Scholarly article on topic 'Ion exchange recovery of palladium (II) from nitrate weak acidic solutions'

Ion exchange recovery of palladium (II) from nitrate weak acidic solutions Academic research paper on "Chemical sciences"

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Academic research paper on topic "Ion exchange recovery of palladium (II) from nitrate weak acidic solutions"

Vol.1, No.3, 166-175 (2009)

doi:10.4236/ns.2009.13021

Natural Science

Ion exchange recovery of palladium (II) from nitrate weak acidic solutions

Olga N. Kononova1*, Nataliya G. Goryaeva1, Olga V. Dychko1

'Department of Chemistry, Siberian Federal University, Krasnoyarsk, Russian Federation; cm2@bk.ru Received 12 August 2009; revised 2 September 2009; accepted 4 September 2009.

ABSTRACT

Sorption recovery of palladium (II) from nitrate weak acidic model solutions and solutions of spent catalysts on some ion exchangers with different physical and chemical structure has been investigated. The palladium concentration in contacting solutions was 5.0 ■ 10-5 - 1.0 ■ 10-3 mol/L at nitric acid and potassium nitrate concentrations 0.01 and 1.0 mol/L, respectively. It was shown that anion exchangers AV-17-8 as well as Purolite S 985 and A 500 possess the best sorption and kinetic properties. These sorbents can be recommended for selective recovery of palladium from solutions of spent catalysts.

Keywords: Palladium; Ion Exchange; Anion Exchangers; Nitrate Solutions

1. INTRODUCTION

As natural deposits of precious metals are being depleted, the technologies for precious metals recovery from different secondary raw materials are becoming more important. The hydrometallurgical methods are successfully used for these purposes [1-3]. One of the most promising methods for recovery of platinum group metals (in particular, of palladium) is sorption, characterized by high efficiency and selectivity [1,3-5]. However, the majority of investigations devoted to the sorption recovery of palladium, deal with chloride or sulfate solutions [6-14], and the studies of sorption of noble metals from nitric acidic media are rather limited [1,15-20]. At the same time, the recovery of palladium from some kinds of secondary sources (e.g. electronic scrap and exhausted nuclear fuel) requires its isolation from nitric acidic and nitrate solutions [1,21].

Our previous investigations were focused on sorption recovery of palladium from chloride model solutions and solutions of spent catalysts by various ion exchangers and carbon adsorbents [9,22,23]. Apart from

this, we started the research of sorption concentration of palladium on carbon adsorbents during its recovery from model nitric acidic solutions [24]. We have revealed high sorption abilities of some carbon adsorbents to palladium (II) ions depending on initial concentrations of nitric acid and Pd (II).

The present paper is focused on sorption recovery of palladium from nitrate weak acidic solutions (model and of spent catalysts) by some ion exchangers with different physical and chemical structure.

2. MATERIALS AND METHODS

2.1. Characteristics of Ion Echangers

Some ion exchangers from various manufacturers were taken for investigation. These sorbents possess different physical and chemical structure. Their physical-chemical characteristics are summarized in Table 1. It should be noted that ion exchangers produced by Purolite Company for the first time were used for recovery of platinum group metals. However, these ion exchangers were successfully applied in our previous investigations on sorption recovery of gold and silver [25].

Before sorption all the ion exchangers were prepared according to the standard procedures and then loaded with 1 M NaCl solution, in order to convert them to chloride form (anion exchangers) or to Na+, Cl~ -form (amphoteric resin).

The acid-base properties of ion exchangers investigated were studied by a potentiometric titration with the glass electrode. Based on the experimental data obtained, we have calculated the average apparent ionization constants of functional groups of ion exchangers [5]. The calculation procedure is described below and the values of constants are presented in Table 1.

2.2. Preparation of Palladium Ntrate Solutions

The initial model stock solution of palladium was prepared according to works [26,27]. The accurately

Table 1. Physical-chemical properties of ion exchangers investigated.

Trade name Exchanger type Copoly-mer Physical structure Functional groups Exchange capacity to Cl-ion (mmol/g) Swelling grade (%) PKa Manufacturer

Purolite A 500 Strong base anion exchanger St - DVB MP QAB 1.2 15 2.31 Purolite, UK

Purolite A 530 Strong base anion exchanger St - DVB MP QAB 0.60 12 1.15 Purolite, UK

Purolite S 985 Weak base anion exchanger Ac - DVB MP PA 2.3 42 0.74 Purolite, UK

AV-17-8 Strong base anion exchanger St - DVB G QAB 3.6 23 0.99 TOKEM, Russia

AN-25 1 Weak base anion exchanger VP - DVB MP TAG, PN 5.3 10 1.78 Chercassy, Ukraine

ANKF-5 Amphoteric ion exchanger VP - DVB P PAG, TAG, PN 3.8 (2.6 to Na+) 22 1.42 ( PK =1 1.83) Chercassy, Ukraine

St-styrene; DVB-divinylbenzene; Ac-acryl; VP-vinylpyridine; MP-macroporous; G-gel; P-porous; QAB-quaternary ammonium base; PA-polyamine; TAG-tertiary aminogroups; PAG-phosphorylic acid groups; PN-pyridine nitrogen.

