# Evaluation of the Use ofAcacia nilotica Leaf as an Ecofriendly Adsorbent for Cr (VI) and Its Suitability in Real Waste Water: Study of Residual Errors

Authors: Ashly Leena Prasad; Santhi Thirumalisamy
Journal: Journal of Chemistry
 (2013)

---

## Abstract

The present paper aims to investigate the physical characteristics ofAcacia nilotica leaves (MVM) relative to their use as an adsorbent for removal of hazardous Cr (VI) from waste water. The adsorbent was characterized by FTIR and SEM studies. The applicability of the Langmuir model to MVM was proved by the high coefficient of determination. Eight error analysis methods, namely, residual root mean square error (RMSE), chi-square (χ2), sum of the square of the errors (ERRSQ), composite functional error (HYBRD), derivative of Marquardt's percent standard deviation (MPSD), average relative error (ARE), sum of absolute error (EABS), and average percentage error (APE) were used to evaluate the suitability of the adsorption isotherm. Desorption reveals that recovery of the metal from adsorbent was possible. The ecofriendly adsorbent MVM is expected to be an environmentally and economically feasible adsorbent for the removal of Cr (VI) from aqueous solution and real waste water.


---

## Body

## 1. Introduction

Mobilization of heavy metals in the environment due to industrial activities is of serious concern as these metals are toxic to all forms of life including humans [1]. Chromium compounds are widely used in various industries, such as, electroplating, metal finishing, leather tanning, and chromate preparation, and as a result they are often found in industrial waste waters [2]. Chromium occurs in natural water is in two main oxidation states, Cr (III) and Cr (VI). Although Cr (III) is an essential nutrient in mammalian metabolism, Cr (VI) is highly toxic and mutagenic. The recommended limit for Cr (VI) in potable water is 0.05 mg dm−3. Acacia nilotica is a species of Acacia, native to Africa and the Indian subcontinent. In Haryana, Acacia-nilotica-based agro forestry systems reduced the yield of wheat [3]. In this paper the preparation, characterization, and the adsorption properties of microwave activated carbon from Acacia nilotica leaves are discussed. The microwave activation method was used because of its one-step simple process.


## 2. Experimental

### 2.1. Preparation and Characterization of Sorbent

The leaves ofAcacia nilotica were obtained from Coimbatore district (Tamilnadu), were washed with distilled water, air-dried, and heated in a microwave oven (Samsung; Triple Distribution System) at 800 W for 5 minutes. The carbonized sample (MVM) was crushed into granules, sieved to different particle sizes (125 to 250 μm), and then preserved in an air-tight container for further studies. The surface morphology and fundamental physical properties of the sorbent were obtained by the scanning electron microscope (LEO 435 VP model) and Fourier Transform Infrared (FTIR) analysis (Shimadzu spec).Determination of zero point charge (pHzpc) was done to investigate the surface charge of the adsorbent. For the determination of pHzpc, 1 g of the sample suspension (particle size: 125 to 250 μm) was prepared in 50 mL solution of sodium nitrate electrolyte of concentration 10−2 M. The aliquots of suspension were adjusted to various pH values with dilute NaOH and HNO3 solution. After 60 minutes for equilibrium, the initial pH value is measured.Then 1 g of NaNO3 was added to each aliquot to bring final electrolyte concentration to about 0.45 M.After an additional 60 minutes agitation, final pH was measured. The results were plotted with ΔpH (final pH − initial pH)against final pH. The point of intersection of the resulting curve with abscissa, at which pH = 0, gave the pHzpc [4].


