Influence of phosphorus and nitrogen co-doping of activated carbon from littered cigarette filters for adsorption of methylene blue dye from wastewater

Abstract

Global access to sanitary water is of utmost importance to human health. Presently, textile dye water pollution and cigarette pollution are both plaguing the environment. Herein, waste cigarette filters (CFs) are converted into useful carbon-based adsorbent materials via a facile, microwave-assisted carbonization procedure. The CFs are activated and co-doped with phosphorus and nitrogen simultaneously to enhance their surface characteristics and adsorbent capability by introducing chemisorptive binding sites to the surface. The doped carbonized CF (DCCF) and undoped carbonized CF (CCF) adsorbents are characterized physically to examine their surface area, elemental composition, and surface charge properties. The maximum adsorption capacity of synthesized adsorbents was determined via batch adsorption experiments and Langmuir modelling. Additionally, the influence of different parameters on the adsorption process was studied by varying the adsorption conditions such as adsorbent dosage, initial concentration, contact time, temperature, and pH. The DCCF adsorbent showed a maximum adsorption capacity of 303 mg g^− 1. Adsorption of both adsorbents fit best to Langmuir model and pseudo-second order kinetics, indicating chemisorptive mechanism. Both adsorbents showed endothermic adsorption process which is indicated by increasing adsorption capacity with increased temperatures. DCCF exhibited greater adsorption capability than CCF at all temperatures from 25 to 55 °C. The pH of the solution significantly affected the adsorption capacity of CCF while DCCF adsorption is favorable at a wide pH range due to low value of the adsorbent’s point of zero charge. Reusability results showed that both adsorbents can be used over several cycles for removal of dye. Thus, results conclude that the waste DCCF-based adsorbent does not only show a profound potential as a sustainable solution to combat textile dye water pollution but also addresses the valuable use of the CF pollution simultaneously. This approach, which can target two major pollutants, is attractive due to its ease of preparation, negligible cost, and versatility in application.

Introduction

Water pollution is an enormous problem worldwide, with the textile industry contributing to the overall pollution of water in a major way. Textile mills account for around 20% of all industrial water pollution; an approximate of 20,000 different chemicals and dyes contaminate water [1]. These synthetic dyes are incredibly stable, and thus are resistant to degradation under high temperatures, light exposure, and chemical treatment. Moreover, many of these dyes cannot be biodegraded under aerobic conditions and are highly soluble in water with visibility to the naked eye at minute concentrations (down to 1 ppm) [2]. As a result of their immense stability, current large-scale wastewater treatments are ineffective for dye removal, high in cost, or both, causing a significant portion of industrial dyes to be released into the environment.

Several prominent chemical and physical methods are used currently for textile dye removal from effluents, such as coagulation-flocculation, aerobic degradation, and adsorption [3]. Adsorption is a common choice to remove dye from solution as it is a relatively simple and inexpensive method [4, 5]. Recently, many researchers are examining the potential of waste resources for preparing activated carbons. A variety of precursors have been investigated such as tea [6], chitosan [7], and citrus peels [8]. There are also an increasing number of reports using heteroatoms such as nitrogen [9,10,11], phosphorus [12], or sulfur [13] doped activated carbon materials, to achieve enhanced adsorption. These heteroatoms produce various functional groups at the adsorbent’s surface that aid in binding dye molecules to the surface of adsorbent via alteration of surface polarity and acidity [14]. Many materials have shown promising results using dual or co-doping with two different elements [15, 16]. In this work, cigarette filter (CF) waste will be explored as a carbon precursor for synthesis of co-doped carbon material.

Cigarette waste contributes to the largest amount of plastic pollution around the world [17]. Most CFs, the part of the cigarette that remains after smoking, are tossed onto the ground, leading to immense ecological pollution. CFs are composed mainly of plastic, viz. cellulose acetate, which is not readily biodegradable [18]. Additionally, CFs contain toxic metals that can be leeched into soil and water, causing direct harm to plants and animals [19]. Due to the posed ecological threat of the litter, new methods of reducing cigarette pollution are needed. Since CFs are comprised mostly of cellulose acetate, a carbon-based polymer, these waste products can easily be utilized as carbon precursors for production of activated carbons [20,21,22].

