Adsorption of Copper(II) and Lead(II) Ions from Aqueous Solutions by Porcellanite  

A.Y. Hmood1 , T.E. Jassim2
1. Marine Science Centre, College of Education for Pure Science, University of Basrah, Basrah-Iraq
2. College of Education for Pure Science, University of Basrah, Basrah-Iraq
Author    Correspondence author
International Journal of Marine Science, 2015, Vol. 5, No. 29   doi: 10.5376/ijms.2015.05.0029
Received: 22 Apr., 2015    Accepted: 03 May, 2015    Published: 06 May, 2015
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This article was first published in Mesopot. J. Mar. Sci., 2013, 28(2): 109 - 120, and here was authorized to redistribute under the terms of Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.
Preferred citation for this article:

Hmood and Jassim, 2015, Adsorption of copper(II) and lead(II) ions from aqueous solutions by porcellanite, International Journal of Marine Science, Vol.5, No.29 1-7 (doi: 10.5376/ijms.2015.05.0029)

Abstract

This work is concerned with one of the applications of adsorption behavior from aqueous solution. It deals with the adsorption of copper (II) and lead (II)ions on the surface of porcellanite, which is locally available in Iraq. The purpose of this study is to search for surfaces that are highly applicable for copper (II) and lead (II)ions adsorption to treat the pollution of aqueous solution in nature. The different variables affecting the adsorption capacity of the porcellanite such as contact time, initial metal ion concentration in the feed solution, pH of the medium and temperature, were investigated on a batch process mode. The optimum contact time to attain equilibrium is 90 min for copper (II) ion, 30 min for lead (II) ion, and the pH values in the range of 2-10. The results showed the optimum pH for Cu(II) is 8 and for Pb(II) is 4. The experimental data of adsorption were fitted to two different isotherms, namely; Langmuir and Freundlich. These isotherms equations were applied at different temperatures. The results obtained showed that, the Langmuir isotherm equation is better fitted to the experimental data than the Freundlich isotherm equation. The thermodynamic parameters indicated that ΔH was endothermic, ΔG was a spontaneous process and ΔS was positive value.

