PAPER Cite this: RSC Adv., 2015, 5, 22973 Amino-functionalized magnetic magnesium silicate double-shelled hollow microspheres for enhanced removal of lead ions Bingfang Zou, ab Ke Chen, a Yongqiang Wang,* a Chunyu Niu a and Shaomin Zhou a Received 23rd January 2015 Accepted 23rd February 2015 DOI: 10.1039/c5ra01373a www.rsc.org/advances Magnesium silicate hollow microspheres with porous structure were synthesized using silica microspheres as chemical template, which exhibited excellent adsorption properties to heavy metal ions in water in our previous report. Herein, both an iron magnetic core and amino-groups were put forward to functionalize the magnesium silicate hollow microspheres for a fast recoverable and highly efficient absorbent. In the synthesis process, double-shelled hollow microspheres with iron oxide (Fe 3 O 4 ) inner shell and magnesium silicate outer shell (DS-Fe 3 O 4 /MS) were realized via hydrothermal treatment of Fe 3 O 4 @SiO 2 double-shelled hollow microspheres in ammonia solution containing magnesium ions, and the amino-group was introduced into the porous surface of the magnesium silicate shell by a refluxing method to increase the active adsorption sites. The experimental results show that the amino-functionalized magnetic magnesium silicate double-shelled hollow microspheres (DS-Fe 3 O 4 /MS-AG) exhibited a high adsorption capacity of 315.5 mg g 1, and the high adsorption capacity was proposed to be due to synergic adsorption from the magnesium silicate shell (ionexchange adsorption), surface-modified amino-groups (complexation adsorption) and the carboxyl groups on the inner iron oxide hollow microspheres (electrostatic adsorption). Additionally, the used DS-Fe 3 O 4 /MS-AG hollow microspheres could be easily regenerated through immersing them in a solution containing magnesium ions. 1. Introduction Heavy metal pollutants (such as Pb 2+,Cd 2+ and Hg 2+ ) in aquatic environments have brought a severe threat to public health and ecological systems. 1 Considerable efforts have been made to develop effective treatment techniques for removing heavy metal ions from water; including electrochemical methods, adsorption, chemical coagulation, photo degradation, and biodegradation. 2 Among these methods, adsorption is probably the most common method in practical use, for the adsorbent could be used repeatedly, meanwhile the heavy metal ions could be recovered through a desorption process. Unquestionably, the development of the adsorption technique relies heavily on research progress of adsorbent materials, thus development of heavy metal adsorbents with high adsorption capacity, fast adsorption desorption kinetics, and easy separation and regeneration is in great demand. a Key Laboratory for Special Functional Materials of the Ministry of Education, Henan University, Kaifeng 475004, P. R. China. E-mail: wangyq@henu.edu.cn; Fax: +86 3712 3881358; Tel: +86 3712 3881358 b School of Physics and Electronics, Henan University, Kaifeng 475004, P. R. China Electronic supplementary information (ESI) available: SEM and TEM images of Fe 3 O 4 @MS hollow microspheres; N 2 adsorption desorption isotherm of DS-Fe 3 O 4 /MS and DS-Fe 3 O 4 /MS-AG microspheres. See DOI: 10.1039/c5ra01373a The rapid advance of nanoscience and nanotechnology has brought new opportunities for water treatment. 2 Due to unique physical and chemical properties such as large speci c surface areas, high adsorption capacity and fast adsorption rate, nanomaterials have shown their tremendous potential for capture of inorganic or organic pollutants in water. Up to now, various kinds of nanomaterials, especially micro/ nanostructured material like metal oxide, 3 5 silicate, 6 10 and surface modi ed mesoporous silica, 11 13 have been focused on as the adsorbents in waste-water treatment, and proven to be promising for environmental remediation. Among them, silicate nanomaterials were attracted many researchers' interest for their stable and environment-friendly features. Our group reported a serial silicate nanomaterial through using silica particles as chemical template, 14 16 like magnesium silicate hollow microspheres assembled by nanosheets, which could be used as excellent and environment-friendly absorbents of heavy metal ions through ions exchange. 16 Although this kind of silicate adsorbent exhibited good adsorption performance, it is very difficult to recycle them due to their dispersive properties, which are o en encountered in other micro/nanostructured absorbents. Therefore, magnetic-based silicate adsorbents have been extensively studied due to their special magnetic properties. These magnetic adsorbents can be easily separated from aqueous systems by an external magnet, then lower This journal is The Royal Society of Chemistry 2015 RSC Adv., 2015, 5, 22973 22979 22973
