New Hybrid Adsorbents Based on Polyaniline and Polypyrrole with Silicon Dioxide: Synthesis, Characterization, Kinetics, Equilibrium, and Thermodynamic Studies for the Removal of 2,4-Dichlorophenol

In the current study, polyaniline and polypyrrole with silicon dioxide (PAni:PPy@SiO2) were combined to formulate a new adsorbent, which was examined using XRD, TEM, SEM, FTIR, TGA, and BET, and the adsorption kinetics were investigated by UV–vis spectroscopy. The optical band gap was also evaluated. The electrochemical behavior was investigated using cyclic voltammograms. Moreover, experimental conditions were used to evaluate the 2,4-dichlorophenol (2,4-DCP) adsorption based on the pH, temperature, reaction time, and initial concentration. The analytical isotherm data were determined by Langmuir, Freundlich, Temkin, Sips, and Redlich–Peterson models. For the analysis of the kinetic data, the pseudo-first- and -second-order models and the intraparticle diffusion model were investigated. It was found that this new adsorbent possessed the highest adsorption efficiency after several regeneration cycles. Furthermore, the thermodynamic parameters of adsorption, such as entropy (ΔS), enthalpy (ΔH), and standard Gibbs were measured. These results suggest that the PAni:PPy backbone can generally be better applied for the elimination of 2,4-dichlorophenol by appropriately dispersing it over the surface of suitable SiO2. This search provides a novel way to develop separable, high-performance adsorbents for adsorbing organic contamination from wastewater.


Introduction
Today, water contamination is a major problem worldwide. Chlorophenols are common organic pollutants used widely in the preparation of many pharmaceuticals and pesticides. Chlorinated phenol waste discharge into water exhibits toxicity to humans, aquatic organisms, and the environment [1,2]. Consequently, 2,4-dichlorophenol (2,4-DCP) is highly toxic, carcinogenic, and mutagenic and is listed as one of the environmental priority pollutants [3,4]. Hence, it is very significant to find a way to eliminate 2,4-DCP. Among the existing treatment methods, including photocatalytic degradation [5], electrochemical oxidation [6], membrane filtration [7], flocculation coagulation [8], adsorption [9], and so on, the adsorption process is one of the more efficient and promising technologies owing to its low cost, simplicity in design and operation, and superior adsorption effectiveness even at low concentrations [9][10][11]. In addition to its toxic effect, the presence of 2,4-DCP in water in even trace amounts (5-10 µg/L) produces a specific odor and makes it undrinkable [1][2][3][4].

Characterization Methods
The UV-visible spectrum was recorded using a Hitachi (U-3000) spectrophotometer. The X-ray diffraction (XRD) patterns of the adsorbents were defined on a Bruker, CCD-Apex instrument by Cu-Kα radiation (λ = 1.5418 Å). Fourier-transform infrared (FT-IR) spectroscopy was performed using a Bruker spectrophotometer in the spectral range of 4000-400 cm −1 . The morphological analysis was performed using transmission electron microscopy (TEM) (JEOL/JEM-2010). The surface and morphological characterization of the samples was performed with a scanning electron microscope (SEM; Hitachi S-4700). Their thermal stability was analyzed through thermogravimetric analysis (TGA) using a Hitachi (STA-7200) instrument. The Brunauer-Emmitt-Teller (BET) measurements were performed to determine the specific surface area and pore volume on AutoSorb (6-Quantachrome, Boynton Beach, FL, USA) [10,19]. The adsorption temperature was controlled using an Alpha Immersion thermostat (230 V, 50/60 Hz, Germany) and the initial pH was measured using a portable PHYWE pH meter (Cobra, Bremen, Germany).

PAni:PPy@SiO 2 Hybrid Adsorbent Preparation
Polyaniline:polypyrrole (PAni:PPy) was prepared by in situ chemical oxidation polymerization in 1 M HCl. The Ani and Py monomers were oxidized by APS in the presence of SiO 2 . The constant mole ratio of monomers (Ani and Py) and oxidant was n(Ani):n(Py):n(APS) = 1:1:1, the weight ratio of m(PAni:PPy):m(SiO 2 ) was 90:10 for all prepared samples. The polymerization procedure was carried out in a stirred, cooled (5 • C) reactor. The APS solution was added dropwise to the monomer solution and the reaction took 24 h (Scheme 1) [10,19]. The reactor contents were then vacuum filtered and washed repeatedly with 1 M HCl, C 2 H 5 OH, and H 2 O to eliminate excess oxidant with oligomers until the filtered solution became clear. The precipitates were then dried in an oven at 60 • C for 3 h. In the same way, PAni:Ppy was prepared in the absence of SiO 2 , considering a yield of 70-73% of the adsorbents' chemical polymerization.
performed to determine the specific surface area and pore volume on AutoSorb (6-Quantachrome, Boynton Beach, FL, USA) [10,19]. The adsorption temperature was controlled using an Alpha Immersion thermostat (230 V, 50/60 Hz, Germany) and the initial pH was measured using a portable PHYWE pH meter (Cobra, Bremen, Germany).

PAni:PPy@SiO2 Hybrid Adsorbent Preparation
Polyaniline:polypyrrole (PAni:PPy) was prepared by in situ chemical oxidation polymerization in 1 M HCl. The Ani and Py monomers were oxidized by APS in the presence of SiO2. The constant mole ratio of monomers (Ani and Py) and oxidant was n(Ani):n(Py):n(APS) = 1:1:1, the weight ratio of m(PAni:PPy):m(SiO2) was 90:10 for all prepared samples. The polymerization procedure was carried out in a stirred, cooled (5 °C) reactor. The APS solution was added dropwise to the monomer solution and the reaction took 24 h (Scheme 1) [10,19]. The reactor contents were then vacuum filtered and washed repeatedly with 1 M HCl, C2H5OH, and H2O to eliminate excess oxidant with oligomers until the filtered solution became clear. The precipitates were then dried in an oven at 60 °C for 3 h. In the same way, PAni:Ppy was prepared in the absence of SiO2, considering a yield of 70-73% of the adsorbents chemical polymerization.

