# Removing and Recovering Phosphate from Poultry Wastewater Using Amorphous Ceramics

Authors: Youhui Xie; Qin Li; Xianzhi Zhao; Yi Luo; Yangming Wang; Xiangwei Peng; Qigui Wang; Jian Su; Yin Lu
Journal: Journal of Chemistry
 (2014)

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## Abstract

A novel and effective technique for phosphate from poultry wastewater was developed using amorphous ceramics. Amorphous ceramics, which showed high performance for phosphate removal and recovery from poultry wastewater, were synthesized using unlimitedly available, inexpensive materials such as silica fume and lime. Dissolved phosphate in poultry wastewater can be deposited as a solid on the surface of amorphous ceramics. Phosphate content on the surface of amorphous ceramics could reach 14.20%. The phosphate removal and recovery process and mechanism was revealed by a series of characterizations, such as XRD, FESEM, BET, and so on. The present study demonstrated that amorphous ceramics have great potential as a novel, beneficial material for removing and recovering phosphate from poultry wastewater.


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## Body

## 1. Introduction

The pollution caused by livestock and poultry breeding is not only a local environmental problem, but also a big basin environmental issue [1, 2]. Especially, high concentration of phosphate discharged from poultry wastewater was one of the main incentives of eutrophication [3, 4]. Therefore, removing phosphate from poultry wastewater has been the present research hotspot [5–7].According to the supersaturation theory, when the concentration of Ca2+, OH−, and phosphate ion reaches saturation state, phosphate can be deposited in the form of calcium orthophosphate on the surface of crystal seed [8, 9]. Previous studies showed that calcium silicate hydrate can be used as the crystal seed [10–13]. And the phosphate recovery efficiency of calcium silicate hydrate was about 13% according to the existing research [14, 15]. The crystallization process could remove phosphate in wastewater by producing calcium orthophosphate on the surface of granular seed crystal [16–18]. This process possesses the advantages of easy dewatering and potential phosphate recycling for the product. Due to the unique chemical composition of amorphous ceramics, it could ensure the efficient removal and the recovery of soluble phosphate [19]. From a theoretical and practical point of view, micromorphology of amorphous ceramics was also important for increasing reaction rate of phosphate recovery [20]. This critical issue has not yet been sufficiently solved so far. Overall, the goal of this study was to define the micromorphology properties and to optimize the influence conditions for amorphous ceramics to remove and recover phosphate.Laboratory experiments were carried out to investigate the key features of the removing and recovering process. Theoretical analysis and experimental evidences were also provided to demonstrate the underlying principles of crystallization and mechanism of the process. The originality and importance that can be drawn from this study are summarized, such as examining the effects of pH value, stirring intensity and dosage of amorphous ceramics on the phosphate removal and recovery efficiency. Then, cycling phosphate removal experiments were performed to evaluate the phosphate recovery performance of amorphous ceramics. The applicability of the phosphate recovery system using amorphous ceramics as a seed crystal was also examined. At last, by using Avrami kinetics equation, the capacity of Ca2+ release and the pore structure of amorphous ceramics were determined. The mechanism of phosphate recovery by amorphous ceramics as seed crystal on the condition of weak alkaline was also revealed.


## 2. Materials and Methods

### 2.1. Materials

Amorphous ceramics were synthesized using silica fume as the silicon oxide materials and lime as calcium oxide materials, respectively. Lime (calcareous, hoar and powdery, Chongqing Changshou Chemical Co., Ltd.) was calcined at 700°C for 2 h. The chemical constituents of silica fume (Particles present spherical with homogeneous diameter, Chongqing Jianfeng chemical Co., Ltd.) and lime are in Table1. The phosphate solution was poultry wastewater. The phosphate concentration of poultry wastewater was 40 mg/L, and pH value was 7.0~7.5. The above materials and chemicals were placed into sealed bottles for storage.Table 1
Chemical components of silica fume and lime.
Chemical components (contents)/%
CaO
SiO2
Al2O3
SO2
MgO
Fe2O3
NaOH
CuO
H2O
Lime
79.60
3.35
2.36
1.18
0.66
0.17
—
—
12.68
Silica fume
0.04
97.50
0.15
1.83
—
0.02
0.30
0.01
0.15


### 2.2. Preparation of Amorphous Ceramics

Amorphous ceramics were prepared with lime (providing CaO) and silica fume (providing SiO2). Lime and silica fume were mixed with a molar ratio of 1.5~1.6. The mixture was then added to prepared slurries. The slurry was hydrothermal reacted at 165~170°C for 6 h and taken out when the temperature was reduced to the natural conditions. The hydrothermal reaction was carried out with a liquid/solid ratio of 29~30. The obtained products were dried at 105°C for 2 h and then were ground through a sieve of 200 meshes.


