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Original article
10 (
1_suppl
); S412-S421
doi:
10.1016/j.arabjc.2012.09.013

Adsorption of Pb(II) on Mentha piperita carbon (MTC) in single and quaternary systems

,
 Environmental Research Laboratory, Department of Applied Chemistry, Aligarh Muslim University, Aligarh 202002, India

⁎Corresponding author. Address: Department of Applied Chemistry, Faculty of Engineering and Technology, Aligarh 202002, India. Tel.: +91 0571 2700920 23x3000; fax: +91 0571 2400528. rais45@rediffmal.com (Rais Ahmad)

Received: , Accepted: ,
© The Author(s) 2012
Disclaimer:
This article was originally published by Elsevier and was migrated to Scientific Scholar after the change of Publisher.

Peer review under responsibility of King Saud University.

Abstract

In the present study mentha treated carbon (MTC) has been utilized as a novel adsorbent for the removal of Pb(II) in single and quaternary systems from aqueous solution. The effects of various parameters like pH, contact time and ionic strength have been studied. The adsorbent was characterized by FTIR in order to find the functional groups present on the adsorbent. The equilibrium was attained in 180 min. The maximum adsorption of Pb(II) was observed at pH 6. The adsorption isotherm studies show that data are fitted well with Freundlich and Temkin isotherms model. The kinetics data show that boundary layer diffusion is the rate controlling step for the adsorption process and it is dominant when Pb(II) ion concentration is higher. The adsorption of Pb(II) increases with the increase in the ionic strength of the solution. The positive value of ΔH0 indicates the reaction to be endothermic in nature. The activation energy was found to be 20.60 kJ/mol K indicating physiosorption.

Keywords

Mentha piperita
Adsorption
Freundlich
Temkin
Physiosorption
1

1 Introduction

Heavy metal ions such as lead, cadmium, mercury, chromium, nickel, zinc and copper are non-biodegradable. Therefore, they can be toxic and carcinogenic even at very low concentrations, and hence, usually pose a serious threat to the environmental and public health (Liu et al., 2008). Lead is a common contaminant in industrial wastewaters, and considerable attention has been paid for its removal from industrial wastewater. According to the ranking of metal interested priorities referred by Volesky (2001) lead is one of the most interesting heavy metals for removal and recovery considering the combination of environmental risk and reserve depletion. This metal is widely used in many industrial applications, such as storage battery manufacturing, painting pigment, fuels, photographic materials, explosive manufacturing, coating, automobile, aeronautical and steel industries (Jalali et al., 2002; Igbal and Edyvean, 2004; Sekhar et al., 2004; Selania et al., 2004). Lead pollution also results from textile dyeing, ceramic and glass industries, petroleum refining, battery manufacture and mining operations (Aksu, 1998). Lead is a highly toxic and cumulative poison, accumulates mainly in the bones, brain, kidneys and muscles. Lead poisoning in human causes severe damage to the kidneys, nervous and reproductive systems, liver and brain (Naiyaa et al., 2009). In drinking water, even a low concentration may cause anemia, encephalopathy, hepatitis and nephritis syndrome (Lo et al., 1999). The permissible limit for Pb(II) in waste water as set by the Environmental Protection Agency (EPA) is 0.05 mg L−1 and that of the Bureau of Indian Standard (BIS) is 0.1 mg L−1 (Anonymous, 1981) and in drinking water intended for drinking, as set by the EU, USEPA and WHO is 0.010, 0.015 and 0.010 mg L−1, respectively (Bhattacharjee et al., 2003; Balaria et al., 2008). It is therefore, essential to remove Pb(II) from wastewater before disposal.

