# Removal of Sulfur Dioxide from Flue Gas Using the Sludge Sodium Humate

Authors: Yu Zhao; Guoxin Hu
Journal: The Scientific World Journal
 (2013)

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## Abstract

This study shows the ability of sodium humate from alkaline treatment sludge on removing sulfur dioxide (SO2) in the simulated flue gas. Experiments were conducted to examine the effect of various operating parameters, like the inlet SO2 concentration or temperature or O2, on the SO2 absorption efficiency and desulfurization time in a lab-scale bubbling reactor. The sludge sodium humate in the supernatant after alkaline sludge treatment shows great performance in SO2 absorption, and such efficiency can be maintained above 98% with 100 mL of this absorption solution at 298 K (flue gas rate of 0.12 m3/h). The highest SO2 absorption by 1.63 g SHA-Na is 0.946 mmol in the process, which is translated to 0.037 g SO2 g−1 SHA-Na. The experimental results indicate that the inlet SO2 concentration slightly influences the SO2 absorption efficiency and significantly influences the desulfurization time. The pH of the absorption solution should be above 3.5 in this process in order to make an effective desulfurization. The products of this process were characterized by Fourier transform infrared spectroscopy and X-ray diffraction. It can be seen that the desulfurization products mainly contain sludge humic acid sediment, which can be used as fertilizer components.


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## Body

## 1. Introduction

Flue gas emissions, which mainly come from power plants by burning fossil fuels, have been causing serious air pollution for decades [1–3]. The reason for serious air pollution caused by flue gas emissions is that flue gas contains large amounts of sulfur dioxide (SO2) and other pollutants [4]. Many researchers have been actively exploring technologies in effective flue gas desulfurization field [5–8]. Among these technologies, one of the most effective methods is the wet flue gas desulfurization which is mainly based on limestone [9]. However, it has many disadvantages, such as higher operating costs and greater water requirement and the potential to cause secondary pollution. Thus, cost-effective technologies in removing SO2 have become the focus of investigations.Common commercial sodium humate, which is derived from peat, brown coal, and weathered coal, is a cheap absorbent. Green and Manahan started to use sodium humate to absorb SO2 from flue gas in the 1980s [10, 11]. Sun et al. were using humic acid as an additive to modify adsorbents for flue gas desulfurization [12]. Our team used sodium humate solution to remove SO2 and NOx in flue gas [13, 14]. Sludge sodium humate (SHA-Na) can be extracted from sludge through alkaline treatment method [15]. This paper proposed a new process for the removal of SO2 from flue gas by the absorption solution from sludge treatment and the production of fertilizer.The new process shown in Figure1 includes the following stages. (a) Excess sludge is disintegrated by sodium hydroxide in stirred reactor at 313 K. (b) The disintegrated sludge is centrifuged and the supernatant is concentrated through membrane filter to spray into a desulfurization tower. (c) SO2 can be absorbed by SHA-Na in the desulfurization tower. The desulfurization liquid, which mainly contains sludge humic acid (SHA) and H2SO3, flows into the reactor. (d) In the reactor, SO32- is oxidized to SO42- through diffused aeration. (e) Afterward, the reaction liquid from the reactor flows into a sedimentation tank and stands for 12 h. Due to the poor solubility of SHA, SHA may be separated as sediment from acidic solution. The separated SHA can be used as a kind of material for compound fertilizer after drying in spray dryer. From the above process, it is believed that the removal of SO2 by the supernatant from alkaline sludge treatment is a resourceful type of environmental protection technology for FGD. It carries the following advantages: (a) realizes sludge reduction and (b) utilizes the desulfurization product as a useful fertilizer. Therefore, it is hopeful to be applied in the future.Figure 1
Simplified scheme of application of the SHA-Na for flue gas desulfurization.In this paper, we attempt to use a kind of absorption solution from alkaline treatment sludge to remove SO2in flue gas. The effects of the inlet SO2 concentration, temperature, and presence or absence of O2, on the SO2 absorption efficiency, together with desulfurization time in a lab-scale bubbling reactor, are studied. Desulfurization products are characterized by Fourier transform infrared spectroscopy and X-ray diffraction.


## 2. Experimental Section

### 2.1. Materials

Sludge samples were collected from the thickening tank of a wastewater treatment plant. The sludge samples carry water of approximately 98%, a suspended solid (SS) content of 20.0 g/L, a volatile suspended solid (VSS) content of 16.0 g/L, and a soluble chemical oxygen demand (SCOD) of 270 mg/L. Sodium hydroxide (NaOH, AR) was collected from chemical reagent. HA-Na was supplied with purity of 99%. Sulfur dioxide gas with a purity of 99.95% was obtained from the market.


### 2.2. The Absorption Solution Extraction

A slightly modified method [16] was used to extract SHA-Na. The extraction of SHA-Na was conducted in 2.0 L batch mixed reactor that was placed in a water bath to maintain the temperature for this reaction at 313 K while the NaOH is at 0.2 mol/L. Following alkaline sludge treatment, the samples were centrifuged at 5000 r/m for 10 min. After alkaline sludge treatment and centrifugal separation, the sample was filtered through a membrane with a mesh size of 0.45 μm.