### 2.3. Phosphate Removal and Recovery Using Amorphous Ceramics

The pH values of phosphate-content solution were in the range of 7.0–7.5 before the amorphous ceramics samples were added to this solution. The experiment temperature condition is 20°C. Continuous phosphate removal tests were carried out using amorphous ceramics for the removal of phosphate from poultry wastewater. Amorphous ceramics samples (dosage of samples 0.5, 1.0, 2.0, 3.0, and 4.0 g/L, resp.) were added to a series of bottles and stirring (40, 60 80, 100, and 120 r/min, resp.) under controlled temperature conditions (20°C). Phosphate concentration of supernatant was measured according to the molybdenum blue ascorbic acid method (the relative error of data is 0.3%) with a spectrophotometer (UV-2012PCS, Shanghai Unico Instruments Co., Ltd., China). The solid samples were then separated from the removed synthetic solution with the addition of samples after reaction. Finally, the produced sediments were separated from removed synthetic solution, dried, and weighted. Phosphate is contented by (1), where Ct is the restrained phosphate concentration in synthetic solution (mg/L), v is the volume of the solution (L), w is the mass of produced sediment after phosphate recovery (mg), and C0 is the initial phosphate concentration (mg/L):
(1)P=(c0-ct)×vw×100%.


### 2.4. Ca2+ Release Experimental of Amorphous Ceramics

1 g of amorphous ceramics samples was immersed in 1 L of demonized water contained in a glass bottle, generating samples with a solution concentration of 1 g/L. The bottle was placed on an agitation table and shaken at 40 r/min under controlled temperature conditions (20°C). Samples of solution were taken after 5, 10, 15, 20, 40, and 60 min of agitation. Ca2+ concentration of samples was determined by EDTA titration (the relative error of data is 0.05%).


### 2.5. Characterization Methods

X-ray diffraction (XRD) patterns were collected in an XD-2 instrument (Persee, China) using Cu Kα radiation.Field emission scanning electron microscopy (FESEM) images were collected on an S-4800 field emission scanning electron microscope (Hitachi, Japan).Brunauer-Emmett-Teller (BET) surface areas were measured by nitrogen adsorption at 77.35 K on an ASAP-2010 adsorption apparatus (Micromeritics, USA).


## 2.1. Materials

Amorphous ceramics were synthesized using silica fume as the silicon oxide materials and lime as calcium oxide materials, respectively. Lime (calcareous, hoar and powdery, Chongqing Changshou Chemical Co., Ltd.) was calcined at 700°C for 2 h. The chemical constituents of silica fume (Particles present spherical with homogeneous diameter, Chongqing Jianfeng chemical Co., Ltd.) and lime are in Table1. The phosphate solution was poultry wastewater. The phosphate concentration of poultry wastewater was 40 mg/L, and pH value was 7.0~7.5. The above materials and chemicals were placed into sealed bottles for storage.Table 1
Chemical components of silica fume and lime.
Chemical components (contents)/%
CaO
SiO2
Al2O3
SO2
MgO
Fe2O3
NaOH
CuO
H2O
Lime
79.60
3.35
2.36
1.18
0.66
0.17
—
—
12.68
Silica fume
0.04
97.50
0.15
1.83
—
0.02
0.30
0.01
0.15


## 2.2. Preparation of Amorphous Ceramics

Amorphous ceramics were prepared with lime (providing CaO) and silica fume (providing SiO2). Lime and silica fume were mixed with a molar ratio of 1.5~1.6. The mixture was then added to prepared slurries. The slurry was hydrothermal reacted at 165~170°C for 6 h and taken out when the temperature was reduced to the natural conditions. The hydrothermal reaction was carried out with a liquid/solid ratio of 29~30. The obtained products were dried at 105°C for 2 h and then were ground through a sieve of 200 meshes.


## 2.3. Phosphate Removal and Recovery Using Amorphous Ceramics

The pH values of phosphate-content solution were in the range of 7.0–7.5 before the amorphous ceramics samples were added to this solution. The experiment temperature condition is 20°C. Continuous phosphate removal tests were carried out using amorphous ceramics for the removal of phosphate from poultry wastewater. Amorphous ceramics samples (dosage of samples 0.5, 1.0, 2.0, 3.0, and 4.0 g/L, resp.) were added to a series of bottles and stirring (40, 60 80, 100, and 120 r/min, resp.) under controlled temperature conditions (20°C). Phosphate concentration of supernatant was measured according to the molybdenum blue ascorbic acid method (the relative error of data is 0.3%) with a spectrophotometer (UV-2012PCS, Shanghai Unico Instruments Co., Ltd., China). The solid samples were then separated from the removed synthetic solution with the addition of samples after reaction. Finally, the produced sediments were separated from removed synthetic solution, dried, and weighted. Phosphate is contented by (1), where Ct is the restrained phosphate concentration in synthetic solution (mg/L), v is the volume of the solution (L), w is the mass of produced sediment after phosphate recovery (mg), and C0 is the initial phosphate concentration (mg/L):
(1)P=(c0-ct)×vw×100%.


