Anion Exchange Sorption of Chromate from Aqueous Solutions by Activated Carbon.
Water decontamination from chromium (Cr) is of prime importance because of its carcinogenic nature. The sample of activated carbon was characterized by surface area analyzer, SEM/EDX, TGA, FTIR and PZC. This study was focused on adsorption of hexavalent chromium from the aqueous phase onto activated carbon. Both the temperature and pH had a positive effect on the chromate uptake by activated carbon. The chromate uptake at different pH values followed the trend: pH 2 > pH 3 > pH 5 > pH 7 > pH 8. The sorption maxima at pH 2 was explained on the basis of electrostatic attraction between the negatively charged chromate anions and positively charged surface of the activated carbon. Different models were tested to access the sorption maxima and to probe into the chromate adsorption mechanism. The thermodynamic parameters suggested that heat is needed to shift the hexavalent chromium from solution to the solid surface.
It was concluded that the anion exchange sorption was involved in removing the chromate anion from the aqueous system into the surface of activated carbon.
Keywords: Chromate, Activated carbon, Anion exchange, Sorption.
Water pollution caused by heavy metal has become a serious threat to the human being for the last 20 years . Numerous people die each year all over the world because of the diseases caused by drinking water. Heavy metals is believed to be one of the major causes of water pollution [2, 3] and consequently, these heavy metals enter into the food chain and create a severe risk to living organism due to their long bio-accumulation . Millions of people die on account of the diseases caused by drinking water contaminated with heavy metals [3,5]. Chromium (Cr) is highly toxic metal on account of its carcinogenic nature [6,7]. Chromium generally exists in the Cr (0), Cr (lll) and Cr (Vl) oxidation states [8, 9]. The Agency for Toxic Substances and Disease Registry (ATSDR) depicted that the salts of Cr (Vl) are relatively more toxic due to their mobilities than Cr (lll) [10,11].
The hexavalent chromium exists in different forms of HCrO4-, Cr2O -2 and CrO -2 in aqueous phase [12, 13]. Different industrial processes such as electroplating, surface finishing, metal fabrication, metal extraction and manufacture of batteries are seen to be the major contributors of chromium to the atmosphere [14, 15]. Several researchers studied the chromium adsorption from aqueous solution [16, 17] using different adsorbents to reduce the concentration of chromium in the aquatic environment. The materials used for the decontamination of water from the dyes and hexavalent chromium include kaolinite, sand, goethite, activated alumina, activated organic resins and zeolite etc. [18, 19]. According to a survey, more than one billion people are unable to access to safe drinking water. Due attention is required for the decontamination of water from heavy metals in general and chromium in particular because of its carcinogenic nature.
Activated carbon is a good choice to be used for the decontamination of water from chromate anion because of its high surface area and excellent performance as compared to its counterparts reported in the literature . Activated carbon can be used as a capable materials for the cleansing of water from toxins. Though, the adsorption of chromate on carbon materials has been studied previously. However, the mechanism of adsorption and thermodynamic studies of chromium (VI) adsorption from aqueous solution onto activated carbon have not been given due attention. The present study not only focuses to probe into the mechanism of chromate adsorption onto activate carbon but also to evaluate the thermodynamic feasibility of the process.
Materials and Methods
Research grade reagents were used throughout the experimental work. Commercial activated carbon and (K2Cr2O7) were purchased from Merck. All the working solutions were prepared in deionized water.
The surface area of the activated carbon (AC) was determined by Quantachrome NOVA 2200e surface area analyzer. The powder sample was also analyzed using the X-ray diffractometer, model JDX-3532 with Mn filtered Cu-K[alpha] radiations. The X-rays patterns were taken at 2I, values ranging from 10 - 80 C with step size 0.30 and a step time 5 s. The scanning electron microscopy (SEM) was carried out to study the surface morphology of AC. Energy dispersive X-ray (EDX) analyses were conducted by the EDX model INCA 200. Thermogravimetric analysis (TGA) of AC was performed to determine the weight of a sample as a function of temperature by thermal Analyzer model Perkin Elmer 6300. The sample was heated at a rate of 10C per minute starting from 30 C to 1000AdegC. FTIR analyses of AC before and after chromate adsorption were performed by Infrared spectrophotometer, model Shimadzu 8201PC. Salt addition method was applied to determine the PZC .
