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

Authors: Van Hai Nguyen; Van Chien Nguyen; Thuy Chinh Nguyen; Do Mai Trang Tran; Thi Thu Trang Nguyen; Quoc Trung Vu; Duy Trinh Nguyen; Hoang Thai
Journal: Journal of Chemistry
 (2020)

---

## Abstract

Yellow phosphorus is used widely in the world for production of phosphoric acid, various phosphates, flame retardant, detergent, water treatment, metal surface treatment, etc. After the production of yellow phosphorus, a large amount of phosphorus sludge is discharged to environment, causing environment pollution. This work focused on treatment of yellow phosphorus slag (YPS) and application of it as an absorbent for chromium (VI) ion and methylene blue. The YPS was first washed with water to remove phosphoferrite (FeP) and impurities and then being milled and transferred to a float sorting system to obtain YPS particles. The characteristics of YPS particles were determined by inductively coupled plasma-mass-spectrometry (ICP-MS), energy-dispersive X-ray spectroscopy (EDX), infrared spectroscopy (IR), scanning electron microscopy (SEM), X-ray diffraction (XRD), zeta potential, and nitrogen adsorption methods. The YPS particles were retreated with NaOH, HNO3, and EDTA solutions to evaluate the influence of these agents on metal ion and organic compound adsorption ability by YPS. The adsorption parameters of chromium (VI) ion and methylene blue (MB) by treated YPS particles were recognized by the ultraviolet-visible (UV-Vis) spectrometer. The effects of temperature, pH solution, and initial concentration of absorbed substances on the adsorption ability were investigated. The adsorption isotherms and adsorption kinetics of chromium (VI) ion and MB by YPS particles were also determined. The obtained results confirmed that the green technology used to treat the YPS2 particles is suitable to obtain an effective absorbent. The adsorption efficiency of YPS2 particles for removal of chromium (VI) ions is smaller than that for removal of MB in aqueous solutions. The adsorption isotherm of MB adsorption process is complied with the Langmuir isotherm while the adsorption kinetic fits well with the pseudo-second-order reaction model. The thermodynamic parameters of MB adsorption processed on YPS2 were calculated and discussed.


---

## Body

## 1. Introduction

Yellow phosphorus slag (YPS) is a waste product of manufacturing yellow phosphorus (P4) using the electrical furnace method at 1400°C–1600°C [1]. The worldwide yellow phosphorus production yields an average of 1.5 million tons of P4 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 P4, about 8 to 10 tons of yellow phosphorus slag are produced [1]. This waste product is often left accumulated in the landfills, proposing a potential pollution thread to the environment. The majority of YPS particles compose of CaO and SiO2, accounting for approximately 85% of the slag mass [3]. Other components of the YPS are Al2O3, Fe2O3, MgO, and some rare earth metals [4, 5]. In Vietnam, the P4 is mainly produced and supplied by Lao Cai Yellow Phosphorus JSC (Tang Loong Industrial Zone, Bao Thang District, Lao Cai Province, Vietnam), with the productivity of 93,800 tons P4/year and about 750,000–1,031,000 tons of YPS waste are produced and released directly into the surrounding environment [6]. Therefore, 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 [11–13]. 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. This is a combination of the water washing flotation system with milling and sorting flotation. The waste water system was treated to recover P2O5, F, and minerals for other applications. The 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%). The minimized weight of chemicals was used, and treatment process was carried in room temperature. This approached to the green technology, the general trend of the world.The 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 [17–19]. 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. This 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. Thanks to its high affinity for metal ions, EDTA can enormously enhance the chelation properties of the adsorbent. Therefore, in this work, NaOH, HNO3, 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.


## 2. Experiment

### 2.1. Materials

Yellow phosphorus slag (YPS0) is waste product of Lao Cai Yellow Phosphorus JSC (Tang Loong Industrial Zone, Bao Thang District, Lao Cai Province, Vietnam) with a particle size of 50–100µm; density of 2.75 g/cm3; hardness of 1–3; compressive strength of 80–100 MPa; water absorption of 1–4%; and porosity of 10–12%. Ethylenediaminetetraacetic acid (EDTA); 1,5-diphenylcarbazide (DCP); potassium chromate; and methylene blue (MB) were purchased from Merck Co. HNO3 and NaOH are the commercial products which are used as received.


### 2.2. Surface Treatment of Yellow Phosphorus Slag

#### 2.2.1. 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, P2O5, 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). These 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. The solid part was then rotated in a spinning double-drum composter and dried at 100°C until unchanged weight. The product was designed as YPS2 with the calcium silicate content in particles higher than 90%. The waste water system was treated to recover P2O5, fluorine compounds, and minerals for other applications. The BET surface area/t-plot micropore area, pore diameter, and pore volume of YPS2 product are 1.3145 m2g−1/0.3024 m2g−1, 21.4897 nm, and 0.000134 cm³g−1, respectively (determined by the nitrogen adsorption method on a TriStar 3000 V6.07 A device).


#### 2.2.2. Surface Treatment of Yellow Phosphorus Slag (YPS) Using NaOH and HNO3 Solutions

The YPS particles were retreated by NaOH or HNO3 solution as follows: 200 mL of NaOH 1 M (or HNO3 1 M) solution was added into a flask containing 20 g of YPS particles and stirred at 70°C for 3 hours. Then, the treated YPS particles by NaOH (or HNO3) 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. The YPS0 particles and YPS2 particles which were treated with NaOH or HNO3 solution were designed as YPS0-NaOH, YPS2-NaOH, YPS0-HNO3, and YPS2-HNO3.


#### 2.2.3. 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. This 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.


### 2.3. Characterizations

#### 2.3.1. Infrared Spectroscopy (IR)

IR spectra of YPS samples were recorded using a Nicolet iS10 spectrometer (Thermo 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.


#### 2.3.2. Energy-Dispersive X-Ray Spectroscopy (EDX)

EDX spectra of the YPS samples were carried out on a SEM/EDS device (Oxford Instruments, UK).


#### 2.3.3. Inductively Coupled Plasma-Mass-Spectrometry (ICP-MS)

The element content of YPS samples was detected by NexION 2000 ICP-DRC-QMS (Perkin Elmer, USA).


#### 2.3.4. Scanning Electron Microscopy (SEM)

Scanning electron microscopy (SEM) of YPS samples was taken on a SEM-S-4800 device (Hitachi, Japan). The samples were coated a Pt layer on the surface to enhance the resolution of images.


#### 2.3.5. X-Ray Diffraction Analysis (XRD)

XRD patterns of YPS samples were performed on a Siemens D5000 X-ray diffractometer (XRD) with CuKα 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°.


#### 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. The 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.


#### 2.3.7. 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.


### 2.4. 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. The solution was stirred on a magnetic stirrer at room temperature for 120 minutes. The 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) atλmax = 664 nm. For Cr (VI) adsorption, 1 mL of H2SO4 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 λmax = 540 nm. All studies were performed in triplicate to increase accuracy.


### 2.5. Determination of Cr (VI) Ion and Methylene Blue Adsorption Isotherms and Adsorption Kinetics of Yellow Phosphorus Slag

#### 2.5.1. Adsorption of Cr (VI) Ions and Methylene Blue Using YPS Samples

The amount of adsorbate per amount of adsorbent at equilibrium condition,Q (mg/g), was calculated as follows:(1)Q=Co−Ce⋅VW,where Co and Ce 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).The percentage of metal ions removed,H (%), was calculated using the following equation:(2)H=Co−Ce⋅100Ce.


#### 2.5.2. 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:(3)Qe=QoKLCe1+KLCe,whereQo is the maximum monolayer adsorption capacity (mg/g) and kL is the Langmuir isotherm constant representing binding energy of the adsorption system (L/mg).Freundlich isotherm equation:(4)Qe=kFCe1/nF,wherekF is the Freundlich isotherm constant (mg/g) indicating adsorption capacity and nF is adsorption intensity.Temkin isotherm equation:(5)Qe=BlnAT+BlnCe,withB=RTbT,whereAT is the Temkin isotherm equilibrium binding constant (L/g), bT 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:(6)lnQe=lnQs−Kadε2,withε=RTln1+1Ce,whereQs is the theoretical isotherm saturation capacity (mg/g) and Kad is the Dubinin–Radushkevich isotherm constant (mol2/kJ2).


#### 2.5.3. 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:(7)lnCt=lnCo−k1t.Pseudo-first-order reaction model:(8)lnQo−Qt=lnQo−ks1t.Second-order reaction model:(9)1Ct=1Co+k2t.Pseudo-second-order reaction model:(10)1Qe−Qt=1Qe+ks2t⟶tQt=1h+1Qet,withh=ks2Qe2,whereQo is the maximum monolayer coverage capacity (mg/g); Qe and Qt are the amount of adsorbate adsorbed per gram of adsorbent at equilibrium time and testing time t (mg/g); Co and Ct are the solution concentration at the initial time and the testing time t (mg/l); and k1,ks1,k2,andks2 are the rate constant (per minute) of the first-order reaction model, pseudo-first-order reaction model, second-order reaction model, and pseudo-second-order reaction model, respectively.