Paper sonication for 30 min, then a solution of TEOS in ethanol was slowly dropped into the above solution under a mechanical stirrer. A er the reaction was performed for 120 min, the product was collected with a magnet, and washed with ethanol and water for several times. 30 Finally, the product was dried in vacuum for 6 h to obtain the Fe 3 O 4 /SiO 2 microspheres. Scheme 1 The synthesis of amino-functionalized magnetic magnesium silicate double-shelled hollow microspheres. operational costs for absorbent separations and recycling of the adsorbent materials could be easily achieved. 17 19 Moreover, higher adsorption capacity are still required and pursued at all time when using absorbent to remove pollutants. 20 It is well-known that higher speci c surface area means more adsorption active sites, thus absorbents with porous or hierarchical, even hollow structures was continually developed. For example, urchin-like or ower-like iron oxide, especial with hollow interior, were successively synthesized to improve their high speci c surface area as efficient adsorbents. 21 23 However, the speci c surface area couldn't be improved in nitely, thus composite adsorbents were becoming attractive recently, for all the compositions could contribute to the adsorption of pollutants, and this complex structure could also achieved higher adsorption capacity, for example, amino-groups or thiol-groups was o en used to functionalize mesoporous silica materials; 12,24 graphene oxide with carboxyl groups were used to modify other absorbents like iron oxides and silicates for improved adsorption capability. 25 28 Therefore, new structures or composites are still needed to be explored and developed. Here in this paper, a kind of composite adsorbent with magnetic core and amino-modi ed surface was developed as illustrated in Scheme 1. Fe 3 O 4 hollow microspheres coated with silica were used as chemical template, for the silica shell were transformed into porous magnesium shell with high speci c area under hydrothermal treatment, which both exhibited fast magnetic separability and high adsorption capacity. Furthermore, the large speci c surface area of porous magnesium silicate shell was further utilized to be functionalized with amino-groups, which could increase the adsorption sites for higher adsorption capacities. Therefore, the special designed composite structure was expected to both exhibit high adsorption capacity and fast recoverability when used as adsorbent of Pb 2+ ions in wastewater. 2. Experimental section 2.1 Double-shelled Fe 3 O 4 /SiO 2 hollow microspheres The magnetic Fe 3 O 4 hollow microspheres with diameter about 250 nm were prepared through a hydrothermal reaction. 29 The as-obtained Fe 3 O 4 (0.1 g) microspheres were then dispersed in water ammonia ethanol mixture (10 ml/8 ml/180 ml) by 2.2 Double-shelled Fe 3 O 4 /magnesium silicate hollow microspheres (DS-Fe 3 O 4 /MS) The above DS-Fe 3 O 4 /SiO 2 microspheres (0.075 g) were dispersed in 40 ml H 2 O, then MgCl 2 (0.15 g), NH 4 Cl (1.5 g) and NH 3 $H 2 O (1.5 ml) were added into the above solution in turn. The above mixture was sonicated for 30 min, and then was transferred into ate on-lined stainless-steel autoclave (80 ml) and then sealed to heat at 140 C. A er a 12 h reaction period, the autoclave was cooled to room temperature. The precipitate was collected by the help of a magnet, and then dried in vacuum oven for 12 h. 2.3 Double-shelled Fe 3 O 4 /MS hollow microspheres functionalized with amino-group (DS-Fe 3 O 4 /MS-AG) Amino-functionalized double-shelled Fe 3 O 4 /MS hollow microspheres were prepared by surface modi cation