Isothermal and Kinetic Studies of Simultaneous Removal of Mn (II) and Pb (II) Ions in Aqueous Solution by Adsorption onto Clay from Bikougou Deposit (Gabon)
J. Ndong Nlo,
Z.H. Moussambi Membetsi,
R. Kouya Biboutou
P. Edou Engonga
This work aimed to evaluate the potential of the clay from Bikougou to adsorb simultaneously Mn (II) and Pb (II) from binary aqueous solutions. The experiments were realized by using batch technique at the temperature of 308 K and pH 4 with adsorption isotherms and the interaction of adsorbent-adsorbate time as parameters. Adsorption isotherm models of Freundlich, Langmuir and Dubinin-Kaganer-Radushkevich are all appropriate to describe the experimental adsorption results with their correlation coefficients above 0.95. The maximum amount of Mn (II) and Pb (II) ions adsorbed simultaneously is 85.379 mg g-1 and was obtained by applying the model of Dubinin-Kaganer-Radushkevich. The Mn (II) ions are preferentially adsorbed at multilayer available Freundlich surface sites and Pb (II) ions on the available adsorption sites on monolayer Langmuir homogeneous surface. The Pb (II) and Mn (II) mean adsorption energies are indicative of chemical and physical processes. In the bi-solute of Mn(II)-Pb(II) system, Pb(II) adsorption is promoted during its competition with Mn(II) for the adsorption sites. Mn(II) and Pb(II) ions compete for the attainment of adsorption sites following the kinetics of pseudo-second order with correlation coefficients greater than 0.99. All these results have shown the efficiency of clay adsorbent for the simultaneous removal of Pb (II) and Mn (II) from aqueous solution.
to cite this article:
F. Eba, J. Ndong Nlo, Z.H. Moussambi Membetsi, J.A. Ondo, R. Kouya Biboutou and P. Edou Engonga, 2012. Isothermal and Kinetic Studies of Simultaneous Removal of Mn (II) and Pb (II) Ions in Aqueous Solution by Adsorption onto Clay from Bikougou Deposit (Gabon). International Journal of Chemical Technology, 4: 1-16.
Received: December 16, 2010;
Accepted: May 30, 2011;
Published: March 05, 2012
Heavy metals as Mn and Pb released to environment through industrial effluents
have been found toxic and responsible of serious pollution. The accumulation
of Mn and Pb through ingestion and inhalation has shown adverse effects against
human health including: kidneys damage, nervous and reproductive systems attack
as reported by Lin and Juang (2002) and Eba
et al. (2007). It is necessary that heavy metal must be removed before
the industrial effluents transferred to the environment. Several methods are
used for treatment of heavy metal aqueous solutions, such as ion exchange, precipitation,
phytoextraction, ultrafiltration, reverse osmosis, electrochemical deposition,
adsorption using activated carbons (Gueu et al.,
2007) or zeolites (Erdem et al., 2004). Because
of the high cost of above processes, recourse of low-cost adsorbents has been
appeared to be an alternative opportunity in adsorption technology and interest
towards these materials is growing (Babel and Kurniawan,
2003; Unlu and Ersoz, 2006).
A non-exhaustic list of low-cost adsorbent includes wood sawdust, clays, clay
materials and other materials of agricultural and industrial wastes origin (Ahmad
et al., 2009; Larous et al., 2005;
Shukla et al., 2002; Gueu
et al., 2006).
Clays are widely used in many fields of technology and science such as paints,
paper, cosmetics, plastics, rubbers, refractory materials, pharmaceuticals,
pesticides, food industries, ceramics, lubricants, hazards prevention (Al-Jlil
et al., 2009; Ekosse, 2000; Carretero,
2002; Yvon et al., 2002; Bizi
et al., 2003; Petit et al., 2004;
Martin et al., 2004; Clerc
et al., 2005; Denac et al., 2005a,
b; Yao et al., 2005).
