pp 1–11 | Cite as

Removal of 2,4-D herbicide from aqueous solution by aminosilane-grafted mesoporous carbons

  • Joanna GoscianskaEmail author
  • Anna Olejnik
Open Access


2,4-Dichlorophenoxyacetic acid (2,4-D) is the most commonly used herbicide in plant protection products. 2,4-D is poorly biodegradable and it is often found in aquatic environment. The development of an effective way to reduce the amount of this toxic contaminant from aqueous solution became an urgent issue. Therefore, in this study series of aminosilane-grafted mesoporous carbons were synthesized, characterized and then applied as adsorbents for 2,4-D. The impact of various factors such as the contact time (0–360 min) of herbicide with adsorbents, pH (2–11), temperature (25, 45, 60 °C) and initial concentration (6.25–150 mg/l) of the 2,4-D on the sorption capacity of materials was analyzed. The results proved that functionalization of mesoporous carbons with aminosilane increased the sorption capacity (qe = 142–191 mg/g) towards herbicide compared to pristine material (qe = 109 mg/g). The functional groups presented on the surface of materials enhanced the interaction between mesoporous carbons and herbicide. The most effective adsorbent for 2,4-D was the material that had the highest amount of basic groups on the surface (2.79 mmol/g) of all samples tested (0.06–0.52 mmol/g). For all studied materials the Langmuir model was the most suitable to describe the isotherms of 2,4-D adsorption (R2 = 0.999). While the kinetics of herbicide adsorption on the functionalized mesoporous carbons were best fitted to the pseudo-second-order model. The presented study proved that the aminosilane-grafted mesoporous carbons could be promising adsorbents for effective removal of 2,4-D from aqueous environment.


2,4-Dichlorophenoxyacetic acid Pesticide Adsorption Functionalization of mesoporous carbons Hard template method 3-Aminopropyltriethoxysilane 

1 Introduction

Large amounts of synthetic organic pollutants including pesticides, herbicides, dyes and pharmaceuticals are daily released into many types of wastewaters and enter into natural water channels to be accumulated in the aquatic environment (Agarwal et al. 2016; Bartczak et al. 2016; Goscianska et al. 2017). These contaminations arise from urban, industrial and agricultural human activities. Among numerous herbicides, 2,4-dichlorophenoxyacetic acid (2,4-D) is the most popular component of plant protection products. 2,4-D is commonly applied in agriculture due to its low cost and good selectivity (Liu et al. 2016). It stimulates the cells to uncontrolled growth that leads to the plant’s death in the last stage (Bartczak et al. 2016). 2,4-dichlorophenoxyacetic acid is widely applied in the cultivation of soya, maize, sugar cane and wheat. It is extensively used to control the growth of broad-leaf weeds in grain and cereal crops. However, this compound is poorly biodegradable therefore it is often found in water reservoir all over the world (Aksu and Kabasakal 2004). It has been proved that this pesticide could not only pose a threat to aquatic life but also could be toxic to animals and humans (Bus and Hammond 2007). It was reported that 2,4-D could have a negative influence on the proper functioning of the human beings. The oral exposure of humans to 2,4-D may induce headache, diarrhea and confusion (Reigart and Roberts 1999). Moreover, this compound is classified as carcinogenic, mutagenic and can have negative effect on the central nervous system and kidneys (Bradberry et al. 2004). Furthermore, the long-term exposure to 2,4-D may cause moderate and serious skin irritation (Njoku and Hameed 2011). Therefore, the development of an effective way to reduce the amount of 2,4-D in environment became an urgent and important issue. So far different methods have been used to remove herbicides from aqueous solutions such as coagulation, photodegradation, sedimentation, flotation, filtration and chemical oxidation (Ormad et al. 2008; Tsogas et al. 2006; Broseus et al. 2009). However, adsorption has been found to be the most competitive method due to its low cost, mild operation conditions, flexibility and ease of operation (Ova and Ovex 2013). It is assumed that this process could be a promising alternative to conventional water treatment systems. So far 2,4-D was adsorbed on different types of materials such as activated carbon (Njoku et al. 2015), modified silica gel (Koner et al. 2013), polystyrene beads (Olejnik et al. 2018a, b), chitosan (Harmoudi et al. 2014), bentonite (Li et al. 2009), magnetic graphene (Liu et al. 2016) and graphene oxide coated with porous iron oxide ribbons (Nethaji and Sivasamy 2017). However, the application of these materials on a larger scale has some drawbacks. On one hand the production and regeneration costs of activated carbons are very high. On the other hand the adsorption capacity of other sorption materials was not satisfactory enough. Therefore, there is still demand to search for new efficient adsorbent for 2,4-D. The recent progress in obtaining novel functionalized nanomaterials such mesoporous carbons has open new path for their applications (Barczak et al. 2015; Goscianska et al. 2016a, b, 2017; Yang et al. 2018). In the present study, 3-aminopropyltriethoxysilane-functionalized mesoporous carbons were applied for the first time as adsorbents of 2,4-D (Fig. 1). The effect of the contact time of adsorbate with adsorbents, pH, initial concentration of the 2,4-D anionic herbicide solution and temperature on the sorption capacity of materials was established. The experimental data obtained from the equilibrium studies were fitted to Langmuir and Freundlich adsorption models. In addition, kinetic studies were also carried out to determine both adsorption and desorption processes.