Keywords
Porcellanite; Batch adsorption; Copper and lead; Langmuir and Frendlich; Thermodynamics
Pollution is the addition of undesirable foreign matter to the environment as a result of enormous industrial development and modernization (Zietz et al., 2003). Heavy metal ions existing in aqueous waste streams of various industries such as metal plating, mining operations, battery manufacturing and tannery Fabrication are posing serious risk to the environment. Leaking of the toxic heavy metals to the soil contaminates ground and surface water leading to serious impacts on the health of human and animals. Treatment of high volumes of waste water containing low concentrations of heavy metals pollutants is becoming increasingly important as the discharge regulations become more stringent (Zhu et al., 2008). The harmful heavy metals ions associated with such industrial activities include Ni(II), Cr(II), Cu(II), Cd(II), Pb(II), Fe(III), Mn(II), Zn(II) and Hg(II) (Amdur et al., 1991).
Copper contamination of the environment is primarily due to man made (anthropogenic) activities, making it the most everywhere toxic metal in the environment. Copper is one of the most common toxic metals that find its way to water sources from various industries, includes electroplating, mining, electrical and electronics ion and steal production,printing and photographic industries. Copper concentration in humans have increased to toxic levels causing various diseases and disorders such as liver damage )Zhu et al., 2008).
Lead pollution includes the use of tetra methyl and tetra ethyl lead as gasoline additives, the main facture of storage batteries, the formation of alloys with antimony and tin to be use in power and telephone cables, the manufacture of soldering materials and lead paints (Newland and Dawn, 1982). In addition lead is also generated in the effluents from the production of television picture tubes, pigments, petroleum, fuels, photographic materials, explosives, printing, glass industrial operations and inorganic chemical manufacturing industries are also main sources of lead pollution. The toxicity and deleterious of lead are well documented, as it has been recognized for centuries as accumulative poison (WHO, 1977; ltorrison and laven, 1981). Acute lead poisoning in humans causes sever destruction in kidney, reproductive system, liver, brain and central nervous system. Mild lead poisoning causes anemia, the victim may have headache and sore muscles and may generally feel fatigue and irritable. Lead is also toxic to aquatic organisms. The concentration of lead in water below the world health organization standard (50 mg/l) cannot be considered as a serious of lead intake (Fugas and Saric, 1981). The accumulation of relatively small amounts of lead over along period of time in human body can lead to the malfunctioning of the organs and chronic toxicity (Stoker and Seager, 1976). According to the WHO, the maximum permissible limit (MPL) of lead in drinking water is (0.05 mg/l) (WHO, 1984). For these reasons, copper and lead must be removed as much as possible from industrial effluents. Several methods has been reported such as cementation of Pb(II) on spheres, on affixed bed contractor, adsorption on inert material treated with chelating reagent having selective affinity for Pb(II), non aqueous solvent extraction using organo-phosphorous compounds and chemical treatment followed by removal as precipitated carbonated (Taher et al., 2011), precipitation, ion exchange, electro chemical reduction, exploration, reverse osmosis, etc. Most of these methods are very costly and economically unfavorable. Adsorption is effective, cheap method among the chemical treatments (Hawari et al., 2009). A number of materials have been used to remove heavy toxic metals from water such as sawdust (Bulut and Tez, 2007), magnetic egg shell Fe3O4 powder (Jianwe et al., 2011), nation 117 membrane (Nasef and Yahaya, 2009), activated carbon from pesia populnea bark (Prabakaran et al., 2011), Conocarpus erectus leaves (Al-tameemi et al., 2012), activated carbon synthesized from water melon shell and walnut shell (Moreno-Barbosa et al., 2013).The present study is to investigate the possible use of locally porcellanite as an adsorbent material for removal of Cu(II) and Pb(II) ions from aqueous solution. The effect of adsorbent dose, contact time, initial metal ion concentration, temperature of solution and pH of the medium were calculated and discussed.
1 Materials and Methods
1.1 Preparation of adsorbent
Porcellanite rock was obtained from the General Company for GeologicalSurvey and Mining, Baghdad, Iraq, washed with deionized water to be completely free from dirt, dried in an oven at 120°C for a period of 3h, then ground and sieved in, to different particle sizes ranges between 75 to 300 µm, the powder was preserved in glass bottles for use as adsorbent.
1.2Chemical reagents
Metal salts used was of analytical reagent grade (Merk). Deionized water was used for the preparation of solution. Stock solutions of different concentrations (0.02-4 mg/l) of Cu(II) and (0.5-12 mg/l) of Pb(II) were prepared by dissolving exactly the amount of metal salt in deionized water.
1.3 Adsorption studies
Batch adsorption method was employed for the study of adsorption of Cu(II) and Pb(II) onto adsorbent. Adsorption of ions was carried out in 50ml stopper conical flask by adding 0.5g of porcellanite of particle size of 75 µm to 50 ml of 50 mg/l of Cu(II) and Pb(II) ions. All experiments were done at room temperature, often gentle shaking for desired time at 120rpm. The contents were filtered through filter paper (Qualitative filter paper). Concentrations of ions in the filtrate were then determined by using flame atomic absorption spectrophotometer (Pg instruments AA500). The amount of ions adsorbed were calculated based on the difference between the ions concentration in aqueous solution before and after adsorption from relation (Chu and Hashim, 2001).
Qe = V(C0 – Ce)/m ........... (1)
Where; Qe is the equilibrium adsorption capacity (mg/g), V is the volume of solution (l), m is the weight of the adsorbent (g), Co= Initial concentration of solution, Ce= Concentration of the solution after adsorption.
2 Results and Discussion
2.1Characterization of the adsorbent
FT-IR apparatus type Shimadzu (400-4000 cm-1) was used in order to identify the functional groups in the powder of porcellanite. The FTIR spectra as show in Figure 1 indicate the appearance of strong band in the region (3460-3621 cm-1) attributed to stretching vibration of hydroxyl group, the band at 1138 cm-1 belong to the stretching vibration of the (Si = O) group, the band at 476.42 cm-1 related to the stretching vibration Fe-O group and the band at 792 cm-1 related to the stretching vibration Al-O group (Silverstein et al., 2005).


Figure 1 FT-IR of porcellanite powder

2.2 Effect of contact time
The effect of contact time on the amount of metal ions adsorbed was investigated at different period (5-180 min) at 25°C. Figure 2 shows that the metal ions removal percentages increased with an increase in contact time before attaining equilibrium. The rate of metal removal is higher at the beginning due to the large surface area of the adsorbent being available for the adsorption of the metal (El-Ashtoukhy et al., 2008). Equilibrium time was attained at 90 min for Cu(II) and 30min for Pb(II). The removal percentage of metal ions in porcellanite powder for Cu(II) and Pb(II) were found to be 68.96% and 97.43% respectively.