In adsorption technology, considered as low-cost adsorbents, clays have already
been showed to have high adsorption capacity which may even exceed that of activated
carbon under the same conditions of temperature and pH. Clays are characterized
by many properties which are useful in adsorption technology such as: high specific
surface area, mechanical and chemical stability, high cation exchange capacity,
Bronsted and Lewis acidities, negative surface charge and structural variability
(Ijagbemi et al., 2009).
Several studies on the adsorption in aqueous solution of lead and manganese
were conducted. Without being exhaustive, we mention Babel
and Kurniawan, 2003 who reported that the montmorillonite, kaolinite, illite
and bentonite adsorb respectively 0.68, 0.12, 1.41, 4.29 and 0.68 mg g-1
of Pb (II) as given by applying the Langmuir isotherm.
Similarly Gupta and Bhattacharyya (2005, 2008)
have obtained with pure kaolinite and montmorillonite and modified stared respectively
11.5 and 31.1 mg g-1 respectively and 5.44 and 31.44 mg g-1
of Pb (II) at their surface.
The lead adsorption was also obtained with other families of clays such as
bentonite (Naseem and Tahir, 2001; Inglezakis
et al., 2007; Ayari et al., 2007;
Zhu et al., 2008), kaolinite (Jiang
et al., 2009; Unuabonah et al., 2009;
Bosco, 2009), montmorillonite, smectite, palygorskite
(Erdem et al., 2004; Da-Fonseca
et al., 2006; Potgieter et al., 2006;
Eloussaief and Benzina, 2010). Experiments on adsorption
of manganese by clay (Da-Fonseca et al., 2006;
Eba et al., 2010), as clinoptilolite (Doula,
2009) and kaolinite (Bosco, 2009) have been reported.
The results of these most previous studies are best described by applying the
Langmuir isotherm and kinetics is generally either first order or second order.
Wastewaters contain generally more than one heavy metal (Doula,
2009; Mohan and Singh, 2002). The protection of
the environment requires more studies on multi-solute system solutions. It is
to be noted the large number of references related to literature concerning
single sorption of heavy metal ions studies in comparison of the few studies
of multi-component systems. The main difficulty is the obtainment of adsorption
models which describe accurately the experimental adsorption data from multi-solute
solutions. At the purpose to make the problem tractable, in spite the system
complexity, some simplified modeling approaches have been introduced. Machida
et al. (2005), Lin and Juang (2002), Bedelean
et al. (2009), Amer et al. (2010)
and Ho and McKay (1999b) used competitive Langmuir model
to compute simultaneous adsorption respectively of Cu (II) and Pb (II) onto
activated carbon, Cu (II) and Zn (II) on surfactant modified montmorillonite
and on sphagnum peat moss. In the binary solution of Pb (II) and Zn (II) and
Pb (II) and Cd (II) (Minceva et al., 2007), Pb
(II) is quantitatively better fixed than Cd (II) and Zn (II) on natural zeolite.
These results were interpreted based on the isotherms of Langmuir and Freundlich.
In addition, for binary and ternary solutions of Cd, Pb, and Zn (Stefan
et al., 2008), montmorillonite fixed with greater affinity Pb and
the adsorption followed the sequence Zn<Cd<Pb. Chotpantarat
et al. (2011) studied competitive sorption of Pb2+, Ni2+,
Zn2+ and Mn2+ on the lateritic soil where they found Pb2+
preferably settled on the sorbent surface than Ni2+, Zn2+
and Mn2+. In these previous works, batch and column techniques were
used to investigate the mutual effects of metals in multi-metals system by measuring
the ratio of the sorption capacity of one metal in multi-metals systems, qi
(mix),to the sorption capacity of given metal in single-metal system, qi(o).
If qi(mix)/qi(o)>1, sorption of metal, i, is enhanced
by the other metals ions. If qi(mix)/ qi (o) = 1, metals
had no effects on each other. If qi(mix)/qi(o)<1, metals i competed
with other metals for sorption sites of the adsorbent . These works require
the knowledge of the adsorption amount of a metal in the multi-solute system
and in single system. Similar demand concerns the applicability of the extended
forms of Langmuir, Freundlich and D.K.R. models. That takes more time to reach
the end of a study.
