High Performance of UiO-66 Metal-Organic Framework Modified with Melamine for Uptaking of Lead and Cadmium from Aqueous Solutions

doi:10.21203/rs.3.rs-1195293/v1

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Research Article

High Performance of UiO-66 Metal-Organic Framework Modified with Melamine for Uptaking of Lead and Cadmium from Aqueous Solutions

https://doi.org/10.21203/rs.3.rs-1195293/v1

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published 19 Apr, 2022

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In this paper, UiO-66 metal-organic framework (MOF) was prepared by a hydrothermal method and modified consequently with melamine (MUiO-66), as so as enhance the adsorption properties of these materials in liquid-phase adsorption. With respect to this, the adsorption of lead and cadmium divalent ions was performed under varying conditions of pH, metal ion concentration, contact time, adsorbent dose and temperature. Morphology, texture properties, functional groups, crystallinity and thermal properties of both MOFs were examined. UiO-66 composed of sphere-like particles and covered by layers of melamine with enhancing in crystallinity and active sites as well as the total surface area increased from 1080 to 1160 m²/g. The modified UiO-66 with melamine (MUiO-66) showed a notable adsorption capacity of 177.5 and 146.6 mg/g for Pb and Cd (II) ions, respectively. Adsorption of both metals fitted well with the pseudo-second-order kinetic and Langmuir models and controlled by a physisorption mechanism at pH of 5. Also, adsorption process is an endothermic in nature and desorption is achieved well for three cycles by MUiO-66. Therefore, UiO-66 and MUiO-66 obtained in this work have a great promise in adsorption of heavy metals such as Pb and Cd(II) ions from wastewater.

Materials Chemistry

Polymer Science

UiO-66

metal-organic framework

Modification

Melamine

Adsorption

Lead (II)

Cadmium (II)

With the development of industrial and agricultural modernization, an increase in the activities of mining, electroplating, smelting, batteries industry and others is occurred and caused serious water pollution with heavy metals such as cadmium (Cd), copper (Cu), lead (Pb), arsenic (As) and chromium (Cr), which cause high toxicity to human and environment. Heavy metals are difficult to be degraded in water, and can cause serious threats to the survival of aquatic organisms or enter the human body through the food chain to cause health risks. For example, lead can cause many diseases related to digestive, circulatory, respiratory and other systems, and even death when it enters the human body. Also, cadmium ions can accumulate in the body and cause diseases of the lung, bone and kidney. Thus, it is essential to develop promising techniques for simultaneous removal of Pb (II) and Cd(II) from wastewater prior to their discharge into the environment. To date, the treatment techniques for heavy metals contaminated wastewater mainly include chemical precipitation, electrolysis, ion exchange, biological treatment and adsorption (1-5). The efficiency of these processes depends on its nature and the contaminated pollutants. Among these methods, the adsorption process is the more acceptable to apply for their simplicity and low cost (1, 2). The most familiar adsorbent materials are activated carbons, carbon nano-particles, zeolite, clays, fly ash and some metal oxides (6-9). Often these adsorbents materials need pretreatments to increase their removal efficiency. During the last three decades, the works directed to the synthetic adsorbents with high surface area and environmentally friendly such as metal-organic frameworks (MOFs).

Metal-organic frameworks (MOFs) are novel class of porous crystalline materials composed of two fragments, i.e. inorganic cations and organic linkers (10). Such materials have quickly moved to the forefront of materials research due to their extraordinary internal surface areas and porosity, chemical stability, and surface capability to selectively capture of guest species (10-19). Accordingly, MOFs can be used in many applications such as gas storage, separation, catalysis, sensing, drug delivery, biological and proton conduction.