Batch Adsorption Experiments
The adsorption experiment was carried out for the adsorption of 2,4-DCP from an aqueous solution. An amount of 25mL of 2,4-DCP was taken in 100mL flasks with a concentration of 10-200 mg.L −1 . The adsorption test was carried out at a pH (2−12) that was adjusted by NaOH or HCl and the sample was placed in a shaker for different time periods (5-180 min) at 150 rpm in a thermal bath from 25 to 50 °C. The adsorption was determined by a UV-visible spectrophotometer at 285 nm. The adsorption efficiency of 2,4-DCP was calculated using an equation [20].
where (mg·g −1 ) denotes the adsorption capacity, w (g·L −1 ) is the adsorbent dose of 2,4-DCP solution, (mg·L −1 ) is the initial concentration of 2,4-DCP in contact with the adsorbent, and is the 2,4-DCP concentration (mg·L −1 ) after the adsorption and time (t). The adsorption kinetics of the 2,4-DCP were investigated at 25 °C, the adsorbent dose was introduced into 100 mL of 2,4-DCP ( = 50 mg.L −1 ) for 4 h, and then the filtration and washing were performed. The experimental data were analyzed using the following models [18].

Batch Adsorption Experiments
The adsorption experiment was carried out for the adsorption of 2,4-DCP from an aqueous solution. An amount of 25mL of 2,4-DCP was taken in 100mL flasks with a concentration of 10-200 mg·L −1 . The adsorption test was carried out at a pH (2−12) that was adjusted by NaOH or HCl and the sample was placed in a shaker for different time periods (5-180 min) at 150 rpm in a thermal bath from 25 to 50 • C. The adsorption was determined by a UV-visible spectrophotometer at 285 nm. The adsorption efficiency of 2,4-DCP was calculated using an equation [20].
where q eq (mg·g −1 ) denotes the adsorption capacity, w (g·L −1 ) is the adsorbent dose of 2,4-DCP solution, C 0 (mg·L −1 ) is the initial concentration of 2,4-DCP in contact with the adsorbent, and C eq is the 2,4-DCP concentration (mg·L −1 ) after the adsorption and time (t). The adsorption kinetics of the 2,4-DCP were investigated at 25 • C, the adsorbent dose was introduced into 100 mL of 2,4-DCP (C 0 = 50 mg·L −1 ) for 4 h, and then the filtration and washing were performed. The experimental data were analyzed using the following models [18].
The adsorption isotherm can be explained as the process of mass transfer between a solid and an adsorbate at a constant temperature. There are many adsorption models such as Langmuir, Freundlich, and Temkin [21]. They are expressed by: where q eq (mg·g −1 ): the amount adsorbed at equilibrium; C eq (mg·L −1 ): the equilibrium concentration; K l (L·mg −1 ): the Langmuir constant; and q m (mg·g −1 ): the maximum amount adsorbed.
Freundlich equation where K f (mg 1−1/n ·g −1 ·L 1/n ): the constant of Freundlich; and n: the heterogeneity factor. The adsorption efficiency is connected to the K f constant, whereas the adsorption is related to the 1 n constant. Temkin equation where B (kJ·mol −1 ): the Temkin constant of the adsorption heat; and K T (L·mg −1 ): the constant of the Temkin isotherm.
Sips equation q eq = q m K s C eq n s 1 + K s n s where K s (L·g −1 ): the Sips constant; and n s (L·g −1 ): the Sips isotherm exponent.
Redlich-Peterson q eq = K RP C eq 1 + a RP C eq β where K RP (L·g −1 ): the Redlich-Peterson constant; and β: the Redlich-Peterson isotherm exponent developed to overcome the disadvantage of the Freundlich model. At high and low adsorbate concentrations, the Sips isotherm approaches the Langmuir and Freundlich isotherms [22], respectively. The equation of the Sips isotherm is given below.
The root mean square error (RMSE) functions were adopted to optimize the model parameters, which can be expressed as: where m: the number of data points evaluated; and p: the number of parameters in the regression model. Thermodynamic equations were used to determine the change in enthalpy (∆H), the change in free energy (∆G 0 ), and the change in entropy (∆S 0 ) for 2,4-DCP adsorption on the adsorbents. These variables are used to determine the sorption type [23]. K D defines the equilibrium constant, which can be measured by the following equations: K D = q eq C eq Free enthalpy where T (K): absolute temperature; R (8.314 J·mol −1 ·K −1 ): ideal gas constant; and K D : the distribution coefficient. The ∆H 0 and ∆S 0 values can be measured from the Van't Hoff formula:

Characterization Analysis
The XRD patterns of the as-synthesized PAni, PAni:PPy, SiO 2 , and PAni:PPy@SiO 2 are shown in Figure 1a. PAni has a semi-crystalline structure, as the patterns show two peaks at 2θ = 8.21 • and 24.86 • , which are attributed to the presence of quinonoid with benzenoid functions in the polymer backbone [19]. Moreover, the XRD patterns of PAni:PPy show a relatively intense band at 2θ = 19.95 • with two distinct shoulders at 8.34 • and 25.05 • . The observed peak at 2θ = 25.05 • might be due to the overlapping between the prevailing (110) reflection of PPy and the peak associated with the PAni. For the SiO 2 sample, a peak at 2θ = 22.41 • is observed, which can be attributed to the amorphous silica (SiO 2 , JCPDS No. 29-0085) [24]. No other peaks can be found. In the case of the PAni:PPy@SiO 2 adsorbent, aside from the characteristic peak of SiO 2 , all other XRD peaks can be indexed to the PAni:PPy sample, indicating that the PAni:PPy matrix was formed on the SiO 2 surface. This indicates that reactions occurring between the SiO 2 and the polymer chains occur during its preparation.

