# A Novel Absorbent of Nano-Fe Loaded Biomass Char and Its Enhanced Adsorption Capacity for Phosphate in Water

Authors: Hongguang Zhou; Zhenmao Jiang; Shiqiang Wei
Journal: Journal of Chemistry
 (2013)

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## Abstract

A novel composite adsorbent of Fe loaded biomass char (Fe-BC) was fabricated to treat phosphorus in water. Fe-BC was prepared by a procedure including metal complex anion incorporation and precipitation with the pyrolysis char of corn straw as supporting material. The abundant porous structures of the as-prepared sample can be easily observed from its scanning electron microscopy (SEM) images. Observations by X-ray diffraction (XRD) and X-ray photoelectron spectroscopy (XPS) analyses show that inorganic nanoiron oxides deposited in the composite could be amorphous hydrous iron oxideα-FeOOH. Adsorption of phosphate onto the Fe-BC composite and its precursor (BC) from aqueous solutions were investigated and discussed. The equilibrium adsorption data of phosphate was described by Langmuir and Freundlich models, and Langmuir isotherm was found to be better fitted than Freundlich isotherm. The maximum phosphate adsorption capacity for phosphate of Fe-BC was as high as 35.43 mg/g, approximately 2.3 times of BC at 25°C. The adsorption kinetics data were better fitted by pseudo-second-order model and intraparticle diffusion model, indicating that the adsorption process was complex. The Fe-BC composite has been proved as an effective adsorbent of phosphate from aqueous solutions owing to its unique porous structures and the greater Lewis basicity of the α-FeOOH.


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## Body

## 1. Introduction

Phosphorus is considered as the main culprit of lake eutrophication [1]. Excess phosphorus will stimulate the algal blooms, causing deterioration of water quality [2]. In recent years, human activities dramatically increased the loads of phosphate in environment and its cycling rate on Earth, such as the production and application of a plenty of detergents, agricultural pesticides, and fertilizers [3]. The increased amount of phosphorus in water bodies poses greater potentials to the occurring of eutrophication. It has been reported that the red tide may occur at concentration of phosphorus higher than 0.03 mg/L in the lake (sea) [4].Municipal wastewater may contain variety concentrations of phosphate ranging from 4 to 15 mg-P/L, and industrial wastewater (such as detergent manufacturing) may contain phosphate levels well in excess of 10 mg-P/L [5]. Hence high effective methods for the removal of phosphate from wastewater need to be established. Traditional biological treatment of phosphorus has been proved to be highly variable due to its hard operation conditions [6]; thus discharge limits of phosphate were hardly matched depending only on this technology regardless of its high cost. Chemical precipitation technology has been wildly used in phosphate removal, usually with salts of iron (such as ferric chloride) [7–9], aluminum [10, 11], or lime [12]. However, the difficulties of excessive sludge handling and cost of added chemical materials would hinder its widespread application. Other effective phosphorus removal techniques such as ion exchange and electrodialysis also encountered difficulties of complicated management and high cost. Adsorption has been regarded as one of the most effective and economical methods for the removal of phosphorus. The key to the success of the method depends on the selection of adsorbent with high adsorption capacity. Numerous studies have been conducted for this purpose, such as activated alumina [4, 13], metal oxide hydroxides [14–21], hydrotalcite [22], palygorskite [23, 24], zeolite [13, 25–27], slag [28–31] and layered double hydroxides [32–36], as well as some waste materials such as red mud [37, 38], fly ash [39, 40], activated carbon [41], modified wheat residues [42, 43], and peat [44].Metal oxides are well known for their industrial applications as adsorbents, catalysts, and catalyst supports [45]. Hydrous iron oxides performance is highlighted in phosphate removal, and their adsorption capacity of phosphorus can reach up to 17 mg-P/g [21]. This is mainly attributed to the formation of a stable bidentate ligand between ion oxides and phosphate. In particular, with the rapid development of nanotechnology, these kinds of metal oxide hydroxides have been prepared in nanoscale size by some researchers (Pan et al. 2009) [46]. Inorganic nanosize adsorbents showed high adsorption capacity due to their surface effect and the small size effect brought by the miniaturization of the particle size. However, conventional nanosized powder adsorbent has intrinsic drawback due to the difficulties of sedimentation and separation in such a slurry type system. Many efforts had been made to structure inorganic or organic materials with specific size, aperture, and morphology to overcome this limitation and extend its environmental applications, such as microspheres [47]. Precursor immersion-surface deposition method is another useful way to solve these problems; nanosize materials were well diffused into the precursor and then fixed by changing its chemical speciation.There are various kinds of materials which can be used as precursor. Biomass char (BC) was considered as one of the best for its large surface areas, richness of inherent porous structures, and low cost. Biomass char can be obtained from biomass waste easily. Biomass wastes, derived from plants, are the most widely available renewable resource [48]. However, improper disposal of the increasing quantities of biomass waste may lead to various environmental issues. Agriculture produces large amount of biomass waste; for example, the annual production of corn straw reached about 0.22 billion tons only in China in 2009 [49], most of which were burnt directly outside in the field, causing atmospheric pollution, such as increased concentration of PM2.5, enhanced carbon emission, and CO2 concentration. The pyrolysis technology of biomass waste for bioenergy production had been considered as a promising method with higher energy conversion efficiency [50]. Recently, biomass waste pyrolysis for fuel gas or biooil also aroused some attention [51, 52].As a byproduct of biomass waste pyrolysis, biomass char is only about 10–40% of the total production [53]. BC deriving from biomass waste pyrolysis has relatively high fixed-carbon content and inherent porous structures. It has been reported that BC obtained from biomass pyrolysis at 673–873 K has a surface area ranging from 80 to 450 m2/g [43–57]. Thus BC could be a potential absorbent for the removal of pollutants from water. Some studies have showed that biomass char could effectively adsorb many kinds of cation [53, 56] and anion [55–57], including phosphate anion. In order to make use of the advantages of abundant biomass based BC and the high adsorptive capacity of nanohydrous iron oxides, a novel composite adsorbent has been fabricated following the procedure of incorporation of hydrous iron oxides nanoparticles into the biochar from the pyrolysis of corn straw. The basic physicochemical properties of the composite and its precursor were characterized and their performances on phosphate adsorption were investigated. Adsorption isotherms and the kinetics of phosphate adsorption on the composite adsorbents were compared with its precursor and some similar absorbents from literature; the results show that the synthesized Fe-BC is a promising absorbent for phosphate with remarkably high adsorption capacity.