Recently, MOFs have attracted great interest with respect to the capture of hazardous pollutants which existed in wastewater (10, 11). These materials are recognized to be considerably superior adsorbents as compared to conventional materials such as activated carbons and zeolites (14). Among various MOFs, UiO-MOF formulations (UiO-66, UiO-67, UiO-68, and UiO-69) have superior stability in different chemical media with large porosity (11, 16-21). Thus they can be emerged as effectively adsorbents for removal of heavy metal ions from a variety of wastewater samples (11, 16). It was found that the maximum adsorption capacity of melamine-UiO-66 prepared hydrothermally at 120^oC toward Pb(II) was 122 mg/g (16). However in another study, NH₂-functionalized Zr-MOFs sample prepared via rapid microwave were examined for removal of Pb and Cd (II) ions. The adsorption capacity was reached to 166.7 mg/g of Pb (II) and 177.3 mg/g of Cd(II) ions (21).

In a recent paper by Hanna et al. (22), Cu-MOF and Cu-MOF modified with melamine were prepared and used as antimicrobial agents. The results showed that both MOF samples exhibited a high antimicrobial activity and the incorporation of melamine to Cu-MOF increased this activity. Objective of the current study is to prepare MOF samples of UiO-66 hydrothermally at 140^oC for 36 h and then UiO-66 was modified with melamine (MUiO-66); not like conditions reported by Yin et al. (16) at 120^oC for 24h. The adsorption experiments of Pb (II) and Cd (II) from their aqueous solutions were conducted using the obtained MOF materials. With regard to this, the adsorption of both metal divalent ions was performed under varying conditions of pH, metal ion concentration, contact time, adsorbent dose and temperature. Equilibrium adsorption studies were analyzed using Lagergren’s pseudo first-order and pseudo second-order models as well as Langmuir, Freundlich, and Dubinin–Radushkevich (D-R) and Redlich-Peterson isotherms were applied to identify the adsorption behavior of Pb and Cd (II) ions by UiO-66 and MUiO-66 adsorbents.

2.1 Materials

Anhydrous N, N-dimethylformamide (DMF, 99%), terephthalic acid (H₂BDC, 98%), melamine, ethanol and zirconium tetrachloride (ZrCl₄) were obtained from Sigma Aldrich.

2.2 Synthesis of UiO-66

Synthesis of UiO-66 was carried out by hydrothermal method through dissolving 0.480g of Zirconium tetraclorid (ZrCl₄) and (3.66 g) terephthalic acid (H₂BDC) in 45 mL N, N-Dimethylformamide (DMF), and then stirred with magnetic stirrer for 60 minutes. The reaction mixture was then heated in an oven at 140°C for 36 h. The reaction mixture was removed from the oven and allowed to cool at room temperature. The solvent was then removed from the vial bottles by decantation, the solid was washed by adding 45 mL of DMF and left for 24 hours. The washing process was repeated twice with chloroform as the solvent. The obtained solid was then dried under vacuum at 60°C.

2.3. Synthesis of melamine-coated UiO-66 (MUiO-66)

About 0.5 g of UiO-66 and 1.0 g of melamine (M) were dispersed in 50 mL and 100 mL absolute ethanol, respectively. The two dispersions were mixed and sonicated for 10 h before the mixture was transferred to a flask. When the condensation reflux reaction had lasted for 24 h at 100°C, the product was centrifugally rinsed with absolute ethanol and vacuum desiccation at 50°C overnight to obtain melamine-coated UiO-66 (MUiO-66).

2.4 Characterization Techniques

The dried samples were exposed to different techniques as follows.

Transmission Electron Microscope (TEM) to identify the morphology and the particle size of the prepared samples was examined by using a transmission electron microscope (TEM) quanta FEG working at 100 keV.

BET surface area measurements were performed at liquid nitrogen temperature (−196°C) with an Auto-sorb BET apparatus from Quanta chrome Corporation. The BET analysis procedure is automated and operates with the static volumetric technique. Before each measurement, the samples were degassed firstly at 200°C for 2 hours, at 5 × 10⁻³torr and then at room temperature for 2 hours, at 0.75 × 10⁻⁶torr. The isotherm methods were used to determine the specific surface areas using the BET equation.

Fourier transforms infrared (FTIR) spectroscopy to give the main functional groups on the obtained samples was done using a KBr disk technique and FTIR 6500 spectrometer (JASCO, Japan) in the range of 400-4000cm⁻¹.