Fig. 1

Structure of 2,4-dichlorophenoxyacetic acid

2 Experimental

2.1 Adsorbent preparation

2.1.1 Synthesis of KIT-6 template

Ordered mesoporous silica KIT-6 of cubic structure was hydrothermally synthesized according to the procedure described previously (Goscianska et al. 2013). Briefly, 4 g of Pluronic P123 triblock copolymer (EO20PO70EO20, Aldrich) was dissolved in a mixture of 144 g of distilled water and 7.9 g of hydrochloric acid (35–38%, made by POCh), and stirred at 35 °C for 2 h. Then 4 ml of butan-1-ol (POCh) was added. After 1 h of stirring, 8.6 ml of tetraethyl orthosilicate (98 wt%, Sigma-Aldrich) was introduced dropwise to the solution, which was maintained at 35 °C for further 24 h under stirring. The resulting sol–gel slurries were hydrothermally aged for 24 h at 100 °C. Next, the solid product was filtered without washing and dried at 100 °C for 24 h in an air oven. Finally, the sample was calcined at 550 °C in air to remove the triblock copolymer and to obtain KIT-6 silica material.

2.1.2 Synthesis of ordered mesoporous carbon

In a typical synthesis of carbon material CKIT-6, 1 g of silica material KIT-6 was immersed in a solution of 1.25 g of sucrose (Aldrich), 0.14 g of concentrated H2SO4 (95%, Chempur) and 5 ml of distilled water. The mixture was heated for 6 h at 100 °C and then the temperature was increased to 160 °C for another 6 h. The resulting solid was again immersed into a solution of 0.8 g of sucrose, 0.09 g of H2SO4 and 5 ml of water. The heating process was repeated again by drying the mixture at 100 °C and 160 °C for 6 h. The carbonization was completed by pyrolysis with heating to typically 900 °C for 6 h in argon atmosphere. After carbonization, the template-containing carbon was washed with 5 wt% hydrofluoric acid (Sigma-Aldrich) twice at room temperature to remove the silica template. The template-free product was washed with water and then with ethanol before drying at 100 °C overnight.

2.1.3 Functionalization of mesoporous carbon

The main goal of the modification was the creation of basic groups on the surface of the pristine mesoporous carbon. The functionalization of CKIT-6 material was performed in two steps: Oxidation

For a typical treatment, 0.5 g of CKIT-6 sample was put into the reactor filled with 30 ml of 1 mol/l acidic ammonium persulfate solution and stirred for 6 h at 60 °C. After that, the mixture was filtered and washed with distilled water and ethanol. The material obtained was dried at 100 °C overnight. Grafting with 3-aminopropyltriethoxysilane (APTES)

At first 1.2, 3 or 6 ml of APTES were stirred for 30 min with 30 ml of methanol (POCh) in three round-bottomed flasks and then 3 g portions of oxidized carbon material was introduced. The mixtures were stirred at 40 °C for 8 h. In the next step, the grafted carbon materials were filtered, washed with methanol and dried at 100 °C overnight. Aminosilane-functionalized samples were labelled as CKIT-6-A1 (material modified with 1.2 ml of APTES), CKIT-6-A2 (material modified with 3 ml of APTES) and CKIT-6-A3 (sample modified with 6 ml of APTES).

2.2 Adsorbent characterization

Textural characteristic of the mesoporous carbons was performed with the use of a Quantachrome Autosorb IQ apparatus by nitrogen adsorption/desorption measurements at − 196 °C. The Brunauer–Emmett–Teller (BET) method was employed for the determination of surface areas (SBET) of carbon materials. Micropore surface areas were found using the t-plot method, whereas the total pore volumes were obtained from the amount of N2 adsorbed at a relative pressure close to unity. The average pore size was estimated from the adsorption branch of isotherm using Barret-Joyner-Halenda (BJH) method.

For TEM measurements, all adsorbents were deposited on a grid with a perforated carbon film and transferred to a JEOL 2000 electron microscope operating at 80 kV.

The content of oxygen functional groups on the surface of the aminosilane-grafted mesoporous carbons was determined by the Boehm method (Boehm 1994). The acidic surface functional groups were neutralized by 0.1 mol/l solution of sodium hydroxide, while the basic surface functional groups were neutralized by 0.1 mol/l solution of hydrochloric acid. The excess of the reagent used was titrated with 0.1 mol/l solution of HCl (upon neutralization with NaOH solution) or 0.1 mol/l solution of NaOH (upon neutralization with HCl solution) against methyl orange as an indicator.

2.3 Adsorption studies

For each adsorption test, 20 mg of mesoporous carbon was flooded with 50 ml of earlier prepared 2,4-D solutions of different concentrations from the range 6.25–150 mg/l. The flooded materials were continuously stirred in the temperature-controlled orbital shaker (KS 4000i control, IKA, Germany) at a fixed shaking rate of 250 rpm over a given period of time. Then the samples were filtered off and the solid phase was separated from the liquid. The absorbance of the filtrate was measured by using Agilent Cary 60 UV–Vis spectrophotometer (at the wavelength of 282 nm).