## 2.1. Materials

Yellow phosphorus slag (YPS0) is waste product of Lao Cai Yellow Phosphorus JSC (Tang Loong Industrial Zone, Bao Thang District, Lao Cai Province, Vietnam) with a particle size of 50–100µm; density of 2.75 g/cm3; hardness of 1–3; compressive strength of 80–100 MPa; water absorption of 1–4%; and porosity of 10–12%. Ethylenediaminetetraacetic acid (EDTA); 1,5-diphenylcarbazide (DCP); potassium chromate; and methylene blue (MB) were purchased from Merck Co. HNO3 and NaOH are the commercial products which are used as received.


## 2.2. Surface Treatment of Yellow Phosphorus Slag

### 2.2.1. 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, P2O5, 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). These 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. The solid part was then rotated in a spinning double-drum composter and dried at 100°C until unchanged weight. The product was designed as YPS2 with the calcium silicate content in particles higher than 90%. The waste water system was treated to recover P2O5, fluorine compounds, and minerals for other applications. The BET surface area/t-plot micropore area, pore diameter, and pore volume of YPS2 product are 1.3145 m2g−1/0.3024 m2g−1, 21.4897 nm, and 0.000134 cm³g−1, respectively (determined by the nitrogen adsorption method on a TriStar 3000 V6.07 A device).


### 2.2.2. Surface Treatment of Yellow Phosphorus Slag (YPS) Using NaOH and HNO3 Solutions

The YPS particles were retreated by NaOH or HNO3 solution as follows: 200 mL of NaOH 1 M (or HNO3 1 M) solution was added into a flask containing 20 g of YPS particles and stirred at 70°C for 3 hours. Then, the treated YPS particles by NaOH (or HNO3) 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. The YPS0 particles and YPS2 particles which were treated with NaOH or HNO3 solution were designed as YPS0-NaOH, YPS2-NaOH, YPS0-HNO3, and YPS2-HNO3.


### 2.2.3. 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. This 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.


## 2.2.1. 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, P2O5, 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). These 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. The solid part was then rotated in a spinning double-drum composter and dried at 100°C until unchanged weight. The product was designed as YPS2 with the calcium silicate content in particles higher than 90%. The waste water system was treated to recover P2O5, fluorine compounds, and minerals for other applications. The BET surface area/t-plot micropore area, pore diameter, and pore volume of YPS2 product are 1.3145 m2g−1/0.3024 m2g−1, 21.4897 nm, and 0.000134 cm³g−1, respectively (determined by the nitrogen adsorption method on a TriStar 3000 V6.07 A device).


## 2.2.2. Surface Treatment of Yellow Phosphorus Slag (YPS) Using NaOH and HNO3 Solutions

The YPS particles were retreated by NaOH or HNO3 solution as follows: 200 mL of NaOH 1 M (or HNO3 1 M) solution was added into a flask containing 20 g of YPS particles and stirred at 70°C for 3 hours. Then, the treated YPS particles by NaOH (or HNO3) 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. The YPS0 particles and YPS2 particles which were treated with NaOH or HNO3 solution were designed as YPS0-NaOH, YPS2-NaOH, YPS0-HNO3, and YPS2-HNO3.


## 2.2.3. 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. This 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.


## 2.3. Characterizations

### 2.3.1. Infrared Spectroscopy (IR)

IR spectra of YPS samples were recorded using a Nicolet iS10 spectrometer (Thermo 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.


### 2.3.2. Energy-Dispersive X-Ray Spectroscopy (EDX)

EDX spectra of the YPS samples were carried out on a SEM/EDS device (Oxford Instruments, UK).


### 2.3.3. Inductively Coupled Plasma-Mass-Spectrometry (ICP-MS)

The element content of YPS samples was detected by NexION 2000 ICP-DRC-QMS (Perkin Elmer, USA).


### 2.3.4. Scanning Electron Microscopy (SEM)

Scanning electron microscopy (SEM) of YPS samples was taken on a SEM-S-4800 device (Hitachi, Japan). The samples were coated a Pt layer on the surface to enhance the resolution of images.


### 2.3.5. X-Ray Diffraction Analysis (XRD)

XRD patterns of YPS samples were performed on a Siemens D5000 X-ray diffractometer (XRD) with CuKα 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°.


### 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. The 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.


### 2.3.7. 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.


## 2.3.1. Infrared Spectroscopy (IR)

IR spectra of YPS samples were recorded using a Nicolet iS10 spectrometer (Thermo 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.


## 2.3.2. Energy-Dispersive X-Ray Spectroscopy (EDX)

EDX spectra of the YPS samples were carried out on a SEM/EDS device (Oxford Instruments, UK).


## 2.3.3. Inductively Coupled Plasma-Mass-Spectrometry (ICP-MS)

The element content of YPS samples was detected by NexION 2000 ICP-DRC-QMS (Perkin Elmer, USA).


## 2.3.4. Scanning Electron Microscopy (SEM)

Scanning electron microscopy (SEM) of YPS samples was taken on a SEM-S-4800 device (Hitachi, Japan). The samples were coated a Pt layer on the surface to enhance the resolution of images.


## 2.3.5. X-Ray Diffraction Analysis (XRD)

XRD patterns of YPS samples were performed on a Siemens D5000 X-ray diffractometer (XRD) with CuKα 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°.


## 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. The 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.


## 2.3.7. 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.


## 2.4. 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. The solution was stirred on a magnetic stirrer at room temperature for 120 minutes. The 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) atλmax = 664 nm. For Cr (VI) adsorption, 1 mL of H2SO4 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 λmax = 540 nm. All studies were performed in triplicate to increase accuracy.


## 2.5. Determination of Cr (VI) Ion and Methylene Blue Adsorption Isotherms and Adsorption Kinetics of Yellow Phosphorus Slag

### 2.5.1. Adsorption of Cr (VI) Ions and Methylene Blue Using YPS Samples

The amount of adsorbate per amount of adsorbent at equilibrium condition,Q (mg/g), was calculated as follows:(1)Q=Co−Ce⋅VW,where Co and Ce 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).The percentage of metal ions removed,H (%), was calculated using the following equation:(2)H=Co−Ce⋅100Ce.


### 2.5.2. 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:(3)Qe=QoKLCe1+KLCe,whereQo is the maximum monolayer adsorption capacity (mg/g) and kL is the Langmuir isotherm constant representing binding energy of the adsorption system (L/mg).Freundlich isotherm equation:(4)Qe=kFCe1/nF,wherekF is the Freundlich isotherm constant (mg/g) indicating adsorption capacity and nF is adsorption intensity.Temkin isotherm equation:(5)Qe=BlnAT+BlnCe,withB=RTbT,whereAT is the Temkin isotherm equilibrium binding constant (L/g), bT 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:(6)lnQe=lnQs−Kadε2,withε=RTln1+1Ce,whereQs is the theoretical isotherm saturation capacity (mg/g) and Kad is the Dubinin–Radushkevich isotherm constant (mol2/kJ2).


### 2.5.3. 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:(7)lnCt=lnCo−k1t.Pseudo-first-order reaction model:(8)lnQo−Qt=lnQo−ks1t.Second-order reaction model:(9)1Ct=1Co+k2t.Pseudo-second-order reaction model:(10)1Qe−Qt=1Qe+ks2t⟶tQt=1h+1Qet,withh=ks2Qe2,whereQo is the maximum monolayer coverage capacity (mg/g); Qe and Qt are the amount of adsorbate adsorbed per gram of adsorbent at equilibrium time and testing time t (mg/g); Co and Ct are the solution concentration at the initial time and the testing time t (mg/l); and k1,ks1,k2,andks2 are the rate constant (per minute) of the first-order reaction model, pseudo-first-order reaction model, second-order reaction model, and pseudo-second-order reaction model, respectively.


## 2.5.1. Adsorption of Cr (VI) Ions and Methylene Blue Using YPS Samples

The amount of adsorbate per amount of adsorbent at equilibrium condition,Q (mg/g), was calculated as follows:(1)Q=Co−Ce⋅VW,where Co and Ce 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).The percentage of metal ions removed,H (%), was calculated using the following equation:(2)H=Co−Ce⋅100Ce.


## 2.5.2. 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:(3)Qe=QoKLCe1+KLCe,whereQo is the maximum monolayer adsorption capacity (mg/g) and kL is the Langmuir isotherm constant representing binding energy of the adsorption system (L/mg).Freundlich isotherm equation:(4)Qe=kFCe1/nF,wherekF is the Freundlich isotherm constant (mg/g) indicating adsorption capacity and nF is adsorption intensity.Temkin isotherm equation:(5)Qe=BlnAT+BlnCe,withB=RTbT,whereAT is the Temkin isotherm equilibrium binding constant (L/g), bT 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:(6)lnQe=lnQs−Kadε2,withε=RTln1+1Ce,whereQs is the theoretical isotherm saturation capacity (mg/g) and Kad is the Dubinin–Radushkevich isotherm constant (mol2/kJ2).