Figure 2 Effect of contact time on adsorption of Cu, Pb ions onto porcelanite

2.3 Effect of pH on the adsorption
pH is an important parameter for adsorption of metal ions from aqueous solution, because it affects the solubility of the metal ions, concentration of the counter ions on the functional groups of the adsorbent and degree of ionization of the adsorbate during reaction (Adamson and Gast, 2001).The effect of pH on the adsorption of Cu(II) and Pb(II) ions on the porcellanitein different media (pH=2, 4, 6, 8 and 10) was studied by using a fixed concentration 50 mg/l and time contact of 30, 90min for Cu(II) and Pb(II) at 25°C respectively. Figure 3 demonstrate the influence of pH on the adsorption.


Figure 3 Effect of pH on Cu(II) and Pb(II) adsorption on porcellanite

The results showed an increase in the removal percentage of Cu(II) and Pb(II) with increasing pH values of the solution. At low pH value, binding sites are generally protanated or positively charged by the hydronium ions, this repulsion occurs between the metal cation and the adsorbent. At a higher pH value, binding sites start deprotonation, and make different functional groups available for metal binding. In general, cation binding increase as pH increases (Esposito et al., 2012). In addition, the solubility of Cu(II) and Pb(II) ions are greatly decreased as the pH increased causing an increase in the adsosption affinity towards the porcellanite surface (Lund, 1994). Accordingly, the subsequent experiments were done at pH 6.5 to avoid uncertainly in results as additional mechanism such as precipitation might play a role in metal removal from solution.
2.4 Effect of initial concentration of Cu(II) and Pb(II) ions
The effect of initial concentration of metal ions on the adsorption was carried out for different initial concentrations of metal ions in the range of (10-100mg/l), (50-400mg/l) to Cu(II) and Pb(II), respectively. The dependence of percent of metal ion removal on initial concentration of metal ions is represented in Figure 4. Percent removal was found to be maximum at low initial concentrations of metal ions. It is 89.25 %, 97.43 % for 10 mg/l, 50 mg/l of Cu(II) and Pb(II), respectively. At low initial concentrations of metal ions nearly all the metal ions adsorbed due to availability of active adsorption sites. As the metal concentration increases active sites become occupied and hence the less adsorption (Meena et al., 2005).


Figure 4 Effect of initial concentration on adsorption of Cu(II), Pb(II)
 
2.5 Adsorption isotherm
The adsorption of Cu(II), Pb(II) from aqueous solution on porcelanite has been studied at different temperatures (10, 25, 37.5 and 50°C). The general shapes of Cu(II), Pb(II) adsorption isotherm are shown in Figure 5 where the quantities adsorbed on porcelanite (Qe) are plotted as a function of equilibrium concentration (Ce) at (10, 25, 37.5 and 50°C).


Figure 5 Adsorption isotherm of Cu(II), Pb(II) on porcellanite surface at different temperatures
 
The shape of the adsorption isotherm of Cu(II), Pb(II) on porcellanite is consistent with H-type on the Giles classification. H-type adsorption isotherm indicated high affinity between Cu(II), Pb(II) and porcellanite surface in very diluted solution (Giles et al., 1960). The experimental adsorption data were applied to both the theoretical Langmuir isotherm equation and empirical Freundlich equation. The results of applying Freundlich (eq.2) and Langmuir (eq. 3) (Veena and Robert, 2002), isotherm on the adsorption data are listed in Table 1.


Table 1 Results of the application of Freundlich and Langmuir isotherms on the system studied

log Qe = log Kf + 1/n log Ce……… (2)
Where Kf is a fanction of the adsorption capacity and n is the intensity of adsorption.
Ce/Qe = 1/Qmb + Ce/Qm ………(3)
Where Qm is the maximum adsorption capacities (mg/g) and b is related to the adsorption energy.
The Freundlich and Langmuir isotherms are applied on the experimental data of the adsorption of Cu(II) and Pb(II) ions on porcellanite by plotting log Qe versus log Ce and Ce /Qe versus Ce, respectively (Figure 6 and 7). The results of Table 1 show that the Langmuir isotherms is better fitted on this system than the Freundlich as shown by the linear relationship of (Ce/Qe) versus (Ce) (Figure 7).