X-ray diffraction (XRD) analysis to determine the main crystalline was performed with power D8 ADVANCE diffractometer (Germany) using CuKa radiation (1.542°A, 40 KV, 40mA) in the 2Ө range of 4–80. The acquisition parameters were as: a step size of 0.02 and a step time of 0.4s.

Thermal analysis (TGA) was performed by USA Berkin – Elmer thermo-gravimeter. Samples of approximately 10 mg were heated from 50^oC to 800^oC with heating rate 10/m under a nitrogen atmosphere, and the flow of nitrogen was 50 mL/min.

2.5. Adsorption studies

The adsorption behavior of the prepared MOFs for metal ions of Pb (II) and Cd (II) was investigated by batch removal experiments at room temperature (298K). Stock solutions of the metal ions were prepared using Pb(NO₃)₂.6H₂O and CdCl₂ salts dissolved in deionized water. Freshly prepared working metals solutions of concentrations 10 mg/ l by diluting stock solutions with deionized water were used in the experiments. The samples were collected at different time intervals and filtered with a 0.45 µm syringe filter membrane. The pH effect on the adsorption was studied by adjusting the solution pH with sodium hydroxide (NaOH) and nitric acid (HNO₃).The effect of adsorbent dose was studied by changing the dose from 0.05 -2 g/L. All adsorption tests were performed in triplicate.

The removal efficiency and the adsorbed amount were calculated using the following equations:

$$Metals Removal \left(\%\right)=\frac{Co-Ce}{Co}\times 100$$

The experimental data obtained in batch studies were used to calculate the adsorption capacity q_e (mg/g) at equilibrium using the following equation,

$${q}_{e = }({C}_{^\circ }-{C}_{e})\frac{V}{m}$$

Where C₀ and C_e are the initial and equilibrium concentrations (mg/L) of the metal solutions, respectively. V (L) is volume of metal solution and m (g) is the total mass of the used adsorbent.

To investigate the adsorption performance, adsorption isotherms for the individual adsorption of (Pb (II), and Cd (II)) were studied by contacting the optimum dose of adsorbent with different metals solutions at different initial concentration (25-250 mg/L).

The data of isotherms were analyzed, fitted and plotted using Origin Pro 2016 Ver. 9.3.226 for different non-linear regression models as shown in Table 1.

Table 1

Texture properties of UiO-66 and MUiO-66
Materials	BET Surface area (m² g⁻¹)	Pore volume (cm³ g⁻¹)
UiO-66	1080	0.58
MUiO-66	1160	0.70

The mechanism of adsorption was studied by applying kinetic models using the optimized dose and pH for different time intervals (5, 10, 15, 20, 25, 30, 40,60, 90, 120, 150 min) and the used kinetic models are shown in Table 1.

Thermodynamic studies are important to determine the feasibility and spontaneity of the adsorption process. Thermodynamic parameters as Gibbs free energy (ΔG°), the enthalpy change (ΔH°) and entropy change (ΔS°) were obtained by applying the adsorption of Pb(II) and Cd(II) ions at different temperatures (T= 313,333 and 353 K) and the experimental data obtained were fitted by the following equations:

$${\Delta }\text{G}^\circ =-\text{R}\text{T} \text{l}\text{n}{K}_{d}$$

$${\text{K}}_{\text{d}}\text{=}\frac{\text{∆ S}}{\text{R}}\text{–}\frac{\text{∆H}}{\text{RT}}$$

Where, K_d is the distribution coefficient of the solute which is equal q_e/C_e, and R is the ideal gas constant (8.314 J/mol K).

2.6 Desorption studies of metal ions

Desorption studies were done to estimate and reusability of adsorbents and leaching studies of metal-loaded MOF samples under initial concentration of metal ions 10 mg/L and room temperature. After adsorption experiments, metal ions were eluted using HNO₃ 0.1 M. After desorption, the MOF sample was separated by filtration and metals concentrations were measured then the adsorbent was rinsed with deionized water till the pH was neutral then dried and reconditioned for reuse in another run.

