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. 2018 Nov 9;3(11):15140–15148. doi: 10.1021/acsomega.8b02498

Alginate-Based Hydrogel Beads as a Biocompatible and Efficient Adsorbent for Dye Removal from Aqueous Solutions

Safoura Asadi 1, Setareh Eris 1, Saeid Azizian 1,*
PMCID: PMC6289535  PMID: 30555996

Abstract

graphic file with name ao-2018-024982_0011.jpg

In this study, sodium alginate was employed as a starting material for preparing two kinds of biocompatible adsorbents, including calcium alginate hydrogel beads and magnetic hydrogel beads. Fourier transform infrared spectroscopy, X-ray diffraction pattern, and scanning electron microscopy/energy-dispersive X-ray techniques were used to characterize the prepared adsorbents. The performance of the prepared adsorbents for the removal of methyl violet from aqueous solution was studied in detail. Both kinetics and equilibrium aspects of methyl violet adsorption were investigated, and the obtained equilibrium and kinetics data were described with various adsorption models. The effects of initial dye concentration, adsorbent dosage, and temperature on adsorption performance were investigated. Thermodynamic parameters of adsorption were obtained as well.

1. Introduction

In the last century, the massive growth of population on one hand and the rapid industrialization on the other resulted in release of different pollutants in the environment, including dyes. Dyes are synthetic compounds which are widely used in cosmetics industry, paper, plastic, and so on.1,2 Therefore, the wastewater of such industries contains high concentration of dyes. Discharging of this wastewater into the water sources reduces water quality and affects aquatic living organism, damages human health, and aesthetic nature of the water. Therefore, the removal of synthetic dyes from water is environmentally important.

Removal of dye compounds from aqueous solutions has been widely studied, and several physical and chemical techniques have been proposed for purification of water from these compounds including photocatalysis, oxidation, filtration, coagulation–flocculation, ozonation, and adsorption.3−5 Among all of these techniques, adsorption is considered as one of the most useful methods for the removal of dyes because its operation is facile and efficient and the adsorbent can be recovered and reused.6,7 Dissolved dye molecules can bind to the surface of the adsorbent by physical or chemical bonds.8

Methyl violet (MV) is one of the poison dye compounds, which is used in textile and paper dyeing and so on (the chemical structure of MV is shown in Figure S1). Various adsorbents have been applied for the removal of MV from wastewater such as membrane9 waste materials,10 chitosan,11 agricultural waste,12 sepiolite,13 fly ash,14 perlite,15 and powdered activated carbon.16 However, most of these adsorbents are neither cost effective nor biodegradable.17,18

To improve these weaknesses, a new class of adsorbents, biopolymer-based adsorbents, are introduced in water purification applications. In recent years, many studies have been carried out on using biopolymers as the adsorbent because of their simple synthesis, environmental compatibility, biodegradability, and low cost.

Also, these materials can be modified for specific pollutant removal.19,20 Biopolymers and, in particular, sodium alginate are biodegradable compounds that have many hydroxyl and carboxylate functional group in their internal structure.21−23 Therefore, because of the presence of numerous anionic groups, they can be considered as a new candidate for the removal of cationic pollutions from waste water (similar to cationic dyes). Dye adsorption on biopolymer-based adsorbents occurs through electrostatic attractions between adsorbents and contaminants.24

Sodium alginate, a natural water-soluble salt of alginic acid, is a linear polysaccharides that is extracted from brown algae. It has high bioavailability, and its extraction process is easy. This natural polymer consists of α-L-guluronic (G) and β-d-mannuronic (M) acid residues (Figure 1), and these produce a variety of sequential 1,4-linkage with other materials. The ability to form hydrogels is one of the main properties of alginate; this property of sodium alginate is mainly because of the substitution of sodium ions from the guluronic acid residues by different divalent cations (Ca2+, Sr2+, Ba2+, etc.). Therefore, a 3D network is formed as a result of binding divalent cation to the α-l-guluronic block (and between two different chains) (Figure 1).25,26 Hydrogels of calcium alginate can be used as a potential sorbent because of its low cost, hydrophilicity, nontoxicity, and biocompatibility.

