Comparison of Solid−Liquid Equilibrium Data for the Adsorption of Propionic Acid and Tartaric Acid from Aqueous Solution onto Amberlite IRA67 (original) (raw)
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Chemical Engineering Journal, 2009
Formic acid is an important chemical and biochemical compound used in various industries. It is important to separate this acid from wastewater streams. In this study, adsorption of formic acid was studied from aqueous solution by using weakly basic adsorbent (Amberlite IRA-67) at three different temperatures (298 K, 318 K, and 328 K). Adsorption of formic acid was investigated in terms of equilibrium, kinetics and thermodynamic conditions. Optimal amount of IRA-67 was determined as 1.00 g. The most used isotherms, Freundlich and Langmuir, were applied to experimental data. Langmuir isotherm gave good results with R 2 value over 0.99 at different temperatures. Pseudo-second-order model was fitted for this adsorption system. Thermodynamic parameters, H • ads , S • ads and G • ads , were calculated.
Adsorption Equilibria of l -(+)-Tartaric Acid onto Alumina
Journal of Chemical and Engineering Data, 2009
The adsorption equilibria of L-(+)-tartaric acid onto alumina from wastewaters of wineries were studied, and it has been found that the equilibrium adsorption fits the Langmuir and Freundlich isotherms. Adsorption experiments were carried out at three different temperatures (298, 310, and 325) K. The adsorption of L-(+)tartaric acid is dependent on the acid concentration and the amount of alumina. The maximum percentage removal of L-(+)-tartaric acid was 22 % by alumina at 298 K. The Langmuir and Freundlich constants have been found to be 0.023 g · g -1 and 0.014 (g · g -1 )/(L · g -1 ) -1/n , respectively, at 298 K. The thermodynamic parameters ∆H ads 0 and ∆S ads 0 for the adsorption of tartaric acid on alumina have been calculated to be -5.62 kJ · mol -1 and 50.65 J · mol -1 · K -1 , respectively.
Adsorption of Picric Acid from Aqueous Solution by the Weakly Basic Adsorbent Amberlite IRA-67
Journal of Chemical & Engineering Data, 2010
The presence of nitrophenols in wastewater is of great environmental concern. Therefore, it is important to separate picric acid from wastewater streams. In this study, adsorption of picric acid was studied from aqueous solutions by using a weakly basic adsorbent (Amberlite IRA-67) at three different temperatures (298 K, 308 K, and 318 K). Adsorption of picric acid was investigated in terms of equilibrium, kinetics, and thermodynamic conditions. In the equilibrium studies, 1.00 g of Amberlite IRA-67 was determined as the optimal amount. The most used isotherms, Freundlich and Langmuir, were applied to the experimental data. The Langmuir isotherm gave good results with R squared values over 0.99 at different temperatures. In the kinetic studies, pseudofirst-and pseudosecond-order models and the Elovich equation were applied to the kinetic experiments. The pseudosecond-order model was fitted to this adsorption system with an R squared value of 0.996. In the thermodynamic studies, ∆H ads 0 ) -21.204 kJ · mol -1 , ∆S ads 0 ) -200.043 J · mol -1 · K -1 , and ∆G ads 0 for different temperatures were calculated.
Journal of Chemical & Engineering …, 2011
The adsorption equilibria of propionic acid and glyoxylic acid on alumina are investigated experimentally and theoretically in this study. Alumina was used as the adsorbent. The period of achieving the equilibrium state and the effects of the amount of adsorbent, temperature, and initial acid concentration were investigated experimentally. Langmuir, Freundlich, and Temkin adsorption isotherm equations are fitted well with the experimentally measured data. It was found that the equilibrium isotherms depended on the initial acid concentration significantly. The Langmuir isotherm was found to best represent the data for both of the acids. The pseudosecond-order model, intraparticle diffusion model, and Elovich model were applied to experimental data. The adsorption of both acids followed pseudosecond-order kinetics. Diffusion is not the only rate-controlling step.
Tartaric acid is one of the most valuable compounds that can be obtained from secondary wine products. The last are accumulating in big quantities at winemaking factories from Moldova. This work describes an investigation of the process of reactive ion-exchange separation of tartaric acid from model systems with macroreticular resin Amberlite XAD2 impregnated with liquid ion-exchanger Amberlite LA-2 in batch equipment. The condition of Amberlite XAD2 impregnation process was investigated. Freudlich and Langmuir equations were verified and values of enthalpy, entropy and Gibbs energy were calculated.
