Treatment of Yellow Phosphorus Slag and Reuse of It as an Absorbent of Chromium (VI) Ions and Methylene Blue

Faculty of Chemistry, Hanoi National University of Education, 136 Xuan uy Road, Cau Giay, Ha Noi 100000, Vietnam Institute for Tropical Technology, Vietnam Academy of Science and Technology, 18, Hoang Quoc Viet, Cau Giay, Ha Noi 100000, Vietnam Graduate University of Science and Technology, Vietnam Academy of Science and Technology, 18 Hoang Quoc Viet, Cau Giay, Ha Noi 100000, Vietnam Nguyen Tat anh University, 300A Nguyen Tat anh, District 4, Ho Chi Minh City 700000, Vietnam


Introduction
Yellow phosphorus slag (YPS) is a waste product of manufacturing yellow phosphorus (P 4 ) using the electrical furnace method at 1400°C-1600°C [1]. e worldwide yellow phosphorus production yields an average of 1.5 million tons of P 4 each year [2]. In which, the countries discharge a large YPS weight including Chinese (75%), Kazakhstan (13%), America (8%), Western Europe (6%), Russia (4%), and the rest of India. For each ton of manufactured P 4 , about 8 to 10 tons of yellow phosphorus slag are produced [1]. is waste product is often left accumulated in the landfills, proposing a potential pollution thread to the environment. e majority of YPS particles compose of CaO and SiO 2 , accounting for approximately 85% of the slag mass [3]. Other components of the YPS are Al 2 O 3, Fe 2 O 3 , MgO, and some rare earth metals [4,5]. In Vietnam, the P 4 is mainly produced and supplied by Lao Cai Yellow Phosphorus JSC (Tang Loong Industrial Zone, Bao ang District, Lao Cai Province, Vietnam), with the productivity of 93,800 tons P 4 /year and about 750,000-1,031,000 tons of YPS waste are produced and released directly into the surrounding environment [6]. erefore, it is important to find different ways to utilize this waste product. Recent studies have been focusing on applying YPS into asphalt or asphalt binder [7,8], cemented backfilling [9], retarding the early hydration of cement [10] or recovering rare earth metals [5]. YPS had been treated by different technologies and methods [11][12][13]. In German Auslegeschrift No. 1,804,172, the YPS particles were heat treated at 1000°C to 1100°C in a rotary furnace [11]. In German Offenlegungsschrift No. 2,211,505, a physical separation method, for example, by gravity separation with tetrabromoethane as the liquid phase, the refinement of silicate slag phase was reported [12]. US patent No. 4,243,425 presented a method for refining of silicatic slag phase with steam at a temperature between 600°C and softening temperature of the slag [13].
In this work, an effective method for treatment of YPS was developed. is is a combination of the water washing flotation system with milling and sorting flotation. e waste water system was treated to recover P 2 O 5 , F, and minerals for other applications. e advantages of this technology were low energy consumption, reduction of noise and dust pollution, closed technology, and environmental friendly and waste water can be easily processed and reused (about 80-90%). e minimized weight of chemicals was used, and treatment process was carried in room temperature. is approached to the green technology, the general trend of the world. e study on metal ion adsorption ability of YPS in aqueous solutions has been limited in the research. Herein, the YPS was chosen as an absorbent due to its silicate structure with high content of silica. Moreover, the small size particle as compared with micrometer inorganic additives is an advantage of the YPS. Hence, the obtained YPS could be expected to use as an absorbent for removing toxicity substances in aqueous solutions. In this paper, chromium (VI) and methylene blue have been chosen as the model substances to study the adsorption ability of YPS. Chromium, commonly found in various sources of industrial waste water, is one of the most toxic metal ions, which influences seriously the biodiversity of the environment and causes several health issues to humans. Chromium often comes from discharge of industrial activities such as leather tanning, electroplating, or textiles [14]. It exists in water with various oxidation forms, but mainly in trivalent and hexavalent state [15], in which the hexavalent state is considered the most toxic because it is easily dilution and can bioaccumulate in human organs [16]. Some studies reveal that Cr (VI) ions can cause digestive system and lungs cancer, gastrointestinal and dermatological problems, severe diarrhea, and hemorrhage [17][18][19]. Many materials have been utilized to adsorb Cr (VI) ions in aqueous solutions including banana peel [20], coffee resins [21], fly ash [22], groundnut hull [23], or zeolite NaX [24] and showed good results.
Dye has been an important ingredient in many common daily industries such as textile, leather, cosmetics, plastics, and food production [25]. Nevertheless, colored dye waste water constitutes considerable issues to the environment and water sources [26]. Complex aromatic molecular structures of dyes make them nondegradable [27]. Dyes, which have high demand for chemical and biological oxygen, high toxicity, and capability to hinder sunlight penetration into water bodies, are harmful pollutants to the aquatic ecosystem [28]. Methylene blue (MB), a cationic dye, is widely used in biology, medical science, chemistry, and dye field. However, long-term exposure to MB can cause certain symptoms and illnesses such as increased heart rate, vomiting, nausea, anemia, cyanosis, and tissue necrosis [29,30]. Various adsorbents have been used to adsorb MB in aqueous solutions with promising output such as activated carbon [29], natural clay [31], sea grass dead leaves [32], or modified pumice stone [33].
According to our calculation, the price of one tone of YPS at the Tang Loong Industrial Zone is only about 22 USD. is indicates that YPS product is cost-effective and promising for application not only as an absorbent but also as an additive for other fields (composites, paint, coating, etc.). Acids and bases are used for treatment of inorganic waste, for example, fly ash and gypsum, to improve the adsorption ability of these waste products [18,20,22,23]. Besides, EDTA is known as a chemical used for both industrial and medical purposes. In the industry, it is mainly used to sequester metal ions in aqueous solution. anks to its high affinity for metal ions, EDTA can enormously enhance the chelation properties of the adsorbent. erefore, in this work, NaOH, HNO 3 , and EDTA were chosen for retreatment of YPS particles to evaluate their adsorption ability. We mainly focused on the characterization of YPS products as well as investigation of the factors affecting on the adsorption ability of YPS products for removal of chromium (VI) ions and methylene blue in aqueous solutions.