## 2. Experimental

### 2.1. Materials and Methods

The raw biomass material was corn straw, a common agricultural waste, obtained from the countryside in Pengshui, Chongqing Province, China. Fresh corn straw was air-dried, cut into 1–4 cm small pieces, washed several times with deionized water, dried in a furnace at 333 K for 24 h, and then being sieved to the particle diameters 1 mm after grated for pyrolysis. The phosphate solution was prepared by dissolving potassium dihydrogen phosphate (KH2PO4) in deionized water. All chemicals used were of analytical grade.


#### 2.1.1. Pyrolysis Experiments

The biochar samples were obtained by pyrolysis experiments, which were carried out in a packed bed reactor in flowing nitrogen atmosphere with a heating rate of 5°C/min. The final temperature was kept at 773 K and the solid residence time was about one hour.


#### 2.1.2. Preparation of Nano-Fe Loaded Biochar

There are some basic groups on the BC as well as some acidic functional groups, which provide different adsorption active sites. The acidic functional groups may be more dominant than the basic groups on BC. In our preliminary experiment, the mass of Fe loaded on the composite withFeCl4- is 3.7 times higher than the FeCl3. BC was weighed and immersed into 1 mol/L FeCl4- aqueous solution (ratio of solid/solution is 1 : 20) at pH 2.0 under continuous stirring at room temperature for 24 h. Then it was filtered by a 0.45 μm microfiltration membrane to collect the upside solid and washed with deionized water until the filtrate becomes clear. The solid sample was transferred into a saturated NaCl solution, and the pH of the solution was maintained at 12.0 by adding 0.1 M NaOH solutions. During this process it was stirred by mixer, and the mixing time lasts for 30 minutes. After that, the sample was filtered off, washed thoroughly three times with deionized water, and then dried in a vacuum oven with a −0.05 Kpa vacuum at 60°C for 24 h. The dried power was kept in a drier to make sure it was totally dried. The amount of Fe(III) loaded onto BC was then measured using atomic absorption spectroscopy (AAS) method [58].


### 2.2. Characterization Methods

The specific surface area of obtained biomass char (BC) and Fe loaded BC was analyzed by nitrogen adsorption using the Brunauer-Eett-Teller (BET) method with a Micromeritics ASAP-2010C automatic analyzer (Micromeritics Col Inc., Australia) at the temperature of 77 K. Also, the char was also observed using Scanning Electron microscopy (SEM) analysis by SEM-EDS (S-3400N HITACHI Japan). X-ray powder diffraction (XRD) experiments were performed on a D/max-3B diffractometer with Cu Kα irradiation at a scan rate of 0.02°2θs−1, to determine the identity of any phase present and its crystallite size. The composites were vacuum-dried at 30°C before characterization and ground for SEM and XRD analysis. XPS spectra of the Fe-BC adsorbent before and after adsorption were performed by an X-ray photoelectron spectroscopy (Kratos AXIS Ultra, UK) with the monochromatic Al Kα X-ray radiation (1486.7 eV). The wide scans were conducted from 0 to 1400 eV with pass energy of 160 eV. The high resolution scans were conducted according to the peak being examined with pass energy of 40 eV. The energy scale of the XPS spectra was calibrated with graphitic carbon as the reference at a binding energy of 284.8 eV due to the surface contamination. The XPS spectra peaks of Fe 2s were fitted using the XPS peak software.


