New insight into the adsorption of ruthenium, rhodium, and palladium from nitric acid solution by a silica-polymer adsorbent

New insight into the adsorption of ruthenium, rhodium, and palladium from nitric acid solution by a silica-polymer adsorbent a first-author a https://orcid.org/0000-0002-9573-5960 a a a a a b https://orcid.org/0000-0003-3821-9078 Guangxi Key Laboratory of Processing for Non-ferrous Metals and Featured Materials,School of Resources, Environment and Materials, Guangxi University, Nanning 530004, China. Guangxi Key Laboratory of Processing for Non-ferrous Metals and Featured Materials,School of Resources, Environment and Materials, Guangxi University, Nanning 530004, China. School of Nuclear Science and Engineering, Shanghai Jiao Tong University, Shanghai 200240, China. School of Nuclear Science and Engineering, Shanghai Jiao Tong University, Shanghai 200240, China. A porous silica-polymer based adsorbent, iso Bu-BTP/SiO 2 -P, was prepared by a vacuum impregnation method and used for the recovery of ruthenium, rhodium, and palladium from nitric acid solution. The experimental results revealed that iso Bu-BTP/SiO 2 -P exhibited unique adsorption properties such as high saturation adsorption capacity (Ru: 0.35 mmol g -1 , Rh: 0.32 mmol g -1 , Pd: 1.05 mmol g -1 ) and excellent selectivity over other metal ions, such as lanthanides ( SF PGM/M > 40) in 1 M HNO 3 solution, The adsorption process conformed to the pseudo-second-order model and Langmuir model. From the UV, FT-IR and XPS analyses, it can be concluded that the strong affinity between functional groups (C-N=C) and metal ions, as well as NO 3 - played a role in coordination during the adsorption process. Furthermore, the desorption behavior was studied, and it was found that the adsorbed Pd, Rh, and Ru could be eluted with a 0.01 M nitric acid-0.1 M thiocarbamide solution, 5 M hydrochloric acid, and sodium hypochlorite (CP) solution, respectively. Finally, based on those findings, a simple process for the separation and recovery of Pd, Rh, and Ru from high-level liquid waste using iso Bu-BTP/SiO 2 -P was designed and proposed. BTP adsorption Ruthenium Rhodium Palladium High-level liquid waste 1. Introduction 1 The platinum group metals (PGMs: Ru, Rh, Pd, Os, Pt, and Ir) have unique properties in many industrial applications, e.g., the aerospace materials, automobile and electroplating industries [ 1 1 ]. However, the abundance of PGMs in the earth’s crust is very low, ranging from 0.022 to 0.52 µg L -1 [ 2 2 , 3 3 ]. On the other hand, high-level liquid waste (HLLW) contains significant quantities of PGMs, mainly Ru, Rh, and Pd. One ton of spent fuel from a commercial light water reactor or fast breeder reactor contains approximately 4 kg and 19 kg PGMs, respectively. Thus, those spent fuels and can be regarded as important PGM sources, comparable with the PGM reserves in the earth [ 4 4 ]. In addition, Ru is easily oxidized to RuO 4 at high temperature; some of this Ru is radiotoxic, such as 106 Ru (t 1/2 : 373.6 days), which will enlarge the area contaminated with radioactively. Some Ru is coextracted with uranium and plutonium in the plutonium uranium extraction (PUREX) process; the coextracted Ru is difficult to strip and will reduce the decontamination coefficients of uranium and plutonium, which may interfere with the PUREX process. In addition, the 107 Pd content of spent fuel is approximately 0.17 kg ton -1 ; this isotope has a half-life of approximately 6.5 ×10 6 years. Furthermore, during the vitrification process, PGMs increase the glass melting point and phase separation, resulting in uneven distribution of the glass matrix [ 5 5 - 7 7 5-7 ]. Thus, from the viewpoints of resource recovery, radiotoxicity reduction and enhancement of the PUREX and vitrification processes, the removal of PGMs from HLLW is crucial. However, the PGM separation