weighed metallic palladium (0.50 g) was dissolved under heating in concentrated HNO3 (analytical grade) according to the following reaction:

3Pd + 8HNO3 ^ 3Pd(NO3 )2 + 2NO t +4H2O (1)

The palladium concentration in initial stock solution was 0.01 mol/L. The working solutions with palladium concentrations 5.0 • 10-5 - 1.0 • 10-3 mol/L were prepared from the stock solution. The nitric acid concentration in these solutions was 0.01 mol/L and the constant ionic strengths was made by means of 1.0 M KNO3. Before the preparation of working solutions, the palladium concentration in initial stock solution was controlled by gravimetric method with dimethylglyoxime as a reagent [26]. The palladium (II) concentration in working solutions and in solutions after sorption was determined by spectrophotometrical with nitroso-R-salt [27,28].

We chose the range of palladium and nitric acid concentrations for our experiment, aiming to make it closer to real industrial conditions.

Apart from the model nitrate solutions of palladium, we also used the solutions of spent palladium-containing catalysts. These solutions were prepared as follows: the catalyst quantities (0.20 g) were dissolved under heating in concentrated nitric acid, similar to preparation of model solution. The working solutions of spent catalysts with palladium concentrations 5.0 10-5-5.0 10-4 mol/L were prepared from the initial solution. Before dissolution of spent catalysts samples in nitric acid, we have determined their average composition by X-ray-fluorescence method. The results are represented in Table 2.

2.3. Batch Studies

The sorption of palladium was studied under batch experimental conditions: resin mass-0.20 g, volume of contacting solution-20.0 mL, stirring in a thermostat at (20 ± 1) °C. The equilibrium time determined by special tests was about 24 h.

Sorption ability of ion exchangers investigated was estimated by means of the recovery degree (R,%) and distribution coefficient ( D, L / g), which were calculated from:

(C - C, )

•100%

where C0 and C q are the initial and equilibrium molar concentrations of palladium solution; EC is the exchange capacity of the resin for palladium, mmol/g.

The kinetics of sorption of palladium from weak acidic nitrate solutions on ion exchangers investigated was studied by the "limited bath" method [29,30] and diffusion coefficients of Pd(II) ( Ds,cm2/s ) were calculated. The kinetic experiment procedure is described below.

The desorption of palladium was carried out by 1 M thiourea solution in 0.01 M HNO3 or in 1 M NaOH . The mechanism of palladium sorption recovery by ion exchangers from nitrate systems was studied by means of IR-spectroscopy and diffuse reflectance spectroscopy. The preparation procedures of samples are present be low.

Table 2. Average composition of initial sample of palladium-containing spent catalyst.

Component Content (%)

Palladium 0.79

Sodium 0.41

Aluminum oxide ~ 84

Silicon 0.03

Sulfur 0.12

Chlorine 0.80

Iron 0.19

Nickel < 0.02

Zinc < 0.02

Gallium < 0.02

All the results were statistically processed by standard methods [31,32]. The average experimental error for 3-4 parallel runs was below 6 %.

2.4. Calculation of Apparent Constants of Acid-Base Ionization of Ion Exchangers

The constants values were calculated using potentiomet-ric titration data. For each point of the titration curve, the functional groups content was determined and the apparent ionization degree (a ) of the resin was calculated:

[H + ]

where [H+ ] is the equilibrium concentration of H+ ions in the ion exchanger phase, mmol/mL; C0 is the initial concentration of the titrant solution (0.1 M

Then a curve was plotted on the coordinates

pH = f (log-) and at a = 0.5 , the apparent

acid-base ionization constants of functional groups of the ion exchangers (pKa) were calculated from Henderson's equation:

PKa = PH - m log(--)

where m is the slope angle tangent of the curve.

2.5. "Limited Bath" Method for Sorption Kinetics of Palladium (Ii)

The quantities of preswollen resin (0.10 g) were stirred with 25.0 mL of palladium nitrate solutions at (20 ± 1)°C over a period of 30 s to 24 h. The suspensions were in-

tensively stirred (more than 800 rev/min). After a certain time period, the resins and solutions were quickly separated and the concentration of Pd(II) was determined in the solutions. Then the exchange degree (F) was calculated from

where Qt and Qœ are the amounts (in mmol) of the palladium sorbed to the time t (s) and to the equilibrium time.

According to the Boyd's method [29,30,33], the kinetic coefficient B was calculated from

(1.08)2 • F2

The data obtained were plotted as a function Bt = f (t). If the process is controlled by gel diffusion [29,30,33], this function should be linear. After that, the diffusion coefficients ( Ds ) were calculated according to the equation:

d = BB-2

where r is the radius of the resin grain (cm).

The half-exchange time of the kinetic process (t1/2) was

calculated as follows:

4^2 Ds

2.6. Preparation of Sample for FT-IR-Spectroscopy

IR-spectra of ion exchangers investigated were recorded by means of FT-IR- spectrometer Vector 22 (Bruker). Before that, ion exchanger samples were dried during 4 h at 40°C in convection drier. Then the samples were held in a vacuum-desiccator over freshly calcinated calcium chloride. The specimens were ground in a mechanical mill without air access and after that were pressed with spectrally pure KBr to discs. The quantities of resin samples and potassium bromide were constant (200 mg each of resin and KBr ).

