Removal of copper and cobalt from aqueous solutions using natural clinoptilolite A.F. Mulaba-Bafubiandi,1 B.B. Mamba,2 D.W Nyembe2 1: Minerals Processing and Technology, Department of Extraction Metallurgy, Faculty of Engineering and the Built Environment, University of Johannesburg, PO Box 526, Wits 2050 2: Department of Chemical Technology, Faculty of Science, University of Johannesburg, PO Box 17011, Doornfontein, South Africa Email: amulaba@uj.ac.za Abstract Clinoptilolite, a natural zeolite, was used in the removal of copper and cobalt from synthetic solutions and mine water from gold mines in Nigel (Gauteng Province). Removal isotherms for both copper and cobalt synthetic solutions were constructed. In the single-salt solutions, uptakes of 79% and 63% for Cu and Co were recorded with 0.02 M and 0.04M HCl activation, respectively. In the mixed salt solutions, Co and Cu both recorded 79% uptake with 0.02 M activation. The 0.04 M activation gave percentage removals of 79% and 77% for Co and Cu respectively. Removal of copper and cobalt from mine water was found to be 100% for certain sites. On the whole, clinoptilolite removal efficiency was not affected by the presence of more than one heavy metal in dilute solutions which demonstrates its potential application in the treatment of effluents contaminated with mixed heavy metals. Introduction Water pollutants emanating from metallurgical operations have been highlighted as one of the avenues by which groundwater can be polluted, thus threatening valuable water sources. The need for clean drinking water is vital for the promotion of good health and with it comes the challenge to provide safe and high quality drinking water. Groundwater is one of the major sources of drinking water in South Africa. Unfortunately, these fresh water sources are faced with an eventuality of vanishing due to the plight of pollution. The need for recovery and purification of these waters is great if they are to be preserved. A number of purification methods are currently employed in the water purification industry and these include ion exchange, ultrafiltration, phytoextraction, electrodialysis and reverse osmosis (Geselbracht, 1996; Schnoor 1997). However, industrial wastewaters often contain a cuisine of metals that may impose cost implications when it comes to purifying it. Out of all the water purification technologies, ion exchange is the most commonly used (Inglezakis et al., 2005). The ion exchange reaction occurs between two or more phases, one of which is liquid (solution or melt), which exchanges two or more ions (cations or anions), more or less strongly bound to each phase. The ion exchanger may be a resin, activated carbon or a zeolite. Zeolites may be synthetic or natural aluminosilicates that have a framework structure that encloses cavities and tunnels which are occupied by freely moving hydrated cations that make ion exchange possible(Inglezakis et al., 2005). Clinoptilolite is the most abundant and cosmopolitan zeolite. It has been widely exploited for its ion exchange capabilities since it can easily exchange its interstitial sodium for external cations in solution (Kuronen et al., 2006). Natural zeolites often do not perform the best way that industrial standards require. When such is the case, chemical conditioning of zeolites to improve their performance is employed. The chemical removes certain cations from zeolites that may hinder ion exchange and locate easily exchangeable ones. It has been previously reported in literature (Zamzow et al., 1992) that sodium type natural clinoptilolite favours the exchange of Cu2+ over Co2+. Herein, we report the ability of South African natural and modified clinoptilolite at removing heavy metals such as copper and cobalt from synthetic solutions and mine water using the ion exchange capability of clinoptilolite. The effect of concentration of the aqueous solutions and the degree of HCl-activation of the clinoptilolite in its removal efficiency of the clinoptilolite was studied. The possibility of establishing the selectivity of clinoptilolite towards copper and cobalt in the synthetic solutions and mine