### 2.3. Kinetic Adsorption Experiments

Simulation phosphate solutions were used throughout the adsorption tests. Initially, a stock solution was prepared by dissolving a certain amount of analytically pure KH2PO4 in deionized water. For adsorption experiments, the phosphate solutions with concentrations in the range of 1–100 mg/L were prepared by successive dilution of the stock solution with deionized water at room temperature. The supernatant solution was separated from the adsorbent by microfiltration membrane. Phosphate concentration in the supernatant was estimated spectrophotometrically by the molybdenum blue method; absorbance at 700 nm was monitored by UV-vis spectrophotometer.Kinetic studies were carried out to establish the effect of contact time on the adsorption process and to quantify the adsorption rate. For kinetics adsorption experiments, each 0.05 g of adsorbents (BC, Fe-BC) was added into a series of flasks containing 50 mL phosphate solution (20 mg-P/L), separately. The initial pH of the solution was maintained at 3.0 by adding 0.1 M NaOH or 0.1 M HCl solutions. The flasks were placed in a thermostatic shaker at 25°C. At given time, each one of the flasks was taken out and immediately filtered by a 0.45μm microfiltration membrane to collect the filtrate and then the concentration of residual phosphate in the filtrate was determined by the method mentioned above.


### 2.4. Equilibrium Adsorption Experiments

For the equilibrium adsorption experiments, each 0.05 g of absorbents was added into a series of flasks containing 50 mL solution with phosphate concentration ranging from 1 to 100 mg-P/L. The flasks were then sealed and put in a thermostatic shaker at various constant temperatures and shaken at the 120 rpm for 240 min. Then the solution in the flasks was filtered and the phosphate concentration in the filtrate was measured. The phosphate absorbed at equilibrium was calculated using the following equation:(1)Q=V(C0-Ce)m,
where Q (mg/g) is the amount of phosphate adsorbed, V (mL) is the volume of the solution,C0 and Ce (mg/L) are the initial and equilibrium concentrations of phosphate, respectively, and m (g) is the weight of adsorbent.


## 2.1. Materials and Methods

The raw biomass material was corn straw, a common agricultural waste, obtained from the countryside in Pengshui, Chongqing Province, China. Fresh corn straw was air-dried, cut into 1–4 cm small pieces, washed several times with deionized water, dried in a furnace at 333 K for 24 h, and then being sieved to the particle diameters 1 mm after grated for pyrolysis. The phosphate solution was prepared by dissolving potassium dihydrogen phosphate (KH2PO4) in deionized water. All chemicals used were of analytical grade.


### 2.1.1. Pyrolysis Experiments

The biochar samples were obtained by pyrolysis experiments, which were carried out in a packed bed reactor in flowing nitrogen atmosphere with a heating rate of 5°C/min. The final temperature was kept at 773 K and the solid residence time was about one hour.


### 2.1.2. Preparation of Nano-Fe Loaded Biochar

There are some basic groups on the BC as well as some acidic functional groups, which provide different adsorption active sites. The acidic functional groups may be more dominant than the basic groups on BC. In our preliminary experiment, the mass of Fe loaded on the composite withFeCl4- is 3.7 times higher than the FeCl3. BC was weighed and immersed into 1 mol/L FeCl4- aqueous solution (ratio of solid/solution is 1 : 20) at pH 2.0 under continuous stirring at room temperature for 24 h. Then it was filtered by a 0.45 μm microfiltration membrane to collect the upside solid and washed with deionized water until the filtrate becomes clear. The solid sample was transferred into a saturated NaCl solution, and the pH of the solution was maintained at 12.0 by adding 0.1 M NaOH solutions. During this process it was stirred by mixer, and the mixing time lasts for 30 minutes. After that, the sample was filtered off, washed thoroughly three times with deionized water, and then dried in a vacuum oven with a −0.05 Kpa vacuum at 60°C for 24 h. The dried power was kept in a drier to make sure it was totally dried. The amount of Fe(III) loaded onto BC was then measured using atomic absorption spectroscopy (AAS) method [58].


## 2.1.1. Pyrolysis Experiments

The biochar samples were obtained by pyrolysis experiments, which were carried out in a packed bed reactor in flowing nitrogen atmosphere with a heating rate of 5°C/min. The final temperature was kept at 773 K and the solid residence time was about one hour.


## 2.1.2. Preparation of Nano-Fe Loaded Biochar

There are some basic groups on the BC as well as some acidic functional groups, which provide different adsorption active sites. The acidic functional groups may be more dominant than the basic groups on BC. In our preliminary experiment, the mass of Fe loaded on the composite withFeCl4- is 3.7 times higher than the FeCl3. BC was weighed and immersed into 1 mol/L FeCl4- aqueous solution (ratio of solid/solution is 1 : 20) at pH 2.0 under continuous stirring at room temperature for 24 h. Then it was filtered by a 0.45 μm microfiltration membrane to collect the upside solid and washed with deionized water until the filtrate becomes clear. The solid sample was transferred into a saturated NaCl solution, and the pH of the solution was maintained at 12.0 by adding 0.1 M NaOH solutions. During this process it was stirred by mixer, and the mixing time lasts for 30 minutes. After that, the sample was filtered off, washed thoroughly three times with deionized water, and then dried in a vacuum oven with a −0.05 Kpa vacuum at 60°C for 24 h. The dried power was kept in a drier to make sure it was totally dried. The amount of Fe(III) loaded onto BC was then measured using atomic absorption spectroscopy (AAS) method [58].