2.7. Preparation of Samples for Diffuse Reflectance Spectroscopy

The diffuse reflectance spectra were recorded by means of spectrometer PULSAR (Russia). The resin quantities (0.20 g) were preliminary saturated with palladium (II) ions with concentration 5.0- 10-4 mol/L during 24 h. After that, the resins were filtered and wet samples were placed into cell. Then the diffuse reflectance spectra

were recorded.

3. RESULTS AND DISCUSSIONS

3.1. Ionic State of Palladium in Contacting Solutions

It is known from [26,27,34,35] that the ionic state of platinum group metals in solutions depends on acidity of contacting solution as well as on concentration of chloride or nitrate ions (for chloride and nitrate systems, respectively). It is determined at present that Pd(NO3)2 • (H 2O)2 is formed after the dissolution of metallic palladium in concentrated nitric acid according to reaction (1) and subsequent diluting of the solution obtained [36,37]. It is also determined [38] that the hydrated palladium (II) ions [Pd(H2O)4]2+ and their mononitrate complexes [ PdNO3]+ are present in solution at Cimo^ > 1 mol/L.

With the increase in nitric acid con- centration, the amount of different nitrate cationic and anionic complexes as well as of neutral species is growing [19,20]: [Pd(H2OXNO3]+ , [Pd^O^NO^] , [Pd^OXNO,),]- , [ Pd (NO3)4]2-. When the nitric acid concentration diminishes from 1 mol/L to 0.01 - 0.001 mol/L, the formation of hydroxocomplexes with the general formula [ Pd (OH )n is observed in solution [36,38]. That

occurs due to the so-called "aging" of solutions, which takes place in weak acidic media, and especially after keeping of such solutions for longer than 24 h. This phenomenon is typical for solutions of platinum group metals [27,34,38]. At CHNO^ < 0.001mol/L, the solution

does not contain aquatic Pd(II) ions and its nitrate complexes, and only hydroxocomplexes of different composition exist in this media [38].

The above discussion concerns only the Pd(II) -HNO3 systems, i.e. without adding background electrolytes. Our previous investigation [24] was focused on palladium (II) recovery from strong acidic solutions (CHNO3 was 1, 2 and 5 mol/L) in the system sorbent

- Pd(II) - HNO3. However, the sorption of palladium from weak acidic solutions in the presence of salt background is also of practical interest, since such media are formed in number of technological schemes [1,3]. Therefore, we have also studied the following system: ion exchanger - Pd(II) - 0.01 M HNO3 - 1 M KNO3. It should be noted that data on ionic state of palladium in such systems are not available at present and this problem requires a special study. However, we have attempted to make some conclusions on this matter in the present paper, as discussed below.

Before studying the palladium sorption recovery, we have obtained electron absorption spectra of freshly

prepared palladium solutions in 1 M HNO3 and at pH=2, presented in Figure 1. It should be noted that palladium sorption was carried out from freshly prepared solutions to minimize their "aging". It can be seen from Figure 1 that absorption maximum in spectrum 1 ( Pd in 1 M HNO3 ) is located at 390 nm and indicates the presence of complexes [Pd(H2O)(NO3)3]- as a prevailing form [36-38]. However, the absorption maxima in spectra 2 and 3 ( Pd in 0.01 M HNO3 in the presence of 1 M KNO3) are also located at 390 nm and show presence of the same Pd ( II ) complexes in solution. Probably, the formation of anionic nitrate complexes of palla dium (II) is promoted by the high concentration of nitrate ions, despite the weak acidity of solution (pH=2). Later, during our experiments on Pd (II ) sorption, we have not observed any precipitation of metal specimens on a surface of resins, unlike authors [20]. It means that there was no hydrolysis in the investigated systems under chosen conditions (fresh prepared weak acidic solutions and presence of 1 M KNO3 ). However, the precipitation effect was clearly observed when palladium sorption was carried out from solutions kept more than 8 h or from freshly prepared solutions with pH=4. This proves the formation of different hydroxocomplexes. Therefore, we can conclude from the absorption spectra that complexes [ Pd ( H 2O)

( NO3)3]- prevail in contacting freshly prepared solutions under the chosen conditions.

3.2. Sorption Recovery of Palladium from Model Nitrate Solutions

The sorption properties of ion exchangers investigated to palladium (II) are presented in Table 3. It can be seen from these data that in general all the resins reveal high sorption ability, since they recover Pd on the level ~70

300 310 320 330 340 350 360 370 330 390 400 410 420 430 440 450 460 470 480 490 500

Figure 1. Absorption spectra of palladium (II) working solutions in 1 M HNO3 (1) and in the system 0.01 M KNO3 + 1.0 M

KNO3 (2,3), C0(Pd) = 2.0 X10-3 mol/L (1,2) and 1.0x10-3 mol/L (3).

% (ANKF-5) and more than 90 % (Purolite S 985). The studied sorbents can be arranged by their affinity grade to palladium in the following order: Purolite S 985 > Purolite A 530 > Purolite A 500 ~ AV-17-8 > AN-251 > ANKF-5.

