Synthesis of Single-Phase Zeolite A by Coal Gasification Fine Slag from Ningdong and Its Application as a High-Efficiency Adsorbent for Cu²⁺ and Pb²⁺ in Simulated Waste Water

Abstract

Coal gasification is a new direction for the clean utilization of coal, but it also brings huge environmental pressure on solid waste. In this paper, the high-crystallinity single-phase zeolite A was prepared by solid-phase alkali fusion synthesis from coal gasification fine slag (CGFS), without template agent, with low water consumption, and with low cost, and it was used to remove heavy metals such as Pb²⁺ and Cu²⁺ in simulated waste water. The main factors affecting the solid-phase and green synthesis methods were analyzed, and the optimum conditions for solid-phase synthesis of high-crystallinity single-phase zeolite A were determined as follows: NaOH/CGFS = 1.2; solid-phase alkali fusion temperature 823 K, solid-phase alkali fusion 90 min, liquid–solid ratio 4.5, and 353 K hydrothermal reaction for 12 h. The relative crystallinity, specific surface area, and ion-exchange capacity of single-phase zeolites A are 93.1%, 61.09 m²/g, and 268.4 mmol/100 g. The removal rates of Pb²⁺ and Cu²⁺ can reach more than 99%, especially for the removal efficiency of Pb²⁺, which is common in simulated waste water. This is an effective method with important application prospects, and it formed an effective way to recycle solid waste of coal chemical industry.

1. Introduction

Ningdong Coal and Chemical Base in China has the largest single capacity coal gasification plant in the world. With the continuous increase of its production capacity and great environmental pressure, the annual output of Coal gasification slag is close to 10 million tons, of which fine slag accounts for about 50%. Due to the high carbon content of fine slag (20 ≤ 30%), it cannot be used as building materials [1,2,3,4]. Coal Gasified slag has a chemical composition similar to that of zeolites, and if it can be converted at a low cost, it will have great economic and environmental benefits. Coal gasification fine slag can be used in the fields of adsorption of heavy metal pollution, sewage treatment, catalysis, and so on. At the same time, it can reduce environmental pollution and realize the resource utilization of waste and the realization of “Using waste treat waste” [5,6].

Although there are many studies on the preparation of microporous materials with fly ash [7,8,9,10,11,12,13], fine slag of coal gasification in Ningdong is produced in the reducing atmosphere (CO and H₂) at 1400–1500 °C, and obtained after washing gas, flocculation, and filtration. Not only its composition and structure but also its structure and system utilization are different from fly ash [14,15,16]. No technology can be directly used. At present, the comprehensive utilization of coal gasification slag is seldom studied, and the preparation of zeolite from coal gasification slag is rarely reported. For the utilization of solid waste, the method that is of low cost, with little secondary pollution, and of simple operation should be chosen; otherwise, it is difficult to realize the application [14,15,16]. In this paper, the solid phase synthesis method is used to synthesize microporous materials from fine slag of coal gasification. The method has the advantages of low cost, simple operation, low water consumption, and low secondary pollution. At the same time, it can also improve the performance of zeolites as a stable ion exchanger, and the products are usually composed of zeolites with high crystallization and a single phase. In that coal gasification fine slag, Si and Al occupy a high proportion in the quartz and mullite crystal phase and are difficult to be dissolved in water; the dissolution of the Si and Al components plays a critical role in the nucleation and crystallization of the zeolite [6,17,18,19,20,21].

Zeolite A is a widely used synthetic zeolite and is widely used in sewage treatment and purification [20]. As we all know, the application of zeolite in the removal of heavy metals in sewage has important application prospects, but its synthetic raw materials are often expensive and require expensive template agents. The method is complex, the water consumption is huge, and it causes serious secondary pollution. This kind of zeolite prepared with natural low cost and even solid waste will show greater application prospects. Heavy metal pollution has become one of the most serious environmental problems, and if the coal gasification slag is synthesized into zeolite and applied to the treatment of heavy metal ions in simulated waste water, the purpose of “using waste to treat waste” and resource utilization, it will be beneficial to the environment.

