Separation of Spherical Nanosilica from Agricultural Wastes in Vietnam via Ultrasonic-Assisted Precipitation and Application for Effective Removal of Methylene Blue from Aqueous Solution

Agricultural wastes including bagasse and rice husk ashes are employed for synthesizing spherical nanosilica materials via the ultrasonic-assisted precipitation process in the present study. Te comparison between them and nanosilica prepared from pure sodium silicate is also carried out. Te role of the NH 4 OH:ethanol volume ratio is demonstrated. Te obtained nanosilica is characterized by modern methods including X-ray difraction (XRD), energy-dispersive X-ray spectroscopy (EDS), infrared spectroscopy (IR), scanning electron microscopy (SEM), and nitrogen adsorption/desorption isotherms (BET). Te nanosilica material is employed as an efective adsorbent for the removal of methylene blue (MB) from an aqueous solution. Te suitable pH and adsorbent dosage are determined at 8 and 0.375g · L − 1 . Te adsorption isotherm study is surveyed based on Langmuir and Freundlich isotherm models. Pseudo-second-order kinetic model and Weber–Morris intraparticle difusion model well describe the chemical nature of the adsorption. Te thermodynamic parameters of the reaction are determined based on the Van’t Hof equation.


Introduction
Water pollution is one of the serious and urgent problems not only in Vietnam but also globally, which is increasingly threatening human life and health because most rivers, ponds, and lakes in large urban areas are heavily polluted.One of the notable problems is the existence of toxic and nonbiodegradable organic pigments used in the dyeing industry that is able to accumulate in the organism and cause acute and chronic toxicity for human [1,2].Terefore, the treatment of these pollutants in wastewater is a hot issue in recent decades, and scientists have been studying to establish treatment technology for polluted water such as adsorption [3][4][5], biology combined oxidation-adsorption, or biology [6][7][8][9][10][11].Among them, adsorption is proven to be a method with many advantages such as low cost, simplicity, and high efciency [6][7][8][12][13][14].Te adsorbents used are nontoxic and environmentally friendly.
Te sources used for the synthesis of nanosilica can be natural such as rice husk, bagasse, coir, and mud [15,16,33] or pure chemicals such as sodium silicate salt and tetraethyl orthosilicate (TEOS) [34].Nanosilica synthesized from pure chemicals usually exhibits uniform particle size and high purity resulting in particles that do not agglomerate into larger particles [34].Tis is one of the important properties of nanomaterials.Besides, its large surface area leads to high adsorption capacity.However, the obtained nanosilica will be a high-cost product.From this limitation, many researches on the synthesis of nanosilica from cheap raw materials are performed [35].
In Vietnam and many agricultural countries, rice husk and bagasse are cheap and quality sources for nanosilica extraction [36,37].Tese redundant agricultural wastes are discharged in all provinces and villages where they are mainly used as domestic raw fuel.Te secondary waste of rice husk ash (RHA) and bagasse ash (BA) is responsible for domestic water pollution [38].Terefore, studies on the formation of useful nanosilica from RHA (RHA-SiO 2 ) and BA (BA-SiO 2 ) are necessary.
Among the silica synthesis methods, precipitation is proven to be easy and efective.In comparison with other methods, it ofers the high purity of silica, the simplicity at low temperatures in cheap equipment, the time saving, and the low cost of the product [35,39,40].However, the morphology and particle size could not be controlled with the only common precipitation agent of acid.
In previous studies, the comparison of the structure and adsorption capacity of pollutants from aqueous solution between spherical RHA-SiO 2 and BA-SiO 2 has not been made fully [15,16,36,39,41].In this study, nanosilica is separated from rice husk and bagasse collected from Phu Vang district, Tua Tien Hue province, Vietnam, by ultrasonic-assisted precipitation process with the appearance of mixture of NH 4 OH : ethanol.Te nature of the methylene blue adsorption process onto the obtained material is clarifed.Besides, the comparison of the characteristics of two obtained nanosilica materials with this material prepared from pure sodium silicate and their methylene blue (MB) adsorption capacity is carried out.