## 2.2. Characterization Methods

The specific surface area of obtained biomass char (BC) and Fe loaded BC was analyzed by nitrogen adsorption using the Brunauer-Eett-Teller (BET) method with a Micromeritics ASAP-2010C automatic analyzer (Micromeritics Col Inc., Australia) at the temperature of 77 K. Also, the char was also observed using Scanning Electron microscopy (SEM) analysis by SEM-EDS (S-3400N HITACHI Japan). X-ray powder diffraction (XRD) experiments were performed on a D/max-3B diffractometer with Cu Kα irradiation at a scan rate of 0.02°2θs−1, to determine the identity of any phase present and its crystallite size. The composites were vacuum-dried at 30°C before characterization and ground for SEM and XRD analysis. XPS spectra of the Fe-BC adsorbent before and after adsorption were performed by an X-ray photoelectron spectroscopy (Kratos AXIS Ultra, UK) with the monochromatic Al Kα X-ray radiation (1486.7 eV). The wide scans were conducted from 0 to 1400 eV with pass energy of 160 eV. The high resolution scans were conducted according to the peak being examined with pass energy of 40 eV. The energy scale of the XPS spectra was calibrated with graphitic carbon as the reference at a binding energy of 284.8 eV due to the surface contamination. The XPS spectra peaks of Fe 2s were fitted using the XPS peak software.


## 2.3. Kinetic Adsorption Experiments

Simulation phosphate solutions were used throughout the adsorption tests. Initially, a stock solution was prepared by dissolving a certain amount of analytically pure KH2PO4 in deionized water. For adsorption experiments, the phosphate solutions with concentrations in the range of 1–100 mg/L were prepared by successive dilution of the stock solution with deionized water at room temperature. The supernatant solution was separated from the adsorbent by microfiltration membrane. Phosphate concentration in the supernatant was estimated spectrophotometrically by the molybdenum blue method; absorbance at 700 nm was monitored by UV-vis spectrophotometer.Kinetic studies were carried out to establish the effect of contact time on the adsorption process and to quantify the adsorption rate. For kinetics adsorption experiments, each 0.05 g of adsorbents (BC, Fe-BC) was added into a series of flasks containing 50 mL phosphate solution (20 mg-P/L), separately. The initial pH of the solution was maintained at 3.0 by adding 0.1 M NaOH or 0.1 M HCl solutions. The flasks were placed in a thermostatic shaker at 25°C. At given time, each one of the flasks was taken out and immediately filtered by a 0.45μm microfiltration membrane to collect the filtrate and then the concentration of residual phosphate in the filtrate was determined by the method mentioned above.


## 2.4. Equilibrium Adsorption Experiments

For the equilibrium adsorption experiments, each 0.05 g of absorbents was added into a series of flasks containing 50 mL solution with phosphate concentration ranging from 1 to 100 mg-P/L. The flasks were then sealed and put in a thermostatic shaker at various constant temperatures and shaken at the 120 rpm for 240 min. Then the solution in the flasks was filtered and the phosphate concentration in the filtrate was measured. The phosphate absorbed at equilibrium was calculated using the following equation:(1)Q=V(C0-Ce)m,
where Q (mg/g) is the amount of phosphate adsorbed, V (mL) is the volume of the solution,C0 and Ce (mg/L) are the initial and equilibrium concentrations of phosphate, respectively, and m (g) is the weight of adsorbent.


## 3. Results and Discussion

### 3.1. Characterization of BC Samples

The BC sample with very high BET surface area (434.7 m2/g) and narrow pore size distribution (Figure 1), its average pore diameter is about 3.5 nm. It may provide very good adsorption capacity and modified potentialities. The loaded treatment may decrease the BET surface area of composite which is only 18.71 m2/g. As suggested, the preloaded nano-Fe particles would block some inner pores or make the pores narrower. Similar result was also reported by Shi concerning the effect of Fe(III) loadings on the pore volume and surface area of the resulting hybrid [58]. The mass of Fe in hybrid treated by FeCl4- is about 4.53%. And the curve of average pore diameter performs a bimodal distribution, which means that the loaded treatment changed the structure and property. Incorporation of nano-Fe into BC also altered its surface and textural morphology as shown by the SEM images in Figure 2. With different magnification (×600 and ×3000), different surface and structure can be seen clearly. The more irregular fragmented structure and pore structure of BC sample may contribute to its high surface area and pore volume.Figure 1
The pore size distribution of samples BC and Fe-BC.Figure 2
SEM images of samples BC and Fe-BC.As shown in Figure3, there are no obvious peaks in the XRD patters which indicated that the iron oxides in the samples existed as amorphous state.Figure 3
XRD diffraction pattern of BC and Fe-BC.