In this paper, the solid phase of coal gasification fine slag was used to synthesize high-crystallinity single-phase zeolite A. Through the comparative experiment of the synthesis conditions, XRD, SEM, BET, and other in situ techniques were used to characterize the synthesis products, and the main factors influencing the solid phase and oligosaprobic methods were analyzed. Given the characteristics of coal gasification fine slag, a template-free, low-cost, easy-to-use solid-phase alkaline fusion synthesis method is proposed, which has good application prospects. The prepared high-crystallinity single-phase zeolites A has a good effect on the treatment of heavy Pb²⁺, Cu²⁺ in simulated waste water, especially for Pb²⁺ with better selectivity. The solid-phase alkali fusion synthesis of coal gasification fine slag into high-crystallinity single-phase zeolite A. This study provides a new idea for solving the large-scale accumulation of coal gasification fine slag (CGFS) and the treatment of ammonia nitrogen and heavy metals, especially Pb²⁺ and Cu²⁺, in industrial-simulated waste water. This is a very promising green environmental protection and “waste control waste” route.

2. Experimental Section

2.1. Materials and Reagents

We used coal gasification fine slag (CGFS) from Ningdong Coal Chemical Base of China as the raw material for the synthesis of zeolites. The fine slag of coal gasification was dried at 378 K in a constant temperature drying box for 24 h and preserved after grinding. The sodium hydroxide particles were used as alkaline activating agent, the silicon and aluminum in the coal gasification slag are activated, and the sodium aluminate (NaAlO₂) was used as aluminum source. The ratio of silicon to aluminum (SiO₂/Al₂O₃ ≈ 1) in the reaction mixture was adjusted to prepare the target molecular sieves. Pure lead nitrate and copper nitrate were analyzed as raw materials for simulating different heavy metal ions in simulated waste water.

2.2. Zeolite A Synthesis

3.5 g dried fine coal gasification slag samples were weighed in a mortar, and 4.2 g NaOH was added according to NaOH/CGFS = 1.2 to grind for 10 min and then put into a nickel vessel. Solid-state was melted for 90 min at 823 K in muff furnace before cooling. NaAlO₂ was added to the product after fusion to adjust the ratio (SiO₂/Al₂O₃ ≈ 1) of the mixture. After grinding the mixture for 5 min, the mixture was transferred to 100 mL Teflon liner and deionized water (liquid–solid ratio, 4.5~5.5) was added for full stirring. The mixture was put into a hydrothermal reaction kettle and kept the constant temperature in a thermostatic drying box 353 K for 12 h. After cooling at the end of reaction time, the product was washed and filtered to a pH of about 10. The solid product after filtration was dried overnight at 378 K. The process flow chart is shown in Figure 1.The reaction chemical equation is as follows:

$$\left(2\mathrm{x}+2\mathrm{y}\right)\mathrm{NaOH}+{\mathrm{xAl}}_2{\mathrm{O}}_3·{\mathrm{ySiO}}_2\stackrel{\mathrm{fusion}}{\to }{\mathrm{yNa}}_2{\mathrm{SiO}}_3+2{\mathrm{xNaAlO}}_2+\left(\mathrm{y}+\mathrm{x}\right){\mathrm{H}}_2\mathrm{O}$$

(1)

$$12{\mathrm{Na}}_2{\mathrm{SiO}}_3+12{\mathrm{NaAlO}}_2+39{\mathrm{H}}_2\mathrm{O}\to {\mathrm{Na}}_{12}{\mathrm{Al}}_{12}{\mathrm{Si}}_{12}{\mathrm{O}}_{48}·27{\mathrm{H}}_2\mathrm{O}+24\mathrm{NaOH}$$

(2)

2.3. Heavy Metal Treatment Experiment

15,985 g and 37,750 g of analytically pure lead nitrate and copper nitrate were weighed in a beaker, respectively, and added to deionized water, and stirred until completely dissolved. The mixture was placed in a volumetric flask with a constant volume of 1000 mL. Heavy metal ion reserve solution with a concentration of 1000 mg/L was prepared, and heavy metal simulated waste water with different concentrations was simulated according to different experimental requirements.