Experimental Setup
2.1.Materials.Rice husk and bagasse were collected in Phu Vang district, Tua Tien Hue province, Vietnam.After being washed with water, the rice husk and bagasse were dried and calcined at 500 °C for 3 hours to obtain RHA and BA.
Liquid glass solution was synthesized from ash by soaking the ash in NaOH (Sigma-Aldrich) solution with the molar ratio of NaOH/SiO 2 of 1.2 (for BA) and 1.5 (for RHA) and NaOH concentration of 2.2 M. Nanosilica particles were prepared from liquid glass solution by precipitation method as shown in Schema 1.Under strong stirring, a mixture of NH 4 OH : ethanol with a defned volume ratio was slowly added to the liquid glass solution.Ten, a 1 : 1 HCl solution (by volume) was slowly added to it until the precipitate was completely formed.Te mixture was further sonicated for 1 hour using a 400 W ultrasonic bath with a frequency of 37 kHz at 40 °C.Te fne precipitate was fltered and washed using distilled water to a pH of 7. Nanosilica particles were obtained after drying the precipitate at 80 °C for 24 hours.

Characterization of Material. X-ray difraction (XRD)
was employed to express the crystal phase of the obtained nanosilica using RINT2000/PC device (Rigaku, Japan) with the tube anode made by Cu with K α � 1.54 Å, and the pattern was obtained at 40 kV of tube voltage and 40 mA of tube current in step scan mode (step size of 0.0297 °).Te existence of elements in nanosilica was checked from the energy-dispersive X-ray spectrum (EDS) using a Hitachi S4800 device (Japan).Te material's morphology was observed through scanning electron microscopy (SEM) (Hitachi S4800, Japan).Te porosity of the material was confrmed by the N 2 adsorption and desorption method using a Tristar-3030 system (Micromeritics, USA).A Fourier transform infrared (FT-IR) spectrometer (model IRPrestige-21; Shimadzu, Kyoto, Japan) was used to detect the functional groups on the surface of nanosilica.

Determination of Methylene
Blue.Methylene blue (MB) concentration was determined by UV-Vis molecular absorption spectrometry at the wavelength of 660 nm using a Cary 60 UV-Vis (Agilent).Te standard curve equation expresses a good linear correlation between absorbance (Abs) and investigates methylene blue concentration (C MB ) (Abs � 0.1384.C MB -0.0121) with a very high determination coefcient (0.994).

Determination of Zero Charge Point.
Te zero charge point (PZC) is a value indicating the pH at which the charge on the surface of the material is zero.Tis value is determined by using the pH drift method [42].Nine beakers containing 20 mL of 0.1 M NaCl solutions were prepared with the initial pH value (pH i ) from 2 to 10 which is adjusted by 0.1 M NaOH or 0.1 M HCl solutions.Distilled water was added into the fask until the total volume of the solution was 25 mL.After that, 0.1 g of nanosilica was added to each fask.Te mixtures were continuously stirred (200 rpm) for 48 hours.Te fnal pH (pH f ) of the solutions was measured to obtain the value of ΔpH (ΔpH � pH i -pH f ).Te plot between ΔpH and pH i was obtained.Te intersection point of the curve with the horizontal axis is the value of PZC.

Determination of Ultrasonic Time.
Te ultrasonic time is investigated from 30 to 180 minutes.All the nanosilica materials synthesized with diferent ultrasonic times are used to remove MB from an aqueous solution with an MB initial concentration of 10 mg•L −1 at a pH of 6 for 120 mins, and the suitable time is chosen based on their adsorption efciency of MB.

