# Removal of Heavy Metals from Drinking Water by Magnetic Carbon Nanostructures Prepared from Biomass

Authors: Muhammad Muneeb Ur Rahman Khattak; Muhammad Zahoor; Bakhtiar Muhammad; Farhat Ali Khan; Riaz Ullah; Naser M. AbdEI-Salam
Journal: Journal of Nanomaterials
 (2017)

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## Abstract

Heavy metals contamination of drinking water has significant adverse effects on human health due to their toxic nature. In this study a new adsorbent, magnetic graphitic nanostructures were prepared from watermelon waste. The adsorbent was characterized by different instrumental techniques (surface area analyzer, FTIR, XRD, EDX, SEM, and TG/DTA) and was used for the removal of heavy metals (As, Cr, Cu, Pb, and Zn) from water. The adsorption parameters were determined for heavy metals adsorption using Freundlich and Langmuir isotherms. The adsorption kinetics and effect of time, pH, and temperature on heavy metal ions were also determined. The best fits were obtained for Freundlich isotherm. The percent adsorption showed a decline at high pH. Best fit was obtained with second-order kinetics model for the kinetics experiments. The values ofΔH° and ΔG° were negative while that of ΔS° was positive. The prepared adsorbent has high adsorption capacities and can be efficiently used for the removal of heavy metals from water.


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## Body

## 1. Introduction

Presently, the heavy metals contamination in drinking water is being investigated by many scientists in both the natural and anthropogenic sources [1–3]. Heavy metals contaminate both surface and ground water affecting the quality of water as these metals are persistent, toxic, and dangerous to human [4–6]. Around the world the research on finding the more efficient technologies for the water treatment to achieve the safe standards is regularly alarming subject of matter for the environmental scientists.In past efforts have led to establishing various unit process or operations like adsorption, filtration, precipitation, ion exchange, and chemical coagulation [7–11]. Out of these, the adsorption process is the most economical, technical, and widely used technique [12]. The research on adsorption process for water treatment has resulted in establishing of alternate adsorption materials and methods for the removal of heavy metals from water which includes clay, aluminosilicate, peat, zeolites, kaolin polysaccharides activated carbon, and adsorbents prepared from biomass [12–22].In this study a novel adsorbent, magnetic carbon nanocomposites were prepared from biomass. The characterization of the prepared adsorbent was carried out by XRD, FTIR, surface area analyzer, Scanning Electron Microscope, EDX, and TG/DTA. This adsorbent was then used for the removal of heavy metals from water as alternative of the conventional adsorbent.


## 2. Material and Methods

### 2.1. Preparation of Magnetic Carbon Nanocomposites

For the preparation of magnetic carbon nanocomposites the waste of watermelon was collected from local market. The peel of watermelon was dried and cut into pieces and transferred to alcoholic solution of FeCl3·6H2O (10% w/v) for 24 hrs. The solution and biomass were then separated and dried in open air at room temperature. This dried biomass was then charred and ignited in a specially designed assembly consisting of an electric heater and wire gauze with an inlet for nitrogen and an exhaust outlet for gases (Figure 1).Figure 1
The chamber used for preparation of magnetic carbon nanocomposites.


### 2.2. Characterization of Iron Oxide Magnetic Carbon Nanocomposites

The most significant physical parameter including the utility and quality of materials is surface area and porosity. Variation in these two parameters greatly influences the activity of the materials. A sample weighing 0.1 g was taken and characterized by using surface area analyzer of model NOVA 2200e, Quantachrome, made in USA. The purging gas used was nitrogen.The X-rays diffraction analysis of magnetic nanoadsorbent was carried out by using X-Ray Diffractometer (Joel, JDX-3532) having Ni Filter while monochromatic Cu Kα was used as a source of radiation which operates at a wavelength of 1.5518 Å. The X-ray generator was run at 45 Kilovolt and 30 mA. The speed and range for scanning were 2θ/θ and 10 min−1, respectively.The IR spectra were obtained by analyzing the prepared adsorbent on FTIR (IR Prestige-21, Shimadzu, Japan) whereas the scanning ranges were set for mid-700–500 cm−1 and for Far region 4000–600 cm−1.Topography of the sample was measured by placing the sample on the grid of SEM, whereas sputter coater was used for gold coating of the sample (made in USA). The image for surface morphology was then recorded by SEM with voltage of 20 KV (Joel JSM-5910).The prepared adsorbents were analyzed by TG/DTA of diamond series made in USA having a reference of Aluminum trioxide as a standard.The EDX analysis was performed using EDX model INCA 200.


### 2.3. Determination of Adsorption Parameters

A series of 25 mL flasks were taken and concentrations of 150, 175, 200, 225, 250, 275, 300, 325, and 350 ppm of standard heavy metals were prepared. A concentration of 0.5% (W/V) of the prepared adsorbent was then added in each flask. These flasks were shaken on orbital shaker at 300 rpm for 480 mins time at room temperature. Every flask was then subjected to magnetic bar for the separation of sorbents. Finally the solution was filtered through Whatman number 1 and then subjected to atomic absorption analysis.


### 2.4. Determination of Kinetics Parameters

25 mL flask series was taken and was spiked with known amount of heavy metal to achieve a concentration of 200 ppm. A concentration of 0.5% (W/V) of the prepared adsorbent was then added in each flask and arbitrarily rotated with a speed of 300 revolutions per minute at a temperature of 25°C. Every flask was then subjected to a magnetic bar for the separation of sorbents. Finally the solution was filtered through Whatman number 1 before atomic absorption analysis.


### 2.5. Determination of Effect of pH on Adsorption of Heavy Metals

A series of flasks with pH ranging from 1 to14 were prepared to optimize pH for heavy metals adsorption. Each flask was spiked with standards of heavy metals to achieve 200 ppm before adding the sorbent. Thereafter the sorbents were removed by using magnetic bar after shaking at 300 revolutions per minute for 250 minutes prior to atomic absorption analysis.


### 2.6. Determination of Thermodynamics Parameters

Another series of flasks was prepared and subjected to similar experimental conditions as mentioned above except for temperatures that were different for each set for a period of 240 minutes. Thereafter, separation and atomic adsorption analysis were carried out.


