Modification and Characterization of Fe3O4 Nanoparticles for Use in Adsorption of Alkaloids

Magnetite (Fe3O4) is a ferromagnetic iron oxide of both Fe(II) and Fe(III), prepared by FeCl2 and FeCl3. XRD was used for the confirmation of Fe3O4. Via the modification of Tetraethyl orthosilicate (TEOS), (3-Aminopropyl)trimethoxysilane (APTMS), and Alginate (AA), Fe3O4@SiO2, Fe3O4@SiO2-NH2, and Fe3O4@SiO2-NH2-AA nanoparticles could be obtained, and IR and SEM were used for the characterizations. Alkaloid adsorption experiments exhibited that, as for Palmatine and Berberine, the most adsorption could be obtained at pH 8 when the adsorption time was 6 min. The adsorption percentage of Palmatine was 22.2%, and the adsorption percentage of Berberine was 23.6% at pH 8. Considering the effect of adsorption time on liquid phase system, the adsorption conditions of 8 min has been chosen when pH 7 was used. The adsorption percentage of Palmatine was 8.67%, and the adsorption percentage of Berberine was 7.25%. Considering the above conditions, pH 8 and the adsorption time of 8min could be chosen for further uses.


Introduction
Although there are many pure phases of iron oxide in nature, the most popular magnetic nanoparticles (MNPs) are the nanoscale zero-valent iron (nZVI), Fe 3 O 4 and γ-Fe 2 O 3 . Magnetite (Fe 3 O 4 ) is a ferromagnetic black color iron oxide of both Fe(II) and Fe(III), which has been the most extensively studied [1]. In 2001, Asher reported co-precipitation method using oleic acid as the surface modification agent to obtain Fe 3 O 4 nanoparticles (2-15 nm) [2]. NaOH and diethylene glycol could also be used as the catalyst and reducing agent to fabricate Fe 3 O 4 nanoparticles of 80-180 nm in size [3][4][5]. However, Fe 3 O 4 nanoparticles could easily aggregate due to the nanoscale effect and magnetic gravitational effect. It is an effective method of preventing the aggregate of these nanoparticles to wrap the surface of Fe 3 O 4 nanoparticles. Fe 3 O 4 @SiO 2 composite nanoparticles have the desirable properties of magnetic nanoparticles while also benefiting from the SiO 2 shell, such as good hydrophilicity, stability, and biocompatibility [6][7][8]. In 2016, Tang reported that (3-aminopropyl)-triethoxysilane (APTES) was used as surface modification reagents to get Fe 3 O 4 @SiO 2 -NH 2 , which could be used for selective removal of Zn(II) ions from wastewater [9]. While Fe 3 O 4 @SiO 2 -NH 2 nanoparticles could also be modified to obtain mercaptoamine-functionalised silica-coated magnetic nanoparticles for the removal of mercury and lead ions from wastewater [10]. As for the removal of ions, arsenate removal could be achieved by calcium alginate-encapsulated magnetic sorbent, which was prepared by physical method [11]. Superparamagnetic sodium alginate-coated Fe 3  Alg-Fe 3 O 4 nanoparticles were synthesized using in situ coprecipitation of FeCl 2 and FeCl 3 in alkaline solution in the presence of sodium alginate [12]. While multifunctional alginate microspheres could also be used for biosensing, drug delivery, and magnetic resonance imaging [13]. To obtain the good biocompatibility, Fe 3 O 4 nanoparticles need to be modified. Fe 3 O 4 @SiO 2 composite nanoparticles have the desirable properties of good hydrophilicity. (3-Aminopropyl)trimethoxysilane (APTMS) was used as surface modification reagents to get Fe 3 O 4 @SiO 2 -NH 2 nanoparticles. While calcium alginate-encapsulated magnetic sorbent could be prepared by physical method. Superparamagnetic sodium alginate-coated Fe 3 O 4 nanoparticles (Alg-Fe 3 O 4 ) could also be synthesized using in situ coprecipitation of FeCl 2 and FeCl 3 in alkaline solution in the presence of sodium alginate. Covalent modification methods via alginate have been rarely seen. In order to investigate the effects of the covalent alginate-modified method, alkaloid adsorption experiments were designed to study the properties of alginate-modified Fe 3 O 4 @SiO 2 -NH 2 nanoparticles.
XPS spectra were recorded using a Kratos Axis Ultra DLD spectrometer (KAI MEIKE CHEMICAL Co., Ltd.) employing a monochromated Al-Kα X-ray source (hv = 1486.6 eV). The vacuum in the main chamber was kept above 3 × 10 −6 Pa during XPS data acquisitions. General survey scans (binding energy range: 0-1200 eV; pass energy: 160 eV) and high-resolution spectra (pass energy: 40 eV) in the regions of N1s were recorded. Binding energies were referenced to the C1s binding energy at 284.60 eV.
The adsorption data were obtained by RP-HPLC (Reversed phase high performance liquid chromatography). The HPLC system was from Agilent Technologies 1260 Infinity (Agilent Technologies, SantaClara, CA, USA), and was equipped with a quaternary pump and UV-Vis detector (Agilent Technologies). The chromatographic separation was carried out on an ACE Super C18 column (250 × 4.6 mm i.d., 5 µm, FLM, Guangzhou, China). Mobile phase consisted of 50% solution (v/v) of acetonitrile in water (0.1% H 3 PO 4 and 0.1% SDS). The flow rate was 1 mL/min and the column temperature was set to 40 • C. The effluent was monitored at 265 nm and the injection volume was 20 µL.