Adsorption Studies.
Te pH of the solution, adsorbent dosage, initial MB concentrations, solution temperature, and contact time were surveyed in batch experiments.Te mixtures consisting of 20 mL of MB solution and nanosilica with the adsorbent dosage of 0.5 g•L −1 were prepared in ten fasks, and the pH of the solution was adjusted from 2 to 11 by HNO 3 (0.1 mol•L −1 ) and NaOH (0.1 mol•L −1 ), sequentially.All the samples were performed under stirring (300 rpm) at 30 °C for 120 mins with the aim of reaching the adsorption equilibrium.Te remaining MB concentration of each sample was determined for calculating adsorption effciency.Te experiment was taken place again with the stable pH chosen from the above investigation, and the adsorbent dosage was varied from 0.25 to 0.75 g•L −1 .
For the adsorption isotherm study, the adsorption capacity was calculated at diferent initial MB contents from 10 to 50 mg•L −1 , and Langmuir and Freundlich isotherm models were employed for describing the experimental data.MB monolayer adsorption capacity was inferred from the Langmuir model.
Te adsorption kinetic study was carried out in 250 mL of MB solution with a defned dosage of adsorbent.Every 10 minutes, 10 mL of the mixture including both MB solution and adsorbent was sucked out for determining the remaining MB content.Te experimental data were analyzed using the frst-order and second-order kinetic models, and Weber-Morris intraparticle difusion model.
Termodynamic parameters were determined from the efect of temperature (from 283 to 333K) on MB adsorption capacity using the Van't Hof plot.

Results and Discussion
3.1.Preparation of RHA and BA.With the aim of eliminating the infuence of metal impurities, the ashes were treated with 1M HCl solution for 24 hours.Te EDS spectra of RHA and BA as shown in Figures 1 and 2 express that most of the main metals are removed from two kinds of ashes.
Te EDS analyses were performed on three diferent samples of each kind of ash (n � 3).Te weight percentages of the elements between the three samples of each kind of ash are not much diferent, as shown in the small values of relative standard deviation.Te SiO 2 content of RHA and BA determined is 49.54% and 79.80%, respectively.

Efect of Volume Ratio of NH 4 OH :
Ethanol on the Morphology of Nanosilica.One of the disadvantages of the precipitation method is the formation of polystructural silica clusters with undefned particle shapes and large particle sizes.Te morphology and particle size of nanosilica strongly depend on the conditions of the synthesis process and can be controlled by the existence of solvent.Te efect of NH 4 OH : ethanol volume ratio on the material morphology was investigated in the present study.For comparison and choice of suitable NH 4 OH : ethanol volume ratio, RHA-SiO 2 , BA-SiO 2 nanoparticles, and nanosilica synthesized from pure Na 2 SiO 3 (pure-SiO 2 ) were obtained with diferent ratios as shown in Figures 3-5.Ultrasonic time is fxed at 60 minutes.
SEM images in Figures 3 and 4 show that NH 4 OH : ethanol volume ratio expresses a great infuence on the formation of spherical particle structure of RHA-SiO 2 and BA-SiO 2 nanomaterials.During the synthesis without the mixture of NH 4 OH and ethanol at the early stage, spherical nanosilica was unformed, and the amorphous structure was obtained instead.Meanwhile, the nanometer-sized spherical particle structure of pure-SiO 2 nanomaterial (Figure 5) was formed at all volume ratios of NH 4 OH : ethanol.However, the absence of the mixture of NH 4 OH and ethanol (Figure 5(o)) resulted in the incomplete formation of spherical nanoparticles, ununiform particle size, and the agglomeration of many particles into large clumps.Te more volume of NH 4 OH in the mixture was, the more complete and round silica nanoparticles were.It is predicted that the bad infuence of impurities in the liquid glass solution separated from rice husk ash and bagasse ash is excluded because of the existence of NH 4 OH and ethanol mixture at a suitable volume ratio.Te suitable volume ratio of NH 4 OH : ethanol of 12 : 3 gave well-shaped particles with clear grain boundaries, smooth surface, and uniform diameter from 100 to 150 nm (Figure 5(t)).
For both natural sources (Figures 3 and 4), in the sample synthesized with ethanol but without NH 4 OH, the spherical particles did not appear that confrms the important role of NH 4 OH.When increasing the amount of NH 4 OH corresponding to NH 4 OH : ethanol volume ratio from 3 : 12 to 15 : 0, the spherical particles in samples gradually achieved and increased in number.Nanosilica particles are partly formed with clear grain boundaries, smooth surface at the ratio of 6 : 9, and wholly at the ratio of 13 : 2. Both materials obtained at NH 4 OH : ethanol volume ratio of 13 : 2 exhibit uniform particle size in the range of 150-200 nm.Nevertheless, when ethanol was absent in the mixture (Figures 3(g) and 4(n)), some particles were agglomerated into clusters which reduced surface area.Tis demonstrates the important role of ethanol in preventing nanosilica particles from agglomerating.
Setyawan et al. [41] also extracted silica from RHA by sol-gel method with the same precipitating agent of HCl solution.However, the lack of NH 4 OH : ethanol mixture seems to be the reason causing the fact that silica appeared agglomerate and was not a single particle.Noushad et al. [39] employed ethanol as a nonpolar solvent and orthophosphoric acid as a precipitating agent to obtain silica from RHA with ununiform spherical particle diameters from 80 to 360 nm.Besides, almost of particles are observed in cluster.From sugarcane bagasse, Athinarayanan et al. [16] synthesized biogenic silica nanoparticles using HCl pretreatment and calcination at 750 °C.Te unemployment of NH 4 OH : ethanol solvent results in large clusters in undefned shapes with an average size of 191 nm.In another study, amorphous silica was separated from BA and RHA using H 2 SO 4 as a precipitating agent and without NH 4 OH : ethanol solvent [43].Te result showed that silica particles exhibited undefned shapes with various sizes and agglomerated.In conclusion, there are few diferences between nanosilica separated from two kinds of the above natural source.Te results conclude that the suitable NH 4 OH : ethanol volume ratio is 12 : 3.