Simulation of 100 mg/L Pb(NO₃)₂, Cu(NO₃)₂ heavy metal simulated waste water 100 mL in a conical flask, add 1.5 g of heavy metal adsorbent, adjust pH = 6 with 2% HNO₃, oscillate in a thermostatic oscillator for 240 min, the rotation speed is 150 r/min. The supernatant was filtered by a glass fiber filter with a pore diameter of 0.45 microns, and the concentration of heavy metal ions in the solution was determined by ICP-MS. Calculation formula of removal rate of heavy metal ions:

$$\mathsf{\eta }(\%)=\frac{C_0-C_t}{C_0}\times 100\%$$

(3)

2.4. Characterization Methods

The concentration of heavy metals in the solution was determined by Thermo Fisher Scientific ICP TQ.

X-ray fluorescence spectroscopy (XRF) used S2 Ranger (Karlsruhe, Baden-Wurttemberg, Germany) spectrometer to study the chemical composition of CGFS. X-ray diffraction (XRD) was carried out on the crystal phase of solid products by D8 advanced diffractometer (Bruker, Karlsruhe, Baden-Wurttemberg, Germany). The working voltage of CuKα radiation source is 40 kV and 40 mA. The 2θ range is 5–60°, and the scanning speed is 2°/min.

The morphology and structure of CGFS were studied with JSM-7500F scanning electron microscope and synthesized zeolite products. The characteristic functional groups on the surface of the zeolite can be analyzed by FTIR. The position of the infrared absorption peak can judge the structure of the functional group and the bond of the material. The silicon–oxygen bond and the aluminum–oxygen bond in the sample have special stretching vibration peaks in the infrared spectrum. This study uses the Fourier transform infrared spectrometer produced by PerkinElmer, USA. Using KBr as the background, the scan was in the range of 400–4000 cm⁻¹.

ASAP2020 physical adsorption analyzer (Micromeritics, USA) was used to obtain the N₂ adsorption–desorption isotherm curve at 77 K. The specific surface area is determined by the BET equation, and the pore size distribution is calculated by the N₂-DFT model.

The cation exchange capacity of the sample was determined by Nessler spectrophotometry. The sample to be tested was dried under the condition of 378 K, and the NH₄Cl standard solution having a concentration of 18.69 mmol/L was accurately set for use. The sample was uniformly mixed at a liquid–solid ratio of 10 g/L and shaken at a constant speed, for 24 h, in a 298 K constant-temperature shaker. The NH⁴⁺ concentration was determined by Nessler spectrophotometry at 420 nm, using an ultraviolet spectrophotometer, and each experiment was repeated three times, in parallel [10]. The formula for calculating the cation exchange capacity is as follows:

$$CEC=\frac{\left(C_0-C_t\right)\times V\times {10}^{-3}}{m}$$

(4)

In the formula, C₀ is the initial concentration of NH₄ ⁺ ions in the solution (mmol/L), C_t is the concentration of NH₄ ⁺ ion mmol/L) in t moment solution, V is the volume of solution (L), and m is the mass of zeolite (g).

The relative crystallinity (D) of the solid-phase synthesis product is calculated as follows [10,12,22,23].

$$D(\%)=\frac{\mathrm{P}}{{\mathrm{P}}_{\mathrm{S}}}\times 100\%$$

(5)

In the formula, P denotes the sum of the areas under the XRD diffraction peaks of zeolites A, and P_S denotes the total area of the XRD diffraction peaks of the synthesized products.

3. Results and Discussion

3.1. Types and Contents of Substances in Coal Gasification Fine Slag

The chemical composition of the coal gasification fine slag is shown in

Table 1. Substance types and contents of coal gasification slag (CGFS).