### 2.3. Desulfurization Test

A schematic diagram of the experimental setup used in this study is shown in our previous paper [17]. The SO2 gas supplied from cylinder was diluted with O2 and N2 in the gas-mixing chamber. Then, this gaseous mixture flew through the bubbling reactor at ambient pressure. Rota meters and valves were used to monitor the gas flow. The concentrations of the simulated flue gas components (SO2 and O2) were controlled by adjusting their flow rate and were monitored by a flue gas analyzer. In the progress of this experiment, the total rate of the gas stream was controlled at 0.12 m3/h during the experiment.


### 2.4. Characterization Methods

In the experiment, the inlet and outlet concentrations of SO2 were measured by a flue gas analyzer. The pH value measuring was conducted with a pH meter using a combination pH electrode PHB-5. Before each pH value was read, the pH buffer solution was used to check the measurements of the electrode. Water content, SS, and volatile dissolved solids (VDS) were measured according to the standard methods [18]. SHA-Na was measured according to the spectrophotometer method recommended by Ye [19]. The protein content was measured using the Coomassie brilliant blue method [20]. FTIR spectra were recorded in the 4000–500 cm−1 range using an EQUINOX 55 FTIR spectrometer, continuously purged with dry air. Spectra were obtained from pressed KBr pellets. Pellets (1 cm diameter) were prepared by mixing 1 or 2 mg samples with 200 mg KBr. Desulfurization products were characterized by XRD with a D/max-2200/PC type-ray diffraction instrument to study the composition of them. The heavy metals in products were analyzed by inductively coupled plasma atomic emission spectrometry.


## 2.1. Materials

Sludge samples were collected from the thickening tank of a wastewater treatment plant. The sludge samples carry water of approximately 98%, a suspended solid (SS) content of 20.0 g/L, a volatile suspended solid (VSS) content of 16.0 g/L, and a soluble chemical oxygen demand (SCOD) of 270 mg/L. Sodium hydroxide (NaOH, AR) was collected from chemical reagent. HA-Na was supplied with purity of 99%. Sulfur dioxide gas with a purity of 99.95% was obtained from the market.


## 2.2. The Absorption Solution Extraction

A slightly modified method [16] was used to extract SHA-Na. The extraction of SHA-Na was conducted in 2.0 L batch mixed reactor that was placed in a water bath to maintain the temperature for this reaction at 313 K while the NaOH is at 0.2 mol/L. Following alkaline sludge treatment, the samples were centrifuged at 5000 r/m for 10 min. After alkaline sludge treatment and centrifugal separation, the sample was filtered through a membrane with a mesh size of 0.45 μm.


## 2.3. Desulfurization Test

A schematic diagram of the experimental setup used in this study is shown in our previous paper [17]. The SO2 gas supplied from cylinder was diluted with O2 and N2 in the gas-mixing chamber. Then, this gaseous mixture flew through the bubbling reactor at ambient pressure. Rota meters and valves were used to monitor the gas flow. The concentrations of the simulated flue gas components (SO2 and O2) were controlled by adjusting their flow rate and were monitored by a flue gas analyzer. In the progress of this experiment, the total rate of the gas stream was controlled at 0.12 m3/h during the experiment.


## 2.4. Characterization Methods

In the experiment, the inlet and outlet concentrations of SO2 were measured by a flue gas analyzer. The pH value measuring was conducted with a pH meter using a combination pH electrode PHB-5. Before each pH value was read, the pH buffer solution was used to check the measurements of the electrode. Water content, SS, and volatile dissolved solids (VDS) were measured according to the standard methods [18]. SHA-Na was measured according to the spectrophotometer method recommended by Ye [19]. The protein content was measured using the Coomassie brilliant blue method [20]. FTIR spectra were recorded in the 4000–500 cm−1 range using an EQUINOX 55 FTIR spectrometer, continuously purged with dry air. Spectra were obtained from pressed KBr pellets. Pellets (1 cm diameter) were prepared by mixing 1 or 2 mg samples with 200 mg KBr. Desulfurization products were characterized by XRD with a D/max-2200/PC type-ray diffraction instrument to study the composition of them. The heavy metals in products were analyzed by inductively coupled plasma atomic emission spectrometry.


## 3. Results and Discussion

### 3.1. Characteristics of the Supernatant after Alkaline Treatment Sludge

The sludge samples were centrifuged after alkaline treatment, and the supernatant was analyzed. Characteristics of the supernatant after alkaline treatment are shown in Table1. The supernatant has a high pH value which is similar to the common commercial sodium humate. The VDS indicated that there was a high content of organic substances including sodium humate, protein, polysaccharides, nucleic acid, and lipids [21]. It can be seen that sodium humate and protein were the primary constituents in this supernatant. Sodium humate accounted for approximately 25% of all of the dissolved organic matter by weight. After alkaline sludge treatment, the humic acid concentration in the supernatant was 1.63 g/L. However, the concentration of sodium humate in the absorption solution should be 10~40 g/L in order to get a better absorption solution of SO2 in our previous papers. Therefore, when the supernatant was concentrated 10 times by ultrafiltration, the content of sodium humate in the retentate reached the required concentration in the process.Table 1
Characteristics of the supernatant after alkaline treatment.
Parameters
Value
Organic substances
Value
Proportion (%)
pH
10.8
Sodium humate
1.63 g/L
24.1%
SS
0.07 g/L
Protein
2.0 g/L
29.6%
VDS
6.756 g/L
Othersa
3.126 g/L
46.3%