Characterization Analysis
The XRD patterns of the as-synthesized PAni, PAni:PPy, SiO2, and PAni:PPy@SiO2 are shown in Figure 1a. PAni has a semi-crystalline structure, as the patterns show two peaks at 2θ = 8.21° and 24.86°, which are attributed to the presence of quinonoid with benzenoid functions in the polymer backbone [19]. Moreover, the XRD patterns of PAni:PPy show a relatively intense band at 2θ = 19.95° with two distinct shoulders at 8.34° and 25.05°. The observed peak at 2θ = 25.05° might be due to the overlapping between the prevailing (110) reflection of PPy and the peak associated with the PAni. For the SiO2 sample, a peak at 2θ = 22.41° is observed, which can be attributed to the amorphous silica (SiO2, JCPDS No. 29-0085) [24]. No other peaks can be found. In the case of the PAni:PPy@SiO2 adsorbent, aside from the characteristic peak of SiO2, all other XRD peaks can be indexed to the PAni:PPy sample, indicating that the PAni:PPy matrix was formed on the SiO2 surface. This indicates that reactions occurring between the SiO2 and the polymer chains occur during its preparation.  Figure 1b represents the FTIR spectra of the samples. The spectra for PAni show the characteristic band of nitrogen quinine at 1579 cm −1 . Bands at 1491 cm −1 , 1315 cm −1 , 1164 cm −1 , and 1101 cm −1 appear, which are associated with a benzene ring and C−N and C=N stretching vibrations. In addition, the band at 3233 cm −1 is associated with a C-H stretching vibration. The peak at 825 cm −1 belongs to the C−H of the PAni ring. Compared to PAni, the bands of PAni:PPy are redshifted. This may be attributed to the strong interactions between the copolymer backbone during the synthesis process [24][25][26], such as π-π stacking or H bonding between nitrogen and hydrogen. The typical spectral bands of PAni and PPy can be observed in the copolymer spectra, indicating that the pyrrole and aniline monomers are present in the copolymer structure. These indicate that the core-shell struc-  Compared to PAni, the bands of PAni:PPy are redshifted. This may be attributed to the strong interactions between the copolymer backbone during the synthesis process [24][25][26], such as π-π stacking or H bonding between nitrogen and hydrogen. The typical spectral bands of PAni and PPy can be observed in the copolymer spectra, indicating that the pyrrole and aniline monomers are present in the copolymer structure. These indicate that the core-shell structure copolymer was successfully prepared and it presents the conductive state, which facilitates the transfer of electrons collected between them. The FTIR spectrum of SiO 2 displayed the presence of symmetric and asymmetric stretching modes for Si−O, Si−OH, and Si−O−Si groups at around 1058 cm −1 , 957 cm −1 , and 781 cm −1 , respectively. In addition, there is a broad band located around 3400 cm −1 and another located at 1634 cm −1 , both attributed to the O-H stretching of H 2 O and the formed silanol groups (Si-OH), respectively [27]. The interactions between the PAni:PPy structure and SiO 2 resulted in a slight redshift of the C=C and C=N bonds from 1542 cm −1 and 1458 cm −1 for copolymer alone to 1586 cm −1 and 1498 cm −1 for PAni:PPy@SiO 2 in the hybrid adsorbent. This confirmed the modification of the PAni:PPy matrix by SiO 2 .
The Brunauer-Emmitt-Teller (BET) method was used to investigate the BET surface areas, pore volumes, and pore size distributions of the samples (Figure 2a), and the results are summarized in Table 1. Clearly, the N 2 adsorption-desorption isotherms of all the materials belonged to type III with H 3 hysteresis loops, indicating the mesoporous structures in these samples [27]. The typical BET-specific surface area of SiO 2 is rather higher (182.02 m 2 ·g −1 ) compared to that of the PAni:PPy@SiO 2 material (113.84 m 2 ·g −1 ). The reduction in the surface area is attributed to the PAni:PPy matrix blocking the pores of the SiO 2 , thus reducing the surface area [27]. ture copolymer was successfully prepared and it presents the conductive state, which facilitates the transfer of electrons collected between them. The FTIR spectrum of SiO2 displayed the presence of symmetric and asymmetric stretching modes for Si−O, Si−OH, and Si−O−Si groups at around 1058 cm −1 , 957 cm −1 , and 781 cm −1 , respectively. In addition, there is a broad band located around 3400 cm −1 and another located at 1634 cm −1 , both attributed to the O-H stretching of H2O and the formed silanol groups (Si-OH), respectively [27]. The interactions between the PAni:PPy structure and SiO2 resulted in a slight redshift of the C=C and C=N bonds from 1542 cm −1 and 1458 cm −1 for copolymer alone to 1586 cm −1 and 1498 cm −1 for PAni:PPy@SiO2 in the hybrid adsorbent. This confirmed the modification of the PAni:PPy matrix by SiO2. The Brunauer-Emmitt-Teller (BET) method was used to investigate the BET surface areas, pore volumes, and pore size distributions of the samples (Figure 2a), and the results are summarized in Table 1. Clearly, the N2 adsorption-desorption isotherms of all the materials belonged to type III with H3 hysteresis loops, indicating the mesoporous structures in these samples [27]. The typical BET-specific surface area of SiO2 is rather higher (182.02 m 2 .g −1 ) compared to that of the PAni:PPy@SiO2 material (113.84 m 2 .g −1 ). The reduction in the surface area is attributed to the PAni:PPy matrix blocking the pores of the SiO2, thus reducing the surface area [27].  TGA is widely used to study the thermal degradation of materials [9]. The technique analyzes the weight loss associated with a continuous increase in temperature. The TGA lines represent the thermal degradation behavior of different synthesized materials in Figure 2b. The thermal treatment of the PAni:PPy@SiO2 composite consists of three levels of weight loss (wt). The first (wt) level up to 110 °C is attributed to the volatilization and decomposition of small organic compounds of 5.27%. The second (wt) level is up to 9.95% at 300 °C due to the evaporation of absorbed moisture and residual monomer or oligomer loss and the following third (wt) level reached up to 420 °C due to the chain degradation and decomposition of the material being 29.03%. In addition, a steady state decrease in  TGA is widely used to study the thermal degradation of materials [9]. The technique analyzes the weight loss associated with a continuous increase in temperature. The TGA lines represent the thermal degradation behavior of different synthesized materials in Figure 2b. The thermal treatment of the PAni:PPy@SiO 2 composite consists of three levels of weight loss (wt). The first (wt) level up to 110 • C is attributed to the volatilization and decomposition of small organic compounds of 5.27%. The second (wt) level is up to 9.95% at 300 • C due to the evaporation of absorbed moisture and residual monomer or oligomer loss and the following Polymers 2023, 15, 2032 7 of 18 third (wt) level reached up to 420 • C due to the chain degradation and decomposition of the material being 29.03%. In addition, a steady state decrease in weight of 11.91% of the PAni:PPy was observed up to 300 • C. Then, a steep decreasing trend in weight was observed up to 37.88% at 410 • C. After this, a steady state was again observed starting from 430 • C up to 900 • C. Moreover, the 13.46% weight of PAni was exhausted at 220 • C, a lower temperature than the PAni:PPy copolymer. Following a similar trend, the 68.89% weight was exhausted at about 630 • C. Finally, the SiO 2 shows initial (wt) corresponding to the evaporation of water followed by steady (wt) up to 900 • C due to the final loss caused by the decomposition of the component with residual mass retained being 6.61%.
The CV curves of PAni, PAni:PPy, and PAni:PPy@SiO 2 are shown in Figure 3. For the pristine PAni, two oxidation-reduction peaks were observed and these peaks are due to redox reactions with H + ions in the electrolyte. The oxidation peak at 0.46 V and the corresponding reduction peak at 0.29 V are attributed to the redox reaction from the leucoemeraldine form to the protonated emeraldine form. In addition, the redox peaks with higher oxidation states (0.89/0.81 V) can be associated with the transition of emeraldine to the totally oxidized pernigraniline [10]. It is noted that the PAni:PPy sample can show good electrochemical performance. Moreover, its CV curve has three pairs of redox peaks at (0.33/0.26 V), (0.50/0.42 V), and (0.81/0.71 V), indicating the copolymer formation. For the CV curve of the PAni:PPy@SiO 2 sample, the oxidation sweep peaks were at 0.50 V and the reduction peaks appeared at almost 0.67 V and 0.38 V. An apparent shift of the peaks was found between PAni and copolymer, which may be due to the formation of SiO 2 on the matrix polymer.
weight of 11.91% of the PAni:PPy was observed up to 300 °C. Then, a steep decr trend in weight was observed up to 37.88% at 410 °C. After this, a steady state wa observed starting from 430 °C up to 900 °C. Moreover, the 13.46% weight of PA exhausted at 220 °C, a lower temperature than the PAni:PPy copolymer. Following ilar trend, the 68.89% weight was exhausted at about 630 °C. Finally, the SiO2 shows (wt) corresponding to the evaporation of water followed by steady (wt) up to 900 to the final loss caused by the decomposition of the component with residual m tained being 6.61%.
The CV curves of PAni, PAni:PPy, and PAni:PPy@SiO2 are shown in Figure 3. pristine PAni, two oxidation-reduction peaks were observed and these peaks are redox reactions with H + ions in the electrolyte. The oxidation peak at 0.46 V and t responding reduction peak at 0.29 V are attributed to the redox reaction from th coemeraldine form to the protonated emeraldine form. In addition, the redox peak higher oxidation states (0.89/0.81 V) can be associated with the transition of emeral the totally oxidized pernigraniline [10]. It is noted that the PAni:PPy sample can good electrochemical performance. Moreover, its CV curve has three pairs of redox at (0.33/0.26 V), (0.50/0.42 V), and (0.81/0.71 V), indicating the copolymer formatio the CV curve of the PAni:PPy@SiO2 sample, the oxidation sweep peaks were at 0.50 the reduction peaks appeared at almost 0.67 V and 0.38 V. An apparent shift of the was found between PAni and copolymer, which may be due to the formation of S the matrix polymer. The morphological characteristics of the materials synthesized were studied by Figure 4 exhibits the TEM images for PAni, PAni:PPy, and PAni:PPy@SiO2. The fir spicuous difference between the PAni and the copolymer that can be observed in t ages is that the degree of aggregation is higher in the copolymer compared to PA addition, the TEM image of the PAni:PPy@SiO2 shows that the material has a very and packed structure. Due to their high surface area and energy, the SiO2 nanopa may have aggregated on the PAni:PPy matrix. An outer shell corresponding to the ymer formed can be seen, explaining the observation of a darker surface area. The morphological characteristics of the materials synthesized were studied by TEM. Figure 4 exhibits the TEM images for PAni, PAni:PPy, and PAni:PPy@SiO 2 . The first conspicuous difference between the PAni and the copolymer that can be observed in the images is that the degree of aggregation is higher in the copolymer compared to PAni. In addition, the TEM image of the PAni:PPy@SiO 2 shows that the material has a very dense and packed structure. Due to their high surface area and energy, the SiO 2 nanoparticles may have aggregated on the PAni:PPy matrix. An outer shell corresponding to the copolymer formed can be seen, explaining the observation of a darker surface area.  SEM was used to investigate the surface morphology of PAni:PPy and PAni:PPy@SiO2. Figure 5a shows that the copolymer has a relatively amorphous nature and the chain structures are well interconnected. Likewise, Figure 5b is the SEM image of PAni:PPy@SiO2 which shows that SiO2 was dispersed homogeneously and buried inside the PAni matrix with a random stacking morphology.  Figure 6a shows the UV-vis spectra of pure PAni, PAni:PPy, and PAni:PPy@SiO2. Two absorption bands were observed near 307-335 nm and 574-625 nm. The first discovered band is assigned to the π-π* transition for the pyrrole and/or benzenoid ring [28]. The second band is assigned to the pyrrole and/or quinoid ring transition [28]. These absorption bands provide general information about the oxidation/reduction state of the polymer backbone. SEM was used to investigate the surface morphology of PAni:PPy and PAni:PPy@SiO 2 . Figure 5a shows that the copolymer has a relatively amorphous nature and the chain structures are well interconnected. Likewise, Figure 5b is the SEM image of PAni:PPy@SiO 2 which shows that SiO 2 was dispersed homogeneously and buried inside the PAni matrix with a random stacking morphology.  SEM was used to investigate the surface morphology of PAni:PPy and PAni:PPy@SiO2. Figure 5a shows that the copolymer has a relatively amorphous nature and the chain structures are well interconnected. Likewise, Figure 5b is the SEM image of PAni:PPy@SiO2 which shows that SiO2 was dispersed homogeneously and buried inside the PAni matrix with a random stacking morphology.  Figure 6a shows the UV-vis spectra of pure PAni, PAni:PPy, and PAni:PPy@SiO2. Two absorption bands were observed near 307-335 nm and 574-625 nm. The first discovered band is assigned to the π-π* transition for the pyrrole and/or benzenoid ring [28]. The second band is assigned to the pyrrole and/or quinoid ring transition [28]. These absorption bands provide general information about the oxidation/reduction state of the polymer backbone.  Figure 6a shows the UV-vis spectra of pure PAni, PAni:PPy, and PAni:PPy@SiO 2 . Two absorption bands were observed near 307-335 nm and 574-625 nm. The first discovered band is assigned to the π-π* transition for the pyrrole and/or benzenoid ring [28]. The second band is assigned to the pyrrole and/or quinoid ring transition [28]. These absorption bands provide general information about the oxidation/reduction state of the polymer backbone.
The effect of the presence of SiO 2 on the optical properties and hence the optical energy band gap (E g ) of the polymer matrix was determined. Tauc's relation was used to determine the E g values of the samples (Figure 6b). In addition, the E g of the samples is derived by the extrapolation of the linear part of the (ahν) curves to fit the (hν) axis.
where hν: the energy of the incident photon; a: the absorption coefficient; B: constant; E g : the optical band gap (eV); and n is a variable exponent (n = 1/2 when the transition is indirect and n = 2 when the transition is direct) [29]. The effect of the presence of SiO2 on the optical properties and hence the optical energy band gap ( ) of the polymer matrix was determined. Tauc s relation was used to determine the values of the samples (Figure 6b). In addition, the of the samples is derived by the extrapolation of the linear part of the ( ℎ ) curves to fit the (ℎ ) axis.
It was found that the band gap energy for PAni:PPy@SiO2 is 3.15 eV; it then decreases to 3.13 eV (for pure PAni) and 3.05 eV (for copolymer PAni:PPy). The shrinkage of the optical band gap is mainly attributed to localized states created in the energy band gap of the SiO2 material. Tailoring the optical properties and hence the optical band gap of PAni:PPy@SiO2 makes it eligible for new applications.