## 2.1. Preparation of Magnetic Carbon Nanocomposites

For the preparation of magnetic carbon nanocomposites the waste of watermelon was collected from local market. The peel of watermelon was dried and cut into pieces and transferred to alcoholic solution of FeCl3·6H2O (10% w/v) for 24 hrs. The solution and biomass were then separated and dried in open air at room temperature. This dried biomass was then charred and ignited in a specially designed assembly consisting of an electric heater and wire gauze with an inlet for nitrogen and an exhaust outlet for gases (Figure 1).Figure 1
The chamber used for preparation of magnetic carbon nanocomposites.


## 2.2. Characterization of Iron Oxide Magnetic Carbon Nanocomposites

The most significant physical parameter including the utility and quality of materials is surface area and porosity. Variation in these two parameters greatly influences the activity of the materials. A sample weighing 0.1 g was taken and characterized by using surface area analyzer of model NOVA 2200e, Quantachrome, made in USA. The purging gas used was nitrogen.The X-rays diffraction analysis of magnetic nanoadsorbent was carried out by using X-Ray Diffractometer (Joel, JDX-3532) having Ni Filter while monochromatic Cu Kα was used as a source of radiation which operates at a wavelength of 1.5518 Å. The X-ray generator was run at 45 Kilovolt and 30 mA. The speed and range for scanning were 2θ/θ and 10 min−1, respectively.The IR spectra were obtained by analyzing the prepared adsorbent on FTIR (IR Prestige-21, Shimadzu, Japan) whereas the scanning ranges were set for mid-700–500 cm−1 and for Far region 4000–600 cm−1.Topography of the sample was measured by placing the sample on the grid of SEM, whereas sputter coater was used for gold coating of the sample (made in USA). The image for surface morphology was then recorded by SEM with voltage of 20 KV (Joel JSM-5910).The prepared adsorbents were analyzed by TG/DTA of diamond series made in USA having a reference of Aluminum trioxide as a standard.The EDX analysis was performed using EDX model INCA 200.


## 2.3. Determination of Adsorption Parameters

A series of 25 mL flasks were taken and concentrations of 150, 175, 200, 225, 250, 275, 300, 325, and 350 ppm of standard heavy metals were prepared. A concentration of 0.5% (W/V) of the prepared adsorbent was then added in each flask. These flasks were shaken on orbital shaker at 300 rpm for 480 mins time at room temperature. Every flask was then subjected to magnetic bar for the separation of sorbents. Finally the solution was filtered through Whatman number 1 and then subjected to atomic absorption analysis.


## 2.4. Determination of Kinetics Parameters

25 mL flask series was taken and was spiked with known amount of heavy metal to achieve a concentration of 200 ppm. A concentration of 0.5% (W/V) of the prepared adsorbent was then added in each flask and arbitrarily rotated with a speed of 300 revolutions per minute at a temperature of 25°C. Every flask was then subjected to a magnetic bar for the separation of sorbents. Finally the solution was filtered through Whatman number 1 before atomic absorption analysis.


## 2.5. Determination of Effect of pH on Adsorption of Heavy Metals

A series of flasks with pH ranging from 1 to14 were prepared to optimize pH for heavy metals adsorption. Each flask was spiked with standards of heavy metals to achieve 200 ppm before adding the sorbent. Thereafter the sorbents were removed by using magnetic bar after shaking at 300 revolutions per minute for 250 minutes prior to atomic absorption analysis.


## 2.6. Determination of Thermodynamics Parameters

Another series of flasks was prepared and subjected to similar experimental conditions as mentioned above except for temperatures that were different for each set for a period of 240 minutes. Thereafter, separation and atomic adsorption analysis were carried out.