## 2.4. Ca2+ Release Experimental of Amorphous Ceramics

1 g of amorphous ceramics samples was immersed in 1 L of demonized water contained in a glass bottle, generating samples with a solution concentration of 1 g/L. The bottle was placed on an agitation table and shaken at 40 r/min under controlled temperature conditions (20°C). Samples of solution were taken after 5, 10, 15, 20, 40, and 60 min of agitation. Ca2+ concentration of samples was determined by EDTA titration (the relative error of data is 0.05%).


## 2.5. Characterization Methods

X-ray diffraction (XRD) patterns were collected in an XD-2 instrument (Persee, China) using Cu Kα radiation.Field emission scanning electron microscopy (FESEM) images were collected on an S-4800 field emission scanning electron microscope (Hitachi, Japan).Brunauer-Emmett-Teller (BET) surface areas were measured by nitrogen adsorption at 77.35 K on an ASAP-2010 adsorption apparatus (Micromeritics, USA).


## 3. Results and Discussion

### 3.1. Phase Structure of Amorphous Ceramics

The XRD patterns of amorphous ceramics before phosphate removal, phosphate removal for the first time, and phosphate removal for 6 times were compared (Figure1). The main phase of amorphous ceramics was Jennite (PDF card 18-1206, chemical formula Ca9Si6O18(OH)6·8H2O). After phosphate removal for the first time, the dominant peaks of Jennite were obviously weakened, and the weak peaks of calcium orthophosphate (PDF card 09-0432, chemical formula Ca5(PO4)3(OH)) emerged at 25.88°, 31.76°, and 53.26°. The sharp dominant peaks of calcium orthophosphate appeared after phosphate removal for 6 times instead of the dominant peaks of Jennite. This phenomenon indicated that original property of amorphous ceramics seed crystal disappeared and transformed to calcium orthophosphate during the phosphate recovery process.Figure 1
XRD patterns of samples.


### 3.2. BET Surface Areas and Pore Structure of Amorphous Ceramics

Nitrogen adsorption-desorption isotherms of amorphous ceramics before and after phosphate removal are shown in Figure2. The specific surface areas of these samples were 114.14, 57.38, 34.25, 23.74, and 7.55 m2/g, respectively. Pore volumes of these samples were 0.52, 0.31, 0.12, 0.09, and 0.04 cm3/g, respectively. These results indicated that the specific surface areas and pore volumes decreased with the increase of phosphate removal times. Figure 2 shows the phenomenon of adsorption hysteresis loop. This implies that mesopore or narrow gap pore exists in the samples. Adsorption in mesopore occurred mainly in medium pressure region (0.4 < P/P0 < 0.9) [21, 22]. The phenomenon of adsorption hysteresis loop disappeared gradually with the increased phosphate removal times. The FESEM photographs of amorphous ceramics before and after removing phosphate are shown in Figure 3. Before phosphate removal, amorphous ceramics possess obvious porous structure with a large number of mesopores (Figure 3(a)). The micrograph in Figure 3(b) reveals that amorphous ceramics are covered with finely distributed crystalline substances, which was calcium orthophosphate as indicated in XRD result.Figure 2
Nitrogen adsorption-desorption isotherms of amorphous ceramics before and after removing phosphate.FESEM photographs of amorphous ceramics before and at the 6th time phosphate removal. (a) Amorphous ceramics before phosphate removal. (b) Amorphous ceramics of the 6th time phosphate removal.
(a)
(b)


### 3.3. Kinetic of Ca2+ Release

The effect of phosphate removal for the first 4 times on the Ca2+ release capacity of amorphous ceramics was investigated (Figure 4). Ca2+ concentration released from amorphous ceramics decreased with the increase of phosphate removal times. The maximum Ca2+ concentration released from amorphous ceramics was 3.02 mg/g before phosphate removal. This concentration decreased to 1 mg/g after phosphate removal for 4 times. Avrami kinetic equation could describe how the solid change from one phase state to another (that means phase transition), which could also describe the chemical reaction rate [23]. So, the experimental capacities of Ca2+ release could be fitted by Avrami kinetic equation; the model is as follows:
(2)-ln⁡(1-x)=ktn,
where k is the kinetic constant, n is the characteristic constant of solid, t is the reaction time (min), and x (x=Ct/Cmax⁡, Ct is concentration of time t (mg/L), and Cmax⁡ is concentration of the maximum (mg/L)) is the fraction conversion. The characteristic constant n was 0.9156. The kinetic constants were determined by fitting the Avrami kinetic equation to the experimental data obtained (Table 2).Table 2
The correlate constants for the Avrami kinetic equation describing Ca2+ release.
Samples
n
k
R
2
Before  phosphate removal
0.9156
0.0758
0.9893
Once  phosphate removal
0.9204
0.0682
0.9752
Twice  phosphate removal
0.9182
0.0602
0.9790
3rd time phosphate removal
0.8687
0.0564
0.9548
4th time phosphate removal
0.9913
0.0301
0.9836Figure 4
Concentration of Ca2+ released from samples.The high correlation coefficients (R2>0.9) indicated that this model could well describe the law of Ca2+ release. Combined with specific surface area (S) of samples, a relationship between k and S could be established:
(3)k=0.1502S0.3695R2=0.9232.According to (3), the larger surface area of amorphous ceramics could result in faster Ca2+ release. Subsequently, the concentration of Ca2+ release increased.


