Electrochemical behavior of Pd(II) and Rh(III) in [EMIm]NTf₂ ionic liquid

Electrochemical behavior of Pd(II) and Rh(III) in [EMIm]NTf 2 ionic liquid 1 first-author 1 1 corresp Corresponding author, yzwei@sjtu.edu.cn Corresponding author, yzwei@sjtu.edu.cn yzwei@sjtu.edu.cn 2 School of Nuclear Science and Engineering, Shanghai 200240, China School of Nuclear Science and Engineering, Shanghai 200240, China Department of Chemical & Biological Engineering, University of British Columbia, 2360 East Mall, Vancouver, Brithish Columbia, V6T 1Z3, Canada Department of Chemical & Biological Engineering, University of British Columbia, 2360 East Mall, Vancouver, Brithish Columbia, V6T 1Z3, Canada The electrochemical behavior of Pd(II) and Rh(III) in [EMIm]NTf 2 ionic liquid has been studied on Pt working electrodes at 298 K by cyclic voltammetry (CV), polarization curve and galvanostatic transient techniques. Cyclic voltammogram of Pd(II) in [EMIm]NTf 2 consists of two cathodic current peaks located at 1.37 V( E pc 2 ), corresponding to Pd 2+ /Pd + , and at 0.69 V ( E pc 1 ) corresponding to Pd + /Pd. The transfer coefficient α was calculated by the Tafel extrapolation from the polarization curves to be 0.306, which is in agreement with the value reported in an aqueous solution system. For Rh(III) in [EMIm]NTf 2 , a cathodic current peak ( E pc ) was observed at -0.39 V, corresponding to Rh 3+ /Rh, and two oxidation peaks were observed at -0.13 V ( E pa 1 ) and 0.37 V ( E pa 2 ) during the reverse scan. A significantly negative shift in the cathodic peak potential was observed with the increase of the scan rate, indicating that the reduction of Pd(II) and Rh(III) on the Pt electrode involves kinetic complications. By using the galvanostatic transient technique, the diffusion coefficients of Pd(II) and Rh(III) in [EMIm]NTf 2 ionic liquid solution were found to be ∼10 -7 cm 2 /s. The potential difference between the reduction of Pd(II) to Pd and the reduction of Rh(III) to Rh obtained from the CV curves of the Pd(II) and Rh(III) co-existing [EMIm]NTf 2 solution is found to be about 0.74 V, which makes it possible to electrodeposit Pd(II) and Rh(III) separately. Ionic liquids Cyclic voltammogram Palladium Rhodium I. INTRODUCTION 1 Palladium and Rhodium are noble metals. Both of them play important roles in many industrial applications due to their unique physical and chemical properties, such as high catalytic activity [ 1 1 - 4 4 1-4 ]. To date, there has been a huge demand for rhodium, palladium, and their compounds in various industrial application areas. The abundance of rhodium and palladium in the Earth’s crust are very low and only found in few countries. Therefore it is necessary to look for alternative sources of rhodium and palladium that is abundant and easily accessible. Meanwhile, spent fuels are composed of significant quantities of platinum group metals (PGMs). Most of the fission palladium and rhodium istopes in the spent fuel are non-radioactive or very weakly radioactive [ 5 5 , 6 6 ]. According to the report, by the year 2030 about 2500–3000 t of fission PGMs will be produced and only 7000 tonne of natural reserves will be left [ 5 5 ]. PGMs are rejected as waste during reprocessing of spent fuel by the PUREX process. In addition, PGMs increase the melting point of waste glass formed and tend to separate at a distinct phase during vitrification leading to a non-homogeneous glass matrix. Direct electrodeposition of palladium from nitric acid [ 7 7 ] and hydrochloric acid [ 8 8 , 9 9 ] have been studie d before. However, it is not easy to obtain palladium films without hydrogen embrittlement by electrodeposition from a conventional aqueous plating bath since palladium has high catalytic activity towards hydrogen evolution and absorbs a great amount of hydrogen. Lately, room-temperature ionic liquids (RTILs) have drawn great attention and been studied in many fields [ 10 10 , 1 1 , 12 12 ]. RTILs have unique characteristics such as negligible vapor pressure, high chemical and thermal stability, acceptable intrinsic ionic conductivity, and a wide potential window. To avoid the influence of moisture in the air, a hydrophobic ionic