In the purpose to minimize the duration of multi-metals system studies, the mutual effects of metal in multi-metals system should be evaluated by measuring the ratio of each metal in multi-metals solution before and after sorption process. In the practice, only the percentage of each solute might be measured in aqueous effluents polluted by more than one metal. An isotherm equation model correlating the variations of each metal ratio in multi- component system and its concentration to equilibrium should be inquired.
The present work aimed to determine the potential of clay from Bikougou (Gabon
11°37E and 1°58N) using batch technique (El-Said,
2010), for the simultaneous removal of Mn (II) and Pb (II) ions from aqueous
solution, without a preceding single adsorption isotherm study of each heavy
metal. The research of an isotherm model connecting the ratio of the sorption
capacity of each heavy metal and its equilibrium concentration in multi-component
solution is tested.
MATERIALS AND METHODS
Adsorbent characterization: Clay (in whole-rock material) from Bikougou
deposit, used as adsorbent, was previously characterized (Eba
et al., 2010). The X-ray powder diffractograms of the natural sample
and of its clay fraction (Fig. 1, 2) indicate
that whole-rock is constituted with four clayey minerals:
||Kaolinite, identified by its ray at 7.19Å in crude clay
(Fig. 1), which is shifted at 10.40 Å by hydrazine
saturation from clay fraction pattern (Fig. 2 curve h)
||Montmorillonite recognized for its typical ray at 14.93 Å (Fig.
1) or at 15.13 Å (Fig. 2, curve U) which is
shifted at 17 Å (Fig. 2, curve G) with the ethylene-glycol
treatment or reduced to 9.80 Å (Figure 2, curve
C) on heating at 490°C
||Illite known for the displaying a doo1 at 9.92 Å (Fig.
1) or at 10.02 Å (Figure 2, curve U) which is
not affected by the above mentioned treatments (Fig. 2).
Other illite rays are at 5.04 Å, 4.45 Å, 3.38 Å, 3.65
Å, 3.34 Å, 2.87 Å, 2.54 Å in Fig.
||Feldspars are revealed by reflections at 3.18, 3.21, 4.04 Å. The
pattern is typical of andesine or albite. Quartz (rays at 3.34 Å,
3.18 Å and 2.56 Å), carbonates as calcite mineral (rays at 3.05
Å, 2.93 Å) and as gaylussite (rays at 3.205 Å, 6.39 Å,
2.63 Å), anatase (rays at 3.51 Å, 2.37 Å and 1.89 Å),
maghemite (rays at 2.93 Å, 2.56 Å) and Ba, Sr-hydroxyapatite
(rays at 4.45 Å, 3.76 Å, 1.82 Å, 2.13 Å and 2.93
Å) are the other mineral species identified in Fig.
|| XRD patterns of crude clay from Bikougou deposit
|| XRD patterns of clay fraction from Bikougou deposit
After X Rays, complementary experiments have been realized. These experiments
are related to determination of Specific Surface Area (SSA) (Santamarina
et al., 2002), according to methylene blue method (Hang
and Brindley, 1970), cation exchange capacity by using ammonium acetate
methods at pH7 (Remi and Orsini, 1976), acid surface
functional groups (Khan et al., 2009) by means
of Boehm titration (Rockstraw, 2000) and point of zero
charge with the employment of potentiometric titration (Ijagbemi
et al., 2009).
Adsorbate and aqueous solution: Mn (II) (MnCl2, 4H2O, MW: 197.90g.mol-1) and Pb (II) (Pb(NO3)2, MW: 325g.mol-1) were used as simultaneous adsorbate in this work. Obtained from Prolabo (analytical grade), they were utilized without further purification. Simultaneous solutions of Mn (II) and Pb (II) were prepared by dissolution weighed amounts of MnCl2, 4H2O and Pb(NO3)2 in de-ionised water to achieve concentration of Mn (II) and Pb (II) wanted.
Adsorption procedure: Weighed amounts (0.15 g) of the adsorbent were introduced into bottles containing 50 mL of Mn (II) and Pb (II) solution kept at pH 4. The bottles were shaken at room temperature (303 K) at constant stirring speed using a thermostatic shaker for various times to attain equilibrium. The dispersions were then filtered out and solutions were analyzed for their Mn and Pb concentration, by using an atomic adsorption spectrometer (Analyst 100 Perkin Elmer).