## 3. Results and Discussion

### 3.1. Characterization of Fe2O3 Magnetic Carbon Nanocomposites Made from Watermelon Waste

A special designed chamber as shown in Figure1 was used to prepare magnetic adsorbent from watermelon waste (peel). The magnetic properties of the prepared adsorbent were noted by subjecting it to the magnetic bar. The attraction of the adsorbent by magnetic bar showed the presence of magnetic oxides in the prepared carbon nanostructures.Figures2 and 3 indicated the surface area and pore distribution of magnetic adsorbent, respectively, whereas Table 1 showed different surface parameters of the prepared adsorbent.Table 1
Parameters (physical) of the adsorbent synthesized from watermelon waste.
BET, surface area (m2/g) 71.35 Langmuir, surface area (m2/g) 261.50 Pore volume total (cm3/g) 0.63 Micropores volume (cm3/g) 0.27 Pore diameter, average (Å) 115.20Figure 2
Graph showing BET surface area of the prepared iron oxide carbon nanocomposite from watermelon waste.Figure 3
Graph showing distribution of pores in the prepared iron oxide magnetic carbon nanocomposites from watermelon waste.The XRD spectra of the prepared adsorbent from watermelon waste are highlighted in Figure4, suggesting that Fe3O4 has been deposited in carbon. XRD not only help in the structure determination but also help in particles size measurement [23]. Peaks of diffraction at 2θ of 28.35, 30.2, 35.6, 40.55, 50.2, and 58.25 indicate corresponding indices (220, 311, 400, 422, 511, and 440 planes of cubic unite cell) as previously reported for magnetite structure [24, 25]. The diffraction peaks at 2θ of 10.45, 13.5, and 20.85 as already reported in literature are related to maghemite and hematite [24]. The size of the prepared adsorbent was calculated by using the equation of Debye-Scherrer. (1)D=KλβCos⁡θ,where the mean size is represented by D, K is constant (0.94), λ is the wavelength (1.55060 Å) of X-ray, and β shows excess line broadening, while Bragg angle is represented by θ.(2)β=B-b,where B is the line width (in radian) and b shows instruments line broadening (in radian) [25]. By using formula (1), the sizes of the nanocomposite were calculated and found in the range of 90–250 nm.Figure 4
XRD spectra of magnetic carbon nanocomposites prepared from watermelon waste.For the characterization of the nanocomposite the most widely used technique is the IR Spectroscopy. The IR shows the structure morphology, nature of surface hydroxyl groups, and adsorbed H2O. At 580 cm−1 and 400 cm−1 broad bands correspond to magnetite structure. The Infrared spectra of iron oxide magnetic carbon nanocomposites prepared from watermelon waste (Far and Mid region) are shown in Figures 5 and 6. The peaks in range 1000–1200 cm−1 represent C-C and C-O stretching while 573.60 cm−1 of iron oxide represents the deposited magnetite in the prepared adsorbent.Figure 5
Far IR spectra of magnetic carbon nanocomposites prepared from watermelon waste.Figure 6
Mid IR spectra of magnetic carbon nanocomposites prepared from watermelon waste.Figure7 shows the surface morphology of the prepared adsorbent (high and low magnification). The SEM analysis shows the differences in size and shape of the prepared composite. The white patches of the images show crystalline structure of the prepared composite whereas grayish/black spots show the presence of carbon. The aggregation of iron oxide in the photograph is attributed to the contents of moisture absorbed by the prepared adsorbent. The aggregation of particles decreases the surface area of adsorbent and thus decreases its adsorption capacity. It was also observed from the images that the shape of the Fe3O4 appears somewhat cubical, while the size of nanocomposite was from 50 to 300 nm.Figure 7
SEM images of magnetic carbon nanocomposites prepared from watermelon waste at different magnification.
(a) (b) (c)Figure8 showed the TGA curve for the prepared adsorbent. The spectra show dehydration in two stages. About 9.6% loss of mass was observed at 400°C to 850°C; however no significant losses were observed above this temperature (up to 970°C). The observed mass loss was due to the dehydration of moisture content from the prepared nanocomposite. In case of DTA analysis two endothermic peaks were seen in the range of 60°C–350°C.Figure 8
TG/DTA curves of magnetic carbon nanocomposites prepared from watermelon waste.Figure9 shows the Electron Dispersive X-ray (EDX) analysis of prepared iron oxide composites of watermelon waste that showed the existence of carbon (C), iron (Fe), and oxygen (O). Also a small peak was observed which represents calcium (Ca) as an impurity. In the prepared iron oxide composites the peaks of Fe-Kα, Fe-Lα, O-Kα, and Fe-Kβ showed the deposition of iron oxide as also reported by Giles et al. [25].Figure 9
EDX spectra of magnetic carbon nanocomposites prepared from watermelon waste.


### 3.2. Adsorption Isotherm

#### 3.2.1. Giles Isotherms

The adsorption of heavy metal on the adsorbents prepared from watermelon waste was studied using Giles isotherm [26]. The Giles adsorption isotherm of the selected heavy metals on iron oxide nanocomposites prepared from watermelon waste is shown in Figure 10. The isotherms for these metals are C type.Figure 10
Giles adsorption isotherms of heavy metals on adsorbent prepared from watermelon waste.


#### 3.2.2. Langmuir Isotherm

Langmuir adsorption isotherm assumes that the maximum adsorption corresponds to a saturated monolayer of solute molecules on the adsorbent surface, having no interaction with molecules adsorbed from lateral sides [27]. The linear form of Langmuir isotherm is given as(3)Cq=CQ0+1Q0b.The above equation shows that q represents quantity of adsorbate adsorbed in mg·g−1, C represents the equilibrium concentration of adsorbate in mg·L−1 while “Q0” and “b” are Langmuir constants, and “Q0” is the maximum adsorption capacity of the adsorbent and also “b” is the energy of the process.Langmuir plot of specific adsorption (C/q) against equilibrium concentration (C) for adsorbent prepared from watermelon waste for selected heavy metals is shown in Figure 11. The slope and intercept were used to calculate the values of Langmuir constants Q0 and b (Table 2).Table 2
Langmuir adsorption constants for heavy metals on nanostructures from watermelon waste.
Heavy metals Langmuir constants R 2 Freundlich constants R 2 Q 0 b 1 / n K Arsenic 32894 0.025 0.929237 0.9040 859.25 0.9810 Chromium 21012 0.021 0.9274 1.0944 277.86 0.9617 Copper 38258 0.0078 0.8194 1.004 261.25 0.9834 Lead 29837 0.0312 0.8267 0.9156 905.87 0.9910 Zinc 18654 0.0307 0.8192 1.1910 292.96 0.9709Figure 11
Langmuir plot for the adsorption of heavy metals on adsorbent prepared from watermelon waste.


#### 3.2.3. Freundlich Isotherm

This isotherm is mostly used to explain the heterogeneous systems [28] and is given by the equation.(4)ln⁡q=ln⁡K+1nln⁡C.In the above equation C shows the equilibrium concentration in mg L−1, q is the amount of adsorbate adsorbed in mg per gm, and K and n are constants of Freundlich. K shows adsorption capacity while n is the adsorption intensity. The Freundlich constants K and 1/n can be obtained from slope and the intercept of ln⁡C against ln⁡q plot.For the selected heavy metals adsorption on adsorbent prepared from watermelon waste the Freundlich isotherm is given in Figure12. The values of K and 1/n are given in Table 2.Figure 12
Freundlich plot for the adsorption of heavy metals on adsorbent prepared from watermelon waste.From Table2 it is clear that Freundlich adsorption isotherm model fitted the data better than Langmuir isotherm. Also R2 values are higher for this model.


### 3.3. Adsorption Kinetics

#### 3.3.1. Effect of Contact Time

In adsorption processes contact time required for reaching equilibrium for an adsorbent is an important factor. For the metals under study the contact time required to reach equilibrium is shown in Figure13. In first few minutes the uptake of contaminants was very fast as initially more sites of adsorbent are available for adsorption of metals. As the time passes maximum number of sites is occupied by the metals and adsorption process slows down. At the end the equilibrium time of adsorption occurs due to saturation of the adsorbents. The equilibrium time for arsenic, chromium, copper, lead, and zinc was 260, 220, 280, 200, and 200 minutes, respectively.Figure 13
Effect of contact time on adsorption of heavy metals on nanocomposites prepared from watermelon waste.


