Next Article in Journal
Characterization of the Structure, Mechanical Properties and Erosive Resistance of the Laser Cladded Inconel 625-Based Coatings Reinforced by TiC Particles
Previous Article in Journal
Effect of Fiber Content and Alignment on the Mechanical Properties of 3D Printing Cementitious Composites
 
 
Search for Articles:
Title / Keyword
Author / Affiliation / Email
Journal
Article Type
 
 
Advanced Search
 
Section
Special Issue
Volume
Issue
Number
Page
 
Journals
Materials
Volume 14
Issue 9
10.3390/ma14092224
materials-logo
Submit to this Journal Review for this Journal Propose a Special Issue
► Article Menu

Article Menu

share Share announcement Help format_quote Cite question_answer Discuss in SciProfiles thumb_up
...
Endorse textsms
...
Comment
first_page
settings
Order Article Reprints
Font Type:
Arial Georgia Verdana
Font Size:
Aa Aa Aa
Line Spacing:
Column Width:
Background:
Article

Adsorption of Hexavalent Chromium by Sodium Alginate Fiber Biochar Loaded with Lanthanum

by
Xinzhe Sun
1,
Peng Guo
2,
Yuanyuan Sun
1,* and
Yuqian Cui
1,*
1
College of Environmental Science and Engineering, Qingdao University, Qingdao 266071, China
2
School of Chemical Engineering, China University of Petroleum (East China), Qingdao 266580, China
*
Authors to whom correspondence should be addressed.
Materials 2021, 14(9), 2224; https://doi.org/10.3390/ma14092224
Submission received: 22 December 2020 / Revised: 5 February 2021 / Accepted: 20 April 2021 / Published: 26 April 2021
Browse Figures
Review Reports Versions Notes

Abstract

:
Lanthanun oxide (La2O3) is a lanthanum chemical compound incorporates a sensible anionic complexing ability; however, it lacks stability at a low pH scale. Biochar fibers will give the benefit of their massive space and plethoric uses on the surface to support a metal chemical compound. Herein, wet spinning technology was used to load La3+ onto sodium alginate fiber, and to convert La3+ into La2O3 through carbonization. The La2O3-modified biochar (La-BC) fiber was characterized by SEM, XRD and XPS, etc. An adsorption experiment proved that La-BC showed an excellent adsorption capacity for chromates, and its saturation adsorption capacity was about 104.9 mg/g. The information suggested that the adsorption was in step with both the Langmuir and Freundlich models, following pseudo-second-order surface assimilation mechanics, which showed that the Cr (VI) adsorption was characterized by single-phase and polyphase adsorption, mainly chemical adsorption. The thermodynamic parameters proved that the adsorption process was spontaneous and endothermic. The mechanistic investigation revealed that the mechanism of the adsorption of Cr (VI) by La-BC may include electrostatic interaction, ligand exchange, or complexation. Moreover, the co-existing anions and regeneration experiments proved that the La-BC is recyclable and has good prospects in the field of chrome-containing wastewater removal.

1. Introduction

Chromium (Cr) is amongst the foremost typical and venomous significant metal ions, which is widely found in wastewater from a variety of industries, such as textiles, metallurgy, metal electroplating, and tanneries [1]. Chromium can cause serious environmental problems and harm human health due to its problematic characteristics of bioaccumulation, non-biodegradability and potential carcinogenicity in the food chain [2,3].
Generally speaking, chromium in nature mainly exists in two stable states in a wide pH range: trivalent chromium (Cr (III)) and hexavalent chromium (Cr (VI)). Cr (III) is non-toxic and can be effectively removed by precipitation (such as chromium hydroxide) or adsorption [4,5,6,7]. Cr (VI) are more dangerous because it has toxicity, and higher solubility and mobility [4]. It appears in the forms of chromate (CrO42−, HCrO4−) and dichromate (Cr2O72−), which have caused great environmental concern [3,8]. As a priority toxic pollutant identified by the US environmental protection agency, Cr (VI) can cause serious toxic and detrimental effects to human health and ecosystems. When the Cr (VI) content in drinking water exceeds 0.05 mg/L and that in water for different uses exceeds 0.1 mg/L, it can cause harm to human health, such as kidney, liver and stomach damage, skin allergies and lung cancer [9], but in contaminated natural water and industrial wastewater, Cr (VI) tends to be more than 200 mg/L [10,11]. Therefore, practical methods must be developed to remove Cr (VI), in order to protect the aquatic environment.
Compared with strategies such as membrane separation, biodegradation, electrochemical oxidation, solvent extraction and other treatment methods, the capture of Cr (VI) using adsorbing media has numerous advantages, such as being a non-toxic and harmless process, easy operation, versatility, and low cost [12,13,14]. The adsorbents with different sites will interact with Cr (VI) through different mechanisms, including direct precipitation, electrostatic interaction, ligand exchange, intra-sphere complexation and redox [1,15,16,17]. Many of the naturally available adsorbents such as sawdust, pine needles and seaweed have the disadvantages of a low adsorption capacity and a slow adsorption process. Thus, in order to realize the unification of economic and environmental benefits, there is a need to create innovative and economical adsorbents for composite materials with high efficiency [18].
Biochar (BC) has recently received significant attention because of its beneficial surface physical/chemical properties for the removal of heavy metals from wastewater [19,20,21]. However, the surface of the original BC is usually negatively charged, with a low anion removal ability. Rare earth metal oxides can participate in chemical reactions as active components, and have been widely used in petroleum, metallurgy, ceramics, textiles and other fields. Lanthanum oxide (La2O3) has a good anionic complexation ability, but lacks stability under low pH conditions. In actuality, biochar fibers can take advantage of their large surface area and abundant surface functional groups to support lanthanum oxide; meanwhile, the pores in biochar could enhance the dispersion of La and improve the consumption efficiency, so biochar is a viable option to support La incorporation [22]. Recently, biochar materials with lanthanum oxide dropped have been extensively studied, and they exhibited several advantages in removing oxygen-containing acids, such as strong adsorption selectivity, remarkable adsorption capacity, a high removal rate and a wide pH range. According to Yang Bei (2019), through inner-sphere complexation, La-dropped biochar can form an La-O-P chemical bond with phosphate to remove PO43− in sewage [23], while Haiyang Yang (2019) stated that Cr (VI) adsorption might be related to the outer-sphere complexation. Therefore, we speculate that chromate can also bond with La-BC with the same chemical bond [24,25]. In addition, other literature data shows that lanthanum-containing materials have an excellent effect on the removal of phosphate, antimonate and arsenate in water [14,21,26,27,28,29,30,31]. As a great biochar doping component, La can improve the adsorption capacity of anions. However, there are few reports in the literature on the use of La-doped BC to remove Cr (VI). Moreover, the adsorption capacity of Cr (VI) by La-based adsorbents is also low in these relevant literatures. For example, the adsorption capacity of hexavalent chromium in chitosan and lanthanum mixed oxyhydroxide is only 48.3 mg/g [32]. In order to investigate the adsorption capacity of La for chromate, a lanthanum-oxide–loaded carbon fiber material was prepared by calcination at 90 0 °C. By using La-BC, Cr (VI) can be effectively removed. The possible mechanism is discussed in detail. It is proved that the adsorption effect of La-BC on Cr (VI) is better than that of other La-based adsorbents reported in the literature. Beyond that, La-BC is recyclable, and has good prospects in the field of chrome-containing wastewater removal.

