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South African Journal of Chemistry

versão On-line ISSN 1996-840X
versão impressa ISSN 0379-4350

S.Afr.j.chem. (Online) vol.71  Durban  2018 



Fabrication of nitrogen donor macro- and meso-porous materials for group 11 metal ions sorption



Kelebohile Mphanje; Orpah Zinyemba*; James Darkwa

Department of Chemistry, University of Johannesburg, Auckland Park Kingsway Campus, Auckland Park, 2006, South Africa. orcid.org0000-0003-3457-1832




Macro(meso) porous polymer materials were prepared via a modified TIPS method using reagent grade polymers mixtures; polyacrylonitrile (PAN) and polyvinylpyridine-co-styrene (PVPS). Reaction conditions such as concentration, temperature and the solvents used were found to affect the morphology of the polymer materials formed. The use of low heat for polymer dissolution, near critical point polymer concentration and a miscible solvent/non-solvent pair in excess non-solvent were found to produce porous polymers. The macro-(meso-) porous materials were further used in metal adsorption/desorption studies and they were found to remove up to 80 % of Cu(II), Ag(I) and Au(III) from aqueous solution. Adsorption/desorption experiments were performed using the polymer monolith KSP1{(PAN : PVPS = 75 : 25 (w/w) in DMSO : H2O = 90 : 10(v/v)} and it showed excellent reusability adsorbing and desorbing up to 90 % of the metal ions in a series of five cycles. Ternary solutions for adsorption/desorption experiments were added in the order Cu(II), Ag(I) and Au(III).

Keywords: Fabrication, polymer monolith, polyacrylonitrile, polyvinylpyridine-co-styrene, adsorption of group 11 metal ions.



1. Introduction

Metal ions in solutions of industrial effluents, as well as those found in acid mine drainage, pose environmental threat when such solutions find their way into water bodies. In order to prevent these metal ions from contaminating the environment and allowing for their remediation, adsorbents that can effectively bind these metals need to be developed. Potential sources of adsorbents are polymers that have monolithic structures having affinity for different metal ions.1 If successfully fabricated into monolithic structures, such polymer-sorbents are expected to have both high adsorption and desorption rates so as to allow for recycling of both the metal ions absorbed and the polymers. Successful fabrication of such polymer-sorbents would pave the way for investigating the ability of these polymers being employed as reusable materials for wastewater cleaning.

The synthesis of porous materials conventionally involves the use of either organic or inorganic templates, with the intention of controlling their physical and chemical properties. The attractiveness of such porous materials as sorbents has grown immensely within the past few decades owing to their versatility and myriad applications, ranging from biological to industrial.2-1 Non-solvent induced phase separation (NIPS) forms the basis to fabricate required sorption materials, which usually result in mesoporous materials." In fabricating mesoporous materials, Dong et al? and Tan et al.8have established solvent (S) to non-solvent (S/NS) ratios that favour fabrication of monolithic structures that can act as good sorbents.5 This fabrication method leads to materials with a high affinity for metal ions, high surface area and excellent sorbent properties.1

Polymers with donor atoms have been investigated as sorbents for absorbing metal ions for nearly two decades.6 In using polymers that carry donor atoms to fabricate sorbent materials to absorb metal ions, thermally induced phase separation is one of the effective methods to fabricate such polymers.5,6 The Uyama group has used NIPS to fabricate a number of macro- and mesoporous materials from polyvinylacrylonitrile (PAN) that act as ion exchange material.8 Uyama and co-workers employed amidoxated PAN monoliths to clean wastewater. Such material has an added advantage of havingboth macro- and mesoporous pores that result in high flow-throughput property as metal ion exchangers.