### 2.2. Metal Uptake Experiments and Determining Isotherm Parameters by Nonlinear Regression

The stock solution (3.39 mmol/L) was prepared by dissolving 2.827 g of potassium dichromate (K2Cr2O7) in double-distilled water. For each isotherm, a series of flasks were prepared with known volumes of serial dilutions of standardized metal salt solutions (2.03, 2.37, 2.71, 3.05, and 3.39 mmol/L, resp.). The pH was adjusted with 0.1 M HCl or 0.1 M NaOH (pH from 2 to 8) by 1,5-diphenylcarbazide method was measured using a pH meter (Deluxe pH meter, model-101 E, Innolab India) with a combined glass electrode calibrated with buffer. About 0.4 g of the sorbent was added, and the flasks were agitated at 160 rpm for 90 minutes. The sorbent was removed by centrifugation, and the supernatant was analyzed. The concentration was measured by using direct UV-vis spectrophotometric method using a Systronic Spectrophotometer-104 at wavelength of 430 nm. Desorption studies were carried out by filtering the metal loaded adsorbent with distilled water and adjusting the initial pH values from 2 to 7. The desorbed Cr (VI) in the solution was separated by centrifugation and analyzed and the % of desorption was calculated.The amount of metal adsorbed at equilibrium [qe (mmolg−1)] onto carbon was calculated by the following mass balance relationship:
(1)qe=(C0-Ce)V/W,
where, C0 and Ce are the concentrations (mmolL−1) of Cr (VI) at initial and at equilibrium, respectively. V is the volume (L) of the solution and W is the weight (g) of the adsorbent used.Nonlinear analysis of isotherm data is an interesting mathematical approach for describing adsorption isotherms at constant temperature for water and waste water treatment and to predict the overall sorption behavior under different operating conditions [5]. The error functions employed were as follows.(i)
Residual root mean square error (RMSE) is(2)1n-2∑i=1N(qeexp⁡-qecal)2.(ii)
TheX-square test is
(3)x2=∑i=1N(qeexp⁡-qecal)2qecal.If data from the model are similar to the experimental data, thenχ2  will be a smaller number; if they are different, then χ2 will be a large number. The subscript “exp” and “cal” shows the experimental and calculated values, and N is the number of observations in the experimental data. The smaller the RMSE value, the better the curve fitting [6].(iii)
The sum of the square of the errors (ERRSQ) is(4)∑i=1N(qeexp⁡-qecal)i2.(iv)
A composite fractional error function (HYBRD) is(5)∑i=1N[(qeexp⁡-qecal)2qeexp⁡]i.(v)
A derivative of Marquardt’s percent standard deviation (MPSD) is(6)∑i=1N[(qeexp⁡-qecal)qeexp⁡]i2.(vi)
The average relative error (ARE) is(7)∑i=1N[(qeexp⁡-qecal)qeexp⁡]i.(vii)
The sum of absolute error (EABS) is(8)∑i=1N[qeexp⁡-qecal]i.(viii)
The average percentage error (APE) is(9)∑i=1N[(qeexp⁡-qecal)/qeexp⁡]iN×100.The calculation method for the “sum of the normalized errors” was as follows.(a)
Select one isotherm and one error function and determine the isotherm parameters that minimize the error function for that isotherm to produce the isotherm parameter set for that error function.(b)
Determine the values for all the other error functions for that isotherm parameter set,calculate all other parameter sets and all their associated error function values for that isotherm.(c)
Select each error measure in turn and the ratio of the value of that error measure for a given parameter set to the largest value of that error from all the parameter sets for that isotherm.(d)
Get sum all these normalized errors for each parameter set.The parameter set thus providing the smallest normalized error sum can be considered to be optimal for that isotherm provided.