process is complicated and costly owing to the high radioactivity, acidity, and complexity of HLLW. Therefore, the question of how to effectively separate and recover PGMs from nitric solution has been receiving increasing attention [ 8 8 - 10 10 8-10 ]. Many methods have been applied to recover PGMs from HNO 3 solution. Sung Ho Lee et al. studied several ion exchange resins for the recovery of Ru and Pd from simulated radioactive liquid waste; the resins exhibited excellent adsorption properties [ 11 11 ]. M Ozawa et al. proposed the used of ion-exchange chromatography and catalytic electrode hybrid extraction technology to separate PGMs from nitric acid solution [ 12 12 ]. Zambrzycka et al. synthesized a novel ion-imprinted polymer (Ru-BnTSn) that exhibits excellent adsorption performance toward Ru(III) at pH 8.0±0.1, and from which Ru can be eluted by 0.3 M thiourea in 0.3 M hydrochloric acid solution [ 13 13 ]. However, previous works have shown very poor efficiency in the separation of PGMs from other metals; this has attracted widespread attention to this subject. R-BTP ligands are well-known for the separation of minor actinides from HLLW. Some studies have found that R-BTPs also have excellent Pd separation ability [ 14 14 - 17 17 14-17 ]. Shunyan Ning et al. used Me 2 -CA-BTP/SiO 2 -P for the effective separation of minor actinides (Am, Cm, etc.) from HLLW and simultaneously realized the separation of Pd and other fission products [ 14 14 ]. Ruiqin Liu used iso HexBTP/SiO 2 -P for the recovery of Pd from 3 M HNO 3 solution with an adsorption capacity of over 0.8 mmol g -1 [ 18 18 ]. However, no research has found BTP ligands exhibit good adsorption properties towards Ru and Rh in nitric acid solution. Occasionally, iso Bu-BTP/SiO 2 -P has been reported to exhibit good adsorption properties towards Ru and Rh at high temperatures, such as 328 K. Based on the above considerations, the porous material iso Bu-BTP/SiO 2 -P ( Fig. 1 Fig. 1 ) was prepared to separate PGMs from nitric solution [ 19 19 ]. The effect of the HNO 3 concentration, temperature, contact time, and initial PGM concentration on adsorption was studied using batch experiments. The elution behavior of the loaded PGMs under various conditions was also evaluated. Furthermore, the underlying mechanism of interaction between the as-prepared adsorbent and the PGMs was evaluated by means of spectroscopy (FT-IR, XPS) in this study. 2 Experimental Section 1 2.1 Reagents 2 All reagents, including nitric acid, hydrochloric acid, perchloric acid, methanol, dichloromethane, and thiourea, were of analytical grade. Stock solutions including those of Ru(III), Rh(III), Pd(II), and other fission products (FPs), were purchased from Aladdin Biochemical Technology Co., Ltd (Shanghai). The purity of iso Bu-BTP was 94% according to HPLC tests. Iso Bu-BTP dissolved in CH 2 Cl 2 was loaded into porous SiO 2 -P with a diameter of approximately 50 µm and a pore size of approximately 60 nm to achieve an iso Bu-BTP loading rate of approximately 33 wt% [ 19 19 ]. 2.2 Evaluation of adsorption performance 2 PGM adsorption experiments were carried out using the as-prepared adsorbents. 0.05 g of the adsorbent was mixed with 2.5 mL of liquid containing the targeted metal ions and then shaken mechanically at a constant speed (120 rpm). A filter with a pore size of 0.45 µm was used for phase separation. The concentrations of the metal ions in the aqueous solutions were tested using ICP-AES (Shimadzu, ICPS-7510). The adsorption capacity Q (mmol g -1 ), adsorption efficiency E (%), distribution coefficient K d (mL g -1 ), and separation factor SF M/N were calculated as follows: <math display="block" id="M1"><mrow><mi>Q</mi><mtext> = </mtext><mfrac><mrow><mtext>(</mtext><msub><mi>C</mi><mtext>o</mtext></msub><mo>−</mo><mi>C</mi><mo stretchy="false">)</mo></mrow><mi>m</mi></mfrac><mo>×</mo><mi>V</mi><mo>,</mo></mrow></math> <math