### 3.4. Phosphate Removal with Amorphous Ceramics

#### 3.4.1. Effect of pH Values

The effect of pH values on the phosphate ions removal performance was investigated with the initial phosphate concentration 40 mg/L (Figure5). The results in Figure 5 show that pH value has an obvious effect on the residual phosphate concentration. The residual phosphate concentration was up to 7.7~9.1 mg/L when the pH values were in the range of 4.0~7.0. In this range of pH values, the solution has not reached supersaturation with Ca2+, OH−, and phosphate ions coexisted. Under this condition, amorphous ceramics did not possess phosphate removal performance. At the pH value of 8.0, the residual phosphate concentration declined to 4.34 mg/L. When the pH value reached to 9.0, the phosphate removal performance of amorphous ceramics increased obviously, and the residual phosphate concentration declined to the minimum of 0.82 mg/L. Phosphate existed in the form of HPO42- in the range of 8.0~9.0 [24]. The residual phosphate concentration increased with the pH values increasing continuously. So, the kinetic models of phosphate removal were established at pH value of 9.0. This reaction is accorded with the tendency of second order reaction kinetics, and the kinetic equation could be established:
(4)dCdt=-kC2
or
(5)1Ct-1C0=kt,
where Ct is the concentration of time t(mg/L), C0 is the initial time, and k is the kinetic constant.Figure 5
Influence of pH value on residual phosphate concentration.


#### 3.4.2. Kinetic of Phosphate Removal

With the pH value unchanged, initial phosphate concentration, stirring intensity, and amorphous ceramics dosage have been predicted as the major factors influencing the phosphate removal rate by calcium orthophosphate crystallization. Hence, the overall rate constantk in (6) is likely to be a function of stirring intensity and amorphous ceramics dosage,
(6)k=f(M,I)=aMbIc,
where b, c, and d were constants and M and I were amorphous ceramics dosage and stirring intensity, respectively.The effect of amorphous ceramics dosage on the removal of phosphate was investigated at amorphous ceramics dosages range of 0.5, 1, 2, 3, and 4 g/L, respectively (Figure6). As shown in Figure 6, when the dosages were in the range of 1~4 g/L, the residue phosphate concentration kept unchanged with 4~5 mg/L. The residue phosphate concentration rose to 9.45 mg/L when the dosage was as low as 0.5 g/L. This result was inconsistent with the conclusion of traditional coagulation precipitation experiment. In the traditional experiment, the removal of phosphate could be better with the increase of dosages of calcium. This is because the removal efficiency of phosphate was much dependent on the alkalinity caused by excess calcium, and the malpractice of this traditional method is reducing the utilization efficiency of calcium. Considering the effective utilization rate from seed, 1 g/L is the proper dosages. The reaction rate of phosphate removal increased with the increase of dosage, and the relationship could be fitted as follows:
(7)k=0.0003M1.3865R2=0.9453.Figure 6
Influence of dosage of amorphous ceramics.Under pH value of 9.0, amorphous ceramics dosage of 1 g/L, the results showed that the residual phosphate concentration declined with the increase of stirring intensity when the stirring intensity was lower than 80 r/min. When the stirring intensity reached 80 r/min, the residual phosphate concentration declined to minimum (Figure7). According to Figure 7, stirring intensity has an obvious influence on the phosphate removal performance of amorphous ceramics. The reaction rate of phosphate removal increased with the increase of stirring intensity. The relationship could be fitted as follows:
(8)k=0.0004I0.4712R2=0.9247.Figure 7
Influence of stirring intensity on residual phosphate concentration.By comprehensive analysis of initial, amorphous ceramics dosage and stirring intensity, (4) could be expressed as follows:
(9)k=aM1.3865I0.4712.According to (7) and (9), the parameter a can be determined to be 0.0034. The kinetic model of phosphate removal could be established by taking the coefficient a into (5):
(10)1Ct=1C0+(0.0046M1.3865I0.4712)t.The phosphate recovery process is the calcium orthophosphate crystallization process on the surface of amorphous ceramics. When the stirring intensity is too low, amorphous ceramics cannot touch phosphate wastewater adequately. When the stirring intensity is too high, the calcium orthophosphate crystal cannot be formed due to the strong shearing force.