The amount of the 2,4-D anionic herbicide adsorbed on a given mesoporous carbon (qe) expressed in (mg/g) was calculated from formula (1):
$${q_e}=\frac{{({C_0} - {C_e}) \cdot V}}{m}$$
where C0 is the initial concentration of the 2,4-D (mg/l), Ce is the 2,4-D herbicide concentration after adsorption (mg/l), V is the volume of herbicide solution (l), m is the mass of mesoporous carbon material (g).

The effect of adsorption parameters such as the contact time of adsorbate-adsorbent (0–360 min), pH (2–11), the initial herbicide concentration (6.25–150 mg/l) and adsorption temperature (25, 45, 60 °C) on the sorption capacity of the materials obtained was investigated in details.

2.4 Desorption studies

For desorption tests, 2,4-D was first adsorbed onto mesoporous carbons by a solvent evaporation technique to obtain the same initial quantity of herbicide in all materials. For this purpose, 25 mg of carbon materials was added to 5 ml of an aqueous solution of 2,4-D with concentration of 1 mg/ml. The adsorption procedure was carried out for 24 h, with stirring. Afterwards the solvent was evaporated and the samples loaded with herbicide were dried for 24 h at 100 °C. The desorption was conducted for 24 h in distilled water maintained at RT. The desorption progress was monitored every 30 min during the first 3 h. Next the samples were withdrawn every hour up to 6 h. The last measurement was performed after 24 h. The concentration of 2,4-D desorbed was measured at 282 nm with the use of Agilent Cary 60 UV–Vis spectrophotometer.

2.5 Desorption kinetics

The desorption data were fitted with five different kinetics models such zero order (% 2,4-D desorbed vs time), first order (log of % 2,4-D remaining vs time), Higuchi model (% 2,4-D desorbed vs square root of time), Hixson-Crowell model (cube root of % of 2,4-D remaining vs time) and Korsmeyer–Peppas model (log of % 2,4-D desorbed vs log time) in which n value describes the desorption mechanism of 2,4-D using the following criteria:

  • n < 0.5 (0.45)—quasi-Fickian diffusion,

  • n = 0.5 (0.45)—diffusion mechanism,

  • 0.5 < n < 1—non Fickian diffusion,

  • n = 1 (0.89)—case II transport (zero order),

  • n > 1 (0.89)—super case II transport (Goscianska et al. 2016a, b; Sahoo et al. 2012; Dash et al. 2010; Olejnik et al. 2018a, b).

3 Results and discussion

3.1 Characterization of adsorbents

Structural and textural characterization of the aminosilane-grafted mesoporous carbons applied in this work as adsorbents of 2,4-D have already been published (Goscianska and Olejnik 2018) and therefore it will be only briefly recalled here.

The porous properties of materials were analyzed by N2 adsorption–desorption measurements and are depicted in Fig. 2. These data indicate that pristine mesoporous carbon exhibits the best developed surface area of 834 m2/g and large pore volume of 1.09 cm3/g with the contribution from micropores of 170 m2/g and 0.08 cm3/g. It was observed that the process of functionalization of the CKIT-6 material with 3-aminopropyltriethoxysilane strongly affected its textural parameters. As it can be seen the specific surface area of carbon decreases from 834 to 228 m2/g for CKIT-6-A1, 169 m2/g for CKIT-6-A2 and 71 m2/g for CKIT-6-A3. The total pore volumes decline gradually in the same order. The changes in the carbon texture are related to the anchoring of organic functional groups in the material pores. Moreover, the samplesCKIT-6-A1, CKIT-6-A2 and CKIT-6-A3 are also characterized by a greater mean pore size than CKIT-6. It can be concluded that the functionalization of the carbon surface with APTES happens at the micropore/mesopore openings, due to the high potential field in small pores and the easy susceptibility of attachment at the pore openings.

Fig. 2

Textural parameters of mesoporous carbons: A specific surface areas, B average pore diameters and total pore volumes

A series of aminosilane-grafted mesoporous carbons were investigated by transmission electron microscopy to observe ordering of their structure. TEM images of the samples synthesized are presented in Fig. 3. The pristine mesoporous carbon shows a highly ordered cubic mesostructure, an inverse replica of KIT-6 silica. TEM images also suggest that pore structure is not destroyed after functionalization of CKIT-6 with APTES, however, some structural changes are observed. The material grafted with the highest amount of aminosilane (CKIT-6-A3) exhibits slightly poorer structure ordering than other samples.

Fig. 3

TEM images of CKIT-6 (A), CKIT-6-A1 (B), CKIT-6-A2 (C), CKIT-6-A3 (D)

The content of oxygen functional groups on the surface of materials was determined by Boehm titration and the results are presented in Fig. 4. As can be observed, CKIT-6-A1, CKIT-6-A2 and CKIT-6-A3 samples are characterized by higher number of oxygen functional groups of basic character than pure mesoporous carbon. This indicates, on the one hand, the efficiency of functionalization, on the other hand, suggests differences in the nature of surface chemistry of the adsorbents. Moreover, the modification of CKIT-6 sample with 3-aminopropyltriethoxysilane in the highest concentration leads to total disappearance of acidic groups.

