Adsorption behavior of Fe (III) in aqueous solution on melamine

Peng, Hao; Guo, Jing; Wang, Bingqing

doi:10.2166/wst.2020.455

Cited by 9 publications

(5 citation statements)

References 34 publications

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“…The adsorption capacity determined by the pseudosecond-order kinetic model shows greater concordance with experimental results compared to its pseudo-first-order counterpart (Table 3). Parallel results were found in a separate study, which established that the adsorption of melamine on Fe(III) and Mn(II) ions adheres to a pseudo-second-order kinetic model (Peng et al, 2020).…”

Section: Adsorption Kinetics and Isothermsupporting

confidence: 70%

Magnetic Composite for Efficient Adsorption of Iron and Magnesium Ions from Aqueous Solution

Purwaningrum,

Hasanudin,

Rachmat

et al. 2023

Ecol. Eng. Environ. Technol.

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Iron Fe(III) and Manganese Mn(II) ions were effectively removed from aqueous solutions using a magnetic composite of Fe 3 O 4 /CaO/PDA, with CaO sourced from green mussel. The composite material was comprehensively characterized using Fourier Transform Infrared Spectroscopy (FTIR), X-ray Diffraction (XRD), Scanning Electron Microscopy with Energy Dispersive -X-ray Spectroscopy (SEM-EDS), Brunauer, Emmett and Teller (BET) surface area analysis, Vibrating Sample Magnetometer (VSM). The impact of physicochemical adsorption parameters, such as solution pH, contact time, and concentration, were investigated. The Fe 3 O 4 /CaO/PDA composite displayed a value of 51.47 emu/g in saturation magnetization, enabling rapid separation through the use of an external magnet without the need for filtration. Optimal conditions for adsorbing Fe(III) ions were achieved at pH 3 and initial concentration of 400 mg/L with maximum efficiency reach after 60 minutes. Similarly, optimal conditions for Mn(II) ion adsorption were observed at pH 4 with the same contact time and initial concentration. The adsorption efficiencies were found to be 88.56% for Fe(III) and 75.65% for Mn(II). The pseudo-second-order model aptly depicted the kinetics associated with the adsorption of both types of ions while the Langmuir isotherm model indicated that monolayer adsorption takes place on the composite's surface. The maximum capacities for adsorption is 322.58 mg/g for Fe(III) ions and 208.33 mg/g for Mn(II) ions. A negative Gibbs free energy value affirmed that the process occurs spontaneously under natural conditions. These results underscored the potential use of this Fe 3 O 4 /CaO/PDA composite in treating wastewater to remove heavy metal ions.

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Section: Adsorption Kinetics and Isothermsupporting

confidence: 70%

Magnetic Composite for Efficient Adsorption of Iron and Magnesium Ions from Aqueous Solution

Purwaningrum,

Hasanudin,

Rachmat

et al. 2023

Ecol. Eng. Environ. Technol.

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“…There are not enough vacant sites for vanadium adsorption on the GA surface at low GA dosage, and the number of vacant sites increases with the increase of GA dosage. 43 Thus, the adsorption efficiency increases with a continuous increase of GA dosage. The adsorption efficiency of vanadium increased from 74.48 to 91.66% as dosage of GA increased from n (glu)/ n (V) = 0.6 to n (glu)/ n (V) = 3.0.…”

Section: Resultsmentioning

confidence: 97%

“…During the adsorption process, the VO 2 + was adsorbed on the surface of GA by hydrogen bonds or van der Waals force. There are not enough vacant sites for vanadium adsorption on the GA surface at low GA dosage, and the number of vacant sites increases with the increase of GA dosage . Thus, the adsorption efficiency increases with a continuous increase of GA dosage.…”

Section: Resultsmentioning

confidence: 98%

“…Increasing the concentration of H 2 SO 4 can make the solution acidic, and vanadium will transform into cations. When the concentration of H 2 SO 4 is over 20 g/L (pH < 1.5), vanadium mostly exists as VO 2 + , which makes a great contribution to high adsorption efficiency of vanadium. ,, Further increasing the concentration has no obvious effect on adsorption efficiency; thus, 20 g/L is chosen as the optimal concentration of H 2 SO 4 for further experiments.…”

Section: Resultsmentioning

confidence: 99%

“…The beaker is placed in a water bath. When the solution is heated to a scheduled temperature, GA is added into the solution and then stirred at 500 rpm for the required reaction time. ,,, The reaction solution is filtrated by vacuum filtration, and then, the concentration of residual vanadium is determined by inductively coupled plasma–optical emission spectrometry. The adsorption efficiency of vanadium is calculated as follows (eq ): where C 0 is the initial concentration of vanadium, mg/L; C t is the concentration of vanadium at different times t , mg/L.…”

Section: Methodsmentioning

confidence: 99%

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Thermodynamic and Kinetic Studies on Adsorption of Vanadium with Glutamic Acid

et al. 2021

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Many hydrometallurgy methods, including chemical precipitation, ion exchange, solvent extraction, and adsorption, have been used to recover vanadium from vanadium solution, but the final step of these methods involved precipitation with ammonium salts, high concentrations of which are harmful to the environment. The key point is to find a new compound to replace ammonium salts without reducing the vanadium precipitation efficiency. The adsorption process of vanadium with glutamic acid is investigated. The effects of experimental factors, including dosage of glutamic acid, reaction temperature, concentration of H 2 SO 4 , and reaction time, on the adsorption process are investigated. The results show that nearly 91.66% vanadium is adsorbed under the following reaction conditions: reaction temperature of 90 °C, H 2 SO 4 concentration of 20 g/L, glutamic acid dosage at n (glu)/ n (V) = 3.0:1, and reaction time of 60 min. The response surface methodology is applied to optimize the reaction conditions. The analysis results indicate that the reaction temperature has the greatest effect on the adsorption efficiency of vanadium and the influence of experimental factors follows the order: reaction temperature > dosage of glutamic acid to vanadium > reaction time > concentration of H 2 SO 4 . The pseudo-second-order model is selected to describe well the adsorption kinetic behavior, and the thermodynamic analysis results indicate that the adsorption process of vanadium is unspontaneous and exothermic. The results will be useful for further applications of glutamic acid, and they provide a bright future for vanadium recovery.

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