### 3.2. Adsorption Kinetics

The adsorption kinetics curves of phosphate adsorption on BC and Fe-BC are shown in Figure4, which may reflect the differences of adsorption rates and their rate control steps. The adsorption curves of BC and Fe-BC go as the same tendency; they rise sharply at the first 5 min and tend to be gentle after 60 and 120 min, respectively, which means that the adsorption speed is not constant during the whole process and the adsorption equilibrium time on BC is shorter than that on Fe-BC. But the y value of BC at the equilibrium condition is lower than that of Fe-BC, indicating that the adsorption capacity of BC is lower than Fe-BC.Figure 4
The variation of adsorption capacity with adsorption time for phosphate on samples BC and Fe-BC (T = 25°C; adsorbent dose = 1 g/L; phosphate concentration = 20 mg/L, and pH = 3).Four kinetic models were adopted to describe the adsorption process. The pseudo-first-order kinetic model has been widely used to predict sorption kinetics. The adsorption rate is proportional to the concentration of adsorbate. It can be used to describe the simple surface physical absorption. The model is defined as(2)ln(Qe-Qt)=lnQe-k1t.The pseudo-second-order equation assumed that the adsorption mechanism was dominant by chemisorption. The adsorption rate is proportional to square of adsorbate concentration. The pseudo-second-order equation can be expressed as(3)tQt=1k2Qe2+tQe,
where k1 (min−1) and k2 are the pseudo-first-order rate constant and the pseudo-second-order rate constant, respectively, reflecting the adsorption rate change along with the concentration change. The results are showed in Table 1.Table 1
Pseudo-first-order and Pseudo-second-order adsorption kinetic constants of samples BC and Fe-BC.
Samples
Q
e
,
exp (mg/g)
Pseudo-first-order model
Pseudo-second-order model
Q
e
,
cal (mg/g)
k
1 (min-1)
R
2
S.D. (%)
Q
e
,
cal (mg/g)
k
2 (gmg-1min−1)
R
2
S.D. (%)
BC
3.58
3.34
0.508
0.905
16.22
3.52
0.211
0.967
9.51
Fe-BC
11.94
10.58
0.135
0.813
32.30
11.31
0.019
0.905
24.24Compared with pseudo-second-order kinetic, the experimentalQe,exp values of first-order kinetic do not well agree with the calculated Qe,cal values obtained from the curve plots, suggesting that the adsorption process is not maintained by simple surface physical absorption, and some other adsorption mechanisms were involved.Generally, the process of the adsorbate adsorbed by adsorbent can be divided into four steps: firstly, adsorbate molecules transferred to the nearby adsorbent from solution; secondly, adsorbate molecules diffusion through the liquid film up to the surface of absorbent particles, this step usually was called external diffusion or mass transfer; thirdly, adsorbate molecules diffused through the absorbent particles and reached the inner side; this step is usually called intraparticle diffusion or diffusion; Fourthly, adsorbate molecules were attracted at the active sites in the interior of the particles. Step one and four were not the rate-controlling steps due to their happening so fast. And the kinetics of the adsorption will be governed either by diffusion or by a mass transfer mechanism depending on which of the above steps is the slowest. Hence, in this study, two models were investigated to find out the rate-controlling step of the adsorption process.Intraparticle diffusion model is based on the theory proposed by Weber and Morris [60]. It was used to identify the diffusion mechanism. According to this theory,
(4)Qt=k3t+C,
where k3 is the intra-particular diffusion rate constant (mg g−1 min−1/2). If intraparticle diffusion is rate-limited, the plots of adsorbates uptake Qt versus the square root of time (t1/2) would result in a linear relationship. k3 and C values can be obtained from these plots.The result ofQt versus t1/2 is shown in Table 2. In diffusion model, the first step is the mass transfer of adsorbates molecule from the bulk solution to the adsorbent surface and second stage is the intraparticle diffusion on samples.Table 2
Liquid film diffusion model and Intraparticle diffusion constants for phosphate.
Samples
Q
e
,
exp (mg/g)
liquid film diffusion model
Intraparticle diffusion model
Q
e
,
cal (mg/g)
R (min-1)
R
2
S.D. (%)
C
K
3 (mg/gmin1/2)
R
2
S.D. (%)
C
3.58
3.34
0.508
0.905
16.22
1.70
0.271
0.770
25.52
BC-Fe
11.94
10.58
0.135
0.813
32.30
2.93
1.025
0.975
20.56Liquid film diffusion model is based on the theory proposed by Boyd et al. [61]. It was also used to identify the diffusion mechanism and find out which step is the rate-controlling step. According to this theory,
(5)log(1-F)=R2.303t,
where F represents the degree of exchange of adsorbate which was adsorbed onto the particles and can be described as Qt/Qe, R is a constant about the particle characters and it can be described as  R=3Dl/r0δk, Dl is the diffusion constant in the liquid, r0 is the radius of spherical adsorbent, δ is the thickness of liquid film, and k is distribution efficient.Normalized standard deviation (S.D.) (%) is used to find the most applicable model that could describe the kinetic study of adsorption of phosphate on samples A and B. The normalized standard deviation (S.D.) (%) was calculated using the following equation [62]:
(6)S.D.(%)=∑{[(Qt,exp-Qt,cal)/Qt,exp]2N-1},
where N is the number of data points, Qt,exp is the experimental values, and Qt,cal is the calculated value by the above four models, respectively. According to the values of S.D. (%) given in Tables 1 and 2, it is clear that pseudo-second-order equation is better in describing the adsorption kinetics of phosphate by samples BC and Fe-BC. And Fe-BC sample is better fitting intraparticle diffusion model than liquid film diffusion model while the carrier material BC shows the opposite result. However, the difference of S.D. values for liquid film diffusion model and Intra-particle diffusion model was not significant, indicating that both intra-particle diffusion and mass transfer were the rate controlling steps.