Treatment of Yellow Phosphorus Slag by Flotation
System. Firstly, the washing flotation system was used to remove preliminary soluble impurities and to separate the particles for next stage. In this stage, the large content of FeP, P 2 O 5 , fluorine compounds, and some other impurities were removed and the YPS0 was then wet sieved down to prepare a granular material which is smaller than 100 µm in diameter (YPS1) (by sieve analysis). ese particles could be applied for cement production or concrete directly. In the next stage, the particles were milled and transferred to a float sorting system to obtain particles in smaller size. e solid part was then rotated in a spinning double-drum composter and dried at 100°C until unchanged weight. e product was designed as YPS2 with the calcium silicate content in particles higher than 90%. e waste water system was treated to recover P 2 O 5 , fluorine compounds, and minerals for other applications.
e BET surface area/t-plot micropore area, pore diameter, and pore volume of YPS2 product are 1.3145 m 2 g −1 /0.3024 m 2 g −1 , 21.4897 nm, and 0.000134 cm g −1 , respectively (determined by the nitrogen adsorption method on a TriStar 3000 V6.07 A device).

Surface Treatment of Yellow Phosphorus Slag (YPS) Using NaOH and HNO 3 Solutions.
e YPS particles were retreated by NaOH or HNO 3 solution as follows: 200 mL of NaOH 1 M (or HNO 3 1 M) solution was added into a flask containing 20 g of YPS particles and stirred at 70°C for 3 hours. en, the treated YPS particles by NaOH (or HNO 3 ) solution were filtered and washed with distilled water until filtered aqueous solution reached to neutral medium (pH 7). After that, the treated YPS particles were dried in an oven at 100°C for 12 hours. e YPS0 particles and YPS2 particles which were treated with NaOH or HNO 3 solution were designed as YPS0-NaOH, YPS2-NaOH, YPS0-HNO 3 , and YPS2-HNO 3 .