2. Materials and Methods

2.1. Materials

The reagents included lanthanum chloride, sodium alginate (alighting), potassium dichromate, hydrochloric acid, sodium hydroxide, sulfuric acid, phosphoric acid, sodium chloride, sodium sulfate, sodium nitrate, sodium bicarbonate, disodium phosphate, acetone, and diphenylcarbazide. All of the chemicals and reagents were analytically pure, and were produced by the Sinopharmaceutical chemical reagent co., Ltd., Shanghai, China except for the sodium alginate (AR, Shanghai Aladdin Bio-Chem Technology Co., Ltd., Shanghai, China). All of the solutions were prepared using deionized water.

2.2. Preparation of the Adsorbent

The La3+-loaded sodium alginate fiber (La-SA) was prepared by wet spinning with 4% sodium alginate solution as the spinning solution and lanthanum chloride (LaCl3) solution with the same concentration as the coagulate bath. The La-SA was placed in an oven at 30 °C and dried for 24 h. The dried La-SA was transferred to a tube furnace and pyrolyzed at 900 °C for 1 h (with a heating rate of 5 °C/min). After being ground and sifted, the biochar (La-BC) loaded with lanthanum oxide (La2O3) was obtained for the experiment. Under the same concentration of sodium alginate, pure sodium alginate fibers were prepared with a mixture of 5% NaCl and 4% HCl as the coagulation bath. Through the same pyrolysis conditions, pure sodium alginate biochar (SA-BC) and pure lanthanum oxide (La2O3) were prepared in order to compare the adsorption performance of the samples.

2.3. Characterization

The Brunauer-Emmett-Teller equation was used to determine the specific surface area, and the pore structures were calculated by nitrogen adsorption/desorption isotherms carried out on a surface area and porosity analyzer (3H-2000PS2, Best Instrument Technology Co., Ltd., Beijing, China). The surface morphology of material was observed by scanning electron microscopy (SEM, SU8020, Hitachi Hi-Tech Co. Ltd., Tokyo, Japan). Besides this, the phase structure of the materials was examined by X-ray diffraction (XRD, DX2700, Shanghai Precision Instrument Co., Ltd., Shanghai, China) at a scan rate (2θ) of 6°/min, from 10° to 80°, and at an accelerating voltage of 40 kV. X-Ray photoelectron spectroscopy (XPS, ULTRAESCALAB 250Xi, Thermo Fisher Scientific, Waltham, MA, USA) was used to analyze the surface functional groups and the valence state of the chromium with monochromatic 150 WAl Kα radiation.

2.4. Adsorption and Desorption Experiments

A series of adsorption and desorption experiments were carried out in order to evaluate the adsorption properties of the La-BC and analyze its adsorption mechanism. Potassium dichromate (2.827 g) was dissolved in distilled water (1000 mL) to make a 1000 mg/L dichromate stock. Then, the stock was diluted to produce dichromate solutions of different concentrations. The effects of the carbonization temperature (700–1000 °C), solution pH (2–10), adsorption isotherm (initial concentration 20–1000 mg/L), adsorption kinetics (shaken for 3 h in oscillator), adsorption thermodynamics (adsorbent temperature 298–318 K) and co-existing acid ions on the adsorption of Cr (VI) were analyzed in turn. In order to assess the reusability of La-BC as a Cr (VI) adsorbent, five adsorption/desorption cycles were conducted. The filtrate was filtered with a 0.45 μm nylon membrane syringe after adsorption. The clear solution was extracted, and the possible leaching concentrations of Cr6+ and La3+ in the adsorbed solution were determined by a visible light spectrophotometer and an inductively coupled plasma emission spectrometer, respectively.
In all of the adsorption experiments, the dosage of La-BC was 1 g/L. The pH of all of the solutions was not adjusted separately, except for the pH experiment. Similarly, all of the experiments were conducted at room temperature (298 K or 303 K), except the adsorption thermodynamics experiment. Due to the indoor temperature difference in different seasons, the specific experimental conditions are described in detail in the results and discussion sections below. In addition, in all of the charts in this paper, the data—such as the Cr (VI) solution concentration and the adsorption capacity—were calculated by the total Cr (VI) content.

3. Results and Discussion

3.1. Preliminary Experiments

Before the formal batch adsorption experiment, the adsorption properties of pure sodium alginate biochar (SA-BC), pure lanthanum oxide (La2O3) and La-BC were compared through the preliminary experiment under the conditions of pH 4.6, 300 rpm, 303 K, contact time 5 h and adsorbent dosage 1 g/L (Figure 1). The data showed that the Cr(VI) adsorption capacity of the sample was ranked as La-BC > La2O3 > SA-BC, which may be due to the following reasons: (1) the surface of SA-BC is negatively charged, which leads to its low ability to remove anionic groups such as Cr2O72− and CrO42−, and the main adsorption process is physical adsorption caused by its porous structure; (2) La2O3 has a good anion complexation ability, but it is not stable in an acidic solution. Therefore, loading La2O3 onto SA-BC to prepare La-BC is a win–win situation. It can take advantage of the larger surface area and rich surface functional groups of biochar to support La2O3, and the pores in biochar can enhance the dispersion of La, improve the stability of La2O3, and aid the removal efficiency of Cr (VI).

