Evaluation of the Use of Acacia nilotica Leaf as an Ecofriendly Adsorbent for Cr ( VI ) and Its Suitability in RealWasteWater : Study of Residual Errors

epresent 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.e adsorbent was characterized by FTIR and SEM studies.e 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 (χχ), 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.e 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.


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 �nishing, leather tanning, and chromate preparation, and as a result they are oen 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.e 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.e microwave activation method was used because of its one-step simple process.

Experimental
2.1.Preparation and Characterization of Sorbent.e leaves of Acacia 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.e carbonized sample (MVM) was crushed into granules, sieved to different particle sizes (125 to 250 m), and then preserved in an air-tight container for further studies.e 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 (pH zpc ) was done to investigate the surface charge of the adsorbent.For the determination of pH zpc , 1 g of the sample suspension (particle size: 125 to 250 m) was prepared in 50 mL solution of sodium nitrate electrolyte of concentration 10 −2 M. e aliquots of suspension were adjusted to various pH values with dilute NaOH and HNO 3 solution.Aer 60 minutes for equilibrium, the initial pH value is measured.en 1 g of NaNO 3 was added to each aliquot to bring �nal electrolyte concentration to about 0.45 M.Aer an additional 60 minutes agitation, �nal pH was measured.e results were plotted with ΔpH (�nal pH − initial pH) against �nal pH.e point of intersection of the resulting curve with abscissa, at which pH = 0, gave the pH zpc [4].

Metal Uptake Experiments and Determining Isotherm
Parameters by Nonlinear Regression.e stock solution (3.39 mmol/L) was prepared by dissolving 2.827 g of potassium dichromate (K 2 Cr 2 O 7 ) in double-distilled water.For each isotherm, a series of �asks 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.).e 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 �asks were agitated at 160 rpm for 90 minutes.e sorbent was removed by centrifugation, and the supernatant was analyzed.e 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 �ltering the metal loaded adsorbent with distilled water and adjusting the initial pH values from 2 to 7. e desorbed Cr (VI) in the solution was separated by centrifugation and analyzed and the % of desorption was calculated.
e amount of metal adsorbed at equilibrium [  (mmolg −1 )] onto carbon was calculated by the following mass balance relationship: where,  0 and   are the concentrations (mmolL −1 ) of Cr (VI) at initial and at equilibrium, respectively. is the volume (L) of the solution and  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].e error functions employed were as follows.
(i) Residual root mean square error (RMSE) is ( (ii) e -square test is If data from the model are similar to the experimental data, then  2 will be a smaller number; if they are different, then  2 will be a large number.e subscript "exp" and "cal" shows the experimental and calculated values, and  is the number of observations in the experimental data.e smaller the RMSE value, the better the curve �tting [6].(iii) e sum of the square of the errors (ERRSQ) is (iv) A composite fractional error function (HYBRD) is (vi) e average relative error (ARE) is (vii) e sum of absolute error (EABS) is (viii) e average percentage error (APE) is e 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.
e parameter set thus providing the smallest normalized error sum can be considered to be optimal for that isotherm provided.