3.1 General features of UiO-66 and MUiO-66

Figure 1 represents the TEM image of UiO-66 and MUiO-66. It can be concluded that the UiO-66 particles were formed from aggregated spheres-like with particle sizes ranged between 20-60 nm as shown in Fig. 1A. This result is consistent with previous study on UiO-66 (16). Upon modification of UiO-66 with melamine, TEM image of MUiO-66 (Fig. 1B) shows covering the surface of UiO-66 with layers from melamine molecules. This treatment enhanced the porous properties and crystallinity of UiO-66 as shown in BET and XRD measurements.

Table 1 lists the BET surface area measurements of the parent UiO-66 and one coated with melamine (MUiO-66). Results explain that the total surface area of UiO-66 equals to 1080 m²/g and total pore volume 0.58 cm³/g while the MUiO-66 has a larger total surface area about 1160 m²/g and total pore volume 0.70 cm³/g. This indicates that both the surface area and pore volume improved by introducing the melamine molecules into the surface of UiO-66. Yin et al. (16) prepared UiO-66 and melamine-UiO-66 during the hydrothermal route at 120^oC for 24 h and found that the total surface areas of both products were 303 and 371 m²/g, respectively, which are lesser than those obtained in this study. On the other hand, Shearer et al. (18) synthesized UiO-66 functionalized with L-Serine and monoethanol amine and activated with HCl having BET-surface areas ranged from 1372 to 1903 m²/g. By the way, the higher total surface area and total pore volume is the larger adsorption capacity and thus MOFs of UiO-66 can candidate to use in the removal of heavy metals from aqueous solutions.

As shown in Fig. 2, FTIR spectra of UiO-66 and MUiO-66 samples are measured. Regarding UiO-66 (Zr), the strong bands belonging to the O-C-O asymmetric and symmetric stretching in the H₂BDC ligand can be found at 1600 and 1419 cm⁻¹. The weak band at 1510cm⁻¹ demonstrates the vibration C=C of a benzene ring. The peaks at 808, 746, and 658 cm⁻¹ are combined with C-H vibration, C=C stretch, OH bend and O-C-O bend in the H₂BDC ligand. In addition, a band related to the C=O asymmetric stretch of the DMF can be demonstrated at 1655 cm⁻¹, which means that DMF resides in the pores. However, no absorption band was observed in 1685 cm⁻¹, which is related to the carboxylate vibration bands of the free H₂BDC ligand, indicating that all carboxylates are connected to zirconium (Zr) ions (18). The absorption bands of FTIR at 3121, 3324, 3415 and 3467 cm⁻¹ (NH₂ stretching), as well as 1651 cm⁻¹ (C=O stretching), which are attributable to primary amine group of melamine, have disappeared or drastically reduced upon reaction of the MOFs with melamine in the synthesis of melamine-MOFs [16, 18, 20]. In addition, the structures of the triazine ring give the strong stretching vibration bands at 1465 cm⁻¹ (C=N vibration), mirroring the successful incorporation of the melamine into the framework (16, 20). The amino groups (-NH₂) have lone pair electrons and act as the Lewis base, they can form coordinate bonds with the heavy metal ions (Lewis acids) (21).

The XRD patterns of the unmodified and modified MOFs (Fig. 3) were very similar, confirming the successful synthesis and the integrity of the crystal structure after modification with melamine. The melamine-UiO-66 MOF exhibited higher peak intensities at about 2θ = 7.4°, 8.5°, 15° and 15.8° showing an increase in the crystalline degree of the UiO-66. Moreover, the two diffraction peaks of the melamine (2θ = 26°and 30°) were seen in the XRD patterns of the melamine-MOFs (16, 18). Thus, there might be mainly chemical interaction between melamine and the MOFs during the prescribed method.