Calculation: The amounts of Mn (II) and Pb (II) ions adsorbed per unit of mass: qt (mg g-1) were calculated by using the equation:
where, Co and Ct are the initial Mn (II) or Pb (II) concentrations and concentrations of the same cations after any time of interaction adsorbent-adsorbate, V is the volume of adsorbate solution and m the mass of clay.
Theoretical basis: The adsorption process is generally described by
the Freundlich (Gupta and Bhattacharyya, 2005; Freundlich,
1906), Langmuir (Langmuir, 1918) and Dubinin-Kaganer-Radushkevich
(DKR) (Karapinar and Donat, 2009) isotherms. Freundlich
isotherm could be expressed by the linearized equation:
Langmuir isotherm in its linearized form is expressed by the equation:
And the DKR isotherm is given by the equation:
where, qt is the amount adsorbed per unit mass of the adsorbent. Ct is the equilibrium concentration of the adsorbate after any time of adsorbate-adsorbent interaction time. KF and n correspond to Freundlich maximum adsorption capacity and adsorption intensity. qm and b represent respectively the Langmuir maximum adsorption capacity and adsorption equilibrium constant and XM, β, ε are respectively the DKR maximum adsorption capacity, activity coefficient related to mean adsorption energy and Polanyi potential.
If the isotherm model fits accurately experimental data, then, linear Freundlich, Langmuir or DKR plots could be obtained by plotting (1) lnqt vs ln Ct, (2) Ct/qt vs Ct or (3) lnqt vs ε2 respectively. Adsorption parameters are computed from these plots. A further analysis of Langmuir equation can be made on the basis of a dimensionless equilibrium constant RL given by:
where, b is the Langmuir equilibrium constant and Co any adsorptive concentration
at which the adsorption is carried out. For favorable adsorption 0<RL<1
and RL>1 represents unfavorable adsorption, RL = 1
linear adsorption and RiL = 0 corresponds to an irreversible process
(Juang et al., 1997; Kadirvelu
and Namasivayam, 2003). An isotherm is found to be suitable if its correlation
coefficient is equal to unity.
When the kinetics of the adsorption follows the pseudo-second-order kinetics
(Tien and Huang, 1991; Ho and McKay,
1999c; Ho et al., 2001), the equation might
where, k2 is the second-order rate constant and qe amount of heavy metal ions adsorbed. Then, the plot t/qt vs. t gives a linear relationship which allows computation of qe and k2.
The competitive adsorption isotherm model, proposed in the present study, is
a Langmuir, Freundlich or D.K.R. equation type in which the amount adsorbed
per unit mass: qt of each metal is replaced by its ratio.
RESULTS AND DISCUSSION
Adsorbent characterization: The chemical composition of the whole-rock
is reported in Table 1. By combining the X-ray results and
the whole-rock chemical analyses, the modal compositions of untreated clay can
be estimated according to a constrained multi-linear calculation as reported
by Yvon et al. (2002). The other clay characteristics
such as specific surface area, cation exchange capacity, acid surface functional
groups and point of zero charge are reported in Table 2 (Eba
et al., 2011).
|| Chemical composition of clay material from bikougou
|Major elements expressed in percentages of oxides and trace
elements expressed in parts per millon (ppm)); L.O.I. (loss on ignition);
< L.D. (below detection limit)
|| Characteristics of bikougou clay deposit
Adsorption isotherms studies: The adsorption isotherm for the simultaneous
removal of Mn (II) and Pb (II) from aqueous solution of pH 4 was realized at
303K using 0.15 g of adsorbent and 50 mL of bi-solute solutions of 146.1446
mg L-1 and 180.933 mg L-1 which contained respectively
51.19% and 68.78% of Mn. The amounts of Mn (II) and Pb (II) simultaneously adsorbed
increased with the increase in initial concentration of the two heavy metals
in solution (Table 3). This may be attributed to the presence
in relatively large concentration of the two heavy metals ions in the same solution.