## 2.5.3. 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:(7)lnCt=lnCo−k1t.Pseudo-first-order reaction model:(8)lnQo−Qt=lnQo−ks1t.Second-order reaction model:(9)1Ct=1Co+k2t.Pseudo-second-order reaction model:(10)1Qe−Qt=1Qe+ks2t⟶tQt=1h+1Qet,withh=ks2Qe2,whereQo is the maximum monolayer coverage capacity (mg/g); Qe and Qt are the amount of adsorbate adsorbed per gram of adsorbent at equilibrium time and testing time t (mg/g); Co and Ct are the solution concentration at the initial time and the testing time t (mg/l); and k1,ks1,k2,andks2 are the rate constant (per minute) of the first-order reaction model, pseudo-first-order reaction model, second-order reaction model, and pseudo-second-order reaction model, respectively.


## 3. Results and Discussion

### 3.1. Characteristics of Yellow Phosphorus Slag (YPS) Samples

#### 3.1.1. FTIR Spectra of YPS Samples

Figure1 shows FTIR spectra of the YPS samples. It can be seen that the absorption peaks of YPS samples mostly appeared in the wavenumber range of 1500–500 cm−1. In the low frequency region, the deformation vibration of bridge Si–O–Si and terminal O–Si–O groups and the metal-oxygen polyhedral (CaOn) results in the absorption bands of about 550 cm−1. The adsorption peak at 699 cm−1 assigned to the Al–O and Si–O bonds and showed the presence of pseudowollastonite α–CaSiO3 in the slag. The spectra from 750 cm−1 to 1050 cm−1 with the peak at 872 and 920 cm−1 correspond to the stretching vibration of Si–O groups, indicating the presence of the glass-like earth silicon. Numerous unbridged connections of Si–O emerging are the result of breach of the polymer network Si–O–Si of the frame due to the introduction of Са atoms for replacement of Si atoms in the Si–O–Si network. Furthermore, the peaks at 1414 and 1484 cm−1 represent the vibration of CO32− in calcite, one of main compositions of YPS samples. This result is similar to the report of Zinesh et al. [34].Figure 1
FTIR spectra of YPS samples.


#### 3.1.2. Energy-Dispersive X-Ray Spectroscopy (EDX)

Figure2 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.Figure 2
SEM images and EDX spectra of YPS samples. YPS0 (a, d); YPS1 (b, e); YPS2 (c, f).
(a)(b)(c)(d)(e)(f)Table 1
Average weight (%) of elements in YPS samples.
No.ElementYPS0YPS1YPS21O46.7348.1546.572Si13.3213.0813.913Ca29.2526.4029.954Mg1.561.451.475K0.420.490.396Cr0.11——7Mn0.300.360.188Na0.170.24—9S0.240.460.3010P1.291.481.1111F3.883.323.6712Al1.031.100.9913W0.980.740.7814Fe0.492.240.2115Ti0.070.150.0716Pm0.070.260.1717Sm0.24—0.1418Ce0.100.140.1219Pr0.220.140.1620Nd0.24—0.23Total100100100


#### 3.1.3. X-Ray Diffraction (XRD)

The crystallographic structure of YPS samples before and after treatment was determined by using the X-ray diffraction method. The results of XRD analysis of YPS particles are performed in Figures3–5. 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. The 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. The YPS2 sample only contains calcium phosphate β crystals. This result proved that the calcium phosphate was detached after treatment process. The 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 4.32 Å, 2.81 Å, and 1.64 Å, respectively.Figure 3
XRD pattern of the YPS0 sample.Figure 4
XRD pattern of the YPS1 sample.Figure 5
XRD pattern of the YPS2 sample.


#### 3.1.4. ICP-MS Spectra

Table2 demonstrates the chemical composition of the YPS1 and YPS2 samples after treatments. As can be seen from this table, CaO and SiO2 compose of approximately 80% of the pretreated YPS samples with each compound accounts for about 40% of the samples. It is noticeable that the percentage of P2O5 decreased greatly after the second treatment process, from 1.30% in the YPS1 sample to 0.01% in the YPS2 sample. 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. This is in agreement with the publication of Ming et al. [35].Table 2
Composition of YPS samples obtained from the ICP method.
No.TargetUnitYPS1YPS21CaO%38.8441.152SiO2%39.1738.673P2O5%1.300.014Femg/kg1425.001142.595Almg/kg7000.006172.606Mnmg/kg798.08846.157Timg/kg28461.5426078.808Nimg/kg969.23260.799Bamg/kg257.69202.6310Srmg/kg798.08819.8911Znmg/kg49.4266.2312Crmg/kg16.4618.4213Cumg/kg6.7310.5614Ptmg/kg0.040.0315Rbmg/kg6.379.2716Sbmg/kg1.532.5317Semg/kg0.430.9318Snmg/kg0.651.5819Tlmg/kg0.020.0220Umg/kg3.734.3721Vmg/kg5.525.1822Wmg/kg0.860.41


#### 3.1.5. Morphology of YPS Samples

Figure6 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)).Figure 6
FESEM images of YPS samples at magnification of 5000 times and 50000 times. YPS1 (a, b); YPS2 (c, d).
(a)(b)(c)(d)From above results and comparing with other methods, it can be concluded that wet milling technology is effective for treatment of YPS to obtain the YPS particles with finer size and high purity at cheap cost. These YPS particles are potential for further advanced applications, for examples, additives for preparation of polymer composites, coating, paint, rubber, flame retardants, absorbents, etc. The similar finding can be seen in the report of Huang et al. [36].


#### 3.1.6. Zeta Potential

Figure7 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. The negative charge on the surface of YPS2 can be due to the presence of CaO and calcite in composition of YPS2.Figure 7
Zeta potential distribution diagram of the YPS2 sample.


### 3.2. Use of YPS Particles as Absorbents

#### 3.2.1. Chromium (VI) Ion Adsorption Ability of YPS Particles

Table3 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, HNO3, and EDTA solutions (Q). The 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 HNO3 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. The raw YPS sample after water treatment (YPS1) presented much higher adsorption ability, 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 HNO3, NaOH, and EDTA solutions for further Cr (VI) ion adsorption study. However, the modified YPS2 samples using HNO3 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). The 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. The presence of EDTA can lead to the covering of the surface of YPS particles and limit the Cr (VI) ion adsorption. Therefore, in this study, the YPS2 sample without any further modification will be used for the following experiments.Table 3
Cr (VI) ion adsorption ability of YPS samples.
No.SampleWeight of adsorbent (g)Time of adsorption (min)H (%)Q(mg g−1)1YPS00.51204.930.0992YPS10.512034.430.6893YPS20.512041.160.8234YPS0-HNO30.512010.130.2035YPS0-NaOH0.51204.270.0856YPS2-HNO30.512019.680.3947YPS2-NaOH0.512041.810.8368YPS2-EDTA0.512023.580.472


#### 3.2.2. Assessment on Chromium (VI) Ion Adsorption Ability of Yellow Phosphorus Slag Samples

(1) Effect of Some Experiment Conditions on Chromium (VI) Ion Adsorption Process. The 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. The obtained results are listed in Tables 4–8.(i)
Effect of pHTable4 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). The 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. The pH higher than 7 was not studied due to the unstableness of Cr (VI) ions in the alkaline environment [14].(ii)
Effect of adsorbent weightTable5 indicates the effect of adsorbent weight on the Cr (VI) ion adsorption process using YPS2 samples. The 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. The others showed good adsorption ability with the percentage of Cr (VI) ions removed were higher than 20%. The highest Cr (VI) ion removal efficiency is achieved using 0.5 g of YPS2 (H = 41.16%).(iii)
Effect of temperatureTable6 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. The highest amount of Cr (VI) ion removal percentage is obtained at room temperature with the H value of 20.33%. The Cr (VI) ion adsorption capacity of YPS2 was decreased significantly with the increasing adsorption temperature.(iv)
Effect of adsorption timeTable7 displays the effect of adsorption time on the Cr (VI) ion adsorption process using YPS2 samples. The 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. This 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 concentrationTable8 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. Then, it was dropped significantly when the initial Cr (VI) ion concentration is 80 mg/L and 100 mg/L. This 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.Table 4
Effect of pH on Cr (VI) ion adsorption process.
No.Mass (g)Time (min)pHTemp. (°C)Q (mg·g−1)H (%)10.51202260.1125.5820.51203260.0904.4930.51204260.1859.2640.51205260.0291.4550.51206260.0904.4960.51207260.40720.33Table 5
Effect of adsorbent weight on Cr (VI) ion adsorption process.
No.Mass (g)Time (min)pHTemp. (°C)Q (mg·g−1)H (%)10.11207202.90129.0120.21207201.15823.1530.31207200.72821.8540.51207200.82341.16511207200.16916.86Table 6
Effect of temperature on the Cr (VI) ion adsorption process.
No.Mass (g)Time (min)pHTemp. (°C)Q (mg·g−1)H (%)10.51207260.40720.3320.51207400.0904.4930.51207600.0030.15Table 7
Effect of adsorption time on the Cr (VI) ion adsorption process.
No.Mass (g)Time (min)pHTemp. (°C)Q (mg·g−1)H (%)10.5307250.0030.1520.5607250.0291.4530.5907250.1296.4440.51207250.61130.5350.51507250.1165.7960.51807250.39419.68Table 8
Effect of initial concentration on the Cr (VI) ion adsorption process.
No.Concentration (mg/L)Volume (mL)pHQ (mg·g−1)H (%)11010070.40720.3322010070.38519.2433010070.38119.0345010070.30715.3458010070.0904.49610010070.0030.15