Preparation of Fe 3 O 4 Nanoparticles
Briefly, 7.5 mL of 0.12 M FeCl 2 and 7.5 mL of 0.2 M FeCl 3 solutions were mixed in a 100-mL flask. The whole reaction system was completed under nitrogen protection. After the magnetic stirring was uniform, the reaction system was heated to 55 • C, which maintained for 15 min. 7.2 mL of 3 M NaOH solution was then added to the reaction system. The reaction system was kept at 55 • C for 40 min. Then the reaction system was stirred at 90 • C for 30 min and cooled to room temperature. The black precipitate was collected by magnetic decantation and washed with deionized water repeatedly until the washings were neutral. The obtained black precipitate was then dried over vacuum at 40 • C overnight, which could be used for XRD measurement [14,15].

Preparation of Fe 3 O 4 @SiO 2
Fe 3 O 4 (10 mg) was acidized by HCl (0.1 mol/L) under the 100 W of ultrasound for 20 min. The supernatant was discarded after adsorption by the magnet. The residue was washed with ultrapure water for twice, and resuspended in ethanol/ultrapure water (20 mL:5 mL). NH 3 ·H 2 O (250 µL) was added to the samples of Fe 3 O 4 , and the mixture was reacted for 20 min under the 100 W of ultrasound. TEOS (32 µL) was added into the samples. And then the samples were oscillated at 37 • C and 140 r/min for 6 h, followed by adsorption by the magnet. The supernatant was discarded, and the residue was washed with ethanol for twice to yield Fe 3 O 4 @SiO 2 , which was resuspended in ethanol (4 mL) [ An AA solution (5 mg/mL in MES buffer, pH 6.0) was mixed with N,N-dimethylformamide (DMF; 3:1, v/v). Then the AA solution (3.75 mg/mL) was converted to N-hydroxysuccinimide esters by sequential reaction with EDC (36.3 mg/mL in MES buffer, pH 6.0) for 15 min and NHS (10.95 mg/mL in MES buffer, pH 6.0) for 60 min. The solution was finally introduced to the freshly Fe 3 O 4 @SiO 2 -NH 2 nanoparticles and reacted overnight at room temperature. After washing by ethanol, the samples of Fe 3 O 4 @SiO 2 -NH 2 -AA could be obtained by vacuum-dried process [18]. 2018, 23,xFOR PEER 3 of 10 solution was then added to the reaction system. The reaction system was kept at 55 °C for 40 min. Then the reaction system was stirred at 90 °C for 30 min and cooled to room temperature. The black precipitate was collected by magnetic decantation and washed with deionized water repeatedly until the washings were neutral. The obtained black precipitate was then dried over vacuum at 40 °C overnight, which could be used for XRD measurement [14,15].