#### 3.3.2. Adsorption Kinetic Models

The knowledge regarding adsorption kinetics plays a significant role in the removal of water pollutants. Therefore to evaluate the kinetic parameters, the Lagergren first-order and pseudo-second-order models were used [29].The pseudo-first-order equation can be expressed by the following relation:(5)ln⁡qe-q=ln⁡qe-Kat,where qe and q (mg g−1) are the amount of adsorbed adsorbate at equilibrium and time t, respectively, and Ka (min−1) is the rate constant. Ka can be calculated from slope of the plot of ln⁡(qe-q) versus t. This equation shows a linear relationship between ln⁡(qe-q) and t.K a and R2 values (Table 3) were calculated by plotting ln⁡(qe-q) against t for metals under study adsorption on adsorbent prepared from watermelon waste as shown in Figure 14. Ka and R2 values (Table 3) were calculated from ln⁡(qe-q) versus t plot.Table 3
Pseudo first- and second-order adsorption kinetics parameters for the adsorption of heavy metals on magnetic carbon nanostructures.
Heavy metals Pseudo-first-order kinetics model Pseudo-second-order kinetics model K a R 2 K 2 R 2 Arsenic 0.0158999 0.974546 2.32 ∗ 10 - 6 0.992 Chromium 0.0140065 0.994028 2.25 ∗ 10 - 6 0.987 Copper 0.0124186 0.907812 6.14 ∗ 10 - 7 0.968 Lead 0.0178124 0.962160 1.72 ∗ 10 - 6 0.946 Zinc 0.0162281 0.967867 2.05 ∗ 10 - 6 0.989Figure 14
Pseudo first-order kinetics plot for the adsorption of heavy metals on nanocomposite prepared from watermelon waste.The pseudo-second-order equation can be expressed by the relation(6)tqt=1K2q2+1qt,where K2 (g mg−1 min−1) is the rate constant of adsorption and q (mg g−1) is the amount of adsorbate adsorbed at equilibrium and qt is the amount of adsorbate adsorbed at time t. The values of K2 and q are calculated from intercept and slope of the straight line, respectively.K a and R2 values (Table 3) were calculated from plotting t/qt versus t plot (Figure 15).Figure 15
Pseudo second-order kinetics plot for the adsorption of heavy metals on nanocomposite prepared from watermelon waste.Table3 shows that the adsorption kinetics could be best explained in terms of the pseudo-second-order rate equation with precision in the correlation coefficients, while the Lagergren rate equation did not reflect the experimental results.


#### 3.3.3. Adsorption Mechanism

In the adsorption process the main steps involved in the removal of adsorbate by adsorbent are the following:(i)
One step is transport of ingoing particles to the external surface of the adsorbent(ii)
Another step is transport of the adsorbate through the pores of adsorbent except for a small amount of the adsorption which occurs on the external surface (interparticle diffusion) and adsorption of the ingoing particles (adsorbate) on to interior surface of the adsorbent(iii)
Amongst these, the rate controlling step, which affects the overall removal rate, is the key stepFor the determination of the rate controlling step, intraparticle diffusion model of Weber’s is usually used:(7)qt=kidt1/2+C,where C is the intercept and kid (mg g−1 min−0.5) is intraparticle diffusion rate constant, which can be evaluated from slope of qt versus t1/2 plot. If the regression of qt versus t1/2 is linear and passes through the origin, the only rate-limiting step is intraparticle diffusion.For the understanding of kinetic mechanism, the amount of heavy metals adsorption on the graphitic magnetic carbon nanostructure prepared from watermelon wasteqt was plotted versus the square root of time (Figure 16). Figure showed an initial curve followed by the linear relationship. The initial curve can be explained by the boundary layer effect while the linear part corresponds to the intraparticle diffusion.Figure 16
Intraparticle diffusion plot for heavy metals adsorption on nanocomposite prepared from watermelon waste.The linear plots deviate from the origin clearly indicating that intraparticular diffusion may have more than one controlling steps in selected heavy metals adsorption.


### 3.4. Effect of pH

One of the most important factors that affects the adsorption process is pH because it affects surface charge of the prepared adsorbent, degree of ionization, and speciation of the adsorbate. The pH effect on adsorption of selected metals is given in Figure17. The figure indicated that the adsorption of arsenic at pH from 1 to 9 was not affected; however a decline was noted at pH above 9. For chromium from 1 to 7 the adsorption was unaffected; however a decline was noted at pH above 7. For copper there was a gradual decrease in adsorption with increase in pH. For lead and zinc at pH from 1 to 10 and 1 to 8, respectively, there was no effect; however a decline was noted above these ranges.Figure 17
Effect of pH of heavy metals adsorption on magnetic carbon nanocomposites prepared from watermelon waste.


### 3.5. Adsorption Thermodynamics

To determine the adsorption thermodynamics, adsorption experiments were carried out at 30, 40, 50, and 60°C. The Van’t Hoff equation was utilized to determineΔH° and ΔS° of the adsorption process.(8)ln⁡K=ΔS°R-ΔHRT;K is the distribution constant of adsorption, ΔH° is the enthalpy change, ΔS° is the entropy change, and T is temperature in Kelvin while R is universal gas constant.The value ofΔH° was calculated from the slope while ΔS° were calculated from intercept of ln⁡K and 1/T plot (Figure 18) for adsorption of heavy metals on adsorbent prepared from watermelon waste. The values of ΔH° and ΔS° are given in Table 4.Table 4
Thermodynamics parameters for the adsorption of heavy metals on carbon nanostructures prepared from watermelon waste.
Heavy metals Δ H ° Δ S ° Δ G ° 25°C 30°C 35°C 40°C 45°C Arsenic −4.0926 29.156 −8.69 −8.84 −8.98 −9.14 9.28 Chromium −9.512 55.742 −16.62 −16.90 −17.18 −17.46 −17.74 Copper −10.795 54.387 −16.22 −16.49 −16.77 −17.04 −17.31 Lead −14.721 61.258 −18.27 −18.58 −18.89 −19.19 −19.50 Zinc −16.645 70.944 −21.16 −21.52 −21.87 −22.23 −22.58Figure 18
Van’t Hoff plot for the adsorption of heavy metals on nanocomposite prepared from watermelon waste.The positive value ofΔS° in Table 4 indicates that, during the adsorption process, there is an increase in the randomness solid/solution system interface whereas the negative values of ΔH° showed that the adsorption on the prepared iron oxide magnetic carbon nanocomposites is an exothermic process.The values of standard free energyΔG° were calculated from (9) and are given in Table 4.(9)ΔG0=ΔH0-TΔS0.The spontaneous character of the process is signified by the negative values of ΔG° at different temperatures and shows high affinity of the heavy metals towards the prepared adsorbents. As the values of ΔG° increase with the increase in temperature it is shown that at high temperature the adsorption process is more favorable for the heavy metals adsorption.Therefore it is concluded that the adsorbent prepared from biomass can be used for the detoxification of heavy metals from water as alternative of powdered activated carbon.