#### 3.2.3. 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. The results of removal efficiency and amount of MB removed per gram of YPS2 are listed in Tables 9–13.Table 9
Effect of pH on methylene blue adsorption process.
No.Mass (g)Time (min)pHQ (mg·g−1)H (%)20.412032.45598.2030.412042.43497.3540.412052.35094.0250.412062.40396.1160.412072.441Table 10
Effect of adsorbent weight on methylene blue adsorption process.
No.Mass (g)Time (min)pHQ (mg·g−1)H (%)10.212074.69293.8520.312073.20095.9930.412072.44197.6340.512071.92496.2251.012070.96496.39Table 11
Effect of temperature on methylene blue adsorption process.
No.Mass (g)Time (min)Temp. (°C)Q (mg·g−1)H (%)10.4120302.44197.6320.4120452.43597.4130.4120652.45898.31Table 12
Effect of adsorption time on methylene blue adsorption process.
No.Mass (g)Time (min)Volume (mL)pHQ (mg·g−1)H (%)10.43010072.35994.3620.46010072.37494.9840.412010072.44197.6350.415010072.45998.3760.418010072.40196.0570.43010042.42597.0180.46010042.40196.0590.412010042.45598.20100.415010042.44597.80110.418010042.42196.84Table 13
Effect of initial concentration on the methylene blue adsorption process.
No.Concentration (mg/L)Volume (mL)pHQ (mg·g−1)H (%)1510072.39695.8221010072.44197.6331510072.31792.6642010072.22689.0552510072.18487.35(1) Effect of Some Conditions on the Methylene Blue Adsorption Process.(i)
Effect of pHTable9 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 weightTable10 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%. This can be caused by the different contact of the adsorbent and MB molecules in solution at various amounts of the adsorbent. Therefore, the YPS2 adsorbent weight of 0.4 g was selected for further investigation.(iii)
Effect of temperatureTable11 presents the effect of adsorption temperature on the MB adsorption process using YPS2 samples. The temperature was changed from 30°C to 65°C. The MB removal efficiency using YPS2 samples was the highest at 65°C with H = 98.31% and lowest at 45°C with H = 97.41%. The amount of MB removed per gram of YPS2 samples (Q) under different temperatures also followed that order.(iv)
Effect of adsorption timeTable12 performs how changing the adsorption time can influence the MB adsorption capacity of YPS2 samples. The time was altered from 30 minutes to 180 minutes, and the experiments were carried out in two different pH solutions (pH 4 and pH 7). For pH 7 solution, the MB removal efficiency was increased with rising adsorption time and reached the highest percentage of MB removed of 98.37% after 150 minutes. After that, the MB adsorption capacity of the YPS2 sample was decreased. This might also be due to the saturation on the surface of YPS2 samples. The 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. Therefore, the suitable time for the MB adsorption study by the YPS2 sample is 120 minutes.(v)
Effect of initial MB concentrationTable13 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. The 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.Figure8 shows IR spectra of the YPS2 sample before and after absorbing MB. The 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). This is due to the consonance of bending vibration of the CH3 group and aromatic C=C of MB with the stretching vibration of the CO32− 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. These 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 8
IR spectra of the YPS2 sample and YPS2-absorbed methylene blue at initial MB concentration of 10 ppm.Figure 9
A hypothesis model for the adsorption of MB ions by YPS2 particles.


#### 3.2.4. Methylene Blue Adsorption Isotherms

Figure10 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 R2 = 0.96 which indicated that the adsorption process is in the monolayer. The separation factor RL=0.434, smaller than 1, also expressed that the equilibrium adsorption to be in favor. The Freundlich model also demonstrated a relatively high correlation coefficient R2 = 0.925, with the adsorption intensity n = 1.422 to display the favorable sorption process. The other isotherm models did not fit well with the MB adsorption process using YPS.Figure 10
Four isotherm models with equations and correlation coefficient values of MB adsorption using YPS. (a) Langmuir adsorption isotherm. (b) Freundlich adsorption isotherm. (c) Temkin adsorption isotherm. (d) Dubinin–Radushkevich adsorption isotherm.
(a)(b)(c)(d)Table 14
Parameters for plotting adsorption isotherms of MB adsorption using YPS.
No.Co (mg·L−1)Ce (mg·L−1)1/CeLogCeLnCeQe (mg·g−1)1/QeLogQeLnQeε2130.0911.49−1.06−2.442.910.340.461.0739.14250.185.57−0.75−1.724.820.210.681.5721.77370.342.90−0.46−1.076.660.150.821.9011.384100.303.38−0.53−1.229.700.100.992.2713.385130.601.67−0.22−0.5212.400.081.092.525.946150.861.16−0.06−0.1514.140.071.152.653.62CoandCe: initial MB concentration and absorbed MB concentration, respectively.Table15 lists the Langmuir, Freundlich, Temkin, and Dubinin–Radushkevich isotherm constants of MB adsorption using YPS. It can be recognized that the maximum adsorption capacity Qo of YPS for the removal of MB is 22.989 mg·g−1. As comparison with the Qo of other adsorbents, for example, orange peel, banana peel, natural clay, and fly ash in Table 16, the Qo value of YPS is quite good. This confirms that YPS is a potential absorbent for the removal of MB in aqueous solution.Table 15
Langmuir, Freundlich, Temkin, and Dubinin–Radushkevich isotherm constants of MB adsorption using YPS.
Langmuir constantFreundlich constantQo (mg·g−1)KL (L·mg−1)RLR21/nNkf (mg·g−1)R222.9891.6420.4340.9600.7031.42216.9240.925Temkin constantDubinin–Radushkevich constantAT (L·mg−1)bTB (J·mol−1)R2Qs (mg·g−1)Kad (mol2·kJ−2)E (kJ·mol−1)R217.398491.1045.0450.89814.8030.0443.3700.905Table 16
Comparison of adsorption capacity of several low-cost adsorbents for the uptake of methylene blue from aqueous solutions.
AdsorbentsSorption capacityQo (mg·g−1)ReferencesActivated date pits12.90[38]Fly ash5.57[38]Orange peel18.60[38]Glass2.24[38]Clay6.30[38]Natural clay15.40[38]Silica nanosheets11.77[38]Ilmenite nanoparticles71.90[38]Banana peel20.80[38]Garlic peel142.86[39]Mango seed kernel142.86[39]Rejected tea156.00[39]Neem leaves8.76[39]Empty fruit bunch50.76[39]YPS22.99This work


#### 3.2.5. Methylene Blue Adsorption Kinetics

MB adsorption kinetics were studied using four linear adsorption kinetic models as represented in Figure11.Figure 11
Adsorption kinetics of MB adsorption process using YPS. (a) First-order reaction model. (b) Pseudo-first-order reaction model. (c) Second-order reaction model. (d) Pseudo-second-order reaction model.
(a)(b)(c)(d)From Figure11, we can see that all four linear reaction models show good fitting to the adsorption process of MB using YPS with the correlation coefficient R2 all greater than 0.98. However, the best fit model is the pseudo-second-order reaction model with R2 equal to 0.9999. This 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].


#### 3.2.6. Methylene Blue Adsorption Thermodynamics

Thermodynamics 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:(11)ΔGo=−RTlnKa,(12)ΔGo=ΔHo−TΔSo,where R is the universal gas constant, T is absolute temperature, ΔGo is Gibbs free energy change, ΔHo is enthalpy change, ΔSo is entropy change, and Ka is the Langmuir constant which was calculated as suggested in References [40, 41].Herein, isotherm data were analyzed at 303, 313, and 323 K. FromKa values obtained from Langmuir isotherms at different temperatures, three ΔGo values were calculated and are presented in Table 17. It can be seen that the ΔGo values are negative; it means that MB adsorption processes occur spontaneously. The ΔGo increased with rising temperature indicates more energetically favorable adsorption [37]. From the plot of the ΔGo values versus T in Figure 12 (R2 = 0.9535), ΔHo and ΔSo were also calculated and are listed in Table 17. The negative ΔHo indicating that the sorption reaction is exothermic and the negative ΔSo value showed a decrease in the randomness at the solid/solution interface during the sorption process of MB onto YPS2.Table 17
Thermodynamic parameters of MB adsorption process by the YPS2 sample.
AdsorbentThermodynamic parametersT (K)ΔGo (kJ·mol−1)ΔHo (kJ·mol−1)ΔSo (kJ·mol−1·K−1)Methylene blue303−32.6642−74.017−0.1371313−30.7693323−29.9231Figure 12
Plot of Gibbs free energy change, ΔGo, versus temperature (T).