water was also explored. Materials and methods Zeolite’s, source, characterization and conditioning The natural clinoptilolite used in this study was sourced from the Vulture Creek, KwaZulu Natal province of South Africa. In preparation for mineralogical studies and characterization, the clinoptilolite was crushed and milled into powder of average particle sizes approximately 75µm. The powder was then examined using an X-ray Powder Diffractometer (XRD) Phillips X’pert Model 0993 to determine its composition. Its elemental composition was determined using X-ray Fluorescence spectrometry (XRF, Phillips Magix Pro) while their surface area was analyzed using BET (Tristar 3000). The measurements were done under nitrogen atmosphere. Prior to porosity and surface area analysis, 2 g of sample was first degassed and nitrogen gas was flushed through for 4 hours at 120oC. Clinoptilolite grains of size in the range of 2.8 mm – 5.6 mm were used for adsorption studies. A fraction of these was treated in HCl at concentrations of 0.02 M and 0.04 M at room temperature over a period of 8 hrs. The clinoptilolite was then washed in deionized water to remove the fine fractions and then dried in the oven at 50 ºC for 24 hr. Synthetic solutions For the initial studies, solutions of Copper and Cobalt were prepared by dissolving CoSO4.7H2O and CuSO4.5H2O in deionized water of pH 6.5, respectively. This procedure helped to generate single-component solutions with copper and cobalt of concentrations 0.07 M, 0.33 M and 0.66 M. Studies on the copper and cobalt mixed solutions were done with solutions of copper and cobalt prepared at stoichiometric ratios of Co:Cu - 1:1, 1:5, 1:9, 5:1 and 9:5 which corresponded to these concentrations 0.07:0.07, 0.07:0.33, 0.07:0.66, 0.33:0.07 and 0.66:0.07 respectively. These solutions were assayed using atomic absorption spectroscopy (AAS), model Varian Spectra (20/20). Batch adsorption studies on synthetic solutions The ion exchange processes of Copper and Cobalt on the clinoptilolite were conducted at room temperature. Glass columns of 2 cm diameter and 30 cm of length were pre-loaded with 25 g of either as-received natural clinoptilolite or HCl-activated clinoptilolite. A volume of 25 mℓ of the prepared copper and cobalt bearing solutions of desired concentrations were passed through each of the two types of zeolites. These were afforded the same solution-zeolite contact time. The resultant solutions after passing through the zeolite-paked column were assayed using Atomic Absorption Spectroscopy (AAS) in order to ascertain the zeolite’s removal efficiency. The flame type used was air-acetylene. The adsorption wavelengths for the two metals are Cu (324.7 nm) and Co (240.7 nm). Standards of 1000 ppm, 2000 ppm, 3000 ppm were then prepared and a calibration curve was drawn using these standards. Dilution was applied stoichiometrically where the concentrations of the unknown solutions of copper and cobalt exceeded the standards’ concentration range of the standards. The metal removal percentage from the solutions and distribution ratio were calculated as follows: % Uptake = Co – Cf x 100, Co (1) Co and Cf are the initial and final metal concentrations, respectively. Kd = Amount of metal in adsorbent x V Amount of metal in solution m (2) In this study V/m = 25ml/25g = 1 V is the volume of the solution (ml) and m, is the weight of the adsorbent (g). In this study, the percentage adsorption and Kd can be correlated by the following equation (Khan et al., 1995). % adsorption = 100Kd Kd + 1 (3) Sampling and storage of mine water Mine water was sampled from Nigel mining area in the Gauteng province. The samples were stored in the refrigerator to preserve them prior to sampling. Ion exchange of mine water samples using clinoptilolite The ion exchange process of mine water on the clinoptilolite was achieved by allowing 25 g of clinoptilolite to come into contact with 25 mℓ of previously assayed mine water for 60 minutes. The subsequently treated mine water was assayed using AAS and results were tabulated. Results and discussion Clinoptilolite characterization Results of the X-Ray Fluorescence (XRF) technique are presented in Table 1. This study showed that clinoptilolite contained exchangeable ions of sodium, potassium, calcium and magnesium. This zeolite has a Si/Al ratio of 5.96 (mol/mol). The corresponding ratio of (Na + K)/Ca is 3.4. The XRF also showed that this is a high silica clinoptilolite enriched with Mg, K and sodium. The XRD plot in Figure 1 shows a typical mineralogical diffraction pattern of a crystallite with a composition of 70% SiO2, 12% Al2O3, 2% Na2O, 5% K2O, 2% CaO, and 2.5% Fe2O3. Table 1: The composition of the alumino–silicate natural clinoptilolite as revealed by XRF. Ion in clinoptilolite % Abundance Ti2+ 0.2% Si2+, Na+ Mg2+ K+ Fe3+ Ca2+ Al3+ 74% 1.3% 1.1% 3.8% 1.5% 1.5% 12.4% 24 000 12000 30 000 10 000 8000 -1 Intensity (s ) 10000 6000 4000 2000 0 0 20000 40000 60000 80000 100000 2 (°) Bragg angle 2 θ (Cu K α) Figure 1: Mineralogical pattern of the natural clinoptilolite. Metal removal from synthetic solutions The ion exchange kinetics of Co2+ and Cu2+ as a function of their concentrations in their respective solutions were studied at room temperature by varying their concentrations with time and keeping all other parameters constant. The results are shown in Figure 2 and 3. “as-rec Percentage removal decreased with increase of metal concentration in the aqueous solutions. This may be due to the fact that particles always move faster when they are less packed, thus they move faster in dilute solutions and slowly in concentrated solutions. 0.07M 0.33M 0,66M 30 0.07M 0.33M 0.66M 25 40 35 30 25 15 % removal % removal 20 10 20 15 10 5 5 0 0 0 10 20 30 40 50 -5 60 0 10 20 Time (min) 30 40 50 60 Time (min) Figure 2. Percentage removal of copper from its sulphate solutions of 0.07M, 0.33M and 0.66M by clinoptilolite at 0.02M HCl 30 minutes activation. Figure 3. Percentage removal of cobalt its sulphate solutions of 0.07M, 0.33M and 0.66M by clinoptilolite at 0.02M HCl 30 minutes activation. Metal removal from the double-component systems The copper/cobalt mixed solutions exhibited results similar to the single-salt solutions in the sense that removal efficiency was high with dilute solutions than it was with concentrated osolutions. The results are shown in Figure 4, 5, 6 and 7. High uptakes ranging between 70 – 79% were recorded with both Cu and Co removal in the concentration ratios of 0.07:0.07 M. 80 70 50 40 30 60 50 40 30 20 20 10 10 0 10 20 30 40 50 60 Time (min) Figure 4 : Co removal from double component system using 0.02 M HClactivated clinoptilolite 1:1 1:5 1:9 5:1 9:1 70 % Removal 60 % Removal 80 1:1 1:5 1:9 5:1 9:1 0 10 20 30 40 50 60 Time (min.) Figure 5 : Cu removal from double component system using 0.02 M HClactivated clinoptilolite 80 70 70 60 % removal % Removal 60 50 40 30 1:1 1:5 1:9 5:1 9:1 80 1:1 1:5 1:9 5:1 9:1 50 40 30 20 20 10 10 0 0 10 20 30 40 50 60 Time (min.) Figure 6 : Co removal from doublecomponent system using 0.04 M HClactivated clinoptilolite. 0 10 20 30 40 50 60 Time (min.) Figure 7 : Cu removal from doublecomponent system using 0.04 M HClactivated clinoptilolite. In solutions where there was more cobalt than copper by ratio (Co:Cu = 9:1 and 5:1) there seems to be difficulty in removing either of the metals. Their removal efficiencies were reduced. It is possible that there is an intermediate complex that is formed between Co, Cu and water that is too bulky (Mortimer, 1986) to favour fast removal of these metals from the aqueous solution. The presence of Cu in high concentrations (Co:Cu = 1:9 and 1:5) in the double-component solution favours the removal of both Co and Cu. This is in contradiction with the notion that less concentrated metal solutions favour fast removal of that specific metal than concentrated solutions. Removal from mine water samples In the mine water sample, however metal uptake was highly efficient for both copper and cobalt. The results are shown in Tables 2 and 3. Only the results for sites that recorded the presence of these metals are shown. It was observed that the selectivity of the exchanger towards the cation increases with increasing dilution of the aqueous solution. The mine water results also