3.2. Characterization of the La-BC

Table S1 shows some of the physical properties of carbonized adsorbents at different temperatures. According to the nitrogen adsorption–desorption curve (Figure S1), it can be found that all of the four carbon adsorbents are type IV with H4 hysteresis loops, indicating that the lanthanum-supported biochar, through high temperature carbonization, is a mesoporous material [28,33]. The specific surface area and porosity of the adsorbent have an important influence on its adsorption capacity [20,34]. Generally speaking, the larger the specific surface area is, the more adsorption points are available, and the larger the adsorption capacity will be. The specific surface area of La-BC (900 °C) reached 177.41 m2/g, while the specific surface areas of La-BC (700 °C), La-BC (800 °C) and La-BC (1000 °C) were 8.21 m2/g, 38.61 m2/g and 52.08 m2/g respectively, indicating that La-BC (900 °) might be the adsorbent with the highest adsorption capacity. In addition, by comparing the pore volume, it was found that the pore volume of La-BC (900 °C) was 0.2515 cm3/g, which was larger than the other three adsorbents. Larger pore volumes also facilitate the adsorption of the target elements.
SEM images, TEM images and element mapping were used to research and analyze the surface morphology and element distribution of La-BC (900 °C) (Figure 2). As a porous material, biochar is a good substrate for lanthanum deposition. The sodium alginate biochar supported by lanthanum was fibrous, with a diameter of about 20–50 μm. The surface was rough and irregular, with a large number of acicular crystals and loose pores distributed upon it (Figure 2a–c). The same morphology was also shown in TEM images, in which the fractured biochar fibers were supported by needle-like or rod-like crystals (Figure 2d–f). The lattice fringe of La-BC can be observed more clearly through the analysis of the high-resolution TEM image (Figure 2g). Compared with the standard card La2O3 (PDF#05-0602), the lattice spacings of 0.335 nm and 0.346 nm both correspond to the (100) plane of La2O3. In the SEM-EDS element mapping image of the La-BC (900 °C), the La element can be observed evenly (Figure 2h), proving that the La element has been successfully loaded onto the surface of the biochar.
The XRD patterns of La-BC (900 °C) at four different carbonization temperatures are shown in Figure 3. The composition of its elements and substances was analyzed. It was found that the existing forms of La change with the increase of the calcining temperature. For La-BC at 700 °C and La-BC at 800 °C, there were diffraction peaks of La2CO5 (PDF#23-0320), while for La-BC at 900 °C and La-BC at 1000 °C, there were characteristic peaks of La2O3 (PDF#05-0602), which proves that La was successfully loaded onto the adsorption materials [30], and that the lanthanum-containing products were different at different carbonization temperatures.
In order to further identify the functional groups on the La-BC and to obtain the possible adsorption mechanism of Cr (VI), the sample La-BC (900 °C) was analyzed by X-ray photoelectron spectroscopy (Figure 4). All of the peaks are calibrated by using C 1s (284.3 eV) as a reference. The wide-scan XPS spectrum of La-BC showed that the elements C (63.4%) and O (28.96%) were the main components (Figure 4a). The peaks at the binding energies of 835.6 eV, 839.0 eV, 852.6 eV and 855.8 eV confirmed the introduction of La3+ on the biochar surface (Figure 4b).

3.3. Adsorption Isotherm

The adsorption isotherm refers to the relationship curve between the adsorption amount of the adsorbent and the equilibrium concentration of the adsorbent after the adsorption process occurs at the set adsorption temperature. This process can be fitted by the adsorption isotherm model (Text S1). The correlation between the Langmuir and Freundlich isotherm models and the experimental data with different initial chromium concentrations was studied. The isothermal adsorption model fitting of carbonized La-BC at four temperatures is shown in Figure 5. Under the conditions of pH 4.6, 300 rpm, 303 K, contact time 5 h and a 1 g/L dosage of the adsorbent, adsorption experiments were carried out with four kinds of La-BC, in which the range of the initial potassium dichromate concentration was from 20 to 1000 mg/L. It was found that the adsorption capacity of La-BC (700–1000 °C) increased from 2.2 to 37.6 mg/g, 9.6 to 56.3 mg/g, 5.8 to 83.5 mg/g, and 3.2 to 39.6 mg/g, respectively. The increase of the initial concentration of the potassium dichromate solution might result in the improvement of the collisions between La-BC and Cr (VI), and might increase the driving force of removing Cr (VI), thus promoting adsorption [35]. The adsorption isotherm shows that, in the carbonized La-BC at four different temperatures, the adsorption capacity of 900 °C La-BC is higher, which may be attributed to the following two reasons: (1) as the specific surface area and pore size of 900 °C La-BC are larger than those of the other three kinds of La-modified biochar (Table S1), there are more available adsorption sites, enhancing the adsorption capacity of 900 °C La-BC; (2) according to the XRD pattern (Figure 3), the lanthanum compound loaded with 900 °C La-BC and 1000 °C La-BC was La2O3, which could be used as an active adsorption site for metal ions. The Langmuir isotherm model showed that the saturated adsorption amounts of Cr (VI) with four kinds of La-BCs, respectively, were 41.4 mg/g, 67.4 mg/g, 104.9 mg/g and 49.9 mg/g (Table S2). The fitting results showed that the adsorption process had consistency with both the Langmuir model and the Freundlich model, but conformed to the Langmuir model more, suggesting that the adsorption process should exist in monolayer and multilayer adsorption, especially the adsorption of a single molecule layer [35,36].