## 2.1. Preparation and Characterization of Sorbent

The leaves ofAcacia nilotica were obtained from Coimbatore district (Tamilnadu), were washed with distilled water, air-dried, and heated in a microwave oven (Samsung; Triple Distribution System) at 800 W for 5 minutes. The carbonized sample (MVM) was crushed into granules, sieved to different particle sizes (125 to 250 μm), and then preserved in an air-tight container for further studies. The surface morphology and fundamental physical properties of the sorbent were obtained by the scanning electron microscope (LEO 435 VP model) and Fourier Transform Infrared (FTIR) analysis (Shimadzu spec).Determination of zero point charge (pHzpc) was done to investigate the surface charge of the adsorbent. For the determination of pHzpc, 1 g of the sample suspension (particle size: 125 to 250 μm) was prepared in 50 mL solution of sodium nitrate electrolyte of concentration 10−2 M. The aliquots of suspension were adjusted to various pH values with dilute NaOH and HNO3 solution. After 60 minutes for equilibrium, the initial pH value is measured.Then 1 g of NaNO3 was added to each aliquot to bring final electrolyte concentration to about 0.45 M.After an additional 60 minutes agitation, final pH was measured. The results were plotted with ΔpH (final pH − initial pH)against final pH. The point of intersection of the resulting curve with abscissa, at which pH = 0, gave the pHzpc [4].


## 2.2. Metal Uptake Experiments and Determining Isotherm Parameters by Nonlinear Regression

The stock solution (3.39 mmol/L) was prepared by dissolving 2.827 g of potassium dichromate (K2Cr2O7) in double-distilled water. For each isotherm, a series of flasks were prepared with known volumes of serial dilutions of standardized metal salt solutions (2.03, 2.37, 2.71, 3.05, and 3.39 mmol/L, resp.). The pH was adjusted with 0.1 M HCl or 0.1 M NaOH (pH from 2 to 8) by 1,5-diphenylcarbazide method was measured using a pH meter (Deluxe pH meter, model-101 E, Innolab India) with a combined glass electrode calibrated with buffer. About 0.4 g of the sorbent was added, and the flasks were agitated at 160 rpm for 90 minutes. The sorbent was removed by centrifugation, and the supernatant was analyzed. The concentration was measured by using direct UV-vis spectrophotometric method using a Systronic Spectrophotometer-104 at wavelength of 430 nm. Desorption studies were carried out by filtering the metal loaded adsorbent with distilled water and adjusting the initial pH values from 2 to 7. The desorbed Cr (VI) in the solution was separated by centrifugation and analyzed and the % of desorption was calculated.The amount of metal adsorbed at equilibrium [qe (mmolg−1)] onto carbon was calculated by the following mass balance relationship:
(1)qe=(C0-Ce)V/W,
where, C0 and Ce are the concentrations (mmolL−1) of Cr (VI) at initial and at equilibrium, respectively. V is the volume (L) of the solution and W is the weight (g) of the adsorbent used.Nonlinear analysis of isotherm data is an interesting mathematical approach for describing adsorption isotherms at constant temperature for water and waste water treatment and to predict the overall sorption behavior under different operating conditions [5]. The error functions employed were as follows.(i)
Residual root mean square error (RMSE) is(2)1n-2∑i=1N(qeexp⁡-qecal)2.(ii)
TheX-square test is
(3)x2=∑i=1N(qeexp⁡-qecal)2qecal.If data from the model are similar to the experimental data, thenχ2  will be a smaller number; if they are different, then χ2 will be a large number. The subscript “exp” and “cal” shows the experimental and calculated values, and N is the number of observations in the experimental data. The smaller the RMSE value, the better the curve fitting [6].(iii)
The sum of the square of the errors (ERRSQ) is(4)∑i=1N(qeexp⁡-qecal)i2.(iv)
A composite fractional error function (HYBRD) is(5)∑i=1N[(qeexp⁡-qecal)2qeexp⁡]i.(v)
A derivative of Marquardt’s percent standard deviation (MPSD) is(6)∑i=1N[(qeexp⁡-qecal)qeexp⁡]i2.(vi)
The average relative error (ARE) is(7)∑i=1N[(qeexp⁡-qecal)qeexp⁡]i.(vii)
The sum of absolute error (EABS) is(8)∑i=1N[qeexp⁡-qecal]i.(viii)
The average percentage error (APE) is(9)∑i=1N[(qeexp⁡-qecal)/qeexp⁡]iN×100.The calculation method for the “sum of the normalized errors” was as follows.(a)
Select one isotherm and one error function and determine the isotherm parameters that minimize the error function for that isotherm to produce the isotherm parameter set for that error function.(b)
Determine the values for all the other error functions for that isotherm parameter set,calculate all other parameter sets and all their associated error function values for that isotherm.(c)
Select each error measure in turn and the ratio of the value of that error measure for a given parameter set to the largest value of that error from all the parameter sets for that isotherm.(d)
Get sum all these normalized errors for each parameter set.The parameter set thus providing the smallest normalized error sum can be considered to be optimal for that isotherm provided.