Chemical Composition (wt %)
SiO2	Al2O3	Na2O	Fe2O3	MgO	CaO	K2O	TiO2	Total
54.5	15.7	1.77	7.32	2.76	10.1	3.43	1.23	96.81

S2 Ranger X-ray fluorescence spectrometer (XRF), using brook AXS, Germany; system flushing with helium, X-ray tube as Pd target, maximum power: 50 max voltage: 50 max current 2 mA.

. The total content of coal gasification fine slag SiO₂ (54.5%) and Al₂O₃ (15.7%) is over 70%, and the corresponding silicon–aluminum ratio (SiO₂: Al₂O₃) is about 5. The XRD pattern of the coal gasification fine slag (Figure 2) shows that the main diffraction peak appears as quartz, and the “tap peak” indicates that most of the coal gasification fine slag exists in a glassy form. Under the condition of NaOH/CGFS = 1.5, the melting temperature of solid phase was 823 K for 90 min; the XRD pattern of the resulting products showed that the solid phase melting removed the unburned carbon remaining in the fine slag of coal gasification. Because of the action of alkali, the quartz phase was transformed into soluble aluminosilicates such as NaAlO₂ and Na₂SiO₃, proving that the solid-phase melting could activate the silicon and aluminum in the fine slag of coal gasification.

3.2. Zeolite Synthesis and Optimization

3.2.1. Effect of Solid-Phase Alkali Fusion Temperature

The activation of coal gasification fine slag is influenced by different solid melt temperature. The Si and Al components in the fine slag of coal gasification can be transformed into a large number of silicate and aluminosilicate through high-temperature alkali fusion, increasing the number of minerals and participating in the crystallization of zeolite in the subsequent hydrothermal reaction. An appropriate amount of Na⁺ can achieve the highest degree of crystallization nucleation of activated Si and Al and reduce energy and water consumption. Figure 3 is the XRD pattern of zeolite synthesized under different solid-phase alkali melting temperatures. The results show that different solid-phase alkali melting temperatures produce different XRD diffraction peak intensity of the zeolite product; the conversion of quartz phase is not complete at a lower temperature; the product’s relative crystallinity is only 30.03%, which may be due to the decrease in the amount of NaAlO₂; and Na₂SiO₃ generated at lower reaction temperatures and the formation of fewer nuclear sites. With the increase of temperature, the intensity of the zeolite diffraction peak of the product increases, and there is no significant difference between 823 and 873 K. Therefore, 823 K is the appropriate solid-phase melt-activation temperature.

3.2.2. Effect of Hydrothermal Reaction Temperature

The hydrothermal reaction temperature has a great influence on the purity of the synthesized zeolite. Figure 4 is an XRD pattern of the zeolite synthesized under different hydrothermal reaction temperatures. It can be seen from the figure that the characteristic diffraction peak intensity of zeolite A is low at 343 K, and the relative crystallinity is the smallest. Since the hydrothermal reaction is carried out in a closed autoclave when the temperature rises, the dissolution and crystallization rate of the hydrothermal reaction are improved. As the hydrothermal reaction temperature increases again, the intensity of the diffraction peak of the product decreases, and the characteristic diffraction peak of the hydroxides (Hydroxysodalite) is obviously enhanced. Since the sodalite is a relatively stable crystalline phase, the zeolite A phase begins to dissolve, thus indicating that higher temperatures are not conducive to the formation of zeolite A [20,22,23,24]. At 353 K, the obtained diffraction peak type zeolite sharp and miscellaneous crystals least facilitate the synthesis of high-crystallinity single-phase zeolite A. The temperature is too high or too low, which is not conducive to the formation of zeolite A. In this experiment, 353 K is selected as the hydrothermal reaction temperature.