### 3.2. Absorption Process of SO2 in the Absorption Solution

The change of the SO2 concentration in outlet flue gas with time is shown in Figure 2. It can be observed that the SO2 absorption curve in absorption solution is divided into three sections: a descending section, a nearly horizontal section, and an ascending section. Also, the pH of the absorption solution in this process was clearly illustrated in Figure 2. The change of pH in the absorption solution is related to the SO2 concentration in outlet flue gas. In the descending section of SO2 absorption curve, the pH value of the absorption solution drops rapidly from 10.8 to 7.4, because of the faster consumption of OH− in the absorption solution. The pH value of the absorption solution decreases slowly from 7.4 to 3.4 in the nearly horizontal section of SO2 absorption curve, as the SHA-Na in the absorption solution is a sort of pH buffer solution [22], this behavior was interpreted as a buffer action of –COOH [23], which may lower the rate of pH value decrease. In the ascending section of SO2 absorption curve the pH value of SHA-Na maintains a constant number. It can be explained as follows: the absorption solution loses the desulfurization capability as the SHA-Na in the absorption solution has converted to SHA sediment. From the above analyses, it can be seen that when the pH value of the absorption solution drops to 3.4, the absorption solution will loose the desulfurization capability. Hence, the pH value of the absorption solution should be above 3.4 in this process in order to make it an effective desulfurization.Figure 2
The profile absorption process of SO2 in absorption solution. (SO2, 2500 ppm; gas flow, 0.12 m3/h; absorption solution 100 mL; O2, 5 vol%; 298 K).


### 3.3. Analysis of the Desulfurization Mechanism

In removing SO2 process with this absorption solution, the main reactions are that SO2 from simulated flue gas react with SHA-Na, which is an acid-base reaction, and the acid-base theory predicts that SHA-Na should react with SO2 by following neutralization reaction [10, 11]:
(1)SHA-Na(aq)+SO2(g)+H2O⟷SHA(s)+HSO3-(aq)+Na+(aq)Simultaneously, when SO2 is dissolved in the absorption solution, based on its alkalinity, the following reactions occur [24, 25]:
(2)SO2(g)⟷SO2(aq)(3)SO2(aq)+H2O⟷H2SO3(aq)(4)H2SO3(aq)⟷H+(aq)+HSO3-(aq)(5)HSO3-(aq)⟷H+(aq)+SO32-(aq)Generally, the above reactions can be described by the following equilibrium equations (6) and (7):
(6)SO2(aq)+OH-⟷HSO3-(aq)(7)HSO3-(aq)+OH-⟷SO32-(aq)+H2OThen,SO32- is oxidized to SO42- by catalysis with transition metal ions, which is the step for (6) and (7) to move to the right. The dissolved SO2 also produced H+ by ionization in this process. The acidic groups of SHA-Na, such as carboxyl (COO−) and hydroxyl (OH−), can react rapidly with H+, and SHA-Na is transferred to sludge humic acid. According to (1) and (5), this reaction also moves the reaction equilibrium to the right, which results in the fact that more SO2 is dissolved into the absorption solution. When entire SHA-Na is consumed, the desulfurization reaction is terminated in the process.