3.4. Adsorption Kinetics

Adsorption is a continuous dynamic process characterized by ‘external diffusion —internal diffusion’. This process can be fitted by the adsorption kinetic model (Text S2). In order to evaluate the chromate adsorption rates of La-BC, the time-dependent sorption was conducted under the conditions of an initial Cr (VI) concentration of 200 mg/L, pH 4.6, 300 rpm, 303 K, contact time 5 h and a 1 g/L adsorbent dose. The relationship between the adsorption amount of Cr (VI) and the time of the La-BC carbonized at four temperatures is shown in Figure 6a. The adsorption process can be divided into three stages: a rapid adsorption stage, a slow adsorption stage, and an adsorption equilibrium stage. In the first 20 min, the adsorption reaction of Cr (VI) with La-BC was very rapid. The Cr (VI) adsorption capacities of La-BC (700–1000 °C) were 14.1 mg/g, 19.0 mg/g, 30.3 mg/g and 15.5 mg/g, which occupied the corresponding equilibrium adsorption capacities of 95.5%, 93.1%, 93.5% and 95.7%, respectively, and the adsorption capacity of La-BC at 900 °C was far higher than that of the other three adsorbents. The following 70 min is the slow adsorption phase. After 90min, there was no significant difference between the concentration of Cr (VI) and that after 3h in the solvent, showing that the adsorption process entered the equilibrium stage due to the saturation of the sites [1,37]. The differences between these stages can be explained as follows: (1) at first, the concentration of Cr (VI) at the interface of the adsorbent was the highest, forming a large adsorption dynamic gradient, which drove the Cr (VI) to occupy the adsorption site on the outer surface of the La-BC rapidly; (2) when Cr (VI) entered the interior of La-BC, the adsorption rate decreased due to the blockage of the pores and the decrease of the active adsorption sites; (3) when the slow adsorption continued, the adsorption rate gradually decreased until it reached the dynamic adsorption equilibrium.
In order to determine the adsorption mechanism, the equilibrium data were used to fit the pseudo-first-order and pseudo-second-order models (Table S3). The fitting results showed that the pseudo second-order kinetic equation can better describe the adsorption behavior. In other words, the adsorption of Cr (VI) on La-BC was closer to chemisorption, which is carried out through polar functional groups sharing or exchanging electrons between the adsorbate and adsorbent [38,39].

3.5. Adsorption Thermodynamics

Temperature is an important factor affecting the adsorption effect. Temperature changes affect the value of the thermodynamic parameters (Text S3). Under the conditions of an initial Cr (VI) concentration of 100–900 mg/L, contact time 5 h, pH = 4.6, adsorbent 300 rpm and a 1 g/L dose, the relationship between the adsorption amount of Cr (VI) with La-BC (900 °C) and the adsorption temperature is shown in Figure 6b. The increase of the adsorption temperature makes the adsorption amount increase. The calculated adsorption reaction enthalpy change ΔH was 41.66 KJ/mol, ΔS was 144.6 J/(mol·K), and the Gibbs free energy change ΔG < 0 at each temperature (Table S4), which showed that the adsorption was a spontaneous endothermic reaction; in other words, the rising of the temperature lead to a prompt reaction [12,16,40].

3.6. Effect of the Solution pH on the Adsorption Experiment

Under the conditions of an initial concentration of 250 mg/L, 300 rpm, 298 K, contact time 5 h and an adsorbent of 1 g/L, the effect of the pH on the adsorption capacity of Cr (VI) with La-BC (900 °C) is shown in Figure 7a, and the comparison of the initial and final pH of the solution before and after adsorption is also demonstrated. The selected pH range was 2–10, within which the adsorption capacity of the chromate decreased significantly with the increase of the pH, and the maximum adsorption capacity was 68.52 mg/g, appearing at pH = 2. The existent form of chromate is related to the pH of the solution. At an acidic pH, the main types of chromate existent forms are Cr2O72−, HCrO4− and CrO42− [12,41]. At the same time, the surface of La-loaded biochar is positively charged; therefore, under acidic conditions, the adsorption mechanism of chromate by La-BC may be explained as an electrostatic interaction [14,32]. The change of pH before and after the adsorption proves another possible mechanism: the final pH of the solution was higher than the initial pH, indicating that OH− was released during the process of the chromate adsorption, which confirms that a ligand exchange interaction was involved [30]. Based on the above, several possible adsorption equations are summarized as follows:
La2O3 + HCrO4− + H+ → La2CrO6 + H2O
La2O3 + Cr2O72− + H+ → La2Cr2O9 + OH−
La2O3 + CrO42− + H2O → La2CrO6 + 2OH−
With the increase of pH (>pHpzc), a large amount of OH− was released into the solution, which can compete with chromate ions for active adsorption sites, and can generate electrostatic repulsion [23]. All of the above resulted in a significant decrease of the adsorption of the chromate at higher pH values; therefore, the range of pH > 7 was no longer taken into account in the subsequent experiments.
The XRD images of La-BC (900 °C) before and after the adsorption of the dichromate solutions with a pH range of 2–7 were compared (Figure 7b). The results showed that when pH > 2, the main peaks after adsorption were characteristic peaks of La (OH)3 (PDF#36-1481). When pH = 2, the XRD image of the La-BC was a smooth curve without any peak. The reason may be that the La2O3 in the La-BC (900 °C) was largely dissolved into the solution in a strong acidic environment. For this reason, the amount of La dissolution of the adsorbed dichromate solution was detected (Figure S2), and the results confirmed that a large amount of La was dissolved at pH = 2. The initial pH of the dichromate solution was about 4–5; within this range, not only can the adsorption amount of La-BC be guaranteed not to be too low but also the dissolution amount of La can be kept at a low level. Based on the results, it was finally decided that the experiment would not take too much adjustment to the pH of the initial solution, and it should be kept at pH = 4.6.

3.7. Effect of Coexisting Acid Ions on the Adsorption Experiments

Five kinds of 100 mg/L K2Cr2O7 solutions containing NaCl, Na2SO4, NaNO3, NaHCO3 and Na2HPO4 were prepared, in which the concentrations of the coexisting ions were 0.05 mol/L, 0.1 mol/L and 0.2 mol/L, respectively. The pure 100 mg/L K2Cr2O7 was used as a blank control, and the adsorption experiments were carried out under the conditions of 300 rpm, 303 K, contact time 5 h, pH 4.6 and a 1 g/L dosage of La-BC (900 °C). It was shown that different interfering ions had different influences on the adsorption amount of Cr (VI) (Figure 8a). The results showed that Cl− and NO3− had no effect on the adsorption of chromate, and SO42− had little effect. However, HCO3− and HPO42− seriously interfered the adsorption of chromate, which may be for the following two reasons: (1) the structure of these oxygen-containing acid groups was similar to that of Cr2O72− and CrO42−, resulting in competition in the adsorption process; (2) both carbonic acid and phosphoric acid are weak acids, so the hydrolysis degree of HCO3− and HPO42− in the solution is greater than the degree of ionization—this is why NaHCO3 and Na2HPO4 solutions are weakly alkaline. The release of OH− led to the decrease of the adsorption amount of the chromate.