The traditional methods for the treatment of lead and other toxic heavy metals contaminated in wastewaters include complexation, chemical oxidation or reduction, solvent extraction, chemical precipitation, reverse osmosis, ion exchange, filtration, membrane processes, evaporation and coagulation, nevertheless these techniques have disadvantages including incomplete metal removal, high consumption of reagent and energy, low selectivity, high capital and operational cost and generation of secondary wastes that are difficult to dispose off (Eren et al., 2009; Aksu et al., 2002). Adsorption, on the other hand, is one of the most recommended physico-chemical treatment processes that is well recognized as one of the highly efficient methods for recovery and treatment of heavy metals from their matrices, samples and aqueous solutions based on the utilization of solid adsorbents from either organic, inorganic, biological or low-cost materials (Mahmoud, 2006). In our earlier studies we have utilized various types of low cost adsorbents like coniferous Pinus bark powder, treated ginger carbon, Polyaniline/iron oxide composite, and alumina reinforced polystyrene for the removal of dyes/metals from aqueous solution (Rais, 2009; Rais and Kumar, 2010, 2011).

In the present work, Mentha piperita (an agricultural solid waste) has been utilized as a potential adsorbent for the treatment of Pb(II) in single and quaternary systems (Pb + Cu + Ni + Cd) from aqueous solution by systematic evaluation using a set of parameters like pH, concentration, time, temperature and ionic strength. The resultant data were examined using pseudo-first-order, pseudo-second-order, intraparticle diffusion and elovich equation. Isotherm studies and thermodynamic behavior of adsorption were also evaluated. The desorption studies were also carried out in order to make the process more economical and feasible.

2

2 Experimental methods

2.1

2.1 Materials

Solutions of different metal ions (lead nitrate, cadmium nitrate, nickel nitrate and copper nitrate) were of analytical grade. Stock solutions (1000 mg/L) of different metal ions were prepared by dissolving the required quantity in double distilled water. HCl, NaOH, ZnCl2, and NaNO3 used in the experiments were of analytical grade.

2.2

2.2 Adsorbent preparation

The adsorbent was collected from one of the villages of Aligarh city, India. Prior to use, the mentha was washed with double distilled water to remove the adhering dirt and dried at 80 °C. The dried material was then placed in the silica crucible and kept in the muffle furnace at 750 °C. The resultant carbon was cooled in the desiccators and ground and sieved to (50–100) mesh size. The carbon prepared was then treated with 0.1 M ZnCl2 for 24 h. It was then filtered and washed with double distilled water. The material was further washed with 0.5 M HCl and then again rinsed with double distilled water to remove the acid. It was further dried in an oven and used as such for adsorption studies.

2.3

2.3 Characterization

The surface morphology of Mentha treated carbon (MTC) was analyzed by scanning electron microscopy (SEM, LEO-450, England) at 1500 magnification. The Fourier transform infrared spectroscopy (FTIR) analysis was done to study the functional groups in the range of 400–4000 cm−1 using a FTIR spectrophotometer (Inter-spec 2020, Spectrolab, UK) in KBr pellets. The concentration of Pb(II) and the combination of metal ions were analyzed using a Atomic absorption spectrophotometer (GBC 902, Australia). The pH measurements were made using a pH meter (Elico Li-120, India). The elemental analysis of the adsorbent was performed using EA1108 (Carlo-Erba).The total number of acidic sites matching carboxylic, phenolic and lactonic sites were neutralized using alkaline solutions (0.1 N NaOH, 0.1 N Na2CO3, and 0.1 N NaHCO3) (Ghodbane et al., 2008).

2.4

2.4 Point of zero charge

The determination of the point of zero charge (pHzpc) was done to investigate the surface charge and acid and basic characters of the adsorbent (Rodavic, 2008). For that 0.1 M KCl solution was prepared and its initial pH was adjusted between 2 and 12 by NaOH and HCl and then 25 ml of 0.1 M KCl was taken in 100 ml flasks and 0.05 g of the adsorbent was added to each solution. The flasks were kept for 24 h and the final pH of the solution was measured by using the pH meter. The graph was plotted between initial and final pH and the point of Zero charge was determined.