Efect of Ultrasonic Time on MB Adsorption Efciency.
Te ultrasonic technique is an efective way for particle dispersion and deagglomeration of nanomaterials during their synthesis process [44].Te ultrasound energy causes the formation, growth, and collapse of cavitation bubbles in the liquid medium.Under the violent collapse of acoustic cavitation bubbles, hydrogen and hydroxyl radicals are formed, which prevents the agglomeration of nanoparticles [45].Te adsorption efciency of MB increases signifcantly from 38.1% without the ultrasonic process to 68.0% with 30 mins of ultrasonic time.Ten, the longer the ultrasonic time is, the higher the adsorption efciency is.After 60 minutes of ultrasonic time, most of the MB is removed from the aqueous solution (adsorption efciency of around 97%).

Characterization of Nanosilica.
Te XRD patterns expressed in Figure 6 expose the crystalline nature of the obtained nanosilica in the range of 2θ from 10 °to 70 °.Te only broad peak at 2θ of 22 °appearing in three XRD spectra of RHA-SiO 2 , BA-SiO 2 , and pure-SiO 2 nanomaterials corresponds to amorphous phase SiO 2 [16,42,43,46].
Te morphology of the best nanosilica samples was observed on SEM images as shown in Figures 3(f ), 4(m), and 5(t).Te spherical particles with clear grain boundaries, smooth surface, no agglomeration, and uniform diameter of about 100-150 nm appeared in sample separated from pure chemical, and 150-200 nm was obtained in two samples made from natural sources.
Te porosity of SiO 2 materials was evaluated by the N 2 adsorption and desorption method.According to the IUPAC classifcation, the adsorption and desorption curves of the materials as shown in Figure 7 are confrmed in IV type corresponding to the adsorption of micromesoporous material.Te form of hysteresis curves means the mesopores created among SiO 2 nanoparticles are disordered.It is predicted that the pore cavity distribution is wide compared with the neck size distribution [47].Te hysteresis curve of pure-SiO 2 nanomaterial (Figure 7(c)) (P/P o ∼ 0.6) appears at the higher pressure in comparison with RHA-SiO 2 nanomaterial (Figure 7(b)) and BA-SiO 2 nanomaterial (Figure 7(a)) (P/ P o ∼ 0.4).Tis confrms that the pore neck size of pure-SiO 2 nanomaterial is smaller than that of RHA-SiO 2 and BA-SiO 2 nanomaterials.Te smaller the particle size is, the narrower the pore neck size is.
Te pore volume distribution of the materials expressed according to the Barrett-Joyner-Halenda (BJH) model is shown in Figure 8.As can be seen, the pore size of the material concentrates in the range from 2 to 10 nm for all 3 samples.Te BET surface area of pure-SiO 2 , RHA-SiO 2 , and BA-SiO 2 nanomaterials is 214.0, 180.6, and 187.5 m 2 •g −1 , respectively.It is found that the BET surface areas of SiO 2 nanomaterials synthesized from natural sources are similar together and signifcantly lower than those of SiO 2 nanomaterials made from pure Na 2 SiO 3 .Tis could be due to the impurities of RHA and BA.Te functional groups on the surface of nanosilica were confrmed on FT-IR spectra as shown in Figure 10.Te O-H groups are detected based on stretching vibration noticed at the broadband from 3000 to 3700 cm −1 and the peak of 1631 cm −1 .Te presence of the peak at 1099 and 464 cm −1 relating to the bending variations of Si-O-Si and 952 cm −1 assigned to stretching vibrations of Si-OH demonstrates the existence of Si element in the material [48,49].