## 3. Results and Discussion

SEM studies (Figure1) show that MVM have considerable number of heterogeneous pores, where there is a good possibility for adsorbate to be trapped and adsorbed [7]. The FTIR spectrum of MVM (Figure 2) shows that the band at 3412 cm−1 represents the presence of –OH and –NH groups. The band observed at 2926 cm−1 and at 2856 cm−1 represents the presence of asymmetric and symmetric stretching vibrations of –CH group [8]. The bands at 1637 and 1452 cm−1 indicate the presence of –COO, –C=O, and –NH groups. The peak at 1564 cm−1 is attributed to the formation of oxygen functional groups, such as, a highly conjugated C–O stretching in carboxylic groups and due to the presence of quinone structure. The bands at 1390 to 1408 cm−1 assigned to C–H bending in alkanes or alkyl groups were observed. The broad band between 1325 and 1109 cm−1 has been assigned to C–O stretching in alcohols and phenols [9]. The band at 1261 cm−1 implied the C–N stretching of Amide ||| is present in MVM. The characteristics of MVM are presented in (Table 1).Table 1
Physicochemical characteristics of MVM.
Parameters
Values
Moisture content (%)
8.713
Ash content (%)
9.950
pH
7.020
Decolorizing power (mgg−1)
1.200
Specific gravity
1.220
Matter soluble water (%)
12.44
Conductivity (μscm−1)
0.260
Zero-point charge (pHzpc)
4.400
Apparent density (gmL−1)
0.272Figure 1
SEM image of MVM.Figure 2
FTIR spectra of MVM.The maximum adsorption capacity for Cr (VI) was observed at pH 6, as depicted in Figure3. The effect of solution pH is very important when the adsorbing molecules are capable of ionizing in response to the current pH. Activated carbons are material that has amphoteric characteristics, so the pH on its surface always changes depending on initial pH of the solution. Generally, the adsorption capacity and the rate constant have the tendency to increase as initial pH of the solution increases. When solution pH increases, high OH− ions accumulate on the adsorbent surface [8]. Therefore, electrostatic interaction between negatively charged adsorbent surface and cationic metal molecule caused the increase in adsorption. The optimum pH value of Cr (VI) onto MVM was 6 pH, and it was used for the subsequent experiments.Figure 3
Percentage of adsorption and desorption of Cr (VI) onto MVM.The equilibrium isotherms are used to describe experimental data. The adsorption isotherm is important from both a theoretical and a practical point of view. To optimize the design of an adsorption system it is important to establish the most appropriate correlation for the equilibrium curves [10]. The equation parameters of these equilibrium models often provide some insight into the sorption mechanism, the surface properties, and affinity of the adsorbent [11]. The adsorption isotherm equations like Langmuir, Freundlich, Dubinin-Radushkevich (D-R), and Temkin were used to describe the equilibrium characteristics of the adsorption.The Langmuir isotherm theory assumes monolayer coverage of adsorbate over a homogeneous adsorbent surface [12]. Once a metal molecule occupies a site, no further adsorption can take place at that site. It is commonly expressed as follows:
(10)qe=(QmKaCe)(1+KaCe).
The Langmuir isotherm equation (10) can be linearized into the following form [13]:
(11)Ceqe=1KaQm+(1Qm×Ce),
where qe and Ce are defined before in (1), Qm is a constant, reflecting a complete monolayer (mgg−1); Ka is adsorption equilibrium constant (Lmg−1) that is related to the apparent energy of sorption. A plot of Ce/qe versus Ce should indicate a straight line of slope 1/Qm and an intercept of 1/(KaQm).The result obtained from the Langmuir model for the removal of Cr (VI) onto MVM is shown in Table2. The related error function values are shown in Table 3. These values are near the experimental adsorbed amounts and correspond closely to the adsorption isotherm plateau, which is acceptable. The correlation coefficient (R2=0.9984) showed strong positive evidence on the adsorption follows the Langmuir isotherm.Table 2
Isotherm constants for Cr (VI) adsorption onto 0.4 g of MVM.
Isotherm model
Values
Langmuir
Qm (mgg−1)
69.4440
b (Lmg−1)
0.0296
R2
0.9984
Freundlich
1/n
0.1079
Kf (mgg−1)
33.3960
R2
0.9501
Dubinin-Radushkevich
Qm (mgg−1)
64.3894
K (mol2kJ−2)
0.0004
E (kJmol−1)
0.0353
R2
0.8395
Temkin
α (Lg−1)
40.3360
β (mgL−1)
6.5784
b
379.1499
R2
0.9460Table 3
Values of error function of the isotherm models of Cr (VI) onto MVM.
Error function model
Isotherm model
Langmuir