## 3.1. Characteristics of Yellow Phosphorus Slag (YPS) Samples

### 3.1.1. FTIR Spectra of YPS Samples

Figure1 shows FTIR spectra of the YPS samples. It can be seen that the absorption peaks of YPS samples mostly appeared in the wavenumber range of 1500–500 cm−1. In the low frequency region, the deformation vibration of bridge Si–O–Si and terminal O–Si–O groups and the metal-oxygen polyhedral (CaOn) results in the absorption bands of about 550 cm−1. The adsorption peak at 699 cm−1 assigned to the Al–O and Si–O bonds and showed the presence of pseudowollastonite α–CaSiO3 in the slag. The spectra from 750 cm−1 to 1050 cm−1 with the peak at 872 and 920 cm−1 correspond to the stretching vibration of Si–O groups, indicating the presence of the glass-like earth silicon. Numerous unbridged connections of Si–O emerging are the result of breach of the polymer network Si–O–Si of the frame due to the introduction of Са atoms for replacement of Si atoms in the Si–O–Si network. Furthermore, the peaks at 1414 and 1484 cm−1 represent the vibration of CO32− in calcite, one of main compositions of YPS samples. This result is similar to the report of Zinesh et al. [34].Figure 1
FTIR spectra of YPS samples.


### 3.1.2. Energy-Dispersive X-Ray Spectroscopy (EDX)

Figure2 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.Figure 2
SEM images and EDX spectra of YPS samples. YPS0 (a, d); YPS1 (b, e); YPS2 (c, f).
(a)(b)(c)(d)(e)(f)Table 1
Average weight (%) of elements in YPS samples.
No.ElementYPS0YPS1YPS21O46.7348.1546.572Si13.3213.0813.913Ca29.2526.4029.954Mg1.561.451.475K0.420.490.396Cr0.11——7Mn0.300.360.188Na0.170.24—9S0.240.460.3010P1.291.481.1111F3.883.323.6712Al1.031.100.9913W0.980.740.7814Fe0.492.240.2115Ti0.070.150.0716Pm0.070.260.1717Sm0.24—0.1418Ce0.100.140.1219Pr0.220.140.1620Nd0.24—0.23Total100100100


### 3.1.3. X-Ray Diffraction (XRD)

The crystallographic structure of YPS samples before and after treatment was determined by using the X-ray diffraction method. The results of XRD analysis of YPS particles are performed in Figures3–5. 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. The 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. The YPS2 sample only contains calcium phosphate β crystals. This result proved that the calcium phosphate was detached after treatment process. The 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 4.32 Å, 2.81 Å, and 1.64 Å, respectively.Figure 3
XRD pattern of the YPS0 sample.Figure 4
XRD pattern of the YPS1 sample.Figure 5
XRD pattern of the YPS2 sample.


### 3.1.4. ICP-MS Spectra

Table2 demonstrates the chemical composition of the YPS1 and YPS2 samples after treatments. As can be seen from this table, CaO and SiO2 compose of approximately 80% of the pretreated YPS samples with each compound accounts for about 40% of the samples. It is noticeable that the percentage of P2O5 decreased greatly after the second treatment process, from 1.30% in the YPS1 sample to 0.01% in the YPS2 sample. 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. This is in agreement with the publication of Ming et al. [35].Table 2
Composition of YPS samples obtained from the ICP method.
No.TargetUnitYPS1YPS21CaO%38.8441.152SiO2%39.1738.673P2O5%1.300.014Femg/kg1425.001142.595Almg/kg7000.006172.606Mnmg/kg798.08846.157Timg/kg28461.5426078.808Nimg/kg969.23260.799Bamg/kg257.69202.6310Srmg/kg798.08819.8911Znmg/kg49.4266.2312Crmg/kg16.4618.4213Cumg/kg6.7310.5614Ptmg/kg0.040.0315Rbmg/kg6.379.2716Sbmg/kg1.532.5317Semg/kg0.430.9318Snmg/kg0.651.5819Tlmg/kg0.020.0220Umg/kg3.734.3721Vmg/kg5.525.1822Wmg/kg0.860.41


### 3.1.5. Morphology of YPS Samples

Figure6 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)).Figure 6
FESEM images of YPS samples at magnification of 5000 times and 50000 times. YPS1 (a, b); YPS2 (c, d).
(a)(b)(c)(d)From above results and comparing with other methods, it can be concluded that wet milling technology is effective for treatment of YPS to obtain the YPS particles with finer size and high purity at cheap cost. These YPS particles are potential for further advanced applications, for examples, additives for preparation of polymer composites, coating, paint, rubber, flame retardants, absorbents, etc. The similar finding can be seen in the report of Huang et al. [36].


### 3.1.6. Zeta Potential

Figure7 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. The negative charge on the surface of YPS2 can be due to the presence of CaO and calcite in composition of YPS2.Figure 7
Zeta potential distribution diagram of the YPS2 sample.


## 3.1.1. FTIR Spectra of YPS Samples

Figure1 shows FTIR spectra of the YPS samples. It can be seen that the absorption peaks of YPS samples mostly appeared in the wavenumber range of 1500–500 cm−1. In the low frequency region, the deformation vibration of bridge Si–O–Si and terminal O–Si–O groups and the metal-oxygen polyhedral (CaOn) results in the absorption bands of about 550 cm−1. The adsorption peak at 699 cm−1 assigned to the Al–O and Si–O bonds and showed the presence of pseudowollastonite α–CaSiO3 in the slag. The spectra from 750 cm−1 to 1050 cm−1 with the peak at 872 and 920 cm−1 correspond to the stretching vibration of Si–O groups, indicating the presence of the glass-like earth silicon. Numerous unbridged connections of Si–O emerging are the result of breach of the polymer network Si–O–Si of the frame due to the introduction of Са atoms for replacement of Si atoms in the Si–O–Si network. Furthermore, the peaks at 1414 and 1484 cm−1 represent the vibration of CO32− in calcite, one of main compositions of YPS samples. This result is similar to the report of Zinesh et al. [34].Figure 1
FTIR spectra of YPS samples.


## 3.1.2. Energy-Dispersive X-Ray Spectroscopy (EDX)

Figure2 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.Figure 2
SEM images and EDX spectra of YPS samples. YPS0 (a, d); YPS1 (b, e); YPS2 (c, f).
(a)(b)(c)(d)(e)(f)Table 1
Average weight (%) of elements in YPS samples.
No.ElementYPS0YPS1YPS21O46.7348.1546.572Si13.3213.0813.913Ca29.2526.4029.954Mg1.561.451.475K0.420.490.396Cr0.11——7Mn0.300.360.188Na0.170.24—9S0.240.460.3010P1.291.481.1111F3.883.323.6712Al1.031.100.9913W0.980.740.7814Fe0.492.240.2115Ti0.070.150.0716Pm0.070.260.1717Sm0.24—0.1418Ce0.100.140.1219Pr0.220.140.1620Nd0.24—0.23Total100100100


## 3.1.3. X-Ray Diffraction (XRD)

The crystallographic structure of YPS samples before and after treatment was determined by using the X-ray diffraction method. The results of XRD analysis of YPS particles are performed in Figures3–5. 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. The 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. The YPS2 sample only contains calcium phosphate β crystals. This result proved that the calcium phosphate was detached after treatment process. The 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 4.32 Å, 2.81 Å, and 1.64 Å, respectively.Figure 3
XRD pattern of the YPS0 sample.Figure 4
XRD pattern of the YPS1 sample.Figure 5
XRD pattern of the YPS2 sample.