display="block" id="M2"><mrow><mi>E</mi><mtext> = </mtext><mfrac><mrow><mtext>(</mtext><msub><mi>C</mi><mtext>o</mtext></msub><mo>−</mo><mi>C</mi><mo stretchy="false">)</mo></mrow><mrow><msub><mi>C</mi><mtext>o</mtext></msub></mrow></mfrac><mo>×</mo><mn>100</mn><mi>%</mi><mo>,</mo></mrow></math> <math display="block" id="M3"><mrow><msub><mi>K</mi><mtext>d</mtext></msub><mtext> = </mtext><mfrac><mrow><mtext>(</mtext><msub><mi>C</mi><mtext>o</mtext></msub><mo>−</mo><mi>C</mi><mo stretchy="false">)</mo></mrow><mi>C</mi></mfrac><mo>×</mo><mfrac><mi>V</mi><mi>m</mi></mfrac><mo>,</mo></mrow></math> <math display="block" id="M4"><mrow><mi>S</mi><msub><mi>F</mi><mrow><mtext>M/N</mtext></mrow></msub><mo>=</mo><msub><mi>K</mi><mtext>d</mtext></msub><msub><mrow/><mtext>M</mtext></msub><mo>/</mo><msub><mi>K</mi><mtext>d</mtext></msub><msub><mrow/><mrow><mtext>N,</mtext></mrow></msub></mrow></math> where C o , and C (mg L -1 ) are the concentration of the original solution and the concentration at adsorption equilibrium, respectively. V (mL) and m (g) are the volume of the initial solution and the weight of the adsorbent. 2.3 Mechanistic study 2 UV spectroscopy (UV-3600 Plus, SHIMADZU) was applied to analyze the effect of the H + concentration and temperature on the PGM adsorption mechanism of iso Bu-BTP/SiO 2 -P. The analysis of the effect of the H + concentration was performed in a mixed solution of acetonitrile/HClO 4 ( V : V =1:1) by fixing the concentration of fresh iso Bu-BTP (1×10 -4 M) and varying the HClO 4 concentration. HClO 4 was chosen to adjust the H + concentration because ClO 4 - cannot coordinate with the adsorbent, thus eliminating a potential anion effect. To analyze the temperature effect, iso Bu-BTP/SiO 2 -P was first placed in contact with 1 M HNO 3 at different temperatures for three days. After phase separation and drying in a vacuum oven, the iso Bu-BTP was dissolved in acetonitrile to achieve a 2×10 -4 M iso Bu-BTP concentration. The changes in the functional groups of fresh iso Bu-BTP/SiO 2 -P and PGM-loaded iso Bu-BTP/SiO 2 -P were characterized by FT-IR using an IRTracer-100 instrument (SHIMADZU). The sample was prepared by mixing the iso Bu-BTP/SiO 2 -P with potassium bromide (KBr), fully grinding the resulting mixture, and pressing it into thin sheets. Furthermore, XPS (Thermo ESCALAB 250XI) was used to analyze chemical changes in the adsorbent before and after adsorption. The C1 s peak was corrected to 284.6 eV. The samples were dried by placing them in a vacuum constant temperature drying oven (VOC-210C, EYELA) at 313 K. 3 Results and discussion 1 3.1 Batch adsorption experiments 2 3.1.1 Effects of HNO 3 concentration and temperature 3 The effect of the HNO 3 concentration at 328 K and that of the temperature on the adsorption behavior of iso Bu-BTP/SiO 2 -P towards the PGMs were evaluated ( Fig. 2 Fig. 2 ). The adsorption of the adsorbent towards PGMs first increased with increasing HNO 3 concentration and reached a maximum at 1 M HNO 3 with Pd, Ru, and Rh adsorption efficiencies, as high as 99.9%, 96.7% and 67.4% respectively, and then decreased with further increase in the HNO 3 concentration ( Fig. 2 (a) Fig. 2 (a) ). Furthermore, the changes in the adsorption behavior with temperature were also investigated. As the temperature was increased from 298 K to 328 K ( Fig. 2 (b) Fig. 2 (b) ), the adsorption efficiency towards Pd(II) exhibited almost no change, while the adsorption efficiency towards Ru(III) and Rh(III) increased rapidly. UV spectra were used to elucidate the adsorption phenomena caused by temperature and acid ( Fig. 3 Fig. 3 ). With increasing H + concentration, an isosbestic point appeared at approximately 305 nm, indicating the generation of a new species which was supposed to be protonated iso Bu-BTP/SiO 2 -P [ 20 20 ]. The UV absorption intensity