In the present study we have used for the first time the Uyama approach to fabricate novel marco-and mesoporous monoliths from polyacrylonitrile (PAN), polyvinyl-4-pyridine (PVP) and polyvinyl-4-pyridine-co-sytrene (PVPS) as sorbent materials and investigated their absorption capacity for group 11 metal ions that are typical base metals found in mining effluents. This paper is a pilot study aimed at eventually determining the effectiveness of the above-mentioned polymer monoliths as recyclable adsorbents for purification of water in the Mpumalanga region. The water quality in the Mpumalanga province of South Africa has been a cause for concern in South Africa for almost two decades.9-10 Acid mine drainage from coal mining is a problem in the Highveld coalfield in Mpumalanga. This problem has received media attention as a result of severe pollution observed in the Loskop Dam as well as the Olifants River catchment where water is contaminated by base metals and other effluents.11,12 This has resulted in depletion of aquatic life, disruption of the food chain, contamination of portable water owing to the heavy metals dissolved in the drinking water and deterioration of eco-systems.10

In this preliminary study, only results from sorption/desorption studies using standard solutions are reported aimed at highlighting the potential these monolithic materials possess in acting as reusable sorbents for group 11 metals. The recovery of precious metals such as gold and silver, even at very low concentrations, is something that can potentially be of economic value. Our future communication is intended to include analysis of real samples hence this communication serves as proof of concept only. We report our preliminary findings in this paper.


2. Experimental

2.1. Chemicals and Reagents

Polyacrylonitrile (PAN) (Mw ~150 000) and polyvinylpyridine-co-styrene (PVPS) (Mw ~220 000) were purchased from Sigma Aldrich (Johannesburg, South Africa) and used as received. Analytical grade dimethyl sulfoxide (DMSO), dimethyl formamide (DMF), 25 % NH4OH, 85 % glacial CH3COOH and methanol were purchased from Rochelle Chemicals (Johannesburg, South Africa). Milli-Q H2O used was purified using 18 W cm-1 millipore system by Merck (Johannesburg, South Africa).

2.2. Instrumentation

Pore sizes in macro- and meso-porous monoliths were determined using a Tuscan Vega3LMH Scanning Electron Microscope (SEM) at 8 kV and working distance ranging from 30-5 mm. Pore size distributions and surface area for the samples were determined by conducting isothermal Brunaer-Emmet-Teller (BET) N2-physisorption using a Micromeritics Tristar 3000. Differential scanning calorimetry (DSC) and thermogravimetric analyses (TGA) experiments were conducted on macro- and meso-porous monoliths to determine whether any of these composite materials had taken any new properties from the parent polymers. This was done using a Mettler Toledo DSC822e and TA Q500 TGA thermal analyzer. Metal uptake by monoliths was determined using an Analitikjena ContrAA 700 Graphite furnace instrument (Germany).

2.3. Preparation of Macro- and Meso-porous Monoliths

In a typical experiment 0.081 g of PAN was dissolved in a 10 mL mixture of (90:10 v/v) of DMSO and Milli-Q water. The mixture was heated at 80 °C until it became a clear homogeneous solution (ca. 6 h). The solution was rapidly cooled on attaining homogeneity in a liquid nitrogen bath, resulting in the formation of a white solid and left in 500 mL of Milli-Q water for 2 h with stirring to aid solvent or non-solvent exchange. This process was repeated three times before the sample was isolated by decanting and the solid material washed with small aliquots (ca. 50 mL) methanol and dried in vacuo, leading to spherical materials as the final product. Table 1 is a summary of polymer and solvent ratios that were used in fabricating polymer monoliths. All experiments were repeated at least three times.



2.3.1. Polyacrylonitrile (PAN)

For PAN 1, 2 and 4, different ratios of DMSO and water were used whilst for PAN 3, DMF was used in place of DMSO in a specific ratio. The KPV monolith was fabricated from a mixture of PAN and poly-4-vinylpyridine (PV4P) in a solvent mixture of DMSO and water. These experiments were repeated at least three times.

2.3.2. Polyacrylonitrile (PAN): Poly-4-vinylpryidine (PV4P)

Polymer composite KPV1 and two monoliths were prepared from PAN (0.065 g) and PV4P (0.016 g) in a similar manner as described for the PAN monoliths, using a 80:20 w/w of PAN and PV4P. Experiments were repeated at least three times.