Figure 4 represents the thermo-gravimetric analysis (TGA) of the UiO-66 and melamine/UiO-66 (MuiO-66). From this UiO-66 it is observed that the thermal degradation of the sample passes through at three progressive steps. The first one starts from the room temperature and ends nearly at 150^oC can be attributed to evaporate the water content and the other volatile materials. The second step starts gradually until t0 200^oC and then the degradation become rapidly until 350^oC, and this step represents the main degradation of the UiO-66. The third steps starts at 350^oC and continue in the degradation to the 800^oC. This stage may due to the decomposition of the inorganic fragments. For MUiO-66, it is observed that there are similarities with that observed for the sample without melamine. In comparison between the two profiles it is observed that the thermal degradation of the main product goes gradually between about 200^oC to 350^oC and continues. This may be due to the presence of the melamine as confirmed by previous work (16, 18).

3.2 Factors affecting adsorption studies

3.2.i Effect of pH

Figure 5 shows the variation of % removal of both heavy metals using two MOF samples with increasing pH of solution from 2 to 7. The highest removal of Pb (II) and Cd (II) ions is occurred at pH of 5. Increasing pH over 5, the % removal of both metals decreases slightly as result of presence of Pb(OH)₂ or Cd(OH)₂ in the solution. It can be seen that MUiO-66 exhibits a high removal of Pb and Cd (II) ions (> 75% removal) within studied pH range between 2 and 7. This confirms the superiority of MUiO-66 adsorbent to work at different media of pH.

3.2. ii Effect of initial concentrations and contact time

Figure 6 illustrates the removal percentage of both Pb and Cd ions by UiO-66 and MUiO-66 samples as function of variation in contact time and initial concentrations of metal ions studied here. When initial concentrations of metal ions increase from 5 to 100 mg/L the removal percentage of Pb and Cd divalent ions is decreased gradually by both samples. MUiO-66 sample exhibits superior removal toward both metal ions than by UiO-66 sample because of it possesses high total surface area and accessible micropores in addition to presence of –NH₂ groups. In addition, the removal percentage of Pb (II) (91-83% at 5 min and 96-88% at 150 min) ions is higher than that of Cd (II) ions (74-66% at 5 min and 84-73%) by UiO-66 as concentration increases from 5 to 100 mg/L. This finding may be ascribed to that the hydrated ionic radius of cadmium ions (0.426 nm) is greater than that of lead ions (0.401 nm) when attached with water molecules (23, 24).

Generally, the removal of both metals ions is increased by increasing the contact time and equilibrium time is occurred almost after 50 min for Pb (II) ions and 60 min for Cd (II) ions adsorption over both MOF samples. For Pb (II) adsorption, the removal by two samples is very fast at early stage and then began to be slow at equilibrium that is owing to the saturation of the available adsorption sites.

3.2. iii Effect of MOF dosage

Figure 7 depicts the effect of UiO-66 and MUiO-66 samples on the adsorption of Pb and Cd (II) ions at pH 5 and 25^oC. As MOF dosage increases from 0.05 to 1 g/L, the removal of each metal ion increases gradually and then starts to decrease slightly at 1.5g/L, resulting in the high availability of binding sites on the surface at a higher adsorbent dose. Thus, a 1 g/L adsorbent was selected as adsorbent dosage for all further experiments due to its higher removal efficiency.

Based on the high removal efficiency of lead and cadmium by MUiO-66 sample under varying variables such as pH, initial concentration, contact time and adsorbent dosage, this sample was used to estimate the kinetic and equilibrium adsorption of Pb and Cd (II) ions using different models as summarized in Table 2.