Figure 1.

Figure 1

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Chemical structure of sodium alginate.

Introducing nanoparticles into the biopolymer matrices can significantly improve thermal, chemical, mechanical, and surface properties of biopolymers.27,28 Recently, interests in biopolymer-based metal oxide nanoparticles have been increased because of biocompatibility, their ability for the removal of dyes and other containments from water, and so on.

Magnetic nanoparticle (MNP) adsorbents based on iron oxide have received great attention. This attention is because of the fundamental properties of MNPs such as particle size and large surface area.29 One of the most important advantages of using magnetic-based adsorbent is the ease of separation from treated water through an external magnetic field. This property leads to a possibility of reusing the adsorbent (and also recovering the adsorbed substrate).30,31 Preparation of nanocomposites of calcium alginate polysaccharides with iron oxide provides materials which have desired properties of good adsorbents.26,32

In this study, calcium alginate and magnetic composite beads were prepared and used as adsorbents for the removal of MV from aqueous solution. Adsorption of MV was studied from equilibrium and kinetics viewpoints. Furthermore, the effect of different parameters including temperature, adsorbent mass, and initial concentration of MV was studied too.

2. Results and Discussion

2.1. Samples Characterization

Scanning electron microscopy (SEM) images of the synthesized iron oxide are shown in Figure 2.

Figure 2.

Figure 2

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SEM images of the synthesized iron oxide with increasing magnification from (a–d).

Figure 2a,b shows that the as-synthesized iron oxide structures are microspheres with a diameter of ≈1.5 μm. Figure 2c shows that each microsphere is composed of several nanosheets. Figure 2d shows that the nanosheets are formed by aggregation of nanoparticles (15–20 nm). Figure 3 represents the SEM images of dried magnetic beads. This figure clearly shows that the iron oxide microparticles were coated with a thin layer of calcium alginate.

Figure 3.

Figure 3

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SEM images of dried magnetic beads with (a) low and (b) high magnifications.

From the results of the EDX (energy-dispersive X-ray) spectra of iron oxide (Figure S2a), it can be found that the synthesized iron oxide is only composed of iron (Fe) and oxygen (O). Furthermore, the EDX spectrum of the dried magnetic beads is shown in Figure S2b, which confirms the presence of oxygen (O) and iron (Fe) elements. Also, the appearance of C and Ca peaks confirms the presence of calcium alginate layer.

Figure 4 shows the X-ray diffraction (XRD) pattern of the dried magnetic composite hydrogel beads. The XRD pattern shows six characteristic peaks of Fe3O4 at 2θ = 30.1, 35.8, 43.1, 53.9, 57.2, and 63.1° that can be indexed to (220), (311), (400), (422), (511), and (440) planes of Fe3O4, and a characteristic peak at 2θ = 33.0° that can be assigned to (104) plane of α-Fe2O3. Therefore, from the XRD pattern, it can be concluded that the synthesized iron oxide is composed of Fe3O4 and α-Fe2O3.33,34

Figure 4.

Figure 4

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XRD pattern of dried magnetic beads.

The FTIR (Fourier transform infrared) spectrums of calcium alginate beads, magnetic calcium alginate beads, MV-loaded calcium alginate beads, and MV-loaded magnetic calcium alginate beads are shown in Figure 5.

Figure 5.

Figure 5

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FTIR spectra of: (a) calcium alginate hydrogel beads, (b) MV-loaded calcium alginate hydrogel beads, (c) magnetic hydrogel beads, and (d) MV-loaded magnetic hydrogel beads.