Effect of Key Factors
The point of zero charges (pHPZC) can be formed when the pH surface charge tends to zero, and such pHPZC is employed to define the electrostatic interaction between the adsorbent surface and adsorbate. For the determination of the pHPZC value, 0.05 g of each adsorbent was mixed for 24 h at room temperature with 50 mL of 0.1 M NaCl solution. A NaOH and HCl solution (0.01 M) was used to adjust the pH between 2 to 12. When the pH is less than pHPZC, the surface of the adsorbent is expected to be negatively charged and it allows the adsorption of positive ions. At a pH greater than pHPZC, the adsorption of anions is more favorable due to increased positive ions at the adsorbent surface [30].
The pH not only affects the specific adsorption and the charge on the adsorbent surface but also influences the solubility of the phenolic compounds [3,31]. Therefore, the adsorption percentage changes when the pH of a solution is varied. The effect of the initial pH value was investigated by varying the pH from 2 to 12 on the adsorption of 2,4-DCP by the three adsorbents, and the results are shown in Figure 7. It is clear that the adsorption capacity of PAni:PPy@SiO2 increased gradually with increasing pH from 2.0 to 6.0 and then greatly decreased at pH 12.0. Meanwhile, pH values can significantly affect the surface charges of the adsorbate and thus the protonation level of functional groups on its surface [32]. The surface charge (pHzpc) of PAni:PPy@SiO2 was measured to be 8.5. This signifies that at pH > 8.5, the charge on the PAni:PPy@SiO2 surface is negative, whereas, at pH < 8.5, this charge is positive. Furthermore, the maximum qeq of the PAni:PPy@SiO2