One of the important characteristics of the adsorbent is its zero charge point.Figure 11 shows the data for the determination of the zero charge point of BA-SiO 2 (a), RHA-SiO 2 (b), and pure-SiO 2 (c) nanomaterials following the

8
Journal of Nanotechnology pure-SiO 2 sample compared to BA-SiO 2 and RHA-SiO 2 ones.Terefore, it can be seen that the nanosilica made from pure chemicals can be replaced by nanosilica synthesized from natural sources for MB-efective adsorption.
Te change in adsorption efciency with pH could be explained based on the PZC value of the material (PZC ∼ 3).At a pH lower than 3, the positive surface of the material prevents MB + ions from reaching the material.However, the higher the pH is, the less the positive charge covers the surface.Tis is explained by the higher adsorption efciency as the pH of the solution increases from 2 to 3. Te surface of the material becomes negative at a pH higher than 3 and gradually rises with pH.Terefore, the adsorption efciency is rapidly enhanced when increasing pH from 4 to 11 due to the easy attraction of MB + ions to the surface of the adsorbent.

Efect of Adsorbent Dosage.
With the initial MB concentration of 20 mg•L −1 , at a pH of 8, the dosage of adsorbent was investigated from 0.125 to 0.375 g•L −1 .For all three materials, the adsorption efciencies achieve more than 80% at the dosage of 0.250 g•L −1 .Ten, almost MB is removed from the solution when rising the adsorbent dosage to 0.375 g•L −1 .Te adsorption efciency reaches over 99% for BA-SiO 2 and pure-SiO 2 samples and over 94% for RHA-SiO 2 sample.

Study of Isotherm Adsorption.
From the data in Table 1, it can be seen that MB adsorption capacity tends to gradually increase with the rising of initial MB concentration from 10 to 50 mg•L −1 in the same reaction conditions including the adsorbent dosage of 0.25 g/L for 180 mins at room temperature, at which, the pure-SiO 2 nanoparticles exhibit a rather better adsorption capacity than BA-SiO 2 and RHA-SiO 2 ones.
Langmuir and Freundlich nonlinear isotherm equations have been employed for reviewing the data as shown in ( 1) and ( 2) equations which are illustrated in Figure 12 [50]: where K L is the Langmuir constant which is related to the strength of adsorption, and K F and n are the Freundlich constants.
For each material, it is found that the determination coefcient for the Freundlich model is slightly higher than that for the Langmuir model (Table 2).Tis fact demonstrates that the adsorption is mainly in the multilayer form with a heterogeneous surface.1/n value calculated from the nonlinearized Freundlich equation is between 0 and 0.5, suggesting that the adsorption is favorable [51].Te singlelayer adsorption capacity (q m ) inferred from the Langmuir model is all rather higher than some others as shown in Table 3. BA-SiO 2 adsorbent exhibits the highest capacity (214.97 mg•g −1 ) in the three obtained materials (169.21mg•g −1 for RHA-SiO 2 and 196.78 mg•g −1 for pure-SiO 2 .).