It is interesting to note, that all ion exchangers except Purolite S 985 possess approximately equal affinity to Pd , despite of their different physical and chemical structure. The nature of functional groups of the ion exchangers investigated allows to form the following types of chemical bonds during their contact with noble metal ions [5,6,19,20]:

• ionic, i.e. ion - ion interaction, which takes place on strong basic anion exchangers;

• coordination, forming as a result of conservation of electron pair between ligand (electron-pair donor), which is the nitrogen atom of resin functional groups, and the metal (electron-pair acceptor); this bond takes place on weak basic anion exchangers.

The fact that amphoteric ion exchanger ANKF-5 recovers Pd (II) ions from nitrate solutions on the same level (and even less) than anion exchanger AN-251 (both resins were synthesized on the basis of vinylpyridine), unambiguously points out to ionic state of Pd (II) in contacting solution. If cationic hydroxocomplexes or hydrated ions [Pd (H 2O)4]2+ were present in this solution, the degree of palladium (II) recovery would probably be above 69% due to the activity of phosphorylic acid and pyridine nitrogen functional groups in weak acidic media.

Moreover, it is noteworthy that strong basic anion exchangers recover Pd(II) to a greater extent (Table 3), although the additional complex formation of palladium ions with functional groups of quaternary ammonium base is impossible (unlike the weak basic anion exchangers). Therefore, we consider highly probable that anionic palladium complexes [Pd(H2O)(NO3)3]- or

[Pd (NO3)4]2- exist in the systems investigated in the presence of 1 M KNO3.

Table 3. Sorption of palladium from nitrate model solutions on ion exchangers investigated Initial Pd(II) concentration is 5.0 • 10-4 mol/L, pH = 2.

Trade name log D R(%) Trade name log D R(%)

Purolite A 500 2.79 86 AV-17-8 2.77 85

Purolite A 530 2.87 88 AN-251 2.54 78

Purolite S 985 3.23 94 ANKF-5 2.34 69

As for sorption recovery of palladium (II) on anion exchanger Purolite S 985, which reaches 94%, there is little doubt that this recovery proceeds according not only to anion exchange, but also to complexation process, taking into account the presence of polyamine groups in the structure of this sorbent.

3.3. FT-IR Study of Palladium Sorption

To study the palladium recovery from nitrate solutions in more detail, we have carried out IR-spectroscopic investigation. We have obtained IR-spectra of anion exchangers Purolite S 985, AV-17-8 and AN-251, the fragments of which are shown in Figure 2. IR-spectra of initial samples of these resins in chloride form are presented for comparison.

It can be seen from IR-spectra that appearance of intensive peaks in the range of 1400-1300 cm-1 (1384, 1352 and 1300 cm-1) is observed for all the ion exchangers, independently of their basicity and structure of polymeric matrix. These peaks are assigned to vibrations of N-O bonds of nitrate ion: peak at 1384 cm-1 corresponds with stretching vibrations of free NO3- [20,39], whereas peaks at 1352 and 1300 cm-1 can be assigned to the N-O stretching vibrations in palladium complex [39]. It should be noted that the greatest intensity of these peaks is revealed in IR-spectrum of strong basic anion exchanger AV-17-8 (Figure 2, spectrum 5). It was mentioned above that the functional groups of this resin (quaternary ammonium base) cannot react with palladium through additional coordination. Therefore, it can be concluded that the anion exchange takes place in this case:

RCl + [Pd(H2O)(NO3 )3]- » R[Pd(H2O)(NO3 )3] +Cl-

Since the similar but less intensive peaks are revealed in IR-spectra of weak basic anion exchangers Purolite S 985 and AN-251 (Figure 2, spectra 1 and 3), it can be concluded that the reaction (10) is to some extent attributable to these resins too.

However, in case of Pd(II) recovery on weak basic anion exchanger AN-251, the redistribution of the intensities in the range of 1700 - 1400 cm-1, corresponding to symmetric and asymmetric stretching vibrations of pyridine ring, is observed in IR-spectrum of this resin (Figure 2, spectrum 3). The absorption bands at 1600, 1558, 1494 and 1417 cm-1 are assigned to C = C and C = N stretching in pyridine ring [20,39,40]. The reduction of peak intensity at 1510 cm-1 and depression of that one at 1492 cm-1 points out to the probable complexation between palladium and pyridine nitrogen [5,40].

Figure 2. IR-spectra fragments of anion exchanger samples Purolite S 985 (1), AN-251 (3), AV-17-8 (5) saturated from nitrate solutions of palladium (II) C0(Pd) = 5.0x 10-4 mol/ L;

C0(HNO3) = 0.01 mol/L; C0(KNO3)=1.0 mol/L

Spectra (2), (4) and (6) correspond respectively to initial samples of Purolite S 985, AN-251 and AV-17-8 in chloride form.

850 820 790 760 730 700 670

Figure 3. IR-spectra fragments of samples of anion exchanger Purolite S 985 saturated from nitrate palladium (II) solution (1) and of initial resin in chloride form (2) C0(Pd) = 5.0x10-4 mol/L;

C0(HNO3) = 0.01 mol/L; C0(KNO3) = 1.0 mol/L.