Freundlich
D-R
Temkin
RMSE
13.918
14.3534
14.012
14.3268
χ
2
3.2 × 10−7
4.2 × 10−3
9.2 × 10−4
3.9 × 10−3
ERRSQ
2.0 × 10−5
0.2615
0.0570
0.2455
HYBRD
3.2 × 10−7
4.2 × 10−3
9.2 × 10−4
3.9 × 10−3
MPSD
5.3 × 10−9
6.9 × 10−5
1.5 × 10−5
6.4 × 10−5
ARE
7.3 × 10−5
8.3 × 10−3
3.8 × 10−3
8.0 × 10−3
EABS
0.0045
0.5114
0.2388
0.4955
APE
1.4 × 10−3
0.1663
0.0776
0.1612The Freundlich isotherm [9] can be applied to nonideal adsorption on heterogeneous surfaces as well as multilayer sorption. The Freundlich isotherm can be derived assuming a logarithmic decrease in enthalpy of adsorption with the increase in the fraction of occupied sites and is commonly given by the following nonlinear equation:
(12)qe=KFCe1/n.
Equation (12) can be linearized in the logarithmic form (13), and the Freundlich constants can be determined:
(13)log⁡qe=log⁡KF+1nlog⁡Ce.
A plot of log qe versus log Ce enables us to determine the constant Kf and 1/n. Kf is roughly an indicator of the adsorption capacity, related to the bond energy, and 1/n is the adsorption intensity of Cr (VI) onto the adsorbent of surface heterogeneity. The magnitude of the exponent, 1/n, gives an indication of the favorability of adsorption. A value for 1/n below one indicates a normal Langmuir isotherm, while 1/n above one is indicative of cooperative adsorption [14] and is equal to 0.1079. It is lower than the experimental amounts corresponding to the adsorption isotherm plateau, which is unacceptable.The D-R isotherm was also applied to estimate the porosity apparent free energy and the characteristics of adsorption [15, 16]. It can be used to describe adsorption on both homogenous and heterogeneous surfaces [17]. The D-R equation can be defined by the following equation:
(14)ln⁡qe=ln⁡Qm-Kε2,
where K is a constant related to the adsorption energy, Qm the theoretical saturation capacity, and ε is the Polanyi potential, calculated from (15),
(15)ε=RTln⁡(1+1Ce),
where Ce is the equilibrium concentration of Cr (VI) (molL−1), R is the gas constant (8.314 J mol−1 K−1), and T is the temperature (K). By plotting lnqe versus ε2, it is possible to determine the value of K from the slope and the value of Qm (mgg−1) from the intercept. The mean free energy E (kJmol−1) of sorption can be estimated by using K values as expressed in the following equation [18]:
(16)E=12K.
The parameters obtained using the above equations are summarized in Table 2. The saturation adsorption capacity Qm obtained using the D-R isotherm model is 64.3894 mgg−1. The E value calculated using (16) is 0.0353 kJmol−1 for Cr (VI) adsorption onto MVM. This indicated that the physical adsorption plays the significant role in the uptake of Cr (VI) onto MVM [18]. The error functions indicate that the D-R isotherm is not fit in this adsorption.Temkin and Pyzhey [19] considered the effects of some indirect adsorbate or adsorbate interactions on adsorption isotherms and suggested that because of these interactions the heat of adsorption of all the molecules in the layer would decrease linearly with coverage. The Temkin isotherm has commonly been applied in the following form:
(17)qe=RTbln⁡(ACe).
The Temkin isotherm equation (17) can be simplified to the following equation:
(18)qe=βln⁡α+βln⁡Ce,
where
(19)β=(RT)b.The constantβ is related to the heat of adsorption [20]. The adsorption data were analyzed according to the linear form of Temkin isotherm equation (18). The linear isotherm constants and coefficients of determination are presented in Table 2. The correlation coefficients R2 obtained from Temkin model were comparable to that obtained for Langmuir and Freundlich equations, which explains the applicability of Temkin model to the adsorption of Cr (VI) onto MVM.It can be seen that the Langmuir isotherm fits the data better than Freundlich, D-R, and Temkin isotherms. This is also confirmed by the high value ofR2 in case of Langmuir. Moreover, among the eight errors analysis methods the Langmuir shows smaller value, which describes the better the curve fitting.Over the past few decades, linear regression has been developed as a major option in designing the adsorption systems. However, recent investigations have indicated the growing discrepancy (between the predictions and experimental data) and disability of the model, propagating towards a different outcome. However, the expanding of the nonlinear isotherms represents a potentially viable and powerful tool, leading to the superior improvement in the area of adsorption science [21].