Figure 6 Linear form of Freundlich isotherms of Cu(II), Pb(II) on porcellanite at different temperatures


Figure 7 Linear form of Langmuir isotherms of Cu(II), Pb(II) on porcellanite at different temperatures

2.6 Thermodynamic studies
The effect of temperature on the adsorption of Cu(II) and Pb(II) was studied in the range of 10-50°C using different initial concentrations .The feasibitility of the adsorption process can be estimated by the Thermodynamic parameters of Gibbs energy change (DG), enthalpy change (DH) and entropy change (DS) by the following equations.
ΔG = -RT lnk………………..…(4)
K = Csolid / Cliquid……….……..(5)
lnK = ΔS / R – ΔH / RT……(6)
Where DG is the Gibbs energy change (KJ.mol-1), K is the equilibrium constant, Csolid is the solid phase concentration at equilibrium (mg/l), Cliquid is the liquid phase concentration at equilibrium (mg/l), T is the temperature in Kelvin and R is the gas constant (0.0083 KJ.mol-1 K-1).
ΔH (KJ.mol-1) and ΔS (KJ.mol-1.k-1) can be calculated from the slope and intercept of Eq.(6), respectively. The Thermodynamic parameters at the studied temperature ranges are listed in Table 2.


Table 2 Thermodynamic functions for adsorption of Cu(II), Pb(II) ions

The plots of lnK versus. 1/T were found to be linear with a correlation coefficient (R2 = 0.871-0.977) and (0.948-0.990) for adsorption of Cu(II) and Pb(II), respectively (Figure 8).