Fig. 4

Acid-base properties of pristine and functionalized mesoporous carbons

3.2 Adsorption studies

The relations between the amount of the 2,4-D adsorbed (qe) and the contact time of the mesoporous carbons surface with herbicide solution are presented in Fig. 5. For the first 20 min of contact the process is very fast, which can be explained by a large number of free adsorption sites available for the 2,4-D molecules. At the next stage, from 30 to about 100 min, adsorption is much slower because most of free adsorption sites on the surface of carbon materials have been occupied by herbicide molecules. After about 120 min the state of equilibrium is reached, (Fig. 5). After this time the value of qe shows no further increase.

Fig. 5

Influence of contact time on the amount of 2,4-D adsorbed onto mesoporous carbons

Kinetics of 2,4-D herbicide adsorption onto aminosilane-grafted mesoporous carbons was characterized on the basis of comparison to two kinetic models. The Lagergren model of pseudo-first order kinetics is described by the following equation (Lagergren 1898):
$$\ln ({q_e} - {q_t})=\ln \;{q_e} - \frac{{{k_1}t}}{{2.303}}$$
where qe is the amount of 2,4-D herbicide adsorbed at equilibrium (mg/g), qt is the amount of 2,4-D herbicide adsorbed in time t (mg/g), t is the time (min), k1 is the adsorption rate constant of pseudo-first order kinetics (1/min). For adsorption of 2,4-D herbicide the values of k1 were found from the plots of ln(qe − qt) on t (Fig. 6a).
Fig. 6

Pseudo-first-order (A) and pseudo-second-order (B) kinetic plots for adsorption of herbicide onto mesoporous carbons (initial solution concentration of 2,4-D—100 mg/l)

A linear form of pseudo-second-order kinetic model of Ho and McKay was expressed by equation (Ho and McKay 1999):
where k2 is the adsorption rate constant of pseudo-second order kinetics (g/mg/min). The values k2 were found from the plots of t/qt on t (Fig. 6b).

The values of the constants k1, k2, correlation coefficients (R2) and the calculated values of adsorbed 2,4-D (qe(cal)) are given in Table 1. Much higher values of R2 were obtained for the pseudo-second-order kinetic model, so this model better describes the herbicide adsorption (R2 ∼ 0.999) than the Lagergren model. The values of R2 for the pseudo-first-order kinetic are much lower (0.918–0.987). Moreover, the experimental values of qe are closer to qcal calculated on the basis of the pseudo-second-order model (Table 1).

Table 1

Parameters of pseudo-first-order and pseudo-second-order kinetic models for adsorption of 2,4-D herbicide onto mesoporous carbons


qe(exp) (mg/g)

Pseudo-first-order model

Pseudo-second-order model

qe(cal) (mg/g)

k1 (1/min)


qe(cal) (mg/g)

k2 (g/mg/min)


































The pH of aqueous solutions has an important role that influences uptake of adsorbate by mesoporous carbons. The adsorption performance of 2,4-D herbicide on the samples CKIT-6, CKIT-6-A1, CKIT-6-A2, CKIT-6-A3 as a function of pH was investigated in the range of 2–11, and the results are presented in Fig. 7. It was found that removal of 2,4-D by carbon adsorbents at the initial stage increased with an increase in pH from 2 to 3, then remained almost unaffected up to pH of 5. Further increase of pH in the range from 7 to 11 led to a decrease in sorption capacity of materials towards 2,4-D. Because of low pKa value (2.73) of herbicide, it exists predominantly in anionic form (Bartczak et al. 2016; Koner et al. 2013). In acidic solutions the aminosilane-grafted mesoporous carbons become more positively charged which results in greater adsorption of anionic species.

Fig. 7

Effect of pH on the removal of 2,4-D herbicide by aminosilane-functionalized mesoporous carbons (initial solution concentration of 2,4-D—100 mg/l)

The effectiveness of adsorption process is significantly influenced by the initial concentration of 2,4-D. Figure 8 presents the equilibrium adsorption isotherms of anionic herbicide onto aminosilane-grafted mesoporous carbons in aqueous solution. The adsorption is measured in milligrams of 2,4-D per a gram of adsorbent. For all samples the adsorbed amount of herbicide increases with increasing initial concentration until the plateau is reached. A higher initial 2,4-D concentration led to an increase in the mass gradient between the aqueous solution and the carbon materials, which then functions as a driving force for the transfer of herbicide molecules from the bulk solution to the adsorbents surface.

Fig. 8

Adsorption isotherms of 2,4-D herbicide onto mesoporous carbons

According to Fig. 8, the maximum sorption capacities of the mesoporous carbons are in the range 109–191 mg/g. As follows from analysis, much more effective adsorbents of 2,4-D are the samples grafted with 3-aminopropyltriethoxysilane than pristine carbon CKIT-6. It can be concluded that basic functional groups present on the surface of CKIT-6-A1, CKIT-6-A2 and CKIT-6-A3 enhance the interaction between the carbon materials and the anionic herbicide.

