2), 141-163 (2000).
    12. M. Okumura, H. Nakamura, and M. Machida, “Mechanism of Strong Affinity of Clay Minerals to Radioactive Cesium: First-Principles Calculation Study for Adsorption of Cesium at Frayed Edge Sites in Muscovite”, J. Phys. Soc. Japan, 82(3), 033802 (2013).
    13. H. Mukai, T. Hatta, H. Kitazawa, H. Yamada, T. Yaita, and T. Kogure, “Speciation of Radioactive Soil Particles in the Fukushima Contaminated Area by IP Autoradiography and Microanalyses”, Environ. Sci. Technol., 48(22), 13053-13059 (2014).
    14. K. Tamura, T. Kogure, Y. Watanabe, C. Nagai, and H. Yamada, “Uptake of Cesium and Strontium Ions by Artificially Altered Phlogopite”, Environ. Sci. Technol., 48(10), 5808-5815 (2014).
    15. T. Kogure, K. Morimoto, K. Tamura, H. Sato, and A. Yamagishi, “XRD and HRTEM Evidence for Fixation of Cesium Ions in Vermiculite Clay”, Chem. Lett., 41(4), 380-382 (2012).
    16. B.H. Kim, C.W. Park, H.M. Yang, B.K. Seo, B.S. Lee, K.W. Lee, and S.J. Park, “Comparison of Cs Desorption from Hydrobiotite by Cationic Polyelectrolyte and Cationic Surfactant”, Colloids Surfaces A Physicochem. Eng. Asp., 522, 382-388 (2017).
    17. A.J. Fuller, S. Shaw, M.B. Ward, S.J. Haigh, J.F.W. Mosselmans, C.L. Peacock, S. Stackhouse, A.J. Dent, D. Trivedi, and I.T. Burke, “Caesium Incorporation and Retention in Illite Interlayers”, Appl. Clay Sci., 108, 128-134 (2015).
    18. A. de Koning and R.N.J. Comans, “Reversibility of Radiocaesium Sorption on Illite”, Geochim. Cosmochim. Acta, 68(13), 2815-2823 (2004).
    19. B.C. Bostick, M.A. Vairavamurthy, K.G. Karthikeyan, and J. Chorover, “Cesium Adsorption on Clay minerals: An EXAFS Spectroscopic Investigation”, Environ. Sci. Technol., 36(12), 2670-2676 (2002).
    20. C.W. Park, B.H. Kim, H.M. Yang, B.K. Seo, J.K. Moon, and K.W. Lee, “Removal of Cesium Ions from Clays by Cationic Surfactant Intercalation”, Chemosphere, 168, 1068-1074 (2017).
    21. S.M. Park, J.G. Kim, H.B. Kim, Y.H. Kim, and K. Baek, “Desorption Technologies for Remediation of Cesium-Contaminated Soils: A Short Review”, Environ. Geochem. Health, 1-10 (2020).
    22. L. Dzene, E. Tertre, F. Hubert, and E. Ferrage, “Nature of the Sites Involved in the Process of Cesium Desorption from Vermiculite”, J. Colloid Interface Sci., 455, 254-260 (2015).
    23. K. Tamura, H. Sato, and A. Yamagishi, “Desorption of Cs+ Ions from a Vermiculite by Exchanging with Mg2+ Ions: Effects of Cs+ –Capturing Ligand”, J. Radioanal. Nucl. Chem., 303(3), 2205-2210 (2014).
    24. C.W. Park, B.H. Kim, H.M. Yang, B.K. Seo, and K.W. Lee, “Enhanced Desorption of Cs from Clays by a Polymeric Cation-Exchange Agent”, J. Hazard. Mater., 327, 127-134 (2017).
    25. B.H. Kim, C.W. Park, H.M. Yang, B.K. Seo, S.J. Park, and K.W. Lee, “Effect of Alkyl Length of Cationic Surfactants on Desorption of Cs from Contaminated Clay”, J. Nucl. Fuel Cycle Waste Technol., 15(1), 27- 34 (2017).
    26. I. Kim, J.H. Kim, S.M. Kim, C.W. Park, I.H. Yoon, H.M. Yang, and K.W. Lee, “Desorption of Cesium from Hydrobiotite by Hydrogen Peroxide with Divalent Cations”, J. Hazard. Mater., 390, 121381 (2020).
    27. S.M. Kim, I.H. Yoon, I.G. Kim, C.W. Park, Y.H. Sihn, J.H. Kim, and S.J. Park, “Cs Desorption Behavior During Hydrothermal Treatment of Illite with Oxalic Acid", Environ. Sci. Pollut. Res., 27(28), 35580-35590 (2020).
    28. K. Van Rompaey, E. Van Ranst, F. De Coninck, and N. Vindevogel, “Dissolution Characteristics of Hectorite in Inorganic Acids”, Appl. Clay Sci., 21(2), 241-256 (2002).
    29. L.A. Wendling, J.B. Harsh, C.D. Palmer, M.A. Hamilton, and M. Flury, “Cesium Sorption to Illite as Affected by Oxalate”, Clays Clay Miner., 52(3), 375-381 (2004).
    30. J. Wu, B. Li, J. Liao, Y. Feng, D. Zhang, J. Zhao, W. Wen, Y. Yang, and N. Liu, “Behavior and Analysis of Cesium Adsorption on Montmorillonite Mineral.”, J. Environ. Radioact., 100(10), 914-920 (2009).
    31. C. Liu, J.M. Zachara, S.C. Smith, J.P. McKinley, and C.C. Ainsworth, “Desorption Kinetics of Radiocesium from Subsurface Sediments at Hanford Site, USA”, Geochim. Cosmochim. Acta, 67(16), 2893-2912 (2003).
    32. C.W. Park, B.H. Kim, H.M. Yang, B.K. Seo, and K.W. Lee, “Enhanced Desorption of Cs from Clays by a Polymeric Cation-Exchange Agent”, J. Hazard. Mater., 327, 127-134 (2017).
    33. L.J. Poppe, V.F. Paskevich, J.C. Hathaway, and D.S. Blackwood. A Laboratory Manual for X-Ray Powder Diffraction, U.S. Geological Survey Open-File Report, 01-041 (2001).
    34. D. Carroll, “Clay Minerals: A Guide to Their X-Ray Identification”, Spec. Pap. Geol. Soc. Am., 126, 1-80 (1970).
    35. P. Komadel, J. Madejová, M. Janek, W.P. Gates, R.J. Kirkpatrick, and J.W. Stucki, “Dissolution of Hectorite in Inorganic Acids”, Clays Clay Miner., 44(2), 228- 236 (1996).
    36. D. Carroll and H.C. Starkey, “Reactivity of Clay Minerals with Acids and Alkalies”, Clays Clay Miner., 19(5), 321-333 (1971).
    37. J. Lee, S.M. Park, E.K. Jeon, and K. Baek, “Selective and Irreversible Adsorption Mechanism of Cesium on Illite”, Appl. Geochemistry, 85, 188-193 (2017).
    38. C.W. Park, S.M. Kim, I. Kim, I.H. Yoon, J. Hwang, J.H. Kim, H.M. Yang, and B.K. Seo, “Sorption Behavior of Cesium on Silt and Clay Soil Fractions”, J. Environ. Radioact., 233, 106592 (2021).
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