liquid, [EMIm] NTf 2 , was chosen for the study of the electrochemical behavior of Rh(III) and Pd(II). II. EXPERIMENTAL SECTION 1 A. Materials and methods 2 [EMIm]NTf 2 was bought from the Lanzhou Institute of Chemical Physics, Chinese Academy of Sciences, and purified by recrystallization and vacuum drying at 353 K for 48 hours prior to use. Pd(NO 3 ) 2 (Sinopharm Chemical Reagent Co., Ltd. analytical pure, purity 99%) and RhCl 3 (J & K Scientific Ltd, analytical pure, purity 98%) were dissolved in [EMIm]NTf 2 in a container maintained at 353 K. The solution obtained after the complete dissolution was transferred into an electrochemical cell, which was maintained at 298 K in a water bath. The electrochemical experiments were carried out in a conventional three-electrode system. The working electrode was a platinum foil (apparent surface area = 1 cm 2 ). A platinum wire electrode was used as the counter electrode. A reference electrode consisted of a sliver wire immersed in 10 mmol/L AgCF 3 SO 3 /[EMIm]NTf 2 separated from the bulk solution by a porous glass. The potential of this reference electrode was measured by redox of ferrocene (Fc). Prior to each experiment, surface pretreatment of the working and counter electrodes were performed by hand polishing the electrode surface with 1.0, 0.3, 0.05 micro Gamma-Alpha alumina powder in a sequence to a mirror finish followed by immersing the electrode in 3 M HCl, acetone, methanol, and distilled water in an ultrasonic cleaner for 20 minutes, respectively, to remove any surface impurity. The electrolyte was deaereated by N 2 prior to each experiment. B. Electrochemical measurements and software 2 All of the electrochemical measurements were conducted using an electrochemical workstation, CorrTestTM model CS1350, equipped with electrochemical testing and analysis tools, Version 4.3 software. III. RESULTS AND DISCUSSION 1 A. CV behavior of Fc + /Fc in [EMIm]NTf 2 2 Cyclic voltammogram of Fc + /Fc in [EMIm]NTf 2 obtained at the scan rate of 10 mV/s with the potential scan range from 1.10 V to 0.50 V is shown in Fig. 1 Fig. 1 . The electrolyte solution consisted of 2 mL of [EMIm]NTf 2 and 10 mmol/L Fc. The potential scan started from the OCP (Open Circuit Potential) to more positive potentials up to 1.10 V and then was reversed to 0.50 V. During the scan in the cathodic direction, the cathodic current density increased at a potential more negative than 0.90 V. The reduction peak was observed at ca. 0.74 V and after that the current starts to decrease due to the decreased Fc + concentration on the surface. During the reverse scan, the anodic peak was recognized at ca. 0.82 V, which is related to the oxidation of Fc to Fc + . It is clear that the Fc + /Fc is a simple single-step one-electron-transfer reaction. The fact that the ratio of i pc / i pa approaches 1 and E pc - E pa = 0.08 V in Fig. 1 Fig. 1 imply that the reaction of Fc + /Fc in [EMIm]NTf 2 is a reversible reaction. The formula E f = ( E pa + E pc )/2 allows for the calculation of the formal potential ( E f ) of the process in Fig. 1 Fig. 1 , which is calculated to be (0.82 + 0.74)/2 = 0.78 V. Taking the fact that the Fc + /Fc couple E ° = 0.40 V vs. NHE into consideration we can calculate the potential of the reference electrode is -0.38 V vs. NHE. All electrode potentials reported in this work are referred to the potential of the reference electrode. B. Electrochemical behavior of Pd(II) or Rh(III) in [EMIm]NTf 2 2 Figure 2 Figure 2 shows the CV plot of platinum electrodes in the [EMIm]NTf 2 ionic liquids solution containing 5 mM PdCl 2 at the scan rate of 15 mV/s with the potential scan starting at 2.10 V to 0.12 V. A cathodic current peak ( E pc 2 ) was observed at ca. 1.37 V and the other cathodic current peak ( E pc 1 ) was observed at 0.69 V which can be explained by Eqs. (1), (2) and (3). During the reverse scan two oxidation peaks are observed at 1.33 V ( E pa 1 ) and 1.72 V ( E pa 2 ). The reduction of Pd(II) in an aqueous solution was reported to be a two-step electron transfer process [ 13 13 , 14 14 ], as described by the Eqs. (1) and (2). The slower step (Eq. (1)) may lead to the accumulation of Pd(I) at the electrode surface when