This work aims to convert used CFs into useful carbon adsorbents via inexpensive and facile microwave-assisted approach. The phosphorus and nitrogen heteroatom-doped carbon contains functional groups which may have a synergistic effect on the adsorption capacity. Both undoped and doped carbons from CFs are characterized in detail. Methylene Blue (MB) dye is used to investigate the adsorption characteristics of the newly developed phosphorus and nitrogen co-doped carbon from cigarette filter (DCCF) and undoped carbonized cigarette filter (CCF). To the best of our knowledge, no work has reported the use of this one-step microwave-assisted method for producing DCCF and its use as an adsorbent.

Materials and methods

Chemicals

Waste CFs were collected from the University of Arkansas at Little Rock campus and rinsed with deionized (DI) water to remove any external residues like dust, and they were dried in air prior to their use. The paper casing was removed prior to carbonization. Ammonium polyphosphate (APP, avg. mw: 97) was a gift from JLS Chemicals. Sodium nitrate (NaNO₃) was purchased from ACROS. MB dye was purchased from Sigma Aldrich. Elga model PURELAB ultra water-filtration system was used to collect DI water (18.2 MΩ cm). Reagent grade hydrochloric acid (HCl), sodium hydroxide (NaOH), and ethanol were purchased from VWR and diluted to 0.01 M solutions to adjust pH.

Adsorbent synthesis

Waste CFs were collected from receptacles located around University of Arkansas at Little Rock campus and carbonized through a facile, low-cost, microwave-assisted method described previously [23]. For synthesis of DCCF, the CFs were weighed and combined with APP in a mass ratio of 1:0.4, and 2 drops of water was added to help initiate microwave carbonization process. An undoped carbonized sample of used CF (CCF) was prepared without APP. In this regard, CF along with 2 drops of water were placed into a boron nitride crucible, which was promptly situated in a foamed aluminum oxide box to contain the reaction. The box was subjected to microwave irradiation in a conventional microwave oven for 30 min at high power (2.45 GHz and 1.25 kW power) to carbonize the waste filters and then cooled to room temperature. Afterwards, the resulting products were powdered using a mortar and pestle and stored in a desiccator for later use.

Physical characterization

Physical characterization of CCF and DCCF were examined using various techniques. Scanning electron microscopy (SEM, JEOL JSM-7000F) was carried out to analyze the surface morphology of the bulk materials. For sample preparation to perform SEM imaging, double-sided carbon tape on aluminum mount substrate was used to hold carbon sample. Surface area and porosity analyzer (ASAP 2020 Micrometrics) with tandem Brunauer–Emmett–Teller (BET) method was used to determine surface area and pore characteristics of adsorbents using nitrogen gas (N₂) adsorption/desorption studies at 77 K. X-ray photoelectron spectrometer (XPS, Thermo K-Alpha) was used to analyze surface elemental composition of dried carbonized samples. Fourier transform infrared (FTIR, Thermo Scientific Nicolet 6700) spectroscopy was conducted to confirm that MB was adsorbed onto adsorbent surface and not degraded during adsorption. Point of zero charge (PZC) was determined using a simple salt addition method in order to find the pH where adsorbent carries no net surface charge. Briefly, a suspension of adsorbent (0.01 g) was prepared in 0.1 M NaNO₃ aqueous solution in different reaction vessels (5 g L^− 1 CCF or DCCF).

Adsorption studies

Adsorbent dosage

To optimize the adsorbent dosage for adsorption, various masses (5, 7.5, 10, 15, and 20 mg) were contacted with 50 mL of 20 ppm MB solution with 120 rpm stirring speed. After reaching equilibrium (24 h), the treated MB solutions were centrifuged at 3800 rpm for 10 min to remove the adsorbent from dye solution. Absorption spectrophotometry (Lambda 850 UV-Vis spectrophotometer with 1 cm path length quartz cuvette at 665 nm wavelength) was utilized to determine the concentration of MB remaining in solution at equilibrium. From this, the percent removal and adsorption capacity were determined.

Initial concentration

Batch adsorption experiments were conducted to analyze the effects of MB concentration adsorb onto CCF and DCCF from CFs. From stock, 50 mL MB solutions of different concentration (5 to 100 ppm) were prepared. 10 mg of adsorbent samples were placed into each MB solution. The solutions with adsorbent were stirred with a constant speed at room temperature until equilibrium was assumed (24 h). The equilibrium data were then fitted into Langmuir and Freundlich isotherm models to analyze the interactions between MB and CCF or DCCF.