Preparation of Fe3O4@SiO2
Fe3O4 (10 mg) was acidized by HCl (0.1 mol/L) under the 100 W of ultrasound for 20 min. The supernatant was discarded after adsorption by the magnet. The residue was washed with ultrapure water for twice, and resuspended in ethanol/ultrapure water (20 mL:5 mL). NH3H2O (250 μL) was added to the samples of Fe3O4, and the mixture was reacted for 20 min under the 100 W of ultrasound. TEOS (32 μL) was added into the samples. And then the samples were oscillated at 37 °C and 140 r/min for 6 h, followed by adsorption by the magnet. The supernatant was discarded, and the residue was washed with ethanol for twice to yield Fe3O4@SiO2, which was resuspended in ethanol (4 mL) [16].

Preparation of Fe3O4@SiO2-NH2
APTMS (50 μL) was dropwise added to the samples of Fe3O4@SiO2 obtained previously, and the mixture was reacted for 24 h. After rinsing with ethanol for twice, the samples named as Fe3O4@SiO2-NH2 were vacuum-dried at 80 °C overnight [17].

Preparation of Fe3O4@SiO2-NH2-AA
An AA solution (5 mg/mL in MES buffer, pH 6.0) was mixed with N,N-dimethylformamide (DMF; 3:1, v/v). Then the AA solution (3.75 mg/mL) was converted to N-hydroxysuccinimide esters by sequential reaction with EDC (36.3 mg/mL in MES buffer, pH 6.0) for 15 min and NHS (10.95 mg/mL in MES buffer, pH 6.0) for 60 min. The solution was finally introduced to the freshly Fe3O4@SiO2-NH2 nanoparticles and reacted overnight at room temperature. After washing by ethanol, the samples of Fe3O4@SiO2-NH2-AA could be obtained by vacuum-dried process [18].

Influence from pH
Approximate 8 mL of mixed standard stock solution (0.5 μg/mL, in methanol, pH 5, 6,7,8,9), 10 mg of Fe3O4@SiO2-NH2-AA nanoparticles was ultrasonic shocked for 6 min, and then the supernatant and magnetic nanoparticles were obtained by magnetic separation. The magnetic

Influence from pH
Approximate 8 mL of mixed standard stock solution (0.5 µg/mL, in methanol, pH 5, 6,7,8,9), 10 mg of Fe 3 O 4 @SiO 2 -NH 2 -AA nanoparticles was ultrasonic shocked for 6 min, and then the supernatant and magnetic nanoparticles were obtained by magnetic separation. The magnetic nanoparticles were washed by deionized water (1 mL × 2). The supernatant and detergent were combined. 1.5 mL of the mixture was dried by nitrogen blower at 80 • C. The residue was redissolved in 400 µL of methanol, which was filtered (0.22 µm) for subsequent HPLC analysis.

Influence from Adsorption Time
Approximate 8 mL of mixed standard stock solution (0.5 µg/mL, in methanol), 10 mg of Fe 3 O 4 @SiO 2 -NH 2 -AA nanoparticles was ultrasonic shocked for a certain time (2 min, 4 min, 6 min, 8 min, 10 min), and then the supernatant and magnetic particles were obtained by magnetic separation. The magnetic nanoparticles were washed by deionized water (1 mL × 2). The supernatant and detergent were combined. The mixture was dried by nitrogen blower at 80 • C. The residue was redissolved in 400 µL of methanol, which was filtered (0.22 µm) for subsequent HPLC analysis [19][20][21].

XRD Analysis of Fe 3 O 4 Nanoparticles
The XRD pattern of nanoparticles were washed by deionized water (1 mL × 2). The supernatant and detergent were combined. 1.5 mL of the mixture was dried by nitrogen blower at 80 °C. The residue was redissolved in 400 μL of methanol, which was filtered (0.22 μm) for subsequent HPLC analysis.