2.3.3. Polyacrylonitrile (PAN): Poly-4-vinylpyridine-co-styrene (PV4PPS)

Polymer composite monoliths KPS1 and two from PAN and PV4PPS were prepared in a similar manner as described for the PAN monoliths, using a 80:20 w/w of PAN and PV4PPS. Experiments were repeated at least three times.

2.3.4. Determination of Porosity of Polymer Monoliths

In a typical experiment a small amount of granules of the sample were adhered to doubled sided tape and to a glass slide after which the excess sample was shaken off. The sample was then thoroughly coated using an Emscope SC500 gold coating machine. After obtaining sufficient coating on the sample, scanning electron microscope (SEM) analyses were performed by means of a Tuscan Vega3LMH SEM at 8kV and working distances ranging between 30 mm and 5 mm to determine the porosity of the polymer monolith. Typical micrographs are shown in Fig. 1.

2.3.5. Determination of Pore Size Distribution of Polymer Monoliths

Nitrogen sorption measurements were performed by weighing of 0.081g of monolith sample into a sample vial. The samples were degassed at 80 °C for 6 h and introduced into a cryogenic chamber and adsorption/desorption tests conducted at sub-zero temperatures on a Micromeritics Tristar 3000 sorption system. The surface areas were calculated by the Brunauer-Emmett-Teller (BET) method, and the pore size distributions were obtained by the Barret-Joyner-Heled(BJH) method from the desorption branch of the isotherms. A typical pore size distribution is depicted in Fig. 2.

2.3.6. Optimization of Metal Uptake by Polymer Monolith

To achieve maximum uptake of metal ions, the sorption conditions, including concentration, volume, sorption time and pH were optimized. All optimization experiments were repeated at least three time. Influence of Metal Concentration in the Sample

The optimization conditions used were kept constant for the five polymers (PAN2, PAN3, PAN4, KPV1 and KPS1) which were investigated to determine the optimum concentration of metal ion solution that would be required per 100 mg of polymer sample. PAN1, which was the starting point based on the Uyama study6 proved to be difficult to reproduce consistently; hence PAN1 was not used in the sorption experiments. For each polymer material, 100 mg was accurately weighed into poly-tops and four 10 mL solutions of Cu ions were prepared at 1, 3,8 and 13 mg L-1 in each the four separate poly-tops containers in order to investigate the sorption at mg L-1 range. The polymer and solution mixture was left to soak for 1 h, after which the solution was quantitatively extracted and transferred into a 25 mL sample vial. The volume was filled to the mark usinga1%HNO3 acid solution The above procedure was repeated to optimize for the ug L-1 range using five solutions at 12, 25, 50, 100 and 200 ug L-1. Each experiment was repeated at least three times. Influence of Sample Volume

The above achieved optimization conditions were kept constant for the five polymers which were being investigated in order to determine the optimum volume of metal ion solution that would be required to allow the maximum sorption per 100 mg polymer material. 100 mg of polymer materials were accurately weighed in triplicate for each of the five different types of polymers. For a Cu ion solution of a 200 /g L-1, three different volumes of 3, 5.5 and 10 mL were accurately measured and added to each polymer material. These polymer materials were allowed to soak for an hour after which they were quantitatively transferred into a 25 mL sample vial. The volume was subsequently filled to the mark usinga1%HNO3acid solution. The optimum volume was used in subsequent optimization. Influence of Sorption Time

The achieved optimization conditions were kept constant for the five polymer materials which were being investigated in order to determine the optimum time interval that was required for maximum sorption of metal ions by 100 mg of polymer sample. Four 100 mg polymer materials were accurately weighed for each of the five polymer samples prepared. Four aliquots of 5.5 mL Cu(II) ion solution at a concentration of 200 ugL-1 were transferred into the weighed polymer samples. The aliquots were quantitatively transferred into 25 mL sample vials at periods of 1, 3,4 and 5 h. The volume was subsequently filled to the mark usinga1%HNO3 acid solution. The optimum sorption time was used for subsequent optimization. Influence of Sample pH