3.8. Cycle Experiments

The experiment of the adsorption of Cr (VI) by La-BC (900 °C) was carried out under the conditions of an initial Cr (VI) concentration 200 mg/L, pH 4.6, 300 rpm, 303 K, contact time 5 h and a 1 g/L adsorbent dosage, and five cycles were carried out for the desorption treatment of 1 mol/L NaOH (Figure 8b). After each cycle, the recovered product was calcined in inert gas at a high temperature in order to ensure that the composition of the recovered product was the same as the original La-BC material. The experimental results showed that La-BC (900 °C) had good stability, a low loss in five cycles, and a good reuse effect. The circulating experiment also proved the possibility of the use of La-BC in treating chromium-containing wastewater.

3.9. Adsorption Mechanism

The pH experiments and XRD characterization results indicated that the adsorption behavior of La-BC on Cr (VI) might have an electrostatic interaction and a ligand exchange (Figure 7). In addition, X-Ray photoelectron spectroscopy analysis was performed on the La-BC (900 °C) after the adsorption of chromite, and a comparison was made with an XPS image of La-BC (900 °C) before the adsorption (Figure 9). The wide-scan XPS spectrum of La-BC after the experiments showed that the peak of the Cr element appeared in La-BC (900 °C) (Figure 9a). Moreover, the corresponding peaks where the binding capacity was 577.8 eV, 579.7 eV proved that Cr (VI) was successfully absorbed (Figure 9b) [42]. The Cr has been absorbed successfully. In the La3d images, the binding energy of the element La had a negative displacement (0.4–0.7 eV) after adsorption (Figure 9c), indicating that electron transfer occurred between La-BC (900 °C) and chromite, which formed a strong chemical bond [30]. The O1s spectrum changed significantly before and after the adsorption, which could explain the adsorption mechanism (Figure 9d,e). The O1s deconvolution (Figure 9d) indicated that three main oxygen components—lattice oxygen La-O (530.8 eV), OH− (531.9 eV), and adsorbed H2O (533.0 eV)—existed in the La-BC. However, after the Cr (VI) sorption, the peak of La-O nearly disappeared, while the H2O percentage increased (Figure 9e). This was because La2O3 is hygroscopic, and it adsorbed moisture to become La (OH)3 [28]. All of the above results show that the adsorption may be caused by ligand exchange or complexation. The increase of the proportion of the element O from 28.96% to 32.47% might also be explained by the adsorption of the oxygen-containing acid radicals CrO42− and Cr2O72−.

4. Conclusions

In this experiment, wet spinning and ion exchange were combined to load La3+ onto sodium alginate fiber, and then La3+ was converted to La2O3 in the process of high-temperature carbonization. Lanthanum-oxide–modified biochar showed an excellent adsorption capacity for chromate, and it also had a high adsorption capacity in a potassium dichromate solution with a high concentration at room temperature, and its saturated adsorption capacity was about 104.9 mg/g. The isotherm data showed that the adsorption process is more consistent with the Langmuir model, and that it has a higher correlation with the adsorption of a single molecular layer. The adsorption kinetic data followed the pseudo-second-order kinetic model, showing that the adsorption process was dominated by chemisorption. The thermodynamic parameters proved that the adsorption of chromate by La-BC is spontaneous and endothermic. In addition to physical adsorption, the adsorption mechanism of Cr (VI) in La-BC may be electrostatic interaction, ligand exchange, or complexation (Figure 10). Compared with Cr (VI) adsorbents in other literatures (Table 1), La-BC has the advantages of a large adsorption capacity, a simple preparation process and good recycling performance.
Therefore, La-BC can be used as a new type of environmentally friendly adsorbent, which has great research significance and broad development prospects in the field of sewage treatment.

Supplementary Materials

The following are available online at https://www.mdpi.com/article/10.3390/ma14092224/s1, Text S1: Langmuir and Freundlich isotherm models, Text S2: Pseudo-first- and pseudo-second-order kinetic models, Text S3: Absorption thermodynamics, Table S1: Physical properties of the different samples, Table S2: Parameters of the Cr (VI) adsorption isotherms based on the Freundlich and Langmuir models, Table S3: Parameters of the Cr (VI) adsorption kinetics based on the pseudo-first-order and pseudo-second-order dynamic models, Table S4: Thermodynamic parameters for chromate adsorption with La-BC (900 ℃), Figure S1: Nitrogen adsorption/desorption isotherms for different samples, Figure S2: The leaching rate of lanthanum when the pH is in the range 2–7.

Author Contributions

Conceptualization, X.S. and Y.S.; methodology, X.S. and Y.S.; investigation, X.S. and Y.S.; software, X.S.; validation, X.S.; formal analysis, X.S., Y.S. and Y.C.; resources, P.G., Y.S. and Y.C.; data curation, X.S. and P.G.; writing—original draft preparation, X.S.; writing—review and editing, X.S., P.G., Y.S. and Y.C.; supervision, Y.S. and Y.C.; project administration, Y.C. All authors have read and agreed to the published version of the manuscript.

Funding

This research was funded by the Science and Technology Support Plan for Youth Innovation of Colleges in Shandong Province (DC2000000961), China Geological Survey (Grant DD20189503) and the Natural Science Foundation of Shandong Province, China (No. ZR2019BF031).

Institutional Review Board Statement

Not applicable.

Informed Consent Statement

Not applicable.

Data Availability Statement

Data sharing is not applicable for this article.

Conflicts of Interest

The authors declare no conflict of interest. The funders had no role in the design of the study; in the collection, analyses, or interpretation of data; in the writing of the manuscript, or in the decision to publish the results.

