Guest Editor: C. T. Yavuz
Beilstein J. Nanotechnol. 2020, 11, 597–605. https://doi.org/10.3762/bjnano.11.47
Received 24 Dec 2019, Accepted 16 Mar 2020, Published 08 Apr 2020
Polyaniline-derived carbon (PDC) was obtained via pyrolysis of polyaniline under different temperatures and applied for the purification of water contaminated with dye molecules of different sizes and charge by adsorption. With increasing pyrolysis temperature, it was found that the hydrophobicity, pore size and mesopore volume increased. A mesoporous PDC sample obtained via pyrolysis at 900 °C showed remarkable performance in the adsorption of dye molecules, irrespective of dye charge, especially in the removal of bulky dye molecules, such as acid red 1 (AR1) and Janus green B (JGB). For example, the most competitive PDC material showed a Q0 value (maximum adsorption capacity) 8.1 times that of commercial, activated carbon for AR1. The remarkable adsorption of AR1 and JGB over KOH-900 could be explained by the combined mechanisms of hydrophobic, π–π, electrostatic and van der Waals interactions.
Keywords: acid red 1; adsorption; bulky dye molecules; Janus green B; polyaniline-derived carbon; water purification
Dyes have been widely used in a wide range of industries including textile, leather and paper, causing serious concern worldwide mainly because of the contamination of water resources. For example, around 700,000 tons of textile dyes are produced annually; and a considerable quantity of the produced dyes is discharged into waste water . Such dyes are usually toxic or are converted into toxic substances after further treatment [1,2], and dyes discarded in waste water inevitably increase the biochemical oxygen demand (BOD) and chemical oxygen demand (COD) levels. Additionally, dyes decrease sunlight penetration through water, decreasing the natural restoration activity of rivers. Moreover, dyes in waste water are also considered problematic in the aesthetic sense, since the absorbance of dyes is usually very high (therefore, even small quantity of dyes can affect the color of the water).
The removal of dye molecules from contaminated water is very important and has been carried out via various methods such as oxidation [3,4], including advanced oxidation processing (AOP), photocatalysis , biological treatment, coagulation, and membrane separation [2,6,7]. However, these techniques are not very satisfactory for applications on a large scale. For example, dyes are very resistant against degradation by catalysis, with a common example given by the stable characteristics of dyes under even sunlight. Recently, adsorption has been regarded to be very effective and attractive because of its operation under mild conditions and no need of oxidant, active catalyst, and irradiation [8,9]. Therefore, adsorption with carbon nanotubes, activated carbon (AC), biomass, and metallic–organic frameworks (MOFs) has been actively studied for the removal of dye molecules from water [10-15]. However, adsorbents with high adsorption capacity, structural integrity, low cost and facile recyclability are required for the practical operations or commercial applications.
So far, the development of various adsorbents has been successful because of functional carbon materials (graphene  or porous carbon ), mesoporous materials  and MOFs [19-22]. For example, MOFs [23-25], carbonaceous materials (such as carbon nanotubes, graphene, biochar and activated carbon)  and clay  have been applied in adsorptive removal of contaminants of emerging concern, hazardous organics and persistent organic pollutants. Carbonaceous materials have been particularly attractive in the purification of contaminated water via adsorption because of the easy preparation of carbon materials , especially from waste materials . Moreover, highly porous carbon materials, especially with high nitrogen content, have been produced from various precursors including organic polymers [29-33] and MOFs [34-38].
Polyaniline (PANI), prepared from aniline, is a useful polymer in various fields because of its facile synthesis, high conductivity and nitrogen content. Porous carbon materials, with high porosity and nitrogen content, have also been obtained from PANI. In other words, functional carbon, for catalysts and supercapacitors can be derived from high temperature carbonization of PANI, especially in the co-presence of activating agents such as KOH, H3PO4 or ZnCl2 . Even though PANI-derived carbon (PDC) was used in gas-phase adsorption [40,41], it has been scarcely applied in liquid phase adsorption. Only recently we applied PDC for the possible purification of water contaminated with organics and fuel containing dibenzothiophene or dimethyldibenzothiophene [42,43]. However, further research is required to utilize the highly porous PDC materials for the purification of water contaminated with organics such as dyes.
Herein, we utilized PDC, prepared especially at high temperature, for the purification of water contaminated with dyes, such as acid red 1 (AR1), Janus green B (JGB), methyl orange (MO) and methylene blue (MB), via adsorption. AR1 is a large anionic dye which is toxic and widely applied in the paper industry . Janus green B (JGB) is one of the most typical large cationic dyes that is widely used in several industries . MO and MB are widely applied anionic and cationic dyes, respectively . The chemical structures of the studied dyes are shown in Supporting Information File 1, Figure S1.