### 3.5. The Phosphate Recovery Performance of Amorphous Ceramics

According to (1) and (10), the kinetic model verified the experimental result of phosphate removal. Analysis from the view of phosphate recovery showed that the conditions such as the improvement of initial phosphate concentration, stirring intensity, and the decrease of dosage were beneficial for the improvement of phosphate content of solid segment. But the value of k was only 0.00007 when the amorphous ceramics dosage was 0.5 g/L. This reaction rate was too low to the engineering application. Thus, the proper dosage should be 1 g/L, and the reaction rate k was 0.0005. So, the proper process condition for phosphate recovery using amorphous ceramics is as follows: amorphous ceramics dosage of 1 g/L and stirring intensity of 80 r/min. To obtain the maximum efficiency of phosphate recovery continuous experiments were carried out using amorphous ceramics calculated for the removal of phosphate. Changes of residual phosphate concentration by circulation of phosphate removal were shown in Figure 8. For the first 4 times of phosphate removal, the restrained phosphate concentration was changed greatly. The restrained phosphate concentration almost remained stable when phosphate removal circulated for 6 times. The quality of solid segment was 1.08 g and the phosphate content of solid segment was 14.20% after the circulation of phosphate removal. The changes of pH values showed that amorphous ceramics could maintain the pH value between 8.0 and 9.0 at the first 4 times phosphate removal. Calcium phosphate had been crystallized on the surface of amorphous ceramics during the 6 times phosphate recovery process. Thus, BET surface areas and pore volume decreased. Due to the large BET surface areas and pore volume of amorphous ceramics, Ca2+ and OH− can be released continuously, and pH values increased. During the phosphate recovery process, phosphate sedimentation produced on the surface of amorphous ceramics to block the pore structure to restrain the release of Ca2+ and OH−. The pH values declined with the increased circulate times of phosphate removal. Subsequently, the phosphate removal performance of amorphous ceramics decreased. The pH value declined to 7.5 after the circulation of phosphate removal for 6 times. At this time, the restrained phosphate concentration was up to 95.47 mg/L, which indicated that amorphous ceramics did not possess phosphate removal capacity in neutral condition.Figure 8
Changes of residual phosphate concentration and pH values.Indeed, the phosphate recovery process is the form process of calcium orthophosphate, which is also different from the traditional chemical phosphate removal process. Because the traditional chemical phosphate removal process needs a high alkalinity (pH = 10.5~12.5) condition to make Ca2+, OH−, and PO43- reach supersaturated, the phosphate sedimentation precipitated would be produced. Under the proper process condition, amorphous ceramics could release a suitable concentration of Ca2+ and OH− to maintain the pH value during 8.0~9.0. Phosphate existed in the form of HPO42- in the range of these pH values. Ca2+, OH−, and HPO42- formed a local condition with high concentration. This condition was beneficial to the formation of calcium orthophosphate with pH = 8.0~9.0.


## 3.1. Phase Structure of Amorphous Ceramics

The XRD patterns of amorphous ceramics before phosphate removal, phosphate removal for the first time, and phosphate removal for 6 times were compared (Figure1). The main phase of amorphous ceramics was Jennite (PDF card 18-1206, chemical formula Ca9Si6O18(OH)6·8H2O). After phosphate removal for the first time, the dominant peaks of Jennite were obviously weakened, and the weak peaks of calcium orthophosphate (PDF card 09-0432, chemical formula Ca5(PO4)3(OH)) emerged at 25.88°, 31.76°, and 53.26°. The sharp dominant peaks of calcium orthophosphate appeared after phosphate removal for 6 times instead of the dominant peaks of Jennite. This phenomenon indicated that original property of amorphous ceramics seed crystal disappeared and transformed to calcium orthophosphate during the phosphate recovery process.Figure 1
XRD patterns of samples.


## 3.2. BET Surface Areas and Pore Structure of Amorphous Ceramics

Nitrogen adsorption-desorption isotherms of amorphous ceramics before and after phosphate removal are shown in Figure2. The specific surface areas of these samples were 114.14, 57.38, 34.25, 23.74, and 7.55 m2/g, respectively. Pore volumes of these samples were 0.52, 0.31, 0.12, 0.09, and 0.04 cm3/g, respectively. These results indicated that the specific surface areas and pore volumes decreased with the increase of phosphate removal times. Figure 2 shows the phenomenon of adsorption hysteresis loop. This implies that mesopore or narrow gap pore exists in the samples. Adsorption in mesopore occurred mainly in medium pressure region (0.4 < P/P0 < 0.9) [21, 22]. The phenomenon of adsorption hysteresis loop disappeared gradually with the increased phosphate removal times. The FESEM photographs of amorphous ceramics before and after removing phosphate are shown in Figure 3. Before phosphate removal, amorphous ceramics possess obvious porous structure with a large number of mesopores (Figure 3(a)). The micrograph in Figure 3(b) reveals that amorphous ceramics are covered with finely distributed crystalline substances, which was calcium orthophosphate as indicated in XRD result.Figure 2
Nitrogen adsorption-desorption isotherms of amorphous ceramics before and after removing phosphate.FESEM photographs of amorphous ceramics before and at the 6th time phosphate removal. (a) Amorphous ceramics before phosphate removal. (b) Amorphous ceramics of the 6th time phosphate removal.
(a)
(b)