Influence from Adsorption Time
Approximate 8 mL of mixed standard stock solution (0.5 μg/mL, in methanol), 10 mg of Fe3O4@SiO2-NH2-AA nanoparticles was ultrasonic shocked for a certain time (2 min, 4 min, 6 min, 8 min, 10 min), and then the supernatant and magnetic particles were obtained by magnetic separation. The magnetic nanoparticles were washed by deionized water (1 mL × 2). The supernatant and detergent were combined. The mixture was dried by nitrogen blower at 80 °C. The residue was redissolved in 400 μL of methanol, which was filtered (0.22 μm) for subsequent HPLC analysis [19][20][21].

XRD Analysis of Fe3O4 Nanoparticles
The XRD pattern of Fe3O4 nanoparticles is shown in the

FTIR Spectra Analysis of Nanoparticles
The Fe3O4@SiO2-NH2 and Fe3O4@SiO2-NH2-AA nanoparticles were obtained after the surface modification steps. It is apparent that the IR spectra contains not only the peaks in spectra of Fe3O4 nanoparticles (Fe-O, 567 cm −1 ) [15]. 1560 cm −1 (C-N vibration) reflected that APTMS was successfully modified onto Fe3O4@SiO2nanoparticles [22]. A strong IR peak appears at 1648 cm −1 , corresponding to the strong bending vibration of the amide I group, which showed that the modification was successful and Fe3O4@SiO2-NH2nanoparticles were indeed coated with AA ( Figure 3) [17,23,24].

FTIR Spectra Analysis of Nanoparticles
The Fe 3 O 4 @SiO 2 -NH 2 and Fe 3 O 4 @SiO 2 -NH 2 -AA nanoparticles were obtained after the surface modification steps. It is apparent that the IR spectra contains not only the peaks in spectra of Fe 3 O 4 nanoparticles (Fe-O, 567 cm −1 ) [15]. 1560 cm −1 (C-N vibration) reflected that APTMS was successfully modified onto Fe 3 O 4 @SiO 2 nanoparticles [22]. A strong IR peak appears at 1648 cm −1 , corresponding to the strong bending vibration of the amide I group, which showed that the modification was successful and Fe 3 O 4 @SiO 2 -NH 2 nanoparticles were indeed coated with AA ( Figure 3) [17,23,24].  (Figure 4c), which showed that amide reaction was successful [25].  (Figure 4c), which showed that amide reaction was successful [25].

SEM Analysis of Nanoparticles
Figure 5a-c show SEM images of Fe3O4, Fe3O4@SiO2-NH2, and Fe3O4@SiO2-NH2-AA nanoparticles. Small particle size of Fe3O4 particles is obvious, while a good dispersion effect could be achieved by Fe3O4@SiO2-NH2 nanoparticles. As for Fe3O4@SiO2-NH2-AA nanoparticles, no good dispersion could be achieved, while better morphology could be achieved, which showed that AA was successfully modified onto Fe3O4@SiO2-NH2 nanoparticles [22]. Almost all particle size of Fe3O4 particlesis below 100 nm, as for Fe3O4@SiO2-NH2 nanoparticles and Fe3O4@SiO2-NH2-AA nanoparticles, particle size is becoming larger and larger, which could also prove that the modification is successful.  (Figure 4c), which showed that amide reaction was successful [25].