### 3.3. Adsorption Isotherm Models

Equilibrium adsorption curves of BC and Fe-BC are showed in Figure5. With the concentration of phosphate increasing, the equilibrium adsorption capacity Qe increased at the low concentration level and remained unchanged when the concentration is higher than a certain value.Figure 5
The adsorption capacity of phosphate onto samples BC and Fe-BC at variety initial concentration (T = 25°C, adsorbent dose = 1 g/L, and pH = 3).Langmuir and Freundlich isotherms were applied to describe the relationship between the amount of phosphate absorbed on absorbent and its equilibrium concentration in aqueous solution. The Langmuir and Freundlich equations were listed in Table3, where kl (L/mg) is Langmuir constants related to adsorption capacity and energy of adsorption and kf (mg/g) and n are the constants of the Freundlich isotherm that measure the adsorption capacity and intensity of adsorption, respectively. In Freundlich equation, 1/n values between 0 and 1 indicated a good adsorption.Table 3
Adsorption isotherm parameters of samples BC and Fe-BC.
Samples
Langmuir isotherm modelCe/Qe=1/(Qmaxkl) + Ce/Qmax
Freundlich isotherm modellgQe = lgkf + n-1lgCe
Q
max (mg/g)
k
l (L/mg)
R
2
k
f (mg/g) (L/mg)1/n
n
-
1
R
2
BC
15.44
0.038
0.978
1.628
0.484
0.943
Fe-BC
35.43
0.091
0.985
6.045
0.388
0.968The equilibrium adsorption data was analyzed using the Langmuir and Freundlich models. The estimated adsorption constants with corresponding correlation coefficients (R2) are summarized in Table 3. The results indicate that both models can be used to describe the adsorption isotherms, while the Langmuir model provides a better fitness than Freundlich model for phosphorus adsorption on BC absorbents. The maximum adsorption capacity obtained from Langmuir equation was 15.44 mg/g and 35.43 mg/g for BC and Fe-BC, respectively, indicating that incorporation of nanohydrous iron oxides into the biochar greatly increased the adsorption capacity for phosphate.As shown in Figure6, the XPS patters indicated that the iron oxides mainly exist in FeOOH forms. In addition, from XRD patters there is no fixed crystal, confirming that the iron oxides might be amorphous α-FeOOH, which is more active than other species [16]. Several signals of the iron oxide shell (peaks at 711.5 and 724.3 eV [63] for FeOOH) were observed. After adsorption, the banding energy of iron oxides is lower than before, and a new peak appeared at 712.8 eV [64], suggesting that a kind of iron oxide was formed during the adsorption process.Figure 6
Fe 2s XPS spectra of BC-Fe before and after phosphate adsorption.The significant increase of adsorption capacity for Fe-BC is probably due to the greater Lewis basicity of the FeOOH incorporated. The pH of the solution was maintained at 3.0, which was lower than the isoelectric point of FeOOH (8.7) [65], causing positively charged FeOOH surface. Therefore, it is not surprising that negative phosphate molecules are easily adsorbed on the Fe-BC surface at a low pH range due to strong electrostatic attraction between phosphate and FeOOH.To compare the phosphate adsorption capacity of the synthesized composite in this study, the phosphate adsorption parameters of several other waste materials at similar conditions are cited from literature as shown in Table4. It can be seen that the phosphate adsorption capacity of Fe-BC was fairly large and its adsorption rate and intensity are higher than most of other materials. Thus, the Fe-BC was a potentially adsorbent to remove phosphate from waste water for its high adsorption capacity and rate.Table 4
Phosphate adsorption parameters of different waste materials.
Materials
Adsorption capacity (mg/g)
k
l
k
f
n
-
1
Reference
Red mud
0.58
146.39
0.632
4.281
[38]
Wheat straw
2.81
0.008
0.044
1.087
[43]
ZnCl2-activated coir pith carbon
5.1
0.282
1.482
0.330
[41]
Zeolite
6.45
0.139
0.91
0.437
[59]
Peat
8.91
0.033
0.713
2.042
[44]
Nano Fe loaded BC
35.43
0.091
6.045
0.388
This study


## 3.1. Characterization of BC Samples

The BC sample with very high BET surface area (434.7 m2/g) and narrow pore size distribution (Figure 1), its average pore diameter is about 3.5 nm. It may provide very good adsorption capacity and modified potentialities. The loaded treatment may decrease the BET surface area of composite which is only 18.71 m2/g. As suggested, the preloaded nano-Fe particles would block some inner pores or make the pores narrower. Similar result was also reported by Shi concerning the effect of Fe(III) loadings on the pore volume and surface area of the resulting hybrid [58]. The mass of Fe in hybrid treated by FeCl4- is about 4.53%. And the curve of average pore diameter performs a bimodal distribution, which means that the loaded treatment changed the structure and property. Incorporation of nano-Fe into BC also altered its surface and textural morphology as shown by the SEM images in Figure 2. With different magnification (×600 and ×3000), different surface and structure can be seen clearly. The more irregular fragmented structure and pore structure of BC sample may contribute to its high surface area and pore volume.Figure 1
The pore size distribution of samples BC and Fe-BC.Figure 2
SEM images of samples BC and Fe-BC.As shown in Figure3, there are no obvious peaks in the XRD patters which indicated that the iron oxides in the samples existed as amorphous state.Figure 3
XRD diffraction pattern of BC and Fe-BC.