The polymer materials prepared were investigated for possible use in the reclamation of mine wastewater hence pH optimization was carried out under acidic conditions (pH 1-5) as the pH of mine waste is typically below 5. To determine the optimum pH at which the polymer sample would remove the most metal ions in acidic conditions, the pH of a Cu ion solution of 200 fig L-1 was adjusted to 1, 2, 3, 4 and 5 with NH4OH in an NH/Acetate buffer. An amount of 100 mg of polymer sample was accurately weighed and 5.5 mL aliquots of solution at the above mentioned pH values added. The polymer sample was left to soak for a period of 3 h after which the Cu ion solution was extracted and transferred quantitatively into a 25 mL sample vial. The volume was filled to the mark by1%HNO3 acid solution followed by analysis of the samples. These optimization experiments were repeated at least three times in each case. Optimized Sorption Study Procedure

A 5.5 mL aliquot of the metal ion solution at a pH 4 (adjusted by NH/Acetate buffer) was added to 100 mg of polymer sample and left to soak for a period of 3 h, the solution was quantitatively transferred into a 50 mL sample vial. The volume was filled to the mark usinga1%HNO3 acid that was pH adjusted using the buffer solution. The spectroscopic method chosen for analysis in this case was GF-AAS owing to the low concentration ranges expected in the samples which were in the L-1 range. Adsorption and Desorption Studies

Metal adsorption and desorption experiments were carried out to determine if the monoliths used for initial uptake experiments could be recycled. It is important to note that only ternary solutions were investigated added to the monolith in the sequence Cu(II), Ag(I) and Au(III). Adsorption experiments were performed as described in section with the metal ion dose kept at 200 L-1 in five cycle. The polymer monoliths used in the adsorption experiment were preserved and used for the further adsorption/desorption experiments. The monoliths were rinsed with Milli-Q water to remove physisorbed metal ions on the surface to avoid metal ions carry over from the previous experiment. The metal-loaded monoliths were then immersed in HNO3 at pH ~1 and stirred at 100 rpm for 3 h at ambient temperature. After filtration to recover the polymer, the monoliths were rinsed several times with Milli-Q water. The filtrate plus the rinsing water were made up to 50 mL with 1 % HNO3 in a sample vial and analyzed for metal content. Five consecutive adsorption/desorption experiments were performed. The quantity of metal ions after each adsorption and desorption experiment was determined using GF-AAS and the efficiencies of desorption processes were calculated as follows:

where Qdes and Qads are quantities of metal ions in ug L-1 desorbed and adsorbed, respectively.

Experiments were run in triplicate (n = 3). Only KPS1, the polymer that demonstrated the best metal uptake under our given conditions was used to perform the adsorption/desorption experiments.

2.4. Analysis of Samples

Graphite furnace analyses were conducted using an Analitik-jena ContrAA 700 at the recommended heating programme as set in the 'cookbook' since these conditions did not differ from those obtained after optimization for both pyrolysis and atomization. The analytes were quantified with relative ease and no apparent interferences were observed. The recoveries of the analytes fell within the acceptable range of 80-120 %. Calibrations were performed using working-ranges recommended by the instrument manufacturer. The standard concentrations ranged from 0-100 L-1 for each analyte.