The IR-spectrum of weak basic anion exchanger Purolite S 985 saturated with palladium shows the greatest changes compared to the spectrum of its initial sample in

chloride form (Figure 2, spectra 1 and 2). The peaks at 1384, 1352 and 1304 cm-1, which correspond to nitrate ion and are characteristic for anion exchange in accordance with reaction (10), also appear in the spectrum 1. In the range of stretching vibrations of aminogroups (1550 - 1530 cm-1), the reduction of peak intensities takes place, and in the range of 1450-1420 cm-1, the peak disappears, corresponding to vibrations of methylene groups [5,40]. Such changes indicate that complexa-tion processes in the sorbent's phase take place [5].

In case of Purolite S 985, special attention should be paid to the short-wavelength fragments of IR-spectra, shown in Figure 3. It contains an increase in peak intensity at 771 cm-1 and appearance of bands at 822 and 711 cm-1. These changes correspond to deformation vibrations of N ^ Pd bond, which is characteristic for coordination compounds [5,40,41].

Therefore, it can be concluded that palladium sorption from nitrate weak acidic solutions on weak basic anion exchangers proceeds not only according to anion exchange mechanism (reaction (10)), but also is accompanied by coordination:

RN + [PdLn ] » [RNPdLn-l ] + L

where L = H2O;NO3-;n = 2-4.

3.4. Sorption Isotherm Studies

The isotherms of palladium sorption from nitrate solutions on anion exchangers Purolite S 985, A 500 and A 530 are represented in Figure 4. It is known [29,33] that the shape of these curves is an evidence of sorption selectivity. It can be seen from Figure 4 that all the isotherms are convex curves and they are classified to Langmuir isotherms, which are described as follows:

K • C EC = EC--¿^2-

1 + K q • Ceq

where ECm is the maximal equilibrium exchange capacity of the resin to palladium, mmol/g; Keq is the

apparent constant of ion exchange equilibrium, L/mmol.

By transforming the Eq. (12) to the linear form, we calculated ion exchange equilibrium constants and determination coefficients (r2), which are presented in Table 4. It can be seen from these data that coefficients r2 are close to 1. This fact supports our hypothesis about Langmuir-type isotherms for palladium sorption.

3.5. Kinetics Studies

The successful application of ion exchangers in industrial conditions requires their good kinetic properties. That is why the research on kinetics of Pd (II) sorption on Purolite ion exchangers in the investigated systems is both of theoretical and practical interest. The

30 -, 25 -20 15 10 5 0

EC-10 mmol/g

CPHT0" , mol/L

0 10 20 30 40 50

70 80 90 100

Figure 4. Isotherms of palladium sorption on anion exchangers Purolite A 530 (1), A 500 (2) and S 985 (3) C0(HNO3) = 0.01 mol/L; C0(KNO3) = 1.0 mol/L.

Table 4. Apparent constants of ion exchange equilibrium ( Keq ) and determination coefficients (r2) during recovery of palladium (II) from nitrate model solutions.

Trade name r2

Purolite A 500 135 0.894

Purolite A 530 34.4 0.991

Purolite S 985 588 0.975

0,6 0,5 0,4 0,3 0,2 0,1 0

1000 2000 3000 4000 5000 6000 7000

Figure 5. Kinetic dependencies of Bt function on time t for anion exchangers Purolite A 530 (1), S 985 (2) and A 500 (3).

Table 5. Kinetic parameters of palladium (II) sorption from nitrate model solutions C0(Pd) = 5.0x10-4 mol/L; C0(HNO3) = 0.01 mol/L; Co(KN03) = 1.0 mol/L.

Trade name ü-106 (mmol/g-s) Ds -10s (cm2/s) t1/2 (s)

Purolite A 500 11.70 8.26 1558

Purolite A 530 2.06 0.58 23164

Purolite S 985 9.26 5.94 2390

calculated main kinetic parameters are summarized in Table 5 and Figure 5 contains the dependencies

Bt = f (t).

It can be seen from Figure 5 that dependencies Bt = f (t) are the straight lines for all the resins Purolite investigated and comply with criterion of gel kinetics, i.e. the whole sorption process is controlled by interdiffusion of the ions exchanged in a resin grain [29,30,33]. As for the main kinetic parameters, it should be noted that average rate of ion exchange process is higher on strong basic anion exchanger Purolite A 500 (Table 5). Consequently, the value of average diffusion coefficient for this resin exceeds such values for the other sorbents and the half-exchange time is lesser. A comparison of kinetic process between anion exchangers Purolite S 985 and A 500 shows that such behavior of these sorbents is in good consistence with our above-mentioned assumptions about sorption mechanism. Since the palladium sorption on Purolite A 500 is not complicated by additional complexation (in contrast to Purolite S 985), the rate of this process is higher and diffusion coefficient values are also bigger, whereas the half-exchange times are lesser for this resin. However, it is interesting to note that the strong basic anion exchanger Purolite A 530, which is not practically distinguished from A 500 in its sorption properties (Table 3), compares much unfavorably with A 500 in its kinetic properties (Table 5). The average rate of ion exchange process on Purolite A 530 is about 5 times lower than on Purolite A 500. Also the average diffusion coefficient values for A 530 are by one order smaller and the half-exchange time is by one order greater (Table 5). Such behavior of anion exchanger Purolite A 530 in comparison with also strong basic resin A 500 can be probably explained by its exchange capacity, which is less by half than this value for A 500, and by its lesser swelling as well (Table 1). Moreover, it can be assumed that the sorbed complex ions of palladium (II), which possess a square spatial configuration [42], have not enough time to reach the active centers of the sorbent A 530, where the anion exchange occurs, because of its small exchange capacity (there are few available exchange centers on a resin surface). Certainly this phenomenon requires a special study, but from the practical point of view the anion exchanger Purolite A 500 is preferable than sorbent Purolite A 530 for recovery of palladium (II) from nitrate solutions.