The stock solution of 1000 ppm chromium was prepared from K2Cr2O7 which was then diluted to the desired concentration of chromium in the range of 10-150 ppm. During the adsorption experiments, 0.1 g AC was added into 30 ml chromium solutions of different concentrations. The initial pH of the suspension was fixed at a desired pH value by standard solutions of either nitric acid or sodium hydroxide. The system was equilibrated for 24 h at 120 rpm. The final pH of each suspension was recorded. After the filtration, the concentr-ations of chromium in the filtrates were determined by the atomic absorption model Perkin-Elmer Analyst 800. Similar adsorption experiments were conducted at different temperatures. Moreover, the pH effect on the uptake of chromium by AC was investigated by varying the pH from 2 to 8 at 298K.
Chromium adsorption was computed from the difference of the initial and the final concentration of the chromium in aqueous solution using the following mathematical relationship:
qe = VL(Co - Ce)/1000m
where qe refers to the amount of chromium adsorbed (mol g), VL is the volume of solution (ml), m is the amount of AC (g), Co and Ce are the initial and final chromium concentrations-1 (mol L). The solid samples of AC were air dried and subjected to EDX and FTIR analyses for the confirmation of chromate adsorption.
Results and Discussion
The BET surface area of the activated carbon (AC) determined by the Quantachrome model NOVA 1200e was found to be 177m2/g, which is similar to the one previously recorded by Borah et al. .
The XRD image indicates that the sample of AC is amorphous in nature and its PZC value is found to be 3.2 (Fig. 1). Similar PZC values for different materials have been recorded in the literature [22, 23]. As expected, the EDX spectrum of AC indicates that the sample contains only carbon and oxygen (Fig. 2). A close inspection of the IR spectrum (Fig. 3) of AC reveals smaller peaks at 1701, 1589, and 1384cm-1 which can be assigned to the vibration of C= O groups as was suggested by Rao et al. . These peaks are most probably due to the existence of carboxyl group available on the surface of virgin AC. The band at 3387 cm-1 represents the water molecules absorbed into the solid surface as this band is assigned to the OH stretching vibration . The peak at 2345 cm-1 is attributed to the evacuation of CO2 while the bands at 1544, 1680-1720 cm-1 are assigned to the C = O and C = C linkages as proposed by the Calahorro et al. .
Similarly, a small peak at 490 cm-1 represents the (C = O) stretching vibration of the carboxyl group. The SEM micrograph (Fig. 4) of AC reveals that the particles of activated carbon are irregular in shape and lack a definite morphology. Mostly the particles of AC are in the aggregated form and its external surface area seems to be porous in nature .
Effect of media dosage, concentration of chromate and temperature on adsorption
Adsorbent dose has a significant effect on the extent of chromate adsorption. The effect of adsorbent dosage on chromate adsorption was studied in a batch system using AC dose of 0.1-1.00 g and initial chromate concentration 100 mg/L at 298 K. The results are shown in (Fig. 5) which indicate that the equilibrium amount of chromate ions adsorbed decreased with increase in AC dosage. At a low adsorbent dose, the adsorption sites are exposed and the adsorption is faster resulting in higher adsorption capacity. On the other hand, the low adsorption capacity at higher dose is due to the decrease in the availability of adsorption sites because of the aggregation of adsorbent particles. Temperature role is important in the adsorption of both anion and cation from aqueous solution to the solid substrate. The influence of temperature (293K, 303K, 313K, and 323K) on the anion exchange sorption of chromate by the virgin sample of AC (Fig. 6) was also investigated.