3. Results and Discussion

3.1. Fabrication of Macro- and Mesoporous Monoliths

The monoliths were generally fabricated by dissolving either neat PAN or a mixture of PAN and PV4P or PV4PPS in a solvent mixture made up ofDMSO or DMF and H2O orMeOH. The optimum w/w composition of the polymers in any of the monoliths was established by varying the weight of the PAN in relation to the weight of the other polymer based on the porosity of the final composite material obtained (Fig. 1). In all composite materials, the optimum w/w mixture was found to be 80:20 (Table 1). Furthermore different solvent mixtures also affected the porosity of a monolith. Firstly by comparing DMSO to DMF as solvents that dissolved a polymer and using water as a non-solvent; monoliths prepared with DMSO had better porosity (Fig. S1). Also as a non-solvent, water produced monoliths with better porosity than methanol (Fig. S2). From SEM analyses the monoliths were generally found to be macro- or mesoporous with the majority of the pores lying in the macro-porous range. We also found that temperature and time of heating affected the porosity of all the monoliths, whether they were neat or composite materials. For example, a shorter heating period at constant temperature resulted in materials with better porosity; whilst increasing temperature even at the same heating time produced materials with poorer porosity (Figs. 1 and 2). The nascent outer layer is shown in (A) of Fig. 1. This layer is non-porous and is formed by the initial rapid change of temperature from high to low. (B) and (C) show the pores and structure that resulted as phase separation occurred. Some of this structure is monolithic and this can be explained to be a result of the diffusion gradient as the non-solvent displaces the solvent.

SEM images revealed that polymer samples formed an outer layer (skin), resulting from the sudden change of the environment upon quenching. The bulk of the sample showed an interconnected monolithic structure. Figure 1 shows a typical microstructure of these samples as observed under scanning electron microscopy (SEM). The intrinsic structure that resulted from a homogenous mixture of the polymers being rapidly cooled is depicted in the same figure. The nascent outer layer is shown in (A). This layer is non-porous and is formed by initial rapid change of temperature from high to low. (B) and (C) show the pores and structure that resulted as phase separation occurred. Some of this structure is monolithic and this can be explained to be a result of the diffusion gradient as the nonsolvent displaces the solvent.

In summary, the best fabrication conditions for making the desired macro- and mesoporous monoliths were found to be: (i) solvent: non-solvent ratio of 90:10 DMSO/H2O for either neat or composite material; (ii) temperature of 80 °C and (iii) a maximum heating time of 6 h.

3.2. Quality and Quantitative Pore Size Determination

Initial indications of whether any of the materials fabricated were porous or not was determined by its SEM micrographs. In experiments where the solvent, non-solvent pair used deviated too much from the 88:12 critical concentration recommended by Uyama,5 resulted in glassy non-porous materials (Figs. S3 and S4). This observation is possibly owing to remnants of the solvent that was used to dissolve a polymer not being completely removed when a large amount of a non-solvent is used to wash the monolith. To support this assertion we performed thermal analysis experiments of fabricated monoliths and they invariably contained DMSO (Figs. S5-S7).

Quantitative pore size distributions in all monoliths were determined by BET experiments. Typical BET data for the monolith are depicted in Figs. 3 and S8 and show that these monoliths are composed of mainly macro-pore sizes and only a small amount of meso-pores. The isotherms exhibit type III behaviour according to the IUPAC adsorption isotherms.13 These isotherms have a 'knee' around low relative pressure (P/Po) ranges, which is characteristic of materials with a low or no micropore volume.

This can be seen as the percentage incremental volume of the micropores in these samples which is close to zero and therefore negligible. These isotherms are depicted in Fig. S9.

The obtained average pore size and surface area of the prepared monoliths (PAN2, PAN3, PAN4, KPV1 and KPS1) as determined by BET analyses is approximately 15.89 nm with an average surface area of 18.79 m2g-1. This surface area is considerably smaller than that obtained by the Uyama group for PAN monoliths who obtained an average surface area of 188 m2 g-1 and a pore volume of 0.71 cm3 g-1. Their reported experimental conditions were not identical to what we used in the fabrication of our polymers.6,14 This could be owing to the larger percentage of the pores lying in the macroporous range as opposed to the mesoporous range (see Figs. 3 and 4). This implies that the prepared polymer samples would not have a good metal ion removal capacity at high concentrations. This was observed in the optimization experiments where the removal capacity was less than 5 % in the mg L-1 concentration range but sorption was found to be maximized in concentration ranges between 25 and 200 /g L-1.