References

  1. Fan, Z.; Zhang, Q.; Gao, B.; Li, M.; Liu, C.; Qiu, Y. Removal of hexavalent chromium by biochar supported nZVI composite: Batch and fixed-bed column evaluations, mechanisms, and secondary contamination prevention. Chemosphere 2019, 217, 85–94. [Google Scholar] [CrossRef]
  2. Lyu, H.; Tang, J.; Huang, Y.; Gai, L.; Zeng, E.Y.; Liber, K.; Gong, Y. Removal of hexavalent chromium from aqueous solutions by a novel biochar supported nanoscale iron sulfide composite. Chem. Eng. J. 2017, 322, 516–524. [Google Scholar] [CrossRef]
  3. Shi, S.; Yang, J.; Liang, S.; Li, M.; Gan, Q.; Xiao, K.; Hu, J. Enhanced Cr(VI) removal from acidic solutions using biochar modified by Fe3O4@SiO2-NH2 particles. Sci. Total Environ. 2018, 628–629, 499–508. [Google Scholar] [CrossRef]
  4. Kieber, R.J.; Helz, G.R. Indirect photoreduction of aqueous chromium(VI). Environ. Sci. Technol. 1992, 26, 307–312. [Google Scholar] [CrossRef]
  5. Fu, H.; Zhou, Z.; Zheng, S.; Xu, Z.; Alvarez, P.J.J.; Yin, D.; Qu, X.; Zhu, D. Dissolved Mineral Ash Generated by Vegetation Fire Is Photoactive under the Solar Spectrum. Environ. Sci. Technol. 2018, 52, 10453–10461. [Google Scholar] [CrossRef] [PubMed]
  6. Hausladen, D.M.; Alexander-Ozinskas, A.; McClain, C.N.; Fendorf, S. Hexavalent Chromium Sources and Distribution in California Groundwater. Environ. Sci. Technol. 2018, 52, 8242–8251. [Google Scholar] [CrossRef]
  7. Zhang, W.; Liu, F.; Sun, Y.; Zhang, J.; Hao, Z. Simultaneous redox conversion and sequestration of chromate(VI) and arsenite(III) by iron(III)-alginate based photocatalysis. Appl. Catal. B Environ. 2019, 259, 118046. [Google Scholar] [CrossRef]
  8. Liu, T.; Zhao, L.; Sun, D.; Tan, X. Entrapment of nanoscale zero-valent iron in chitosan beads for hexavalent chromium removal from wastewater. J. Hazard. Mater. 2010, 184, 724–730. [Google Scholar] [CrossRef]
  9. World Health Organization. Guidelines for Drinking Water Quality; World Health Organization: Geneva, Switzerland, 2011. [Google Scholar]
  10. Lu, A.; Zhong, S.; Chen, J.; Shi, J.; Tang, J.; Lu, X. Removal of Cr(VI) and Cr(III) from Aqueous Solutions and Industrial Wastewaters by Natural Clinopyrrhotite. Environ. Sci. Technol. 2006, 40, 3064–3069. [Google Scholar] [CrossRef]
  11. Ai, Z.; Cheng, Y.; Zhang, L.; Qiu, J. Efficient Removal of Cr(VI) from Aqueous Solution with Fe@Fe2O3Core−Shell Nanowires. Environ. Sci. Technol. 2008, 42, 6955–6960. [Google Scholar] [CrossRef] [PubMed]
  12. Ajmani, A.; Shahnaz, T.; Subbiah, S.; Narayanasamy, S. Hexavalent chromium adsorption on virgin, biochar, and chemically modified carbons prepared from Phanera vahlii fruit biomass: Equilibrium, kinetics, and thermodynamics approach. Environ. Sci. Pollut. Res. 2019, 26, 32137–32150. [Google Scholar] [CrossRef]
  13. Li, Y.; Zhang, D.; Li, W.; Lan, Y.; Li, Y. Efficient removal of As(III) from aqueous solution by S-doped copper-lanthanum bimetallic oxides: Simultaneous oxidation and adsorption. Chem. Eng. J. 2020, 384, 123274. [Google Scholar] [CrossRef]
  14. Siddiqui, M.F.; Khan, T.A. Gelatin-polyvinyl alcohol/lanthanum oxide composite: A novel adsorbent for sequestration of arsenic species from aqueous environment. J. Water Process Eng. 2020, 34, 101071. [Google Scholar] [CrossRef]
  15. Peng, Y.; Tang, D.; Wang, Q.; He, T.; Chu, Y.; Li, R. Adsorption of Chromate from Aqueous Solution by Polyethylenimine Modified Multi-Walled Carbon Nanotubes. J. Nanosci. Nanotechnol. 2018, 18, 4006–4013. [Google Scholar] [CrossRef]
  16. Wang, B.; Li, F.; Wang, L. Enhanced hexavalent chromium (Cr(VI)) removal from aqueous solution by Fe–Mn oxide-modified cattail biochar: Adsorption characteristics and mechanism. Chem. Ecol. 2019, 36, 138–154. [Google Scholar] [CrossRef]
  17. Yin, Z.; Xu, S.; Liu, S.; Xu, S.; Li, J.; Zhanga, Y. A novel magnetic biochar prepared by K2FeO4-promoted oxidative pyrolysis of pomelo peel for adsorption of hexavalent chromium. Bioresour. Technol. 2020, 300, 122680. [Google Scholar] [CrossRef]
  18. Gupta, V.; Agarwal, S.; Saleh, T.A. Chromium removal by combining the magnetic properties of iron oxide with adsorption properties of carbon nanotubes. Water Res. 2011, 45, 2207–2212. [Google Scholar] [CrossRef]
  19. Inyang, M.I.; Gao, B.; Yao, Y.; Xue, Y.; Zimmerman, A.; Mosa, A.; Pullammanappallil, P.; Ok, Y.S.; Cao, X. A review of biochar as a low-cost adsorbent for aqueous heavy metal removal. Crit. Rev. Environ. Sci. Technol. 2016, 46, 406–433. [Google Scholar] [CrossRef]
  20. Li, H.; Dong, X.; da Silva, E.B.; de Oliveira, L.M.; Chen, Y.; Ma, L.Q. Mechanisms of metal sorption by biochars: Biochar characteristics and modifications. Chemosphere 2017, 178, 466–478. [Google Scholar] [CrossRef]
  21. Wang, L.; Wang, J.; Wang, Z.; He, C.; Lyu, W.; Yan, W.; Yang, L. Enhanced antimonate (Sb(V)) removal from aqueous solution by La-doped magnetic biochars. Chem. Eng. J. 2018, 354, 623–632. [Google Scholar] [CrossRef]
  22. Koilraj, P.; Sasaki, K. Selective removal of phosphate using La-porous carbon composites from aqueous solutions: Batch and column studies. Chem. Eng. J. 2017, 317, 1059–1068. [Google Scholar] [CrossRef]