The adsorption isotherms were fitted to the two models proposed by Langmuir and Freundlich. The Langmuir adsorption isotherm is described by the following linear equation (Langmuir 1918):
where qe is the experimentally determined amount of the 2,4-D herbicide adsorbed on the samples (mg/g), qm is the theoretically predicted amount of adsorbed 2,4-D herbicide (mg/g), Ce is the equilibrium concentration of the 2,4-D solution (mg/l), KL is the Langmuir constant. The parameters were computed from the intercept and linear gradient of the graphs of Ce/qe and Ce (Fig. 9a).
Fig. 9

Fit of experimental data concerning adsorption of 2,4-D herbicide onto mesoporous carbons, to the Langmuir (A) and Freundlich (B) models

The linear form of Freundlich isotherm equation is expressed as (Freundlich 1906):
$${\text{ln }}{{\text{q}}_{\text{e}}}={\text{ ln }}{{\text{K}}_{\text{F}}}+{\text{ 1}}/{\text{n ln }}{{\text{C}}_{\text{e}}}$$
where qe is the experimentally determined amount of the 2,4-D herbicide adsorbed on the samples (mg/g), Ce is the equilibrium concentration of the 2,4-D herbicide solution (mg/l), KF and 1/n is the Freundlich constants, characteristic of a given system. The value of 1/n (varying from 0 to 1) is a measure of the intensity of adsorption or heterogeneity of the surface. The closer it is to zero, the more heterogeneous the surface. The plots of lnqe versus lnCe are shown in Fig. 9b.

The calculated parameters of the Langmuir and Freundlich isotherms based on the experimental data are collected in Table 2. The results indicate that the experimental data could be better described by Langmuir model than the Freundlich model in terms of higher R2 values. Therefore, the 2,4-D molecules were adsorbed on the surface of carbon materials via monolayer adsorption in homogeneous adsorption sites. Moreover, it should be mentioned that the experimental values of maximum adsorption capacities (qe) are close to the theoretical value of the maximum adsorption capacity (qm) calculated with the use Langmuir model.

Table 2

Summary of parameters calculated from fitting the results of adsorption isotherms of 2,4-D herbicide onto mesoporous carbons to different models


qe(exp) (mg/g)



qm (mg/g)

KL (l/mg)


KF (mg/g (l/mg)1/n)



































The effect of temperature on the sorption capacity of aminosilane-grafted mesoporous carbons towards 2,4-D was also studied. According to the results, presented in Fig. 10, with temperature increasing from 25 to 60 °C, the amount of adsorbed anionic herbicide slightly increased. It can be related to greater mobility of the 2,4-D molecules in the aqueous solution. Within the porous structure of the carbon adsorbents the barrier of activation energy is overcome, which leads to the increase in the amount of the adsorbed herbicide.

Fig. 10

Effect of temperature on the removal of 2,4-D herbicide by aminosilane-functionalized mesoporous carbons (initial solution concentration of 2,4-D—100 mg/l)

Table 3 presents the values of the three thermodynamic parameters (∆G°, ∆H°, ∆S°) for the sorption of 2,4-D. The values of ΔG° (Gibbs free energy change) for each temperature were calculated taking into account the dimensionless constant KC, from the following thermodynamic equation:
$$\Delta {\text{G}}^\circ = -\, {\text{RT}}\;\ln \;{{\text{K}}_{\text{C}}}$$
where R is the universal gas constant (8.314 (J/K mol)), T is the absolute temperature (K), and KC is the adsorption constant (Bartczak et al. 2016; Koner et al. 2013; Gupta et al. 2016).
Table 3

Thermodynamic parameters for the adsorption of 2,4-D herbicide onto mesoporous carbons


Temperature (°C)

ΔG° (kJ/mol)

ΔH° (kJ/mol)

ΔS° (J/Kmol)



− 16.85




− 18.08


− 19.20



− 19.09




− 20.59


− 21.66



− 19.43




− 20.95


− 22.11



− 20.48




− 21.91


− 23.07

In order to determine the changes in enthalpy (ΔH°) and entropy (ΔS°), the plots of ln KC on 1/T were made using the following equation (Verma et al. 2017):
$$\ln {{\text{K}}_{\text{C}}}=~\frac{{{{\varvec{\Delta}S}}}}{{\text{R}}} - ~\frac{{{{\varvec{\Delta}H}}}}{{{\text{RT}}}}$$

The positive values of ∆H° (in the range 1.48–3.34 kJ/mol) obtained for all samples suggest that the 2,4-D adsorption is of endothermic nature, while the negative values of ΔG° imply that it is a spontaneous process. When temperature is increased from 25 to 60 °C, ∆G° decreases, so the degree of spontaneity of the thermodynamic reaction increases. The values of entropy vary in the range 66.69–76.39 J/K mol (Table 3).

Thus far, numerous adsorbents have been applied for 2,4-D removal from aqueous solutions. A comparison of literature sorption capacities of different materials towards 2,4-D herbicide is presented in Table 4. Aminosilane-grafted mesoporous carbons are more effective adsorbents of 2,4-D than powdered activated carbons (Aksu and Kabasakal 2004), Cladium mariscus (Bartczak et al. 2016), chitosan (Harmoudi et al. 2014), chitin (Harmoudi et al. 2014), blast furnace sludge (Gupta et al. 2006), blast furnace dust (Gupta et al. 2006) or modified silica gel (Koner et al. 2013). This high adsorption capacity could be ascribed to the unique properties of carbon materials obtained (Goscianska and Olejnik 2018). The samples modified with APTES have good dispersibility in water solutions due to the presence of organic functional groups on their surface. Therefore, the diffusion resistance between adsorbents and 2,4-D molecules could be reduced.