## 3.1. Characterization of Fe2O3 Magnetic Carbon Nanocomposites Made from Watermelon Waste

A special designed chamber as shown in Figure1 was used to prepare magnetic adsorbent from watermelon waste (peel). The magnetic properties of the prepared adsorbent were noted by subjecting it to the magnetic bar. The attraction of the adsorbent by magnetic bar showed the presence of magnetic oxides in the prepared carbon nanostructures.Figures2 and 3 indicated the surface area and pore distribution of magnetic adsorbent, respectively, whereas Table 1 showed different surface parameters of the prepared adsorbent.Table 1
Parameters (physical) of the adsorbent synthesized from watermelon waste.
BET, surface area (m2/g) 71.35 Langmuir, surface area (m2/g) 261.50 Pore volume total (cm3/g) 0.63 Micropores volume (cm3/g) 0.27 Pore diameter, average (Å) 115.20Figure 2
Graph showing BET surface area of the prepared iron oxide carbon nanocomposite from watermelon waste.Figure 3
Graph showing distribution of pores in the prepared iron oxide magnetic carbon nanocomposites from watermelon waste.The XRD spectra of the prepared adsorbent from watermelon waste are highlighted in Figure4, suggesting that Fe3O4 has been deposited in carbon. XRD not only help in the structure determination but also help in particles size measurement [23]. Peaks of diffraction at 2θ of 28.35, 30.2, 35.6, 40.55, 50.2, and 58.25 indicate corresponding indices (220, 311, 400, 422, 511, and 440 planes of cubic unite cell) as previously reported for magnetite structure [24, 25]. The diffraction peaks at 2θ of 10.45, 13.5, and 20.85 as already reported in literature are related to maghemite and hematite [24]. The size of the prepared adsorbent was calculated by using the equation of Debye-Scherrer. (1)D=KλβCos⁡θ,where the mean size is represented by D, K is constant (0.94), λ is the wavelength (1.55060 Å) of X-ray, and β shows excess line broadening, while Bragg angle is represented by θ.(2)β=B-b,where B is the line width (in radian) and b shows instruments line broadening (in radian) [25]. By using formula (1), the sizes of the nanocomposite were calculated and found in the range of 90–250 nm.Figure 4
XRD spectra of magnetic carbon nanocomposites prepared from watermelon waste.For the characterization of the nanocomposite the most widely used technique is the IR Spectroscopy. The IR shows the structure morphology, nature of surface hydroxyl groups, and adsorbed H2O. At 580 cm−1 and 400 cm−1 broad bands correspond to magnetite structure. The Infrared spectra of iron oxide magnetic carbon nanocomposites prepared from watermelon waste (Far and Mid region) are shown in Figures 5 and 6. The peaks in range 1000–1200 cm−1 represent C-C and C-O stretching while 573.60 cm−1 of iron oxide represents the deposited magnetite in the prepared adsorbent.Figure 5
Far IR spectra of magnetic carbon nanocomposites prepared from watermelon waste.Figure 6
Mid IR spectra of magnetic carbon nanocomposites prepared from watermelon waste.Figure7 shows the surface morphology of the prepared adsorbent (high and low magnification). The SEM analysis shows the differences in size and shape of the prepared composite. The white patches of the images show crystalline structure of the prepared composite whereas grayish/black spots show the presence of carbon. The aggregation of iron oxide in the photograph is attributed to the contents of moisture absorbed by the prepared adsorbent. The aggregation of particles decreases the surface area of adsorbent and thus decreases its adsorption capacity. It was also observed from the images that the shape of the Fe3O4 appears somewhat cubical, while the size of nanocomposite was from 50 to 300 nm.Figure 7
SEM images of magnetic carbon nanocomposites prepared from watermelon waste at different magnification.
(a) (b) (c)Figure8 showed the TGA curve for the prepared adsorbent. The spectra show dehydration in two stages. About 9.6% loss of mass was observed at 400°C to 850°C; however no significant losses were observed above this temperature (up to 970°C). The observed mass loss was due to the dehydration of moisture content from the prepared nanocomposite. In case of DTA analysis two endothermic peaks were seen in the range of 60°C–350°C.Figure 8
TG/DTA curves of magnetic carbon nanocomposites prepared from watermelon waste.Figure9 shows the Electron Dispersive X-ray (EDX) analysis of prepared iron oxide composites of watermelon waste that showed the existence of carbon (C), iron (Fe), and oxygen (O). Also a small peak was observed which represents calcium (Ca) as an impurity. In the prepared iron oxide composites the peaks of Fe-Kα, Fe-Lα, O-Kα, and Fe-Kβ showed the deposition of iron oxide as also reported by Giles et al. [25].Figure 9
EDX spectra of magnetic carbon nanocomposites prepared from watermelon waste.


## 3.2. Adsorption Isotherm

### 3.2.1. Giles Isotherms

The adsorption of heavy metal on the adsorbents prepared from watermelon waste was studied using Giles isotherm [26]. The Giles adsorption isotherm of the selected heavy metals on iron oxide nanocomposites prepared from watermelon waste is shown in Figure 10. The isotherms for these metals are C type.Figure 10
Giles adsorption isotherms of heavy metals on adsorbent prepared from watermelon waste.