  23. Yang, B.; Feng, Y.; Yu, Y.; He, S.; Liu, H.; Xue, L.; Yang, L. Lanthanum ferrite nanoparticles modification onto biochar: Derivation from four different methods and high performance for phosphate adsorption. Environ. Sci. Pollut. Res. 2019, 26, 2010–22020. [Google Scholar] [CrossRef]
  24. Yang, H.; Wang, Y.; Bender, J.; Xu, S. Removal of Arsenate and Chromate by Lanthanum-modified Granular Ceramic Material: The Critical Role of Coating Temperature. Sci. Rep. 2019, 9, 1–12. [Google Scholar] [CrossRef] [Green Version]
  25. Catalano, J.G.; Park, C.; Fenter, P.; Zhang, Z. Simultaneous inner- and outer-sphere arsenate adsorption on corundum and hematite. Geochim. Cosmochim. Acta 2008, 72, 1986–2004. [Google Scholar] [CrossRef]
  26. Liao, T.; Li, T.; Su, X.; Yu, X.; Song, H.; Zhu, Y.; Zhang, Y. La(OH)3-modified magnetic pineapple biochar as novel adsorbents for efficient phosphate removal. Bioresour. Technol. 2018, 263, 207–213. [Google Scholar] [CrossRef] [PubMed]
  27. Lin, L.; Song, Z.; Khan, Z.H.; Liu, X.; Qiu, W. Enhanced As(III) removal from aqueous solution by Fe-Mn-La-impregnated biochar composites. Sci. Total Environ. 2019, 686, 1185–1193. [Google Scholar] [CrossRef] [PubMed]
  28. Chen, C.; Xu, L.; Huo, J.B.; Gupta, K.; Fu, M.-L. Simultaneous removal of butylparaben and arsenite by MOF-derived porous carbon coated lanthanum oxide: Combination of persulfate activation and adsorption. Chem. Eng. J. 2020, 391, 123552. [Google Scholar] [CrossRef]
  29. Li, X.; Chen, J.; Zhang, Z.; Kuang, Y.; Yang, R.; Wu, D. Interactions of phosphate and dissolved organic carbon with lanthanum modified bentonite: Implications for the inactivation of phosphorus in lakes. Water Res. 2020, 181, 115941. [Google Scholar] [CrossRef]
  30. Shan, S.; Wang, W.; Liu, D.; Zhao, Z.; Shi, W.; Cui, F. Remarkable phosphate removal and recovery from wastewater by magnetically recyclable La2O2CO3/gamma-Fe2O3 nanocomposites. J. Hazard. Mater. 2020, 397, 122597. [Google Scholar] [CrossRef]
  31. Zhong, Z.; Lu, X.; Yan, R.; Lin, S.; Wu, X.; Huang, M.; Liu, Z.; Zhang, F.; Zhang, B.; Zhu, H.; et al. Phosphate sequestration by magnetic La-impregnated bentonite granules: A combined experimental and DFT study. Sci. Total Environ. 2020, 738, 139636. [Google Scholar] [CrossRef]
  32. Preethi, J.; Vigneshwaran, S.; Meenakshi, S. Performance of chitosan engraved iron and lanthanum mixed oxyhydroxide for the detoxification of hexavalent chromium. Int. J. Biol. Macromol. 2019, 130, 491–498. [Google Scholar] [CrossRef]
  33. Xing, Y.; Cheng, J.; Wu, J.; Zhang, M.; Li, X.-A.; Pan, W. Direct electrospinned La2O3 nanowires decorated with metal particles: Novel 1 D adsorbents for rapid removal of dyes in wastewater. J. Mater. Sci. Technol. 2020, 45, 84–91. [Google Scholar] [CrossRef]
  34. Bagreev, A.; Bandosz, T.J.; Locke, D.C. Pore structure and surface chemistry of adsorbents obtained by pyrolysis of sewage sludge-derived fertilizer. Carbon 2001, 39, 1971–1979. [Google Scholar] [CrossRef]
  35. Moussavi, G.; Barikbin, B. Biosorption of chromium(VI) from industrial wastewater onto pistachio hull waste biomass. Chem. Eng. J. 2010, 162, 893–900. [Google Scholar] [CrossRef]
  36. Gupta, V.K.; Rastogi, A. Biosorption of hexavalent chromium by raw and acid-treated green alga Oedogonium hatei from aqueous solutions. J. Hazard. Mater. 2009, 163, 396–402. [Google Scholar] [CrossRef] [PubMed]
  37. Liang, J.; Li, X.; Yu, Z.; Zeng, G.; Luo, Y.; Jiang, L.; Yang, Z.; Qian, Y.; Wu, H. Amorphous MnO2 Modified Biochar Derived from Aerobically Composted Swine Manure for Adsorption of Pb(II) and Cd(II). ACS Sustain. Chem. Eng. 2017, 5, 5049–5058. [Google Scholar] [CrossRef]
  38. Ho, Y.S.; McKay, G. Pseudo-second-order model for sorption processes. Process Biochem. 1999, 34, 451–465. [Google Scholar] [CrossRef]
  39. Zhang, X.; Zhang, L.; Li, A. Eucalyptus sawdust derived biochar generated by combining the hydrothermal carbonization and low concentration KOH modification for hexavalent chromium removal. J. Environ. Manag. 2018, 206, 989–998. [Google Scholar] [CrossRef]
  40. You, N.; Wang, X.F.; Li, J.Y.; Fan, H.T.; Shen, H.; Zhang, Q. Synergistic removal of arsanilic acid using adsorption and magnetic separation technique based on Fe3O4@ graphene nanocomposite. J. Ind. Eng. Chem. 2019, 70, 346–354. [Google Scholar] [CrossRef]
  41. Labied, R.; Benturki, O.; Hamitouche, A.E.; Donnot, A. Adsorption of hexavalent chromium by activated carbon obtained from a waste lignocellulosic material (Ziziphus jujubacores): Kinetic, equilibrium, and thermodynamic study. Adsorpt. Sci. Technol. 2018, 36, 1066–1099. [Google Scholar] [CrossRef] [Green Version]
  42. Koilraj, P.; Sasaki, K. Eco-Friendly Alkali-Free Arginine-Assisted Hydrothermal Synthesis of Different Layered Double Hydroxides and Their Chromate Adsorption/Reduction Efficiency. ChemistrySelect 2017, 2, 10459–10469. [Google Scholar] [CrossRef]
  43. Yan, E.; Cao, M.; Ren, X.; Jiang, J.; An, Q.; Zhang, Z.; Gao, J.; Yang, X.; Zhang, D. Synthesis of Fe3O4 nanoparticles functionalized polyvinyl alcohol/chitosan magnetic composite hydrogel as an efficient adsorbent for chromium (VI) removal. J. Phys. Chem. Solids 2018, 121, 102–109. [Google Scholar] [CrossRef]