confirm this. Table 2: Co removal from mine water Name of site Nigel river Big Dam HVH mine site A Shaft No 2 A B C Piet farm A Artisanal point Conc. before removal (ppm) 2 1 8 2 2 1 1 8 Conc. after removal with ‘as-received’ clinoptlolite (ppm) 1 0 3 1 1 0 0 4 Conc. after removal with 0.02 M HClactivated clinoptilolite (ppm) 0 0 1 0 0 0 0 0 Conc. after removal with 0.04 M HClactivated clinoptilolite (ppm) 1 0 3 0 0 0 0 5 Table 3: Cu removal from mine water using ‘as-received’ and activated clinoptilolite Name of site Nigel river Big Dam HVH minesite A Shaft No 2A B C Piet farm A C D E Artisanal point Conc. before Conc. after removal (ppm) removal with ‘as-received’ clinoptlolite (ppm) 5 3 20 2 2 4 6 3 2 6 2 4 1 16 1 1 3 2 1 2 2 1 Conc. after removal with 0.02 M HClactivated clinoptilolite (ppm) 1 0 2 0 0 0 1 0 0 0 1 Conc. after removal with 0.04 M HClactivated clinoptilolite (ppm) 2 1 5 1 1 3 1 1 1 1 1 The selectivity of a zeolite for one ion over the other in a matrix is a result of physicochemical and stereochemical factors. These are hydrated radii, the hydration enthalpy of the cation and the space requirements in the micropores of clinoptilolite (Inglezakis et al., 2005). Every metal cation that is dissolved in water possesses a hydrated layer which has a characteristic thickness and degree of stability. It has been proven that ions with large radii often show large rejections while smaller ions are often favoured by exchangers (Tansel et al., 2006). Cu2+ is a smaller ion with a small hydrated radius than Co2+ and therefore Cu2+ is highly favored by clinoptilolite within the parameters in this study. It is also known that the hydration enthalpy of Cu2+ is low due to the number of water molecules solvating it (Carrillo-Tripp et al., 2006). The easy removal of copper compared to cobalt can also be attributed to the geometry of the hydrated copper ion (Inglezakis et al., 2005). Cu2+ forms a square-planar complex in water, [Cu(H2O)4]2+, while Co2+ forms a tetrahedral aqua-complex, [Co(H2O)6]2+ due to its hexavalent ion. The square planar complex is less bulky and therefore moves easily in solution compared to the bulky tetrahedral aqua-complex. However, it cannot be ruled out that ion exchangers generally have greater affinities for ions with increasing valences. Among ions with the same charge higher affinities are observed for heavier ions. This is because heavier ions have a smaller hydrated radius and this property makes them to be easily picked by an ion exchanger (Carrillo-Tripp et al., 2006, Inglezakis et al., 2005). The strength of the exchange sites on the zeolite also affects the exchange rate. Natural clinoptilolite is weakly acidic hence the rate of ion exchange in clinoptilolite is expected to be high. This is even more so with the acid activated clinoptilolite. However, the concentration of the acid used to modify the zeolite has to be monitored since it can reduce the pore volume and consequently lower the exchange ability as observed in BET results shown in Table 1. Effect of solution concentration In general, natural clinoptilolite appeared to remove the metals efficiently from dilute solutions than concentrated ones. Athanasiadis and Helmreich (2004) documented that high metal solution concentrations showed low ion exchange rates compared to low concentrations. They concluded that this was due to the high concentration of the counter ion in the solution which was generally true for all the analytes. However, an outliar was observed with Co removal from the cobalt mixed soution using 0.04 M HCl-activated clinoptilolite (Figure 6). This must have been due to an unevenly mixed size propotion of the zeolite used. It is possible that more of the smaller size range was present in this batch. A small particle size increases exchange efficiency due to surface area : volume ratio. The cation being exchanged travels a shorter distance in smaller grains than in larger ones thus speeding the exchange rate. The mine water samples were the most dilute of all the analytes (see Tables 1 and 2). There was total (100%) removal with some water samples depending on the site from which they