Results and Discussion
SEM studies (Figure 1) show that MVM have considerable number of heterogeneous pores, where there is a good possibility for adsorbate to be trapped and adsorbed [7].e FTIR spectrum of MVM (Figure 2) shows that the band at 3412 cm −1 represents the presence of -OH and -NH groups.e band observed at 2926 cm −1 and at 2856 cm −1 represents the presence of asymmetric and symmetric stretching vibrations of -CH group [8].e bands at 1637 and 1452 cm −1 indicate the presence of -COO, -C=O, and -NH groups.e 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.e bands at 1390 to 1408 cm −1 assigned to C-H bending in alkanes or alkyl groups were observed.e broad band between 1325 and 1109 cm −1 has been assigned to C-O stretching in alcohols and phenols [9].e band at 1261 cm −1 implied the C-N stretching of Amide ||| is present in MVM.e characteristics of MVM are presented in (Table 1).e maximum adsorption capacity for Cr (VI) was observed at pH 6, as depicted in Figure 3. e 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].erefore, electrostatic interaction between negatively charged adsorbent surface and cationic metal molecule caused the increase in adsorption.e optimum pH value of Cr (VI) onto MVM was 6 pH, and it was used for the subsequent experiments.e equilibrium isotherms are used to describe experimental data.e 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].e equation parameters of these equilibrium models oen provide some insight into the sorption mechanism, the surface properties, and affinity of the adsorbent [11].e adsorption isotherm equations like Langmuir, Freundlich, Dubinin-Radushkevich (D-R), and Temkin were used to describe the equilibrium characteristics of the adsorption.
e 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: e Langmuir isotherm equation ( 10) can be linearized into the following form [13]: where   and   are de�ned before in (1),   is a constant, re�ecting a complete monolayer (mgg  3. ese values are near the experimental adsorbed amounts and correspond closely to the adsorption isotherm plateau, which is acceptable.e correlation coefficient ( 2 = 0.9984) showed strong positive evidence on the adsorption follows the Langmuir isotherm.
e Freundlich isotherm [9] can be applied to nonideal adsorption on heterogeneous surfaces as well as multilayer sorption.e 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: Equation ( 12) can be linearized in the logarithmic form (13), and the Freundlich constants can be determined: A plot of log   versus log   enables us to determine the constant   and 1/.  is roughly an indicator of the adsorption capacity, related to the bond energy, and 1/ is the adsorption intensity of Cr (VI) onto the adsorbent of surface heterogeneity.e magnitude of the exponent, 1/, gives an indication of the favorability of adsorption.A value for 1/ below one indicates a normal Langmuir isotherm, while 1/ 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.e 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].e D-R equation can be de�ned by the following equation: where  is a constant related to the adsorption energy,   the theoretical saturation capacity, and  is the Polanyi potential, calculated from (15), where   is the equilibrium concentration of Cr (VI) (molL −1 ),  is the gas constant (8.314J mol −1 K −1 ), and  is the temperature ().By plotting ln   versus  2 , it is possible to determine the value of  from the slope and the value of   (mgg −1 ) from the intercept.e mean free energy  (kJmol −1 ) of sorption can be estimated by using  values as expressed in the following equation [18]: e parameters obtained using the above equations are summarized in Table 2. e saturation adsorption capacity   obtained using the D-R isotherm model is 64.3894 mgg −1 .e  value calculated using ( 16) is 0.0353 kJmol −1 for Cr (VI) adsorption onto MVM.is indicated that the physical adsorption plays the signi�cant role in the uptake of Cr (VI) onto MVM [18].e error functions indicate that the D-R isotherm is not �t 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.e Temkin isotherm has commonly been applied in the following form:  e Temkin isotherm equation ( 17) can be simpli�ed to the following equation: where e constant  is related to the heat of adsorption [20].e adsorption data were analyzed according to the linear form of Temkin isotherm equation (18).e linear isotherm constants and coefficients of determination are presented in Table 2. e correlation coefficients  2 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 �ts the data better than Freundlich, D-R, and Temkin isotherms.is is also con�rmed by the high value of  2 in case of Langmuir.Moreover, among the eight errors analysis methods the Langmuir shows smaller value, which describes the better the curve �tting.
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].

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.e adsorption capacity and rate constant have the tendency to increase as initial pH of the solution increases.is is due to the pH zpc (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.ese negatively charged carboxylate ligands (-COO − ) can attract the positively charged Cr (VI) molecules, and binding can occur.us 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.e maximum desorption of Cr (VI) onto MVM (22.34%) is obtained at 3 pH (Figure 3).

Suitability of MVM onto Real Industrial Waste Water.
e industrial waste water was collected locally from a metal �nishing industry in Tirupur near to Coimbatore.e adsorption technique was carried out in the real waste water onto MVM, in order to remove the toxic metal from water.e 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.Figure 4 show that the adsorption was highly pH dependent.e uptake increased with increasing pH up to a maximum (0.22 mmol/g at pH 6) and then decreased gradually.e optimum pH value (pH 6) was adjusted for further experiments.e 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.e percentage removal versus adsorbent dosage is shown in Figure 5.An increase in the percentage of adsorption with increasing adsorbent dosage was observed.
Desorption studies help to elucidate one mechanism of adsorption and recovery of the adsorbate and adsorbent.e maximum desorption of MVM from real industrial waste water is shown in Figure 4.It suggests that the recovery of metal from the adsorbent was possible and it make the process more feasible.

Conclusions
Results from this study con�rmed that MVM can be used as a suitable biosorbent for Cr (VI) ions from aqueous solutions and in terms of real industrial waste water.e removal of Cr (VI) was highly dependent on solution pH.e equilibrium data were best described by the Langmuir isotherm model, exclusively for all the error function selection methods.e recycling ability of MVM reveals that recovery of Cr (VI) from adsorbent was possible.e desorption experiment suggests that the Cr (VI) sorption is generally of an irreversible nature, owing to strong interaction between Cr 2 O 7 2− and the surface active sites of the sorbent.Strong bonding between sorbate and sorbent does not make the regeneration of the sorbent economically viable.e Acacia nilotica leaves used in this work are freely and abundantly available.e 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.

F 1 :
SEM image of MVM.

F 3 :
Percentage of adsorption and desorption of Cr (VI) onto MVM.

F 4 :
Percentage of adsorption and desorption of real industrial waste water onto MVM.
VI) onto MVM is shown in Table2.e related error function values are shown in Table −1);   is adsorption equilibrium constant (Lmg −1 ) that is related to the apparent energy of sorption.A plot of   /  versus   should indicate a straight line of slope 1/  and an intercept of 1/(    ).
T 3: Values of error function of the isotherm models of Cr (VI) onto MVM.