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Brazilian Journal of Chemical Engineering

Print version ISSN 0104-6632

Braz. J. Chem. Eng. vol.29 no.2 São Paulo Apr./June 2012

http://dx.doi.org/10.1590/S0104-66322012000200018 

SEPARATION PROCESSES

 

Determination of the maximum retention of cobalt by ion exchange in h-zeolites

 

 

A. S. ZolaI; M. A. S. D. BarrosI; E. F. Sousa-AguiarII; P. A. ArroyoI,*

IChemical Engineering Department, State University of Maringá, Phone: + (55) (44) 30114758, Fax: + (55) (44) 30114792, Av. Colombo 5790, 87020-900, Maringá - PR, Brazil. E-mail: arroyo@deq.uem.br
IIPETROBRAS/CENPES/PDEDS/ER, Av. Jequitibá 950, 21941-589, Rio de Janeiro - RJ, Brazil

 

 


ABSTRACT

This work aimed to determine the maximum content of cobalt that can be incorporated by ion exchange in zeolites H-USY, H-Beta, H-Mordenite, and H-ZSM-5. To reach this goal, batch isotherms at 75ºC were constructed after addition of zeolite samples in flasks filled with cobalt nitrate solution. The equilibrium data were fitted to Langmuir, Freundlich, and Tóth adsorption isotherm models. Langmuir was the best model for zeolites H-Beta, H-Mordenite, and H-ZSM-5, whereas experimental data for H-USY were better fitted to the Freundlich isotherm model. From the isotherms, it was possible to determine the maximum cobalt exchange level (qmax) that can be incorporated in each zeolite through ion exchange. In this sense, H-USY presented the highest qmax value (2.40 meq/gzeol), while H-ZSM-5 showed the lowest one (0.64 meq/gzeol). These results also show the influence of the zeolite framework related to the channel system, pore opening, presence of cavities and secondary porosity and SiO2/Al2O3 ratio (SAR) on the maximum capacity and behavior of cobalt ion exchange in protonic zeolites.

Keywords: Cobalt; Ion exchange; Isotherms; qmax; Protonic zeolite.


 

 

INTRODUCTION

Co-zeolites have been shown to catalyze a wide range of organic reactions, including some environmentally friendly processes. Many studies have reported Co-zeolites obtained specifically from acid zeolites. This is probably due to the fact that, in this case, zeolites presented a better catalytic activity when compared to the directly exchanged cobalt zeolites (Gutierrez et al., 2007; Pedrosa et al., 2006; Chupin et al., 2006; Mies et al., 2007; Lónyi et al., 2007; Li and Armor, 1999, Zola et al, 2007). The most investigated Co-zeolites used in organic reactions are Co-ZSM-5 (Chupin et al., 2006), Co-Beta (Mies et al., 2007), Co-Mordenite (Lónyi et al., 2007) and Co-USY (Li and Armor, 1999). One example is the Fischer-Tropsch Synthesis (FTS) to hydrogenate CO (Zola et al., 2007). The small Co metal particle confined in the zeolite framework is one of the most important parameters, as well as the shape selectivity of the zeolite and the presence of acid sites. These three parameters may easily influence the selectivity and activity of CO hydrogenation (Guczi and Kiricsi, 1999, Zola et al., 2007).

According to Tang et al. (2004) and Wang et al. (2005), introduction of cobalt ions into zeolites by ion exchange, followed by reduction with sodium hydroxide, is the most convenient method for synthesis of metal nanoparticles encapsulated in zeolites. In this way, the ion exchange method can provide cobalt cations in the pores or cages of a zeolite (Tang et al., 2004). The smaller cobalt nanoparticles encapsulated inside these pores or cages can exhibit high CO conversion in the Fischer-Tropsch Synthesis (Wang et al., 2005).

Usually estimation of the maximum cobalt loading is based on the SiO2/Al2O3 ratio (SAR), which represents the theoretical cation exchange capacity (CEC) of the zeolite framework. However, it does not provide the real cation exchange capacity because there are inaccessible or hindered cationic sites in the zeolite structure. Thus, it becomes important to study cobalt ion exchange, before catalyst preparation, in order to determine the real maximum content of cation that can be incorporated into the zeolite by ion exchange. This procedure allows choosing the appropriate zeolitic support or the cobalt content that can be incorporated into different zeolites.