Interestingly, all monoliths except the composite materials from PAN and PV4PPS, show a Gaussian distribution of pore sizes around a specific pore size. For example PAN4 has its Gaussian distribution from 453.0-908.3 A (Fig. 3 and Fig. S9). Another interesting observation to note is that KPS1, which showed a non-Gaussian pore size distribution (see Fig. S9) showed the best metal ion uptake (vide infra). Here the majority of pore sizes are in the macro range between 417.5-2182.8 A. Hence, it is not surprising that this particular material performs the best in metal uptake experiments.

3.3. Metal Sorption

3.3.1. Optimization Results of Metal Uptake by Polymer Materials using Cu as Model Metal Ion

The working concentration of metal ions was determined for sorption studies using the prepared polymer samples. Preliminary sorption experiments were carried out in the concentration range of 1-10 mg L-1 as most reported studies using polymer sorbents indicate this as the working range. It was observed that the amount of metal ions adsorbed by the polymer increases steadily with increasing metal ion concentration but abruptly declines following a peak which implies saturation of binding sites on the polymer by the metal ions.

Sorption capacity of monolith was studied by varying the amount of sorbent material, contact time of sorbent with metal ions and pH of the aqueous mixture of the sorbent and metal ions. Typical results are shown in Figs. S10-S12 for Cu(II) ions which showed optimum sorbent concentration of 18 mg L-1 and contact time of 3 h at pH 4 for Cu(II) ions.

3.3.2. Polymer Metal Uptake of Cu, Au and Ag in Single and Multi-components

Sorption studies were performed using three Group 11 metals. These studies were carried out in single ion solutions as well as binary and ternary solutions in order to observe the sorption behaviour in a multi-ion solution.

The sorption results for the various metal ion solutions are illustrated in Figs. 4-6 and these show the sorption profile of the synthesized polymers as well as for KPS specifically for Cu(II), Ag(I), Au(III). Figure 4 illustrates the removal of Cu ions from solution. It is observed that in a single ion solution, sorption capacities reaching about 80 % can be achieved dependent on the polymer sample used. When more ions are introduced into solution, it is observed that this sorption capacity declines to reach maximum at about 60 %. From Fig. 4 it is observed that the polymer sample with the highest sorption capacity is KPS1. The sorption of Ag as shown by Fig. 5 shows maximum sorption at around 80 %. It is further observed that the sorption of Ag in solution is not influenced by the presence of other metal-ions in solution but rather by the polymer sample used as observed by a narrower standard deviation across each polymer sample which ranged between 1 % and 5 %. The Au sorption profile in Fig. 6 shows that Au reached an average sorption maximum of about 80 %. For all polymer samples, Au reaches peak sorption in binary solutions and a decline in sorption for ternary solutions possibly owing to increased competition for binding sites. The percentage relative standard deviations ranged between 1 % and5%in data represented in Figs. 4-7 but a larger range of 1-10 % was observed for some of the data in Figs. 8 and 9 but this is still within an acceptable range. The sequence in which the metal ions were added to the polymers affected the quantity of metal taken up.

3.3.3. Competitive Uptake of Metal Ions by Polymer Monoliths KPVand KPS

In order to determine how the metal ions were adsorbed by the polymer monoliths KPV and KPS, several experiments in which single, binary and ternary metal ions solutions were adsorbed were conducted. Figures 6-8 show the sorption of these metal ions by KPV and KPS.

