Kinetics and thermodynamic studies for removal of acid blue 129 from aqueous solution by almond shell
© Fat’hi et al.; licensee BioMed Central Ltd. 2014
Received: 22 August 2012
Accepted: 5 March 2014
Published: 12 March 2014
Efficiency and performance of Almond shell (AS) adsorbent for the removal and recovery of Acid Blue 129 (AB129) from wastewater is presented in this report. The influence of variables including pH, initial dye concentration, adsorbent dosage, particle size, contact time and temperature on the dye removal have been investigated in batch method by one at a time optimization method. The experimental equilibrium data were tested by four widely used isotherm models namely, Langmuir, Freundlich, Tempkin and Dubinin-Radushkevich (D–R). It was found that adsorption of AB129 on AS well with the Langmuir isotherm model, implying monolayer coverage of dye molecules onto the surface of the adsorbent. More than 98% removal efficiency was obtained within 14 min at adsorbent dose of 0.4 g for initial dye concentration of 40 mg/L at pH 2. Kinetics of the adsorption process was tested by pseudo-first-order and pseudo-second-order kinetics, and intraparticle diffusion mechanism. Pseudo-second-order kinetic model provided a better correlation for the experimental data studied in comparison to the pseudo-first-order model. Calculation of various thermodynamic parameters such as, Gibb’s free energy, entropy and enthalpy of the on-going adsorption process indicate feasibility and endothermic nature of AB129 adsorption on all adsorbents. This work can be used in design of adsorption columns for dyes removal.
Properties of the acid blue 129
Acid blue 129
Sodiume-1-amino-4-(2, 4, 6-trimethylanilino) anthraquinone-2-sulfonate.
Maximum wavelength (nm)
Traditionally, well known protocols such as coagulation, nano filtration and ozonalysis, membrane filtration, oxidation and adsorption process are applied to remove color and other contaminations from aqueous media [3–7]. Adsorption is most popular technique that benefit from advantages such as high efficiency and ability to use generable non-toxic and cheap adsorbents [8–22]. Although, activated carbon appears to be the widely used techniques for dye removal, but in view of the high cost and regeneration problems scope of many adsorption studies has been focused to derive cheaper adsorbents from the waste materials . During the past decades, several researches are to utilize low cost and easily available natural materials as potential adsorbents for removal of dyes [24–29]. The present work aims to study a convenient and economic method for AB129 removal from water by adsorption on AS as low cost and abundantly available adsorbent. The effects of initial AB129 concentration, contact time, pH, particle size and amount of adsorbent on AB129 removal have been evaluated.
Materials and methods
Chemicals and instruments
AS were supplied from the Arctic Sea Region of Iran. They were firstly dried, crushed in a ball mill and sieved to obtain a particle size between 0–177, 210–297 and 350–500 μm. All chemical used were of analytical grade and doubled distilled water was used throughout. A stock solution of 200 mg/L of AB129 was prepared by dissolving 0.100 g of solid dye in water and diluting to 500 mL in a volumetric flask. The AB129 concentration evaluation was carried out using Shimadzu UV–vis spectrophotometer model 160A (Shimadzu, Japan) at a wavelength of 600 nm. The pH measurements were carried out using pH/Ion meter model 691 (Metrohm, Switzerland, Swiss).
To study the effect of important parameters like the pH, adsorbent dosage, contact time, initial dye concentration and temperature on the adsorptive removal of AB129 batch experiments were conducted. For each experimental run, 25 mL of AB129 solution of known concentration, pH and amount of the adsorbent were taken in a 50 ml Erlenmeyer flask with middle magnet. This mixture was agitated on stirrer at a constant speed in a temperature controlled. Samples were withdrawn at different time intervals (0–15 min for AS) and kinetics, thermodynamic, isotherm and other parameters of adsorption was determined by analyzing of remaining dye concentration from aqueous solution.