## 3.3. Kinetic of Ca2+ Release

The effect of phosphate removal for the first 4 times on the Ca2+ release capacity of amorphous ceramics was investigated (Figure 4). Ca2+ concentration released from amorphous ceramics decreased with the increase of phosphate removal times. The maximum Ca2+ concentration released from amorphous ceramics was 3.02 mg/g before phosphate removal. This concentration decreased to 1 mg/g after phosphate removal for 4 times. Avrami kinetic equation could describe how the solid change from one phase state to another (that means phase transition), which could also describe the chemical reaction rate [23]. So, the experimental capacities of Ca2+ release could be fitted by Avrami kinetic equation; the model is as follows:
(2)-ln⁡(1-x)=ktn,
where k is the kinetic constant, n is the characteristic constant of solid, t is the reaction time (min), and x (x=Ct/Cmax⁡, Ct is concentration of time t (mg/L), and Cmax⁡ is concentration of the maximum (mg/L)) is the fraction conversion. The characteristic constant n was 0.9156. The kinetic constants were determined by fitting the Avrami kinetic equation to the experimental data obtained (Table 2).Table 2
The correlate constants for the Avrami kinetic equation describing Ca2+ release.
Samples
n
k
R
2
Before  phosphate removal
0.9156
0.0758
0.9893
Once  phosphate removal
0.9204
0.0682
0.9752
Twice  phosphate removal
0.9182
0.0602
0.9790
3rd time phosphate removal
0.8687
0.0564
0.9548
4th time phosphate removal
0.9913
0.0301
0.9836Figure 4
Concentration of Ca2+ released from samples.The high correlation coefficients (R2>0.9) indicated that this model could well describe the law of Ca2+ release. Combined with specific surface area (S) of samples, a relationship between k and S could be established:
(3)k=0.1502S0.3695R2=0.9232.According to (3), the larger surface area of amorphous ceramics could result in faster Ca2+ release. Subsequently, the concentration of Ca2+ release increased.


## 3.4. Phosphate Removal with Amorphous Ceramics

### 3.4.1. Effect of pH Values

The effect of pH values on the phosphate ions removal performance was investigated with the initial phosphate concentration 40 mg/L (Figure5). The results in Figure 5 show that pH value has an obvious effect on the residual phosphate concentration. The residual phosphate concentration was up to 7.7~9.1 mg/L when the pH values were in the range of 4.0~7.0. In this range of pH values, the solution has not reached supersaturation with Ca2+, OH−, and phosphate ions coexisted. Under this condition, amorphous ceramics did not possess phosphate removal performance. At the pH value of 8.0, the residual phosphate concentration declined to 4.34 mg/L. When the pH value reached to 9.0, the phosphate removal performance of amorphous ceramics increased obviously, and the residual phosphate concentration declined to the minimum of 0.82 mg/L. Phosphate existed in the form of HPO42- in the range of 8.0~9.0 [24]. The residual phosphate concentration increased with the pH values increasing continuously. So, the kinetic models of phosphate removal were established at pH value of 9.0. This reaction is accorded with the tendency of second order reaction kinetics, and the kinetic equation could be established:
(4)dCdt=-kC2
or
(5)1Ct-1C0=kt,
where Ct is the concentration of time t(mg/L), C0 is the initial time, and k is the kinetic constant.Figure 5
Influence of pH value on residual phosphate concentration.