Since previous research has focused on catalysis itself and location and state of Co (Khodakov et al., 2007; Park et al., 2004; Mhamdi et al., 2009; Dědečk and Wichterlová, 1999; Dědečk et al., 2000; Dědečk et al., 2002) using mainly spectroscopic techniques, the ion exchange isotherms have hardly been studied (Guczi and Kiricsi, 1999). Therefore, this work aimed to determine the maximum content of cobalt ions that can be incorporated into the protonic zeolites Beta, Mordenite, USY and ZSM-5 by ion exchange. To accomplish this goal, the first step was to obtain the experimental equilibrium data at 75ºC. These data were adjusted to the isotherm models of Langmuir, Freundlich and Tóth. The best isotherm model then allowed the estimation of the maximum retention capacity (qmax). These values reflect the influence of the zeolite structure and SAR on the cobalt loading and the ion exchange behavior under equilibrium conditions.

 

EXPERIMENTAL

Zeolite Pre-Treatment

The commercial samples of zeolites Na-ZSM-5, Na-Mordenite, H-Beta, and H-USY were generously donated by CENPES/PETROBRAS - Brazil. The SiO2/Al2O3 molar ratios (SAR), theoretical cation exchange capacities (CEC) and textural properties are presented in Table 1.

Before cobalt ion exchange, the zeolites ZSM-5 and Mordenite were converted to their protonic form. Hence, Na-ZSM-5 was pre-treated by contacting the powdered material with an aqueous solution of 2 mol/L NH4Cl (NH4+/Al3+ = 7) at 70ºC/1 h, under stirring. During the filtration process, the zeolite was submitted to a new exchange procedure by the addition of ammonium solution on the filtration cake. The solid was exhaustively washed with deionized water, dried overnight, and calcined at 500ºC/3 h, in order to obtain the H-ZSM-5 sample. The H-Mordenite sample was prepared by an aqueous ion-exchange method involving continuous addition of 0.5 mol/L HCl to Na-Mordenite (H+/Na+ = 2.0) on a filtration cake at room temperature. The resultant ion-exchanged zeolite was washed thoroughly with an excess of deionized water and then dried at 120ºC overnight.

Samples of H-Beta and H-USY were used as received.

Determination of the Equilibrium Time

Determination of the equilibrium time involved the addition of 50 mg of each H-Zeolite to different glass tubes containing 20 mL of Co(NO3)2.6H2O aqueous solution (20 mg Co/L) in a bath maintained at 75ºC under constant stirring. Each tube was removed after different exchange times and the samples were filtered using a quantitative paper. The cobalt concentration in the filtrate was determined by atomic absorption spectrometry using a Varian SpectrAA 50B equipment under suitable conditions (λ = 240.7 nm and air/acetylene flame). The cobalt standards employed were prepared from stock solutions (Carlo Erba) and the samples were analyzed after incorporation using the necessary dilutions.

Isotherm Construction

After establishing the equilibrium time, the batch isotherms were obtained for each zeolite studied. Tests were carried out by the addition of the zeolite mass (0.01 up to 1.50 g) to glass tubes already filled with 20 mL of the cobalt solution. The system was maintained at 75ºC under constant stirring. When the equilibrium time was attained, samples were filtered and the cobalt concentration in the liquid phase was analyzed by atomic absorption spectrometry as described above.

Several authors have used adsorption models to describe experimental data for ion exchange in zeolites and other materials (Misak, 1995; Malekian et al., 2010; Ostroski et al., 2009; Al-Anber and Al-Anber, 2008, Silva et al., 2003, Torab-Mostaedi et al., 2010, Senthil Kumar et al., 2010, Mousavi et al., 2010). In applying such models, one should bear in mind that the ion exchange process is the most important sorption mechanism although the subsequent adsorption phenomena should not be neglected.

The software ORIGIN 7.5® was used to adjust the experimental equilibrium data to the isotherm models described below:

1) Freundlich isotherm

where: q is the amount adsorbed at equilibrium per amount of adsorbent (meq/g);

C is the equilibrium concentration (meq/L) of the adsorbate in the solution;

K' (L/g) and 1/n (dimensionless) are constants depending on several experimental factors associated with the active site distribution and the adsorbent capacity (Suzuki, 1990; Maheria and Chudasama, 2006).

2) Langmuir isotherm

where: C and q have the same meaning as described for the Freundlich isotherm;

b is a constant that represents the adsorption bond energy (L/meq);

qmax is a constant that represent the maximum adsorption capacity (meq/g), corresponding to a monolayer covering the surface of the adsorbent (Maheria and Chudasama, 2006; Pereira et al., 2006).