DESALINATION AND WATER TREATMENT, 2017
Study on removal of anionic dye methyl orange (MO) from aqueous solution was investigated using ion exchange resin Amberlite IRA-400 batch adsorption process. Effect of operating adsorption factors that influence on the adsorption process such as contact time (1-300 min), initial dye concentration (25-500 ppm), solution pH (2.5-11.5), resin dose (5-100 g/L) and temperature (293-353 K) were studied. The extent of MO adsorption was increased with increase in the contact time, agitation speed, temperature, initial dye concentration and adsorbent dose but decreased with increase/decrease of the solution pH (maximum at pH-6.5). Equilibrium data were analyzed by both Langmuir isotherm and Freundlich adsorption isotherm. The maximum monolayer adsorption capacity of Amberlite IRA-400 was resulted as 74.4 mg/g at 303 K. The value of separation factor (R L) from Langmuir equation and Freundlich constant (n) indicated on favorability of adsorption. Thermodynamic parameters such as ΔG°, ΔH° and ΔS° were calculated and the positive value of ΔH° (4.13, 3.63 and 7.09 kJ mol-1) for corresponding initial MO dye concentrations: 50, 100 and 200 ppm, respectively, in the solution indicated that the adsorption was of endothermic in nature. Kinetics result revealed that the adsorption of MO is of pseudo second-order and chemisorptions type.
Journal of Hazardous Materials, 2006
The adsorption of Acid Red 57 (AR57) onto calcined-alunite was examined in aqueous solution in a batch system with respect to contact time, pH and temperature. The first-order, pseudo-second-order kinetic and the intraparticle diffusion models were used to describe the kinetic data and the rate constants were evaluated. The experimental data fitted very well the pseudo-second-order kinetic model and also followed the intraparticle diffusion model up to 90 min. The Langmuir and Freundlich adsorption models were applied to describe the equilibrium isotherms and the isotherm constants were also determined. The equilibrium data are successfully fitted to the Langmuir adsorption isotherm. The Langmuir isotherm constant, K L , was used to evaluate the changes of free energy, enthalpy and entropy of adsorption for the adsorption of AR57 onto calcined-alunite. The results indicate that calcined-alunite could be employed as low-cost material for the removal of acid dyes from textile effluents.
Cation exchange effective equilibrium distribution coefficients(K' d ) of 18 metal ions with resin Amberlite IR-120 have been determined in varying adipic acid [H 2 AA] concentrations, viz., 2.0×10 -2 _ 7.6×10 -2 M [H 2 AA]. Separation factors of metal ion species were calculated and some possible binary separations were worked out on the basis of their K' d values. An entirely different approach has been proposed for the association of adipate anion involving its partial exchange with the resin site along the complexation of the metal species.
Adsorption of Picric Acid from Aqueous Solution
2014
The presence of nitrophenols in wastewater is of great environmental concern. Therefore, it is important to separate picric acid from wastewater streams. In this study, adsorption of picric acid was studied from aqueous solutions by using a weakly basic adsorbent (Amberlite IRA-67) at three different temperatures (298 K, 308 K, and 318 K). Adsorption of picric acid was investigated in terms of equilibrium, kinetics, and thermodynamic conditions. In the equilibrium studies, 1.00 g of Amberlite IRA-67 was determined as the optimal amount. The most used isotherms, Freundlich and Langmuir, were applied to the experimental data. The Langmuir isotherm gave good results with R squared values over 0.99 at different temperatures. In the kinetic studies, pseudofirst-and pseudosecond-order models and the Elovich equation were applied to the kinetic experiments. The pseudosecond-order model was fitted to this adsorption system with an R squared value of 0.996. In the thermodynamic studies, ∆H ads 0 ) -21.204 kJ · mol -1 , ∆S ads 0 ) -200.043 J · mol -1 · K -1 , and ∆G ads 0 for different temperatures were calculated.
Measurement of heats of adsorption of amino acids on amberlite XAD-2 by an HPLC technique
The chemical engineering journal, 1988
The heats of adsorption from aqueous solutions of cephalosporin-C, D,L-trytophan, D,L-phenylalanine and D,L-tyrosine on XAD-2 resin have been investigated using high pressure liquid chromatography (HPLC). The amino acids were adsorbed from phosphatebuffered aqueous solutions. The pH range studied was 3.3-7.5, the temperature range was 291.15-313.15 K and the ionic strength was maintained at 0.1 M. Over the range of variables investigated the adsorption isotherms are linear and can be characterized by temperature and pH dependent apparent adsorption equilibrium constants, characteristic of the adsorbent-adsorbate system. By studying the dependence on temperature of this adsorption constant, heats of adsorption at small surface coverages have been estimated. In terms of the heat liberated on adsorption, the amino acids can be ranked thus: cephalosporin-C > D, L-tryp top han > D,L-tyrosine > D,L-phenylalanine.