Table 4

Comparison of the adsorption capacity of mesoporous carbons towards 2,4-D herbicide with various adsorbents


Sorption capacities (mg/g)


Cladium mariscus


Bartczak et al. (2016)



Harmoudi et al. (2014)



Harmoudi et al. (2014)

Powdered activated carbon


Aksu and Kabasakal (2004)

Commercial activated carbon (AC F400)


Son Tran et al. (2015)

Modified silica gel


Koner et al. (2013)

Blast furnace sludge


Gupta et al. (2006)

Blast furnace dust


Gupta et al. (2006)

Mesoporous carbon CKIT-6


This study

Aminosilane-grafted mesoporous carbons


This study

3.3 Desorption studies

It can be seen in Fig. 11 that functionalization of mesoporous carbon material has an influence on the desorption process of herbicide. After 24 h the percentage of desorbed 2,4-D from mesoporous carbons was as follows 30% (CKIT-6), 45% (CKIT-6-A3), 56% (CKIT-6-A2), 63% (CKIT-6-A1). This pattern may be related to the sorption strength of the herbicide on the carbon materials. Much lower amount of 2,4-D was desorbed from non-functionalized mesoporous carbon than from the modified materials. We suggest that the 2,4-D molecules were loaded inside the pores of CKIT-6 and therefore they could not be easily desorbed to receptor medium. The modification of mesoporous carbon surface changed the sorption–desorption properties towards 2,4-D. Moreover, the amount of basic and acidic groups on the surface may influence the yield of herbicide’s desorption. The amount of 2,4-D desorbed from functionalized materials decreased when higher amount of basic groups were loaded on the surface of mesoporous carbons. According to Aquino et al. (2007) the molecules of 2,4-D can interact via hydrogen bonds with different functional groups in polar solvents. The mechanism of 2,4-D adsorption could be also based on electrostatic interactions between the negatively charged herbicide and positively charged aminosilane-grafted mesoporous carbon. Furthermore, van der Waals forces could also contribute to interactions between 2,4-D and aminosilane-grafted mesoporous carbons. Depending on the strength of hydrogen bonds, van der Walls forces and electrostatic interactions, that act simultaneously, the desorption profiles were different. It is assumed that one fraction of 2,4-D molecules was located on the outer surface of the material. The total amount of 2,4-D was not desorbed in any case therefore we suggest that the second fraction of herbicide molecules might be located inside the pores of the carbon materials or may interact with their walls.

Fig. 11

2,4-D herbicide desorption curves for pristine and functionalized mesoporous carbons in distilled water

The mechanism of 2,4-D desorption from mesoporous carbon materials was explained by fitting the results with five different kinetics models. For all aminosilane-grafted mesoporus carbons the highest values of regression coefficient was observed for the Korsmeyer–Peppas model (Table 5). This suggests that the desorption of 2,4-D from CKIT-6-A1, CKIT-6-A2, CKIT-6-A3 followed this kinetics equation. The n values of all these materials were below 0.5 that indicates the Fickian diffusion mechanism. However, for pristine material the highest regression coefficient was calculated for the Higuchi model, which implies that the desorption of 2,4-D involved diffusion process.

Table 5

Kinetics models used to describe 2,4-D desorption from mesoporous carbon materials


Zero order

First order

Higuchi model

Hixson–Crowell model

Korsmeyer–Peppas model






























4 Conclusion

Ordered mesoporous carbon of cubic structure has been subjected to surface oxidation followed by functionalization with different amounts of 3-aminopropyltriethoxysilane. Aminosilane-grafted materials show smaller surface areas and total pore volumes but greater average pore diameter than the unmodified sample. The modification of mesoporous carbon with APTES leads to generation of basic functional groups on its surface.

According to the results obtained, the most effective adsorbent of 2,4-D from water solutions is the material CKIT-6-A3 whose surface shows the most basic character of all samples studied. The presence of amine groups on the carbon surface increases its sorption capacity towards the 2,4-D herbicide. The isotherms of 2,4-D adsorption, recorded for all samples studied, have been established to be of Langmuir type. The kinetics of herbicide adsorption on the aminosilane-grafted mesoporous carbons were better described by the pseudo-second-order model. With temperature increased from 25 to 60 °C, the sorption capacities of the materials studied towards 2,4-D increased. The process of 2,4-D adsorption was found to be endothermic and of spontaneous character as indicated by the positive values of ∆H and negative values of ∆G. According to the results obtained, the herbicide sorption was more effective in an acidic environment. The desorption efficiency was strongly affected by the amount of basic and acidic groups on the surface of functionalized carbons. It was observed that with increase in the amount of basic groups decreased the ability of 2,4-D to be desorbed from materials obtained.



Financial support from Polish Ministry of Science and Higher Education is acknowledged.