Although the assumptions of the Langmuir model are related to the adsorption process, the mathematical equation has been prominently used in ion exchange process (Helferich, 1962). Indeed, successful mathematical approaches have been used (Misak, 1995), even for zeolites (Helferich, 1962).

Rengaraj and Moon (2002) proposed that the essential characteristics of the Langmuir isotherm could be expressed in terms of a dimensionless constant or equilibrium parameter (RL), which is defined as:

where: b is the Langmuir constant (L/meq);

Co is the initial concentration of cobalt (meq/L).

3) Tóth isotherm

where: qm is the maximum adsorption capacity (meq/g);

C has the same meaning as described for the Freundlich isotherm;

Km is the equilibrium constant;

m is the model constant.

 

RESULTS AND DISCUSSION

The concentration of cobalt in solution as a function of ion exchange time is shown in Figure 1. As can be observed, the ion exchange equilibrium is reached at about 36 h of ion exchange for all H-Zeolites studied. However, to ensure that the ion exchange equilibrium was actually reached, a three-day period was adopted for the ion exchange process.

 

 

The equilibrium results, as well as the model adjustments, are presented in Figure 2.

All fitted models for the H-Zeolite systems presented favorable shape (McCabe et al., 2001). According to the classification system for adsorption isotherms proposed by Giles et al. (1960), all experimental data are of the S type, indicating the horizontal orientation of cobalt molecules on the zeolitic surface. These observed shapes could be related to the octahedral geometry of Co2+ ions (Dědečk and Wichterlová, 1999; Dědečk et al., 2000; Dědečk et al., 2002). The accommodation of Co2+ ions seems to form layers until the isotherm plateau, when it becomes more stable. Such a plateau is not well defined due to the rapid adsorption process in multilayers. The adsorption layers would be formed starting from the moment that, due to the electrostatics attraction of the zeolite with Co2+ ions, there is a new accommodation, and the in-going cobalt ions are present in vertical form. Then, the multilayer adsorption occurs as the monolayer, reflecting the strongest ion exchange process, becomes more and more crowded. This fact explains the sigmoid shape of the isotherms with inflexion points at different q values corresponding to the difficulty of Co2+ in occupying different sites located in the zeolite channels and cavities. This behavior is more pronounced for the H-USY system, in which some cobalt cations are exchanged into less accessible sites located in sodalite and hexagonal prisms cages (Barros et al., 2003a,b).

Table 2 presents the isotherm parameters for the models investigated here.

It can be verified that the Tóth isotherm showed the highest correlation coefficient values for all zeolites, as expected, since it is a three-parameter model. However, the errors associated with the model parameters were very high, exceeding the value of the parameter itself. Considering such analysis, the Langmuir model was the most representative of the equilibrium data at 75ºC for zeolites H-Beta, H-Mordenite, and H-ZSM-5. On the other hand, the Freundlich model presented the best fit for the H-USY system.

The dimensionless separation factor (RL) values, obtained from the Langmuir isotherm parameters (Eq. (3)), were 0.016, 0.013, and 0.018 for H-Beta, H-Mordenite, and H-ZSM-5, respectively. According to Rangaraj and Moon (2002), values between 0 and 1 confirm the favorable cobalt uptake, which is in agreement with the experimental equilibrium data already shown.

The Freundlich isotherm describes reversible adsorption and is not restricted to the formation of a monolayer, as might indicate the Langmuir model. Further, the Freundlich model predicts that the cobalt concentration in the zeolite will increase steadily with increasing cobalt concentration in the liquid phase (Hameed et al., 2007). As the Freundlich model was the most representative for the H-USY system, it suggests that initially there is a cobalt exchange with H+ ions in the accessible supercages and then an increase of ion exchange with parent ions located in the sodalite units and some less accessible hexagonal prisms at higher external cobalt concentrations (Kim and Keane, 2000). These ion exchange conditions lead to a favorable behavior that is represented by an exponent n higher than 1 for zeolite H-USY (Rengaraj and Moon, 2002).

From the best-fit isotherm models, it was possible to determine the qmax values, i.e., the maximum amount of cobalt that can be exchanged per gram of H-Zeolite (except USY). The values obtained for each zeolite and the maximum content of cobalt that can be theoretically incorporated by ion exchange are presented in Table 3.