Adsorption kinetics

To gain insight on how the mechanism of adsorption of MB onto CCF and DCCF is influenced by time, adsorption kinetic experiments were designed. Various initial concentrations of MB solution (5–100 ppm) were prepared in 50 mL water, and each solution was contacted with a constant 10 mg of adsorbent powder sample. These samples were stirred continuously. After specified time intervals, absorbance of an aliquot of the MB solution was analyzed by absorbance spectroscopy. This data was fitted using pseudo-first and second order modelling to ascertain the primary adsorption mechanism for the two adsorbent materials derived from CFs.

Effect of temperature

Solutions of MB were prepared at 30 ppm and adjusted to various temperatures: 25, 35, 45, and 55 °C. Then, 10 mg of adsorbent was added and stirred for 24 h. Afterwards, remaining concentration of MB dye was analyzed via absorbance spectrophotometry, and adsorption capacity was calculated.

Effect of pH

This experiment was designed by keeping the amount of adsorbent and the concentration of adsorbate (MB dye) constant while changing only the pH of the sample. Multiple solutions of 50 mL of 30 ppm MB of various pH were prepared by using dilute concentrations of NaOH and HCl. 10 mg of adsorbent was contacted in the aforementioned test solutions. The mixture was stirred at 120 rpm until equilibrium was assumed (24 h) at different initial pH.

Reusability of adsorbents

Reusability of adsorbents was determined by comparing Q_e values after 4 cycles of washing and reuse of materials. Test solutions of MB were prepared at 20 ppm (50 mL) to which 10 mg CCF or DCCF were added and stirred (120 rpm) at room temperature for 24 h at neutral pH. Afterwards, absorption was used to determine Q_e value. Adsorbents were recovered using centrifugation and washed with 10 mL ethanol a total of three times. Then, the adsorbent was dried in oven at 70 °C for 1 h. This was repeated over a total of 4 cycles.

Results and discussion

Physical characterization

SEM

SEM imaging was performed on adsorbent materials to analyze their surface morphologies. SEM image of CCF exhibits a rigid amorphous structure with smaller microstructures decorated on the surface (Fig. 1a). Imaging of DCCF sample displays cave-like structures and ridges at the macrostructure with spherical microscale structures distributed throughout (Fig. 1b). The doped sample also exhibited more sponge-like morphology indicating possession of a more well-formed pore structure than the undoped adsorbent. In order to confirm this, surface area analysis by BET was also performed.

Fig. 1

a CCF and b DCCF adsorbents SEM images at 2500 X magnification

BET surface area analysis

Both adsorbents were characterized by BET in order to gain insight into their surface area and porosity. From adsorption-desorption isotherms, both adsorbents exhibit a type IV isotherm characterized by Langmuir-like behavior at relative low pressure and hysteresis loop at higher pressure (Fig. 2) [24]. The hysteresis loop is formed by capillary condensation in the mesoporous structures of the material. The BET surface area of CCF and DCCF adsorbents are 176 and 177 m² g^− 1, respectively. The microwave activation process causes the formation of reducing gases leading to high surface area carbon materials. This result indicates that doping with APP does not play a significant role in altering the overall surface area of the activated material. However, DCCF is significantly more mesoporous (88% mesopores by volume). This could be due to larger reducing gas formation when combined with APP. The overall results of BET analysis are tabulated in Table 1.

Fig. 2

Adsorption and desorption curves of a CCF and b DCCF

Table 1 Surface area characteristics from BET

XPS

In order to determine surface elemental composition of adsorbent materials, XPS was performed. Various functional groups of atoms at the surface can greatly enhance adsorption mechanism by allowing chemisorption processes to occur. Survey scan spectra of both samples reveal the presence of carbon, oxygen, and phosphorus at the surface (Fig. 3). Results of CCF reveals the additional presence of silicon at a low percentage (1.13%, Table 2). This is expected, as silicates can be formed in cigarette smoke and deposited in the filter during smoking [25]. DCCF contains much greater amount of phosphorus (3.98%) and nitrogen at the surface, confirming that the doping of the material was successful. Nitrogen and phosphorus at the surface of adsorbent can aid in binding MB by altering the surface chemistry such as polarity and acid/base properties as well as introducing functional groups that can interact with MB in solution [9, 14].