### 3.2.2. Langmuir Isotherm

Langmuir adsorption isotherm assumes that the maximum adsorption corresponds to a saturated monolayer of solute molecules on the adsorbent surface, having no interaction with molecules adsorbed from lateral sides [27]. The linear form of Langmuir isotherm is given as(3)Cq=CQ0+1Q0b.The above equation shows that q represents quantity of adsorbate adsorbed in mg·g−1, C represents the equilibrium concentration of adsorbate in mg·L−1 while “Q0” and “b” are Langmuir constants, and “Q0” is the maximum adsorption capacity of the adsorbent and also “b” is the energy of the process.Langmuir plot of specific adsorption (C/q) against equilibrium concentration (C) for adsorbent prepared from watermelon waste for selected heavy metals is shown in Figure 11. The slope and intercept were used to calculate the values of Langmuir constants Q0 and b (Table 2).Table 2
Langmuir adsorption constants for heavy metals on nanostructures from watermelon waste.
Heavy metals Langmuir constants R 2 Freundlich constants R 2 Q 0 b 1 / n K Arsenic 32894 0.025 0.929237 0.9040 859.25 0.9810 Chromium 21012 0.021 0.9274 1.0944 277.86 0.9617 Copper 38258 0.0078 0.8194 1.004 261.25 0.9834 Lead 29837 0.0312 0.8267 0.9156 905.87 0.9910 Zinc 18654 0.0307 0.8192 1.1910 292.96 0.9709Figure 11
Langmuir plot for the adsorption of heavy metals on adsorbent prepared from watermelon waste.


### 3.2.3. Freundlich Isotherm

This isotherm is mostly used to explain the heterogeneous systems [28] and is given by the equation.(4)ln⁡q=ln⁡K+1nln⁡C.In the above equation C shows the equilibrium concentration in mg L−1, q is the amount of adsorbate adsorbed in mg per gm, and K and n are constants of Freundlich. K shows adsorption capacity while n is the adsorption intensity. The Freundlich constants K and 1/n can be obtained from slope and the intercept of ln⁡C against ln⁡q plot.For the selected heavy metals adsorption on adsorbent prepared from watermelon waste the Freundlich isotherm is given in Figure12. The values of K and 1/n are given in Table 2.Figure 12
Freundlich plot for the adsorption of heavy metals on adsorbent prepared from watermelon waste.From Table2 it is clear that Freundlich adsorption isotherm model fitted the data better than Langmuir isotherm. Also R2 values are higher for this model.


## 3.2.1. Giles Isotherms

The adsorption of heavy metal on the adsorbents prepared from watermelon waste was studied using Giles isotherm [26]. The Giles adsorption isotherm of the selected heavy metals on iron oxide nanocomposites prepared from watermelon waste is shown in Figure 10. The isotherms for these metals are C type.Figure 10
Giles adsorption isotherms of heavy metals on adsorbent prepared from watermelon waste.


## 3.2.2. Langmuir Isotherm

Langmuir adsorption isotherm assumes that the maximum adsorption corresponds to a saturated monolayer of solute molecules on the adsorbent surface, having no interaction with molecules adsorbed from lateral sides [27]. The linear form of Langmuir isotherm is given as(3)Cq=CQ0+1Q0b.The above equation shows that q represents quantity of adsorbate adsorbed in mg·g−1, C represents the equilibrium concentration of adsorbate in mg·L−1 while “Q0” and “b” are Langmuir constants, and “Q0” is the maximum adsorption capacity of the adsorbent and also “b” is the energy of the process.Langmuir plot of specific adsorption (C/q) against equilibrium concentration (C) for adsorbent prepared from watermelon waste for selected heavy metals is shown in Figure 11. The slope and intercept were used to calculate the values of Langmuir constants Q0 and b (Table 2).Table 2
Langmuir adsorption constants for heavy metals on nanostructures from watermelon waste.
Heavy metals Langmuir constants R 2 Freundlich constants R 2 Q 0 b 1 / n K Arsenic 32894 0.025 0.929237 0.9040 859.25 0.9810 Chromium 21012 0.021 0.9274 1.0944 277.86 0.9617 Copper 38258 0.0078 0.8194 1.004 261.25 0.9834 Lead 29837 0.0312 0.8267 0.9156 905.87 0.9910 Zinc 18654 0.0307 0.8192 1.1910 292.96 0.9709Figure 11
Langmuir plot for the adsorption of heavy metals on adsorbent prepared from watermelon waste.


## 3.2.3. Freundlich Isotherm

This isotherm is mostly used to explain the heterogeneous systems [28] and is given by the equation.(4)ln⁡q=ln⁡K+1nln⁡C.In the above equation C shows the equilibrium concentration in mg L−1, q is the amount of adsorbate adsorbed in mg per gm, and K and n are constants of Freundlich. K shows adsorption capacity while n is the adsorption intensity. The Freundlich constants K and 1/n can be obtained from slope and the intercept of ln⁡C against ln⁡q plot.For the selected heavy metals adsorption on adsorbent prepared from watermelon waste the Freundlich isotherm is given in Figure12. The values of K and 1/n are given in Table 2.Figure 12
Freundlich plot for the adsorption of heavy metals on adsorbent prepared from watermelon waste.From Table2 it is clear that Freundlich adsorption isotherm model fitted the data better than Langmuir isotherm. Also R2 values are higher for this model.


## 3.3. Adsorption Kinetics

### 3.3.1. Effect of Contact Time

In adsorption processes contact time required for reaching equilibrium for an adsorbent is an important factor. For the metals under study the contact time required to reach equilibrium is shown in Figure13. In first few minutes the uptake of contaminants was very fast as initially more sites of adsorbent are available for adsorption of metals. As the time passes maximum number of sites is occupied by the metals and adsorption process slows down. At the end the equilibrium time of adsorption occurs due to saturation of the adsorbents. The equilibrium time for arsenic, chromium, copper, lead, and zinc was 260, 220, 280, 200, and 200 minutes, respectively.Figure 13
Effect of contact time on adsorption of heavy metals on nanocomposites prepared from watermelon waste.