### 3.4.2. Kinetic of Phosphate Removal

With the pH value unchanged, initial phosphate concentration, stirring intensity, and amorphous ceramics dosage have been predicted as the major factors influencing the phosphate removal rate by calcium orthophosphate crystallization. Hence, the overall rate constantk in (6) is likely to be a function of stirring intensity and amorphous ceramics dosage,
(6)k=f(M,I)=aMbIc,
where b, c, and d were constants and M and I were amorphous ceramics dosage and stirring intensity, respectively.The effect of amorphous ceramics dosage on the removal of phosphate was investigated at amorphous ceramics dosages range of 0.5, 1, 2, 3, and 4 g/L, respectively (Figure6). As shown in Figure 6, when the dosages were in the range of 1~4 g/L, the residue phosphate concentration kept unchanged with 4~5 mg/L. The residue phosphate concentration rose to 9.45 mg/L when the dosage was as low as 0.5 g/L. This result was inconsistent with the conclusion of traditional coagulation precipitation experiment. In the traditional experiment, the removal of phosphate could be better with the increase of dosages of calcium. This is because the removal efficiency of phosphate was much dependent on the alkalinity caused by excess calcium, and the malpractice of this traditional method is reducing the utilization efficiency of calcium. Considering the effective utilization rate from seed, 1 g/L is the proper dosages. The reaction rate of phosphate removal increased with the increase of dosage, and the relationship could be fitted as follows:
(7)k=0.0003M1.3865R2=0.9453.Figure 6
Influence of dosage of amorphous ceramics.Under pH value of 9.0, amorphous ceramics dosage of 1 g/L, the results showed that the residual phosphate concentration declined with the increase of stirring intensity when the stirring intensity was lower than 80 r/min. When the stirring intensity reached 80 r/min, the residual phosphate concentration declined to minimum (Figure7). According to Figure 7, stirring intensity has an obvious influence on the phosphate removal performance of amorphous ceramics. The reaction rate of phosphate removal increased with the increase of stirring intensity. The relationship could be fitted as follows:
(8)k=0.0004I0.4712R2=0.9247.Figure 7
Influence of stirring intensity on residual phosphate concentration.By comprehensive analysis of initial, amorphous ceramics dosage and stirring intensity, (4) could be expressed as follows:
(9)k=aM1.3865I0.4712.According to (7) and (9), the parameter a can be determined to be 0.0034. The kinetic model of phosphate removal could be established by taking the coefficient a into (5):
(10)1Ct=1C0+(0.0046M1.3865I0.4712)t.The phosphate recovery process is the calcium orthophosphate crystallization process on the surface of amorphous ceramics. When the stirring intensity is too low, amorphous ceramics cannot touch phosphate wastewater adequately. When the stirring intensity is too high, the calcium orthophosphate crystal cannot be formed due to the strong shearing force.


## 3.4.1. Effect of pH Values

The effect of pH values on the phosphate ions removal performance was investigated with the initial phosphate concentration 40 mg/L (Figure5). The results in Figure 5 show that pH value has an obvious effect on the residual phosphate concentration. The residual phosphate concentration was up to 7.7~9.1 mg/L when the pH values were in the range of 4.0~7.0. In this range of pH values, the solution has not reached supersaturation with Ca2+, OH−, and phosphate ions coexisted. Under this condition, amorphous ceramics did not possess phosphate removal performance. At the pH value of 8.0, the residual phosphate concentration declined to 4.34 mg/L. When the pH value reached to 9.0, the phosphate removal performance of amorphous ceramics increased obviously, and the residual phosphate concentration declined to the minimum of 0.82 mg/L. Phosphate existed in the form of HPO42- in the range of 8.0~9.0 [24]. The residual phosphate concentration increased with the pH values increasing continuously. So, the kinetic models of phosphate removal were established at pH value of 9.0. This reaction is accorded with the tendency of second order reaction kinetics, and the kinetic equation could be established:
(4)dCdt=-kC2
or
(5)1Ct-1C0=kt,
where Ct is the concentration of time t(mg/L), C0 is the initial time, and k is the kinetic constant.Figure 5
Influence of pH value on residual phosphate concentration.


## 3.4.2. Kinetic of Phosphate Removal

With the pH value unchanged, initial phosphate concentration, stirring intensity, and amorphous ceramics dosage have been predicted as the major factors influencing the phosphate removal rate by calcium orthophosphate crystallization. Hence, the overall rate constantk in (6) is likely to be a function of stirring intensity and amorphous ceramics dosage,
(6)k=f(M,I)=aMbIc,
where b, c, and d were constants and M and I were amorphous ceramics dosage and stirring intensity, respectively.The effect of amorphous ceramics dosage on the removal of phosphate was investigated at amorphous ceramics dosages range of 0.5, 1, 2, 3, and 4 g/L, respectively (Figure6). As shown in Figure 6, when the dosages were in the range of 1~4 g/L, the residue phosphate concentration kept unchanged with 4~5 mg/L. The residue phosphate concentration rose to 9.45 mg/L when the dosage was as low as 0.5 g/L. This result was inconsistent with the conclusion of traditional coagulation precipitation experiment. In the traditional experiment, the removal of phosphate could be better with the increase of dosages of calcium. This is because the removal efficiency of phosphate was much dependent on the alkalinity caused by excess calcium, and the malpractice of this traditional method is reducing the utilization efficiency of calcium. Considering the effective utilization rate from seed, 1 g/L is the proper dosages. The reaction rate of phosphate removal increased with the increase of dosage, and the relationship could be fitted as follows:
(7)k=0.0003M1.3865R2=0.9453.Figure 6
Influence of dosage of amorphous ceramics.Under pH value of 9.0, amorphous ceramics dosage of 1 g/L, the results showed that the residual phosphate concentration declined with the increase of stirring intensity when the stirring intensity was lower than 80 r/min. When the stirring intensity reached 80 r/min, the residual phosphate concentration declined to minimum (Figure7). According to Figure 7, stirring intensity has an obvious influence on the phosphate removal performance of amorphous ceramics. The reaction rate of phosphate removal increased with the increase of stirring intensity. The relationship could be fitted as follows:
(8)k=0.0004I0.4712R2=0.9247.Figure 7
Influence of stirring intensity on residual phosphate concentration.By comprehensive analysis of initial, amorphous ceramics dosage and stirring intensity, (4) could be expressed as follows:
(9)k=aM1.3865I0.4712.According to (7) and (9), the parameter a can be determined to be 0.0034. The kinetic model of phosphate removal could be established by taking the coefficient a into (5):
(10)1Ct=1C0+(0.0046M1.3865I0.4712)t.The phosphate recovery process is the calcium orthophosphate crystallization process on the surface of amorphous ceramics. When the stirring intensity is too low, amorphous ceramics cannot touch phosphate wastewater adequately. When the stirring intensity is too high, the calcium orthophosphate crystal cannot be formed due to the strong shearing force.