It is to be noted that, generally, when heavy metal concentration increases,
number of ions to be adsorbed increases, consequently adsorption increases,
indicating that the number of ions to be adsorbed is lower sometime to that
of available adsorption sites on adsorbent surface. Similar results are reported
in the literature (Ayari et al., 2007; Gupta
and Bhattacharyya, 2008).
The data obtained were tested to the well known isotherms of Langmuir, Freundlich and DKR. The plots Ct/qt vs t (Fig. 3), lnqt vs ln Ct, (Fig. 4) and lnqt vs ε2 (Fig. 5), illustrate the adherence of each model to the experimental data. Satisfactory agreement between experimental data and the model predicted values are expressed by the correlation coefficient (R2). The parameters for Langmuir, Freundlich and DKR isotherm models are reported in Table 4. The three models are applicable to describe the simultaneous adsorption of Mn (II) and Pb (II) ions on the adsorbent surface.
The Langmuir model effectively described the adsorption data with all correlation
coefficients (R2) ranged between 0.9812 and 0.9982 for Mn (II) and
from 0.9992 to 0.9998 for Pb (II) (Table 4). This was confirmed
by the variations of the dimensionless parameter RL remained between
0.16 and 0.19 for Mn (II), and between 0.013 and 0.00176 for Pb (II).
|| Amounts of Mn (II) and Pb (II) ions adsorbed at equilibrium
at 303K (pH 4, contact time 45 min clay 3 g L-1)
|Where: q(Mn) and q(Pb) in mg g-1, are the equilibrium
amount of Mn (II) and Pb(II) adsorbed per specified amount of adsorbent
respectively; q(Mn) + q(Pb) is the equilibrium amount of Mn (II) and Pb(II)
adsorbed simultaneously per specified amount of adsorbent
||Plots of variations of the ratio of the equilibrium concentration
(Ct, mg L-1) on amount adsorbed specified amount of
adsorbent (qt, mg/g)as a function of equilibrium concentration
for Pb (II) and Mn(II) ions adsorption for simultaneous removal of Mn and
Pb with Mn percentage of 51.19% (303K, pH4 clay 3 g L-1 and contact
time 45 min)
||Plots of variations of the logarithm of amount adsorbed per
specified amount of adsorbent (qe, mg g-1) as a function
of the logarithm of equilibrium concentration of binary solution of Mn(II)
and Pb (II) (with Mn (II) percentage of 51.19%; 303K, pH4 clay 3 g L-1
and contact time 45 min)
||Plots of variations of the logarithm of amount adsorbed per
specified amount of adsorbent (qt, mg g-1) as a function
of the square of Polanyi potential (ε2, (Kj/mol)2)
for simultaneous removal of Mn(II) and Pb(II) (with Mn percentage of 51.19%
(303K, pH 4 clay 3g L-1, contact time 45 min)
||Langmuir, Freundlich and DKR parameters and statisticals for
simultaneous adsorption of Mn (II) and Pb (II) ions at 303K, pH4 and contact
time 45 min
|Where: qm is the Langmuir monolayer maximum capacity; b is
the Langmuir equilibrium constant; RL is the Langmuir dimensionless
factor; R2 is the correlation coefficient; KF is the
Freundlich maximum adsorption capacity; n is the adsorption intensity; Xm
is the DKR maximum adsorption capacity; E is the adsorption mean energy
The monolayer capacity, qm, for Pb (II) is appreciably high with
values of 11.07 and 10.14 mg g-1 compared to that of Mn (II) with
values of 3.8 and 7.79 mg g-1. The high b values for Pb more than
unity, corresponded to a strong bonding, probably chemically controlled sorption.
In the opposite, the weak b values for Mn, were an indication of physical interaction.