### 3.3.2. Adsorption Kinetic Models

The knowledge regarding adsorption kinetics plays a significant role in the removal of water pollutants. Therefore to evaluate the kinetic parameters, the Lagergren first-order and pseudo-second-order models were used [29].The pseudo-first-order equation can be expressed by the following relation:(5)ln⁡qe-q=ln⁡qe-Kat,where qe and q (mg g−1) are the amount of adsorbed adsorbate at equilibrium and time t, respectively, and Ka (min−1) is the rate constant. Ka can be calculated from slope of the plot of ln⁡(qe-q) versus t. This equation shows a linear relationship between ln⁡(qe-q) and t.K a and R2 values (Table 3) were calculated by plotting ln⁡(qe-q) against t for metals under study adsorption on adsorbent prepared from watermelon waste as shown in Figure 14. Ka and R2 values (Table 3) were calculated from ln⁡(qe-q) versus t plot.Table 3
Pseudo first- and second-order adsorption kinetics parameters for the adsorption of heavy metals on magnetic carbon nanostructures.
Heavy metals Pseudo-first-order kinetics model Pseudo-second-order kinetics model K a R 2 K 2 R 2 Arsenic 0.0158999 0.974546 2.32 ∗ 10 - 6 0.992 Chromium 0.0140065 0.994028 2.25 ∗ 10 - 6 0.987 Copper 0.0124186 0.907812 6.14 ∗ 10 - 7 0.968 Lead 0.0178124 0.962160 1.72 ∗ 10 - 6 0.946 Zinc 0.0162281 0.967867 2.05 ∗ 10 - 6 0.989Figure 14
Pseudo first-order kinetics plot for the adsorption of heavy metals on nanocomposite prepared from watermelon waste.The pseudo-second-order equation can be expressed by the relation(6)tqt=1K2q2+1qt,where K2 (g mg−1 min−1) is the rate constant of adsorption and q (mg g−1) is the amount of adsorbate adsorbed at equilibrium and qt is the amount of adsorbate adsorbed at time t. The values of K2 and q are calculated from intercept and slope of the straight line, respectively.K a and R2 values (Table 3) were calculated from plotting t/qt versus t plot (Figure 15).Figure 15
Pseudo second-order kinetics plot for the adsorption of heavy metals on nanocomposite prepared from watermelon waste.Table3 shows that the adsorption kinetics could be best explained in terms of the pseudo-second-order rate equation with precision in the correlation coefficients, while the Lagergren rate equation did not reflect the experimental results.


### 3.3.3. Adsorption Mechanism

In the adsorption process the main steps involved in the removal of adsorbate by adsorbent are the following:(i)
One step is transport of ingoing particles to the external surface of the adsorbent(ii)
Another step is transport of the adsorbate through the pores of adsorbent except for a small amount of the adsorption which occurs on the external surface (interparticle diffusion) and adsorption of the ingoing particles (adsorbate) on to interior surface of the adsorbent(iii)
Amongst these, the rate controlling step, which affects the overall removal rate, is the key stepFor the determination of the rate controlling step, intraparticle diffusion model of Weber’s is usually used:(7)qt=kidt1/2+C,where C is the intercept and kid (mg g−1 min−0.5) is intraparticle diffusion rate constant, which can be evaluated from slope of qt versus t1/2 plot. If the regression of qt versus t1/2 is linear and passes through the origin, the only rate-limiting step is intraparticle diffusion.For the understanding of kinetic mechanism, the amount of heavy metals adsorption on the graphitic magnetic carbon nanostructure prepared from watermelon wasteqt was plotted versus the square root of time (Figure 16). Figure showed an initial curve followed by the linear relationship. The initial curve can be explained by the boundary layer effect while the linear part corresponds to the intraparticle diffusion.Figure 16
Intraparticle diffusion plot for heavy metals adsorption on nanocomposite prepared from watermelon waste.The linear plots deviate from the origin clearly indicating that intraparticular diffusion may have more than one controlling steps in selected heavy metals adsorption.


## 3.3.1. Effect of Contact Time

In adsorption processes contact time required for reaching equilibrium for an adsorbent is an important factor. For the metals under study the contact time required to reach equilibrium is shown in Figure13. In first few minutes the uptake of contaminants was very fast as initially more sites of adsorbent are available for adsorption of metals. As the time passes maximum number of sites is occupied by the metals and adsorption process slows down. At the end the equilibrium time of adsorption occurs due to saturation of the adsorbents. The equilibrium time for arsenic, chromium, copper, lead, and zinc was 260, 220, 280, 200, and 200 minutes, respectively.Figure 13
Effect of contact time on adsorption of heavy metals on nanocomposites prepared from watermelon waste.


## 3.3.2. Adsorption Kinetic Models

The knowledge regarding adsorption kinetics plays a significant role in the removal of water pollutants. Therefore to evaluate the kinetic parameters, the Lagergren first-order and pseudo-second-order models were used [29].The pseudo-first-order equation can be expressed by the following relation:(5)ln⁡qe-q=ln⁡qe-Kat,where qe and q (mg g−1) are the amount of adsorbed adsorbate at equilibrium and time t, respectively, and Ka (min−1) is the rate constant. Ka can be calculated from slope of the plot of ln⁡(qe-q) versus t. This equation shows a linear relationship between ln⁡(qe-q) and t.K a and R2 values (Table 3) were calculated by plotting ln⁡(qe-q) against t for metals under study adsorption on adsorbent prepared from watermelon waste as shown in Figure 14. Ka and R2 values (Table 3) were calculated from ln⁡(qe-q) versus t plot.Table 3
Pseudo first- and second-order adsorption kinetics parameters for the adsorption of heavy metals on magnetic carbon nanostructures.
Heavy metals Pseudo-first-order kinetics model Pseudo-second-order kinetics model K a R 2 K 2 R 2 Arsenic 0.0158999 0.974546 2.32 ∗ 10 - 6 0.992 Chromium 0.0140065 0.994028 2.25 ∗ 10 - 6 0.987 Copper 0.0124186 0.907812 6.14 ∗ 10 - 7 0.968 Lead 0.0178124 0.962160 1.72 ∗ 10 - 6 0.946 Zinc 0.0162281 0.967867 2.05 ∗ 10 - 6 0.989Figure 14
Pseudo first-order kinetics plot for the adsorption of heavy metals on nanocomposite prepared from watermelon waste.The pseudo-second-order equation can be expressed by the relation(6)tqt=1K2q2+1qt,where K2 (g mg−1 min−1) is the rate constant of adsorption and q (mg g−1) is the amount of adsorbate adsorbed at equilibrium and qt is the amount of adsorbate adsorbed at time t. The values of K2 and q are calculated from intercept and slope of the straight line, respectively.K a and R2 values (Table 3) were calculated from plotting t/qt versus t plot (Figure 15).Figure 15
Pseudo second-order kinetics plot for the adsorption of heavy metals on nanocomposite prepared from watermelon waste.Table3 shows that the adsorption kinetics could be best explained in terms of the pseudo-second-order rate equation with precision in the correlation coefficients, while the Lagergren rate equation did not reflect the experimental results.