of Fe 3 O 4 /MS hollow microspheres using (3-aminopropyl) trimethoxysilane (APTMS). Double-shelled Fe 3 O 4 /MS hollow microspheres (0.05 g), toluene (50 ml) and APTMS (5 ml) were added to a 250 ml three-necked ask. A er the mixture was ultrasonically dispersed for 30 min, it was re uxed at 100 C with continuous stirring for 6 h under a nitrogen ow (30 ml min 1 ). The nal product was collected by the help of a magnet, followed by washing with ethanol several times and drying at 60 C in vacuum oven for 12 h. 2.4 Characterization The products were analyzed by X-ray diffraction (XRD), in a 2q range from 10 to 80, using CuKa radiation (Philips X'pert diffractometer). The morphology of the prepared products was studied by eld emission scanning electron microscopy (FESEM, Sirion 200 FEG) and eld emission transmission electron microscopy (FETEM, JEOL-2010, 200 kv). The powders were dispersed in ethanol using ultrasonic vibration. The samples for microscopy studies were prepared by deposition of dispersions of the powder in ethanol directly on the SEM stubs or holey carbon grid for TEM examination. Infrared (IR) spectra were recorded in the wave numbers ranging from 4000 to 400 cm 1 with a Nicolet model 759 Fourier transform infrared (FT-IR) spectrometer using a KBr wafer. Magnetic measurements were performed with a superconducting quantum interference device (SQUID) magnetometer (Quantum Design, MPMS XL). The surface area of the samples was determined by nitrogen adsorption (Micrometrics ASAP 2020). 2.5 Pb 2+ ions removal experiments Pb(NO 3 ) 2 was used as the source of Pb 2+ ions. Pb 2+ ions solution (20 ml) with different concentrations were rstly prepared, and then the above as-prepared absorbent (20 mg) was added to test 22974 RSC Adv., 2015, 5, 22973 22979 This journal is The Royal Society of Chemistry 2015
Paper the adsorption performance. The mixtures were shaken at a speed of 100 rpm for 6 hours to establish adsorption equilibrium at room temperature, and then the adsorbent was separated from the mixture by a magnet. To determine Pb 2+ ions removal by the adsorbent, the Pb 2+ concentration in the remaining solution was measured by an inductively coupled plasma atomic emission spectrophotometer (ICP-AES). The adsorption rate experiments were carried out inside 100 ml bottle by using DS-Fe 3 O 4 /MS-AG hollow microspheres (50 mg) as adsorbent, and the samples were collected at desired time intervals and separated by a magnet immediately. The Pb 2+ - loaded amino-functionalized Fe 3 O 4 /MS hollow microspheres were regenerated through immersing in magnesium chloride solution for 6 h. A er that, the absorbent was washed with distilled water for cyclic adsorption, and the adsorption process were measured by similar steps. 3. Results and discussion 3.1. Morphology and phase characterizations of Fe 3 O 4, DS- Fe 3 O 4 /MS, DS-Fe 3 O 4 /MS-AG hollow microspheres The superparamagnetic Fe 3 O 4 hollow microspheres were prepared according to our previous report shown in Fig. 1a, the hollow microspheres had a diameter of 250 nm in Fig 1b. These as-prepared Fe 3 O 4 hollow microspheres are highly water dispersible for abundant carboxyl surface groups which made the outer SiO 2 coating easily. As shown in Fig 1b, monodispersed double-shelled Fe 3 O 4 /SiO 2 (DS-Fe 3 O 4 /SiO 2 ) hollow RSC Advances microspheres were synthesized successfully by sol gel method using tetra-ethoxysilane (TEOS) as the silica source, a thick SiO 2 layer about 100 nm could be seen around Fe 3 O 4 hollow microspheres. As marked by the dotted line in Fig. 1b, the hollow structure of magnetic core still could be seen clearly. A er hydrothermal treatment in alkaline solution containing magnesium ions, the SiO 2 shell is gradually dissolved and reacted with Mg 2+ to generated magnesium silicates, then magnetic magnesium silicate double-shelled hollow microspheres (DS-Fe 3 O 4 /MS) were obtained in Fig. 1c. Clear core shell structure were observed from SEM image, and the core was surrounded by lamellae-assembled shell, and the magnesium silicate grew in the form of a lamellar structure which were origin of its talc structure. The thin lamellae wrapped together and formed porous shell which was subsequently