3.2.3. Effect of NaOH/CGFS (Mass Ratio)

The activation of Al is an important part of the preparation of zeolite. By fusing the solid phase with the alkaline hydroxide, the Si and Al components in the coal gasification fine slag can be converted into a large amount of silicate and an aluminosilicate, and the quantity of the minerals is increased. These new phases are very soluble in alkaline solutions, to produce high concentrations of silicon and aluminum, which promotes the formation of the zeolite and participates in the crystallization of the zeolite in a subsequent hydrothermal reaction. When the solid-phase sodium hydroxide is melted and activates the coal gasification slag, the crystallization and the nucleation process of the Na⁺ on the synthesis process of the zeolite have a good catalytic effect, and a proper amount of Na⁺ can enable the activated Si and Al to reach the highest degree of crystal nucleation [25]. Moreover, the energy and water resource consumption can be reduced, so that the coal gasification slag solid phase, the green, and the large-scale synthetic zeolite can be made possible. Figure 5 is an XRD pattern of a synthetic zeolite under different NaOH/CGFS. The reaction mixture forms soluble silicate and aluminate in the solid-phase fusion process, wherein NaOH acts as an activator, and different NaOH/CGFSs affect the activation degree of Si and Al in the coal gasification fine slag, thereby affecting the water heat and the crystallinity of the synthetic zeolite. Na⁺ also plays an important role in the zeolitic process and can be used as a sub-structural unit (especially a six-molecular ring) that stabilizes the zeolite framework [17,18,25]. The experimental results show that the crystallinity of the synthesized zeolite increases with the increase of the amount of NaOH. When the NaOH/CGFS is greater than 1.2, the crystal of sodalite is gradually formed, and the intensity of the diffraction peak is gradually increased. Therefore, in this experiment, NaOH/CGFS = 1.2 was selected to synthesize zeolite A.

3.2.4. Effect of Hydrothermal Synthesis Time

The hydrothermal synthesis time affects the crystallization of zeolite. Figure 6 shows the XRD pattern of zeolite A synthesized by different hydrothermal synthesis time. The results show that the hydrothermal reaction time is insufficient, the zeolite crystal cannot grow completely, the hydrothermal reaction time is too long, and the cost is increased. At the same time, the zeolite is also converted into other crystals, reducing the crystallinity of the target product. The characteristic diffraction peak of zeolite A occurs when the hydrothermal reaction time is 6 h, but the intensity of the diffraction peak is weak at this time, and the relative crystallinity of the zeolite A is low. As the reaction time increases, the synthesized product is mainly zeolite A, and the intensity of the characteristic diffraction peak is significantly increased, and the peak is less. However, when the reaction time is increased to 24 h, there are obvious characteristic peaks of sodalite in the product, which are the main products. When the reaction time exceeds 24 h, the characteristic diffraction peak of zeolite A disappears, and the crystals are transformed into more Stable sodalite crystal [26]. Therefore, the hydrothermal reaction time of the synthesized zeolite A is preferably 12 h, and the product has the best relative crystallinity.

3.2.5. The Effect of Different Liquid–Solid Ratios

Adjusting the liquid–solid ratio means water consumption and secondary pollution. After solid-phase fusion and activation, to meet the goal of green synthesis, water consumption and energy consumption should be minimized. It is necessary to find a synthetic single phase with less water and higher crystallinity. The condition of zeolite A is an inevitable requirement for scale production. Figure 7 is an XRD pattern of zeolite A synthesized under different liquid–solid ratios. The results show that, in the hydrothermal reaction process, the zeolite A product is present under the selected liquid–solid ratio synthesis conditions. The difference is that, when the reaction liquid–solid ratio is 2.5 and 3.5, the intensity of the product diffraction peak is low, and there is also a peak of hydroxysodalite, and when the liquid–solid ratio reaches about 5, the characteristics of the type A molecular sieve appear in the product. The peak fits well with the standard card (PDF #73-2340) and has a better relative crystallinity. Therefore, in this experiment, a liquid–solid ratio of 4.5 synthetic zeolite A was selected.