Surface Treatment of Yellow Phosphorus Slag (YPS)
Using EDTA. In this research, YPS was modified by using EDTA as follows: 5 g of YPS was added into 100 mL distilled water in a 250 mL glass beaker containing 0.5 g of EDTA.
is solution was then stirred on a magnetic machine at a speed of 500 rpm for 2 hours at 60°C. Next, the solution was filtered to obtain the solid part. Finally, the solid part was dried in an oven at 100°C for 3 hours.

Infrared Spectroscopy (IR)
. IR spectra of YPS samples were recorded using a Nicolet iS10 spectrometer ( ermo Scientific, USA) in the range of wavenumbers from 4000 cm −1 to 400 cm −1 , resolution of 8 cm −1 , and scan average of 32 times. (EDX). EDX spectra of the YPS samples were carried out on a SEM/EDS device (Oxford Instruments, UK).

Scanning Electron Microscopy (SEM).
Scanning electron microscopy (SEM) of YPS samples was taken on a SEM-S-4800 device (Hitachi, Japan). e samples were coated a Pt layer on the surface to enhance the resolution of images. (XRD). XRD patterns of YPS samples were performed on a Siemens D5000 X-ray diffractometer (XRD) with CuK α radiation source (λ � 0.154 nm) at 40 kV generator voltage with 0.03°step and 30 mA current by 0.043°/s scan speed in the range of 2θ from 2°to 70°.

X-Ray Diffraction Analysis
2.3.6. Zeta Potential. Zeta potential of the YPS2 sample was conducted on a Zetasizer, ver. 6.2, Malvern Instruments, with zeta runs of 12, count rate (kcps) of 288.7, and measurement position of 4.5 mm at 25°C. e YPS2 was dispersed in water (pH ≈ 7) with its dispersant RI of 1.330, viscosity of 0.8872 cP, and dispersant dielectric constant of 78.5.

Ultraviolet-Visible (UV-Vis) Absorption Spectrometry.
Spectra of samples were determined on a UV spectrophotometer (CINTRA 40, GBC, USA) in the range of wavelength from 200 to 800 nm.

Determination of Adsorption Ability of Yellow Phosphorus Slag in Aqueous
Solution. An exact weight of the YPS samples was added into a 100 mL of Cr (VI) or MB solution. e solution was stirred on a magnetic stirrer at room temperature for 120 minutes. e solution was then filtered, and 25 mL of aliquots was withdrawn. For MB adsorption, the withdrawn solution was monitored by a UV-Vis spectrophotometer (CINTRA 40, GBC, USA) at λ max � 664 nm. For Cr (VI) adsorption, 1 mL of H 2 SO 4 1M and 1 mL of DCP 0.5% solution were introduced into the withdrawn solution and this solution was kept for 10 minutes before taking on a UV-Vis spectrophotometer at λ max � 540 nm. All studies were performed in triplicate to increase accuracy.

Adsorption of Cr (VI) Ions and Methylene Blue Using YPS Samples.
e amount of adsorbate per amount of adsorbent at equilibrium condition, Q (mg/g), was calculated as follows: where C o and C e are the concentration of adsorbate in solution at initial and equilibrium (mg/L), V is the solution volume (L), and W is the mass of YPS samples (g). e percentage of metal ions removed, H (%), was calculated using the following equation: (2)

Adsorption Isotherms.
In this work, we study the adsorption behavior in the solid-liquid system using four adsorption isotherms: Langmuir, Freundlich, Temkin, and Dubinin-Radushkevich isotherms.
Langmuir isotherm equation for ion adsorption: where Q o is the maximum monolayer adsorption capacity (mg/g) and k L is the Langmuir isotherm constant representing binding energy of the adsorption system (L/mg). Freundlich isotherm equation: where k F is the Freundlich isotherm constant (mg/g) indicating adsorption capacity and n F is adsorption intensity. Temkin isotherm equation: where A T is the Temkin isotherm equilibrium binding constant (L/g), b T is the Temkin isotherm constant related to heat sorption (J/mg), T is absolute temperature (K), and R is the gas constant (8.314 J/mol/K). Dubinin-Radushkevich (DR) isotherm equation: where Q s is the theoretical isotherm saturation capacity (mg/g) and K ad is the Dubinin-Radushkevich isotherm constant (mol 2 /kJ 2 ).