Fig. 3

Survey scan plots of a CCF and b DCCF adsorbents

Table 2 Surface elemental composition (At%) of adsorbents

PZC

The PZC of the adsorbents is analyzed in order to gain a deeper understanding of the possible adsorption mechanism onto the materials. The PZC can be defined as the pH where the net charge of an adsorbent is zero. MB is a cationic dye, and thus adsorption is favored when the solution pH is greater than the PZC of an adsorbent (adsorbent carries net negative charge). In order to determine PZC, a salt addition method was used as described previously [15]. A plot of ΔpH versus pH_initial was formed where ΔpH = 0 was deemed to be the PZC (Fig. 4). The PZC of CCF and DCCF were found to be 7.25 and 3.23, respectively. This implies that MB adsorption will be more favorable onto the doped adsorbent (DCCF) at a wider range of pH.

Fig. 4

Point of Zero Charge (PZC) plots for CCF and DCCF

FTIR

In order to confirm that MB was adsorbed onto DCCF and not degraded during adsorption process, FTIR was used to identify characteristic carbon-sulfur bonds post-adsorption onto DCCF. Compared to the raw adsorbent material, there are two additional peaks at 1191 and 1321 cm^− 1 which are correlated to the C=S double bond and the C—S bond, respectively (Fig. 5). The introduction of these carbon sulfur bonds post-adsorption confirms that MB is adsorbed to the surface and its structure is not altered during adsorption process. A similar band at 1396 cm^− 1 was observed for CCF post MB adsorption (Fig. S1 of Supplemental Materials), indicating a similar nondegradative adsorption process for the undoped sample as well.

Fig. 5

FTIR of DCCF adsorbent before and after adsorption of MB

Adsorption characterization

Adsorbent dosage

Various masses of CCF or DCCF were contacted with 50 mL solutions of MB dye, separately, and allowed to reach equilibrium. Afterwards, the percent removal of dye was calculated using Eq. (1).

$$ Percent\ Removal=\left(\frac{C_0-{C}_e}{C_0}\right)\ast 100 $$

(1)

where C is the concentration of MB in solution initially and at equilibrium. The amount of dye adsorbed at equilibrium, Q_e (mg g^− 1) was determined with Eq. (2):

$$ {Q}_e=\frac{\left({C}_o-{C}_e\right)V}{W} $$

(2)

where V is the volume of solution and W is the weight of adsorbent. For both samples, percent removal of dye increases with an increase in adsorbent dosage (Fig. 6). However, Q_e increases to a maximum value and then decreases after a certain mass dosage. For CCF, the maximum Q_e value is obtained at a mass dosage of 10 mg. For DCCF, this occurs at a slightly lower mass of 7.5 mg. To keep conditions the same for both adsorbents, a mass loading of 10 mg is used for further adsorption experiments.

Fig. 6

Effects of adsorbent dosage on adsorption capacities and % MB removal for a CCF and b DCCF

Effect of initial concentration

The effect of initial concentration of MB adsorption onto the adsorbents was investigated by contacting a fixed mass of 10 mg adsorbent to varying concentration of MB from 5 to 100 ppm. For both adsorbents, it was observed that the adsorption capacity increased as the initial concentration of MB increased (Fig. 7). This is due to the mass transfer driving force between liquid-solid interface involved in heterogeneous adsorption. More dye molecules in the liquid phase shifts equilibrium toward adsorption onto the solid phase. Also, when the initial concentration is very low (5 ppm), both adsorbents exhibit a similar Q_e value. However, for CCF, the maximum experimental Q_e value achieved is 195 mg g^− 1 while DCCF reaches a value of 294 mg g^− 1. This indicates the enhanced adsorptive capabilities of DCCF compared to CCF.

Fig. 7

Effects of initial MB concentration on the equilibrium adsorption capacity of CCF and DCCF

Adsorption isotherms

Adsorption isothermal modelling of the data allows a detailed investigation of possible adsorption mechanisms. The models help to describe the interactions between adsorbent and dissolved dye species at the liquid-solid phase boundary and allow an estimation of the maximum adsorption capacity. The two most common models, Langmuir and Freundlich, were applied to the adsorption data of CCF and DCCF samples.