Effect of Key Factors
The point of zero charges (pH PZC ) can be formed when the pH surface charge tends to zero, and such pH PZC is employed to define the electrostatic interaction between the adsorbent surface and adsorbate. For the determination of the pH PZC value, 0.05 g of each adsorbent was mixed for 24 h at room temperature with 50 mL of 0.1 M NaCl solution. A NaOH and HCl solution (0.01 M) was used to adjust the pH between 2 to 12. When the pH is less than pH PZC , the surface of the adsorbent is expected to be negatively charged and it allows the adsorption of positive ions. At a pH greater than pH PZC , the adsorption of anions is more favorable due to increased positive ions at the adsorbent surface [30].
The pH not only affects the specific adsorption and the charge on the adsorbent surface but also influences the solubility of the phenolic compounds [3,31]. Therefore, the adsorption percentage changes when the pH of a solution is varied. The effect of the initial pH value was investigated by varying the pH from 2 to 12 on the adsorption of 2,4-DCP by the three adsorbents, and the results are shown in Figure 7. It is clear that the adsorption capacity of PAni:PPy@SiO 2 increased gradually with increasing pH from 2.0 to 6.0 and then greatly decreased at pH 12.0. Meanwhile, pH values can significantly affect the surface charges of the adsorbate and thus the protonation level of functional groups on its surface [32]. The surface charge (pH zpc ) of PAni:PPy@SiO 2 was measured to be 8.5. This signifies that at pH > 8.5, the charge on the PAni:PPy@SiO 2 surface is negative, whereas, at pH < 8.5, this charge is positive. Furthermore, the maximum q eq of the PAni:PPy@SiO 2 was 24.9 mg·g −1 reached at pH 6.0, which is comparable to the removal of 2,4-DCP adsorbate on silicate adsorbent, where the am value was 2.16 mg·g −1 [30]. This was 7.43 mg·g −1 for PAni/barley husk (PAni/BH) and 9.73 mg·g −1 for PPy/barley husk (PPY/BH) adsorbent [3]. As the pH increased to 12.0, the q eq of the adsorbent decreased sharply to 14.0 mg·g −1 . Moreover, it is well known that the pK a value of 2,4-DCP is 7.90 [33], and its molecules favor a hydrophilic form when pH > pK a . More specifically, in the medium with a higher pH value (from 6.5 to 8.5), the removal rate rapidly decreased due to the ionization and the hydrophilic behavior of the chlorophenols. Although there is a π−π interaction and electrostatic attraction between the positive surface of the adsorbent sites and the anionic 2,4-DCP species, it plays only a secondary role in the removal process because the anionic 2,4-DCP molecules could not form H bonds and inclusion complexes with PAni:PPy@SiO 2 in a higher pH solution. On the other hand, at pH > 8.5, the adsorption capacity is significantly decreased due to the repulsion between the adsorbent surface and the negative charge of the 2,4-DCP molecules. As it is known, the adsorbate is mainly in a protonated form at pH < pK a (7.90) and in a deprotonated form at pH > pK a . Therefore, a pH of 6.0 was chosen for the present study. Furthermore, the pH pzc was found to be 4.0 in the case of PAni and PAni:PPy [2]. The removal capacity (q eq ) of 2,4-DCP by these adsorbents decreased with the increase in pH. As can be seen, the trend of q eq over pH in the range of 2-6 was typically the same as the trend of 2,4-DCP adsorption using treated PAni and PAni:PPy, which is due to the excess of H + ions competing with the adsorbate for active surface sites. However, when the pH was increased to 12, the adsorption capacity decreased to 4.73 mg·g −1 (PAni:PPy) and 3.53 mg·g −1 (PAni), respectively.
2,4-DCP species, it plays only a secondary role in the removal process b 2,4-DCP molecules could not form H bonds and inclusion complexes w in a higher pH solution. On the other hand, at pH > 8.5, the adsorption cantly decreased due to the repulsion between the adsorbent surfac charge of the 2,4-DCP molecules. As it is known, the adsorbate is mai form at pH < pKa (7.90) and in a deprotonated form at pH > pKa. The was chosen for the present study. Furthermore, the pHpzc was found t of PAni and PAni:PPy [2]. The removal capacity (qeq) of 2,4-DCP by th creased with the increase in pH. As can be seen, the trend of over 2-6 was typically the same as the trend of 2,4-DCP adsorption using PAni:PPy, which is due to the excess of H + ions competing with the a surface sites. However, when the pH was increased to 12, the adsor creased to 4.73 mg.g −1 (PAni:PPy) and 3.53 mg.g −1 (PAni), respectively. The contact time greatly affects the adsorption capacity of the ads sponse is depicted in Figure 8a. Obviously, the value increased sh due to the sufficient mass transfer stimulus and became slower with adsorption reached equilibrium at 120 min. Thereafter, there was no si the adsorption rate. Therefore, the optimum contact time to obtain the to be 120 min for the three adsorbent materials. The cause of such adso 2,4-DCP may be due to the accessibility of active sites on the adsorbent sites were readily available for adsorbent binding, which saturated wit adsorbate progressively started to move inwards, leading to the slow ties [32]. The slow adsorption rate in the subsequent phases might be d lecular diffusion mechanism [34]. Similar behavior has been studied The contact time greatly affects the adsorption capacity of the adsorbent, and the response is depicted in Figure 8a. Obviously, the q eq value increased sharply within 5 min due to the sufficient mass transfer stimulus and became slower with time, and then the adsorption reached equilibrium at 120 min. Thereafter, there was no significant change in the adsorption rate. Therefore, the optimum contact time to obtain the q eq was observed to be 120 min for the three adsorbent materials. The cause of such adsorption behavior of 2,4-DCP may be due to the accessibility of active sites on the adsorbent; mainly, the active sites were readily available for adsorbent binding, which saturated with time and then the adsorbate progressively started to move inwards, leading to the slow adsorption capacities [32]. The slow adsorption rate in the subsequent phases might be due to the intramolecular diffusion mechanism [34]. Similar behavior has been studied previously: as the contact time progresses, adsorption may decrease due to the saturation of binding sites [3,34]. contact time progresses, adsorption may decrease due to the saturation of binding sites [3,34]. To understand the adsorption-rate-determining step, the PFO, PSO, and intraparticle diffusion (ID) models were used to describe the 2,4-DCP adsorption process by three adsorbent samples [35]. Furthermore, adsorption kinetics data were fitted by the PSO model ( Figure 8b). Interestingly, Table 2 lists the measured values for different adsorption kinetic models. The coefficient of determination (R 2 ) and the root mean square error (RMSE) were used as error parameters for each model. The results indicate that the PSO model had the lowest values for the error parameters RMSE and the highest R 2 values. In addition, the values calculated for the PSO are in good agreement with the experimental findings. Thus, it can be said that the PSO model gave the best approximation of the kinetics of 2,4-DCP adsorption by the adsorbents than the PFO and ID models.  To understand the adsorption-rate-determining step, the PFO, PSO, and intraparticle diffusion (ID) models were used to describe the 2,4-DCP adsorption process by three adsorbent samples [35]. Furthermore, adsorption kinetics data were fitted by the PSO model ( Figure 8b). Interestingly, Table 2 lists the measured values for different adsorption kinetic models. The coefficient of determination (R 2 ) and the root mean square error (RMSE) were used as error parameters for each model. The results indicate that the PSO model had the lowest values for the error parameters RMSE and the highest R 2 values. In addition, the q eq values calculated for the PSO are in good agreement with the experimental findings. Thus, it can be said that the PSO model gave the best approximation of the kinetics of 2,4-DCP adsorption by the adsorbents than the PFO and ID models.