The Freundlich linear correlation coefficients were found R2>0.93
both for Mn (II) and Pb (II) (Table 4). Values of Freundlich
maximum multilayer capacity (KF) decreased for Mn (II) when Mn (II)
concentrations increase while KF for Pb (II) decreased when Pb (II)
ions concentration de creased. That is an illustration of competitive adsorption
between Mn (II) and Pb (II) on sorption sites. The values of Freundlich intensity;
n, remained were found higher than unity in conformity with the requirement
of favourable adsorption. The fact that Pb n values were found more high than
those of Mn implied that, Pb (II) ions followed a chemical sorption process
contrary to Mn (II) ions adsorption which was physical (Ijagbemi
et al., 2009).
Parameters of D.K.R isotherm indicated that this model fitted also the adsorption experimental data, with its all correlation coefficients R2>0.98 (Table 4). The saturation limit, Xm, representing the total specific micropore volume of the clay, diminished for Mn (II) from 68.854 to 23.543 mg g-1 when the Mn percentage rised from 51.1 to 68.78%, (Mn initial concentration increased from 74.814 to 124.44 mg L-1) and for Pb (II) from 14.525 to 11.213 mg g-1 when Pb initial concentration decreased from 71.329 to 56.448 mg L-1. The sorption energy E worked out by using the following relationship was determined:
For Mn (II) and Pb (II), the sorpti on energy (E) varied respectively from
-4.18 to -5.913 kJ mol-1 and -9.805 to -9.533 kJ mol-1.
This is an indication that Mn2+ and Pb2+ sorption reactions
are respectively physically and chemically controlled (Saeed
et al., 2003).
Values of adsorption parameters found were in good agreement with those reported
by other workers. Taty-Costodes et al. (2003),
found Langmuir adsorption capacity, qm, from studies of adsorption
of Pb (II) and Cd (II) on sawdust, between 8.45 and 22.22 mg/g in the pH range
7-4 (R2 = 0.91-0.99) for Pb (II) adsorption. Gupta
and Bhattacharyya, 2008 have reported Freundlich adsorption capacity, KF,
as 0.4-7.5 mg g-1 for adsorption of Pb (II) on kaolinite and on montmorillonite
respectively (R2 = 0.99, n = 0.7). Eba et
al. (2010) studied the adsorption of Mn (II) on clay from Bikougou in
single system. Their results showed the decrease of Mn (II) monolayer capacity,
great increase of multilayer capacities and weak adsorption mean energy of Mn
(II) in bi-solute system of Mn (II)-Pb (II). This is a consequence of mutual
effect observed when numerous cations compete in multi-component system to adsorption
sites. In this case, some metals ions are preferably adsorbed in comparison
to other metals ions.
In a multi-element system of heavy metals in which previous experiments concerning
sorption of single metal ions are not realized, the comparison of percentages
for each metal, in initial solution and on solid surface at the equilibrium
could help, using the sign of deviation, to appreciate the selectivity of clay
surface for a given metal. The ratio in initial solution should be found equal
to that on the adsorbent surface. A positive value of deviation indicates a
promoted adsorption of this ion metal compared to the other ions metal. Table
5 presents comparison of percentages of Mn (II) and Pb (II) in initial solution
and on adsorbent surface.
||Comparison between initial percentages of Mn (II) and Pb (II)
in aqueous solution and percentages of amount adsorbed of Mn (II) and Pb
(II) on clay. pH 4; 0.15 g of clay; temperature 308 K; interaction time
When the initial percentage values of Mn (II) increased from 51.19 to 68.79%,
those of its amounts adsorbed increase from 42.89% with a deviation of -18 %,
to 56.83 % with a deviation of -17.39%. Pb (II) initial percentage values in
aqueous solution decrease from 48.81, to 31.21% with the corresponding ratio
of amounts adsorbed decreasing relatively from 57.1051% with a deviation of
14.52, to 43.17% with a deviation of 38.32%. It is demonstrated the promoted
adsorption of Pb (II) as compared to that decreasing of Mn (II) in a binary:
Pb(II)-Mn (II) solution According to our results, in which Pb (II) ions are
selectively adsorbed than Mn (II) ions, the selectivity in adsorption ions on
adsorbent surface has been reported by other workers. Thus, in binary systems
(Cd (II) / Zn (II), Zn (II) / Pb (II) and Cd (II) / Pb (II)) natural zeolite
as adsorbent, selectively binds these ions according to the sequence Pb (II)>Cd
(II)>Zn (II) (Minceva et al., 2007). The same
selectivity is obtained on the binary and ternary systems involving the same
ions adsorption on montmorillonite (Stefan et al.,
2008). However, selectivity was not observed during the adsorption of lead
and manganese on kaolinite by Kamel et al. (2004),
indicating that both Mn (II) and Pb (II) were determined quantitatively at the
same level. In opposite, Chotpantarat et al. (2011)
found in a multi-system of Pb (II), Ni (II), Mn (II) and Zn (II) that Pb (II)
is more adsorbed on a lateritic soil than Mn (II).