In the FTIR spectrum of calcium alginate beads (Figure 5a), the broad peak at 3452 cm–1 is corresponded to −OH stretching vibration of calcium alginate, and the peaks at 2926 and 2736 cm–1 belong to symmetric and asymmetric C–H stretching, respectively. The bands which appeared at 1645 and 1423 cm–1 are assigned to asymmetric and symmetric stretching vibrations of carboxyl groups of calcium alginate, respectively. The band at 1091 cm–1 attributes to C–O–C group. Figure 5c, which is FTIR spectra of magnetic beads, shows that the band at 3444 cm–1 is because of the −OH stretching and bending vibration and bands at 1602 and 1409 cm–1 are because of asymmetrical and symmetrical stretching vibration of carboxyl group for magnetic beads. Also, the weak band of bending vibration of C–O–C group is appeared in 1033.07 cm–1.

The absorption band at the low-frequency zone of 500–700 cm–1 (569 cm–1) corresponds to the stretching vibration of Fe–O bands in iron oxide and the FTIR spectrum of calcium alginate beads and magnetic beads after being loaded with MV. Figure 5b,c shows a shift of the peaks and reduction of peak intensity (especially significant reduction in −OH and C=O bands). These changes imply that MV is chemically adsorbed on the surface of the adsorbents.

2.2. Adsorption Kinetics

The study of adsorption kinetics provides indispensable information about the mechanism and rate of adsorption. Also, kinetic studies are of prime importance to design and operate adsorption equipment. Figure 6 shows the changes in adsorbed amounts with time for both types of adsorbents. This figure clearly shows that the adsorption of MV by both types of adsorbents is initially fast, and most of the adsorption occurs within 10 min. Also, it can be seen that by increasing the initial MV concentration, the adsorption rate and capacity increased. Furthermore, from Figure 6, it can be concluded that the rate of MV adsorption on to calcium alginate hydrogel beads is faster than that of magnetic hydrogel beads. The adsorption kinetics data were evaluated using several adsorption kinetics models including pseudo-first order (PFO),35 pseudo-second order (PSO),35,36 mixed 1,2-order (MOE),37 fractal-like pseudo-first order (FL-PFO),38,39 fractal-like pseudo-second order (FL-PSO),38,39 fractal-like mixed 1,2-order (FL-MOE),38,39 and Elovich.40 The obtained results of data fitting are listed in Tables 1 and S1. The correlation coefficients show that the adsorption kinetic data for MV onto calcium alginate hydrogel beads were better correlated by FL-PSO model. Also, for the adsorption of MV by magnetic hydrogel beads, best kinetic model is FL-MOE.

Figure 6.

Figure 6

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Experimental kinetics data for the adsorption of MV by (a) calcium alginate hydrogel beads and (b) magnetic hydrogel beads at different initial concentrations of MV. The solid lines show the predicted values by the best fitted model.

Table 1. Obtained Contacts of Different Kinetic Models for Adsorption of MV on to Calcium Alginate Hydrogel Beads.