2.5

2.5 Batch adsorption study

The batch adsorption experiments were carried out in 250 ml erlenmeyer flasks containing 50 ml Pb(II) and a quaternary system (50 mg/L) on a rotary shaker at 120 rpm at a temperature of 30 °C. The samples were taken at definite time intervals of (5, 10, 15, 30, 60, 120 and 180 min) and were filtered after 3 h. The Pb(II) in the remaining solution was then analyzed. The effect of solution pH was performed in the range (2–7) for 50 mg/L. The initial metal ion concentration was determined between (20 and 100 mg/L). The adsorption efficiency (%) and capacity of the adsorbent were calculated from the formula:

(1)
% = 100 × ( C 0 - C ) / C
(2)
Q e = ( C 0 - C ) / W × V whereC0 is the initial metal ion concentration (mg/L), C is the final metal ion concentration (mg/L), Qe is the adsorption capacity (mg/g), W is the weight of the adsorbent in gm, and V is the volume of the metal ion solution (L).

3

3 Results and discussions

3.1

3.1 Characterization

Figure 1 shows the morphology of MTC samples. Sample (A) exhibits a porous and amorphous structure before adsorption. Sample (B) exhibits that the pores have been occupied by lead ions after adsorption. The FTIR spectra of mentha treated carbon before and after adsorption of Pb(II) have been shown in Figure 2. The shift in the peak from 2361.2 to 2358.7 cm−1 is attributed to CH-groups. The shift in the peak from 1457.9 to 1590.4 cm−1 is attributed to C–C-bonds of aromatic rings (Ngah and Hanafiah, 2008). The shift in the peak from 1702.1–1723.0 cm−1 is due to C = 0 groups. The shift in the peaks from 1221.4 to 1219.8 cm−1 is attributed to C−0 groups.

SEM micrographs (A) before adsorption and (B) after adsorption.
Figure 1
SEM micrographs (A) before adsorption and (B) after adsorption.
FTIR spectra (A) before and (B) after adsorption.
Figure 2
FTIR spectra (A) before and (B) after adsorption.

3.2

3.2 Elemental and active site analysis

The elemental analysis of mentha treated carbon is shown in Table 1.The high percentage of carbon (77.96%) present in the material is responsible for greater amount of adsorption of lead from aqueous solution. Table 2 shows the various active sites present on the adsorbent and among all the acid sites are predominant and probably responsible for Pb(II) ion adsorption.

Table 1 Elemental analysis of mentha treated adsorbent.
Element %
Carbon 77.96
Hydrogen 2.59
Nitrogen 0.93
Table 2 Determination of active sites.
Active sites Concentration (mg/L)
Acidic 0.1
Carboxylic 0.03
Lactonic + carboxylic 0.13
Phenolic 0.09
Basic 0.057

3.3

3.3 Effect of contact time

The contact time was studied in the range of 5–180 min at 30 °C, pH 6 and initial concentration of 50 mg/L for both Pb(II) and combination of metal ions (Figure 3). This shows a very fast adsorption in the beginning and then slows down. The adsorption equilibrium was attained in 180 min and the maximum adsorption capacity was found to be 18 mg/g for single and 23.5 mg/g for multimetal ions and the similar result has also been reported by (Srivastava et al., 2005). After this period the amount of metal ions adsorbed did not change significantly with time. The rapid uptake of metal ions on the adsorbent may indicate that most of reaction sites of the adsorbent were exposed for interaction with metal ions.

Effect of contact time.
Figure 3
Effect of contact time.