It can be observed in Table 3 that H-ZSM-5 presents the smallest amount of cobalt incorporated. In fact, it is the only zeolite studied that presents medium micropores and a bi-dimensional channel system, whose openings are 5.1 x 5.7 and 5.4 x 5.6 Å (Gianneto-Pace et al., 2000), while the other zeolites possess large micropores. As the H-ZSM-5 pore opening is small, the entrance of the cobalt cation, which has a hydrated radius of 4.23 Å, is hindered. Furthermore, it should be taken into account that low valence cations are preferred by zeolites of higher SAR (Townsend, 1991). Zeolite H-ZSM-5 has a higher SAR of 39.9, corresponding to a CEC of 0.783 meq/gzeol, which is much smaller than those of the other zeolites. Therefore, this feature could lead to a lower preference and retention capacity of H-ZSM-5 for Co2+ cations, which is in agreement with the values presented in Table 3.

The zeolite H-USY presented the highest cobalt content that can be incorporated by ion exchange. It is probably due to the three-dimensional pore system, the higher CEC of 3.63 meq/gzeol (smallest SAR among the zeolites studied), and the pore opening of 7.4 Ǻ, that permits a quite free access into supercages α of 12.4 Ǻ diameter (Gianneto-Pace et al., 2000). Additionally, it is also possible that the dealumination of zeolite Y, in the process of obtaining zeolite USY, generates a secondary porosity that allows a better access to the exchange sites located in the channels and large cavities of this structure. It justifies the smaller resistance to diffusion inside the crystals experienced by the hydrated cobalt cations present in the ion exchange solution.

Moreover, it is also possible to verify in Table 3 that the maximum capacity of cobalt incorporation into H-Mordenite is a little higher than those observed for H-Beta (4.08 wt.% and 2.93 wt.% of Co, respectively). Zeolites H-Beta and H-Mordenite have three-dimensional and pseudo-one-dimensional pore systems (elliptic rings with 12 oxygen atoms), respectively. Thus, an opposite tendency would be expected for the qmax values. However, it should be considered that H-Mordenite has a pore opening of 7.1 x 6.7 Ǻ, in contrast to the smaller openings of approximately 7.3 x 6.0 Ǻ and 5.6 x 5.6 Ǻ for zeolite H-Beta (Gianneto-Pace et al., 2000). This fact itself would not be enough to explain such a difference. Besides, H-Mordenite presents a lower SAR (13.0) and consequently a higher CEC (2.22 meq/gzeol). Thus, a higher Co2+ retention in H-Mordenite is justified. These results evidence the influence of the zeolite structure on the ion exchange process. The channel system, the pore opening and the presence of cavities and secondary porosity may affect the maximum capacity of Co2+ retention and exchange behavior. Moreover, SAR plays an important role in determining the maximum amount of cation that can be incorporated in the zeolites by ion exchange.

Therefore, it is possible to incorporate Co contents from 1.9 wt.% in H-ZSM-5 up to approximately 6.5 wt.% in H-USY. The high incorporation of cobalt in H-USY makes us conclude that this zeolite is a potential support for cobalt catalysts prepared by the ion exchange method.

 

CONCLUSIONS

The cobalt isotherms obtained at 75ºC are favorable, showing the good affinity of the H-Zeolites for Co2+ cations. The equilibrium data for Co2+ ion exchange are best fitted with Langmuir isotherm model for H-Beta, H-Mordenite, and H-ZSM-5, while the Freundlich isotherm model fit the experimental data better for H-USY. The maximum cobalt contents that can be incorporated (qmax) by ion exchange are 1.06, 1.43, 2.40 and 0.64 meq Co/gzeol for H-Beta, H-Mordenite, H-USY, and H-ZSM-5, respectively, which clearly shows the influence of the zeolite structure and composition on the ion exchange process. Therefore, the maximum amount of Co cation that can be incorporated into the zeolite structure and the ion exchange behavior are strongly influenced by the SiO2/Al2O3 ratio (SAR), the channel system, the pore opening, and the presence of cavities and secondary porosity. The results obtained here also demonstrate that is necessary to determine experimentally the proper maximum value of cation exchange capacity for each zeolite system, since theoretical ion exchange capacities do not usually allow incorporation of the desired cobalt content into the zeolite support. Considering all these factors the zeolite USY presents the highest potential as an appropriate support for Co catalysts prepared by the ion exchange method.

 

ACKNOWLEDGEMENT

The authors thank to the CNPq/Brazil and PROCAD/CAPES/Brazil for financial support.

 

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(Submitted: September 15, 2010 ; Revised: September 8, 2011 ; Accepted: September 27, 2011)

 

 

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