increased ( C HNO3 < 1 M), and then remained stable as the H + concentration was further increased to 2 M ( Fig. 3(a) Fig. 3(a) ), indicating that protonated iso Bu-BTP/SiO 2 -P was gradually formed [ 20 20 ]. It is well-known that the dominant form of Pd is Pd 2+ and that the main forms of Rh are Rh 3+ and Rh(NO 3 ) 2+ , while Ru(III) can exist in the form of complex complexes such as Ru(NO) 3+ and [RuNO(NO 3 ) n (H 2 O) 5-n ] 3-n in nitric acid solution [ 2 2 , 11 11 , 21 21 ]. The positive charge of the protonated adsorbent would not be beneficial to adsorption of metal ions with positive charges, such as Pd 2+ and Rh(NO 3 ) 2+ . Thus the decrease in adsorption may be caused by the increase in protonation with acidity. However, the overall adsorption process requires NO 3 - to maintain charge balance, as was proven later by IR and XPS analysis. This leads to the increase in adsorption with increasing acidity in the 0.1-1 M HNO 3 range. The effect of temperature on the UV spectra of iso Bu-BTP/SiO 2 -P after contact with 1 M HNO 3 solution at 298-328 K was also studied ( Fig. 3 (b) Fig. 3 (b) ). The absorption intensity of the UV spectra decreased with increasing temperature, which indicates a decreased degree of protonation that resulted in the increase in adsorption with temperature [ 20 20 , 22 22 , 23 23 ]. Moreover, the adsorption behavior of the adsorbent towards other elements that are usually present in HLLW, such as Sr, Zr, Mo, Y, La, Ce, Pr, Nd, Sm, Eu, and Gd, was studied at 328 K ( Fig. 4 Fig. 4 ). The K d values of the PGMs were much higher than those of the other metal ions, with an SF PGMs/M value of over 40, indicating that Ru, Rh, and Pd could be effectively and efficiently separated from other metal ions using iso Bu-BTP/SiO 2 -P. 3.1.2. Kinetics study 3 The kinetics of PGM adsorption at various temperatures was studied ( Fig. 5 Fig. 5 ). The adsorption of Ru(III) ( Fig. 5 (a) Fig. 5 (a) ) was relatively slow at 298 K, and with the uptake rate still increasing at a contact time of 144 h. The adsorption kinetics were significantly improved at higher temperatures, equilibrium was obtained within approximately two days at 318 K and 328 K. In the case of Rh(III) ( Fig. 5 (b) Fig. 5 (b) ), the adsorption kinetics improved with increasing temperature, but a long time was required to reach equilibrium even at 328 K. For Pd(II) ( Fig. 5 (c) Fig. 5 (c) ), adsorption was relatively fast compared with Ru and Rh, with equilibrium being obtained within 1 day. To clearly understand the adsorption characteristics, both a pseudo-first-order kinetics model (PFORE, Eq. 5) and a pseudo-second-order kinetic model (PSORE, Eq. 6) were employed to analyze the experimental data [ 24 24 ]: <math display="block" id="M5"><mrow><mi>ln</mi><mo stretchy="false">(</mo><msub><mi>Q</mi><mtext>e</mtext></msub><mo>−</mo><msub><mi>Q</mi><mi>t</mi></msub><mo stretchy="false">)</mo><mo>=</mo><mi>ln</mi><msub><mi>Q</mi><mi>e</mi></msub><mo>−</mo><msub><mi>k</mi><mn>1</mn></msub><mi>t</mi><mo>,</mo></mrow></math> <math display="block" id="M6"><mrow><mfrac><mi>t</mi><mrow><msub><mi>Q</mi><mi>t</mi></msub></mrow></mfrac><mo>=</mo><mfrac><mn>1</mn><mrow><msub><mi>k</mi><mn>2</mn></msub><msub><mi>Q</mi><mi>e</mi></msub></mrow></mfrac><mo>+</mo><mfrac><mi>t</mi><mrow><msub><mi>Q</mi><mi>e</mi></msub></mrow></mfrac><mo>,</mo></mrow></math> where Q t , and Q e (mmol g -1 ) are the adsorption capacity at t (h) and equilibrium, and k 1 (h -1 ) and k 2 (mmol g -1 h -1 ) are the constants of the PFORE and PSORE respectively. The fitting results are shown in Table 1 Table 1 and Fig. 5 (d) Fig. 5 (d) for Ru(III), Fig. 5 (e) Fig. 5 (e) for Rh(III), and Fig. 5 (f) Fig. 5 (f) for Pd(II). As shown in Table 1 Table 1 , based on the higher correlation coefficients (R 2 ) and excellent consistency between the calculated equilibrium adsorption capacities ( Q e ) and the experimental ones ( Q e,exp ), the experimental results were well-fitted by the PSORE model, which indicates that the overall process is mainly chemical adsorption. Moreover, k 2 also increases quickly with temperature, which means that the adsorption rate increases quickly. 