3.4

3.4 Effect of pH

The pH plays an important role in the adsorption process by affecting the surface charge of the adsorbent, the degree of ionization and speciation of the adsorbate. Thus the effect of pH in the solutions on the removal efficiency of Pb(II) in single and quaternary systems was studied at different pHs range from 2 to 7 and the results are shown in Figure 4. The acidity of medium affects the competition of H+ ion and the metal ions for active sites on the adsorbent surface (Behmou coubi and Tanouti Nibou, 2005). At a lower pH, there is more competition of H+ ion and metal ions for the available adsorption sites. However, as pH increases, this competition decreases as these surface active sites become more negatively charged, which enhances the adsorption of the positively charged metal ions through electrostatic force of attraction (Unuabonah et al., 2008a). The maximum removal of Pb(II) in single and quaternary metal ions was observed at pH 6 and after pH 6 it starts dissociating. The point of zero charge (pHzpc) was found to be 6 (Figure 5).

Effect of pH.
Figure 4
Effect of pH.
Point of zero charge.
Figure 5
Point of zero charge.

3.5

3.5 Adsorption isotherms

The adsorption equilibrium is usually described by an isotherm equation whose parameters express the surface properties and affinity of the adsorbent. Adsorption isotherms can be generated based on theoretical models where Langmuir and Freundlich models are the most commonly used (Unuabonah et al., 2008). The Langmuir model assumes that uptake of metal ions occurs on a homogenous surface by monolayer adsorption without any interaction between adsorbed ions. The linear form of Langmuir isotherm equation is given as (Langmuir, 1918):

(3)
C e / q e = 1 / b . q m + Ce / qm where qe is the equilibrium capacity of Pb on the adsorbent (mg/g), Ce is the equilibrium concentration of lead solution (mg/L), qm is the monolayer adsorption capacity of the adsorbent (mg/g), and b is the Langmuir constant (L/mg) which is related to free energy of adsorption. A plot of Ce/qe vs. Ce at different temperatures is shown in Figure 6 and the values obtained are given in Table 3.
Langmuir isotherm.
Figure 6
Langmuir isotherm.
Table 3 Adsorption Isotherms of Pb (II) ion for 30 °C.
Langmuir Isotherm qm b R2
Pb 53.19 0.1345 0.8647
Pb + Cu + Ni + Cd 50.50 0.4186 0.8809
Freundlich Isotherm Kf 1/n R2
Pb 9.189 0.4918 0.9673
Pb + Cu + Ni + Cd 14.28 0.4340 0.8409
Temkin Isotherm Kt B1 R2
Pb −7.163 21.706 0.9521
Pb + Cu + Ni + Cd 4.017 10.365 0.9083
D-R Isotherm qm β R2
Pb 29.26 0.4036 0.7867
Pb + Cu + Ni + Cd 35.8 0.3154 0.8116

Freundlich isotherm is applied for multilayer adsorption on heterogeneous adsorbents and it is assumed that adsorption sites increase exponentially with respect to heat of adsorption and Freundlich equation is an empirical equation. The linear form of Freundlich equation is given as (Freundlich, 1906):

(4)
log q e = log K f + log C m where Kf ((mg/g) (L/mg)(1/n)) and 1/n are Freundlich constants related to adsorption capacity and adsorption intensity respectively. The plot of log qe vs. log Ce at 30 °C is shown in Figure 7 and the values of the constant and correlation coefficient (R2) are given in Table 3. The values of R2 and n predict the feasibility and favorability of adsorption isotherm.
Freundlich Isotherm.
Figure 7
Freundlich Isotherm.

Heat of adsorption and the adsorbent–adsorbate interaction on adsorption isotherm were studied by Temkin and Pyzhev (1940). The Temkin isotherm equation is given by

(5)
Qe = RT / b × ln ( K t Ce ) The linearized form of equation is
(6)
Qe = B 1 ln K t + B 1 ln Ce where B1 = RT/b, T is the absolute temperature in Kelvin, R is the universal gas constant (8.314 J/mol K), Kt is the equilibrium binding constant (L/mg) and B1 is related to heat of adsorption. A plot of ln qe vs. ln Ce at different temperatures is shown in Figure 8 and the values of constant are given in Table 3.
Temkin Isotherm.
Figure 8
Temkin Isotherm.