kinetic model equation qe (mg/g) k k1 (1/min) k2 [g/(mg min)] f2 a b α r2
C0 = 2 (mg/L)
PFO35 qt = qe(1 – exp(−k1t)) 6.44   0.358           0.9226
PSO35,36 qt = k2qe2t/(1 + k2qet) 6.85     0.081         0.9775
MOE37 qt = qe((1 – exp(−k1t))/(1 – f2 exp(−k1t))) 6.67   0.052   0.9       0.9733
Elovich40 qt = (1/b) ln(1 + abt)           1.390 143.34   0.9831
FL-PSO38,39 qt = kqe2tα/(1 + kqetα) 7.07 0.096           0.550 0.9898
FL-PFO38,39 qt = qe(1 – e–ktα) 7.08 0.633           0.408 0.9909
FL-MOE38,39
graphic file with name ao-2018-024982_m011.jpg
 7.08 0.632     0.001     0.385 0.9913
C0 = 4 (mg/L)
PFO35 qt = qe(1 – exp(−k1t)) 11.17   0.297           0.9850
PSO35,36 qt = k2qe2t/(1 + k2qet) 11.73     0.044         0.9962
MOE37 qt = qe((1 – exp(−k1t))/(1 – f2 exp(−k1t))) 11.44   0.05   0.9       0.9953
Elovich40 qt = (1/b) ln(1 + abt)           0.989 1170.73   0.9725
FL-PSO38,39 qt = kqe2tα/(1 + kqetα) 11.61 0.047           1 0.9962
FL-PFO38,39 qt = qe(1 – e–ktα) 11.45 0.538           0.557 0.9940
FL-MOE38,39
graphic file with name ao-2018-024982_m012.jpg
 11.24 0.047     0.9     1 0.9953
C0= 6 (mg/L)  
PFO35 qt = qe(1 – exp(−k1t)) 19.02   0.153           0.9555
PSO35,36 qt = k2qe2t/(1 + k2qet) 20.70     0.011         0.9964
MOE37 qt = qe((1 – exp(−k1t))/(1 – f2 exp(−k1t))) 20.09   0.022   0.9       0.9936
Elovich40 qt = (1/b) ln(1 + abt)           0.366 41.30   0.9600
FL-PSO38,39 qt = kqe2tα/(1 + kqetα) 21.31 0.013           0.867 0.9983
FL-PFO38,39 qt = qe(1 – e–ktα) 20.42 0.317           0.562 0.9947
FL-MOE38,39
graphic file with name ao-2018-024982_m013.jpg
 20.75 0.029     0.5     0.828 0.9978
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Therefore, it can be said that the kinetics of MV adsorption on both of the adsorption was found to follow fractal-like kinetic models. The fractal-like model implies that the adsorption rate coefficient is time-dependent for these systems. This means that the adsorption pathway (or site) changes with time.38,39 The solid lines in Figure 6 show the predicated values by FL-PSO (for calcium alginate hydrogel beads) and FL-MOE (for magnetic hydrogel beads).

2.3. Effect of Adsorbent Dosage

The effect of adsorbent dosage on adsorption of MV (with the concentration of 6 ppm) was studied using different amounts of adsorbents (0.0013–0.0026 g dry mass of calcium alginate hydrogel beads and 0.0019–0.0039 g dry mass of magnetic hydrogel beads).

Figure S3 shows the plots of adspecies amount versus time for different adsorbent dosages. As can be seen in these figures, increasing the adsorbent dosage leads to decreasing the adsorbed amount per unit mass of adsorbent. However, as the adsorbent dosage increases, the required time for reaching equilibrium decreases because of increasing the number of active sites on the surface of the adsorbent.

More recently, a simple graphical method was proposed to elucidate the effect of adsorbent dosages on the rate of adsorption process.41 The base of this method is the plot of normalized adsorbed amount, Inline graphic, versus the normalized time scale, t[m]n (where m is the mass of the adsorbent and n is the order in the adsorbent mass). In fact, the normalization of time was performed by multiplying each point time by the used adsorbed mass (in each experiment), which was raised by an arbitrary power. The value of this power should be changed until the curves overlay. Here, we used this method for finding the order of the adsorbent mass in the rate equation. For this purpose, the plot of Inline graphic versus t[m]n was drawn for the adsorption of MV on calcium alginate hydrogel beads (or magnetic hydrogel beads). By choosing the correct value for n, all curves (for different masses of adsorbent) coincided, as shown in Figure 7.

Figure 7.

Figure 7

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Coincidence of curves for n-values of (a) n = 0.8 for calcium alginate hydrogel beads and (b) n = 0.5 for magnetic hydrogel beads.

Therefore, it can be found that the order of mass of calcium alginate beads in the rate equation is around 0.8 and of magnetic hydrogel beads is about 0.5 (Figure 7a,b).

Also, by finding the order of the adsorption with respect to the adsorbent dosage, it is possible to determine the adsorbent rate constant, which is independent of the adsorbent mass. For this purpose, the linear form of extended pseudo-second-order rate model was used41

2.3.

where the values of mass independent rate constant, k2, and qe can be obtained from the intercept and the slope of the plot of Inline graphic versus t[m]n, respectively. Figure 8 shows the linear plot of Inline graphic versus t[m]n for the adsorption of MV onto different dosages of adsorbents. Also, the adsorption kinetic data of MV onto calcium alginate hydrogel beads and magnetic hydrogel beads were correlated with the linear form of classical pseudo-second-order rate model Inline graphic(35,36) for comparison.