were obtained. However, the fact that mine waters are multicomponent systems cannot be ruled out since the species present in such systems behave in unpredictable ways (ref). A full assay of the water and study of the behaviour of such a system is required to draw concrete conclusions. Effect of HCl conditioning BET and SEM analyses revealed changes in the zeolite structure. A decreasing pore volume with increase in HCl concentration was revealed by BET. Analyses of 0.00 M (“asreceived”), 0.02 M, 0.04 M and 0.10 M HCl-activated clinoptilolite revealed that there is a decrease pore volume and surface area as the HCl concentration increases. The results of the surface are and pore volume measurements are shown in Table 3. The decrease in pore volume is expected to hinder ion exchange. The BET results agree with the results obtained for the performance of the clinoptilolite where 0.02 M HCl-activated zeolite was the best performer i.e. high percentage extractions were obtained with this form of zeolite than those obtained with 0.00 M, 0.0 0.04 M concentrations. The 0.02 M acidactivation concentration also did not alter the pore volume of the clinoptilolite. There were however, some morphological changes brought about by acid activation on clinoptilolite structure when the two SEM images are compared. The SEM image in Figure 9 shows a more open stucture of the HCl-activated clinoptilolite’s surface compared to the unactivated zeolite in Figure 8. This could explain why the acid-activated clinoptilolite performed better than the “as-received” zeolite. However, in the copper/cobalt mixed solutions were less affected by these changes in the zeolite structure. The highest uptake of the 1:1 concentration ratio with 0.04 M HCl-activation was >70%. This can be attributed to the fact that there is free movement in dilute solutions (Ouki and Kavannagh, 1999). The 0.04 M HCl-activation concentration in the 1:1 did not affect the metal uptake. Figure 8. ‘As-received’ clinoptilolite at X2000 magnification Figure 9. HCl activated clinoptilolite at X2000 magnification In the non-mixed salt solutions activated clinoptilolite generally performed better as a metal up-taker than the “as-received” zeolite. The “as-received” clinoptilolite showed capacity to remove 37% Cu and 39% Co. Uptakes of 79% and 63% for copper and cobalt were recorded with 0.02 M and 0.04M HCl activation, respectively. In the mixed solutions, both cobalt and copper recorded 79% uptake with 0.02 M activation. The 0.04 M activation gave percentage removals of 79% and 77% for Co and Cu respectively. It has been documented that acid treatment of natural clinoptilolite improves its adsorbent properties (Korkuna et al., 2006, Inglezakiz et al., 2001, Athanasiadis et al., 2005). This is due to decatination, dealumination and dissolving of amorphous silica fragments blocking the channels. The study by Korkuna et al (2006) also revealed that there is a change on clinoptilolite structure after acid treatment. Dilute acid activations improved the removal capacity of the clinoptilolite’s. Studies by Vasylechko et al (1999), and Hernandez (2000) are also confirm this finding. Conclusions Kinetic isotherms for Cu and Co exchange on ‘as-received’ and natural clinoptilolite were presented for both single- and double- component systems. Cu was easier to remove than Co from the single-component systems (79%). Co and Cu were both easy to remove from the double-component systems (79%). 0.02 M HCl-activated clinoptilolite was the best performing form for both Co and Cu removal. It was followed by 0.04M HCl activation. The “as-received” clinoptilolite was the least performing of the three forms. In the solutions where there was more cobalt than copper by ratio (Co:Cu = 9:1) metal removal was difficult. The removal efficiency was noted to increase with dilute solutions. It was the highest with the mine water which recorded 100% removal of Cu and Co. Acknowledgements The authors would like to acknowledge financial support from the University of Johannesburg, Eskom’ TESP and the National Research Foundation (NRF). 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