## 3.1.4. ICP-MS Spectra

Table2 demonstrates the chemical composition of the YPS1 and YPS2 samples after treatments. As can be seen from this table, CaO and SiO2 compose of approximately 80% of the pretreated YPS samples with each compound accounts for about 40% of the samples. It is noticeable that the percentage of P2O5 decreased greatly after the second treatment process, from 1.30% in the YPS1 sample to 0.01% in the YPS2 sample. 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. This is in agreement with the publication of Ming et al. [35].Table 2
Composition of YPS samples obtained from the ICP method.
No.TargetUnitYPS1YPS21CaO%38.8441.152SiO2%39.1738.673P2O5%1.300.014Femg/kg1425.001142.595Almg/kg7000.006172.606Mnmg/kg798.08846.157Timg/kg28461.5426078.808Nimg/kg969.23260.799Bamg/kg257.69202.6310Srmg/kg798.08819.8911Znmg/kg49.4266.2312Crmg/kg16.4618.4213Cumg/kg6.7310.5614Ptmg/kg0.040.0315Rbmg/kg6.379.2716Sbmg/kg1.532.5317Semg/kg0.430.9318Snmg/kg0.651.5819Tlmg/kg0.020.0220Umg/kg3.734.3721Vmg/kg5.525.1822Wmg/kg0.860.41


## 3.1.5. Morphology of YPS Samples

Figure6 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)).Figure 6
FESEM images of YPS samples at magnification of 5000 times and 50000 times. YPS1 (a, b); YPS2 (c, d).
(a)(b)(c)(d)From above results and comparing with other methods, it can be concluded that wet milling technology is effective for treatment of YPS to obtain the YPS particles with finer size and high purity at cheap cost. These YPS particles are potential for further advanced applications, for examples, additives for preparation of polymer composites, coating, paint, rubber, flame retardants, absorbents, etc. The similar finding can be seen in the report of Huang et al. [36].


## 3.1.6. Zeta Potential

Figure7 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. The negative charge on the surface of YPS2 can be due to the presence of CaO and calcite in composition of YPS2.Figure 7
Zeta potential distribution diagram of the YPS2 sample.


## 3.2. Use of YPS Particles as Absorbents

### 3.2.1. Chromium (VI) Ion Adsorption Ability of YPS Particles

Table3 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, HNO3, and EDTA solutions (Q). The 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 HNO3 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. The raw YPS sample after water treatment (YPS1) presented much higher adsorption ability, 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 HNO3, NaOH, and EDTA solutions for further Cr (VI) ion adsorption study. However, the modified YPS2 samples using HNO3 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). The 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. The presence of EDTA can lead to the covering of the surface of YPS particles and limit the Cr (VI) ion adsorption. Therefore, in this study, the YPS2 sample without any further modification will be used for the following experiments.Table 3
Cr (VI) ion adsorption ability of YPS samples.
No.SampleWeight of adsorbent (g)Time of adsorption (min)H (%)Q(mg g−1)1YPS00.51204.930.0992YPS10.512034.430.6893YPS20.512041.160.8234YPS0-HNO30.512010.130.2035YPS0-NaOH0.51204.270.0856YPS2-HNO30.512019.680.3947YPS2-NaOH0.512041.810.8368YPS2-EDTA0.512023.580.472


### 3.2.2. Assessment on Chromium (VI) Ion Adsorption Ability of Yellow Phosphorus Slag Samples

(1) Effect of Some Experiment Conditions on Chromium (VI) Ion Adsorption Process. The 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. The obtained results are listed in Tables 4–8.(i)
Effect of pHTable4 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). The 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. The pH higher than 7 was not studied due to the unstableness of Cr (VI) ions in the alkaline environment [14].(ii)
Effect of adsorbent weightTable5 indicates the effect of adsorbent weight on the Cr (VI) ion adsorption process using YPS2 samples. The 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. The others showed good adsorption ability with the percentage of Cr (VI) ions removed were higher than 20%. The highest Cr (VI) ion removal efficiency is achieved using 0.5 g of YPS2 (H = 41.16%).(iii)
Effect of temperatureTable6 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. The highest amount of Cr (VI) ion removal percentage is obtained at room temperature with the H value of 20.33%. The Cr (VI) ion adsorption capacity of YPS2 was decreased significantly with the increasing adsorption temperature.(iv)
Effect of adsorption timeTable7 displays the effect of adsorption time on the Cr (VI) ion adsorption process using YPS2 samples. The 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. This 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 concentrationTable8 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. Then, it was dropped significantly when the initial Cr (VI) ion concentration is 80 mg/L and 100 mg/L. This 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.Table 4
Effect of pH on Cr (VI) ion adsorption process.
No.Mass (g)Time (min)pHTemp. (°C)Q (mg·g−1)H (%)10.51202260.1125.5820.51203260.0904.4930.51204260.1859.2640.51205260.0291.4550.51206260.0904.4960.51207260.40720.33Table 5
Effect of adsorbent weight on Cr (VI) ion adsorption process.
No.Mass (g)Time (min)pHTemp. (°C)Q (mg·g−1)H (%)10.11207202.90129.0120.21207201.15823.1530.31207200.72821.8540.51207200.82341.16511207200.16916.86Table 6
Effect of temperature on the Cr (VI) ion adsorption process.
No.Mass (g)Time (min)pHTemp. (°C)Q (mg·g−1)H (%)10.51207260.40720.3320.51207400.0904.4930.51207600.0030.15Table 7
Effect of adsorption time on the Cr (VI) ion adsorption process.
No.Mass (g)Time (min)pHTemp. (°C)Q (mg·g−1)H (%)10.5307250.0030.1520.5607250.0291.4530.5907250.1296.4440.51207250.61130.5350.51507250.1165.7960.51807250.39419.68Table 8
Effect of initial concentration on the Cr (VI) ion adsorption process.
No.Concentration (mg/L)Volume (mL)pHQ (mg·g−1)H (%)11010070.40720.3322010070.38519.2433010070.38119.0345010070.30715.3458010070.0904.49610010070.0030.15


### 3.2.3. 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. The results of removal efficiency and amount of MB removed per gram of YPS2 are listed in Tables 9–13.Table 9
Effect of pH on methylene blue adsorption process.
No.Mass (g)Time (min)pHQ (mg·g−1)H (%)20.412032.45598.2030.412042.43497.3540.412052.35094.0250.412062.40396.1160.412072.441Table 10
Effect of adsorbent weight on methylene blue adsorption process.
No.Mass (g)Time (min)pHQ (mg·g−1)H (%)10.212074.69293.8520.312073.20095.9930.412072.44197.6340.512071.92496.2251.012070.96496.39Table 11
Effect of temperature on methylene blue adsorption process.
No.Mass (g)Time (min)Temp. (°C)Q (mg·g−1)H (%)10.4120302.44197.6320.4120452.43597.4130.4120652.45898.31Table 12
Effect of adsorption time on methylene blue adsorption process.
No.Mass (g)Time (min)Volume (mL)pHQ (mg·g−1)H (%)10.43010072.35994.3620.46010072.37494.9840.412010072.44197.6350.415010072.45998.3760.418010072.40196.0570.43010042.42597.0180.46010042.40196.0590.412010042.45598.20100.415010042.44597.80110.418010042.42196.84Table 13
Effect of initial concentration on the methylene blue adsorption process.
No.Concentration (mg/L)Volume (mL)pHQ (mg·g−1)H (%)1510072.39695.8221010072.44197.6331510072.31792.6642010072.22689.0552510072.18487.35(1) Effect of Some Conditions on the Methylene Blue Adsorption Process.(i)
Effect of pHTable9 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 weightTable10 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%. This can be caused by the different contact of the adsorbent and MB molecules in solution at various amounts of the adsorbent. Therefore, the YPS2 adsorbent weight of 0.4 g was selected for further investigation.(iii)
Effect of temperatureTable11 presents the effect of adsorption temperature on the MB adsorption process using YPS2 samples. The temperature was changed from 30°C to 65°C. The MB removal efficiency using YPS2 samples was the highest at 65°C with H = 98.31% and lowest at 45°C with H = 97.41%. The amount of MB removed per gram of YPS2 samples (Q) under different temperatures also followed that order.(iv)
Effect of adsorption timeTable12 performs how changing the adsorption time can influence the MB adsorption capacity of YPS2 samples. The time was altered from 30 minutes to 180 minutes, and the experiments were carried out in two different pH solutions (pH 4 and pH 7). For pH 7 solution, the MB removal efficiency was increased with rising adsorption time and reached the highest percentage of MB removed of 98.37% after 150 minutes. After that, the MB adsorption capacity of the YPS2 sample was decreased. This might also be due to the saturation on the surface of YPS2 samples. The 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. Therefore, the suitable time for the MB adsorption study by the YPS2 sample is 120 minutes.(v)
Effect of initial MB concentrationTable13 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. The 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.Figure8 shows IR spectra of the YPS2 sample before and after absorbing MB. The 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). This is due to the consonance of bending vibration of the CH3 group and aromatic C=C of MB with the stretching vibration of the CO32− 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. These 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 8
IR spectra of the YPS2 sample and YPS2-absorbed methylene blue at initial MB concentration of 10 ppm.Figure 9
A hypothesis model for the adsorption of MB ions by YPS2 particles.