Through the optimization of the above synthesis conditions, the best conditions for preparing zeolite A using solid-phase alkaline fusion of Ningdong coal gasification fine slag as raw materials are obtained, that is, m(NaOH)/m(CGFS) is 1.2, solid-phase alkaline fusion temperature is 823 K, the hydrothermal reaction temperature is 353 K, the hydrothermal reaction time is 12 h, and the liquid/solid ratio is 4.5 mL/g. The relative crystallinity of the synthetic zeolite A under this condition is calculated to be as high as 93.1% through the calculation of the relative crystallinity formula. Therefore, the process proposed in our research is not only simple in method but low in cost, and the obtained zeolite product has relatively high crystallinity, which is of great significance to waste recycling.

3.3. Characterization of Synthetic Zeolites

3.3.1. Infrared Spectrum

The infrared spectrum of type A zeolite (NaOH/CGFS = 1.2, the calcination temperature is 823 K, calcination time is 90 min, the liquid–solid ratio is 4.5, and the hydrothermal reaction temperature is 353 K, time 12 h) is shown in Figure 8. The absorption peaks appearing at 465 and 562 cm⁻¹ are Al-O-Al stretching vibrations, and the absorption peaks appearing at 668 cm⁻¹ are Si-O-Si or Al-O-Si stretching vibrations. The characteristic peak appearing at 1004 cm⁻¹ is Si-O-Si or Al-O-Si asymmetric stretching vibration, and it is strong -OH stretching vibration and -OH bending vibration at 3422 cm⁻¹ and 1657 cm⁻¹. This is consistent with the XRD results, indicating that the aluminosilicate minerals in the coal gasification fines are converted to specific mineral phases of the zeolite A. The FTIR band was consistent with previous reports, confirming the presence of zeolite A structural unit [26,27,28].

3.3.2. Specific Surface Area and SEM

Figure 9 is a diagram showing the adsorption–desorption curve and the pore size distribution of the solid-phase synthetic zeolite product. The specific surface area and total pore volume of the synthesized product were determined to be 61.1 m²/g and 0.09 cm ³/g, and the average adsorption pore diameter was 6.01 nm. Figure 10d is a scanning electron micrograph of the coal gasification fine slag. The results show that the crystal particles range in size from 1.0 to 2.0 um, and the spherical particles with a smooth surface and the agglomerated porous glass particles are mainly composed. Scanning electron micrographs (Figure 10a–c) confirmed the special cubic morphology of solid-phase fusion synthesis of single-phase zeolite A. The solid-phase synthesis product zeolite A is mainly composed of regular cubic crystal grains, and the distribution of crystalline products is good, presenting a regular cubic structure and a complete crystal plane. By measuring the ion-exchange capacity, the solid-phase fusion synthesis of high-crystallinity single-phase zeolite A has a CEC (cation exchange capacity) = 268.4 mmol/100 g, which has broad application prospects in water purification and ion exchange.

The high-crystallinity single-phase zeolite prepared by solid-phase alkaline fusion was compared with the synthetic zeolite A reported in the literature (

Table 2. CEC and specific surface area of synthesized products in different works in the literature.

Adsorbent	CEC/(mmol⋅(100 g)−1)	SBET/(m2⋅g−1)
Zeolite A	268.4	61.10
Zeolite A [9]	232.2	43.70
Zeolite A [8]	117.7	11.41
Zeolite A [8]	163.1	35.55
Zeolite A [8]	137.6	28.74

) [3,8,9]. Due to the high-crystallinity and the pore structure of zeolite A, a large specific surface area is formed, which is beneficial to ion exchange and has a stronger ability to treat heavy metal ions in simulated waste water. Secondly, from the CEC results, it is also higher than the usual results.

3.4. Treatment of Heavy Metal Ions in Simulated Waste Water

In our research, the high-crystallinity single-phase low-cost A-type zeolite obtained from the resource utilization of coal gasification fine slag can be used for the treatment of heavy metals in industrial simulated waste water. By realizing the on-site transformation of coal gasification slag and “treat waste with waste” concept, we provide a new idea for the treatment of solid waste.