1 1 Element 1 1 T (K) 3 1 Pseudo-first-order model 3 1 Pseudo-second-order model 1 1 Q e,exp (mmol g -1 ) 1 1 1 1 1 1 K (h -1 ) 1 1 Q e (mmol g -1 ) 1 1 R 2 1 1 K (g mmol·h -1 ) 1 1 Q e (mmol g -1 ) 1 1 R 2 1 1 1 1 Ru 1 1 298 1 1 0.48 1 1 0.22 1 1 0.599 1 1 0.27 1 1 0.22 1 1 0.996 1 1 0.22 1 1 1 1 318 1 1 0.29 1 1 0.33 1 1 0.804 1 1 0.26 1 1 0.31 1 1 0.998 1 1 0.30 1 1 1 1 328 1 1 0.72 1 1 0.32 1 1 0.663 1 1 0.55 1 1 0.35 1 1 0.999 1 1 0.35 1 1 Rh 1 1 298 1 1 0.01 1 1 0.13 1 1 0.97 1 1 0.007 1 1 0.12 1 1 0.943 1 1 0.12 1 1 1 1 318 1 1 0.09 1 1 0.30 1 1 0.98 1 1 0.086 1 1 0.29 1 1 0.999 1 1 0.29 1 1 1 1 328 1 1 0.33 1 1 0.33 1 1 0.908 1 1 0.306 1 1 0.32 1 1 0.998 1 1 0.32 1 1 Pd 1 1 298 1 1 1.34 1 1 0.61 1 1 0.682 1 1 1.02 1 1 0.61 1 1 1.000 1 1 0.62 1 1 1 1 318 1 1 3.29 1 1 0.63 1 1 0.282 1 1 2.24 1 1 0.64 1 1 1.000 1 1 0.64 1 1 1 1 328 1 1 3.46 1 1 0.67 1 1 0.272 1 1 2.32 1 1 0.68 1 1 1.000 1 1 0.68 3.1.3 Adsorption isotherms 3 The adsorption isotherms were determined by increasing the initial metal ion concentrations of each PGM individually in solution ( Fig. 6 Fig. 6 ). The uptake amount ( Q e ) increased with the increase in the PGM equilibrium concentrations. Furthermore, Q e increased significantly with temperature, which means that increasing temperature is beneficial to adsorption. Both the Langmuir isotherm model and the Freundlich isotherm model shown in Eq. (7) and Eq. (8) respectively, were used to analyze the experimental data [ 24 24 ]: <math display="block" id="M7"><mrow><msub><mi>Q</mi><mtext>e</mtext></msub><mtext>=</mtext><mfrac><mrow><msub><mi>q</mi><mi>m</mi></msub><mo>×</mo><msub><mi>K</mi><mi>L</mi></msub><mo>×</mo><msub><mi>C</mi><mi>e</mi></msub></mrow><mrow><mn>1</mn><mo>+</mo><msub><mi>K</mi><mi>L</mi></msub><mo>×</mo><msub><mi>C</mi><mi>e</mi></msub></mrow></mfrac><mo>,</mo></mrow></math> <math display="block" id="M8"><mrow><msub><mi>Q</mi><mtext>e</mtext></msub><mo>=</mo><msub><mi>K</mi><mi>F</mi></msub><mo>×</mo><msub><mi>C</mi><mi>e</mi></msub><msup><mrow/><mrow><mfrac><mn>1</mn><mi>n</mi></mfrac></mrow></msup><mo>,</mo></mrow></math> where Q e (mmol g -1 ) is the equilibrium uptake amount, and q m (mmol g -1 ), and C e (mmol L -1 ) are the calculated saturation adsorption capacity and equilibrium ion concentration in solution, respectively. K L (L mmol -1 ) is the Langmuir constant, and K F (mmol 1-n ·L n g -1 ) and n are the Freundlich constants. As shown in Table 2 Table 2 , the higher R 2 values and consistency between q m and Q e,exp indicate that the adsorption behavior of the PGMs is better fitted with the Langmuir model, which in turn suggests that the overall adsorption process is mainly monolayer chemical adsorption. Compared with other adsorbents ( Table 3 Table 3 ), the high adsorption capacity is one of the biggest highlights of iso Bu-BTP/SiO 2 -P. 1 1 Element 1 1 T (K) 3 1 Langmuir isotherm 3 1 Freundlich isotherm 1 1 Q e,exp (mmol g -1 ) 1 1 1 1 1 1 K L (L mmol -1 ) 1 1 q m (mmol g -1 ) 1 1 R 2 1 1 n 1 1 K F ( mmol 1-n ·L n g  -1 ) 1 1 R 2 1 1 1 1 Ru 1 1 308 1 1 1.49 1 1 0.25 1 1 0.989 1 1 4.19 1 1 0.18 1 1 0.927 1 1 0.24 1 1 1 1 318 1 1 2.42 1 1 0.30 1 1 0.971 1 1 2.85 1 1 0.20 1 1 0.939 1 1 0.31 1 1 1 1 328 1 1 3.31 1 1 0.34 1 1 0.893 1 1 3.89 1 1 0.24 1 1 0.819 1 1 0.35 1 1 Rh 1 1 308 1 1 0.93 1 1 0.14 1 1 0.919 1 1 4.95 1 1 0.09 1 1 0.874 1 1 0.13 1 1 1 1 318 1 1 1.81 1 1 0.30 1 1 0.961 1 1 3.83 1 1 0.21 1 1 0.864 1 1 0.30 1 1 1 1 328 1 1 1.82 1 1 0.33 1 1 0.982 1 1 2.60 1 1 0.21 1 1 0.855 1 1 0.32 1 1 Pd 1 1 308 1 1 1.40 1 1 0.91 1 1 0.989 1 1 3.56 1 1 0.57 1 1 0.882 1 1 0.92 1 1 1 1 318 1 1 