## 3.2. Adsorption Kinetics

The adsorption kinetics curves of phosphate adsorption on BC and Fe-BC are shown in Figure4, which may reflect the differences of adsorption rates and their rate control steps. The adsorption curves of BC and Fe-BC go as the same tendency; they rise sharply at the first 5 min and tend to be gentle after 60 and 120 min, respectively, which means that the adsorption speed is not constant during the whole process and the adsorption equilibrium time on BC is shorter than that on Fe-BC. But the y value of BC at the equilibrium condition is lower than that of Fe-BC, indicating that the adsorption capacity of BC is lower than Fe-BC.Figure 4
The variation of adsorption capacity with adsorption time for phosphate on samples BC and Fe-BC (T = 25°C; adsorbent dose = 1 g/L; phosphate concentration = 20 mg/L, and pH = 3).Four kinetic models were adopted to describe the adsorption process. The pseudo-first-order kinetic model has been widely used to predict sorption kinetics. The adsorption rate is proportional to the concentration of adsorbate. It can be used to describe the simple surface physical absorption. The model is defined as(2)ln(Qe-Qt)=lnQe-k1t.The pseudo-second-order equation assumed that the adsorption mechanism was dominant by chemisorption. The adsorption rate is proportional to square of adsorbate concentration. The pseudo-second-order equation can be expressed as(3)tQt=1k2Qe2+tQe,
where k1 (min−1) and k2 are the pseudo-first-order rate constant and the pseudo-second-order rate constant, respectively, reflecting the adsorption rate change along with the concentration change. The results are showed in Table 1.Table 1
Pseudo-first-order and Pseudo-second-order adsorption kinetic constants of samples BC and Fe-BC.
Samples
Q
e
,
exp (mg/g)
Pseudo-first-order model
Pseudo-second-order model
Q
e
,
cal (mg/g)
k
1 (min-1)
R
2
S.D. (%)
Q
e
,
cal (mg/g)
k
2 (gmg-1min−1)
R
2
S.D. (%)
BC
3.58
3.34
0.508
0.905
16.22
3.52
0.211
0.967
9.51
Fe-BC
11.94
10.58
0.135
0.813
32.30
11.31
0.019
0.905
24.24Compared with pseudo-second-order kinetic, the experimentalQe,exp values of first-order kinetic do not well agree with the calculated Qe,cal values obtained from the curve plots, suggesting that the adsorption process is not maintained by simple surface physical absorption, and some other adsorption mechanisms were involved.Generally, the process of the adsorbate adsorbed by adsorbent can be divided into four steps: firstly, adsorbate molecules transferred to the nearby adsorbent from solution; secondly, adsorbate molecules diffusion through the liquid film up to the surface of absorbent particles, this step usually was called external diffusion or mass transfer; thirdly, adsorbate molecules diffused through the absorbent particles and reached the inner side; this step is usually called intraparticle diffusion or diffusion; Fourthly, adsorbate molecules were attracted at the active sites in the interior of the particles. Step one and four were not the rate-controlling steps due to their happening so fast. And the kinetics of the adsorption will be governed either by diffusion or by a mass transfer mechanism depending on which of the above steps is the slowest. Hence, in this study, two models were investigated to find out the rate-controlling step of the adsorption process.Intraparticle diffusion model is based on the theory proposed by Weber and Morris [60]. It was used to identify the diffusion mechanism. According to this theory,
(4)Qt=k3t+C,
where k3 is the intra-particular diffusion rate constant (mg g−1 min−1/2). If intraparticle diffusion is rate-limited, the plots of adsorbates uptake Qt versus the square root of time (t1/2) would result in a linear relationship. k3 and C values can be obtained from these plots.The result ofQt versus t1/2 is shown in Table 2. In diffusion model, the first step is the mass transfer of adsorbates molecule from the bulk solution to the adsorbent surface and second stage is the intraparticle diffusion on samples.Table 2
Liquid film diffusion model and Intraparticle diffusion constants for phosphate.
Samples
Q
e
,
exp (mg/g)
liquid film diffusion model
Intraparticle diffusion model
Q
e
,
cal (mg/g)
R (min-1)
R
2
S.D. (%)
C
K
3 (mg/gmin1/2)
R
2
S.D. (%)
C
3.58
3.34
0.508
0.905
16.22
1.70
0.271
0.770
25.52
BC-Fe
11.94
10.58
0.135
0.813
32.30
2.93
1.025
0.975
20.56Liquid film diffusion model is based on the theory proposed by Boyd et al. [61]. It was also used to identify the diffusion mechanism and find out which step is the rate-controlling step. According to this theory,
(5)log(1-F)=R2.303t,
where F represents the degree of exchange of adsorbate which was adsorbed onto the particles and can be described as Qt/Qe, R is a constant about the particle characters and it can be described as  R=3Dl/r0δk, Dl is the diffusion constant in the liquid, r0 is the radius of spherical adsorbent, δ is the thickness of liquid film, and k is distribution efficient.Normalized standard deviation (S.D.) (%) is used to find the most applicable model that could describe the kinetic study of adsorption of phosphate on samples A and B. The normalized standard deviation (S.D.) (%) was calculated using the following equation [62]:
(6)S.D.(%)=∑{[(Qt,exp-Qt,cal)/Qt,exp]2N-1},
where N is the number of data points, Qt,exp is the experimental values, and Qt,cal is the calculated value by the above four models, respectively. According to the values of S.D. (%) given in Tables 1 and 2, it is clear that pseudo-second-order equation is better in describing the adsorption kinetics of phosphate by samples BC and Fe-BC. And Fe-BC sample is better fitting intraparticle diffusion model than liquid film diffusion model while the carrier material BC shows the opposite result. However, the difference of S.D. values for liquid film diffusion model and Intra-particle diffusion model was not significant, indicating that both intra-particle diffusion and mass transfer were the rate controlling steps.