Figure 8.

Figure 8

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Linear plot of extended pseudo-second-order for the adsorption of MV onto (a) different dosages of calcium alginate hydrogel beads and (b) different dosages of magnetic hydrogel beads.

The obtained values of k2 and qe for these two models are summarized in Table S2.

The obtained results show that in the case of extended pseudo-second-order rate model, the k2 does not change with the adsorbent dosage, whereas for classical pseudo-second-order rate model, it is strongly dependent on the adsorbent dosage. To provide a better visual understanding, the obtained values of k2 at different adsorbent dosages by pseudo-second-order and extended pseudo-second-order models are shown in Figure 9. These figures clearly show that the extended pseudo-second-order model provides the same rate constant for each mass of the adsorbent.

Figure 9.

Figure 9

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Adsorption rate constants derived from (a,c) extended pseudo-second order and (b,d) pseudo-second order for adsorption of MV on (a,b) calcium alginate hydrogel beads and (c,d) magnetic hydrogel beads.

2.4. Adsorption Equilibrium Studies

The knowledge of adsorption isotherms furnishes basic information on adsorbate–adsorbent interactions. The adsorption isotherms are mathematical relationships which describe the distribution of the adsorbate species between the liquid phase and the adsorbed phase at a specific temperature and also at equilibrium conditions.

The equilibrium adsorption data of MV on calcium alginate hydrogel beads and magnetic hydrogel beads are shown in Figure 10a,b. The equilibrium data were modeled with recently presented models including modified Langmuir (ML)42 and modified Langmuir–Freundlich (ML–F)42 isotherms and also the classical ones including Freundlich (F),43 Redlich–Peterson (R–P),43 and Toth43 isotherms.

Figure 10.

Figure 10

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Adsorption isotherm of MV by (a) calcium alginate hydrogel beads and (b) magnetic hydrogel beads. The experimental data are shown with symbols, whereas the solid lines are the predicted values the by ML–F isotherm.

The obtained isotherm parameters along with their correlation coefficients are tabulated in Tables 2 and S3. According to the results, the best correlation coefficients were obtained for ML–F model, indicating that the surface of both adsorbents is heterogeneous. The solid lines in Figure 10a,b show results of fitting by ML–F isotherm. The maximum adsorption capacities of MV, calculated by the ML–F model, are 889 and 713 (mg/g) for calcium alginate hydrogel beads and magnetic hydrogel beads, respectively.

Table 2. Obtained Constants of Different Isotherms for Adsorption of MV on to Calcium Alginate Hydrogel Beads.

isotherm model equation qm (mg/g) KML (dimensionless) KF (L mg(1–(1/n))/g) KR (L/g) KMLF (dimensionless) 1/n αR (L/mg)β bT β r2
ML42
graphic file with name ao-2018-024982_m014.jpg
 1151 389               0.9704
F43 qe = KFCe1/n     77     0.48       0.9036
R–P43
graphic file with name ao-2018-024982_m015.jpg
       16     0.0007   1.56 0.9915
ML–F42
graphic file with name ao-2018-024982_m016.jpg
 889       692         0.9971
Toth43
graphic file with name ao-2018-024982_m017.jpg
 850         3.45   0.0171   0.9950
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2.5. Thermodynamics of Adsorption

Isothermal studies of MV adsorption onto calcium alginate hydrogel were carried out at different temperatures ranging from 25 to 45 °C, and the results are shown in Figure S4. This figure shows that the adsorption capacity of MV onto calcium alginate hydrogel beads decreases slightly with the increasing temperature. The equilibrium data of MV adsorption on calcium alginate hydrogel beads were analyzed with ML–F isotherm. The obtained results of this fitting are listed in Table 3.