Adsorption Kinetics.
Adsorption kinetics were studied using four reaction models: first-order, pseudo-first-order, second-order, and pseudo-second-order reaction models.
First-order reaction model: Pseudo-first-order reaction model: Second-order reaction model: Pseudo-second-order reaction model: where Q o is the maximum monolayer coverage capacity (mg/g); Q e and Q t are the amount of adsorbate adsorbed per gram of adsorbent at equilibrium time and testing time t (mg/g); C o and C t are the solution concentration at the initial time and the testing time t (mg/l); and k 1 , k s1 , k 2 , and k s2 are the rate constant (per minute) of the first-order reaction model, pseudo-firstorder reaction model, second-order reaction model, and pseudo-second-order reaction model, respectively.  Figure 2 presents SEM/EDX images of the YPS samples. By observing the SEM images of the samples, it can be seen that after treatment by water and milling, the size of YPS particles was reduced significantly. So, this technology is suitable for obtaining the YPS particles with finer size. From the EDX spectra and data in Table 1, the YPS samples are mainly composed of O, Ca, and Si (total content of O + Ca + Si over 90%). Other elements such as Mg, K, S, P, and F were also appeared in all YPS samples with the percentage of each element less than 2%. Additionally, rare earth elements that are highly chemical active such as Pm, Sm, Ce, Pr, and Nd occupy a relatively high content in the sample. Furthermore, the pretreatment process does not affect much on the content of most of the elements. e crystallographic structure of YPS samples before and after treatment was determined by using the X-ray diffraction method. e results of XRD analysis of YPS particles are performed in Figures 3-5. Figure 3 shows the XRD pattern of the raw YPS sample. In the XRD pattern of the YPS0 sample, the appearance of calcium phosphate β crystal and hatrurite crystal (ref. PDF 00-009-0346 and 01-073-0599) was observed. e peak intensity of calcium phosphate β crystal in the XRD pattern of YPS0 is stronger than that of hatrurite crystal, indicating that calcium phosphate β crystal makes up the most part in the crystallographic structure of the YPS0 sample. After treating according to the first stage to eliminate impurities, the YPS1 sample contains calcium phosphate β crystals (ref. PDF 00-009-0346) and the hatrurite crystal was removed. e YPS2 sample only contains calcium phosphate β crystals. is result proved that the calcium phosphate was detached after treatment process. e diffraction peaks characterized for calcium phosphate β crystals in the XRD pattern of YPS samples were placed at the diffraction angles, 2θ � 20.53°, 31.78°, and 55.92°corresponding to the crystal size of 4.32Å, 2.81Å, and 1.64Å, respectively.    Other metal elements such as Al, Fe, and Mn occupy a very small part in the sample, but they were still remained after treatment process. As mentioned above, the above YPS samples also contain rare earth metals and the treatment process did not affect much on their content in YPS samples. is is in agreement with the publication of Ming et al. [35]. Figure 6 expresses FESEM images of YPS0 and YPS2 samples at magnification of 5000 times and 50000 times. It is clear that the wet milling can reduce the size of the YPS particles, making them finer in size. After treatment, the common particle size of YPS2 particles is about 10 µm. Furthermore, many particles of size 100-400 nm can be observed on the surface of these particles (Figures 6(b) and 6(d)).   3.1.6. Zeta Potential. Figure 7 shows the zeta potential distribution diagram of the YPS2 sample. It can be seen that YPS2 particles had a negative charge ranged in −30 mV-0 mV with a mean value of −15.3 mV. e negative charge on the surface of YPS2 can be due to the presence of CaO and calcite in composition of YPS2. Table 3 shows Cr (VI) ion removal efficiency (H) and amount of Cr (VI) ions removed per gram of YPS samples before and after treatment by NaOH, HNO 3 , and EDTA solutions (Q). e adsorption condition is fixed as follows: the weight of adsorbent is 0.5 gram, concentration of Cr (VI) ions is 10 ppm, and adsorption time is 120 minutes. It is clear that the YPS0 and modified raw YPS samples treated by NaOH and HNO 3 solutions displayed poor Cr (VI) ion adsorption ability with the removal efficiencies are all less than 11% (no. 1, no. 4, and no. 5), hence not suitable for adsorption process, and further treatment of the YPS samples is necessary.