Adsorption Isotherms
Adsorption isotherms provide an understanding of the elimination process. The adsorption mechanism of the adsorbent consists of three steps. First, the 2,4-DCP molecules are transferred from the aqueous solution to the adsorbent surfaces via a liquid boundary film. Next, these adsorbates are transferred from the adsorbent surface to the intramolecular binding site, and finally, there is a strong attraction of the 2,4-DCP with the disposable sites both on the external surface and internal surface of the adsorbents [10]. Figure 9a shows the development of the adsorbed quantity as a function of 2,4-DCP concentration at equilibrium. The figure depicts that the adsorbed amount of 2,4-DCP increases with the concentrations. This is defined by the ease of adsorbent-adsorbate mass transfer [36]. Furthermore, the maximum adsorption efficiency value of PAni:PPy@SiO 2 was 24.9 mg·g −1 , which is approximately 1.5 times higher than that of PAni:PPy (17.34 mg·g −1 ) and 2.5 times higher than that of PAni. The difference in the adsorption capacity indicates that the formation of SiO 2 on the copolymer matrix drastically enhanced the adsorption process. The adsorption capacity of PAni:PPy@SiO 2 was almost the highest value among the adsorbents reported in previous studies for 2,4-DCP (Table 3). Therefore, PAni:PPy@SiO 2 can be an efficient and promising adsorbent material for the removal of organic pollutants. Adsorption isotherms provide an understanding of the elimination process. The adsorption mechanism of the adsorbent consists of three steps. First, the 2,4-DCP molecules are transferred from the aqueous solution to the adsorbent surfaces via a liquid boundary film. Next, these adsorbates are transferred from the adsorbent surface to the intramolecular binding site, and finally, there is a strong attraction of the 2,4-DCP with the disposable sites both on the external surface and internal surface of the adsorbents [10]. Figure 9a shows the development of the adsorbed quantity as a function of 2,4-DCP concentration at equilibrium. The figure depicts that the adsorbed amount of 2,4-DCP increases with the concentrations. This is defined by the ease of adsorbent-adsorbate mass transfer [36]. Furthermore, the maximum adsorption efficiency value of PAni:PPy@SiO2 was 24.9 mg.g −1 , which is approximately 1.5 times higher than that of PAni:PPy (17.34 mg.g −1 ) and 2.5 times higher than that of PAni. The difference in the adsorption capacity indicates that the formation of SiO2 on the copolymer matrix drastically enhanced the adsorption process. The adsorption capacity of PAni:PPy@SiO2 was almost the highest value among the adsorbents reported in previous studies for 2,4-DCP (Table 3). Therefore, PAni:PPy@SiO2 can be an efficient and promising adsorbent material for the removal of organic pollutants.    The results of the adsorption isotherm results are summarized in Table 4. As can be seen from (R 2 ), the values determined for the Freundlich and the Temkin models are less favorable, suggesting that these isotherm models cannot adequately describe this adsorption process. Otherwise, the adsorption isotherm can be better described by the Langmuir and combined models, and the measured adsorption capacity is comparable to the empirical one, suggesting that 2,4-DCP removal on these adsorbents is a monolayer homogeneous adsorption. Furthermore, the PAni:PPy@SiO 2 results offer a better fit by the Temkin model with a value of R 2 = 0.984 compared to the Freundlich isotherm (R 2 = 0.881), suggesting that the adsorption energy decreases linearly as the binding sites are saturated by the 2,4-DCP. Furthermore, the Langmuir constant (K L ) represents the intensity of the adsorbent/adsorbate interaction [41]. Here, it was noted that its value is 0.843 L·mg −1 . The latter is relatively higher compared to the PAni and PANI:PPy adsorbents, indicating a strong interaction between 2,4-DCP and the PAni:PPy@SiO 2 surface. Furthermore, the n value related to the Freundlich isotherm (n > 1) confirmed that the PAni:PPy@SiO 2 material was suitable for 2,4-DCP absorption. On the other hand, the R 2 values were weaker than those measured from other isothermal kinetics. Therefore, Langmuir's isotherm is in complete agreement with the empirical results for this adsorbate on the PAni:PPy@SiO 2 surface. Likewise, the measured results suggested that the as-prepared PAni:PPy and PAni exhibited different adsorption behavior on 2,4-DCP. The data of these adsorbents were well approximated by the Langmuir and Freundlich models with the highest regression coefficients R 2 , respectively. The Freundlich isotherm is better at describing the 2,4-DCP elimination by polymer and copolymer compared to PAni:PPy@SiO 2 , which may be due to the specific surface areas, different morphology, composition, and structural arrangements of these adsorbents. On the other hand, the fitted parameter β in the Redlich-Peterson (R-P) model was between 0.90 and 0.95, indicating that the R-P model could be converted into the Langmuir model in these cases and that the adsorption sites on these adsorbents were on a single layer, and the adsorbed 2,4-DCP had no internal interaction [21]. In addition, the Sips model was well-fitted to 2,4-DCP adsorption data with R 2 values greater than 0.996, suggesting the heterogeneous surface adsorption of 2,4-DCP on adsorbents [10].