Table 3. Obtained Constants of the ML–F Isotherm for the Adsorption of MV by Calcium Alginate Hydrogel Beads at Different Temperatures.

temperature (K) Cs (g/L)a KMLF qm (mg/g) r2
298 20.1 692 889 0.9971
313 35.1 892 886 0.9972
328 64.3 1447 855 0.9975
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a

The values of saturation concentration of MV at different temperatures were obtained experimentally.

Also, the thermodynamic parameters [the standard Gibbs free-energy changes (ΔG°), the standard enthalpy change (ΔH°), and the standard entropy change (ΔS°)] for the adsorption of MV adsorption on calcium alginate hydrogel were calculated. The following equation can be applied for the calculation of standard Gibbs free-energy changes (ΔG°)42

2.5.

where KMLF is ML–F constant (which is a dimensionless parameter). For calculation of the standard enthalpy change (ΔH°) and the standard entropy change (ΔS°), the van’t Hoff equation was used

2.5.

On the basis of this equation, the values of (ΔS°) and (ΔH°) can be derived from the intercept and the slope of ln KMLF versus 1/T plot (Figure S5). The obtained values of ΔG°, ΔH°, and ΔS° are summarized in Table S4. The obtained results show that the adsorption of MV on calcium alginate hydrogel beads is endothermic in nature and entropy driven.

3. Conclusions

In summary, the removal of MV by calcium alginate hydrogel beads and magnetic hydrogel beads as adsorbent were studied using batch experiments. It was found that the initial dye concentration, adsorbent dosage, and temperature can influence on the removal efficiency of MV by calcium alginate hydrogel beads and magnetic hydrogel beads. Studies on the adsorption equilibrium showed that the ML–F model gives a closer fit to the experimental data than the other used isotherms. This observation is an indicator of heterogeneity of the adsorbent surface. The maximum adsorption capacities of calcium alginate hydrogel beads and magnetic hydrogel beads for the removal of MV were obtained as 889 and 713 mg/g, respectively, which are very high. Also, the findings of kinetic studies showed that the adsorption of MV on calcium alginate hydrogel beads and magnetic hydrogel beads complied with extended pseudo-second-order model. By studying various adsorbent dosages, it was found that the mass of the adsorbent affects the rate of adsorption. Also, the thermodynamic studies revealed that the adsorption of MV on calcium alginate beads is spontaneous, endothermic, and entropy driven. Finally, the advantages of the prepared adsorbents in this study which make them potential adsorbents for practical usage are biocompatibility, ease of separation from the solution, and high adsorption capacity.

4. Experimental Section

4.1. Materials

FeCl3·6H2O, urea, ethylene glycol, CaCl2, and MV were purchased from Merck Co.; tetrabutylammonium bromide (TBAB) was a product of Daejung Co; and sodium alginate were purchased from Titra Chem Co. All of the chemicals were used without further purification. In all experiments, deionized water was used.

4.2. Preparation of Calcium Alginate Hydrogel Beads

To prepare calcium alginate hydrogel beads, 1 g of sodium alginate was dissolved in 50 mL of deionized water under continuous magnetic stirring to form a transparent and viscous solution. The obtained viscous solution was added drop by drop using a syringe into a CaCl2 aqueous solution (0.1 mol L–1). Hydrogel beads were formed instantly and were maintained in CaCl2 solution for 16 h. Then, the calcium hydrogel beads were filtered and washed three times with deionized water to remove any unreacted calcium chloride and kept in deionized water bath.44

4.3. Synthesis of Iron Oxide Nanostructures

The preparation of iron oxide was carried out according to a previously reported procedure.33 The precursor was prepared by adding FeCl3·6H2O (1.2 g), TBAB (7.2 g), and urea (2.7 g) to 180 mL of ethylene glycol in a 250 mL round-bottom flask. The obtained red solution was stirred and refluxed at 195 °C for 45 min and then cooled to room temperature. The resulting green precipitate was separated by centrifugation and washed four times by ethanol and then calcined at 500 °C in a furnace under the N2 atmosphere for 3 h and then cooled to 90 °C in the N2 atmosphere. The obtained powder was cooled to room temperature under ambient condition.