## 3.3. Adsorption Isotherm Models

Equilibrium adsorption curves of BC and Fe-BC are showed in Figure5. With the concentration of phosphate increasing, the equilibrium adsorption capacity Qe increased at the low concentration level and remained unchanged when the concentration is higher than a certain value.Figure 5
The adsorption capacity of phosphate onto samples BC and Fe-BC at variety initial concentration (T = 25°C, adsorbent dose = 1 g/L, and pH = 3).Langmuir and Freundlich isotherms were applied to describe the relationship between the amount of phosphate absorbed on absorbent and its equilibrium concentration in aqueous solution. The Langmuir and Freundlich equations were listed in Table3, where kl (L/mg) is Langmuir constants related to adsorption capacity and energy of adsorption and kf (mg/g) and n are the constants of the Freundlich isotherm that measure the adsorption capacity and intensity of adsorption, respectively. In Freundlich equation, 1/n values between 0 and 1 indicated a good adsorption.Table 3
Adsorption isotherm parameters of samples BC and Fe-BC.
Samples
Langmuir isotherm modelCe/Qe=1/(Qmaxkl) + Ce/Qmax
Freundlich isotherm modellgQe = lgkf + n-1lgCe
Q
max (mg/g)
k
l (L/mg)
R
2
k
f (mg/g) (L/mg)1/n
n
-
1
R
2
BC
15.44
0.038
0.978
1.628
0.484
0.943
Fe-BC
35.43
0.091
0.985
6.045
0.388
0.968The equilibrium adsorption data was analyzed using the Langmuir and Freundlich models. The estimated adsorption constants with corresponding correlation coefficients (R2) are summarized in Table 3. The results indicate that both models can be used to describe the adsorption isotherms, while the Langmuir model provides a better fitness than Freundlich model for phosphorus adsorption on BC absorbents. The maximum adsorption capacity obtained from Langmuir equation was 15.44 mg/g and 35.43 mg/g for BC and Fe-BC, respectively, indicating that incorporation of nanohydrous iron oxides into the biochar greatly increased the adsorption capacity for phosphate.As shown in Figure6, the XPS patters indicated that the iron oxides mainly exist in FeOOH forms. In addition, from XRD patters there is no fixed crystal, confirming that the iron oxides might be amorphous α-FeOOH, which is more active than other species [16]. Several signals of the iron oxide shell (peaks at 711.5 and 724.3 eV [63] for FeOOH) were observed. After adsorption, the banding energy of iron oxides is lower than before, and a new peak appeared at 712.8 eV [64], suggesting that a kind of iron oxide was formed during the adsorption process.Figure 6
Fe 2s XPS spectra of BC-Fe before and after phosphate adsorption.The significant increase of adsorption capacity for Fe-BC is probably due to the greater Lewis basicity of the FeOOH incorporated. The pH of the solution was maintained at 3.0, which was lower than the isoelectric point of FeOOH (8.7) [65], causing positively charged FeOOH surface. Therefore, it is not surprising that negative phosphate molecules are easily adsorbed on the Fe-BC surface at a low pH range due to strong electrostatic attraction between phosphate and FeOOH.To compare the phosphate adsorption capacity of the synthesized composite in this study, the phosphate adsorption parameters of several other waste materials at similar conditions are cited from literature as shown in Table4. It can be seen that the phosphate adsorption capacity of Fe-BC was fairly large and its adsorption rate and intensity are higher than most of other materials. Thus, the Fe-BC was a potentially adsorbent to remove phosphate from waste water for its high adsorption capacity and rate.Table 4
Phosphate adsorption parameters of different waste materials.
Materials
Adsorption capacity (mg/g)
k
l
k
f
n
-
1
Reference
Red mud
0.58
146.39
0.632
4.281
[38]
Wheat straw
2.81
0.008
0.044
1.087
[43]
ZnCl2-activated coir pith carbon
5.1
0.282
1.482
0.330
[41]
Zeolite
6.45
0.139
0.91
0.437
[59]
Peat
8.91
0.033
0.713
2.042
[44]
Nano Fe loaded BC
35.43
0.091
6.045
0.388
This study


## 4. Conclusions

The findings of this work indicated that the new iron-containing BC material Fe-BC had great adsorption of phosphate ions. Adsorption fitted better to Langmuir isotherms than to Freundlich isotherm and the maximum phosphate adsorption for Fe-BC was found to be 35.43 mg/g at 25°C which is approximately 2.3 times of BC. Kinetic data were well fit to a pseudo-second-order model and intraparticle diffusion model. The as-prepared Fe-BC is found to be effective adsorbent for the removal of phosphate from aqueous solutions because of its unique hierarchical porous structure and the greater Lewis basicity of theα-FeOOH. This indicated that it is a potential adsorbent material for water treatment.



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*Source: 649868-2013-11-27.xml*