These results show the importance of to keep account of the percentages of each metal ion, in initial solution and at equilibrium on adsorbent surface and also that of the resulted deviation, to establish the selectivity of a clay surface for some metal ions in a multi-element system. A positive deviation of a metal, i, in multi-system, proves that the sorption of this metal is promoted by the presence of the other metals. If deviation of a metal, i, is equal to zero, metals had no effect on each other. When the negative deviation is obtained, metal, i, competes with the other metals for available sorption sites of adsorbent. It is obtained that, in a binary Mn (II)-Pb (II) solution, the adsorption of Pb (II) is enhanced by Mn (II),while Mn (II) ions compete with those of Pb (II) to sorption sites on the clay surface.
The selectivity of heavy metal ions on adsorbent surface depends on the metal ions characteristics and of accessibility to adsorption and/or exchange sites of clay.
Metal ion with higher electronegativity would be fixed more readily than that
possessing low electro negativity. According to the electro negativity, Pb (II)
(2.33) might be more adsorbed on negatively charged clay surface than Mn (II)
(1.56) (Bernard and Busnot, 1996) in conformity with our
results where Pb (II) ions were more selectively adsorbed than Mn (II) ions.
Adsorption and exchange process might depend of size of hydrated metal ions.
The metal ions with larger ionic hydrated radius have lower charge density and
lower electrostatic attraction, which limits the interaction of these metal
ions with the adsorption sites. In this case, Pb (II) with smaller hydrated
radius such 0.187nm would be more adsorbed on the adsorbent sites than Mn (II)
which shows higher hydrated radius of 0.235 nm (Chotpantarat
et al., 2011).
|| Parameters of Langmuir, Freundlich and DKR equation types
|Where: P0 is the ratio of metal ions in initial
bi-solute solution; Pexp is the ratio of metal ions on solid
surface; PL is a maximum ratio of a metal ions on solid surface
as given by Langmuir equation type; b is energetic constant of Langmuir
equation type; RL is a separation factor of Langmuir equation
type; R2 is a correlation coefficients; PF is a maximum
ratio of a metal ions adsorbed as given by Freundlich equation type; n is
adsorption intensity constant as given by Freundlich equation type; PDR
is a maximum ratio of concentration surface of metal ions as given by DKR
equation type and e is mean energy of the adsorption process
This is in good agreement with our results indicating the preferable adsorption
of Pb (II) in the bi-solute Mn (II)-Pb (II) system. Because of the absence of
data on single metal adsorption on the clay, competitive adsorption equations
have been tested by substituting the amount of metal adsorbed per unit weight
by the metal ratio adsorbed in the classic Langmuir, Freundlich and D.K.R isotherm
equations. The results are presented in Table 6. The Langmuir
equation type gives a best fit of experimental data according to the requirement
of favorable adsorption. Freundlich and D.K.R equations types give very weak
correlation coefficients and so that, these models fit wrongly the experimental
data. For the Mn (II) experimental ratio of 42.89 and 56.83% obtained at equilibrium
on the adsorbent surface correspond, according to Langmuir equation type, Mn
(II) maximum ratio of monolayer adsorption of 23.81% (R2 = 0.9868)
and 45.25 % (R2 = 0.9461) respectively. The rest is assigned to multilayer
adsorption. It is demonstrated that, when in initial solution, the ratio of
Mn (II) increases, the part of Mn (II) ions adsorbed on monolayer than on multilayer
sites rises. As observed with classic isotherms, when the Mn (II) and Pb (II)
ions compete for the attainment of adsorption sites, Pb (II) preferably fixed
on adsorption monolayer sites and Mn (II) on adsorption multilayer sites is
also described well by using the Langmuir equation type.