### 3.4. Desulfurization Performance of SHA-Na

Several additional experiments were done to gain a further understanding of desulfurization performance of SHA-Na. The contrast experiments of removing SO2, one used water at the same volume and another used NaOH solution at the same pH (10.8), were conducted, respectively. Total SO2 absorption can be calculated by (8)
(8)Q=∫0T(η×q×C0×M)22.4×3600×103dt,Q=q×C0×M8.064×107∫0Tηdt,
where Q stands for the amount of SO2 absorption, mmol and η stands for the removal efficiency of SO2, %. The formula of the SO2 absorption efficiency can be obtained from the literature [17]. q stands for the gas flow, m3/h; C0 stands for the inlet concentration of SO2, ppm; M stands for the molar mass SO2, g/mol; T stands for the reaction time, s.It is clear as shown in Table2 that experimental results illustrate that SHA-Na performance much better than that of water and NaOH in both the SO2 absorption efficiency and the duration time of high efficiency ((DTHE), the time of the SO2 absorption efficiency is above 70%). Water absorbs the SO2 more slowly because it is only a physical absorption process controlled by molecular diffusion [26]. However, when we use SHA-Na in this absorption solution to remove SO2, the hydroxyl radicals in SHA-Na can react rapidly with the SO2. Thus, it leads to the decrease of the SO2 concentration in the gas-liquid interface. The SO2 diffusion can be promoted due to this decrease of the SO2 concentration in the gas-liquid interface. Furthermore, SHA-Na can react with H+ as what common commercial sodium humate does, and it is transformed into humic acid sediment. Therefore, it can be concluded that the desulfurization capability of SHA-Na mainly depends upon the consumption of the hydroxyl radicals as well as common commercial sodium humate. Compared with NaOH solution, it is also shown in Table 2 that the desulfurization capability of SHA-Na is stronger than NaOH solution at the same volume and pH value in Table 2. It can be explained that the hydroxyl radicals of NaOH solution are less than those of SHA-Na at the same volume and pH value. The contrast experiments of removing SO2 with different sludge as the absorption solution at the same volume are also conducted, respectively. The experimental results illustrate that SHA-Na performance is also much better than that of activated sludge and excess sludge in both the SO2 absorption efficiency and DTHE. It can be explained that the SO2 absorption efficiency and desulfurization time depend on the content of fulvic acid that can excellently absorb SO2 in the activated sludge or excess sludge [25]. The content of fulvic acid in the activated sludge is lower than the content of fuluic acid in the excess sludge, so the SO2 absorption efficiency of the activated sludge is lower than that of the excess sludge and the desulfurization time of the activated sludge is shorter than that of the excess sludge. Therefore, SHA-Na can be practically used as a kind of absorbent for the removal of SO2.Table 2
The SO2 absorption using different absorption solutiona.
Sample
Maximum absorption efficiency of SO2 (%)
DTHE (s)
Q (mmol)
SHA-Na
98.32
4357
0.946
NaOH
81.04
478
0.080
H2O
78.52
240
0.038
Activated sludge
90.32
408
0.075
Excess sludge
92.40
840
0.166
a
C
0: 2500 ppm; q: 0.12 m3/h; absorption solution: 100 mL; O2: 5 vol%; 298 K; ambient pressure.


### 3.5. Effect of the Inlet SO2 Concentration

The effect of the inlet SO2 concentration on absorption efficiency is displayed in Figure 3. The inlet SO2 concentration does not have significant effect on the SO2 absorption efficiency under this condition, and the SO2 absorption efficiency showed a constant value of about 98% in nearly horizontal section. However, the desulfurization time in this section decreases greatly with the increase of the inlet SO2 concentration. This can be explained as follows: according to the model [27], the absorption of SO2 requires the removal of aqueous SO2 from the gas-liquid interface. The reaction with SHA-Na produced by sludge allows the concentration of SO2 in the absorption solution to decrease. However, the absorption effect of SO2 becomes worse because of higher concentration of SO2 at the gas-liquid interface when the inlet SO2 concentration increases. Hence the desulfurization time in the nearly horizontal section decreased. And the absorption amount of SO2 at the inset in Figure 3, which decreases with the increase of the inlet SO2 concentration, shows a reasonable agreement with it.Figure 3
The effect of the inlet SO2 concentration (gas flow, 0.12 m3/h; absorption solution, 100 mL; O2, 5 vol%; 298 K). The inset shows the absorption amount of SO2 and DTHE.


### 3.6. Effect of the Temperature

The effect of the temperature on the SO2 absorption efficiency was also conducted. The experimental results are shown in Figure 4. It indicates that the absorption temperature has slight effect on the SO2 absorption efficiency and the desulfurization time in the nearly horizontal section becomes shorter with the rise of the temperature. The SO2 absorption efficiency increases slightly as the absorption temperature ascends from 298 K to 338 K. However, the desulfurization time in the nearly horizontal section decreases from 3500 s to 1300 s as the absorption temperature ascends from 298 K to 338 K. It can be explained as follows. On one hand, according to the dissolution equilibrium of SO2, the equilibrium partial pressure of SO2 is increasing with the rise of the temperature, which results in the escape of some dissolved SO2 from solution. In addition, the limit of “diffusional regime” is probably reached and this limit depends on temperature proposed by Lancia and Musmarra [28]. The solubility of SO2 decreases with the rise of the absorption temperature in water. On the other hand, the contact time of flue gas and liquid is reduced because the relative velocity of gas molecules speeds up at high temperature. Hence, the absorption amount of SO2 decreases with the increase of the temperature at the inset in Figure 4. Although the removal of SO2 is promoted at low temperature, removing SO2 with SHA-Na solution in the ambient condition at room temperature should be suitable for this process to reduce the desulfurization cost.Figure 4
The effect of the temperature (SO2, 2500 ppm; gas flow, 0.12 m3/h; absorption solution, 100 mL; O2, 5 vol%). The inset shows the absorption amount of SO2 and DTHE.


### 3.7. Effect of Oxygen

Flue gas from power plant usually consists of about 5 vol% O2, trace gases, 15 to 20 vol% CO2, and balance N2 [29]. Hence, oxygen (a concentration of 5 vol%) was introduced into a simple simulated flue gas (N2 + SO2), that is, the simulated flue gas for this study, to understand the potential influence of the presence of O2 on the SHA-Na performances and interaction of SO2 and SHA-Na in the absorption solution. Test was conducted without the presence of O2, where relative to the presence of O2, which is shown in Figure 5. The SO2 absorption efficiency has a slight decrease under an aerobic condition, while the absorption amount of SO2 and DTHE has little increase. It is known that the dissolved O2 in the absorption solution may accelerate the oxidation of sulfite into sulfate. Sulphite oxidation rate can be greatly improved by very low metal concentration [30, 31]. The mass-transfer resistance of the liquid phase in absorption solution is lessened, which results in the promotion of the SO2 mass transfer. Thus, the SO2 absorption efficiency with the presence of oxygen is higher than that with the absence of O2. However, it maybe that the consumption of O2 makes a corresponding growth of the inlet SO2 concentration, which results in the lower absorption amount of SO2 and DTHE. Based on the flue gas, the oxygen concentration was maintained at 5% in the simulated flue gas of N2, O2 and for subsequent experiments.Figure 5
The effects of O2 (SO2, 2500 ppm; gas flow, 0.12 m3/h; absorption solution, 100 mL; 298 K). The inset shows the absorption amount of SO2 and DTHE.