Table 2

Kinetics and isothermal models (Non-linear form)
	Non-linear form	Parameter
Kinetics models Pseudo-first order	${q}_{t}= {q}_{e}-\left(1-{\text{e}}^{\left({\text{-K}}_{1}t\right)}\right)$	k₁(1/min) is the pseudo-first-order rate constant
Pseudo-second order	${q}_{t}=\frac{{K}_{2}{q}_{e}^{2} t}{1+{k}_{2}{q}_{e }t}$	k₂ (mg/g min) is the pseudo-second-order rate constant
Isotherm models	${q_e}={K_F}C_{e}^{{1/n}}$	k_F (L/g) Freundlich constant related to adsorption capacity, n Freundlich constant related to adsorption intensity. q_m (mg/g) maximum monolayer adsorption capacity, k_L (L/mg) Langmuir equilibrium constant.
Freundlich model	${q_e}={K_F}C_{e}^{{1/n}}$
Langmuir model	${q_e}={q_m}{K_L}\frac{{{C_e}}}{{1+{K_L}{C_e}}}$
Dubinin-Radushkevich (DR) model	${\text{q}}_{\text{e}}\text{ = }{q}_{\text{D}-\text{R}}{e}^{\left[-{k}_{D-R}{\left(\text{RTln}\left(\text{1+}\frac{\text{1}}{{\text{C}}_{\text{e}}}\right)\right)}^{\text{2}}\right]}$ $\text{E}=\frac{1}{\sqrt{-2{\beta }}}$	q_D−R (mg/g) maximum adsorption capacity k_D−R (mol²/J²)constant related to the mean free energy of adsorption R ( 8.314 J/mol K) general gas constant T (K) absolute temperature E (kJ/mol) mean free energy:
Redlich–Peterson model	${q}_{e}=\frac{{K}_{RP}{C}_{e}}{1+{a}_{RP}{C}_{e}^{g}}$	K_RP (L/mg) is R–P constant related to the adsorption capacity, a_RP (L/mg) is a constant related to the affinity of the binding sites , g (g) is an exponent related to the adsorption intensity.

3.3 Equilibrium adsorption studies

Lagergren’s pseudo first-order and pseudo second-order models were used for analysis of adsorption kinetics as shown in Table 2.

The Lagergren’s first-order rate constant (k₁) and q_e are calculated from the intercept and slope of the plot between t (min) versus log (q_e-q_t) and listed in Table 3 along with the corresponding correlation coefficients (R²). It was observed that the pseudo first-order model did not fit well the adsorption of Pb and Cd (II) ions by MUiO-66 sample because the calculated q_e values do not agree with the experimental q_e values. This suggests that the adsorption of studied metal ions does not follow first-order kinetic model. On the other hand, the equilibrium sorption capacity (q_e) and the second-order constant k₂ (g/mg min) can be determined experimentally from the slope and intercept of plot t/qt versus t. The values of k₂ and q_e are listed in Table 3 along with the corresponding correlation coefficients (R² = 0.99). It can be seen that there is an agreement between experimental and calculated q_e values for the pseudo second-order model with R² closing to unity (Table 3). Hence, the pseudo second-order model better represents the sorption kinetics.

Table 3

Parameters for kinetics and isotherm models fit
Metal	Pseudo-first order
	q_e,_exp.(mg/g)			q_e,_Cal (mg/g)			K₁						R²
Pb(II) Cd(II)	9.4 8.3		0.89 1.7					0.05 0.03			0.06 0.07
	Pseudo-second order
	q_e,_Cal (mg/g)			K₂ (g /mg.min)					R²
Pb(II) Cd(II)	9.7 8.4	0.14 0.04				0.99 0.99
	Langmuir isotherm parameters
	q_m (mg/ g)				K_L (L/mg)							R²
Pb(II)	177.5				0.07					0.99
Cd(II)	146.6				0.03					0.98
	Freundlich isotherm parameters
	1/n				K_F (L/mg)							R²
Pb(II)	0.38				29							0.94
Cd(II)	0.45				13							0.95
	D-R isotherm parameters
	q_K−D(mg /g)				E(kJ/mol)							R²
Pb(II)	144				11							0.91
Cd(II)	110				9.7							0.90
	Redlich–Peterson parameters
	K_R (L/mg)				a_R (L/mg)					g (g)		R²
Pb(II)	13.4				0.07					1		0.98
Cd(II)	5.5				0.075					0.86		0.95