3.6. Sorption of Palladium from Nitrate Solutions of Spent Catalysts

Further we have studied the sorption recovery of palladium (II) from solutions of spent catalysts on some anion exchangers chosen on the basis of their good sorption and kinetic properties. The results are summarized in Table 6.

It can be seen from these data that the anion exchangers in general possess good sorption ability to Pd (II) ions, but this characteristic is slightly lower in compari-

son with the data obtained for model solutions, excluding anion exchanger AV-17-8 (Table 3). Partly the decrease in Pd (II) recovery from real solutions can be explained by complex composition of initial solution of spent catalyst (Table 2), where a number of ions produce a competing effect on palladium sorption process.

In order to determine the form of palladium in contacting solution of spent catalyst as well as in the phase of strong basic anion exchanger, we have obtained the diffuse reflectance spectra presented in Figure 6. It can be seen from these data that the maximum in diffuse reflectance spectra is located at 410 nm. It corresponds with the maximum in absorption spectrum at 390 nm (Figure 1), since the bathochromic shift of maximum in diffuse reflectance spectra is observed during sorption concentration of noble metal ions in view of matrix effect of solid phase [43,44]. Therefore, the prevailing form of Pd (II) existence in nitrate weak acidic solutions of spent catalysts is its complex [Pd(H2O) (NO3X]-

It is known [2-5,15] that the desorption of noble metals from highly selective ion exchangers is hardly achievable process because of strong retention of adsorbed metal ions by functional groups of resins. Due to that, for the successful regeneration of these sor-bents it is necessary to use the elution agents which form more stable complexes with the recovered metal ions than the complexes of these metals existing in the resin phase. From this point of view, the acidic or basic thiourea solutions are widely applied as eluting agent [1,15,19,22-24,27]. We have also used in the present work the thiourea solutions for palladium desorption after its sorption recovery. The results are shown in Table 7. It can be seen from the presented data that the palladium (II) elution degrees after its recovery from model solutions reach the level of 78-82% - the result which is considered quite satisfactory. However, the palladium desorption after its recovery from solutions of spent catalysts proceeds on the level of 22-25%. When carrying out this process, we have changed thiourea concentration and used its solutions in HNO3 or NaOH , but the best result we could reach was ~ 25% by palladium elution with 1 M thiourea solution in 1 M NaOH . It should be noted that the recovery of noble metals from industrial solutions after their sorption on highly selective ion exchangers is often carried out by burning of such resins, since the value of noble metals exceeds the costs of ion exchange materials, even selective ones [2,4,24,45]. Therefore, it is necessary to continue the research for improving the palladium recovery after its sorption on selective ion exchangers from solutions of spent cata--lysts.

Figure 6. Diffuse reflectance spectra of anion exchangers' samples AV-17-8 (1) and Purolite A 500 (2) saturated with palladium (II) from nitrate solutions of spent catalysts. C0(Pd) = 5. 0x10-4 mol/L; C0(HNO3) = 0.01 mol/L; C0 (KNO3 ) = 1.0 mol/L F(R) - diffuse reflectance coefficient.

Table 6. Sorption recovery of palladium (II) from nitrate solutions of spent catalysts C0(Pd) = 5. 0 C0(HNO3 ) = 0.01 mol/L; C0(KN03) = 1.0 mol/L.

Trade name log D R(%)

Purolite A 500 2.31 65

Purolite S 985 2.86 88

AV-17-8 2.72 84

Table 7. Elution of palladium from anion exchangers investigated by thiourea solution (1.0 mol/L) in 0.01 M HNO3 after palladium sorption from nitrate weak acidic model solutions.

Trade name Desorption degree (%)

Purolite S 985 78

Purolite A 500 82

4. CONCLUSIONS

Sorption recovery of palladium (II) from nitrate weak acidic model solutions and solutions of spent catalysts on some ion exchangers with different physical and chemical structure was investigated. Based on electron absorption spectra, it was determined that complexes [Pd(H2O)(NO3)3]- prevail in contacting solutions. It

was shown that ion exchangers investigated possess good sorption and kinetic properties.

The mechanism of palladium sorption recovery on strong and weak basic anion exchangers from nitrate weak acidic solution was outlined by means of FT-IR-spectroscopy. It was shown that strong basic anion exchangers sorb palladium according to anion exchange, whereas weak basic resins recover Pd(II)

complexes not only by anion exchange, but also by means of additional coordination with nitrogen atoms of functional groups.