A PDC, obtained from PANI at 900 °C, showed remarkable performance in the adsorption of bulky dye molecules such as AR1 and JGB. For example, the PDC material developed in this work shows the highest adsorption capacity compared with any reported results, so far. Moreover, the adsorption capacity of the PDC material is more than 8 times that of a commercial, activated carbon. However, the adsorptive performance of the PDC for small dye molecules, such as MO and MB, was not very impressive, albeit quite competitive against similar reported results. The adsorption mechanisms could be suggested based on the physical properties (including hydrophobicity) of PDC materials and adsorption of AR1 and JGB under a wide range of pH values (from 2 to 12).
The porosity and pore size distribution of the adsorbents were characterized with nitrogen adsorption at 77 K. As shown in Figure 1a, the porosity of the PDC materials was considerable when the pyrolysis temperature was equal to or higher than 700 °C. The detailed porosity data are summarized in Supporting Information File 1, Table S1. With increasing pyrolysis temperature up to 800 °C, the BET surface area, total pore volume and mesopore volume increased. However, all of the porosity data (BET surface area, and total, micro- and mesopore volumes) decreased with further increasing temperature from 800 to 900 °C. Therefore, 800 °C was the optimum temperature to derive PDC materials with the highest porosity, excluding the micropore volume (for this, 750 °C was the most effective). Importantly, the pore size distribution patterns presented in Figure 1b show that the pore size of PDC increased with increasing pyrolysis temperature; and KOH-900, a PDC material that was obtained via pyrolysis of PANI at 900 °C, has an average pore size of ≈3 nm, which is very effective in adsorption of bulky dye molecules (vide infra). On the contrary, the pore size of activated carbon (AC) is very small (or mainly in microporous region); therefore, it might not be effective in adsorption of bulky dye molecules.
The hydrophobicity or hydrophilicity of PDC was estimated by checking the adsorbed quantity of water and n-octane . The quantity of adsorbed water decreased with increasing pyrolysis temperature, as shown in Figure 2a. On the contrary, the adsorbed n-octane showed the very opposite trend (Figure 2b). The adsorbed n-octane was in the order: KOH-900 > KOH-800 > KOH-750 > KOH-700 > KOH-600. The ratio of adsorbed vapors (n-octane/water, mol/mol) is shown as Figure 2c, and the ratio increased monotonically with increasing pyrolysis temperature. Therefore, it could be confirmed that the hydrophobicity of PDC increased with increasing pyrolysis temperature. This is understandable based on the enrichment of carbon (or successive removal of heteroatoms such as nitrogen and oxygen) with increasing pyrolysis temperature [42,43]. The best adsorbent (vide infra) KOH-900 was analyzed further with Raman spectroscopy. As shown in Supporting Information File 1, Figure S1, KOH-900 is composed of both graphitic and defect phases. Therefore, KOH-900 might be useful for adsorption because of defects and the graphitic layers (with π-electrons).
Firstly, adsorption of AR1 over PDC and AC was carried out for 6 h. As illustrated in Figure 3a, the adsorbed quantity (q6h, in mg/g) decreased in the order: KOH-900 > KOH-800 > KOH-750 > KOH-700 > AC > KOH-600. Therefore, the PDC materials are very competitive in AR1 adsorption compared to AC when the pyrolysis temperature is at 700 °C or higher. Considering the dominant role of porosity in adsorption , the q6h values were calculated based on the BET surface area of adsorbents. Curiously, as presented in Figure 3b, the q6h (in mg/m2) for AR1 showed a tendency similar to that of the quantity based on unit weight of adsorbents or PDC (q6h in mg/g). Therefore, it should be emphasized that there is another important contribution, excluding simple porosity, to explain the performance of the PDC materials in AR1 adsorption.
Considering that the best performance was found with KOH-900 (based on both unit weight and BET surface area), further experiments were done with KOH-900 and AC, as a standard adsorbent. Similar to AR1, other dye molecules (with different charge and size) were also adsorbed for 6 h over KOH-900 and AC. As presented in Figure 4, KOH-900 had a much higher q6h than AC for the four dyes studied, namely AR1, MO, MB, and JGB. However, the ratio of adsorbed quantity [q6h (KOH-900)/q6h (AC)] was very much dependent on the size of the adsorbed dye, as summarized in Supporting Information File 1, Table S2. KOH-900 showed much higher efficiency than AC especially in the adsorption of bulky dye molecules, such as AR1 and JGB.
