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. 2022 Nov 5;15(21):7816.
doi: 10.3390/ma15217816.

Isotherm, Kinetic, and Selectivity Studies for the Removal of 133Ba and 137Cs from Aqueous Solution Using Turkish Perlite

Süleyman İnan  1   2 , Vipul Vilas Kusumkar  2 , Michal Galamboš  2 , Eva Viglašová  2 , Oľga Rosskopfová  2 , Martin Daňo  3
Affiliations

Isotherm, Kinetic, and Selectivity Studies for the Removal of 133Ba and 137Cs from Aqueous Solution Using Turkish Perlite

Süleyman İnan et al. Materials (Basel). .

Abstract

The efficiency of 133Ba and 137Cs removal from aqueous solution is vital to mitigate ecological concerns over spreading these radionuclides in the environment. The present work focused on the use of Turkish perlite for the sorptive removal of 133Ba and 137Cs from aqueous solution by the radioindicator method. Perlite was characterized by XRF, XRD, FTIR, SEM−EDX, and BET analyses. The maximum percentage removals of 88.2% and 78.7% were obtained for 133Ba and 137Cs at pH 6 and pH 9, respectively. For both ions, the sorption equilibrium was attained relatively rapidly. Experimental kinetic data were well described with pseudo-second-order and intraparticle diffusion models. The uptake of both ions increased with the increase in metal concentration (1 × 10−5 to 5 × 10−2 mol/L) in solution. The maximum uptake capacities of 133Ba and 137Cs were found to be 1.96 and 2.11 mmol/g, respectively. The effect of competing ions decreased in the order of Ca2+>K+>Ni2+>Na+ for 133Ba sorption, whereas for 137Cs sorption, the order was determined as Ca2+>Ni2+>K+>Na+. Selectivity studies pointed out that sorption of 133Ba onto perlite is preferable to 137Cs. Therefore, Turkish perlite is a promising, cost-effective, and efficient natural material for the removal of 133Ba and 137Cs from relatively diluted aqueous solution.

Keywords: barium; cesium; perlite; radioactive waste; sorption.

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Conflict of interest statement

The authors declare no conflict of interest. The funders had no role in the design of the study; in the collection, analyses, or interpretation of data; in the writing of the manuscript; or in the decision to publish the results.

Figures

Figure 1
Figure 1
Characterization of perlite: (a) XRD pattern; (b) FTIR spectrum; (c) SEM–EDX analysis.
Figure 2
Figure 2
Functional groups on perlite surface.
Figure 3
Figure 3
Possible surface reactions and metal bonding mechanism.
Figure 4
Figure 4
Influence of initial pH on the removal of Ba2+ and Cs+ using perlite (contact time: 60 min; metal ion concentration: 1 × 10−5 mol/L; dosage: 10 g/L; temperature: ambient conditions).
Figure 5
Figure 5
Influence of contact time on the removal of Ba2+ and Cs+ using perlite (initial pH 6 for Ba2+; initial pH 9 for Cs+; metal ion concentration: 1 × 10−5 mol/L; dosage: 10 g/L; temperature: ambient conditions).
Figure 6
Figure 6
Kinetic models for Ba2+ and Cs+ removal: (a) pseudo-second-order model; (b) intraparticle diffusion model.
Figure 7
Figure 7
(a) Influence of metal ion concentration on the removal of Ba2+ and Cs+ using perlite; (b) Freundlich isotherm (initial pH 6 (Ba2+); pH 9 (Cs+); contact time: 60 min; dosage: 10 g/L; temperature: ambient conditions).
Figure 8
Figure 8
Influence of sorbent dosage on the removal of Ba2+ and Cs+ using perlite (initial pH 6 (Ba2+); pH 9 (Cs+); metal ion concentration: 1 × 10−3 mol/L; contact time: 60 min; temperature: ambient conditions).
Figure 9
Figure 9
The variation in sorption percentage of Ba2+ (a) and Cs+ (b) ions on perlite in the presence of competing ions (Na+, K+, Ni2+, and Ca2+) (concentration of Ba2+ and Cs+: 1 × 10−5 mol/L; concentration of competing ions: 1 × 10−5 to 5 × 10−2 mol/L).
Figure 10
Figure 10
The variation in (a) Kd values and (b) selectivity coefficients as a function of initial pH (concentration of Ba2+ and Cs+: 1 × 10−5 mol/L; contact time: 60 min; temperature: ambient conditions).
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