2.14 1 1 1.01 1 1 0.988 1 1 3.73 1 1 0.69 1 1 0.867 1 1 1.00 1 1 1 1 328 1 1 3.23 1 1 1.06 1 1 0.944 1 1 5.47 1 1 0.87 1 1 0.792 1 1 1.05 1 1   1 1 Material 1 1 Acid concentration (M) 1 1 Temperature (K) 1 1 Q (mmol g -1 ) 1 1 Contact time 1 1 Reference 1 1 Ru 1 1 (Cera+Dodec)/SiO 2 -P 1 1 3 M HNO 3 1 1 298 1 1 0.088 1 1 20 h 1 1 [ 25 25 ] 1 1 1 1 Lewatit Mono 1 1 Acetic acid 1 1 298 1 1 0.048 1 1 45 min 1 1 [ 26 26 ] 1 1 1 1 Plus M600 1 1 1 1 Raw. C. glutamicum biomass 1 1 Acetic acid 1 1 298 1 1 0.15 1 1 30min 1 1 [ 26 26 ] 1 1 1 1 This work 1 1 1 M HNO 3 1 1 328 1 1 0.35 1 1 48 h 1 1   1 1 Rh 1 1 (Cera+Dodec)/SiO 2 -P 1 1 3 M HNO 3 1 1 298 1 1 0.072 1 1 72 h 1 1 [ 25 25 ] 1 1 1 1 (Crea+TOA)/SiO 2 -P 1 1 3 M HNO 3 1 1 298 1 1 0.306 1 1 72 h 1 1 [ 27 27 ] 1 1 1 1 Purolite S985 1 1 2.35 HCl 1 1 Room temperature 1 1 0.120 1 1 24 h 1 1 [ 28 28 ] 1 1 1 1 This work 1 1 1 M HNO 3 1 1 328 1 1 0.32 1 1 48 h 1 1   1 1 Pd 1 1 Me 2 -CA-BTP/SiO 2 -P 1 1 3 M HNO 3 1 1 298 1 1 0.80 1 1 12 h 1 1 [ 29 29 ] 1 1 1 1 XAD-16 1 1 3 M HNO 3 1 1 298 1 1 0.19 1 1 45 min 1 1 [ 30 30 ] 1 1 1 1 iso Hex-BTP/SiO 2 -P 1 1 3 M HNO 3 1 1 298 1 1 0.89 1 1 24 h 1 1 [ 31 31 ] 1 1 1 1 This work 1 1 1 M HNO 3 1 1 328 1 1 1.05 1 1 24 h 1 1   3.1.4 Adsorption thermodynamics 3 According to the experimental results, the amount of PGMs adsorbed on iso Bu-BTP/SiO 2 -P increased with temperature. To better understand the adsorption thermodynamics, the main thermodynamic parameters were obtained using the Van’t Hoff equation [ 32 32 ]. <math display="block" id="M9"><mrow><mi>ln</mi><msub><mi>K</mi><mtext>L</mtext></msub><mtext> = </mtext><mo>−</mo><mfrac><mrow><mi>Δ</mi><msup><mi>H</mi><mtext>o</mtext></msup></mrow><mrow><mi>R</mi><mi>T</mi></mrow></mfrac><mo>+</mo><mfrac><mrow><mi>Δ</mi><msup><mi>S</mi><mtext>o</mtext></msup></mrow><mi>R</mi></mfrac><mo>,</mo></mrow></math> <math display="block" id="M10"><mrow><mi>Δ</mi><msup><mtext>G</mtext><mtext>o</mtext></msup><mtext> = </mtext><mi>Δ</mi><msup><mi>H</mi><mtext>o</mtext></msup><mo>−</mo><mi>Δ</mi><msup><mi>S</mi><mtext>o</mtext></msup><mi>T</mi><mo>,</mo></mrow></math> where ∆ G° (J mol -1 ), ∆ H° (J mol -1 ), and ∆ S° (J K -1 ·mol -1 ) are the changes in the Gibbs free energy, enthalpy, and entropy, respectively. R (8.314 J K -1 ·mol -1 ) represents the gas constant at temperature T (K). As depicted in Fig. 6 (d) Fig. 6 (d) and Table 4 Table 4 , the values of positive ∆ H° were positive, which means that the adsorption is endothermic. This is consistent with the observation that the saturation adsorption capacity increases with temperature. The negative ∆ G° values indicate that the adsorption is spontaneous. Moreover, the positive ∆ S° values indicate that the adsorption of PGMs on iso Bu-BTP/SiO 2 -P is an entropy-driven process. 1 1 Element 1 1 T (K) 1 1 K L (L mol -1 ) 1 1 ∆ H° (J mol -1 ) 1 1 ∆ S° (J mol -1 ) 1 1 ∆ G° (J mol -1 ) 1 1 Ru 1 1 308 1 1 1.74×10 3 1 1 3.25×10 3 1 1 11.13 1 1 -0.18×10 3 1 1 1 1 318 1 1 2.55×10 3 1 1 1 1 1 1 -0.29×10 3 1 1 1 1 328 1 1 3.31×10 3 1 1 1 1 1 1 -0.40×10 3 1 1 Rh 1 1 308 1 1 1.07×10 3 1 1 3.26×10 3 1 1 10.66 1 1 -0.02×10 3 1 1 1 1 318 1 1 1.52×10 3 1 1 1 1 1 1 -0.13×10 3 1 1 1 1 328 1 1 2.04×10 3 1 1 1 1 1 1 -0.24×10 3 1 1 Pd 1 1 308 1 1 1.40×10 3 1 1 4.22×10 3 1 1 14.04 1 1 -0.10×10 3 1 1 1 1 318 1 1 2.14×10 3 1 1 1 1 1 1 -0.24×10 3 1 1 1 1 328 1 1 3.23×10 3 1 1 1 1 1 1 -0.39×10 3 3.2 Interaction mechanism study 2 3.2.1 XPS analysis 3 XPS was employed to obtain more information about the changes to the functional groups and electronic states of iso Bu-BTP/SiO 2 -P. As depicted in Fig. 7 (a) Fig. 7 (a) , the peaks of the four main elements (C, N, O, and Si) are observed in all samples, but the signals of the PGMs are only observed in the PGM-loaded adsorbents which indicates that the PGMs were adsorbed successfully. The 3d scans of the PGMs are shown in Fig. 7 (b) Fig. 7 (b) . The doublet separation between the 3d 3/2 and 3d 5/2 peaks of Ru, Rh, and Pd are 3.4 eV, 4.63 eV, and 5.27 eV, respectively, which fit well with the previously reported results [ 33 33 - 36 36 33-36 ]. Due to the overlap of C 1s(284.6 eV) and Ru 3d 3/2(284.61 eV), the peak of Ru 3d 3/2 shows a small deviation [ 37 37 ]. The state of N is very complicated. In the case of fresh iso Bu-BTP/SiO 2 -P ( Fig. 7 (c) Fig. 7 (c) ), only two forms of N are present, i.e., C-N=C and C-N=N. The ratio of C-N=C to C-N=N is 42.82%:57.18% which is very close to the theoretical ratio of 3:4. For the PGM-loaded iso Bu-BTP/SiO 2 -P samples, other forms of N may exist, such as N-O in [RuNO] and NO 3 - complexed with PGMs [ 33 33 , 38 38 - 43 43 38-43 ]. Furthermore, in the N 1s spectra, the binding energy of C-N=C shifts from 399.55 eV to 399.94 eV (Ru), 399.87 eV (Rh), and 400.05 eV (Pd), and the energy of C-N=N shifts from 399.57 eV to 400.13 eV (Ru), 400.09 eV (Rh), and 400.23 eV (Pd). These interesting shifts revealed the strong charge interactions between the PGMs and nitrogen-containing functional groups. 3.2.2 FT-IR analysis 3 FT-IR analysis was employed to further understand the interaction mechanism between the as-prepared adsorbent and Ru and Rh ( Fig. 8 Fig. 8 ). The characteristic peaks at 1113, 802, 475 cm -1 result from the Si-O-Si stretching vibration [ 15 15 ]. The peak at 1379 cm -1 is indicative of the C-H bond. In addition, the transmittance was enhanced after the adsorption of the PGMs. The reason for this phenomenon is that NO 3 - also has a characteristic peak at 1380 cm -1 and two peaks (C-H and NO 3 - ) are superimposed [ 44 44 ], which implies that NO 3 - participates in the adsorption process. The peak at 1635 cm -1 arises from the C-N=N of the pyridine ring and shows almost no change after adsorption. The characteristic peak of C-N=C in the pyridine ring exhibits significant shifts, from 1526 to 1552 cm -1 after Ru adsorption and 1540 cm -1 after Rh adsorption. The two peaks located at the 2870 and 2970 cm -1 should arise from the C-H and SiO 2 -P of iso Bu-BTP, respectively. The peak centered at 3440 cm -1 originates from the O-H of H 2 O. Comparing the spectra before and after adsorption, almost no significant changes were found except for the significant shift in the position of C-N=C, which implies that the C-N=C (pyridine ring) plays an important role in the overall adsorption process. The larger shift of C-N=C in Ru- iso Bu-BTP/SiO 2 -P compared to Rh- iso Bu-BTP/SiO 2 -P indicates stronger interaction between the adsorbent and Ru(III) than Rh(III), which may be attributed to the different ionic radius (Pd 2+ > Ru 3+ > Rh 3+ ) [ 45 45 ] leading to a better match in terms of size. Moreover, the spectra exhibited almost no changes with increasing time, indicating that the interaction mechanism did not change over time. 3.3 Desorption performance 2 To further evaluate the performance of iso Bu-BTP/SiO 2 -P, the desorption performances of different eluents were evaluated; the results are shown in Table 5 Table 5 . In complex mixed metal systems, such as HLLW, other metal ions may also be involved, so the desorption behavior of Ln was also studied. The poorly adsorbed lanthanide(III) could be desorbed by all the experimental eluents, so it could be desorbed first using H 2 O, which had poor elution performance towards the other metal ions in the desorption stage. In our previous research, it was found that Am(III) could be effectively desorbed using 0.01 M DTPA, which is very similar to EDTA-2Na and cannot effectively desorb PGMs, after Ln(III) was desorbed by H 2 O, [ 46 46 ] which can be desorbed using a by 0.01 M HNO 3 -0.1 M thiocarbamide solution but not by water or EDTA-2Na, could then be eluted. After that, Rh(III) could be desorbed using 5 M HCl. Finally, a NaClO solution is used to desorb Ru(III). A simple process to separate PGMs from simulated HLLW using iso Bu-BTP/SiO 2 -P is proposed in Fig. 9 Fig. 9 . 