  1. Agarwal, S., Sadeghi, N., Tyagi, I., Gupta, V.K., Fakhri, A.: Adsorption of toxic carbamate pesticide oxamyl from liquid phase by newly synthesized and characterized grapheme quantum dots nanomaterials. J. Colloid Interface Sci. 478, 430–438 (2016)CrossRefGoogle Scholar
  2. Aksu, Z., Kabasakal, E.: Batch adsorption of 2,4-dichlorophenoxyacetic acid (2,4-D) from aqueous solution by granular activated carbon. Sep. Purif. Technol. 35, 223–240 (2004)CrossRefGoogle Scholar
  3. Aquino, A.J.A., Tunega, D., Haberhauer, G., Gerzabek, M.H., Lischka, H.: Interaction of the 2,4-dichlorophenoxyacetic acid herbicide with soil organic matter moieties: a theoretical study. Eur. J. Soil. Sci. 58, 889–899 (2007)CrossRefGoogle Scholar
  4. Barczak, M., Michalak-Zwierz, K., Gdula, K., Tyszczuk-Rotko, K., Dobrowolski, R., Dąbrowski, A.: Ordered mesoporous carbons as effective sorbents for removal of heavy metal ions. Microporous. Mesoporous. Mater. 211, 162–173 (2015)CrossRefGoogle Scholar
  5. Bartczak, P., Żółtowska, S., Norman, M., Klapiszewski, Ł, Zdarta, J., Komosa, A., Kitowski, I., Ciesielczyk, F., Jesionowski, T.: Saw-sedge Cladium mariscus as functional low-cost adsorbent for effective removal of 2,4-dichlorophenoxyacetic acid from aqueous systems. Adsorption 22, 517–529 (2016)CrossRefGoogle Scholar
  6. Boehm, H.P.: Some aspects of the surface chemistry of carbon blacks and other carbons. Carbon 32, 759–769 (1994)CrossRefGoogle Scholar
  7. Bradberry, S.M., Proudfoot, A.T., Vale, J.A.: Poisoning due to chlorophenoxy herbicides. Toxicol. Rev. 23, 65–73 (2004)CrossRefGoogle Scholar
  8. Broseus, R., Vincent, S., Aboulfadl, K., Daneshvar, A., Sauve, S., Barbeau, B., Prevost, M.: Ozone oxidation of pharmaceuticals, endocrine disruptors and pesticides during water treatment. Water Res. 43, 4707–4717 (2009)CrossRefGoogle Scholar
  9. Bus, J.S., Hammond, L.E.: Regulatory progress, toxicology, and public concerns with 2,4-D: where do we stand after two decades? Crop Prot. 26, 266–269 (2007)CrossRefGoogle Scholar
  10. Dash, S., Murthy, P.M., Nath, L., Chowdhury, P.: Kinetic modeling on drug release from controlled drug delivery systems. Acta Pol. Pharm. 67, 217–223 (2010)Google Scholar
  11. Freundlich, H.M.F.: Over the adsorption in solution. J. Phys. Chem. 57, 385–470 (1906)Google Scholar
  12. Goscianska, J., Olejnik, A.: Dispersion stability of the aminosilane-grafted mesoporous carbons in different solvents. Microporous Mesoporous Mater. 265, 149–161 (2018)CrossRefGoogle Scholar
  13. Goscianska, J., Olejnik, A., Pietrzak, R.: Adsorption of l-phenylalanine onto mesoporous silica. Mater. Chem. Phys. 142, 586–593 (2013)CrossRefGoogle Scholar
  14. Goscianska, J., Olejnik, A., Nowak, I.: Sorptive properties of aluminium ions containing mesoporous silica towards l-histidine. Adsorption 22, 571–579 (2016a)CrossRefGoogle Scholar
  15. Goscianska, J., Olejnik, A., Nowak, I., Marciniak, M., Pietrzak, R.: Stability analysis of functionalized mesoporous carbon materials in aqueous solution. Chem. Eng. J. 290, 209–219 (2016b)CrossRefGoogle Scholar
  16. Goscianska, J., Fathy, N.A., Aboelenin, R.M.M.: Adsorption of solophenyl red 3BL polyazo dye onto amine-functionalized mesoporous carbons. J. Colloid Interface Sci. 505, 593–604 (2017)CrossRefGoogle Scholar
  17. Gupta, V.K., Ali, I., Saini, V.K.: Adsorption of 2,4-D and carbofuran pesticides using fertilizer and steel industry wastes. J. Colloid Interface Sci. 299, 556–563 (2006)CrossRefGoogle Scholar
  18. Gupta, V.K., Chandra, R., Tyagi, I., Verma, M.: Removal of hexavalent chromium ions using CuO nanoparticles for water purification application. J. Colloid Interface Sci. 478, 54–62 (2016)CrossRefGoogle Scholar
  19. Harmoudi, H.El., Gaini, L.El., Daoudi, E., Rhazi, M., Boughaleb, Y., Mhammedi, M.A.El., Migalska-Zalas, A., Bakasse, M.: Removal of 2,4-D from aqueous solution by adsorption processing using two biopolymers: chitin and chitosan and their optical properties. Opt. Mater. 36, 1471–1477 (2014)CrossRefGoogle Scholar
  20. Ho, Y.S., McKay, G.: Pseudo-second order model for sorption processes. Process Biochem. 34, 451–465 (1999)CrossRefGoogle Scholar
  21. Koner, S., Pal, A., Adak, A.: Adsorption of 2,4-D herbicide from water environment on modified silica gel factory waste. Water Environ. Res. 85, 2147–2156 (2013)CrossRefGoogle Scholar