Inspired by the remarkable performance of KOH-900 in the adsorption of bulky dye molecules, adsorption experiments were further carried out for AR1 and JGB over KOH-900 and AC for a wide range of adsorption times from 0.5 to 6 h. As illustrated in Figure 5, KOH-900 had a much higher adsorption capacity than AC for AR1 and JGB, irrespective of the adsorption time and the type of adsorbate or dye. In order to determine the maximum adsorption capacity of KOH-900 and AC for AR1, adsorption isotherms were obtained from adsorption for 6 h with a wide range of AR1 concentrations. The adsorption isotherms and Langmuir plots are illustrated in Figure 6a and 6b, respectively. The high correlation coefficients (R2 > 0.99) shown on Figure 6b confirm that the Langmuir equation can be adequately applied to interpret the observed adsorptions. As summarized in Table 1, KOH-900 had a Q0 (for AR1) value 8.1 times as that of commercial, activated carbon.
Table 1: Maximum adsorption capacity (Q0) of some reported adsorbents for the adsorption of AR1 from water.
|Adsorbents||SABET (m2·g−1)||Solution pH||Q0 (mg·g−1)||Ref.|
|TNTs (HDTMA-modified version) treated with 0.0001 N acid||45||–||396|||
|commercial activated carbon||1016||7.0||148||this work|
Understanding the adsorption mechanism is helpful to develop a competitive adsorption technology and to further improve the performance of an adsorbent. So far, several mechanisms , such as electrostatic [49,50], π–π [51-54], acid–base interactions [55,56], and hydrogen bonding [57-59], were applied to interpret various adsorption events. In order to understand the plausible mechanism, especially in aqueous phase, adsorption over a wide range of pH conditions is very effective  since both the adsorbate and adsorbent can be changed in terms of charge or functional group (for example, via protonation or deprotonation) under different conditions of acidity/basicity.
In this study, the q6h values were checked over KOH-900 for AR1 and JBG under pH 2–12. As shown in Figure 7, the q6h for AR1 decreased monotonously with increasing pH of the solution; however, the adsorption of JGB showed an opposite trend. This very opposite trend, observed in anionic AR1 and cationic JGB, could be explained via electrostatic interactions considering the opposite charges on the studied dyes. Moreover, the studied PDC or KOH-900 might have both positive and negative charges, depending on pH, since the surface charge of porous carbon generally decreases (from positive to negative) with increasing pH of the adsorption solution [61-63]. Therefore, the negative AR1 should have a favorable interaction at low pH; on the contrary, the adsorption of the positive JGB will be more effective at higher pH if the electrostatic interaction is considered.
However, there should be other dominant mechanisms since the q6h values are quite high under a wide range of pH conditions. At first, the very high hydrophobicity of KOH-900, as shown in Figure 2, can be considered. Compared with any other adsorbent, KOH-900 showed the highest performance in AR1 adsorption, as shown in Figure 3. Therefore, hydrophobic interaction can be suggested as a plausible mechanism for AR1 and JGB adsorption. This mechanism, which has been suggested earlier in adsorption of malachite green , aromatics , benzotriazole/benzimidazole , bisphenol A  and pharmaceutical and personal care products (PPCPs) , is acceptable considering the relatively small impact of pH on the q6h. Moreover, π–π interaction [51-54] might be another possible explanation considering that this interaction is hardly dependent on the pH (when aromatic rings are maintained under the studied pH); and both studied dyes (AR1 and JGB) and KOH-900 have ample aromatic rings with π electrons. Finally, the contribution of pore size should be mentioned. As illustrated in Figure 4 and Supporting Information File 1, Table S2, the KOH-900 sample is very effective in the adsorption of bulky dye molecules, as compared with the adsorption of small dyes such as MO and MB. This might be explained by the relatively large pore size of KOH-900, as shown in Figure 1b. Another explanation is that the pore size of KOH-900 is too large for effective adsorption of small MO or MB since van der Waals interactions rely on adequate matching between pore and adsorbates. On the contrary, bulky dye molecules such as AR1 and JGB can interact effectively with KOH-900 via van der Waals interactions, which relies on the suitable pore size of KOH-900 for the bulky dye molecules. In summary, the remarkable adsorption of AR1 and JGB over KOH-900 can be explained by the combined mechanisms of hydrophobic, π–π, electrostatic and van der Waals interactions.
Based on the remarkable performance of KOH-900 in the adsorption of AR1 and JGB, the performance of KOH-900 PDC was compared with earlier results, as shown in Table 1 [44,67-72] and Table 2 [73-77] for AR1 and JGB, respectively. As summarized in Table 1, KOH-900 had a Q0 value (for AR1) 8.1 times that of commercial, activated carbon. Moreover, KOH-900 had the highest Q0, compared with any reported adsorbent, so far. Additionally, KOH-900 showed a Q0 of more than 2 times that of a chitosan–alunite composite (previously the highest Q0)  even though the pH of adsorption solution was not the same. If the pH effect (vide supra, including Figure 7) is considered, the difference in Q0 between KOH-900 and chitosan–alunite composite will increase.