functionalized with amino-groups for increasing adsorption sites. A er functionalized with amino-groups, the product (DS-Fe 3 O 4 /MS- AG) show no obviously change seen from Fig. 1d. The DS-Fe 3 O 4 /MS-AG still kept core shell structure with rough shell in Fig. 1e, further magni ed image in Fig. 1f show that the shell kept thin lamella structure. Since the magnesium silicate was transformed from silica shell in the above experiment, thicker magnesium silicate shell could be obtained easily when Fe 3 O 4 / SiO 2 hollow microspheres with thicker silica shell was used, and the corresponding results could be seen in Fig. S1. Powder XRD was used to monitor the phase structure of the products during the synthesis process (Fig. 2). In the XRD pattern of the obtained Fe 3 O 4 sample (curve a), all the diffraction peaks could be easily indexed to the standard Fe 3 O 4 re ection (JCPDS card no.75-1609). Curve b is a typical XRD pattern of the Fe 3 O 4 /SiO 2 hollow microspheres, which show almost all the same features as those shown in curve a. No diffraction peaks corresponding to SiO 2 were observed except the broad peaks around 23, which was due to the fact that the prepared SiO 2 shell is amorphous. In comparison to the XRD patterns of the Fe 3 O 4 hollow microspheres, four additional Fig. 1 (a) SEM image of Fe 3 O 4 hollow microspheres, (b) TEM image of DS-Fe 3 O 4 /SiO 2 hollow microspheres, (c) SEM image of DS-Fe 3 O 4 /MS hollow microspheres and (d) SEM image of DS-Fe 3 O 4 /MS-AG hollow microspheres, (e) and (f) TEM images of DS-Fe 3 O 4 /MS-AG hollow microspheres. Fig. 2 X-ray diffraction (XRD) patterns of (a) Fe 3 O 4 hollow microspheres, (b) DS-Fe 3 O 4 /SiO 2 hollow microspheres, (c) DS-Fe 3 O 4 /MS hollow microspheres and (d) pure magnesium silicate hollow microspheres. This journal is The Royal Society of Chemistry 2015 RSC Adv., 2015, 5, 22973 22979 22975
peaks like (020), (200), (332) and (335) were vaguely observed in curve c as shown by the arrows, which represent the generation of magnesium silicate hydroxide hydrate (Mg 3 Si 4 O 10 (OH) 2, JCPDS no. 03-0174) and can be indexed through careful comparison with pure magnesium silicate in Fig. 2d. 16 Meanwhile no broad peak around 23 was detected, showing the complete transformation of silica layer into magnesium silicate shell around Fe 3 O 4 hollow microspheres. Therefore, the gradual phase changes of the products at all stages proved the successfully synthesis of magnetic magnesium silicate composite material. A er amino-functionalization, the nal products showed a similar XRD pattern with curve c (not shown here), however, it could be identi ed by other techniques like IR spectrum. 3.2. Characterizations of amino-groups functionalized DS- Fe 3 O 4 /MS (DS-Fe 3 O 4 /MS-AG) hollow microspheres The surface area and pore size distribution of DS-Fe 3 O 4 /MS and DS-Fe 3 O 4 /MS-AG hollow microspheres were tested by nitrogen adsorption desorption. As seen in Fig. S2, both curve a and b belong to type IV isotherm with a type H3 hysteresis loop, which indicated the as-obtained product was mesoporous material. For the introduction of magnetic cores, the BET surface area of DS-Fe 3 O 4 /MS hollow microspheres are calculated to be 438 m 2 g 1, which is a little smaller than that (521 m 2 g 1 ) of our previously reported magnesium silicate hollow microspheres. Although they were further functionalized with amino-groups, the nal DS-Fe 3 O 4 /MS-AG hollow microspheres are still as high as 402 m 2 g 1. Such a high surface area is mainly attributed to the hollow structures and porous shell. There is a sharp pore distribution with an average diameter of 3.97 nm in DS-Fe 3 O 4 /MS, which are most likely from the void space of magnesium silicate self-assembly lamellae structures, and the pore became smaller in size with center peak at 3.76 nm which Paper may be ascribed that small amount of silica generated during the surface functionalization. The high surface area and porous structure of the nal DS-Fe 3 O 4 /MS-AG are bene cial for adsorption of heavy metal ions. FTIR spectra of DS-Fe 3 O 4 /MS and DS-Fe 3 O 4 /MS-AG hollow microspheres are further characterized in Fig. 3. For these two samples, most absorption peaks was