  22. Lagergren, S.: About the theory of so-called adsorption of soluble substances. Kungliga Svenska Vetensk. Handl. 24, 1–39 (1898)Google Scholar
  23. Langmuir, I.: The adsorption of gases on plane surfaces of glass, mica and platinum. J. Am. Chem. Soc. 40, 1361–1403 (1918)CrossRefGoogle Scholar
  24. Li, J., Li, Y., Lu, J.: Adsorption of herbicides 2,4-D and acetochlor on inorganic-organic bentonites. Appl. Clay Sci. 46, 314–318 (2009)CrossRefGoogle Scholar
  25. Liu, W., Yang, Q., Yang, Z., Wang, W.: Adsorption of 2,4-D on magnetic graphene and mechanism study. Colloids Surf. A 509, 367–375 (2016)CrossRefGoogle Scholar
  26. Nethaji, S., Sivasamy, A.: Graphene oxide coated with porous iron oxide ribbons for 2,4-Dichlorophenoxyacetic acid (2,4-D) removal. Ecotoxicol. Environ. Saf. 138, 292–297 (2017)CrossRefGoogle Scholar
  27. Njoku, V.O., Hameed, B.H.: Preparation and characterization of activated carbon from corncob by chemical activation with H3PO4 for 2,4-dichlorophenoxyacetic acid adsorption. Chem. Eng. J. 173, 391–399 (2011)CrossRefGoogle Scholar
  28. Njoku, V.O., Asif, M., Hameed, B.H.: 2,4-Dichlorophenoxyacetic acid adsorption onto coconut shell-activated carbon: isotherm and kinetic modeling. Desalin. Water Treat. 55, 132–141 (2015)CrossRefGoogle Scholar
  29. Olejnik, A., Nowak, I., Schroeder, G.: Functionalized polystyrene beads as carriers in release studies of two herbicides: 2,4-dichlorophenoxyacetic acid and 2-methyl-4-chlorophenoxyacetic acid. Int. J. Environ. Sci. Technol. (2018a)Google Scholar
  30. Olejnik, A., Glowka, A., Nowak, I.: Release studies of undecylenoyl phenylalanine from topical formulations. Saudi Pharm. J. 26, 709–718 (2018b)CrossRefGoogle Scholar
  31. Ormad, M.P., Miguel, N., Calvert, A., Matesanz, J.M., Obelleiro, J.L.: Pesticides removal in the process of drinking water production. Chemosphere 71, 97–106 (2008)CrossRefGoogle Scholar
  32. Ova, D., Ovex, B.: 2,4-Dichlorophenoxyacetic acid removal from aqueous solutions via adsorption in the presence of biological contamination. J. Environ. Chem. Eng. 1, 813–821 (2013)CrossRefGoogle Scholar
  33. Reigart, J.R., Roberts, J.R.: Chlorophenoxy Herbicides, recognition and management of pesticide poisonings, 5th edn., pp. 94–96. U.S. Environmental Protection Agency. Office of Prevention, Pesticides and Toxic Substances, Office of Pesticide Programs, U.S. Government Printing Office, Washington, DC (1999)Google Scholar
  34. Sahoo, S., Chakraborti, C.K., Behera, P.K.: Development and evaluation of gastroretentive controlled release polymeric suspensions containing ciprofloxacin and carbopol polymers. J. Chem. Pharm. Res. 4, 2268–2284 (2012)Google Scholar
  35. Son Tran, V., Ngo, H.H., Guo, W., Zhang, J., Liang, S., Ton-That, C., Zhang, X.: Typical low cost biosorbents for adsorptive removal of specific organic pollutants from water. Bioresour. Technol. 182, 353–363 (2015)CrossRefGoogle Scholar
  36. Tsogas, G.Z., Giokas, D.L., Nikolakopoulos, P.G., Vlessidis, A.G., Evmiridis, N.P.: Determination of the pesticide carbaryl and its photodegradation kinetics in natural waters by flow injection-direct chemiluminescence detection. Anal. Chim. Acta 573–574, 354–359 (2006)CrossRefGoogle Scholar
  37. Verma, M., Tyagi, I., Chandra, R., Gupta, V.K.: Adsorptive removal of Pb(II) ions from aqueous solution using CuO nanoparticles synthesized by sputtering method. J. Mol. Liq. 225, 936–944 (2017)CrossRefGoogle Scholar
  38. Yang, Y., Wang, J., Qian, X., Shan, Y., Zhang, H.: Aminopropyl-functionalized mesoporous carbon (APTMS-CMK-3) as effective phosphate adsorbent. Appl. Surf. Sci. 427, 206–214 (2018)CrossRefGoogle Scholar

Copyright information

© Springer Science+Business Media, LLC, part of Springer Nature 2019

OpenAccessThis article is distributed under the terms of the Creative Commons Attribution 4.0 International License (, which permits unrestricted use, distribution, and reproduction in any medium, provided you give appropriate credit to the original author(s) and the source, provide a link to the Creative Commons license, and indicate if changes were made.

Authors and Affiliations

  1. 1.Faculty of ChemistryAdam Mickiewicz University in PoznańPoznanPoland

Personalised recommendations