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Final storage of radioactive cesium by pollucite hydrothermal synthesis

Scientific Reports volume 4, Article number: 4195 (2014) | Download Citation

Abstract

The Fukushima nuclear accident has highlighted the importance of finding a better final storage method for radioactive cesium species. Cs is highly soluble in water, and can easily exchange with other alkali ions in zeolites or clays to form stable complexes. However, Cs+ is released from Cs+ complexes into water when surrounded by an excess of water. Pollucite may be the best final storage option for Cs+, but its typical synthesis requires heating to about 1200°C in air. Here, we show that the hydrothermal synthesis of pollucite can be completed at 300°C in three hours from any zeolite or clay. Furthermore, our procedure does not require ion exchange before synthesis. Radioactive Cs is usually found in complexes with clays. At that time, this method only requires calcium hydroxide, water, and three hours of hydrothermal synthesis, so the process is both inexpensive and practical for large-scale application. Pollucite is an analog of analcime zeolite, and contains a channel system 2.8 Å in diameter, which is formed by 6-oxygen rings. As the diameter of Cs+ is 3.34 Å and each Cs+ exists independently within a separate portion of the channel, Cs+ cannot exit the pollucite framework without breaking it.

Introduction

After the Fukushima nuclear accident on March 11, 2011, there are still strong emissions of radioactive cesium near the nuclear power plant. The removal and final storage of this cesium is an urgent issue, especially since no good final storage method has yet been discovered. Generally speaking, radioactive cesium is very soluble in water, like other alkali metal elements, but it also binds strongly with clays1,2, so the resulting spread of radiation will cover a wide area and continue for a long time. Many studies have described the successful immobilization of cesium3, but all of the reported methods are suitable for high-level nuclear waste. Radioactive cesium was spread out over a very wide area around the Fukushima nuclear power plant, and most of it is now tightly bound to the clay in the soil. It is very difficult to release these radioactive cesium ions without breaking layer structure of the clay. This will greatly increase the total cost of cleanup. Our procedure will directly convert Cs-clay complex into pollucite.

Pollucite belongs to the analcime zeolite family4,5,6,7, and is one of the best final storage options for radioactive Cs8,9,10 because it has an appropriately sized channel and does not release the radioactive Cs+ ions without complete destruction of the zeolite framework23. Figure 1 shows the channel system in pollucite and several Cs+ ions. The distance between two Cs+ ions in the channel is 5.92 Å11,12. The channel is constructed from 6-oxygen rings and has a diameter of 2.8 Å13,14,15. The diameter of the Cs+ ion is 3.34 Å16, so that after the pollucite has formed, it cannot release the trapped Cs+ ions without destroying the zeolite framework. Pollucite is a natural mineral17, and is also the principal source of elemental cesium18. This means that Cs+ ions within natural pollucite are not released, even over a long period of time. Unfortunately, pollucite is normally synthesized at about 1200°C in air19,20,21,22, or hydrothermally from certain specific zeolites. For example, chabazite transforms into pollucite at 240°C in 6 days23 and phillipsite changes into pollucite at 300°C in 13 hours24.

Figure 1: Illustration of pollucite.
Figure 1

Pollucite has the same framework and the same channel system as analcime, so that Cs+ ions were added into the analcime framework illustrated by Breck28. The diameters of the 6-oxygen ring and the Cs+ ion are 2.8 Å and 3.34 Å, respectively.

We show here a very promising storage method for radioactive Cs. The synthetic mixture had the following molar composition: 1CLP-10.5AlCl3-32Ca(OH)2-32CsCl-2300H2O, where CLP represents clinoptilolite (Na, K)6Al6Si72O196.nH2O, an abundant natural zeolite. Only stable Cs was used in the present experiments. Pollucite was synthesized at 300°C in 3 hours by hydrothermal synthesis, and the hydrothermal pressure was about 8.5 MPa. Pollucite was also synthesized in 3 hours from mordenite (MOR), which is another rich natural zeolite, and even from smectite clay (SMT) at 300°C. All yields were close to 100%. At 240°C and 3 MPa, pollucite can be completely synthesized in 12 days from MOR and in 6 days from CLP, and in a single day from SMT. X-ray fluorescence based elemental analysis of pollucite yielded the following results: Si:Al:Cs:Ca = 32:15:14.3:1.0 (from MOR), 32:20.2:11.8:0.2 (from CLP), 32:12.2:10.8:0 (from SMT), and 32:14.5:11.4:0 (from natural pollucite). XRD data for pollucite formed from CLP are shown in Fig. 2, with pollucite patterns calculated from the reference13. The pattern is the same as the patterns shown on ICDD card number 00-029-0407, PDF2 files. The synthetic process is shown in Fig. 3, and a photograph of the synthesized pollucite is shown in Fig. 4.