Figure 8 shows the studied adsorption isotherms of Pb and Cd (II) ions onto MUiO-66. Meaning, the Langmuir, Freundlich, Dubinin–Radushkevich (D-R) and Redlich-Peterson isotherms (Table 2) were applied to identify the best model fitting the adsorption of both metal ions onto MUiO-66. Constants calculated from these isotherms with the corresponding values of R² are listed in Table 3. Values of R² showed that the adsorption of both metals ions fits finely the isotherms in the sequence order: Langmuir > Redlich-Peterson > Freundlich> D-R. The fact that the Langmuir isotherm fits the adsorption data very well may be attributed to the homogeneous distribution of active sites on MUiO-66 sample. Maximum monolayer adsorption capacity of MUiO-66 accounted from Langmuir isotherm (q_m, mg/g) toward adsorption of Pb (II) and Cd (II) ions was approximately 178 and 147 mg/g, respectively. This finding pointed out the preference of lead adsorption exhibited by MUiO-66 over Cd (II) ions which may be attributed to smaller hydrated radius of Pb (II) ions (23). The MUiO-66 obtained in this study exhibited superb adsorption capacity as compared to that was prepared by Yin et al. [16]. Calculated mean free energy (E, kJ/mol) from DR isotherm can identify the type of adsorption whether is physical or chemical. When the E value ranged between 8 – 16 kJ/mol, the adsorption process is chemical in nature (25, 26). In our study, the value of E is found to be less than 16 kJ/mol, and thus the adsorption of metal ions is a physisorption (25-31).

3.4 Influence of temperature and thermodynamic studies

The feasibility of the adsorption was analyzed by studying the changes in different thermodynamic parameters, such as ΔG^o, ΔH^o and ΔS^o with temperature by the Van’t Hoff plot (Eq. 4). The temperature affected the adsorption, where the ion mobility of Pb (II) and Cd(II) ions increased with the temperature and the adsorption is enhanced due to the increased in ions number on the active sites of the MOF adsorbent. The calculated parameters for the tested metal ions are listed in Table 4. The negative values of ΔG^o for Pb (II) and Cd(II) ions adsorption revealed that the adsorption was spontaneous. Values of ΔG^o are ˂ –20 kJ/mol and suggested to be obtained for the physical adsorption and the interaction occurs between the metal ion and the active sites existed on MOF's surface (25, 26). The positive value of ΔH^o (Table 4) for Pb (II) and Cd(II) adsorption, suggested that the adsorption was endothermic process. The positive value of ΔS^o reveals the randomness between the solid and liquid surface confirming the high affinity between the adsorbent and metal ions (25).

Table 4

Thermodynamic parameters for the adsorption of Pb (II) and Cd (II) ions at different temperatures.
Metal	Temperature (K)	ΔG (kJ/mol))	ΔH(kJ/mol)	ΔS (J/mol K)
Pb(II)	313 333 353	-7.6 -8.7 -11.4	21.4	92.2
Cd(II)	313 333 353	-4.5 -6.4 -7.2	16.4	67.4

3.5 Desorption studies

The reusability experiments of metal loaded adsorbents were carried out and results are shown in Fig. 9. An increase in desorption for Pb(II) and Cd(II) at low pH values was observed. By applying adsorption/ desorption cycles, a small loss (8%) in the adsorption efficiency for the prepared MUiO-66 starting from the third cycle, revealing the good reusability of the prepared adsorbent.

Table 5 lists the adsorption capacities of some adsorbents used in removal of lead and cadmium ions. Results in the table affirms the highest performance of MOFs toward removal of lead and cadmium ions, excepting the natural zeolite which exhibited a superior capacity toward Pb(II) and a lower adsorption of Cd (II) as compared to MUiO-66 prepared in this study.

Table 5

Adsorption capacities of various adsorbents for adsorption of Pb and Cd (II) ions.
Adsorbents	Adsorption Capacity (mg/g)		Ref.
Adsorbents	Pb (II)	Cd (II)	Ref.
HCl-treated Egyptian Kaolin	34.5	-	[6]
UiO-66 Melamine-UiO-66	72 122	- -	[16]
UiO-66 MOFs	110-175	-	[17]
NH2 functionalized Zr-MOFs	166.7	177.3	[21]
semi–carbonized/H₃PO₄ cotton stalks	-	31.6	[23]
KOH-activated carbons	50	-	[27]
H₃PO₄-Activated carbons	-	83.4	[28]
biosilica extracted from marine diatom	120.4	-	[29]
Amino-MIL-101 (Cr)	81.1	-	[30]
Zeolite	286	44.6	[31]
MUiO-66	177.5	146.7	This study