## 3.3.3. Adsorption Mechanism

In the adsorption process the main steps involved in the removal of adsorbate by adsorbent are the following:(i)
One step is transport of ingoing particles to the external surface of the adsorbent(ii)
Another step is transport of the adsorbate through the pores of adsorbent except for a small amount of the adsorption which occurs on the external surface (interparticle diffusion) and adsorption of the ingoing particles (adsorbate) on to interior surface of the adsorbent(iii)
Amongst these, the rate controlling step, which affects the overall removal rate, is the key stepFor the determination of the rate controlling step, intraparticle diffusion model of Weber’s is usually used:(7)qt=kidt1/2+C,where C is the intercept and kid (mg g−1 min−0.5) is intraparticle diffusion rate constant, which can be evaluated from slope of qt versus t1/2 plot. If the regression of qt versus t1/2 is linear and passes through the origin, the only rate-limiting step is intraparticle diffusion.For the understanding of kinetic mechanism, the amount of heavy metals adsorption on the graphitic magnetic carbon nanostructure prepared from watermelon wasteqt was plotted versus the square root of time (Figure 16). Figure showed an initial curve followed by the linear relationship. The initial curve can be explained by the boundary layer effect while the linear part corresponds to the intraparticle diffusion.Figure 16
Intraparticle diffusion plot for heavy metals adsorption on nanocomposite prepared from watermelon waste.The linear plots deviate from the origin clearly indicating that intraparticular diffusion may have more than one controlling steps in selected heavy metals adsorption.


## 3.4. Effect of pH

One of the most important factors that affects the adsorption process is pH because it affects surface charge of the prepared adsorbent, degree of ionization, and speciation of the adsorbate. The pH effect on adsorption of selected metals is given in Figure17. The figure indicated that the adsorption of arsenic at pH from 1 to 9 was not affected; however a decline was noted at pH above 9. For chromium from 1 to 7 the adsorption was unaffected; however a decline was noted at pH above 7. For copper there was a gradual decrease in adsorption with increase in pH. For lead and zinc at pH from 1 to 10 and 1 to 8, respectively, there was no effect; however a decline was noted above these ranges.Figure 17
Effect of pH of heavy metals adsorption on magnetic carbon nanocomposites prepared from watermelon waste.


## 3.5. Adsorption Thermodynamics

To determine the adsorption thermodynamics, adsorption experiments were carried out at 30, 40, 50, and 60°C. The Van’t Hoff equation was utilized to determineΔH° and ΔS° of the adsorption process.(8)ln⁡K=ΔS°R-ΔHRT;K is the distribution constant of adsorption, ΔH° is the enthalpy change, ΔS° is the entropy change, and T is temperature in Kelvin while R is universal gas constant.The value ofΔH° was calculated from the slope while ΔS° were calculated from intercept of ln⁡K and 1/T plot (Figure 18) for adsorption of heavy metals on adsorbent prepared from watermelon waste. The values of ΔH° and ΔS° are given in Table 4.Table 4
Thermodynamics parameters for the adsorption of heavy metals on carbon nanostructures prepared from watermelon waste.
Heavy metals Δ H ° Δ S ° Δ G ° 25°C 30°C 35°C 40°C 45°C Arsenic −4.0926 29.156 −8.69 −8.84 −8.98 −9.14 9.28 Chromium −9.512 55.742 −16.62 −16.90 −17.18 −17.46 −17.74 Copper −10.795 54.387 −16.22 −16.49 −16.77 −17.04 −17.31 Lead −14.721 61.258 −18.27 −18.58 −18.89 −19.19 −19.50 Zinc −16.645 70.944 −21.16 −21.52 −21.87 −22.23 −22.58Figure 18
Van’t Hoff plot for the adsorption of heavy metals on nanocomposite prepared from watermelon waste.The positive value ofΔS° in Table 4 indicates that, during the adsorption process, there is an increase in the randomness solid/solution system interface whereas the negative values of ΔH° showed that the adsorption on the prepared iron oxide magnetic carbon nanocomposites is an exothermic process.The values of standard free energyΔG° were calculated from (9) and are given in Table 4.(9)ΔG0=ΔH0-TΔS0.The spontaneous character of the process is signified by the negative values of ΔG° at different temperatures and shows high affinity of the heavy metals towards the prepared adsorbents. As the values of ΔG° increase with the increase in temperature it is shown that at high temperature the adsorption process is more favorable for the heavy metals adsorption.Therefore it is concluded that the adsorbent prepared from biomass can be used for the detoxification of heavy metals from water as alternative of powdered activated carbon.


## 4. Conclusions

The removal of heavy metals from water samples was studied by using biosorbent prepared from peel of watermelon and was characterized by surface area analyzer, FTIR, XRD, EDX, SEM, and TG/DTA. Freundlich and Langmuir isotherms were used to determine the adsorption parameters. Other adsorption parameters like adsorption kinetics and effects of time, pH, and temperature were also determined. The best fits were obtained for Freundlich isotherm and with second-order kinetics model for the kinetics experiments. At high pH there was a decline in percent adsorption. The values ofΔS° were positive while those of ΔH° and ΔG° were negative. It was concluded from data that adsorbent prepared from watermelon waste has high adsorption capacities and thus can be used as an efficient adsorbent for the removal of heavy metals.



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*Source: 5670371-2017-01-26.xml*