### 3.2.4. Methylene Blue Adsorption Isotherms

Figure10 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 R2 = 0.96 which indicated that the adsorption process is in the monolayer. The separation factor RL=0.434, smaller than 1, also expressed that the equilibrium adsorption to be in favor. The Freundlich model also demonstrated a relatively high correlation coefficient R2 = 0.925, with the adsorption intensity n = 1.422 to display the favorable sorption process. The other isotherm models did not fit well with the MB adsorption process using YPS.Figure 10
Four isotherm models with equations and correlation coefficient values of MB adsorption using YPS. (a) Langmuir adsorption isotherm. (b) Freundlich adsorption isotherm. (c) Temkin adsorption isotherm. (d) Dubinin–Radushkevich adsorption isotherm.
(a)(b)(c)(d)Table 14
Parameters for plotting adsorption isotherms of MB adsorption using YPS.
No.Co (mg·L−1)Ce (mg·L−1)1/CeLogCeLnCeQe (mg·g−1)1/QeLogQeLnQeε2130.0911.49−1.06−2.442.910.340.461.0739.14250.185.57−0.75−1.724.820.210.681.5721.77370.342.90−0.46−1.076.660.150.821.9011.384100.303.38−0.53−1.229.700.100.992.2713.385130.601.67−0.22−0.5212.400.081.092.525.946150.861.16−0.06−0.1514.140.071.152.653.62CoandCe: initial MB concentration and absorbed MB concentration, respectively.Table15 lists the Langmuir, Freundlich, Temkin, and Dubinin–Radushkevich isotherm constants of MB adsorption using YPS. It can be recognized that the maximum adsorption capacity Qo of YPS for the removal of MB is 22.989 mg·g−1. As comparison with the Qo of other adsorbents, for example, orange peel, banana peel, natural clay, and fly ash in Table 16, the Qo value of YPS is quite good. This confirms that YPS is a potential absorbent for the removal of MB in aqueous solution.Table 15
Langmuir, Freundlich, Temkin, and Dubinin–Radushkevich isotherm constants of MB adsorption using YPS.
Langmuir constantFreundlich constantQo (mg·g−1)KL (L·mg−1)RLR21/nNkf (mg·g−1)R222.9891.6420.4340.9600.7031.42216.9240.925Temkin constantDubinin–Radushkevich constantAT (L·mg−1)bTB (J·mol−1)R2Qs (mg·g−1)Kad (mol2·kJ−2)E (kJ·mol−1)R217.398491.1045.0450.89814.8030.0443.3700.905Table 16
Comparison of adsorption capacity of several low-cost adsorbents for the uptake of methylene blue from aqueous solutions.
AdsorbentsSorption capacityQo (mg·g−1)ReferencesActivated date pits12.90[38]Fly ash5.57[38]Orange peel18.60[38]Glass2.24[38]Clay6.30[38]Natural clay15.40[38]Silica nanosheets11.77[38]Ilmenite nanoparticles71.90[38]Banana peel20.80[38]Garlic peel142.86[39]Mango seed kernel142.86[39]Rejected tea156.00[39]Neem leaves8.76[39]Empty fruit bunch50.76[39]YPS22.99This work


### 3.2.5. Methylene Blue Adsorption Kinetics

MB adsorption kinetics were studied using four linear adsorption kinetic models as represented in Figure11.Figure 11
Adsorption kinetics of MB adsorption process using YPS. (a) First-order reaction model. (b) Pseudo-first-order reaction model. (c) Second-order reaction model. (d) Pseudo-second-order reaction model.
(a)(b)(c)(d)From Figure11, we can see that all four linear reaction models show good fitting to the adsorption process of MB using YPS with the correlation coefficient R2 all greater than 0.98. However, the best fit model is the pseudo-second-order reaction model with R2 equal to 0.9999. This 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].


### 3.2.6. Methylene Blue Adsorption Thermodynamics

Thermodynamics 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:(11)ΔGo=−RTlnKa,(12)ΔGo=ΔHo−TΔSo,where R is the universal gas constant, T is absolute temperature, ΔGo is Gibbs free energy change, ΔHo is enthalpy change, ΔSo is entropy change, and Ka is the Langmuir constant which was calculated as suggested in References [40, 41].Herein, isotherm data were analyzed at 303, 313, and 323 K. FromKa values obtained from Langmuir isotherms at different temperatures, three ΔGo values were calculated and are presented in Table 17. It can be seen that the ΔGo values are negative; it means that MB adsorption processes occur spontaneously. The ΔGo increased with rising temperature indicates more energetically favorable adsorption [37]. From the plot of the ΔGo values versus T in Figure 12 (R2 = 0.9535), ΔHo and ΔSo were also calculated and are listed in Table 17. The negative ΔHo indicating that the sorption reaction is exothermic and the negative ΔSo value showed a decrease in the randomness at the solid/solution interface during the sorption process of MB onto YPS2.Table 17
Thermodynamic parameters of MB adsorption process by the YPS2 sample.
AdsorbentThermodynamic parametersT (K)ΔGo (kJ·mol−1)ΔHo (kJ·mol−1)ΔSo (kJ·mol−1·K−1)Methylene blue303−32.6642−74.017−0.1371313−30.7693323−29.9231Figure 12
Plot of Gibbs free energy change, ΔGo, versus temperature (T).


## 3.2.1. Chromium (VI) Ion Adsorption Ability of YPS Particles

Table3 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, HNO3, and EDTA solutions (Q). The 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 HNO3 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. The raw YPS sample after water treatment (YPS1) presented much higher adsorption ability, 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 HNO3, NaOH, and EDTA solutions for further Cr (VI) ion adsorption study. However, the modified YPS2 samples using HNO3 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). The 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. The presence of EDTA can lead to the covering of the surface of YPS particles and limit the Cr (VI) ion adsorption. Therefore, in this study, the YPS2 sample without any further modification will be used for the following experiments.Table 3
Cr (VI) ion adsorption ability of YPS samples.
No.SampleWeight of adsorbent (g)Time of adsorption (min)H (%)Q(mg g−1)1YPS00.51204.930.0992YPS10.512034.430.6893YPS20.512041.160.8234YPS0-HNO30.512010.130.2035YPS0-NaOH0.51204.270.0856YPS2-HNO30.512019.680.3947YPS2-NaOH0.512041.810.8368YPS2-EDTA0.512023.580.472


## 3.2.2. Assessment on Chromium (VI) Ion Adsorption Ability of Yellow Phosphorus Slag Samples

(1) Effect of Some Experiment Conditions on Chromium (VI) Ion Adsorption Process. The 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. The obtained results are listed in Tables 4–8.(i)
Effect of pHTable4 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). The 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. The pH higher than 7 was not studied due to the unstableness of Cr (VI) ions in the alkaline environment [14].(ii)
Effect of adsorbent weightTable5 indicates the effect of adsorbent weight on the Cr (VI) ion adsorption process using YPS2 samples. The 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. The others showed good adsorption ability with the percentage of Cr (VI) ions removed were higher than 20%. The highest Cr (VI) ion removal efficiency is achieved using 0.5 g of YPS2 (H = 41.16%).(iii)
Effect of temperatureTable6 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. The highest amount of Cr (VI) ion removal percentage is obtained at room temperature with the H value of 20.33%. The Cr (VI) ion adsorption capacity of YPS2 was decreased significantly with the increasing adsorption temperature.(iv)
Effect of adsorption timeTable7 displays the effect of adsorption time on the Cr (VI) ion adsorption process using YPS2 samples. The 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. This 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 concentrationTable8 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. Then, it was dropped significantly when the initial Cr (VI) ion concentration is 80 mg/L and 100 mg/L. This 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.Table 4
Effect of pH on Cr (VI) ion adsorption process.
No.Mass (g)Time (min)pHTemp. (°C)Q (mg·g−1)H (%)10.51202260.1125.5820.51203260.0904.4930.51204260.1859.2640.51205260.0291.4550.51206260.0904.4960.51207260.40720.33Table 5
Effect of adsorbent weight on Cr (VI) ion adsorption process.
No.Mass (g)Time (min)pHTemp. (°C)Q (mg·g−1)H (%)10.11207202.90129.0120.21207201.15823.1530.31207200.72821.8540.51207200.82341.16511207200.16916.86Table 6
Effect of temperature on the Cr (VI) ion adsorption process.
No.Mass (g)Time (min)pHTemp. (°C)Q (mg·g−1)H (%)10.51207260.40720.3320.51207400.0904.4930.51207600.0030.15Table 7
Effect of adsorption time on the Cr (VI) ion adsorption process.
No.Mass (g)Time (min)pHTemp. (°C)Q (mg·g−1)H (%)10.5307250.0030.1520.5607250.0291.4530.5907250.1296.4440.51207250.61130.5350.51507250.1165.7960.51807250.39419.68Table 8
Effect of initial concentration on the Cr (VI) ion adsorption process.
No.Concentration (mg/L)Volume (mL)pHQ (mg·g−1)H (%)11010070.40720.3322010070.38519.2433010070.38119.0345010070.30715.3458010070.0904.49610010070.0030.15