Kinetics studies: Assuming a pseudo second order kinetic model (Ho
and McKay, 1999a; Hanafiah et al., 2006).
The plots t/qt vs t (Fig. 6) was linear and indicated
the best applicability of this model to experimental results. All the linear
correlation coefficients (R2) were found greater than 0.99 in conformity
with the requirement (R2 = 1) of the validity of a kinetic model
(Al-Futaisi et al., 2007). As summarized in Table
7, the kinetic rate constants k2 (g/min.g) decreased for Mn (II)
from 10.157 to 0.917 when its percentages in bi-solute solution increased from
51.19 to 68.79%. In the same conditions, adsorption rate constants of Pb (II)
ions increased from 4.208 to 13.697 g/min.g. This demonstrates that, the adsorption
rate constant value increases with the diminution of metal ion adsorbed as reported
by Eba et al. (2010). The high values of the
kinetic rate constant show that the adsorption reaction is fast on the surface
of this clay .The adsorption equilibrium is established after thirty minutes.
The comparison of amounts adsorbed of heavy metals, qe (mg g-1)
(obtained from the slope of the second-order plot) 16.155 and 24.62 mg g-1
for Mn (II) and 21.365 and 18.66 for Pb (II), and experimental (qexp)
16.0511 and 24.508 mg g-1 for Mn (II), and 21.367 and 627 mg g-1
for Pb (II) respectively, shows that the simultaneous adsorption process of
Mn (II) and Pb (II) in aqueous solution followed very accurately the pseudo
second order kinetic model, because deviation is lower than 1% in the solution
of 51.19% of Mn (II) content.
||Plots related to variations of the ratio between adsorbent-adsorbat
contact time (t, min) on the amount adsorbed per specified amount of adsorbent
(Qt, mg g-1) as a function of time for simultaneous
removal of Mn (II) and Pb (II) (with Mn percentage of 51.19%; pH 4, 303
K and clay 3 g L-1)
||The pseudo second order kinetic parameters for the simultaneous
adsorption of the simultaneous adsorption of Mn (II) and Pb (II) ions at
303K (pH 4, clay 3 g L-1)
|Where: qex is the experimental equilibrium amount
of Mn (II) Pb (II) adsorbed per specified amount of adsorbent; qe in mg
g-1, is the equilibrium amount of Pb (II) adsorbed per specified
amount of adsorbent obtained by calculation from the second order kinetics
model; k2 is rate constant; R2 is the correlation
The deviation still existing (between 4.5 and 7.5% in solution of 68.78% of
Mn (II) content) might be due to the uncertainty inherent in obtaining the experimental
This study showed that the natural clay originated from Bikougou deposit is a mixture of kaolinite-albite-montmorillonite-illite clayey minerals and has a great potential as adsorbent exploited here in simultaneous removal of Mn (II) and Pb (II) ions from aqueous solutions. The adsorptions isotherms have revealed that Langmuir, Freundlich and DKR adsorption isotherm models fitted well the experimental results. Pb seemed more adsorbed on monolayer surface and Mn is preferentially adsorbed on multilayer heterogeneous surface. Experimental data have proved every time,that the equilibrium ratio of Pb(II) on solid surface is higher than that in initial bi-metal ions solution. That is a consequence of the promoted adsorption of Pb(II) .Contrary results have been obtained with Mn(II).
The theoretical maximum amounts of simultaneous Mn (II) and Pb (II) ions adsorbed are obtained by using D.K.R model. The values of adsorption mean energy are referring for Mn (II) to a physical process and for Pb (II) to a chemically controlled interaction. The simultaneous removal of Mn (II) and Pb (II) ions on the surface of the clay followed a pseudo second order kinetic model. The adsorption rate constants for Mn (II) decreased and those of Pb (II) increased when the percentage of Mn in the bi-metal solution of Mn (II) and Pb (II) increased.
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