Study of Adsorption Kinetics.
Te insight into the adsorption is provided by the kinetic study including mass transfer, difusion, and surface adsorption [58].Accordingly, the adsorption time was investigated until the adsorption reached the equilibrium as shown in Figure 13.As can be seen, for all surveyed adsorbents, the time of adsorption equilibrium is about 45-60 minutes with the initial MB concentration of 10 mg•L −1 .
Te increase of initial MB concentration from 20 to 50 mg•L −1 results in the enhancement of adsorption equilibrium time to about 75-90 minutes.Here, the adsorption equilibrium time of pure-SiO 2 material is shorter (45 minutes for the concentration of 10 and 75 minutes for the remaining concentrations) than that of the other two materials.
For the purpose of clarifying the kinetic nature of MB adsorption onto the synthesized nanosilica materials, Lagergren's frst-order (LFO) kinetic model (equation ( 3)), Ho's second-order (PSO) kinetic model [59] (equation ( 4)), and Weber-Morris intraparticle difusion model (IPD) [60] (equation ( 5)) were applied.Tese models are given, respectively, as follows: ln q e − q t  � lnq e − k 1 t, (3) where k dif is the intraparticle difusion rate constant ) is a constant which is related to difusion resistance and is a characteristic constant for the layer of the solution surrounding the particle, and k 1 and k 2 are Lagergren's frst-order and Ho's second-order rate constants, respectively.Te study is carried out at diferent initial MB contents from 10 to 50 mg•L −1 .As shown in Table 4, when describing the MB adsorption onto three materials, the linear equation of the PSO kinetic model exhibits slightly higher determination coefcients than that of the LFO kinetic model at all initial MB concentrations.Besides, the experimental adsorption capacity value (q e(ex) ) is quite close to this calculated from the PSO kinetic equation (q e(mo) ).In other words, the PSO model well depicted the kinetics of MB adsorption onto BA-SiO 2 , RHA-SiO 2 , and Pure-SiO 2 , which confrms the chemisorption process [61].Te adsorption rate depends on both concentrations of adsorbent and adsorbate.

Journal of Nanotechnology
Te adsorption includes three stages of the difusion of the adsorbate (i) from the solution to the surface of the adsorbent forming a solution layer surrounding the particle (k dif1 ) and (ii) from this surface into its intraparticle capillary (k dif2 ); after that, the fnal stage is (iii) the adsorption equilibrium.In some cases, such as BA-SiO 2 material or low initial concentration of MB for RHA-SiO 2 and pure-SiO 2 ones, the frst and second stages can be taken place simultaneously resulting strong increase in adsorption capacity (Figure 14).
Te efect of the solution layer surrounding the particle is evaluated based on the constant C of Weber-Morris intraparticle difusion as shown in Table 5. Te greater this constant is, the thicker this layer is.Te thick solution layer will hinder the difusion of the adsorbate into the intraparticle capillary of the adsorbent.10 Journal of Nanotechnology For BA-SiO 2 material, at all of the surveyed MB concentrations, in the initial 50-75 minutes, the C value gets closer to zero corresponding to a thin MB solution layer surrounding the material and the fast movement of MB molecules passing through this layer.Terefore, a strong uptrend of MB adsorption capacity is observed as shown in Figure 13(a), and the stage of intraparticle difusion is predicted as the step determining the rate of MB adsorption.It is found that after 50-75 minutes, the C value is much higher, which means the longer the time is, the thicker the layer is, hindering the difusion of MB inside the material capillary.As a result, the adsorption capacity value varies unremarkable, and the equilibrium is obtained that seems to indicate that almost of active adsorption sites of material are saturated.Nevertheless, the equilibrium adsorption capacity still augments as a consequence of the rising of MB content from 10 to 50 mg•L −1 although the C value gradually increases from 2.62 to 9.40.Besides, it is concluded that the difusion rate constants of stages (k dif ) are seen in a downtrend from k dif1 to k dif2 from Table 5 because of the simultaneous occurrence of the external and intraparticle difusions of MB for initial 50-75 minutes (k dif1 ) and the following equilibrium (k dif2 ).
Regarding the initial MB concentration from 30 to 50 mg•L −1 for RHA-SiO 2 (Figure 13