4.4. Preparation of Magnetic Hydrogel Beads

For the preparation of magnetic hydrogel beads, 1 g of sodium alginate was dissolved in 50 mL of water; then, 0.5 g of iron oxide nanoparticles was dispersed in it by sonication, and the mixture was vigorously stirred for 2 h in a shaker. The viscous suspension was dripped into a CaCl2 bath (0.1 mol L–1), and the magnetic hydrogel beads were obtained. To complete the gelation reaction, the magnetic hydrogel beads were allowed to be in contact with the CaCl2 solution for 16 h. The hydrogel magnetic beads were separated from the solution using a magnet, washed three times by deionized water, and then stored in a deionized water bath for further use.44

4.5. Characterization

The morphology, composition, and particle size of the prepared iron oxide and dried magnetic composite hydrogel beads were characterized using SEM (TESCAN-VEGA//XMU and TESCAN Vega3), and the elemental identification of the samples was performed by EDX spectroscopy. Also, the crystalline structure of the dried magnetic beads was determined using an X-ray diffraction (XRD) (Bruker AXS-D8 ADVANCE). The presence of various functional groups in samples was identified by FTIR (PerkinElmer, Waltham, MA, USA) using a KBr pellet, in the range of 4000–400 cm–1.

4.6. Adsorption Experiments

The adsorption of MV onto calcium alginate hydrogel beads and magnetic hydrogel beads was studied in a batch-mode system. The effect of different parameters including the initial dye concentration, amount of the adsorbent, and temperature on adsorption performance was assessed. The equilibrium experiments were carried out as follows: constant volume of MV solution (5 mL) with different initial concentrations (10–500 mg/L) was mixed with a constant amount of wet adsorbent (0.0972 g). The samples were put in a thermostat shaker (200 rpm and 25 ± 2 °C) and shaken for 24 h to equilibrate. Then, the adsorbent was separated from a solution by a filter or a magnet. The filtrate equilibrium concentration (Ce) was measured by using a UV/vis spectrophotometer (PG Instrument LTD model T80) at 585 nm. The adsorbed amount of MV dye per unit mass of the adsorbent was obtained by

4.6. 1

where C0 and Ce are the initial and equilibrium concentrations (mg L–1) of the dye solution, respectively; m is the dried adsorbent mass (g); and V is the solution volume (L).

The kinetics studies were carried out at different initial concentrations of MV [2, 4, and 8 (mg/L)]. The experimental setup was the same as that for equilibrium experiments. Here, the residual concentration of MV was measured at different time intervals, Ct.

Also, the following equation was used for the determination of the amount of MV adsorbed [qt (mg/g)] at each time interval

4.6. 2

Acknowledgments

The authors are grateful for the financial support from the Bu-Ali Sina University [grant number (32-12-67)].

Supporting Information Available

The Supporting Information is available free of charge on the ACS Publications website at DOI: 10.1021/acsomega.8b02498.

  • Chemical structure of MV; EDX spectrum of adsorbents; plot of variation of q with time for adsorption of MV onto different dosages of adsorbents; obtained kinetic parameters for the adsorption of MV onto magnetic hydrogel beads; kinetic parameters obtained from PSO and EPSO models for MV adsorption onto both of the adsorbents; table of derived constant parameters of isotherm models for the adsorption of MV onto magnetic hydrogel beads; plot of temperature effect on MV adsorption by calcium alginate hydrogel beads; KMLF versus 1/T plot for MV adsorption by calcium alginate beads; and thermodynamic parameters of MV adsorption by calcium alginate hydrogel beads (PDF)

The authors declare no competing financial interest.

Supplementary Material

ao8b02498_si_001.pdf (675.5KB, pdf)

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