the potential is negative enough for Pd(II)/Pd(I) but not negative enough for the Pd(I)/Pd couple, resulting in a decrease of the current. This can explain the appearance of the peak (a) when E pc 2 = 1.37 V. With further decrease of the potential, the absolute value of the current becomes much larger. The peak current at 0.69 V is likely attributed to the three electrode processes, as described by the Eqs. (1), (2), and (3). Namely, E pc 2 and E pa 2 are attributed to the redox process of the Pd(II)/Pd(I) couple, while E pc 1 and E pa 1 correspond to the redox process of the Pd(I)/Pd couple. The difference between E pc 2 and E pa 2 is calculated to be -0.35 V and the difference between E pc 1 and E pa 1 is -0.64 V, which indicate that the redox processes of the Pd(II)/Pd(I) and Pd(I)/Pd couples are both irreversible on the Pt electrode in [EMIm]NTf 2 . <math display="block" id="M1"><mrow><mi>P</mi><msup><mi>d</mi><mrow><mn>2</mn><mo>+</mo></mrow></msup><mo>+</mo><msup><mi>e</mi><mo>−</mo></msup><mo>→</mo><mi>P</mi><msup><mi>d</mi><mo>+</mo></msup><mtext> </mtext><mtext> </mtext><mtext>slow</mtext></mrow></math> <math display="block" id="M2"><mrow><mi>P</mi><msup><mi>d</mi><mo>+</mo></msup><mo>+</mo><msup><mi>e</mi><mo>−</mo></msup><mo>→</mo><mi>P</mi><mi>d</mi><mtext> </mtext><mtext> </mtext><mtext>fast</mtext></mrow></math> <math display="block" id="M3"><mrow><mi>P</mi><msup><mi>d</mi><mrow><mn>2</mn><mo>+</mo></mrow></msup><mo>+</mo><mn>2</mn><msup><mi>e</mi><mo>−</mo></msup><mo>→</mo><mi>P</mi><mi>d</mi></mrow></math> A comparison of cyclic voltammograms of Pd(II) in [EMIm]NTf 2 at different scan rates is shown in Fig. 3 Fig. 3 . The cathodic peak current increases and the cathodic peak potential ( E pc 1 and E pc 2 ) shifts negatively with the increase of scan rate. This indicates that the reduction of Pd(II) at the Pt electrode is irreversible, which is in agreement with the conclusion derived from the CV plot obtained at 15 mV/s. Figure 4 Figure 4 shows the polarization curves and the derived Tafel plots of the platinum electrode in the [EMIm]NTf 2 solution, containing 5 mM Pd(NO 3 ) 2 at the scan rate of 10 mV/s. At the initial cathodic potentials there is a linear relationship between the lg I and E , corresponding to the charge transfer limitation. As seen in Fig. 3 Fig. 3 , the equilibrium potential is located in the area of the one-electron transfer process, and thus the electron number transferred in this potential range is n = 1. According to the Tafel extrapolation method [ 15 15 ], the exchange current density, i o , is estimated to be 8.51×10 -8 mA/cm 2 and the charge transfer coefficient, α = 0.306, which is a little smaller but comparable to the value reported in an aqueous solution [ 16 16 ]. Figure 5 Figure 5 shows the CV plot of the platinum electrode in [EMIm]NTf 2 ionic liquid solution containing 5 mM RhCl 3 at the scan rate of 15 mV/s with the potential scan starting from 0.90 V to -0.70 V. A cathodic current peak ( E pc ) was observed at -0.39 V, which is due to the reduction of Rh(III). During the reverse scan two oxidation peaks were observed at -0.13 V ( E pa 1 ) and 0.37 V ( E pa 2 ). These indicate that Rh(III) in [EMIm]NTf 2 ionic liquid undergoes an irreversible single step three electron transfer at the Pt electrode. The value (i.e., ca. 175 mV) of | E pc - E pc /2 | is much larger than that (i.e., 18.8 mV at 298 K) required [ 17 17 ] for a reversible process indicating that the reduction of Rh(III) in [EMIm] NTf 2 at the Pt electrode is not only controlled by diffusion, but also charge transfer kinetics. A comparison of cyclic voltammograms of Rh(III) in [EMIm]NTf 2 at different scan rates is shown in Fig. 6 Fig. 6 . The cathodic peak current increases and the cathodic peak potential E pc shifts negatively with the increase in the scan rate, also indicating that the reduction of Rh(III) at the Pt electrode is irreversible. Figures 7 Figures 7 and 8 8 show the chronopotentiograms of the Pt electrode in 5 mM Pd(II)/Rh(III) in [EMIm]NTf 2 ionic liquid solution recorded at different applied current densities. The plateau potential shifts negatively as the current density increases, which is a particular behavior