Modelling with the Langmuir equation is performed with several assumptions, one being that only a single layer of adsorbate can be adsorbed onto the active sites of an adsorbent, and there is a limited amount of those sites. Langmuir model also makes the assumptions that those active sites are energetically equivalent regardless of their occupation, meaning the Langmuir equation does not consider repulsive forces of molecules bound to adsorbent surface. The linear form of the Langmuir equation [26], Eq. (3), was used to determine the Langmuir constants related to the maximum adsorption amount (Q_max) and the adsorption energy (K_L).

$$ \frac{C_e}{Q_e}=\frac{1}{Q_{max}{K}_L}+\frac{1}{Q_{max}}{C}_e $$

(3)

From the slope of Eq. (3), Q_max can be obtained and was determined to be 213 and 303 mg g^− 1 for CCF and DCCF, respectively (Table 3). This indicates that DCCF possesses a higher capacity to adsorb MB from solution. The K_L value of DCCF is also much higher than CCF (0.38 vs 0.08) indicating a stronger interaction between doped sample surface and the adsorbate. Both models showed reasonable fitting with R² values of 0.911 and 0.986 for CCF and DCCF, respectively.

Table 3 Langmuir and Freundlich constant value results from linear fitting and free energy values for CCF and DCCF

Modelling with the Freundlich equation is done with the assumptions of heterogeneous adsorbent surfaces and that the adsorption sites have varying energy. The Freundlich equation, Eq. (4), was also used in the linear form:

$$ \mathit{\log}{Q}_e=\mathit{\log}{K}_F+\frac{1}{n}\mathit{\log}{C}_e $$

(4)

where K_F is a constant related to adsorption capacity and n is a constant related to adsorption intensity. Neither adsorbent was well represented by the model with R² values less than 0.88 in both cases. However, both adsorbents possess an n value greater than 1 which is indicative of a favorable process of adsorption. The n value of DCCF is greater than that of CCF (Table 3) which can be correlated to stronger interactions between adsorbate and the adsorbent material due to greater amount of nitrogen and phosphorus at the surface. K_F values are related to adsorption capacity and, like Langmuir modelling of the data, DCCF exhibits a higher K_F value. Langmuir and Freundlich fitting plots are displayed in Fig. S2.

To determine the spontaneity of the adsorption process of CCF and DCCF, Gibbs free energy was calculated from Eq. (5).

$$ \Delta {G}^o=- RTln{k}_0 $$

(5)

where R is the gas constant, (8.314 J mol^− 1 K^− 1) T is the temperature (298 K), and k₀ is equal to Q_e/C_e [27]. Both CCF and DCCF exhibited spontaneous adsorption, due to negative calculated values of ΔG^o. The value of ΔG^o for DCCF is more negative than for CCF (Table 3) which indicates that the doped CF material shows more highly spontaneous adsorption at 298 K.

Kinetics

To investigate the kinetic mechanism of adsorbents, kinetic adsorption was fitted into pseudo-first and pseudo-second order kinetic models. Experiments were performed by varying initial concentration from 5 to 100 ppm of MB at natural pH and recording the dye concentration at various time intervals after contact with adsorbent (Fig. 8a and b). The pseudo-first order model was used in the linear form, Eq. (6), in order to evaluate the first order rate constant, k₁.

$$ \log \left({Q}_e-{Q}_t\right)=\mathit{\log}{Q}_e-\frac{k_1}{2.303}t $$

(6)

where Q_t is the amount of dye adsorbed at time, t. R² values were used to determine the better fitting model. The pseudo-second order equation was also used in the linear form, Eq. (7), to determine second order rate constant, k₂.

$$ \frac{t}{Q_t}=\frac{1}{k_2{Q}_e^2}+\frac{1}{Q_e}\ \mathrm{t} $$

(7)

Fig. 8

Kinetics plot of a CCF and b DCCF and pseudo c first and d second order fitting of data of doped sample

Plotting the linear form of Eq. 6 and 7 generates a straight line in which k can be directly calculated (Fig. 8c, Fig. 8d, and Fig. S3). CCF average R² value is 0.88 (Table S1) while the average value of R² for second order fitting is 0.99. This indicates a better fitting of CCF adsorption to pseudo-second order kinetics. DCCF average R² value for pseudo-first order plot is 0.90 while for pseudo-second, the value average is 0.99. This indicates that the adsorption mechanism is better correlated to a pseudo-second order process for both samples. This process is characterized by strong chemisorptive adsorption between MB and CCF and DCCF adsorbents. This mechanism involves the chemical binding between functional groups on the surface of adsorbent and MB dye. The enhancement of nitrogen, phosphorus, and oxygen elemental composition at the surface of DCCF is attributed to enhancing chemisorptive active sites. Moreover, improved diffusion of MB into the mesoporous structure of the adsorbents can aid to enhance their adsorption performance.