## 3.5. The Phosphate Recovery Performance of Amorphous Ceramics

According to (1) and (10), the kinetic model verified the experimental result of phosphate removal. Analysis from the view of phosphate recovery showed that the conditions such as the improvement of initial phosphate concentration, stirring intensity, and the decrease of dosage were beneficial for the improvement of phosphate content of solid segment. But the value of k was only 0.00007 when the amorphous ceramics dosage was 0.5 g/L. This reaction rate was too low to the engineering application. Thus, the proper dosage should be 1 g/L, and the reaction rate k was 0.0005. So, the proper process condition for phosphate recovery using amorphous ceramics is as follows: amorphous ceramics dosage of 1 g/L and stirring intensity of 80 r/min. To obtain the maximum efficiency of phosphate recovery continuous experiments were carried out using amorphous ceramics calculated for the removal of phosphate. Changes of residual phosphate concentration by circulation of phosphate removal were shown in Figure 8. For the first 4 times of phosphate removal, the restrained phosphate concentration was changed greatly. The restrained phosphate concentration almost remained stable when phosphate removal circulated for 6 times. The quality of solid segment was 1.08 g and the phosphate content of solid segment was 14.20% after the circulation of phosphate removal. The changes of pH values showed that amorphous ceramics could maintain the pH value between 8.0 and 9.0 at the first 4 times phosphate removal. Calcium phosphate had been crystallized on the surface of amorphous ceramics during the 6 times phosphate recovery process. Thus, BET surface areas and pore volume decreased. Due to the large BET surface areas and pore volume of amorphous ceramics, Ca2+ and OH− can be released continuously, and pH values increased. During the phosphate recovery process, phosphate sedimentation produced on the surface of amorphous ceramics to block the pore structure to restrain the release of Ca2+ and OH−. The pH values declined with the increased circulate times of phosphate removal. Subsequently, the phosphate removal performance of amorphous ceramics decreased. The pH value declined to 7.5 after the circulation of phosphate removal for 6 times. At this time, the restrained phosphate concentration was up to 95.47 mg/L, which indicated that amorphous ceramics did not possess phosphate removal capacity in neutral condition.Figure 8
Changes of residual phosphate concentration and pH values.Indeed, the phosphate recovery process is the form process of calcium orthophosphate, which is also different from the traditional chemical phosphate removal process. Because the traditional chemical phosphate removal process needs a high alkalinity (pH = 10.5~12.5) condition to make Ca2+, OH−, and PO43- reach supersaturated, the phosphate sedimentation precipitated would be produced. Under the proper process condition, amorphous ceramics could release a suitable concentration of Ca2+ and OH− to maintain the pH value during 8.0~9.0. Phosphate existed in the form of HPO42- in the range of these pH values. Ca2+, OH−, and HPO42- formed a local condition with high concentration. This condition was beneficial to the formation of calcium orthophosphate with pH = 8.0~9.0.


## 4. Conclusion

The present work demonstrated that phosphate in poultry wastewater was dropped as the pH value increased during 8.0~9.0 at a proper Ca2+ and OH− concentration during calcium orthophosphate crystallization. The design factors for calcium orthophosphate crystallization process were investigated systematically using the model proposed in this study. The calcium orthophosphate crystallization was affected by pH value, stirring intensity, and amorphous ceramics dosage. The phosphate content of regenerated product obtained by amorphous ceramics reached 14.20%, exceeding that of the regenerated product obtained by tobermorite (13%) and xonotlite (10%). Experiments have also demonstrated the applicability of the phosphate crystallization process as a phosphate recovery system for recycling phosphates in poultry wastewater using amorphous ceramics as seed crystal.



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*Source: 132582-2014-05-21.xml*