It was observed that temperature has a profound effect on the chromate adsorption. The uptake of chromate is found to increase from 24 x 10-5 to 50 x 10-5 mol/g when the temperature of the system is raised from 293K to 323 K. The increased uptake of Cr (VI) with rise in temperature reflects that the process of adsorption is endothermic and further suggests that heat energy is needed to divest and transport the chromate anions from the aqueous phase into the solid surface. Similar results for the adsorption of metal anions by different adsorbents have been reported elsewhere [28, 29].
pH effect on adsorption
The pH of the system drastically changes the adsorption capacity of the materials. It is due to the changes in both the speciation of chromium and surface charge properties of the substrate. The adsorption isotherms at different pH values have been presented in (Fig. 7). The uptake of chromate anions at different pH value follows the trend: pH 2 > pH 3 > pH 5 > pH 7 > pH 8. The sorption maxima at pH 2 can be explained on the basis of strong electrostatic attraction between the positively charged surface and negatively charged chromate anions. The increase in final pH further reveals that adsorption is accompanied by the release of hydroxyl anion from the surface to the aqueous phase. From the changes in pH of solution, the following mechanisms may be proposed for the adsorption of chromate onto the activated carbon.
ROH + HCrO - a RHCrO + OH-
2ROH + 2HCrO4 a R2Cr2O7 + 2OH + H2O
2ROH + Cr2O72- a R2Cr2O7 + 2OH-
2ROH + CrO 2- a R2CrO4 + 2OH-
where R represents the solid matrix. The similar adsorption mechanism was described for the uptake of arsenate using binary mixed oxides of iron and silicon .
The following adsorption isotherms were used to investigate the mechanism and sorption capacity of adsorbent. The Langmuir's isotherm  assumes monolayer formation on the surface of adsorbent with no interaction between the sorbed molecules. The Langmuir's isotherm defines the equilibrium set up between the activated carbon and remaining concentration of chromate anions in solution. The most extensively used form of the Langmuir equation may be written as:
Ce/qe = 1/qmax Kb + Ce/qmax
where Ce and qe refer to the chromate anions (mol L-1) and the amount of chromate sorbed (mol.g-1) respectively, Kb represents constant (L mol-1) which is linked to the binding energy of sorption, qmax refers to the monolayer sorption capacity of AC (mol.g-1). The plots of Ce/qe vs. Ce are straight lines (Fig. 8) and monolayer sorption capacity derived from the Langmuir model is consistent with its experimental values which illustrate that the Langmuir model is the best fit to the sorption data. Higher values of the binding energy constant indicate a stronger interaction between the surface and chromate anions (Table 1). Both the sorption capacity (Xm) and apparent binding energy constant (Kb) increase with temperature rising from 293K to 323K which also indicates the chromate adsorption onto AC is an endothermic process. Dubinin-Radushkevich (D-R) model  can be used to explore the adsorption mechanism and its linear form is given as follows:
ln qe = ln qmax - [beta] Iu2
where [beta] is the adsorption energy, and Iu refer to Polayni potential which is calculated from the following relationship.
Iu = RT ln (1 + 1/Ce)
The values of qmax (mol.g-1) and [beta] (mol2.kJ-2) are obtained from the intercepts and the slopes of ln qe against Iu2 plots (Fig. 9). The linear plots of ln qe vs. Iu2 show the applicability of D - R isotherm and the mean free energy (E) is computed according to the following relationship:
E = 1/a-2[beta]
The values of R2, [beta], qmax and E determined from the plots of ln qe vs. Iu2 for chromate sorption by AC are given in Table 2. The reported value of mean free energy (E) for an ion exchange process is in the range of 8-16 kJ mol-1. In the present case, the mean free energy values for chromate adsorption by AC range from 8.63 - 11.04 kJ mol-1 which strongly supports that anion-exchange mechanism is involved in removing chromate anion from aqueous solution through AC. The D.R model further elaborates the mechanism of chromate adsorption to be anion exchange as was proposed on the basis of pH changes after chromate adsorption, according to reaction 3. It is concluded from the above observation that the chromate sorption is accompanied by the hydroxyl anions released from the surface. The present findings are also consistent with those reported for arsenate sorption onto metal oxide .