1 1 Eluent 4 1 Desorption efficiency (%) 1 1 1 1 Ru 1 1 Rh 1 1 Pd 1 1 Ln 1 1 pure water 1 1 2.2 1 1 4.7 1 1 4.8 1 1 89.6 1 1 0.01 M HNO 3 - 0.1M THU 1 1 6.1 1 1 3.9 1 1 90.1 1 1 82.5 1 1 5 M HCl 1 1 6.9 1 1 78.4 1 1 38.6 1 1 85.3 1 1 NaClO(CP) 1 1 68.6 1 1 59.4 1 1 75.5 1 1 74.1 1 1 0.01 M EDTA-2Na 1 1 2.4 1 1 7.6 1 1 5.4 1 1 65.4 4 Conclusion 1 In this work, the silica-polymer based adsorbent iso Bu-BTP/SiO 2 -P was synthesized for the separation and recovery of palladium, rhodium, and ruthenium from a nitric acid medium. The results show that the adsorbent exhibits superior adsorption properties, with uptake rates of over 98% for Ru, 64% for Rh, and 99% for Pd in 1 M nitric acid solution at 328 K. The adsorption behavior towards the PGMs matched well with the PSORE model, with adsorption equilibrium being obtained within 2 d, 3 d, and 1 d for Ru, Rh, and Pd at 328 K, respectively. Furthermore, the experimental data reveal that the saturation adsorption capacities of the adsorbent towards Ru, Rh, and Pd are 0.35, 0.32, and 1.05 mmol g -1 and fit well with the Langmuir model. Moreover, according to the calculated thermodynamics results, it can be concluded that the whole adsorption process is actually endothermic. FT-IR and XPS analysis revealed that nitrogen-containing functional groups (C-N=C) interacted strongly with the metal ions and that NO 3 - participated in coordination during adsorption. In addition, the use of different desorption agents in different stages can successfully achieve the desorption and separation of Ln, Am, Pd, Rh, and Ru. Finally, a process for the separation of PGMs from simulated HLLW based on iso Bu-BTP/SiO 2 -P was proposed. 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Ning , W. Zhang , S. Yu et al ., Selective Separation of MA(III) from Ln(III) by Highly Stable Silica-Polymer-based N-Donor IsoBu-BTP/SiO2-P Adsorbent , Solvent Extr Ion Exc , 1 - 14 ( 2019 ). https://doi.org/10.1080/07366299.2019.1625998 https://doi.org/10.1080/07366299.2019.1625998 Selective Separation of MA(III) from Ln(III) by Highly Stable Silica-Polymer-based N-Donor IsoBu-BTP/SiO2-P Adsorbent 10.1007/s41365-020-0744-6 This work was supported by the National Natural Science Foundation of China (Nos. 11705032, 11675102 and 11975082), the Natural Science Foundation of Guangxi Province (No. 2017GXNSFBA198175), and the Science and Technology Major Project of Guangxi Province (No. AA17204100). 2020-01-03 2020-02-04 2020-02-10 2020-03-17 2020-04-01 2021-04-10 © China Science Publishing & Media Ltd. (Science Press), Shanghai Institute of Applied Physics, the Chinese Academy of Sciences, ChineseNuclear Society and Springer Nature Singapore Pte Ltd. 2020 This is a post-peer-review, pre-copyedit version of an article published in Nuclear Science and Techniques. The final authenticated version is available online at: http://dx.doi.org/10.1007/s41365-020-0744-6 http://dx.doi.org/10.1007/s41365-020-0744-6 . 2020 Notation isoBu-BTP/SiO2-P 2,6-di(5,6-diisobutyl-1,2,4-triazine-3-yl)pyridine PGMs Platinum groups metals HLLW High-level liquid waste C Equilibrium ions concentration m Mass of the adsorbent V Volume of the aqueous phase k 2 Pseudo-second-order constant K L Langmuir isotherm model constant K F Freundlich isotherm model constant T Temperature C e Equilibrium ions concentration q m Calculated saturation adsorption capacity E Adsorption efficiency K d Distribution coefficient SF Separation factor t Contact time Q e Equilibrium adsorption capacity Q t Adsorption capacity at time t k 1 Pseudo-first-order constant n Adsorption intensity ∆ G ° Gibbs free energy ∆ H ° Enthalpy ∆ S ° Entropy Q d Desorption amount C d Concentration of adsorbed metal ions in the eluent E d Desorption efficiency Nuclear Science and Techniques 4 31