Chromium (VI) Ion Adsorption Ability of YPS Particles.
e raw YPS sample after water treatment (YPS1) presented much higher adsorption ability,    Journal of Chemistry about 7 times higher than that of the raw sample (no. 2). It is noteworthy that the YPS2 sample also showed good adsorption ability with the Cr (VI) ion removal efficiency of 41.16% (no. 3) and this sample is chosen to be modified by HNO 3 , NaOH, and EDTA solutions for further Cr (VI) ion adsorption study. However, the modified YPS2 samples using HNO 3 solution and EDTA exhibited a decrease in the percentage of removed Cr (VI) ions (no. 6 and no. 8) while  the modified YPS2 sample using NaOH solution showed a slight improvement (no. 7). e reduction of Cr (VI) ion adsorption ability by retreated YPS may be due to surface erosion/corrosion of the YPS particles in acid and base environment. e presence of EDTA can lead to the covering of the surface of YPS particles and limit the Cr (VI) ion adsorption. erefore, in this study, the YPS2 sample without any further modification will be used for the following experiments.

Assessment on Chromium (VI) Ion Adsorption Ability of Yellow Phosphorus Slag Samples (1) Effect of Some Experiment Conditions on Chromium (VI) Ion Adsorption Process.
e effect of different factors in experimental process such as pH, temperature, YPS2 adsorbent weight, adsorption time, and initial Cr (VI) ion concentration on Cr (VI) ion adsorption process is investigated. e obtained results are listed in Tables 4-8. (i) Effect of pH Table 4 shows the changes in Cr (VI) ion removal efficiency of YPS2 samples when the solution pH is altered from 2 to 7 while the other conditions were fixed (0.5 g of adsorbent and 120 minutes of adsorption time). e Cr (VI) ion adsorption capacity of YPS2 is low for pH less than or equal 6 with the removal efficiency smaller than 10%. Among investigated solutions, the solution having pH 7 is most suitable for the highest percentage of Cr (VI) ions adsorbed by the YPS2 sample and the H value of 20.33%, and the amount of Cr (VI) ions adsorbed per gram of the YPS2 sample is 0.407 mg. e pH higher than 7 was not studied due to the unstableness of Cr (VI) ions in the alkaline environment [14]. (ii) Effect of adsorbent weight Table 5 indicates the effect of adsorbent weight on the Cr (VI) ion adsorption process using YPS2 samples. e mass of adsorbent was changed from 0.1 g to 1.0 g, the pH of solution was 7. and the adsorption time was 120 minutes. It can be seen that adsorbent mass of 1.0 g presented the lowest Cr (VI) ion removal efficiency and the amount of Cr (VI) ions removed per gram of the YPS2 sample. e others showed good adsorption ability with the percentage of Cr (VI) ions removed were higher than 20%. e highest Cr (VI) ion removal efficiency is achieved using 0.5 g of YPS2 (H = 41.16%).    Journal of Chemistry (iii) Effect of temperature Table 6 presents the change in Cr (VI) ion adsorption ability when the experimental temperature is changed from room temperature (26°C) to 40°C and 60°C, pH 7 solution, adsorbent weight of 0.5 g, and each experiment was carried out in 120 minutes. e highest amount of Cr (VI) ion removal percentage is obtained at room temperature with the H value of 20.33%. e Cr (VI) ion adsorption capacity of YPS2 was decreased significantly with the increasing adsorption temperature. (iv) Effect of adsorption time Table 7 displays the effect of adsorption time on the Cr (VI) ion adsorption process using YPS2 samples. e adsorption time was changed from 30 to 180 minutes with the optimal adsorbent weight, pH, and temperature. From 30 minutes to 120 minutes, the Cr (VI) ion adsorption efficiency was increased and reached the highest removal percentage of 30.53% for 120 minutes. is can be explained as the adsorption is the process of heavy metal ions being adsorbed onto the surface of the adsorbent and the longer the reaction time, the more the metal ions being adsorbed. However, after 150 minutes, the Cr (VI) ion removal efficiency dropped remarkably, this may due to the saturated state on the YPS2 sample surface.
(v) Effect of initial Cr (VI) ion concentration Table 8 describes the effect of initial Cr (VI) ion concentration (changing from 10 mg/L to 100 mg/ L) on Cr (VI) ion adsorption ability of YPS2. As can be seen in Table 8, the highest Cr (VI) ion removal efficiency occurred with the initial concentration of 10 mg Cr (VI) per 1L of solution with the amount of removed ions is 0.407 mg per 1 g of slag and H = 20.33%. When initial Cr (VI) ion concentration was increased to 50 mg/L, the Cr (VI) ion adsorption capacity was slightly decreased. en, it was dropped significantly when the initial Cr (VI) ion concentration is 80 mg/L and 100 mg/L. is shows that the Cr (VI) ion adsorption ability of YPS2 is higher at low initial concentration of Cr (VI) ion solution. From all the tables above, we can see that the Cr (VI) ion adsorption capacity of YPS2 samples is not good with the adsorption efficiency less than 50%, so further study on adsorption isotherms and adsorption kinetics will not be carried out in this paper.