Effects of Adsorbent Dosage, Constant Temperature Oscillation Time, pH Value of the Solution, and Mixed Ions on Removal Rate of Heavy Metal Ions

As shown in Figure 11a, at the same oscillation time, the removal rate of Cu²⁺ by 0.5 g of adsorbent was only 53.5%, and the removal rate of Pb²⁺ was higher, reaching 87.7%. With the increase of adsorbent dosage, the removal rate is increasing. When the amount of adsorbent reaches 1.5 g or more, the removal rate of the adsorbent for 100 mL simulated Cu²⁺ and Pb²⁺ heavy metal ions can reach more than 99%.

As shown in Figure 11b, under the low-temperature oscillation time, the removal rates of heavy metal ions are smaller: Heavy metal ions’ removal rate increases with the increase of adsorption time, and, when up to 240 min, the removal rate of heavy metal ions can reach above 99%.

This paper explores the removal efficiency of heavy metal ions by adsorbent at different pH values. As shown in Figure 11c, when pH = 3, the removal rates of Pb²⁺ and Cu²⁺ were 76.7% and 63.5%, respectively, due to the competitive effect with H⁺. With the increase of pH, the removal rate of heavy metal ions increased. When pH = 6, the removal rate of heavy metal ions reached more than 99%. While pH > 10, heavy metal ions in the solution can form precipitation for removal, and the adsorption effect on the removal of heavy metals is not obvious.

Coexisting ions, especially cations, in the simulated waste water have a great influence on the adsorption effect of zeolite. In the mixed solution of Pb²⁺ and Cu²⁺, the removal rate of adsorbent on two kinds of metal ions is shown in Figure 11d. The removal rate of Pb²⁺ in the solution has little influence, while the removal rate of Cu²⁺ decreases. This may be because the radius of Cu²⁺ is much larger than that of Pb²⁺, while the radius of hydrating ion of Pb²⁺ is larger than that of Cu²⁺, so the removal rate of Pb²⁺ is greater than that of Cu²⁺ when both ions exist simultaneously. At the same time, the removal rate of Pb²⁺ is also higher under different adsorbent dosage, different constant temperature oscillation time, and different pH.

The experimental results of the treatment of Pb²⁺ and Cu²⁺ heavy metal ions in simulated waste water by the synthesis of high-crystallinity single-phase zeolite A from Ningdong coal gasification fine slag show that removal rates of Pb²⁺ and Cu²⁺ can reach more than 99%, especially for the removal of Pb²⁺ in simulated waste water, which is more harmful to humans.

4. Conclusions

Since the special composition and structure of coal gasification slag cannot be applied to the treatment of fly ash, under the requirement of resource recycling, using coal gasification slag requires a low cost, low water consumption, and a simple process. we have prepared high-crystallinity single-phase zeolite A with CEC 268.4 (mmol/100 g) and BET 61.1 m²/g by using a solid-phase alkali fusion synthesis method without template agent. The optimum conditions for the preparation of high-crystallinity single-phase zeolite A by solid-phase alkali fusion of coal gasification fine slag are as follows: m(NaOH)/m(CGFS) = 1.2; solid-phase alkali fusion temperature, 823 K; liquid/solid ratio, 5 mL/g; hydrothermal reaction temperature, 353 K; and hydrothermal reaction time, 12 h, where m(NaOH)/m(CGFS) is an important factor affecting the synthesis of single-phase zeolite A. Na⁺ has a good effect on the crystallization and nucleation process in zeolite synthesis. Proper m(NaOH)/m(CGFS) can make coal gasification fine slag more activated, aluminosilicate better crystallize and nucleate, and consume less energy and water.

We applied the obtained high crystallinity single-phase zeolite A to the removal of Pb²⁺ and Cu²⁺ in simulated waste water, and found that the removal rate of heavy metal Pb²⁺ and Cu²⁺ in simulated waste water can reach more than 99% after the amount of zeolite A material 1.5 g/L, pH = 6, and removal of 250 min. In particular, high-crystallinity single-phase zeolite A prepared from Ningdong coal gasification fine slag has better removal efficiency for the Pb²⁺ in simulated waste water. This paper points out a promising road for the recycling of coal gasification slag.