similar, like the peaks at 1023 cm 1 and 461 cm 1, which could be ascribed to Si O Si bonds. However, two other weak peaks including 2922 cm 1 and 1382 cm 1 associated with the stretching vibration of methylene groups were also observed form curve b, 31 which indirectly proved the APTES was attached onto the surface of DS-Fe 3 O 4 /MS shell. For further verifying the existence of aminogroups, ninhydrin test was used in our experiment. The principle of this test is that once the surface amine group reacts with ninhydrin, the solution will become purple color for the generated purple colored molecules. As shown in the inset of Fig. 3c and d, when ninhydrin were added into the solution contained DS-Fe 3 O 4 /MS hollow microspheres, no color was observed even the product was collected to the side of vial under external magnet. However, a er DS-Fe 3 O 4 /MS-AG hollow microspheres were functionalized with amino-groups, the color of the solution became dark in Fig. 3e, and purple color could be observed clearly a er magnetic attraction, which is the typical color of ninhydrin (Fig. 3f), indicating the existence of amino-groups on the surface of DS-Fe 3 O 4 /MS-AG hollow microspheres. These results directly proved the successful shell functionalization with amino-groups. The magnetic hysteresis loops of three products including Fe 3 O 4, DS-Fe 3 O 4 /MS and DS-Fe 3 O 4 /MS-AG hollow microspheres were characterized in the applied eld sweeping from 20 KOe to 20 KOe in Fig. 4. All of them show superparamagnetic behaviors at room temperature, and the magnetic saturation (M s ) values are 78.0, 10.9, and 8.4 emu g 1 for Fe 3 O 4, DS-Fe 3 O 4 / MS and DS-Fe 3 O 4 /MS-AG hollow microspheres, respectively. Compared to the M s value of Fe 3 O 4, both DS-Fe 3 O 4 /MS and DS- Fe 3 O 4 /MS-AG hollow microspheres are quite lower, which may Fig. 3 IR spectra of DS-Fe 3 O 4 /MS hollow microspheres (a) before and (b) after amino-functionalization, and the color of (c) DS-Fe 3 O 4 /MS hollow microspheres and (e) DS-Fe 3 O 4 /MS-AG hollow microspheres aqueous solution after adding ninhydrin, and the solution color of (d) DS-Fe 3 O 4 /MS hollow microspheres and (f) DS-Fe 3 O 4 /MS-AG hollow microspheres aqueous solution after magnetic collection. Fig. 4 Room temperature magnetization curves of the products (a) Fe 3 O 4 hollow microspheres, (b) DS-Fe 3 O 4 /MS hollow microspheres, and (c) DS-Fe 3 O 4 /MS-AG hollow microspheres. 22976 RSC Adv., 2015,5, 22973 22979 This journal is The Royal Society of Chemistry 2015
Paper RSC Advances be due to the decrease in the density of Fe 3 O 4 in the as-obtained microspheres a er external shell was introduced like magnesium silicate. The M s value of DS-Fe 3 O 4 /MS-AG hollow microspheres was a litter lower than that of DS-Fe 3 O 4 /MS hollow microspheres, which may be ascribed to the formation of small amount of silica during the functionalization of amino-groups. Although the magnetic saturation of DS-Fe 3 O 4 /MS-AG hollow microspheres was low, they still demonstrated high magnetic responsivity and could be completely accumulated to the wall of bottle within 2 min under an external magnetic eld. A er removing the magnet, these magnetic composite microspheres will be redispersed in water again by slight agitation. Such an excellent magnetic property allows them to be separated from solution and redispersed into solution easily in practical application. 3.3 Adsorption performance tests of DS-Fe 3 O 4 /MS-AG hollow microspheres Amino-groups were commonly used to functionalize mesoporous silica materials and demonstrated outstanding ability to remove a wide variety of heavy metal ions such as Cu(II), Pb(II), and Cd(II) from aqueous solutions owing to the strong metal complex capability of amino-groups. 