KPS showed better removal of Ag, where 90 % of the initial concentration of Ag ions (200 //g L-1) was removed. The general trend observed for all polymers, including KPS, is Cu>Ag>Au. These polymer samples could have a higher affinity towards these metal ions because of two possibilities. One would be the size of the sample polymer's pores would allow for better sorption of metals from solution through diffusion. It is evident from the pore size distribution (PSD) results that these samples have a large volume that is accounted for by macrovoids, which would allow for easier reach to the 3D microstructure for absorption. However, it has been reported that the sorption process was spontaneous for all metals ions in another study.15 This report states that the physisorption mechanism accounts for most of the metal ions interactions with the sorbent.11 In this case pyridine, styrene and nitrogen could allow for a more favourable interaction.

In support of this view that metals bind to sorbets is a study where PAN resins were aminated and used further to remove metals from solution.12 It was observed that certain bands that are characteristic for the resin shift following sorption experiments, which infers a metal bond that would have formed. The metal ions with the highest affinity for these KPS polymer samples are soft metals, which would preferentially react with softer ligands. The composition of the solution also influences the ability of these metal ions to bind or to be sorbed onto the polymer. In the presence of Ag and Au, however, Cu is seen to be removed at a decreased rate. Ag removal for example will reach 90 % whereas Cu will only be removed up to 65 %. This shows that these polymer samples react selectively to certain metal ions if they are present in solution. Another study noted that in the presence of other ions, the ability of the sorbent to remove metals from solution decreases.16 The same study explains that the reduction in sorption capacity of the same adsorbent in a metal solution composed of many metal ions compared to that composed of a single metal ion solution could be attributed to the lesser availability of binding sites.16 It is also rationalized that a metal with a higher affinity for a given binding site will be able to displace the weaker interacting metals. This would explain the differences observed in behaviour of Cu toward KPS samples in the presence of other metals.

3.3.4. Adsorption and Desorption Studies

Determinations were conducted to establish if the polymer monolith (KPS1) that showed the best metal uptake could be recycled in adsorption/desorption experiments. This was performed using only ternary solutions as it is more likely that the three metal ions we tested would be present in acid mine drainage under similar conditions. Figure 10 shows the adsorption/desorption profiles of these metal ions by KPS1. The average adsorptions for Cu(II) was above 81 %, that for Ag(I) was slightly lower at 79 % and Au(III) showing an above 75 % average in the five cycles. The percentage adsorptions correlated perfectly with the size of the metal ions where the smallest ion showed the highest binding capacity and the largest metal ion the least. The differences in the binding capacities are relatively small, again correlating perfectly with the small differences in the metallic ion sizes. This could be because the adsorption affinities (binding energies) of the polymer and metal ion followed that order. The general trend observed for binding of the metal ions is Cu>Ag>Au. An opposite trend (Cu<Ag<Au) was observed for the desorption experiments with approximately 95 % of Au(III) desorbing with the greatest ease followed by Ag(I) at 90 % and then Cu(II) at 87 %. This trend also makes sense in that it would be expected that the metal ion with the lowest binding affinity would desorb with the greatest ease from the polymer.

The slightly higher adsorption rates in these experiments compared to the results obtained in section 3.3.3 could be attributed to fact that the monoliths in the present case were more finely ground, increasing the surface area. An increase in surface area would have exposed more binding sites from the polymer monolith.


4. Conclusion

Three types of polymer monoliths were prepared in this study; one type that has only PAN, the second a mixture of PAN and PV4P (KPV) and the third a mixture of PAN and PV4PPS (KPS). Of the three monoliths, KPS showed the highest capacity to adsorb Group 11 metal ions. This is likely due to two the nitrogen donor sites in KPS as well as the spacing provided by the pendant phenyl groups in the styrene component of KPS. Secondly, the polymer monoliths adsorbed at lower concentration and became saturated at concentrations higher than 8 mg L-1. The monoliths are therefore considered as ideal adsorbent for the removal of trace metals; and that we are currently investigating their ability to clean wastewater with municipal water samples in the Mpumalanga province in South Africa.



We acknowledge the National Research Foundation and the University of Johannesburg for financial support of this project.



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Received 23 January 2017
Revised 25 June 2018
Accepted 20 July 2018



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Supplementary Data

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