## 3.2.3. 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. The results of removal efficiency and amount of MB removed per gram of YPS2 are listed in Tables 9–13.Table 9
Effect of pH on methylene blue adsorption process.
No.Mass (g)Time (min)pHQ (mg·g−1)H (%)20.412032.45598.2030.412042.43497.3540.412052.35094.0250.412062.40396.1160.412072.441Table 10
Effect of adsorbent weight on methylene blue adsorption process.
No.Mass (g)Time (min)pHQ (mg·g−1)H (%)10.212074.69293.8520.312073.20095.9930.412072.44197.6340.512071.92496.2251.012070.96496.39Table 11
Effect of temperature on methylene blue adsorption process.
No.Mass (g)Time (min)Temp. (°C)Q (mg·g−1)H (%)10.4120302.44197.6320.4120452.43597.4130.4120652.45898.31Table 12
Effect of adsorption time on methylene blue adsorption process.
No.Mass (g)Time (min)Volume (mL)pHQ (mg·g−1)H (%)10.43010072.35994.3620.46010072.37494.9840.412010072.44197.6350.415010072.45998.3760.418010072.40196.0570.43010042.42597.0180.46010042.40196.0590.412010042.45598.20100.415010042.44597.80110.418010042.42196.84Table 13
Effect of initial concentration on the methylene blue adsorption process.
No.Concentration (mg/L)Volume (mL)pHQ (mg·g−1)H (%)1510072.39695.8221010072.44197.6331510072.31792.6642010072.22689.0552510072.18487.35(1) Effect of Some Conditions on the Methylene Blue Adsorption Process.(i)
Effect of pHTable9 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 weightTable10 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%. This can be caused by the different contact of the adsorbent and MB molecules in solution at various amounts of the adsorbent. Therefore, the YPS2 adsorbent weight of 0.4 g was selected for further investigation.(iii)
Effect of temperatureTable11 presents the effect of adsorption temperature on the MB adsorption process using YPS2 samples. The temperature was changed from 30°C to 65°C. The MB removal efficiency using YPS2 samples was the highest at 65°C with H = 98.31% and lowest at 45°C with H = 97.41%. The amount of MB removed per gram of YPS2 samples (Q) under different temperatures also followed that order.(iv)
Effect of adsorption timeTable12 performs how changing the adsorption time can influence the MB adsorption capacity of YPS2 samples. The time was altered from 30 minutes to 180 minutes, and the experiments were carried out in two different pH solutions (pH 4 and pH 7). For pH 7 solution, the MB removal efficiency was increased with rising adsorption time and reached the highest percentage of MB removed of 98.37% after 150 minutes. After that, the MB adsorption capacity of the YPS2 sample was decreased. This might also be due to the saturation on the surface of YPS2 samples. The 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. Therefore, the suitable time for the MB adsorption study by the YPS2 sample is 120 minutes.(v)
Effect of initial MB concentrationTable13 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. The 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.Figure8 shows IR spectra of the YPS2 sample before and after absorbing MB. The 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). This is due to the consonance of bending vibration of the CH3 group and aromatic C=C of MB with the stretching vibration of the CO32− 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. These 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 8
IR spectra of the YPS2 sample and YPS2-absorbed methylene blue at initial MB concentration of 10 ppm.Figure 9
A hypothesis model for the adsorption of MB ions by YPS2 particles.


## 3.2.4. Methylene Blue Adsorption Isotherms

Figure10 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 R2 = 0.96 which indicated that the adsorption process is in the monolayer. The separation factor RL=0.434, smaller than 1, also expressed that the equilibrium adsorption to be in favor. The Freundlich model also demonstrated a relatively high correlation coefficient R2 = 0.925, with the adsorption intensity n = 1.422 to display the favorable sorption process. The other isotherm models did not fit well with the MB adsorption process using YPS.Figure 10
Four isotherm models with equations and correlation coefficient values of MB adsorption using YPS. (a) Langmuir adsorption isotherm. (b) Freundlich adsorption isotherm. (c) Temkin adsorption isotherm. (d) Dubinin–Radushkevich adsorption isotherm.
(a)(b)(c)(d)Table 14
Parameters for plotting adsorption isotherms of MB adsorption using YPS.
No.Co (mg·L−1)Ce (mg·L−1)1/CeLogCeLnCeQe (mg·g−1)1/QeLogQeLnQeε2130.0911.49−1.06−2.442.910.340.461.0739.14250.185.57−0.75−1.724.820.210.681.5721.77370.342.90−0.46−1.076.660.150.821.9011.384100.303.38−0.53−1.229.700.100.992.2713.385130.601.67−0.22−0.5212.400.081.092.525.946150.861.16−0.06−0.1514.140.071.152.653.62CoandCe: initial MB concentration and absorbed MB concentration, respectively.Table15 lists the Langmuir, Freundlich, Temkin, and Dubinin–Radushkevich isotherm constants of MB adsorption using YPS. It can be recognized that the maximum adsorption capacity Qo of YPS for the removal of MB is 22.989 mg·g−1. As comparison with the Qo of other adsorbents, for example, orange peel, banana peel, natural clay, and fly ash in Table 16, the Qo value of YPS is quite good. This confirms that YPS is a potential absorbent for the removal of MB in aqueous solution.Table 15
Langmuir, Freundlich, Temkin, and Dubinin–Radushkevich isotherm constants of MB adsorption using YPS.
Langmuir constantFreundlich constantQo (mg·g−1)KL (L·mg−1)RLR21/nNkf (mg·g−1)R222.9891.6420.4340.9600.7031.42216.9240.925Temkin constantDubinin–Radushkevich constantAT (L·mg−1)bTB (J·mol−1)R2Qs (mg·g−1)Kad (mol2·kJ−2)E (kJ·mol−1)R217.398491.1045.0450.89814.8030.0443.3700.905Table 16
Comparison of adsorption capacity of several low-cost adsorbents for the uptake of methylene blue from aqueous solutions.
AdsorbentsSorption capacityQo (mg·g−1)ReferencesActivated date pits12.90[38]Fly ash5.57[38]Orange peel18.60[38]Glass2.24[38]Clay6.30[38]Natural clay15.40[38]Silica nanosheets11.77[38]Ilmenite nanoparticles71.90[38]Banana peel20.80[38]Garlic peel142.86[39]Mango seed kernel142.86[39]Rejected tea156.00[39]Neem leaves8.76[39]Empty fruit bunch50.76[39]YPS22.99This work


## 3.2.5. Methylene Blue Adsorption Kinetics

MB adsorption kinetics were studied using four linear adsorption kinetic models as represented in Figure11.Figure 11
Adsorption kinetics of MB adsorption process using YPS. (a) First-order reaction model. (b) Pseudo-first-order reaction model. (c) Second-order reaction model. (d) Pseudo-second-order reaction model.
(a)(b)(c)(d)From Figure11, we can see that all four linear reaction models show good fitting to the adsorption process of MB using YPS with the correlation coefficient R2 all greater than 0.98. However, the best fit model is the pseudo-second-order reaction model with R2 equal to 0.9999. This 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].


## 3.2.6. Methylene Blue Adsorption Thermodynamics

Thermodynamics 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:(11)ΔGo=−RTlnKa,(12)ΔGo=ΔHo−TΔSo,where R is the universal gas constant, T is absolute temperature, ΔGo is Gibbs free energy change, ΔHo is enthalpy change, ΔSo is entropy change, and Ka is the Langmuir constant which was calculated as suggested in References [40, 41].Herein, isotherm data were analyzed at 303, 313, and 323 K. FromKa values obtained from Langmuir isotherms at different temperatures, three ΔGo values were calculated and are presented in Table 17. It can be seen that the ΔGo values are negative; it means that MB adsorption processes occur spontaneously. The ΔGo increased with rising temperature indicates more energetically favorable adsorption [37]. From the plot of the ΔGo values versus T in Figure 12 (R2 = 0.9535), ΔHo and ΔSo were also calculated and are listed in Table 17. The negative ΔHo indicating that the sorption reaction is exothermic and the negative ΔSo value showed a decrease in the randomness at the solid/solution interface during the sorption process of MB onto YPS2.Table 17
Thermodynamic parameters of MB adsorption process by the YPS2 sample.
AdsorbentThermodynamic parametersT (K)ΔGo (kJ·mol−1)ΔHo (kJ·mol−1)ΔSo (kJ·mol−1·K−1)Methylene blue303−32.6642−74.017−0.1371313−30.7693323−29.9231Figure 12
Plot of Gibbs free energy change, ΔGo, versus temperature (T).


## 4. 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). The surface of YPS2 has a negative charge. The main composition of YPS2 is calcite, and main oxides of YPS2 are SiO2 and CaO. The 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. The 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%. The FTIR spectrum of YPS2-absorbed MB confirmed that MB was absorbed onto YPS2. The adsorption isotherm of MB adsorption process using YPS2 follows the Langmuir isotherm with R2 = 0.96, and the adsorption kinetic fits well with the pseudo-second-order reaction model with R2 = 0.999. The obtained thermodynamic parameters confirmed that the MB adsorption process onto YPS2 is favorable spontaneous adsorption. These results were also in agreement with others research studies on MB adsorption process using various adsorbents.



---

*Source: 1834829-2020-06-26.xml*