Adsorption Thermodynamics
The effect of temperature on the 2,4-DCP adsorption was studied by changing the temperature of the adsorbent from 298 K to 328 K, as shown in Figure 9b. A decrease in removal productivity was observed with the increase in temperature, which could indicate that an increase in temperature participates in a decrease in adsorption capacity on the three adsorbent samples. These results showed the exothermic character of 2,4-DCP elimination by adsorbents. This adsorption behavior is attributed to the inactivity of active sites at high temperatures [3]. The measured thermodynamic data are summarized in Table 5. The ∆H 0 negative value suggests that the process of adsorption at all investigated temperatures is exothermic in nature. Negative values of ∆S were obtained, showing that there is a decrease in the disorderliness and haphazardness of the adsorbed molecules' movement at elevated temperatures. Moreover, there were decreasing negative values of ∆G 0 in with increasing temperature, signifying that the process and capacity for the adsorption reduce with the increasing temperature; this process is spontaneous, thermodynamically feasible, and chemically controlled [31]. When the values of thermodynamic parameters for the adsorption of the 2,4-DCP solution onto the PAni:PPy@SiO 2 were compared with the polymer adsorbents, higher absolute values of change in the ∆G 0 as well as the ∆H 0 was observed. Precisely, the change in ∆H 0 for the adsorption by PAni:PPy@SiO 2 was obtained as −94.76 kJ·mol −1 compared to −12.08 kJ·mol −1 and −7.15 kJ·mol −1 for PAni:PPy and PAni, respectively, indicating the tendency for higher adsorption capacity in presence of SiO 2 . Importantly, the results also indicate that ∆H 0 lower than 20 kJ·mol −1 denotes that the adsorption mechanism is physisorption (the bond between adsorbent and adsorbate are hydrogen bonds or van der Waals interactions); in addition, physisorption is involved in the process when ∆G 0 ranges from −20 < ∆G 0 < 0 kJ·mol −1 [21,25].

Adsorption Mechanism
Based on the above experimental results and discussions, the proposed adsorption mechanism of 2,4-DCP adsorption on the three adsorbents from aqueous solution is presented as follows.
The adsorption mechanism of 2,4-DCP on PAni and PAni:PPy chain can be attributed to several forms of interactions [3]. The mechanism involves the electrostatic interaction between negatively charged groups available on the adsorbent surface with positively charged groups of the 2,4-DCP. The adsorption mechanism also includes hydrogen bonding interactions between nitrogen atoms in the polymer backbone and hydrogen atoms in the 2,4-DCP molecule. Finally, π-π interactions can occur between the aromatic rings of the polymer matrix and the aromatic ring of 2,4-DCP. According to the possibilities mentioned above, these interactions were responsible and essential for the enhancement of the 2,4-DCP adsorption on the PAni and PAni:PPy surfaces. Similar results have been reported by other studies for the adsorption of 2,4-DCP by biocomposites [3] and herbicide by polyaniline/polypyrrole composites with cellulosic biomass [2]. In the case of the PAni:PPy@SiO 2 adsorbent, we know that the 2,4-DCP is a positively charged molecule that can interact electrostatically with negatively charged molecules for SiO 2 moieties and also with electron-rich moieties in the polymer backbone. In addition, the formation of hydrogen bonds between nitrogen atoms for copolymer (PAni:PPy) and hydrogen-containing groups of 2,4-DCP can also occur. The π-π interactions between the aromatic rings of the adsorbate molecules and the copolymer chain structures of the adsorbent can be expected. Scheme 2 shows the proposed adsorption mechanism of adsorbents of 2.4-DCP by PAni:PPy@SiO 2 . mechanism of 2,4-DCP adsorption on the three adsorbents from aqueous solution is presented as follows.
The adsorption mechanism of 2,4-DCP on PAni and PAni:PPy chain can be attributed to several forms of interactions [3]. The mechanism involves the electrostatic interaction between negatively charged groups available on the adsorbent surface with positively charged groups of the 2,4-DCP. The adsorption mechanism also includes hydrogen bonding interactions between nitrogen atoms in the polymer backbone and hydrogen atoms in the 2,4-DCP molecule. Finally, π-π interactions can occur between the aromatic rings of the polymer matrix and the aromatic ring of 2,4-DCP. According to the possibilities mentioned above, these interactions were responsible and essential for the enhancement of the 2,4-DCP adsorption on the PAni and PAni:PPy surfaces. Similar results have been reported by other studies for the adsorption of 2,4-DCP by biocomposites [3] and herbicide by polyaniline/polypyrrole composites with cellulosic biomass [2]. In the case of the PAni:PPy@SiO2 adsorbent, we know that the 2,4-DCP is a positively charged molecule that can interact electrostatically with negatively charged molecules for SiO2 moieties and also with electron-rich moieties in the polymer backbone. In addition, the formation of hydrogen bonds between nitrogen atoms for copolymer (PAni:PPy) and hydrogen-containing groups of 2,4-DCP can also occur. The π-π interactions between the aromatic rings of the adsorbate molecules and the copolymer chain structures of the adsorbent can be expected. Scheme 2 shows the proposed adsorption mechanism of adsorbents of 2.4-DCP by PAni:PPy@SiO2. Scheme 2. Proposed adsorption mechanism of 2.4-DCP by PAni:PPy@SiO2.