Assessment on Methylene Blue Adsorption Ability of
Yellow Phosphorus Slag Samples. Similar to Cr (VI) ion adsorption process using YPS2 samples, some experimental conditions such as pH, adsorbent weight, adsorption temperature, time, and initial concentration of methylene blue (MB) solution were investigated to determine the most suitable condition for MB adsorption process. e results of removal efficiency and amount of MB removed per gram of YPS2 are listed in Tables 9-13.
(1) Effect of Some Conditions on the Methylene Blue Adsorption Process.
(i) Effect of pH Table 9 describes the effect of pH on the MB adsorption process using YPS2 samples. It is clear that the MB adsorption ability of YPS2 samples was high for all the tested pH with the percentages of MB removed were all more than 90%. Among the examined pH, the highest MB removal efficiency was observed at pH 3 (H � 98.20%), followed at pH 7 (H � 97.63%). However, since the adsorption process was in aqueous solution, the high acidity environment was undesirable, so the pH � 7 was chosen for the further experiments.
(ii) Effect of adsorbent weight Table 10 demonstrates the MB removal efficiency when the adsorbent weight was changed from 0.2 g to 1.0 g. All tested samples exhibited high percentage of removed MB. While using 0.2 g of YPS2, the highest amount of removed MB per gram of YPS2 adsorbent used (Q) was 4.692 mg/g. While using 0.4 g of YPS2, the highest percentage of removed MB (H) was 97.63%. is can be caused by the different contact of the adsorbent and MB   is might also be due to the saturation on the surface of YPS2 samples. e same pattern was observed with the pH 4 solution and the highest MB removal efficiency of 98.20% after 120 minutes of adsorption time. It can be seen from this table that there is a slight difference in the percentage of MB removed by the YPS2 sample in pH 4 and pH 7; however, after 120 minutes of testing, the YPS2 sample exhibited a good MB adsorption ability. erefore, the suitable time for the MB adsorption study by the YPS2 sample is 120 minutes.
(v) Effect of initial MB concentration Table 13 displays the changes in the percentage of removed MB by using YPS2 samples when the initial MB concentration was altered from 5 mg/L to 25 mg/L. e highest MB removal efficiency was obtained when the initial MB concentration was 10 mg/L (H � 97.63%). When the initial MB concentration was increased, the MB adsorption capacity of YPS2 was decreased. Figure 8 shows IR spectra of the YPS2 sample before and after absorbing MB. e presence of MB in YPS2 was reflected by the increase of intensity and the shift of peak at around 1450 cm −1 (1456 cm −1 for the YPS2 sample and 1443 cm −1 for the YPS2-absorbed MB sample). is is due to the consonance of bending vibration of the CH 3 group and aromatic C�C of MB with the stretching vibration of the CO 2− 3 group in calcite in YPS2. Moreover, the stretching vibrations of C�N and benzene zing were found at 1594 cm −1 and 1660 cm −1 , respectively. ese evidences proved that MB was absorbed onto the YPS2 sample. A hypothesis model for the adsorption of MB by YPS2 particles is shown in Figure 9 [37]. Figure 10 and Table 14 show the parameters of MB adsorption process using YPS according to four isotherm models: Langmuir, Freundlich, Temkin, and Dubinin-Radushkevich. It is clear that the adsorption isotherm of MB adsorption process using YPS follows the Langmuir model with the highest correlation coefficient R 2 � 0.96 which indicated that the     adsorption process is in the monolayer. e separation factor R L � 0.434, smaller than 1, also expressed that the equilibrium adsorption to be in favor. e Freundlich model also demonstrated a relatively high correlation coefficient R 2 � 0.925, with the adsorption intensity n � 1.422 to display the favorable sorption process. e other isotherm models did not fit well with the MB adsorption process using YPS. Table 15 lists the Langmuir, Freundlich, Temkin, and Dubinin-Radushkevich isotherm constants of MB adsorption using YPS. It can be recognized that the maximum adsorption capacity (Q o ) of YPS for the removal of MB is 22.989 mg·g −1 . As comparison with the Q o of other adsorbents, for example, orange peel, banana peel, natural clay, and fly ash in Table 16, the Q o value of YPS is quite good. is confirms that YPS is a potential absorbent for the removal of MB in aqueous solution.