Table 2: Maximum adsorption capacity (Q0) of some reported adsorbents for the adsorption of JGB from water.
|Adsorbents||SABET (m2·g−1)||Solution pH||Q0 (mg·g−1)||Ref.|
|TiO2 (254 nm)||–||–||294|||
|commercial activated carbon||1016||7.0||64a||this work|
Based on Table 2, KOH-900 was also very competitive in JGB adsorption against the reported adsorbents. To begin with, KOH-900 had a q6h for JGB 11.5 times that of AC. The q6h of KOH-900 for JGB is more than 2 times that of the Q0 of the Ni0.5Zn0.5Fe2O4 adsorbent. The difference in Q0 should increase if the actual Q0 of KOH-900 is reached (in this work, q6h of KOH-900 was used in comparison) since Q0 is always higher than any qt value. Therefore, it could be confirmed that KOH-900 is remarkably effective in the removal of bulky dye molecules such as AR1 and JGB, irrespective of charge, mainly because of the large pores, high porosity and high hydrophobicity.
The Q0 or qt values of the reported adsorbents for MO and MB are compared in Supporting Information File 1, Tables S3 and S4, respectively. Even though KOH-900 is not very competitive in the adsorption of MO and MB (as compared with the adsorption of AR1 and JGB), the new adsorbent is also attractive in the removal of small dyes like MO and MB. Additionally, KOH-900 showed the second best performance in adsorption of MO or MB, partially because of its high porosity.
PANI-derived carbon materials were prepared from pyrolysis of PANI under a wide range of temperatures and applied in the adsorption of dyes from water. The hydrophobicity, pore size and mesopore volume were found to increase monotonously with increasing pyrolysis temperature. In addition, the best PDC (KOH-900) was very effective in the adsorption of dyes, especially those of a large size such as AR1 and JGB. For example, KOH-900 had a Q0 (for AR1) value 8.1 times that of commercial, activated carbon. Moreover, KOH-900 showed a Q0 value of more than 2 times that of a chitosan–alunite composite which previously showed the highest Q0 to date. The remarkable adsorption of AR1 and JGB over KOH-900 could be explained with combined mechanisms such as hydrophobic, π–π, electrostatic and van der Waals interactions. Finally, the PDC materials presented in this work could be suggested as a potential adsorbent to purify water contaminated with dye molecules, irrespective of size and charge.
AR1 (60%), JGB (65%), MO (85%), MB (82%) and aniline hydrochloride (C6H8ClN, 97%) were acquired from Sigma-Aldrich. Activated carbon (2–3 mm, granule, practical grade) was obtained from Duksan Pure Chemical Co., Ltd. Other chemicals used in this research were of analytical grade and were purchased from commercial venders and applied without any purification.
The PDC materials were obtained via pyrolysis of PANI, derived from aniline hydrochloride, in two steps, following earlier reports [42,43]. In brief, PANI was firstly pyrolyzed at 550 °C for 2 h under nitrogen flow. The pyrolyzed product was mixed well with KOH (the weight of KOH was 2 times that of the pyrolyzed product) and carbonized again at 600–900 °C for 1 h under nitrogen flow. The PDC samples were named KOH-x where x represents the pyrolysis temperature in the second step.
PDC and AC were characterized by nitrogen adsorption (Micromeritics, Tristar II 3020) to understand their porosity characteristics. Nitrogen adsorption was carried out at 77 K after evacuation of samples at 150 °C for 12 h. The Brunauer−Emmett−Teller (BET) equation and t-plot were applied to calculate the surface area and micropore volume, respectively, of the adsorbents. The pore size distributions were calculated with nonlocal density functional theory (NLDFT). The hydrophobicity of the studied adsorbents was evaluated by measuring the relative quantities of adsorbed water and n-octane at 30 °C with thermogravimetric analysis (TGA, Perkin-Elmer TGA 4000 system), similar to a previous work . In brief, an adsorbed quantity of water was measured for up to 60 min by feeding water vapor with the help of a nitrogen carrier. The adsorbed quantity of n-octane was determined similarly, and the relative quantity (n-octane/water, mol/mol) was calculated accordingly.
The adsorption of the dye molecules was carried out with model solution at pH 7.0, considering the usual pH of rainwater and river water . Detailed methods to calculate the adsorbed quantity at time t in h (qt) and maximum adsorption capacity (Q0)  are shown in Supporting Information File 1. In order to understand the adsorption mechanism, the solution pH for AR1 and JGB was controlled (up to 2–12) with aqueous solution of NaOH or HCl (0.1 M each).
|Supporting Information File 1: Additional experimental procedure “Adsorption of dyes from water” and additional experimental results.|
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