Experiments were carried out at pH = 2.0 that the initial pH of the solution was adjusted by addition of aqueous solutions of HCl or NaOH.
For adsorption isotherms, dye solutions of different concentrations (10–90 mg/L) and at temperatures (25°C) were agitated with known amounts of adsorbents until the equilibrium was achieved.
Results and discussion
At acidic pH the H+ ion concentration in the system increased and the surface of the AS acquires positive charge by absorbing H+ ions. As the pH of the system increases, the number of negatively charged sites increases and the number of positively charged sites decreases. Negatively charged surface sites on the AS do not favor the adsorption of AB129 anions due to the electrostatic repulsion. Also lower adsorption of AB129 at alkaline pH is due to the presence of excess OH¯ ions, which destabilize anionic AB129 and compete with the AB129 anions for the adsorption sites. The most effective pH was 2.0 and it was used in further studies.
For adsorbent dosage higher than 0.4 g the AB129 removal remained almost constant. Increases in the percentage of AB129 removal with adsorbent dosage could be attributed to increases in the adsorbent surface areas, augmenting its number of adsorption sites available for adsorption [33, 34]. In order to continue this work, the adsorbent dosage was fixed at 0.4 g, since this adsorbent dosage correspond to the minimum amount of adsorbent which lead to a constant and maximum removal of AB129.
At 40 mg/L of AB129, the removal rate in the first varies from 58.5% to 94.24% of the maximum removal onto AS. For instance, the adsorbents exhibited three stages, which can be attributed to each linear portion of the figure. The first linear portion was attributed to the diffusion process of AB129 to the adsorbent surfaces [35, 36], hence, was the fastest adsorption stage.
This result is corroborated by the factionary-order kinetic model. The second linear portion was attributed to intra-particle diffusion, which was delayed process. The third stage may be regarded as the diffusion through smaller pores, which is followed by the establishment of equilibrium. The surface of AS may contain a large number of active sites and the solute adsorption can be related to the active sites on equilibrium time. Also up to 90% of the total amount of AB129 adsorption was found to occur in the first rapid phase (10 min) and thereafter the adsorption rate was found to decrease. The higher adsorption rate at the initial period (first 10 min) may be due to too number of vacant sites available at the initial stage. As a result there exist too concentration gradients between adsorbate in solution and onto adsorbent surface. This increased in concentration gradients tends to increase in AB129 adsorption at the initial stages.
Adsorption kinetic studies
The mechanism of adsorption was investigated by pseudo first order and pseudo second order models.
Kinetic parameters for the adsorption of 40 mg/L AB129 onto AS
Log (qe ‐ qt) = log(qe) ‐ k1/2.303t
qe (calc) (mg/g)
(t/qt) = 1/(k2qe2) + 1/qe(t)
k2 (g/(mg min))
qe (calc) (mg/g)
H (mg/(g min))
qt = Kdift1/2 + C
Kdiff (mg/(g min1/2))
qt = 1/β ln(αβ) + 1/β ln(t)
α (mg/(g min))
qe (exp) (mg/g)
Figure 6 was used to determine pseudo first order rate constant (k1) and theoretical amount of dye adsorbed per unit mass of adsorbent qe(the). Distance of qe(the) from qe(exp) value indicate that this model was not fit well with the experimental data (Table 2) .
Adsorption equilibrium study
Adsorption isotherms are prerequisites to understand the nature of the interaction between adsorbate and the adsorbent used for the removal of organic pollutants [38, 39]. The equation parameters of various adsorption isotherm equations such as Langmuir, Freundlich, Temkin, Dubinin-Radushkevich (D-R) and Harkins-Jura isotherms provide some insight into the adsorption mechanism, the surface properties and affinity of the adsorbent for adsorbate [40, 41].
The Langmuir isotherm is based on the assumption that the adsorption process takes place at specific homogeneous sites within the adsorbent surface and that once a dye molecule occupies a site, no further adsorption can take place at that site, which concluded that the adsorption process is monolayer in nature.