  44. Bagheri, M.; Younesi, H.; Hajati, S.; Borghei, S.M. Application of chitosan-citric acid nanoparticles for removal of chromium (VI). Int. J. Biol. Macromol. 2015, 80, 431–444. [Google Scholar] [CrossRef] [PubMed]
  45. Liu, Q.; Yang, B.; Zhang, L.; Huang, R. Adsorptive removal of Cr(VI) from aqueous solutions by cross-linked chitosan/bentonite composite. Korean J. Chem. Eng. 2015, 32, 1314–1322. [Google Scholar] [CrossRef]
Materials 14 02224 g001 550
Figure 1. Pre-experiment: comparison of the adsorption capacity of Cr (VI) by SA-BC, La2O3 and La-BC.
Figure 1. Pre-experiment: comparison of the adsorption capacity of Cr (VI) by SA-BC, La2O3 and La-BC.
Materials 14 02224 g001
Materials 14 02224 g002 550
Figure 2. (a–c) SEM images of La-BC; (d–g) TEM images of La-BC; (h) elemental mapping images of La-BC.
Figure 2. (a–c) SEM images of La-BC; (d–g) TEM images of La-BC; (h) elemental mapping images of La-BC.
Materials 14 02224 g002
Materials 14 02224 g003 550
Figure 3. XRD patterns of the different carbonization temperatures of the La-BC samples.
Figure 3. XRD patterns of the different carbonization temperatures of the La-BC samples.
Materials 14 02224 g003
Materials 14 02224 g004 550
Figure 4. (a) XPS spectra of the La-BC (900 °C) before Cr (VI) adsorption; (b) La 3d spectra of La-BC (900 °C) before Cr (VI) adsorption.
Figure 4. (a) XPS spectra of the La-BC (900 °C) before Cr (VI) adsorption; (b) La 3d spectra of La-BC (900 °C) before Cr (VI) adsorption.
Materials 14 02224 g004
Materials 14 02224 g005 550
Figure 5. Fitting the adsorption data of Cr (VI) on La-BC (900 °C) to (a) the Langmuir isotherm, and (b) the Freundlich isotherm.
Figure 5. Fitting the adsorption data of Cr (VI) on La-BC (900 °C) to (a) the Langmuir isotherm, and (b) the Freundlich isotherm.
Materials 14 02224 g005
Materials 14 02224 g006 550
Figure 6. (a) Relationship between the adsorption amount of Cr (VI) and the adsorption time by La-BC at four carbonization temperatures; (b) relationship between the adsorption amount of Cr (VI) and the adsorption temperature by La-BC (900 °C).
Figure 6. (a) Relationship between the adsorption amount of Cr (VI) and the adsorption time by La-BC at four carbonization temperatures; (b) relationship between the adsorption amount of Cr (VI) and the adsorption temperature by La-BC (900 °C).
Materials 14 02224 g006
Materials 14 02224 g007 550
Figure 7. (a) The effect of pH on the adsorption amount, and the comparison of the initial and final pH; (b) the XRD images of La-BC (900 °C) after the adsorption with a pH range of 2–7.
Figure 7. (a) The effect of pH on the adsorption amount, and the comparison of the initial and final pH; (b) the XRD images of La-BC (900 °C) after the adsorption with a pH range of 2–7.
Materials 14 02224 g007
Materials 14 02224 g008 550
Figure 8. (a) Effect of coexisting ions on the adsorption amount of Cr (VI); (b) five cycles of Cr (VI) adsorption by La-BC (900 °C).
Figure 8. (a) Effect of coexisting ions on the adsorption amount of Cr (VI); (b) five cycles of Cr (VI) adsorption by La-BC (900 °C).
Materials 14 02224 g008
Materials 14 02224 g009 550
Figure 9. (a) XPS spectra of the La-BC (900 °C) after Cr (VI) adsorption(a); (b) Cr2p; (c) La3d; (d) the O1s spectra of La-BC (900 °C) before and (e) after Cr (VI) adsorption.
Figure 9. (a) XPS spectra of the La-BC (900 °C) after Cr (VI) adsorption(a); (b) Cr2p; (c) La3d; (d) the O1s spectra of La-BC (900 °C) before and (e) after Cr (VI) adsorption.
Materials 14 02224 g009
Materials 14 02224 g010 550
Figure 10. Preparation process of La-BC and the mechanism of Cr (VI) adsorption with it.
Figure 10. Preparation process of La-BC and the mechanism of Cr (VI) adsorption with it.
Materials 14 02224 g010
Table
Table 1. Literature data on the adsorption of Cr (VI) ions by various adsorbents.
Table 1. Literature data on the adsorption of Cr (VI) ions by various adsorbents.
AdsorbentAdsorption Capacity (mg/g)Ref.
MgAl-LDH84.2[42]
MWCNTs-7017.2[15]
Chitosan engraved iron and lanthanum Mixed oxyhydroxide106.04[32]
Fe3O4 nanoparticles functionalized polyvinyl alcohol/chitosan magnetic composite hydrogel24.69[43]
Chitosan-citric acid nanoparticles106.15[44]
Cross-linked chitosan bentonite composite89.13[45]
Fe–Mn oxide-modified biochar59.8[16]
Biochar supported nZVI composite31.53[1]
La2O3-dropped biochar104.9This article
Publisher’s Note: MDPI stays neutral with regard to jurisdictional claims in published maps and institutional affiliations.

Share and Cite

MDPI and ACS Style

Sun, X.; Guo, P.; Sun, Y.; Cui, Y. Adsorption of Hexavalent Chromium by Sodium Alginate Fiber Biochar Loaded with Lanthanum. Materials 2021, 14, 2224. https://doi.org/10.3390/ma14092224

AMA Style

Sun X, Guo P, Sun Y, Cui Y. Adsorption of Hexavalent Chromium by Sodium Alginate Fiber Biochar Loaded with Lanthanum. Materials. 2021; 14(9):2224. https://doi.org/10.3390/ma14092224

Chicago/Turabian Style

Sun, Xinzhe, Peng Guo, Yuanyuan Sun, and Yuqian Cui. 2021. "Adsorption of Hexavalent Chromium by Sodium Alginate Fiber Biochar Loaded with Lanthanum" Materials 14, no. 9: 2224. https://doi.org/10.3390/ma14092224

Note that from the first issue of 2016, this journal uses article numbers instead of page numbers. See further details here.

Article Metrics

Back to TopTop