From the analysis of the results, it may conclude that UiO-66 composed of sphere-like particles and covered by layers of melamine with enhanced in crystallinity and active surface sites as a result of an incorporation of the melamine. The incorporation of melamine into the UiO-66 increased the surface area from 1080 to 1160 m²/g. The maximum adsorption capacity was found 177.5 and 146.6 mg/g at pH = 5.0 for Pb(II) and for Cd(II), respectively. A better fit of the adsorption results was achieved using Langmuir isotherm with physisorption of both metals ions onto the studied MUiO-66. Pseudo-second order kinetic model had the best fit for the obtained experimental data, indicating that the rate limiting step is chemisorption. The adsorbed metal ions were then desorbed and the prepared MUiO-66 was reused efficiently for other cycles of adsorption. Also, the results show that both UiO-66 and MUiO-66 have high adsorption efficiency as compared with examples of the adsorbent materials in literature.

Acknowledgements

The authors submit their acknowledgment to their institute (National Research Centre, Cairo, Egypt) for encouragement the team work to do this work.

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High Performance of UiO-66 Metal-Organic Framework Modified with Melamine for Uptaking of Lead and Cadmium from Aqueous Solutions

Status:

Journal Publication

Version 1

Abstract

Figures

1 Introduction

2 Experimental

2.1 Materials

2.2 Synthesis of UiO-66

2.3. Synthesis of melamine-coated UiO-66 (MUiO-66)

2.4 Characterization Techniques

2.5. Adsorption studies

2.6 Desorption studies of metal ions

3 Results And Discussion

3.1 General features of UiO-66 and MUiO-66

3.2 Factors affecting adsorption studies

3.2. ii Effect of initial concentrations and contact time

3.2. iii Effect of MOF dosage

3.3 Equilibrium adsorption studies

3.4 Influence of temperature and thermodynamic studies

3.5 Desorption studies

4 Conclusions

Declarations

References

Status:

Journal Publication

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	Non-linear form	Parameter
Kinetics models Pseudo-first order	\({q}_{t}= {q}_{e}-\left(1-{\text{e}}^{\left({\text{-K}}_{1}t\right)}\right)\)	k₁(1/min) is the pseudo-first-order rate constant
Pseudo-second order	\({q}_{t}=\frac{{K}_{2}{q}_{e}^{2} t}{1+{k}_{2}{q}_{e }t}\)	k₂ (mg/g min) is the pseudo-second-order rate constant
Isotherm models	\({q_e}={K_F}C_{e}^{{1/n}}\)	k_F (L/g) Freundlich constant related to adsorption capacity, n Freundlich constant related to adsorption intensity. q_m (mg/g) maximum monolayer adsorption capacity, k_L (L/mg) Langmuir equilibrium constant.
Freundlich model	\({q_e}={K_F}C_{e}^{{1/n}}\)
Langmuir model	\({q_e}={q_m}{K_L}\frac{{{C_e}}}{{1+{K_L}{C_e}}}\)
Dubinin-Radushkevich (DR) model	\({\text{q}}_{\text{e}}\text{ = }{q}_{\text{D}-\text{R}}{e}^{\left[-{k}_{D-R}{\left(\text{RTln}\left(\text{1+}\frac{\text{1}}{{\text{C}}_{\text{e}}}\right)\right)}^{\text{2}}\right]}\) \(\text{E}=\frac{1}{\sqrt{-2{\beta }}}\)	q_D−R (mg/g) maximum adsorption capacity k_D−R (mol²/J²)constant related to the mean free energy of adsorption R ( 8.314 J/mol K) general gas constant T (K) absolute temperature E (kJ/mol) mean free energy:
Redlich–Peterson model	\({q}_{e}=\frac{{K}_{RP}{C}_{e}}{1+{a}_{RP}{C}_{e}^{g}}\)	K_RP (L/mg) is R–P constant related to the adsorption capacity, a_RP (L/mg) is a constant related to the affinity of the binding sites , g (g) is an exponent related to the adsorption intensity.