31 35 Here the porous shell of the as-obtained Fe 3 O 4 /MS hollow microspheres, which showed large speci c surface area, were fully utilized in our experiment and functionalized with the amino-groups to increase the adsorptive sites. In the as-obtained DS-Fe 3 O 4 /MS-AG hollow microspheres, on the one hand, metal ions like Pb 2+ could enter into the skeleton of material through ion-exchange silicate materials which were reported by many researchers and our group. On the other hand, a er functionalized with amino-groups, the porous shell was fully utilized, and the adsorption sites were increased. Besides, the carboxyl groups from the PAAS attached on the Fe 3 O 4 hollow microsphere also contributed to the adsorption performance. Thus, there are three kinds of adsorption active sites in the as-prepared DS-Fe 3 O 4 /MS-AG hollow microspheres including ion-exchange adsorption, complexation adsorption and electrostatic adsorption. The detailed relationship between the removal ability and the concentration of the lead ions solution was rstly illustrated by an adsorption isotherm. The Fig. 5 shows the adsorption isotherm of lead ions for the as-prepared DS-Fe 3 O 4 /MS-AG hollow microspheres. The Langmuir and Freundlich isotherm models are applied to simulate lead ions adsorption. The Langmuir model is expressed as: Q e ¼ bq m C e /(1 + bc e ) (1) The Freundlich isotherm model can be expressed by the following formula: Q e ¼ kc e 1/n (2) where C e is the equilibrium concentration of lead ions in the supernatant (mg L 1 ); Q e is the amount of lead ions adsorbed on per weight of absorbent (mg g 1 ) a er adsorption Fig. 5 The Pb 2+ adsorption isotherm of DS-Fe 3 O 4 /MS-AG hollow microspheres. (The inset was the C e /Q e versus C e plot.) equilibrium; Q m represents the maximum adsorption capacity of lead ions on per weight of absorbent (mg g 1 ); and b is the Langmuir adsorption constant (L mg 1 ). The Freundlich constant k is correlated to the relative adsorption capacity of the adsorbent (mg g 1 ), and 1/n is the adsorption intensity. The experimental data were simulated with the Langmuir and Freundlich isotherm models respectively. The relative parameters calculated from the two models were listed in Table S1, where the correlation coefficient of the Langmuir model (R 2 ¼ 0.99) was higher than that of the Freundlich model (R 2 ¼ 0.78), indicating that the adsorption data are better tted by the Langmuir model. The calculated values of Q m are 315.5 mg g 1 for DS-Fe 3 O 4 /MS-AG hollow microspheres. Obviously, the asobtained magnetic composite silicate microsphere was much higher than many other reported magnetic nanomaterials like metal oxides, mesoporous silica and carbonaceous materials. 22,32,36,37 To investigate the origin of the adsorption sites in DS-Fe 3 O 4 /MS-AG hollow microspheres, the synthesized Fe 3 O 4, and DS-Fe 3 O 4 /MS hollow microspheres in our experiment were further tested as absorbent of Pb 2+ as shown in Fig. S3. Firstly, the adsorption capacity was calculated to be 261.8 mg g 1 for DS-Fe 3 O 4 /MS hollow microspheres in Fig. S3a, thus there was a differential value about 53.7 mg g 1 in adsorption capacities between DS-Fe 3 O 4 /MS and DS-Fe 3 O 4 /MS-AG hollow microspheres, which could be attributed to the surface modi ed amino-groups on DS-Fe 3 O 4 /MS hollow microspheres. Secondly, as for the DS-Fe 3 O 4 /MS hollow microspheres, the mass percentage of magnesium silicate shell could be roughly estimated to be 86% according to the M s values including Fe 3 O 4 and DS-Fe 3 O 4 /MS hollow microspheres in Fig. 4, and then the adsorption value of magnesium silicate shell could be calculated to be 258 mg g 1 (Q m of pure magnesium silicate was about 300 mg g 1 in our previous report 16 ). Therefore the differential value in adsorption capacities between DS-Fe 3 O 4 / MS and magnesium silicate shell was about 3.8 mg g 1, which may be ascribed to the adsorption sites of magnetic core, considering that the adsorption capacity of the polyacrylate modi ed Fe 3 O 4 hollow microspheres was about 24.6 mg g 1 in This journal is The Royal Society of Chemistry 2015 RSC Adv., 2015, 5, 22973 22979 22977