### 3.1. Desorption Studies

Regeneration of the adsorbent may make the treatment more economical and feasible. Desorption studies help to elucidate the mechanism of metal adsorption and recycling of the spent adsorbent and the metal. If the adsorbed metal can be desorbed using neutral pH water, then the attachment of the metal to the adsorbent is by weak bonds. The adsorption capacity and rate constant have the tendency to increase as initial pH of the solution increases. This is due to the pHzpc (4.4) of the adsorbents, which has an acidic value; this is favorable for cation adsorption [22]. At pH above 4.4, the carboxyl groups are deprotonated and as such are negatively charged. These negatively charged carboxylate ligands (–COO−) can attract the positively charged Cr (VI) molecules, and binding can occur. Thus the Cr (VI)+1 binding to the MVM may be ion-exchange mechanism, which may involve electrostatic interaction between the negatively charged groups in the cell walls and the metal cationic molecules. The maximum desorption of Cr (VI) onto MVM (22.34%) is obtained at 3 pH (Figure 3).


### 3.2. Suitability of MVM onto Real Industrial Waste Water

The industrial waste water was collected locally from a metal finishing industry in Tirupur near to Coimbatore. The adsorption technique was carried out in the real waste water onto MVM, in order to remove the toxic metal from water. The effect of pH, adsorption dosage, and desorption was investigated.In this study, Initial pH values were adjusted in the range of 2 to 8 before addition of the adsorbent. Figure4 show that the adsorption was highly pH dependent. The uptake increased with increasing pH up to a maximum (0.22 mmol/g at pH 6) and then decreased gradually. The optimum pH value (pH 6) was adjusted for further experiments.Figure 4
Percentage of adsorption and desorption of real industrial waste water onto MVM.The effect of changing adsorbent dosage on the adsorption rate of real industrial waste water was studied by varying the concentration of the sorbent from 0.4 g to 1 g while keeping the other experimental conditions constant. The percentage removal versus adsorbent dosage is shown in Figure5. An increase in the percentage of adsorption with increasing adsorbent dosage was observed.Figure 5
Effect of sorbent dose on the adsorption of real industrial waste water onto MVM.Desorption studies help to elucidate one mechanism of adsorption and recovery of the adsorbate and adsorbent. The maximum desorption of MVM from real industrial waste water is shown in Figure4. It suggests that the recovery of metal from the adsorbent was possible and it make the process more feasible.