### 3.8. Analysis of Desulfurization Product

After the desulfurization process, the absorption liquid shown in Figure6 was separated into liquid and solid by filtration. The crystals were gained by drying the supernatant layer from the absorption liquid.Figure 6
The photo of (A) SHA-Na solution; (B) desulfurization liquid after standing for 3 hours (SO2, 2500 ppm; gas flow, 0.12 m3/h; absorption solution, 100 mL; O2, 5 vol%; 25°C).FTIR spectroscopy is a powerful and nondestructive tool for the investigation of decomposition in the desulfurization product. Figure7 shows the FTIR spectra comparison diagram of desulfurization products which are from SHA-Na desulfurization process and HA-Na desulfurization process, respectively. The main absorbance bands of them are in common a broad band at the wavenumbers of 3424 cm−1 (H bonds, OH groups), 1384 cm−1 (COO−, CH3), a small peak at 1253 cm−1 (aromatic C, C–O stretch), a slight shoulder around 1097 cm−1 (aliphatic CH2, OH, or C–O stretch of various groups), and a peak at 1050 cm−1 (C–O stretch of polysaccharide) [32, 33]. Compared with spectra of humic acid, it is obvious that distinct differences in the spectra that resulted from the SHA-Na flue gas desulfurization process appear as peaks in the aliphatic region at 2921 and 2860 cm−1, [34] in which sludge humic acid contains a lot of fat material. Three new bands (1652, 1539, and 1460 cm−1) appear in the 1700–1450 cm−1 spectra of all the products of desulfurization. HAs are distinguished by the presence of a strong absorption band near 1650 cm−1, moderately strong absorption at 1540 cm−1, strong absorption near 1050 cm−1, and relatively pronounced absorption near 2900 cm−1 [35]. A unique feature of this spectrum also shows the presence of bands indicated proteins and carbohydrates. Due to its poor solubility, sludge humic acid may be separated as sediment from acidic aqueous solution and converted into humic acid compound fertilizer. The chief product of drying the supernatant layer was characterized by XRD. As shown in Figure 8, the diffraction peaks at the XRD patterns of the catalysts obviously belong to Na2SO4 [36, 37].Figure 7
FTIR spectra of desulfurization product (SO2, 2500 ppm; gas flow, 0.12 m3/h; absorption solution, 100 mL; O2, 5 vol%; 25°C).Figure 8
XRD pattern of the crystals from supernatant (SO2, 2500 ppm; gas flow, 0.12 m3/h; absorption solution, 100 mL; O2, 5 vol%; 25°C).Heavy metals are a limiting factor for sludge fertilizer. The heavy metal content of humic acids extracted from sludge depends on the dissolution rate of sludge heavy metals and the rejection rate of heavy metals by the membrane. During NaOH treatment, the dissolved heavy metals in sludge generally comprise less than 60% of the total heavy metals [38]. Under the strong alkaline conditions, only part of the amphoteric metal in proper forms can be dissolved. Therefore, the heavy metal content in the supernatant was low in Table 3. It can be seen that after the desulfurization process, the desulfurization product contains mainly sludge humic acid sediment, which may be used as fertilizer components.Table 3
The contents of humic acid and heavy metals in the product and the comparison with the standard.
Indexes
In the standard
In the product
Humic acid (g/L)
≥30
15.2
As (mg/L)
≤10
0.56
Cd (mg/L)
≤10
0.41
Pb (mg/L)
≤50
5.31
(SO2: 2500 ppm; gas flow: 0.12 m3/h; absorption solution: 100 mL; O2: 5 vol%; 25°C.)


## 3.1. Characteristics of the Supernatant after Alkaline Treatment Sludge

The sludge samples were centrifuged after alkaline treatment, and the supernatant was analyzed. Characteristics of the supernatant after alkaline treatment are shown in Table1. The supernatant has a high pH value which is similar to the common commercial sodium humate. The VDS indicated that there was a high content of organic substances including sodium humate, protein, polysaccharides, nucleic acid, and lipids [21]. It can be seen that sodium humate and protein were the primary constituents in this supernatant. Sodium humate accounted for approximately 25% of all of the dissolved organic matter by weight. After alkaline sludge treatment, the humic acid concentration in the supernatant was 1.63 g/L. However, the concentration of sodium humate in the absorption solution should be 10~40 g/L in order to get a better absorption solution of SO2 in our previous papers. Therefore, when the supernatant was concentrated 10 times by ultrafiltration, the content of sodium humate in the retentate reached the required concentration in the process.Table 1
Characteristics of the supernatant after alkaline treatment.
Parameters
Value
Organic substances
Value
Proportion (%)
pH
10.8
Sodium humate
1.63 g/L
24.1%
SS
0.07 g/L
Protein
2.0 g/L
29.6%
VDS
6.756 g/L
Othersa
3.126 g/L
46.3%