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Journal of Nanotechnology third one (after 75 minutes) of adsorption equilibrium due to the much thicker solution layer on the surface of the adsorbent, which is expressed by a much higher C value.Furthermore, Table 5 indicates the decrease of k dif values from k dif1 to k dif2 and k dif3 .Among them, a high k dif1 value refers to the external mass transfer to form a boundary layer on the surface of the material.Te lower k dif2 value corresponds to the MB difusion to the most internal adsorption sites of the adsorbent.Finally, k dif3 value might be close to zero because of the saturated adsorption sites [62].

Termodynamic Study.
Te efect of temperature on the MB adsorption process onto synthesized nanosilica materials was studied with the aim of determining thermodynamic parameters describing the process with the investigated temperature range from 283 to 333 K. Te exothermic or endothermic nature of adsorption is examined based on Van't Hof equation as shown in equation (8), while equation ( 7) is the way to calculate the Gibbs free energy (ΔG °) of adsorption, in which the equilibrium constant of the process is inferred from equation ( 6) [50].
As shown in Table 6, the exothermic nature of MB adsorption onto three materials is inferred from all the negative values of standard enthalpy change.All the negative values of standard entropy change demonstrate that the reaction reduces the randomness of the system after the adsorption.Terefore, the mechanism of the process is predicted to be electrostatic bonding between MB + cations and the negatively charged surface of nanosilica as shown in Figure 15.Tis adsorption is spontaneous and favorable at temperatures lower than 323 K due to the negative value of the Gibbs free energy variations (∆G °).From 323 K and up, the desorption rate is much higher than the adsorption one.As a result, ∆G °value exhibits positive values.value demonstrates that the adsorption is an endothermic process.Te adsorption is spontaneous in the range of temperature 283-313 K but unfavorable from 323 K.

Figure 1 :
Figure 1: EDS analyses of bagasse ash before (a) and after (b) treated by HCl 1M.

Figure 2 :
Figure 2: EDS analyses of rice husk ash before (c) and after (d) treated by HCl 1M.
Nanosilica synthesized from rice husk and bagasse ashes was realized to be equivalent efective adsorbents for the removal of methylene blue from aqueous solution in comparison with nanosilica prepared from pure chemical.Te three materials are favorably formed at a volume ratio of NH 4 OH : ethanol of 12 : 3 and for 60 minutes of ultrasonic treatment.Most of MB was removed at ambient temperature with the three materials at a pH of 8 and adsorbent dosage of 0.375 g•L −1 .Te isotherm data ftted well with the Freundlich model.Te pseudo-secondorder kinetic model well described the kinetic data, and the Weber model confrmed that the step-determining reaction rate is intraparticle difusion.Te increase of initial MB concentration results in the rising of adsorption equilibrium time.Te adsorption mechanism of MB on the three nanosilica is the electrostatic bonding between MB + cations and the negatively charged surface of the nanosilica.Te negative enthalpy (ΔH °)

Table 2 :
Isotherm parameters calculated from the Langmuir and Freundlich models of MB adsorption onto BA-SiO 2 , RHA-SiO 2 , and pure-SiO 2 .

Table 3 :
Comparison of the single-layer adsorption capacity (q m ) of MB on silica adsorbents.

Table 4 :
Parameters of pseudo-frst-and second-order kinetic studies on MB adsorption of BA-SiO 2 , RHA-SiO 2 , and pure-SiO 2 at diferent initial MB contents.