## 3.1. Desorption Studies

Regeneration of the adsorbent may make the treatment more economical and feasible. Desorption studies help to elucidate the mechanism of metal adsorption and recycling of the spent adsorbent and the metal. If the adsorbed metal can be desorbed using neutral pH water, then the attachment of the metal to the adsorbent is by weak bonds. The adsorption capacity and rate constant have the tendency to increase as initial pH of the solution increases. This is due to the pHzpc (4.4) of the adsorbents, which has an acidic value; this is favorable for cation adsorption [22]. At pH above 4.4, the carboxyl groups are deprotonated and as such are negatively charged. These negatively charged carboxylate ligands (–COO−) can attract the positively charged Cr (VI) molecules, and binding can occur. Thus the Cr (VI)+1 binding to the MVM may be ion-exchange mechanism, which may involve electrostatic interaction between the negatively charged groups in the cell walls and the metal cationic molecules. The maximum desorption of Cr (VI) onto MVM (22.34%) is obtained at 3 pH (Figure 3).


## 3.2. Suitability of MVM onto Real Industrial Waste Water

The industrial waste water was collected locally from a metal finishing industry in Tirupur near to Coimbatore. The adsorption technique was carried out in the real waste water onto MVM, in order to remove the toxic metal from water. The effect of pH, adsorption dosage, and desorption was investigated.In this study, Initial pH values were adjusted in the range of 2 to 8 before addition of the adsorbent. Figure4 show that the adsorption was highly pH dependent. The uptake increased with increasing pH up to a maximum (0.22 mmol/g at pH 6) and then decreased gradually. The optimum pH value (pH 6) was adjusted for further experiments.Figure 4
Percentage of adsorption and desorption of real industrial waste water onto MVM.The effect of changing adsorbent dosage on the adsorption rate of real industrial waste water was studied by varying the concentration of the sorbent from 0.4 g to 1 g while keeping the other experimental conditions constant. The percentage removal versus adsorbent dosage is shown in Figure5. An increase in the percentage of adsorption with increasing adsorbent dosage was observed.Figure 5
Effect of sorbent dose on the adsorption of real industrial waste water onto MVM.Desorption studies help to elucidate one mechanism of adsorption and recovery of the adsorbate and adsorbent. The maximum desorption of MVM from real industrial waste water is shown in Figure4. It suggests that the recovery of metal from the adsorbent was possible and it make the process more feasible.


## 4. Conclusions

Results from this study confirmed that MVM can be used as a suitable biosorbent for Cr (VI) ions from aqueous solutions and in terms of real industrial waste water. The removal of Cr (VI) was highly dependent on solution pH. The equilibrium data were best described by the Langmuir isotherm model, exclusively for all the error function selection methods. The recycling ability of MVM reveals that recovery of Cr (VI) from adsorbent was possible. The desorption experiment suggests that the Cr (VI) sorption is generally of an irreversible nature, owing to strong interaction betweenCr2O72- and the surface active sites of the sorbent. Strong bonding between sorbate and sorbent does not make the regeneration of the sorbent economically viable. The Acacia niloticaleaves used in this work are freely and abundantly available. The preparation of MVM is agreeing with the principles of green chemistry, and it possesses high adsorption of Cr (VI) from aqueous solution and real industrial waste water.



---

*Source: 354328-2012-07-10.xml*