The palladium (II) desorption after its recovery on selective ion exchangers from model solutions and solutions of spent catalysts was carried out using thiourea solutions. It was shown that the degree of palladium elution by 1 M thiourea solution in 0.01 M HNO3 after its sorption from model solutions is on the level of 78 -82 %, whereas this value does not exceed 25% after Pd (II) sorption from solutions of spent catalysts. The improvement of this process should be a subject for further research.

Based on results of present investigation, the anion exchangers AV-17-8 as well as Purolite S 985 and A 500 can be recommended for selective recovery of palladium (II) from nitrate weak acidic solutions.

5. ACKNOWLEDGEMENT

The authors would like to express profound gratitude to the team of Moscow office of Purolite International Ltd, who kindly provided us with ion exchanger samples.

REFERENCES

[1] R. Pfrepper, (1988) Möglichkeiten Der Wiedergewinnung Von Pd Aus Sekundären Rohstoffquellen. ZFI-Mitteilungen. Akademie-Verlag, Berlin, 3-292.

[2] I. F. Khudyakov, A. P. Doroshkevich, S. V. Karelov, (1990) Metallurgy of the secondary non-ferrous heavy metals. Nauka, Moscow, 15-25.

[3] M. A. Meretukov and A. M. Orlov, (1990) Metallurgy of noble metals. Metallurgiya, Moscow, 27-30.

[4] A. G. Kholmogorov, (1986) Ion exchange in hydro-metallurgical processing of palladium-containing spent catalysts. Sibir, Krasnoyarsk, 150-151.

[5] K. M. Saldadze and V. D. Kopylova-Valova, (1980) Complex-forming ion exchangers. Nauka, Moscow, 3- 336.

[6] S. A. Simanova, A. S. Tevlina, and I. S. Bazhanova,

(1994) Formation of palladium complexes during sorption on high permeable sorbents with heterocyclic nitrogen atoms. J. Inorg. Chem., Moscow, 39(1), 121-126.

[7] I. A. Kovalev, G. I. Tsyzin, and A. A. Formanovskiy,

(1995) Concentration of rhodium, palladium and platinum on sorbent with ethylenetriamine groups. J. Inorg. Chem., Moscow, 40(5), 828-833.

[8] I. A. Tarkovskaya, L. P. Tikhonova, and N. V. Kulik, (1997) Sorption of platinum group metals from aqueous solutions on inorganic and synthetic ion exchange materials. Khimiya I Tekhnologiya Vody, 19(3), 227-239.

[9] A. G. Kholmogorov, O. N. Kononova, S. V. Kachin, and S. V. Razvodovskaya, (1998) Sorption of palladium from chloride solutions on anion exchangers with macro-re-ticular and porous structure. J. Phys. Chem., Moscow, 72(2), 318-321.

[10] O. P. Shvoeva, V. P. Dedkova, and S. B. Savvin, (2004) Effect of masking compounds on color reactions of diSciRes Copyright © 2009

thizone with Pd (II), Hg (II) and Ag (I) after sorption from chloride solutions on fibrous anion exchanger. J. Anal. Chem., Moscow, 59(7), 704-709.

[11] V. P. Dedkova, O. P. Shvoeva, and S. B. Savvin, (2005) Test-method for determination of palladium in chloride solutions in solid phase of fibrous ion exchanger. J. Anal. Chem., Moscow, 60(1), 85-89.

[12] Z. Hubicki and M. Leszczynska, (2005) Sorption of palladium (II) chloride complexes on weakly, intermediate and strongly basic anion exchangers. Desalination, 175, 227-236.

[13] Z. Hubicki and A. Wolowicz, (2009) Adsorption of palladium (II) from chloride solutions on Amberlyst A 29 and Amberlyst A 21 resins. Hydrometallurgy, 96, 159165.

[14] Z. Hubicki and A. Wolowicz, (2009) A comparative study of chelating and cationic ion exchange resins for removal of palladium (II) complexes from acidic chloride media. J. Hazard. Mater., 164, 1414-1419.

[15] V. V. Milyutin, S. V. Peskishev, and V. M. Gelis, (1994) Sorption of palladium, ruthenium and rhodium from nitric acidic solutions on different sorbents. Radiokhimiya, 36(1), 25-28.

[16] G. R. Anpilogova and E. V. Kondratieva, (1996) Study of palladium (II) sorption on polyethylene-monosulfide from nitric acidic solutions. J. Inorg. Chem., Moscow 41(3), 447-452.

[17] V. I. Skorokhodov, O. Y. Goryaeva, B. K. Radionov, (2004) Choice of optimal structure of ion exchangers for palladium sorption from nitric acidic solutions. Tsven-naya Metallurgiya, 1, 31-33.

[18] Z. Hubicki, M. Leszczynska, B. Lodyga, and and A. Lo-dyga, (2007) Recovery of palladium (II) from chloride and chloride-nitrate solutions using ion exchange resins with S-donor atoms. Desalination, 207, 80-86.

[19] K. A. Venkatesan, B. R. Selvan, M. P. Antony, T. G. Srinivasan, and P. R. V. Rao, (2007) Extraction of palladium (II) from nitric acid medium by imidazolium nitrate immobilized resin. Hydrometallurgy, 86, 221-229.