Maximum adsorption corresponds to a saturated monolayer of adsorbate molecules on the adsorbate surface.
The energy of the adsorption is constant.
There is no transmigration of adsorbate molecules in the plane of adsorbent surface . Based on the linear form of Langmuir isotherm model (according to Table 3), the values of K a (the Langmuir adsorption constant (L/mg)) and Q m (theoretical maximum adsorption capacity (mg/g)) were obtained from the intercept and slope of the plot of Ce/qe vs Ce, respectively (Figure 8). The values of Qm and K a are 11.95 m/g and 0.902 L/mg, respectively shown in Table 3. The high correlation coefficient (0.994) shows the applicability of Langmuir model for interpretation of the experimental data.
Isotherm constant parameters and correlation coefficients calculated for the adsorption of AB129 onto AS
1/qe = 1/(KaQmCe) + 1/Qm
ln qe = ln KF + (1/n)ln Ce
qe = B1 ln KT + B1 ln Ce
ln qe = ln Qs ‐ Bε2
B × 10-5
The data was analyzed by the linearized form of Freundlich isotherm model. In this model, qe is the amount of adsorption, kf is the Freundlich constant related to sorption capacity and 1/n is a constant related to energy or intensity of adsorption. This gives an expression encompassing the surface heterogeneity and the exponential distribution of activated sites and their energies. This isotherm dose not predicts any saturation of the adsorbent surface. The Freundlich exponents kF and 1/n can be determined from the linear plot of log qe vs. log Ce is shown in Table 3. The values of the Freundlich constants KF and 1/n are 0.508 respectively shown in Table 3. The slope 1/n ranging between 0 and 1 is a measure of adsorption intensity or surface heterogeneous, becoming more heterogeneous as its value gets closer to zero .
Heat of adsorption and the adsorbent-adsorbate interaction on adsorption isotherms were studied by Tempkin . The constants obtained for Tempkin isotherm are shown in Table 3. The linear form of Dubinin-Radushkevich isotherm equation was applied to estimate the porosity apparent free energy and the characteristic of adsorption . The constant obtained for D–R isotherms are shown in Table 3. The mean adsorption energy (E) gives information about chemical and physical nature of adsorption.
As seen from Table 3, the Langmuir model yields a somewhat better fit (R2 = 0.994), Tempkin isotherm (R2 = 0.993) than the Freundlich model (R2 = 0.929) and Dubinin-Radushkevich model (R2 = 0.948). Equilibrium data fitted well with the Langmuir and Tempkin model.
Thermodynamic parameters for adsorption of AB129
Apricot Stone (AS)
∆G° ( kj/mol)
C 0 (mg/L)
∆S° (J/(mol k))
The positive values of ∆H◦ further confirm the endothermic nature of the adsorption process and the positive ∆S◦ values suggest the increase in adsorbate concentration in solid–liquid interface indicating thereby the increase in adsorbate concentration onto the solid phase. It also confirms the increased randomness at the solid–liquid interface during adsorption. This is the normal consequence of the physical adsorption phenomenon, which takes place through electrostatic interactions.
Comparison with literature
It was observed that the AS is an efficient adsorbent for the removal of AB129S. Removal of AB129 is pH dependent and the maximum removal was attained at pH = 2. The equilibrium data fitted very well in a Langmuir and Tempkin isotherm equations. The data indicate that the adsorption kinetics follow the pseudo-second-order with spontaneous and endothermic nature of the adsorption process. The positive sign of ∆S° indicates that the adsorption process takes place through electrostatic interaction between adsorbent surface and adsorbate species in solution. The present study concludes that the AS could be employed as low-cost adsorbents for the removal of AB129 from aqueous solution in general.
The authors express their appreciation to the Graduate School and Research Council of the Gachsaran Azad University for financial support of this work.
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