## 3.2. Absorption Process of SO2 in the Absorption Solution

The change of the SO2 concentration in outlet flue gas with time is shown in Figure 2. It can be observed that the SO2 absorption curve in absorption solution is divided into three sections: a descending section, a nearly horizontal section, and an ascending section. Also, the pH of the absorption solution in this process was clearly illustrated in Figure 2. The change of pH in the absorption solution is related to the SO2 concentration in outlet flue gas. In the descending section of SO2 absorption curve, the pH value of the absorption solution drops rapidly from 10.8 to 7.4, because of the faster consumption of OH− in the absorption solution. The pH value of the absorption solution decreases slowly from 7.4 to 3.4 in the nearly horizontal section of SO2 absorption curve, as the SHA-Na in the absorption solution is a sort of pH buffer solution [22], this behavior was interpreted as a buffer action of –COOH [23], which may lower the rate of pH value decrease. In the ascending section of SO2 absorption curve the pH value of SHA-Na maintains a constant number. It can be explained as follows: the absorption solution loses the desulfurization capability as the SHA-Na in the absorption solution has converted to SHA sediment. From the above analyses, it can be seen that when the pH value of the absorption solution drops to 3.4, the absorption solution will loose the desulfurization capability. Hence, the pH value of the absorption solution should be above 3.4 in this process in order to make it an effective desulfurization.Figure 2
The profile absorption process of SO2 in absorption solution. (SO2, 2500 ppm; gas flow, 0.12 m3/h; absorption solution 100 mL; O2, 5 vol%; 298 K).


## 3.3. Analysis of the Desulfurization Mechanism

In removing SO2 process with this absorption solution, the main reactions are that SO2 from simulated flue gas react with SHA-Na, which is an acid-base reaction, and the acid-base theory predicts that SHA-Na should react with SO2 by following neutralization reaction [10, 11]:
(1)SHA-Na(aq)+SO2(g)+H2O⟷SHA(s)+HSO3-(aq)+Na+(aq)Simultaneously, when SO2 is dissolved in the absorption solution, based on its alkalinity, the following reactions occur [24, 25]:
(2)SO2(g)⟷SO2(aq)(3)SO2(aq)+H2O⟷H2SO3(aq)(4)H2SO3(aq)⟷H+(aq)+HSO3-(aq)(5)HSO3-(aq)⟷H+(aq)+SO32-(aq)Generally, the above reactions can be described by the following equilibrium equations (6) and (7):
(6)SO2(aq)+OH-⟷HSO3-(aq)(7)HSO3-(aq)+OH-⟷SO32-(aq)+H2OThen,SO32- is oxidized to SO42- by catalysis with transition metal ions, which is the step for (6) and (7) to move to the right. The dissolved SO2 also produced H+ by ionization in this process. The acidic groups of SHA-Na, such as carboxyl (COO−) and hydroxyl (OH−), can react rapidly with H+, and SHA-Na is transferred to sludge humic acid. According to (1) and (5), this reaction also moves the reaction equilibrium to the right, which results in the fact that more SO2 is dissolved into the absorption solution. When entire SHA-Na is consumed, the desulfurization reaction is terminated in the process.