The Dubinin–Radushkevich isotherm (D–R) is more general than the Langmuir isotherm, because it does not assume a homogeneous surface or constant sorption potential. The D–R equation is described as follows (Akcay, 2006).

(7)
ln q e = ln q m - β ε 2 where, β is a constant related to the mean free energy of adsorption per mole of the adsorbate (mol2/KJ2), qm is the theoretical saturation capacity, and ε is the Polanyi potential, which is equal to RT ln (1+(1/Ce)), where R (8.314 J mol−1 K−1) is the gas constant, and T is the absolute temperature. A plot of ln qe vs. ε2 at different temperatures is shown in Figure 9. The adsorption isotherm studies show that data in the case of lead ion are fitted well with Freundlich and Temkin isotherm whereas in the case of combination of metal ions it follow the Temkin isotherm.
D-R Isotherm.
Figure 9
D-R Isotherm.

The Freundlich type adsorption isotherm is an indication of surface heterogeneity of the adsorbent, while Langmuir type isotherm demonstrates surface homogeneity of the adsorbent. This leads to the conclusion that the surface of the adsorbent is made up of small heterogeneous adsorption patches which are very much similar to each other in adsorption capability. This study found that metal uptake differences in adsorption capacity are due to the individual properties of each adsorbent, such as structure, functional groups and surface area (Gok et al., 2008).

3.6

3.6 Adsorption kinetics

In order to examine the controlling mechanism of adsorption process various models such as Pseudo-first-order, pseudo-second-order, intraparticle diffusion and Elovich equation were used to test the experimental data.

The pseudo-first-order equation given by Lagergren (Lagegren, 1898) was widely used for the adsorption of liquid/solid system on the basis of solid capacity. Its linearized form of equation is

(8)
log ( q e - q t ) = log q e - K 1 t / 2.303 where qe is the adsorption capacity of heavy metals (mg/g), qt is the adsorption capacity at time t (mg/g), and K1 is the rate constant (min−1). The values of K1 and R2 at 50 mg/l for Pb(II) in single and quaternary systems of metal ions were calculated from a linear plot of log (qe–qt) vs. t as shown in Figure 10 and are given in Table 4. The calculated values of qe do not match with the experimental values of qe and R2 values are also low, so it do not follow pseudo-first-order kinetics.
Pseudo first order.
Figure 10
Pseudo first order.
Table 4 Kinetic parameter of Pb (II) ion.
Pseudo-first-order
Pb Pb + Cu + Ni + Cd
Qe (cal) 5.33 2.88
Qe (exp) 18.00 23.5
K1 0.10824 0.0693
R2 0.9744 0.9905
Pseudo-second-order
Qe (cal) 18.11 23.58
Qe (exp) 18.00 23.50
K2 6.3807 × 103 25.045 × 103
R2 1 1
Intraparticle diffusion
Kid 0.0294 0.018
C 14.98 21.393
R2 0.8184 0.9143
Elovich equation
A 14.274 20.776
B 0.8129 0.584
R2 0.8444 0.9112

Therefore, the kinetic data were further analyzed by using pseudo-second-order kinetics equation. The linearized form of equation is as follows (Mckay and Ho, 1999).

(9)
t / q t = t / q e + 1 / K 2 q e 2 where qt is the amount of metal ion adsorbed (mg/g) at given time t (min), qe is the amount of metal ion adsorbed at equilibrium (mg/g) and K2 is the pseudo-second-order rate constant for adsorption (g/mg min). A plot of t/qt vs. t is shown in Figure 11. The results were compared with the correlation coefficient (R2) and are given in Table 4. The R2 value for pseudo-second-order is the highest as compared to pseudo-first-order kinetics. The qe (exp) value of pseudo-second-order also agreed well with the qe (cal) as compared to first order kinetics and therefore, the data arebest followed by the pseudo-second-order kinetics in both the cases.
Pseudo 2nd order.
Figure 11
Pseudo 2nd order.