In addition to kinetic modelling, the standard deviation was calculated from Eq. (8):

$$ \Delta Q\left(\%\right)=100\times \sqrt{\frac{\sum {\left[\frac{Q_{t,\mathit{\exp}}-{Q}_{t, cal}}{Q_{t,\mathit{\exp}}}\right]}^2}{n-1}} $$

(8)

For CCF adsorption, ∆Q was found to be between 1 and 9 for second order compared to 7–20 for first order (Table S1). Similarly, DCCF displayed ∆Q values between 5 and 17 for pseudo-first order and 5–8 for pseudo-second order. This data further supports a chemisorptive mechanism of adsorption for the two adsorbents.

The adsorption capacity of CCF and DCCF were compared to those of other waste-derived carbon materials for their removal of MB from solution. The waste precursors and corresponding maximum adsorption capacities are reported in Table 4. From this data, it can be concluded that CCF and DCCF show exceptional application as adsorbents for the removal of cationic MB dye as their adsorption capacities are higher than many other waste-derived carbons. Additionally, many of the previously used waste precursors require chemical activation, whereas this work highlights a simplistic method to produce doped carbons with desirable adsorption characteristics.

Table 4 Comparison of maximum adsorption capacity of MB of CCF and DCCF to other adsorbent materials (at 298 K)

Effect of temperature

In order to evaluate the temperature effect on adsorption onto the cigarette-based samples, experiments were performed at four different temperatures ranging from 25 to 55 °C. It is observed that for both adsorbent materials, the adsorption capacity, Q_e is increasing as the temperature increases (Fig. 9). This is due to an increased diffusion rate of MB molecules into the internal cavities of porous carbons [26]. This occurs mainly due to the lowering of viscosity of the solvent as temperature increases. This is also indicative of an endothermic adsorption process for both adsorbents [35].

Fig. 9

Effect of temperature on equilibrium adsorbent capacity from initial concentration of 30 ppm and 10 mg adsorbent dosage

Effect of pH

The effect of solution pH on MB’s adsorption was analyzed by contacting 10 mg of adsorbent to 50 mL of 30 ppm MB solution (Fig. 10). CCF adsorption is greatly dependent on pH, ranging from 78 to 100 mg g^− 1 in a pH range from 3.9 to 10.2. This is due to the neutral PZC of CCF. Below pH 7, the adsorption is unfavored because of the repulsive forces between MB and the positive adsorbent surface. In contrast, DCCF adsorption capacity remains relatively unchanged over the pH range 3.4 to 10.9. This is because of a low value of PZC value of DCCF, causing it to have a net negative surface charge at pH past 3.2.

Fig. 10

Effect of initial solution pH on adsorption capacity of CCF and DCCF using an initial 50 mL of 30 ppm MB solution

Reusability of adsorbents

Reusability of adsorbents was determined in order to assess the long-term utility of CCF and DCCF. This was carried out using adsorption-desorption experiment where MB was adsorbed onto the adsorbent and desorbed with ethanol thrice prior to reuse. This experiment was performed for a total of 4 cycles where Q_e was calculated for each cycle. It was found that both adsorbents retain their adsorption characteristics up to the second cycle after which the Q_e begins to decrease at a faster rate (Fig. S4). This decrease in Q_e value is attributed to the reduction of active sites at the adsorbent surface during desorption of MB [36]. Thus, both CCF and DCCF have potential to be used over several times before being discarded.

Conclusions

Useful adsorbent materials were successfully prepared from waste CCF using a simple and rapid one-step microwave synthesis. DCCF exhibited an exceptional maximum adsorption value of 303 mg g^− 1, making it a highly efficient and cost efficient adsorbent for MB removal. The materials were characterized in detail to reveal crucial information about their surface area, elemental composition, and morphology. The adsorbents were shown to have exceptional surface area (~ 177 m² g^− 1) and well-developed porosity. Doping of the sample was confirmed using XPS which showed significant contribution of phosphorus and nitrogen on the surface of the material which played a significant role in enhancing the adsorption capacity of the material. Adsorption of MB onto adsorbents was found to be best correlated to a monolayer adsorption process as confirmed by higher R² value with Langmuir fitting. Further, the adsorbents undergo a pseudo-second order adsorption process which is indicative of a chemisorptive process. Adsorption onto the adsorbents is spontaneous (ΔG < 0) and endothermic in nature and can be recycled several times efficicently before being discarded. This work highlights an inexpensive and green method to convert a common litter source into a useful material for water remediation.