[20] R. Kumaresan, K. N. Sabharval, T. G. Srinivasan, P. R. V. Rao, and G. Dhekane, (2008) Studies on the sorption of palladium using cross-linked poly(4-vinylpyridine- divi-nylbenzene) resins in nitric acid medium. Solv. Extr. Ion Exchange, 26, 643-671.

[21] A. V. Belyaev, (2003) Chemical-technological problems of platinum group metals during processing of exhausted nuclear fuel. Zhurnal Strukturnoy Khimii, 44(1), 39-47.

[22] O. N. Kononova, A. G. Kholmogorov, and E. V. Mikhlina, (1998) Palladium sorption on vinylpyridine ion exchangers from chloride solutions obtained from spent catalysts. Hydrometallurgy, 48, 65-72.

[23] O. N. Kononova, N. G. Goryaeva, N. B. Dostovalova, S. V. Kachin, and A. G. Kholmogorov, (2007) Recovery of palladium from acidic solutions using carbon adsorbents. Khimiya Tverdogo Topliva. 4, 71-75.

[24] O. N. Kononova, A. N. Lukianov, M. V. Derevyashkin, A. G. Kholmogorov, S. V. Kachin, and N. G. Goryaeva, (2008) Sorption of palladium on carbon adsorbents from nitric acid solutions. J. Porous Mater. 15, 61-66.

[25] O. N. Kononova, K. A. Shatnykh, K. V. Prikhodiko, D. M. Kashirin, and A. G. Kholmogorov, (2009) Sorption of gold (I) and silver (I) from thiosulfate solutions on anion

exchangers. Tsvetnye Metally, 1, 40-43.

[26] F. E. Beamish, (1966) The analytical chemistry of the noble metals. Pergamon Press, Oxford, London, Edinburgh, New York, Toronto, Paris, Frankfurt, 41-45.

[27] S. I. Ginzburg, N. A. Ezerskaya, I. V. Prokofieva, N. V. Fedorenko, Y. I. Shlenskaya, and N. K. Belskiy, (1972) Analytical chemistry of platinum group metals. Nauka, Moscow, 165-166.

[28] F. Umland, A. Janssen, D. Thierig, and G. Wünsch, (1971) Theorie und praktische Anwendung von Komplexbildnern. Akademische Verlagsgesellschaft, Frankfurt am Main, 364-365.

[29] F. Helfferich, (1962) Ion exchange. McGraw-Hill, New York, 335-360.

[30] F. Helfferich and J. A. Marinsky, (1966) Ion exchange kinetics. (ed.) Ion exchange. A series of advances. McGraw-Hill, Buffalo, New York, 281-331.

[31] D. C. Harris, (1996) Quantitative chemical analysis. Freeman and Company, New York, 374-376.

[32] J. H. Pollard, (1977) A handbook of numerical and statistical techniques. Cambridge University Press, Cambridge, 342-345.

[33] Y. A. Kokotov, (1990) Ion exchangers and ion exchange. Khimiya, Leningrad, 47-52.

[34] Y. A. Zolotov, G. M. Varshal, and V. M. Ivanov, (2003) Analytical chemistry of platinum group metals. Editorial URSS, Moscow, 16-88.

[35] S. E. Livingstone, (1967) The chemistry of ruthenium, rhodium, palladium, osmium, iridium and platinum. Per-gamon Press, Oxford, New York, Toronto, Sydney, Paris, Braunschweig, 178-211.

[36] R. A. Shoytsov, (1972) Spectrophotometrical investigation of palladium (2+) state in aqueous solutions. State University, Moscow, Moscow, PhD-thesis.

[37] V. S. Shmidt, N. A. Shorokhov, A. A. Vashman, and V. E. Samsonov, (1982) Study of complex Pd(NO3)2 ■ (H2O)2. J. Inorg. Chem., Moscow, 27(5), 1254-1256.

[38] P. I. Antyukhin, (1993) About correlation between solubility constants of metal hydroxides and formation constants of their neutral hydroxocomplexes. Sibirskiy Khimicheskiy Zhurnal, 1, 21-25.

[39] L. Bellami, (1963) Infrared spectra of complex molecules. Inostrannaya Literatura, Moscow, 383-590.

[40] V. A. Uglyanskaya, G. A. Chikin, V. F. Selemenev, and G. A. Zavialova, (1989) Infrared spectroscopy of ion exchange materials. Izdatelstvo VGU, Voronezh, 150-207.

[41] K. Nakamoto, (1986) Infrared and raman spectra of inorganic and coordination compounds. Wiley, New York, 360-536.

[42] F. A. Cotton and G. Wilkinson, (1969) Advanced inorganic chemistry. A Comprehensive Text, Mir, Moscow, 460-469.

[43] P. Kubelka, and F. Munk, (1931) Ein Beitrag Zur Optik Der Farbanstriche. Z. Techn. Phys., 12, 593 -601.

[44] G. D. Brykina, D. Y. Marchenko, and O. A. Shpigun, (1995) Solid-phase spectrophotometry. J. Anal. Chem., Moscow, 50(5), 484-491.

[45] V. V. Barchenkov, (1982) Sorption technology of recovery of gold and silver from ores. Nauka, Moscow, 155-286.