Methylene Blue Adsorption
Kinetics. MB adsorption kinetics were studied using four linear adsorption kinetic models as represented in Figure 11.
From Figure 11, we can see that all four linear reaction models show good fitting to the adsorption process of MB using YPS with the correlation coefficient R 2 all greater than 0.98. However, the best fit model is the pseudo-second-order reaction model with R 2 equal to 0.9999. is is in agreement with publications of MB adsorption using activated carbon from tea seed shells or Ficus carica bast, using seaweed or modified pumice stone [28,29,32,33].

Methylene Blue Adsorption
ermodynamics. ermodynamics of MB adsorption process of YPS2 can be calculated according to equations (2)-(4) as reported by Kunde et al. [37] or equations (2) and (3) as reported by Yuh-Shan [40] as follows: where R is the universal gas constant, T is absolute temperature, ΔG o is Gibbs free energy change, ΔH o is enthalpy change, ΔS o is entropy change, and K a is the Langmuir constant which was calculated as suggested in References [40,41]. Herein, isotherm data were analyzed at 303, 313, and 323 K. From K a values obtained from Langmuir isotherms at different temperatures, three ΔG o values were calculated and are presented in Table 17. It can be seen that the ΔG o values       [37]. From the plot of the ΔG o values versus T in Figure 12 (R 2 � 0.9535), ΔH o and ΔS o were also calculated and are listed in Table 17. e negative ΔH o indicating that the sorption reaction is exothermic and the negative ΔS o value showed a decrease in the randomness at the solid/solution interface during the sorption process of MB onto YPS2.

Conclusion
In conclusion, the yellow phosphorus slag (YPS) after being washed with water and wet milled (YPS2) showed a finer particle size and a good adsorption ability of chromium (VI) and methylene blue (MB). e surface of YPS2 has a negative charge. e main composition of YPS2 is calcite, and main oxides of YPS2 are SiO 2 and CaO. e most suitable condition for the chromium (VI) adsorption process was as follows: solution pH of 7, adsorption time of 120 minutes,   and the chromium (VI) initial concentration of 10 mg/L. e neutral pH environment will not create secondary pollution. For chromium (VI) ion adsorption, YPS was not a suitable adsorbent due to low adsorption efficiency, less than 50%. In the case of MB, treated YPS was a promising adsorption material with high MB removal percentage, over 85%. e FTIR spectrum of YPS2-absorbed MB confirmed that MB was absorbed onto YPS2. e adsorption isotherm of MB adsorption process using YPS2 follows the Langmuir isotherm with R 2 � 0.96, and the adsorption kinetic fits well with the pseudo-second-order reaction model with R 2 � 0.999. e obtained thermodynamic parameters confirmed that the MB adsorption process onto YPS2 is favorable spontaneous adsorption. ese results were also in agreement with others research studies on MB adsorption process using various adsorbents.

Data Availability
e data used to support the findings of this study are included within the article.

Conflicts of Interest
e authors declare that there are no conflicts of interest.