of the irreversible electrode reaction. By measuring the transition time, τ, of each chronopotentiogram, we can calculate the diffusion coefficient of Pd(II)/Rh(III) in [EMIm] NTf 2 ionic liquid solution according to the sand equation: <math display="block" id="M4"><mrow><mfrac><mrow><msup><mi>I</mi><mrow><mn>1</mn><mo>/</mo><mn>2</mn></mrow></msup></mrow><mrow><msub><mi>C</mi><mtext>o</mtext></msub></mrow></mfrac><mo>=</mo><mfrac><mrow><mi>n</mi><mi>F</mi></mrow><mn>2</mn></mfrac><msqrt><mrow><mi>π</mi><mi>D</mi></mrow></msqrt><mn>,</mn></mrow></math> where I is the current density, C o the bulk concentration of Pd(II) or Rh(III), n the number of electrons, and F is the Faraday constant. The diffusion coefficient of Pd(II) is calculated as 1.71×10 -7 cm 2 /s and the diffusion coefficient of Rh(III) is calculated as 1.57×10 -7 cm 2 /s. C. Electrochemical behavior of Pd(II) and Rh(III) in [EMIm]NTf 2 2 As we mentioned above, both Pd(II) and Rh(III) are noble metals produced as fission products. The redox behavior of Pd(II) co-existing with Rh(III) was investigated by CV measurements. Fig. 9 Fig. 9 shows the cyclic voltammogram of 5 mM Pd(II), 5 mM Rh(III), and 10 mM Fc + /Fc couple in [EMIm]NTf 2 recorded at the Pt electrode at 298 K at a scan rate of 15 mV/s with the potential scan starting from 2.00 V to -1 V. A cathodic current peak (marked as a) was observed at E pc 1 = 0.73 V and the other cathodic current peak (marked as c) was observed at E pc 2 = -0.45 V. During the reverse scan only one oxidation peak (marked as d) was observed at 0.81 V ( E pa 1 ). According to Figs. 1 Figs. 1 and 9 9 we can draw a safe conclusion that the peaks a and d are the redox process of the Fc + /Fc couple, which proves the excellent reproducible property of the reference electrode. Fig. 10 Fig. 10 shows the cyclic voltammograms of 5 mM Pd(II) and 5 mM Rh(III) in [EMIm]NTf 2 recorded at the Pt electrode at 298 K with different scan rates. A cathodic current peak A ( E pc 1 ) was observed at ca. 0.25–0.35 V, which is attributed to the reduction of Pd(II). This peak was also observed in Fig. 9 Fig. 9 at peak b, which was overlapped by the current of the Fc + /Fc couple. The other cathodic current, peak B ( E pc 2 ), was observed at ca. -0.30 V which is due to the reduction of Rh(III). During the reverse scan, only one oxidation, peak C, was observed. The potential difference between the peaks A and B is about 0.74 V which makes it possible to electrodeposit Pd(II) and Rh(III) separately in [EMIm]NTf 2 ionic liquid solution. IV. CONCLUSION 1 The electrochemical behavior of Pd(II) and Rh(III) in [EMIm]NTf 2 was studied by cyclic voltammetry, polarization curve, and chronopotentiometry measurements at the Pt electrode at 298 K. Two cathodic peaks were observed for the first time in 5 mM Pd(II)/[EMIm]NTf 2 ionic liquid solution. The peak at 1.37 V ( E pc 2 ) is attributed to the electrode process as described in Eq. (1) and the one at 0.69 V ( E pc 1 ) corresponds to the process shown in Eqs. (1), (2), and (3). Based on this assumption the transfer coefficient, α, was calculated by the Tafel curve to be 0.306, which is in agreement with the value reported in an aqueous solution. A cathodic current peak ( E pc ) was observed at -0.39 V, which is due to the reduction of Rh(III). During the reverse scan two oxidation peaks were observed at -0.13 V ( E pa 1 ) and 0.37 V ( E pa 2 ) in 5 mM Rh(III)/[EMIm]NTf 2 ionic liquids solution. A significant negative shift in the cathodic peak potential was observed with the increase of scan rate, indicating that the reduction of Pd(II) and Rh(III) at the Pt electrode involve kinetic complication. The diffusion coefficient of Pd(II) and Rh(III) in [EMIm]NTf 2 ionic liquid solution were found to be ca. 10 -7 cm 2 /s, which is in accordance with the diffusion coefficient under similar conditions. 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Electrochemical methods-fundamentals of electrochemical analysis 10.13538/j.1001-8042/nst.26.S10307 Supported by the National Natural Science Foundation of China (Nos. 91026019 and 91126006) 2013-05-10 2014-06-12 2014-12-20 2015-02-20 2021-04-11 2015 Nuclear Science and Techniques 1 26