Figure 8 Plot of van, t Hoff relationship between LnK versus 1/T

Table 2 indicate, ΔG at all temperatures were negative and increrased with an increase in temperature, indicating the spontaneity of the adsorption of Cu(II) and Pb(II) onto porcellanite powder (Hefne et al., 2008). The positive value of ΔH indicates endothermic nature of the adsorption process, while the positive value of ΔS revealed the increase in randomness at the solid/solution interface during the adsorption process (Al-Saadie and Jassim, 2010).
3 Conclusion
The present study emphasize that porcellanite powder was employed as an adsorbent for the removal of Cu(II) and Pb(II) from aqueous solutions. The material showed enhanced Cu(II) and Pb(II) adsorption capacities compared with most materials reported in literature. the equilibrium data followed Langmuir isotherm model. The maximum percentage removal of 68.96% and 97.43% for Cu(II) and Pb(II) occurred at pH 6.5 and 25°C. It can be concluded that porcellanite powder is a promising low lost and high efficiency adsorbent for Cu(II) and Pb(II) removal from waste water and can be applied in a magnetically assisted water treatment technology.
References
Adamson A.W., and Gast A.P., 2001, Physical chemistry of surfaces, 6th ed, John Wiley and Sons, Inc., New York
Al-Saadie K.A., and Jassim S.B., 2010, Adsorption study for chromium on Iraqi Bentonite. Baghdad Sci. J., 7(1): 1-12
Al-Tameemi I.A., Nasser T., and Ibraheem T.M., 2012,Removal of Pb(II), Cd(II) Ions onto dried Conocarpus erectus leaves using batch adsorption and study the adsorption thermodynamics. J. Chem. Pharm. Res., 4(12): 4961-4968
Amdur, M.O., Doull, J. and Klaasen, C. 1991. In Casarett and Doull,s Toxicology, The basic science of poisons pergamon press, New York
Bulut, Y. and Tez, Z. 2007. Removal of heavy metals from aqueous solution by sawdust adsorption. J. Environ. Sci., 19: 160-166
http://dx.doi.org/10.1016/S1001-0742(07)60026-6
Chu, K.H. and Hashim, M.A. 2001. Desorption of copper from polyvinyl alcohol immobilized seaweed biomass. Acta Biotechnol., 21(4): 295-306
http://dx.doi.org/10.1002/1521-3846(200111)21:4<295::AID-ABIO295>3.0.CO;2-F
El-Ashtoukhy E., Amina, N.K. and Abdelwahab, O. 2008. Removal of lead (II) and copper (II) from aqueous solution using pomegranate peel as anew adsorbent. Desalination, 223: 162-173
http://dx.doi.org/10.1016/j.desal.2007.01.206
Esposito, A., Pagnanelli, F. and Veglio, F. 2002. pH-related equilibria models for biosorption in single metal systems. Chem. Engin. Sci., 57: 307-313
http://dx.doi.org/10.1016/S0009-2509(01)00399-2
Fugas M. and Saric, F. 1981. Health study of lead, D.R. Lyman, L.G. pintandia and cole, Academic Press, New York, 168pp
Giles, C.H., MamEwans, T.H., Nakhwa, S.N. and Smith D. 1960. Studies in Adsorption. A System of classification of solution adsorption isotherms, and its use in diagnosis of adsorption, and its use in diagnosis of adsorption mechanisms and in measurement of specific surface areas of solids. J. Chem.Soc, 786: 3973-3993
http://dx.doi.org/10.1039/jr9600003973
Hawari, A., Rawajfih, Z. and Nsour, N. 2009. Equilibrium and thermodynamic analysis of zinc ions adsorption by olive oil mill solid residues. J. Hazard Mater., 168: 1284-1289
http://dx.doi.org/10.1016/j.jhazmat.2009.03.014
Hefne, J.A., Mekhemer, W.K., Alandis, N.M., Aldayel, O.A. and Alajyan, T. 2008. Kinetic and thermodynamic study of the adsorption of Pb(II) from aqueous solution to the natural and treated bentonite. Int. J. Phy. Sci., 3(11): 281-288
Jianwe, R., Mokgadi, F., Bopape, K.S., Jacobo, O. and Kitinya, M.O. 2012 Sorption of Pb(II) and Cu(II) by Low-Cost magnetic eggshells-Fe3O4 powder, Chem. Industry & Chem. Engineering Quarterly, 18(2): 221-231
http://dx.doi.org/10.2298/CICEQ110919063R
Ltorrison, R.M. and laven, D.P.H. 1981. lead pollution causes and control, London Chapman and Hall
Lund, W. 1994. The Pharmaceutical Codex, 12th ed. The Pharmaceutical Press, London, pp: 774-8512
Meena, A.K., Mishra, G.K., Rai, P.K., Rajagopal, C. and Nagar, P.N. 2005. Removal of heavy metal ions from aqueous solutions using carbon aerogel as an adsorbent. J. Hazard. Mater., 122: 161-170
http://dx.doi.org/10.1016/j.jhazmat.2005.03.024
Moreno-Barbosa, J.J., Catalina, L.V., Delpilar, M.A., Liliana, G., Juancarlos, M.P. 2013. Removal of lead (II) and zinc (II) ions from aqueous solutions by adsorption onto activated carbon synthesized from watermelon shell and walnut shell. Adsorption, 19: 675-685
http://dx.doi.org/10.1007/s10450-013-9491-x
Nasef, M.M. and Yahaya, A.H. 2009. Adsorption of some heavy metal ions from aqueous solutions on Nafion 117 membrane. Desalination, 249: 677-681
http://dx.doi.org/10.1016/j.desal.2008.12.059
Newland, L.W. and Dawn K.A. 1982. In the hand book of environmental chemistry, an thropogenic compounds, 3(B), EDO. Hutzinger. Springer-Verlag Berlin Heidelerg, New York
Prabakaran, R., Arivoli, S., Hema, M. and Kamatchi, C. 2011. Removal of copper ion from aqueous solutions by low cost activated carbon from Thespesia Populnea Bark. J. Chem. Pharm. Res., 3(5): 532-543
Silverstein, M., Robert, M. and Morril, T.C. 2005. Spectrometric identification of organic compounds, 7th ed
Stoker, H.S. and Seager, S.L. 1976 .Environmental Chemistry. Air and water pollution, 2nd ed
Taher, A., Mohsin, M., Maqdoom, F. and Mazahar, F. 2011. Isotherm and thermodynamic studies on the removal of lead by using low cost material. Asian J. Biochem. Pharmaceutical Res., 1: 431-436
Veena, M. and Robert, H.H. 2002. The Role of F-400 granular activated carbon in scavenging dissolved copper ions from aqueous solution. Energeia, 13: 1-4
WHO, 1977. Environmental health criteria 3, lead. World health organization, Geneva
WHO, 1984. Guideline values for Drinking Water Quality Recommendations, Wold Health organization, Genva
Zhu, B., Fan, T. and Zhang, D. 2008. Adsorption of copper ion from aqueous solutions by citric acidmodified soybean straw. J. Hazardous materials, 153: 300-308
http://dx.doi.org/10.1016/j.jhazmat.2007.08.050
 

Zietz, B.P., Dieter , H.H., Lakomek, M.,Schneider, H.,Gaedtke, B.K., and Dunkelberg, H. 2003. Epidemiological investigation on chlronic Copper toxicity to children exposed via the public drinking water supply. Sci. Total Environ., 302: 127-144
http://dx.doi.org/10.1016/S0048-9697(02)00399-6

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