Table 1. Langmuir's constants for chromate adsorption by AC at pH 5.
Adsorbent###T(K)###R2###RL###Kbx10-2###qmax x 10-5
Table 2. D-R constants for chromate adsorption by AC at pH 5.
The entropy (IS) and enthalpy (IH) changes were calculated using the vant Half equation in the form:
1nKb = IS/R - IH/RT
The free energy change (IG) was calculated from the following mathematical expression,
IG = IH - TIS
where Kb is the binding energy constant (L.g-1), R is the molar gas constant (J. mol-1 K-1), and T (K) is the absolute temperature. The plots of 1nKb vs. 1/T (Figure 10) reveal that equation 10 is best applied in the present case. The values of IH and IS (Table 3) are positive. The IH value is greater than 40 kJ/mol which reveals that the process of adsorption is chemical in nature and further illustrates that greater heat energy is needed to shift the hexavalent chromate to the surface of AC. The findings of this study are contrary to the results observed for the adsorption chromate, where the IH value was reported to be negative and process of adsorption was exothermic. Besides, the current values are in also good agreement with the results reported for several exchangers. Moreover, negative IG values that adsorption of Cr (VI) onto AC is favourable.
As expected, the positive value of IS can be assigned to the spontaneous nature of the chromate adsorption. It further illustrates that the chromate anions removes the hydration sheath at the solid - liquid interface which is responsible for the increased entropy of the system. The magnitude of IS value is comparable to the reported values in literature.
Table 3. Thermodynamic parameters for chromate adsorption by AC at pH 5.
The uptake of chromate on activated carbon is observed to be depend upon the temperature and pH. The maximum sorption of chromate is observed at pH 2. Both D-R and Langmuir models are the best choices to explain adsorption data. The anion exchange sorption was involved in removing the chromate anion from the aqueous system into the surface of activated carbon. The thermodynamic studies confirmed that the entropy (IS) is the main controlling factor for the chromate adsorption onto the AC.
The corresponding author is thankful to Dr Asad Habib for providing support to evaluate the experimental data thorough different models.
1. S. Guo, A. Naeem, H. Fida, M. Hamayun, M. Muska and J. Y. Chen. Removal of Cu(II) from aqueous solution by iron vanadate: equilibrium and kinetics studies, Desalination and Water Treatment, vol. 2017, 75, pp.: 124-131, 2017. DOI: 10.5004/dwt.2017.20727
2. A. Naeem, P. Westerhoff and S. Mustafa, Vanadium removal by metal (hydr) oxide adsorbents, Water Research, 41 (2017) 1596. DOI: 10.1016/j.watres.2007.01.002
3. B. Edris, F. Hamed and M. F. Kord, "Removal of arsenic from aqueous environments using moringa peregrina seed extract as a natural coagulant," Asian J. Chem., 25 (2013) 3557. https://dx.doi.org/10.14233/ajchem.2013.13647