Paper Fig. S3b. Based on the above analysis, in the as-obtained DS- Fe 3 O 4 /MS-AG hollow microspheres, there are three kinds of adsorption sites including magnesium silicate shell, surface modi ed amino-groups and the surface attached carboxyl groups in Fe 3 O 4 hollow microspheres, 29 therefore the high adsorption capacity was proposed to be synergic adsorption from the magnesium silicate shell (ion-exchange adsorption), 17 surface-modi ed amino-groups (complexation adsorption) 31 and the surface attached carboxyl groups on Fe 3 O 4 hollow microspheres (electrostatic adsorption). 29 The rate of removal process was an important consideration for industrial water treatment, which directly in uenced the efficiency. During the experiment, the as-prepared DS-Fe 3 O 4 / MS-AG hollow microspheres (50 mg) were used as adsorbent, and added into the Pb 2+ solution (50 ml) with concentration (200 mg L 1 ). As shown in Fig. 6, there are two different stages in the Pb 2+ removal process. At initial stage, the DS-Fe 3 O 4 /MS- AG hollow microspheres demonstrated a fast removal performance, and nearly 70% of Pb 2+ ions were removed in 5 minutes. However, the removal rate of Pb 2+ ions became slow in the following stage, and the adsorption equilibrium was gradually established a er almost 6 h. This kind of adsorption process could be proposed that the initial fast removal was attributed to ions exchange at the absorbent surface layer, and the aminogroups complexation with Pb 2+ ions on the surface was also included. The ions exchange took place quickly for two reasons, one is that the Pb 2+ ions could contact with large surface area of adsorbent, the other is the absorbent was assembled by a lot of nanoscaled and active lamella. A er the Mg 2+ ions in the surface layer were exchanged with Pb 2+ ions, the subsequent ions exchange became slowly. The reason may be that the new adsorption sites would only be provided through the slow diffusion and exchange with Mg 2+ ions in the interior of the absorbent, thus the Pb 2+ removal from water became slow. Although the adsorption equilibrium needed a relative long time, most of Pb 2+ ions could be removed in only 60 min. A large adsorption capacity and rapid uptake rate signi es the Fig. 7 (a) The schematic recycling process of DS-Fe 3 O 4 /MS-AG hollow microspheres and (b) the adsorption efficiency of Pb 2+ at different cycles. advantages of DS-Fe 3 O 4 /MS-AG hollow microspheres as an adsorbent of Pb 2+ ions in water treatment. Obviously, in our experiment, the obtained product could be easily recovered by external magnet, which improve the efficiency signi cantly in the recovery process. It was also found that the adsorbent could be used as absorbent of Pb 2+ ions again a er the following ion exchange in Mg 2+ solution with high concentration, thus the DS-Fe 3 O 4 /MS-AG hollow microspheres could be regenerated through post-treatment as shown in Fig. 7a. Since the reusability of absorbents related closely to the cost, the adsorption desorption cycles was further investigated. As shown in Fig. 7b, the adsorption capacity of the regenerated absorbent decreased, but the DS-Fe 3 O 4 /MS-AG hollow microspheres still demonstrated over 85% of the initial value a er six cycles. We proposed that the decrease of adsorption capacity may come from two aspects, one is that the residual Pb 2+ in the adsorbent increased gradually which is difficult to be replaced by Mg 2+ again, and the other is the lamella structure of adsorbent maybe collapse during the multistep ions exchange process. 14 Additionally, it was noticed that magnesium ions would be continually released in the treated water in every recycling adsorption process according to the ion exchange mechanism, however, magnesium ions are a common ion in drinking water, and the safe concentration of magnesium ions is far too higher than the concentration of lead. 17 Based on the results above, the as-prepared DS-Fe 3 O 4 / MS-AG hollow microspheres exhibit excellent adsorption performance, and are also safe and environment-friendly, thus they could be used as a prospective magnetically recoverable adsorbent. 4. Conclusions Fig. 6 Relationship between the residual concentration of Pb 2+ (C t )at different time during the adsorption process. The magnetic separable DS-Fe 3 O 4 /MS-AG hollow microspheres were facile synthesized as high efficient absorbent of Pb 2+ ions by hydrothermal method. The introduction of iron magnetic core made the absorbent fast recoverable, and amino-group 22978 RSC Adv., 2015, 5, 22973 22979 This journal is The Royal Society of Chemistry 2015