The kinetic data were analyzed by the intra particle diffusion model to elucidate the diffusion mechanism (Ho and Mckay, 1998).

(10)
q t = K id t 1 / 2 + C where Kid (mg/g min−1/2) is the intra-particle diffusion constant and qt is the adsorption capacity at time t (mg/g). The values of Kid, C, and R2 were calculated from the slope of plot qt vs. t1/2 as shown in Figure 12 and given in Table 4. The value of intercept gives an idea about the boundary layer thickness i.e. larger the intercept; greater is the boundary layer effect (Weber and Moriss, 1963). It is seen from Table 4, that the value of intercept is not zero but high and it increases in the case of combination of metal ions. This result implies that boundary layer diffusion is the rate controlling step for the adsorption process and it is dominant when Pb(II) ion concentration is higher.
Intraparticle diffusion.
Figure 12
Intraparticle diffusion.

The adsorption data were further tested with the Elovich equation which is expressed as (Kannan and Sundaram, 2003).

(11)
Qt = A + B ln t where A and B are Elovich constants. The values of A, B and R2 are calculated from Figure 13 and given in Table 4. From Table 4, it is evident that the experimental data are best followed by pseudo-second-order kinetics in both the cases.
Elovich equation.
Figure 13
Elovich equation.

3.7

3.7 Effect of ionic strength

The effect of ionic strength on the adsorption of lead ion was studied using 0.001 N NaNO3, 0.1 N NaNO3, and 0.5 N NaNO3 solutions. It was observed that the rate of adsorption is more in the case of 0.1 N NaNO3 solution. It also suggested that increasing electrolyte concentration can cause screening of surface negative charges by the electrolyte ions leading to a drop in the adsorption of the metal ions (Coles and Yong, 2002). Therefore, a decrease in adsorption of metal ion with increasing ionic strength of electrolyte implies that increasing ionic strength is making the potential of the adsorbent surface less negative and thus would decrease metal ion adsorption (Behmou coubi and Tanouti Nibou, 2005).

3.8

3.8 Thermodynamic studies

The thermodynamic factors were studied in the temperature range of 303–323 K. The thermodynamic parameters such as enthalpy change (ΔH0), entropy change (ΔS0) and Gibbs free energy change (ΔG0) were estimated using the following equations (Namasinayam and Yauuna, 1995).

(12)
Kc = Ca / C e
(13)
Δ G 0 = RT ln Kc where Kc is the equilibrium constant, Ce is the equilibrium concentration in solution (mg/L), and Ca is the solid phase concentration at equilibrium (mg/L). ΔH0 and ΔS0 were determined by Van't Hoff equation:
(14)
log Kc = Δ S 0 / 2.303 R - Δ H 0 / 2.303 RT The values of ΔH0 and ΔS0 were obtained from the slope and the intercept of the plot log Kc vs. 1/T as shown in Figure 14 and presented in Table 5. The values of ΔG0 are negative confirming the adsorption of Pb (II) in single and quaternary systems of metal ions onto adsorbent as spontaneous and thermodynamically favorable at a high temperature. The positive value of ΔH0 indicates the reaction to be endothermic in nature. While the positive value of ΔS0 indicates randomness at solid/liquid solutions interface during adsorption of Pb(II). It was observed that in case of quaternary system, higher values of ΔG0, ΔH0 and ΔS0 as compared to single system.
log Kc vs 1/T.
Figure 14
log Kc vs 1/T.
Table 5 Thermodynamic parameter of Pb(II) ion.
Metal ion Temp (K) ΔG0 ΔH0 ΔS0 R2
Pb 303 −4.176 4.25 0.081 0.8642
313 −5.18
323 −6.55
Pb + Cu + Ni + Cd
303 −6.151 19.28 0.0835 0.9158
313 −7.13
323 −8.51