Figure 2: XRD patterns of pollucite from clinoptilolite at 300°C.
Figure 2
Figure 3: Crystallization curve for the formation of pollucite from clinoptilolite at 300°C.
Figure 3

X-ray intensity vs. synthetic time (hours).

Figure 4: Photos of synthetic pollucite at 240°C.
Figure 4

The samples were treated with 0.1 N HCl for one hour to dissolve the CaCO3. (a) 12 days from mordenite, and (b) 6 days from clinoptilolite.

It is generally recognized that pollucite is the best storage medium for radioactive Cs, but the synthetic method in air at 1200°C is very expensive and exhibits a problematic Cs volatilization at 1200°C. Fortunately, the cost can be drastically reduced by employing a three-hour hydrothermal synthesis with Ca(OH)2 at 300°C. This method is also very environmentally friendly, because no reagents other than Ca(OH)2 are used, and there is no significant Cs volatilization in the hydrothermal synthesis. Almost all other known storage methods involve ion-exchange substances, which all release absorbed radioactive Cs into the environment sooner or later1 without special treatment25 after adsorption. On the other hand, pollucite sequesters each Cs ion in a separate compartment, and the doorway to this compartment is smaller (2.8 Å in diameter) than the Cs ion itself (3.34 Å in diameter). Therefore, the Cs ion is not easily released from the pollucite framework, even if the framework becomes cracked. Only by breaking the framework completely apart can the Cs ion be released23,26. We focus on the final storage of radioactive cesium released into the environment. In this case, beta radiation results in transmutation, which changes both the ionic radius and valence of the element undergoing decay. The radiation damage over 20 years has been researched, and the results indicate that the pollucite structure remains remarkably unaffected by this transmutation27. Pollucite contains many Cs ions (more than 40 wt%) in its framework, is quite heavy, with a specific gravity of 2.9418, and is insoluble in water. Therefore, synthetic radioactive pollucite should be sunk to the bottom of lakes and ponds rather than buried under the ground. This procedure is the safest, easiest, and least expensive option. Our method is to directly convert radioactive Cs in the soil into pollucite. The produced pollucite in the soil is very stable to water, heat, and transmutation for a long time, although the method does not reduce the volume of soil containing radioactive Cs. We believe that the produced pollucite is so fine (less than 10 micrometers in particle diameter), and capable of solidification in cement along with the soil. The resulting compact cement blocks should be sunk into a lake or the sea rather than buried in the ground. It is not always the best way to concentrate radioactive cesium from the soil. As the concentration of radioactive cesium increases, the risk of radiation damage will increase, and the efficiency of processing the contaminated soil will worsen.

Methods

The synthetic mixture had the following molar composition when using MOR or SMT instead of CLP: 1MOR-12AlCl3-30Ca(OH)2-40CsCl-2300H2O or 1SMT-1.5AlCl3-33Ca(OH)2-33CsCl-2300H2O, respectively. MOR represents mordenite (Na8Al8Si40O96.24H2O) and SMT indicates smectite, a kind of clay with the following chemical composition: SiO2(63.8 wt%), Al2O3(24.9 wt%), CaO(0.6 wt%), Na2O(3.7 wt%), and K2O(0.1 wt%). The unit cell formula of pollucite is Cs16Al16Si32O96, and AlCl3 was added until the concentration ratio of [Al] to [Si] became 1/2 in the synthetic mixture. Ca(OH)2 was also added until the ratio of [OH] to [Si] became 1 in the synthetic mixture. Hydrothermal syntheses were carried out at 240°C for 1, 2, 4, 6, 8, 10, 12, 14, and 16 days and at 300°C for 0.5, 1, 3, 6, 12, and 24 hours.

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Affiliations

  1. Department of Applied Chemistry, National Defense Academy, Hashirimizu, Yokosuka 239, Japan

    • Yoshinobu Yokomori
    • , Kazuhito Asazuki
    • , Natsumi Kamiya
    • , Yudai Yano
    • , Koki Akamatsu
    • , Tetsuya Toda
    • , Atsushi Aruga
    •  & Koji Nishi
  2. Zero Sum Earth Co. Ltd., 6-8-081 Ichiba-cho, Chuo-ku, Chiba 260-0855, Japan

    • Yoshiaki Kaneo
    •  & Seiko Matsuoka
  3. Emeritus Professor, Graduate School of Agricultural and Life Sciences, The University of Tokyo, Bunkyo-ku, Tokyo, Japan

    • Satoshi Matsumoto

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Contributions

Y.Y. designed the project, performed experimental work, analyzed results, and wrote the manuscript. K.A., N.K., Y.Y., K.A. and T.T. performed experimental work. A.A. analyzed pollucite and Y.K., S.M. and K.N. designed the experimental work. S.M. oversaw and helped to write the manuscript.

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The authors declare no competing financial interests.

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Correspondence to Yoshinobu Yokomori.

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https://doi.org/10.1038/srep04195

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