Paper surface modi cation increased the active adsorption sites for higher adsorption efficiency. The experimental results show that the amino-functionalized magnetic magnesium silicate double-shelled hollow microspheres (DS-Fe 3 O 4 /MS-AG) exhibited high adsorption capacity with 315.5 mg g 1, and the high adsorption capacity were proposed to be synergic adsorption from the magnesium silicate shell (ion-exchange adsorption), surface-modi ed amino-groups (complexation adsorption) and the surface attached carboxyl groups on Fe 3 O 4 hollow microspheres (electrostatic adsorption). Acknowledgements This work was supported by the Natural Science Foundation of China (no. 51102077, no. 51372070 and no. 21203055), the Excellent Youth Scienti c Research Foundation of Henan University (0000A40409) and Changjiang Scholars and Innovative Research Team in University (no. PCS IRT1126). Notes and references 1 C. J. Vorosmarty, P. B. McIntyre, M. O. Gessner, D. Dudgeon, A. Prusevich, P. Green, S. Glidden, S. E. Bunn, C. A. Sullivan, C. R. Liermann and P. M. Davies, Nature, 2010, 467, 555. 2 L. Zhang and M. Fang, Nano Today, 2010, 5, 128. 3 Y. Wang, G. Wang, H. Wang, W. Cai, C. Liang and L. Zhang, Nanotechnology, 2009, 20, 155604. 4 X. Wang, W. Cai, Y. Lin, G. Wang and C. Liang, J. Mater. Chem., 2010, 20, 8582. 5 G. Liu, Q. Deng, H. Wang, S. Kang, Y. Yang, D. H. Ng, W. Cai and G. Wang, Chem. Eur. J., 2012, 18, 13418. 6 J. Qu, C. Cao, Y. Hong, C. Chen, P. Zhu, W. Song and Z. Wu, J. Mater. Chem., 2012, 22, 3562. 7 R. Jin, Y. Yang, Y. Xing, L. Chen, S. Song and R. Jin, ACS Nano, 2014, 8, 3664. 8 Y. Zhuang, Y. Yang, G. Xiang and X. Wang, J. Phys. Chem. C, 2009, 113, 10441. 9 J. Qu, W. Li, C. Cao, X. Yin, L. Zhao, J. Bai, Z. Qin and W. Song, J. Mater. Chem., 2012, 22, 17222. 10 J. Zheng, B. H. Wu, Z. Y. Jiang, Q. Kuang, X. L. Fang, Z. X. Xie, R. B. Huang and L. S. Zheng, Chem. Asian J., 2010, 5, 1439. 11 A. Walcarius and L. Mercier, J. Mater. Chem., 2010, 20, 4478. 12 L. Mercier and T. J. Pinnavaia, Adv. Mater., 1997, 9, 500. 13 J. Dong, Z. H. Xu and F. Wang, Appl. Surf. Sci., 2008, 254, 3522. RSC Advances 14 Y. Q. Wang, C. J. Tang, Q. A. Deng, C. H. Liang, D. Ng, F. L. Kwong, H. Q. Wang, W. P. Cai, L. D. Zhang and G. Z. Wang, Langmuir, 2010, 26, 14830. 15 Y. Q. Wang, G. Z. Wang, H. Q. Wang, W. P. Cai and L. D. Zhang, Chem. Commun., 2008, 6555. 16 Y. Q. Wang, G. Z. Wang, H. Q. Wang, C. H. Liang, W. P. Cai and L. D. Zhang, Chem. Eur. J., 2010, 16, 3497. 17 C. Cao, F. Wei, J. Qu and W. Song, Chem. Eur. J., 2013, 19, 1558. 18 S. Zhang, W. Xu, M. Zeng, J. Li, J. Li, J. Xu and X. Wang, J. Mater. Chem. A, 2013, 1, 11691. 19 Q. Ou, L. Zhou, S. Zhao, H. Geng, J. Hao, Y. Xu, H. Chen and X. Chen, Chem. Eng. J., 2012, 180, 121. 20 J. Hu, L. Zhong, W. Song and L. Wan, Adv. Mater., 2008, 20, 2977. 21 Y. F. Lin and J. L. Chen, RSC Adv., 2013, 3, 15344. 22 B. Wang, H. Wu, L. Yu, R. Xu, T. Lim and X. W. Lou, Adv. Mater., 2012, 24, 1111. 23 F. Mou, J. Guan, Z. Xiao, Z. Sun, W. Shi and X. Fan, J. Mater. Chem., 2011, 21, 5414. 24 X. Feng, G. E. Fryxell, L. Q. Wang, A. Y. Kim, J. Liu and K. M. Kemner, Science, 1997, 276, 923. 25 C. Gui, Q. Wang, S. Hao, J. Qu, P. Huang, C. Cao, W. Song and Z. Yu, ACS Appl. Mater. Interfaces, 2014, 6, 14653. 26 Y. Jung, H. I. Lee, J. H. Kim, M. H. Yun, J. Hwang, D. H. Ahn, J. N. Park, J. H. Boo, K. S. Choi and J. M. Kim, J. Mater. Chem., 2010, 20, 4663. 27 X. Wu, L. Wang, C. Chen, A. Xu and X. Wang, J. Mater. Chem., 2011, 21, 17353. 28 Y. Lin, W. Cai, X. Tian, X. Liu, G. Wang and C. Liang, J. Mater. Chem., 2011, 21, 991. 29 B. Zou, Y. Liu and Y. Wang, RSC Adv., 2013, 3, 23327. 30 Y. Q. Wang, K. Wang, B. F. Zou, T. Gao, X. L. Zhang, Z. L. Du and S. M. Zhou, J. Mater. Chem. C, 2013, 1, 2441. 31 J. Wang, S. Zheng, Y. Shao, J. Liu, Z. Xu and D. Zhu, J. Colloid Interface Sci., 2010, 349, 293. 32 I. F. Nata, G. W. Salim and C. K. Lee, J. Hazard. Mater., 2010, 183, 853. 33 H. S. Li, X. Y. Miao, Y. X. Hao, H. Y. Zhao, X. Y. Sun and L. J. Wang, J. Colloid Interface Sci., 2008, 318, 309. 34 Y. Hao, C. Man and Z. Hu, J. Hazard. Mater., 2010, 184, 392. 35 S. Huang and D. Chen, J. Hazard. Mater., 2009, 163, 174. 36 H. Wang, Q. Chen, J. Chen, B. Yu and X. Hu, Nanoscale, 2011, 3, 4600. 37 I. F. Nata, G. W. Salim and C. K. Lee, J. Hazard. Mater., 2010, 183, 853. This journal is The Royal Society of Chemistry 2015 RSC Adv., 2015, 5, 22973 22979 22979