4. X. Guo-Xiang, L. Xu-Qiang and C. Wen-Bin, "Equilibrium sorption isotherms of Cr(III) on sphingomonas sp. XJ2," Asian J. Chem., 25 (2013) 3687. https://dx.doi.org/10.14233/ajchem.2013.13718
5. Z. Weixia, S. Hang and D. Kaifeng, "Rapid removal of Cr(VI) ions from aqueous solutions by the macroporous poly(N, N'-Dimethylamino Ethyl Methacrylate) hydrogels," J. Applied Polymer Sci., 128 (2013) 2729.DOI: 10.1002/app.38409
6. Z. Dong and S.Y. Jie, "Preparation of nano-strontium titanate based on glass fiber filter and its application in speciation analysis for chromium," Asian J. Chem., 25 (2013) 3195. https://dx.doi.org/10.14233/ajchem.2013.13589A
7. A. Strkalj, Z. Glavas and I. Brnardic, "Application of foundry waste for adsorption of hexavalent chromium," J. Chem. Biochemical Engineering, 27 (2013) 15. https://hrcak.srce.hr/99432
8. N. V. Nguyen, L. Jae-chun and J. Jinki, "Enhancing the adsorption of chromium(VI) from the acidic chloride media using solvent impregnated resin (SIR)," Chem. Engineering J., 219 (2013) 174. http://dx.doi.org/10.1016/j.cej.2012.12.091
9. A. Onder and A. Ilker, "Sorption and kinetic properties of 2-(Biphenyl-4-Yl)-2-oxoacetaldehyde oxime towards Zn(II) ion," Desalination and Water Treatment, (2013) 2702. http://www.tandfonline.com/loi/tdwt20
10. C. Rajdeep, Md. Khan, R. Motiar and A. R. Das, "Biosorptive removal of chromium by husk of lathyrus sativus: Evaluation of the binding mechanism, kinetic and equilibrium study," Engineering Life Science, 13 (2013) 312 doi: 10.1002/elsc.201200044
11. X. Zhihui, B. Shuangyou and L. Jianru, "Photocatalytic reduction of Cr (VI) by citric and oxalic acids over biogenetic jarosite," Material Science Engineering, 33 (2013) 2192. http://dx.doi.org/10.1016/j.msec.2013.01.040
12. S. Rumpa, M. Kakali, S. Indrajit, G. Aniruddha, K. G. Sumanta and S. Bidyut, "Removal of hexavalent chromium from water by adsorption on mosambi (Citrus Limetta) peel," Res. Chem. International, 39, (2013) 2245. doi. 10.1007/s11164-012-0754-z
13. S. Rumpa, S. Indrajit, N. Rumki, G. Aniruddha, B. Ankita, K. G. Sumanta, S. Bidyut, "Application of Chattim tree (Devil Tree, Alstonia Scholaris) saw dust as a biosorbent for removal of hexavalent chromium from contaminated water," J. Chem. Engineering, 91 (2013) 814. doi:10.1002/cjce.21703
14. A. Sikaily, A. E. Nemar, A. Khaled and O. Abdelwehab, "Removal of toxic chromium from wastewater using green alga ulva lactuca and its activated carbon," J. Hazardous Material, 148 (2007) 216. doi:10.1016/j.jhazmat.2007.01.146
15. D. Mohan, K.P. Singh and V.K. Singh, "Trivalent chromium removal from waste water using low cost activated carbon derived from agricultural waste material and activated carbon fabric cloth," J. Hazardous Material, 135 (2006) 280. doi:10.1016/j.jhazmat.2005.11.075
16. K. Nasira, F. Shana and M. Kamran, "Response of free-living marine nematode community to heavy metal contamination along the coastal areas of sindh and balochistan," Pak. J. Nematol, 28 (2010) 263.