## 3.4. Desulfurization Performance of SHA-Na

Several additional experiments were done to gain a further understanding of desulfurization performance of SHA-Na. The contrast experiments of removing SO2, one used water at the same volume and another used NaOH solution at the same pH (10.8), were conducted, respectively. Total SO2 absorption can be calculated by (8)
(8)Q=∫0T(η×q×C0×M)22.4×3600×103dt,Q=q×C0×M8.064×107∫0Tηdt,
where Q stands for the amount of SO2 absorption, mmol and η stands for the removal efficiency of SO2, %. The formula of the SO2 absorption efficiency can be obtained from the literature [17]. q stands for the gas flow, m3/h; C0 stands for the inlet concentration of SO2, ppm; M stands for the molar mass SO2, g/mol; T stands for the reaction time, s.It is clear as shown in Table2 that experimental results illustrate that SHA-Na performance much better than that of water and NaOH in both the SO2 absorption efficiency and the duration time of high efficiency ((DTHE), the time of the SO2 absorption efficiency is above 70%). Water absorbs the SO2 more slowly because it is only a physical absorption process controlled by molecular diffusion [26]. However, when we use SHA-Na in this absorption solution to remove SO2, the hydroxyl radicals in SHA-Na can react rapidly with the SO2. Thus, it leads to the decrease of the SO2 concentration in the gas-liquid interface. The SO2 diffusion can be promoted due to this decrease of the SO2 concentration in the gas-liquid interface. Furthermore, SHA-Na can react with H+ as what common commercial sodium humate does, and it is transformed into humic acid sediment. Therefore, it can be concluded that the desulfurization capability of SHA-Na mainly depends upon the consumption of the hydroxyl radicals as well as common commercial sodium humate. Compared with NaOH solution, it is also shown in Table 2 that the desulfurization capability of SHA-Na is stronger than NaOH solution at the same volume and pH value in Table 2. It can be explained that the hydroxyl radicals of NaOH solution are less than those of SHA-Na at the same volume and pH value. The contrast experiments of removing SO2 with different sludge as the absorption solution at the same volume are also conducted, respectively. The experimental results illustrate that SHA-Na performance is also much better than that of activated sludge and excess sludge in both the SO2 absorption efficiency and DTHE. It can be explained that the SO2 absorption efficiency and desulfurization time depend on the content of fulvic acid that can excellently absorb SO2 in the activated sludge or excess sludge [25]. The content of fulvic acid in the activated sludge is lower than the content of fuluic acid in the excess sludge, so the SO2 absorption efficiency of the activated sludge is lower than that of the excess sludge and the desulfurization time of the activated sludge is shorter than that of the excess sludge. Therefore, SHA-Na can be practically used as a kind of absorbent for the removal of SO2.Table 2
The SO2 absorption using different absorption solutiona.
Sample
Maximum absorption efficiency of SO2 (%)
DTHE (s)
Q (mmol)
SHA-Na
98.32
4357
0.946
NaOH
81.04
478
0.080
H2O
78.52
240
0.038
Activated sludge
90.32
408
0.075
Excess sludge
92.40
840
0.166
a
C
0: 2500 ppm; q: 0.12 m3/h; absorption solution: 100 mL; O2: 5 vol%; 298 K; ambient pressure.


## 3.5. Effect of the Inlet SO2 Concentration

The effect of the inlet SO2 concentration on absorption efficiency is displayed in Figure 3. The inlet SO2 concentration does not have significant effect on the SO2 absorption efficiency under this condition, and the SO2 absorption efficiency showed a constant value of about 98% in nearly horizontal section. However, the desulfurization time in this section decreases greatly with the increase of the inlet SO2 concentration. This can be explained as follows: according to the model [27], the absorption of SO2 requires the removal of aqueous SO2 from the gas-liquid interface. The reaction with SHA-Na produced by sludge allows the concentration of SO2 in the absorption solution to decrease. However, the absorption effect of SO2 becomes worse because of higher concentration of SO2 at the gas-liquid interface when the inlet SO2 concentration increases. Hence the desulfurization time in the nearly horizontal section decreased. And the absorption amount of SO2 at the inset in Figure 3, which decreases with the increase of the inlet SO2 concentration, shows a reasonable agreement with it.Figure 3
The effect of the inlet SO2 concentration (gas flow, 0.12 m3/h; absorption solution, 100 mL; O2, 5 vol%; 298 K). The inset shows the absorption amount of SO2 and DTHE.


## 3.6. Effect of the Temperature

The effect of the temperature on the SO2 absorption efficiency was also conducted. The experimental results are shown in Figure 4. It indicates that the absorption temperature has slight effect on the SO2 absorption efficiency and the desulfurization time in the nearly horizontal section becomes shorter with the rise of the temperature. The SO2 absorption efficiency increases slightly as the absorption temperature ascends from 298 K to 338 K. However, the desulfurization time in the nearly horizontal section decreases from 3500 s to 1300 s as the absorption temperature ascends from 298 K to 338 K. It can be explained as follows. On one hand, according to the dissolution equilibrium of SO2, the equilibrium partial pressure of SO2 is increasing with the rise of the temperature, which results in the escape of some dissolved SO2 from solution. In addition, the limit of “diffusional regime” is probably reached and this limit depends on temperature proposed by Lancia and Musmarra [28]. The solubility of SO2 decreases with the rise of the absorption temperature in water. On the other hand, the contact time of flue gas and liquid is reduced because the relative velocity of gas molecules speeds up at high temperature. Hence, the absorption amount of SO2 decreases with the increase of the temperature at the inset in Figure 4. Although the removal of SO2 is promoted at low temperature, removing SO2 with SHA-Na solution in the ambient condition at room temperature should be suitable for this process to reduce the desulfurization cost.Figure 4
The effect of the temperature (SO2, 2500 ppm; gas flow, 0.12 m3/h; absorption solution, 100 mL; O2, 5 vol%). The inset shows the absorption amount of SO2 and DTHE.


## 3.7. Effect of Oxygen

Flue gas from power plant usually consists of about 5 vol% O2, trace gases, 15 to 20 vol% CO2, and balance N2 [29]. Hence, oxygen (a concentration of 5 vol%) was introduced into a simple simulated flue gas (N2 + SO2), that is, the simulated flue gas for this study, to understand the potential influence of the presence of O2 on the SHA-Na performances and interaction of SO2 and SHA-Na in the absorption solution. Test was conducted without the presence of O2, where relative to the presence of O2, which is shown in Figure 5. The SO2 absorption efficiency has a slight decrease under an aerobic condition, while the absorption amount of SO2 and DTHE has little increase. It is known that the dissolved O2 in the absorption solution may accelerate the oxidation of sulfite into sulfate. Sulphite oxidation rate can be greatly improved by very low metal concentration [30, 31]. The mass-transfer resistance of the liquid phase in absorption solution is lessened, which results in the promotion of the SO2 mass transfer. Thus, the SO2 absorption efficiency with the presence of oxygen is higher than that with the absence of O2. However, it maybe that the consumption of O2 makes a corresponding growth of the inlet SO2 concentration, which results in the lower absorption amount of SO2 and DTHE. Based on the flue gas, the oxygen concentration was maintained at 5% in the simulated flue gas of N2, O2 and for subsequent experiments.Figure 5
The effects of O2 (SO2, 2500 ppm; gas flow, 0.12 m3/h; absorption solution, 100 mL; 298 K). The inset shows the absorption amount of SO2 and DTHE.