The magnitude of activation energy explains the type of sorption. Two main types of adsorption can occur, physical or chemical. In physical adsorption, the equilibrium is usually attained rapidly and easily reversible, because the energy requirements are small. The activation energy for physical adsorption is usually not more than 4.2 kJ/mol, because the forces involved in physical adsorption are weak. Chemical adsorption is specific and involves forces much stronger than those of physical adsorption. Therefore, activation energy for chemical adsorption is of the same magnitude as the heat of chemical reactions (Ucun et al., 2008). A plot of ln k2 versus 1/T gives a straight line, and the corresponding activation energy was determined from the slope of linear plot as given by Arrhenius relationship (Baysal et al., 2009).

(15)
ln K c = - E a / RT + ln K O The value of activation energy is found to be 20.60 kJ/mol K and Ko is found to be 17.931 for the single metal ion system; whereas in the case of quaternary system the value of activation energy is found to be 19.06 kJ/mol K and Ko is found to be 21.33 KJ/mol.

3.9

3.9 Comparative study of the adsorbent

In order to evaluate the feasibility of the adsorbent and to compare the adsorption capacity with other non conventional adsorbents a comparative study is presented in Table 6. It is evident from the table that Mentha piperita carbon (MTC) has got the highest monolayer adsorption capacity of (53.19 mg/g) among all the adsorbents.

Table 6 Adsorption capacity of Pb(II) on various adsorbents.
Adsorbent Qmax (mg/g) References
Banana peel 2.18 Anwar et al. (2010)
Acacia Nilotica 2.51 Sadia et al. (2012)
Areca waste 3.37 Li et al. (2010)
Sawdust 6.54 Yasemin and Zeki (2007)
Ion imprinted PVI copolymer 7.60 Cesar et al. (2012)
Sawdust pinus sylvestris 9.71 Taty-Costodes et al., 2003
Activated carbon of melocana 10.66 Lalhruaitluanga et al., 2010
Chitosan coated sand 12.32 Wan et al. (2010)
Activated carbon hazelnut 13.05 Imamoglu and Tekir (2008)
Rhizopus 18.00 Smith (1981)
Orange peel 21.05 Tang et al. (2007)
Peanut hull 30.43 Brown et al. (2000)
Activated Carbon date pits 30.70 Abdulkarim and Al-Rub (2004)
Meranti sawdust 34.25 Rafatullah et al. (2009)
Activated carbon agricultural byproducts 36.05 Johns et al. (1998)
Amino functionalized Fe3O4 nanoparticle 40.10 Yanging et al. (2012)
Algal waste 44.00 Vilar et al. (2005)
Mansolnia wood sawdust 51.81 Ofomaja et al. (2010)
Treated sawdust 52.38 Meena et al. (2008)
Mentha piperita 53.19 This study

3.10

3.10 Desorption

The desorption of lead ions was carried out using 0.1 M HCl and 0.1 M acetic acid. It was found that more than 90% of lead ions are desorbed by 0.1 M HCl.

4

4 Conclusion

The mentha treated carbon (MTC) is proved to be a good adsorbent for the removal of Pb(II) from aqueous solution. The equilibrium was attained in 180 min. The maximum adsorption was observed at pH 6. The adsorption isotherm studies show that data are fitted well with Freundlich and Temkin isotherm in the single system whereas in the case of quaternary system it follow the Temkin isotherm. The kinetics data show that boundary layer diffusion is the rate controlling step for the adsorption process and it is dominant when Pb(II) ion concentration is higher. The adsorption of Pb(II) increases with the increase in the ionic strength of the solution. The positive value of ΔH0 indicates the reaction to be endothermic in nature. While the positive value of ΔS0 indicates randomness at solid/liquid solutions interface during adsorption of Pb(II). The value of activation energy is found to be 20.60 kJ/mol K indicating physiosorption.

Acknowledgement

The help from Maulana Azad Foundation is greatly acknowledged for providing financial assistance to Mrs. Shazia Haseeb to carry out the work.

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