17. T. Karthikeyan, S. Rajgopal and L.R. Miranda, "Chromium(vi) adsorption from aqueous solution by hevea brasilinesis sawdust activated carbon," J. Hazardous Material, 124 (2005) 192. https://doi.org/10.1016/j.jhazmat.2005.05.003
18. C. Namasivaym and K. Ranganathan, "Removal of Cd (II) from wastewater by adsorption on waste Fe(III) Cr(III) hydroxide," Water Resource, 29 (1995) 1737. doi:10.1016/0956-053x(94)90036-1
19. A. Ozverdi and M. Erdem, "Cu2+, Cd2+ and Pb2+ adsorption from aqueous solutions by pyrite and synthetic iron sulphide," J. Hazardous Material, 17 (2006) 626. doi:10.1016/j.jhazmat.2006.02.051
20. K. C. Roh, J. B. Park, C. T. Lee and C. W. Park, "Study on synthesis of low surface area activated carbons using multi-step activation for use in electric double layer capacitor," J. Industrial and Engineering Chem., 14 (2008) 247. doi:10.1016/j.jiec.2007.08.012
21. D. J. Kinniburgh, J. K. Syres and M. L. Jacksow, "Specific adsorption of trace amount of calcium and strontium by hydrous oxides of iron and aluminium," Soil Sci. Soc. America Proceeding, 39 (1975) 161. doi: 10.2136/sssaj 1975. 03615995003900
22. D. Borah, T. Kojima, S. Kato, and S. Satokawa, "Surface-modified carbon black for As(v) removal," J. Colloid and Interface Sci., 319 (2008) 53. doi:10.1016/j.jcis.2007.11.019
23. P. Mondal, C. B. Majumder and B. Mohanty, "Treatment of arsenic contaminated water in a batch reactor by using ralstonia eutropha mtcc 2487 and granular activated carbon," J. Hazardous Material, 153 (2008) 588. doi:10.1016/j.jhazmat.2007.09.028
24. M. Rao, G. P. C. Rao, K. Seshaiah, N. V. Choudary, and M. C. Wang, "Activated carbon from ceiba pentandra hulls, an agricultural waste, as an adsorbent in the removal of lead and zinc from aqueous solutions," Waste Management, 28 (2008) 849. doi:10.1016/j.wasman.2007.01.017
25. P. J. M Suhas and M. M. L. R Carrott, "Lignin - from natural adsorbent to activated carbon: a review," Bioresource Technology, 98 (2007) 2301. doi:10.1016/j.biortech.2006.08.008
26. C. V. Calahorro, A. N. GuiJosa, M. Stitou, and E. M. C. Correa, "A comparative study of the adsorption equilibrium of progesterone by a carbon black and a commercial activated carbon," Applied Surface Sci., 253 (2007) 5274. doi:10.1016/j.apsusc.2006.11.047
27. L. Khezami, A. Chetouani, B. Taouk and R. Capart, "Production and characterization of activated carbon from wood components in powder: cellulose, lignin, xylan," Powder Technology, 157 (2005) 48. doi:10.1016/j.powtec.2005.05.009
28. A. Kumar and B. Mandal, "Adsorption of cr (vi) and rhodamine b by surface modified tannery waste: kinetics, mechanistic and thermodynamic studies," J. Hazardous Material, 186 (2011) 1088. doi:10.1016/j.jhazmat.2010.11.104
29. D. Nityanandi and C. V. Subbhuraam, "Kinetics and thermodynamic of adsorption of chromium (vi) from aqueous solution using puresorbe," J. Hazardous Material, 170 (2009) 876. doi:10.1016/j.jhazmat.2009.05.049
30. T. Mahmood, S. U. Din, A. Naeem, S. Mustafa, M. Waseem and M. Hamayun, Adsorption of arsenate from aqueous solution on binary mixed oxide of iron and silicon. Chem. Engineerin J. 192 (2012) 90. doi: 10.1016/j.cej.2012.03.048
31. I. Langmuir, "The constitution and fundamental properties of solids and liquids." J. American Chem. Soc., 38 (1916) 2221. doi: 10.1021/ja02268a002
32. M. M. Dubinin and L. V. Radushkevich. "Equation of the characteristic curve of activated charcoal," The proceedings of academy of science. USSR, Physical Chem. Section, 55 (1947) 331. https://www.researchgate.net/publication/261358223_v26n2a18
|Printer friendly Cite/link Email Feedback|
|Publication:||Pakistan Journal of Analytical and Environmental Chemistry|
|Date:||Dec 31, 2018|
|Previous Article:||Microwave Assisted Urea Modified Bengal Gram Husk for the Batch Wise Removal of Methylene Blue from Aqueous Medium.|
|Next Article:||Assessment of Water Quality and Heavy Metals Contamination of River Ravi in Pakistan.|