## 3.8. Analysis of Desulfurization Product

After the desulfurization process, the absorption liquid shown in Figure6 was separated into liquid and solid by filtration. The crystals were gained by drying the supernatant layer from the absorption liquid.Figure 6
The photo of (A) SHA-Na solution; (B) desulfurization liquid after standing for 3 hours (SO2, 2500 ppm; gas flow, 0.12 m3/h; absorption solution, 100 mL; O2, 5 vol%; 25°C).FTIR spectroscopy is a powerful and nondestructive tool for the investigation of decomposition in the desulfurization product. Figure7 shows the FTIR spectra comparison diagram of desulfurization products which are from SHA-Na desulfurization process and HA-Na desulfurization process, respectively. The main absorbance bands of them are in common a broad band at the wavenumbers of 3424 cm−1 (H bonds, OH groups), 1384 cm−1 (COO−, CH3), a small peak at 1253 cm−1 (aromatic C, C–O stretch), a slight shoulder around 1097 cm−1 (aliphatic CH2, OH, or C–O stretch of various groups), and a peak at 1050 cm−1 (C–O stretch of polysaccharide) [32, 33]. Compared with spectra of humic acid, it is obvious that distinct differences in the spectra that resulted from the SHA-Na flue gas desulfurization process appear as peaks in the aliphatic region at 2921 and 2860 cm−1, [34] in which sludge humic acid contains a lot of fat material. Three new bands (1652, 1539, and 1460 cm−1) appear in the 1700–1450 cm−1 spectra of all the products of desulfurization. HAs are distinguished by the presence of a strong absorption band near 1650 cm−1, moderately strong absorption at 1540 cm−1, strong absorption near 1050 cm−1, and relatively pronounced absorption near 2900 cm−1 [35]. A unique feature of this spectrum also shows the presence of bands indicated proteins and carbohydrates. Due to its poor solubility, sludge humic acid may be separated as sediment from acidic aqueous solution and converted into humic acid compound fertilizer. The chief product of drying the supernatant layer was characterized by XRD. As shown in Figure 8, the diffraction peaks at the XRD patterns of the catalysts obviously belong to Na2SO4 [36, 37].Figure 7
FTIR spectra of desulfurization product (SO2, 2500 ppm; gas flow, 0.12 m3/h; absorption solution, 100 mL; O2, 5 vol%; 25°C).Figure 8
XRD pattern of the crystals from supernatant (SO2, 2500 ppm; gas flow, 0.12 m3/h; absorption solution, 100 mL; O2, 5 vol%; 25°C).Heavy metals are a limiting factor for sludge fertilizer. The heavy metal content of humic acids extracted from sludge depends on the dissolution rate of sludge heavy metals and the rejection rate of heavy metals by the membrane. During NaOH treatment, the dissolved heavy metals in sludge generally comprise less than 60% of the total heavy metals [38]. Under the strong alkaline conditions, only part of the amphoteric metal in proper forms can be dissolved. Therefore, the heavy metal content in the supernatant was low in Table 3. It can be seen that after the desulfurization process, the desulfurization product contains mainly sludge humic acid sediment, which may be used as fertilizer components.Table 3
The contents of humic acid and heavy metals in the product and the comparison with the standard.
Indexes
In the standard
In the product
Humic acid (g/L)
≥30
15.2
As (mg/L)
≤10
0.56
Cd (mg/L)
≤10
0.41
Pb (mg/L)
≤50
5.31
(SO2: 2500 ppm; gas flow: 0.12 m3/h; absorption solution: 100 mL; O2: 5 vol%; 25°C.)


## 4. Conclusion

In the present work, alkaline pretreatment of the activated sludge represented a suitable and effective method for the preparation of SHA-Na. The characteristics of SO2 absorption into the SHA-Na absorption solution have been investigated in a bubbling reactor. The experimental results show, that compared with water (with the same volume) and NaOH solution (with the same pH), SHA-Na shows greater performance in SO2 absorption. The effects on the SO2 absorption efficiency and desulfurization time have been studied, while the inlet SO2 concentration and temperature were changed. Characterization of the desulfurization products was performed by FTIR and XRD analysis. It was found that the desulfurization products can be used as the compound fertilizer. The concept of combat environmental problems by methods such as removing a waste by using another waste source is of economic interest. Therefore, it is possible for the desulfurization process of SHA-Na to be used in future.



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*Source: 573051-2013-12-25.xml*