Reusability of Adsorbents
Adsorbent regeneration was verified, defined as the ability to recover the 2,4-DCP molecules accumulated on the surface of the adsorbent and make it feasible to reuse in further adsorption/desorption cycles. The adsorbent/adsorbate interaction force and the amount of adsorbate loaded on the adsorbent play an important role in the regeneration test. Therefore, in the above context, the response surface optimized conditions were pH 6.0, 0.1 g/100 mL of adsorbent dosage, and an initial 2,4-DCP concentration of 50 mg.L −1 , followed by elution with 0.1 M HNO3. Five successive adsorption-desorption experiments were performed to measure the reusability of the adsorbents. After each experiment, the adsorbents were washed with distilled water, then dried at 60 °C, and reused for the next run. Figure 10 exhibits the materials reusability for 2,4-DCP removal. It can be observed that PAni:PPy@SiO2 maintains a very significant level of 2,4-DCP adsorption during five cycles, thus emerging as a typical alternative to traditional adsorbents for the elimination of this class of pollutants. Conversely, it should be noted that polymer and copolymer showed a decrease in productivity after each cycle. The percentages of adsorption of 2,4-DCP by PAni:PPy for the second, third, fourth, and fifth cycles were 72.45%, 65.82%, 57.42%, and 41.88%, respectively Such a remarkable decrease is due to the fundamental weight loss that took place at the time of regeneration and during the washing of the adsorbent. This also leads to a decrease in adsorption capacity in every regenerated cycle Scheme 2. Proposed adsorption mechanism of 2.4-DCP by PAni:PPy@SiO 2 .

Reusability of Adsorbents
Adsorbent regeneration was verified, defined as the ability to recover the 2,4-DCP molecules accumulated on the surface of the adsorbent and make it feasible to reuse in further adsorption/desorption cycles. The adsorbent/adsorbate interaction force and the amount of adsorbate loaded on the adsorbent play an important role in the regeneration test. Therefore, in the above context, the response surface optimized conditions were pH 6.0, 0.1 g/100 mL of adsorbent dosage, and an initial 2,4-DCP concentration of 50 mg·L −1 , followed by elution with 0.1 M HNO 3 . Five successive adsorption-desorption experiments were performed to measure the reusability of the adsorbents. After each experiment, the adsorbents were washed with distilled water, then dried at 60 • C, and reused for the next run. Figure 10 exhibits the materials' reusability for 2,4-DCP removal. It can be observed that PAni:PPy@SiO 2 maintains a very significant level of 2,4-DCP adsorption during five cycles, thus emerging as a typical alternative to traditional adsorbents for the elimination of this class of pollutants. Conversely, it should be noted that polymer and copolymer showed a decrease in productivity after each cycle. The percentages of adsorption of 2,4-DCP by PAni:PPy for the second, third, fourth, and fifth cycles were 72.45%, 65.82%, 57.42%, and 41.88%, respectively Such a remarkable decrease is due to the fundamental weight loss that took place at the time of regeneration and during the washing of the adsorbent. This also leads to a decrease in adsorption capacity in every regenerated cycle because of the reduction in binding sites present during the process owing to the 2,4-DCP molecules that were adsorbed. The results showed that about 41% of 2,4-DCP was eliminated in the fifth cycle, which is a significant rate, indicating the higher adsorption capacity of PAni:PPy adsorbent. In addition, after the first two runs, PAni progressively reduced its ability to adsorb 2,4-DCP, which is related to a gradual saturation of the active sites, even though its adsorption capacity remained greater than 31% after five cycles. because of the reduction in binding sites present during the process owing to the 2,4-DCP molecules that were adsorbed. The results showed that about 41% of 2,4-DCP was eliminated in the fifth cycle, which is a significant rate, indicating the higher adsorption capacity of PAni:PPy adsorbent. In addition, after the first two runs, PAni progressively reduced its ability to adsorb 2,4-DCP, which is related to a gradual saturation of the active sites, even though its adsorption capacity remained greater than 31% after five cycles.

Conclusions
In this work, a simple method was used to prepare a novel adsorbent of PAni:PPy@SiO2, and its effects on the elimination of 2,4-DCP were studied. This adsorbent was formed by the in situ polymerization of pyrrole and aniline in the presence of SiO2 by APS. In order to determine the composition and electrochemical behavior of the samples, their optical and chemical compositions and morphological characteristics were determined using ultraviolet-visible spectrophotometry, X-ray diffraction, infrared spectros-

Conclusions
In this work, a simple method was used to prepare a novel adsorbent of PAni:PPy@SiO 2 , and its effects on the elimination of 2,4-DCP were studied. This adsorbent was formed by the in situ polymerization of pyrrole and aniline in the presence of SiO 2 by APS. In order to determine the composition and electrochemical behavior of the samples, their optical and chemical compositions and morphological characteristics were determined using ultraviolet-visible spectrophotometry, X-ray diffraction, infrared spectroscopy, thermogravimetric analysis, and transmission electron microscopy. Moreover, the PAni:PPy@SiO 2 obtained a significantly high removal capacity of 24.90 mg·g −1 at pH 6.0, T = 25 • C, [2,4-DCP] = 50 mg·L −1 , and a homogeneous chemical monolayer adsorption process was described according to the PSO and Langmuir isotherm models. The enthalpy change (∆H), free energy change (∆G), and entropy change (∆S) data were also determined, which showed the favorable exothermic adsorption process of 2,4-DCP. Furthermore, the PAni:PPy@SiO 2 showed perfect recyclability, which is an important advantage in the adsorption process.