SEM Analysis of Nanoparticles
Figure 5a-c show SEM images of Fe3O4, Fe3O4@SiO2-NH2, and Fe3O4@SiO2-NH2-AA nanoparticles. Small particle size of Fe3O4 particles is obvious, while a good dispersion effect could be achieved by Fe3O4@SiO2-NH2 nanoparticles. As for Fe3O4@SiO2-NH2-AA nanoparticles, no good dispersion could be achieved, while better morphology could be achieved, which showed that AA was successfully modified onto Fe3O4@SiO2-NH2 nanoparticles [22]. Almost all particle size of Fe3O4 particlesis below 100 nm, as for Fe3O4@SiO2-NH2 nanoparticles and Fe3O4@SiO2-NH2-AA nanoparticles, particle size is becoming larger and larger, which could also prove that the modification is successful.  @SiO 2 -NH 2 -AA nanoparticles. Small particle size of Fe 3 O 4 particles is obvious, while a good dispersion effect could be achieved by Fe 3 O 4 @SiO 2 -NH 2 nanoparticles. As for Fe 3 O 4 @SiO 2 -NH 2 -AA nanoparticles, no good dispersion could be achieved, while better morphology could be achieved, which showed that AA was successfully modified onto Fe 3 O 4 @SiO 2 -NH 2 nanoparticles [22]. Almost all particle size of Fe 3 O 4 particlesis below 100 nm, as for Fe 3 O 4 @SiO 2 -NH 2 nanoparticles and Fe 3 O 4 @SiO 2 -NH 2 -AA nanoparticles, particle size is becoming larger and larger, which could also prove that the modification is successful.

Analysis of Alkaloid Adsorption Test
Electrostatic interactions between alkaloids and charged surfaces, therefore, often play a major role in the adsorption behavior of alkaloids. Therefore, Palmatine and Berberine were selected for alkaloid adsorption assay in the current study. Figure 6a is the chromatogram associated with the concentrations of the standard curve, which belongs to Palmatine. Figure 6b is the chromatogram associated with the concentrations of the standard curve, which belongs to Berberine. The Equation process is as follows: (2) V0 = 10 mL, V1 = 1.5 mL, V2 = 0.4 mL, m is the capacity of alkaloid in the supernatant and detergent, C is the concentration of the supernatant and detergent, which could be obtained by the standard curve. C0 = 0.5 μg/mL, V = 8 mL, Ap is the adsorption percentage of alkaloid. From Table S1, as for Palmatine and Berberine, the most adsorption could be obtained at pH 8. Considering the effect of alkaline on liquid phase system, the adsorption conditions of pH 8 has been chosen. The adsorption percentage of Palmatine was 22.2%, and the adsorption percentage of Berberine was 23.6%. At pH 8, the carboxylic acid of Fe3O4@SiO2-NH2-AA nanoparticles was

Analysis of Alkaloid Adsorption Test
Electrostatic interactions between alkaloids and charged surfaces, therefore, often play a major role in the adsorption behavior of alkaloids. Therefore, Palmatine and Berberine were selected for alkaloid adsorption assay in the current study. Figure 6a is the chromatogram associated with the concentrations of the standard curve, which belongs to Palmatine. Figure 6b is the chromatogram associated with the concentrations of the standard curve, which belongs to Berberine. The Equation process is as follows: V 0 = 10 mL, V 1 = 1.5 mL, V 2 = 0.4 mL, m is the capacity of alkaloid in the supernatant and detergent, C is the concentration of the supernatant and detergent, which could be obtained by the standard curve.
C 0 = 0.5 µg/mL, V = 8 mL, Ap is the adsorption percentage of alkaloid. From Table S1, as for Palmatine and Berberine, the most adsorption could be obtained at pH 8. Considering the effect of alkaline on liquid phase system, the adsorption conditions of pH 8 has been chosen. The adsorption percentage of Palmatine was 22.2%, and the adsorption percentage of Berberine was 23.6%. At pH 8, the carboxylic acid of Fe 3 O 4 @SiO 2 -NH 2 -AA nanoparticles was converted to a negatively-charged carboxylate ion. Therefore, quaternary ammonium alkaloids were Molecules 2018, 23, 562 7 of 10 significantly adsorbed onto the carboxylic acid-rich surface, possibly due to electrostatic interactions. The results from this study seem to fit well with a previous report on the study of the charge interaction of alkaloids and polyelectrolyte films.
From Table S2, as for Berberine, the most adsorption could be obtained at 8 min. While the most adsorption could be obtained at 10 min for Palmatine. Considering the effect of adsorption time on liquid phase system, the adsorption conditions of 8 min has been chosen. The adsorption percentage of Palmatine was 8.67%, and the adsorption percentage of Berberine was 7.25%.
The effect of pH was greater than that of adsorption time. Considering the above conditions, pH 8 and the adsorption time of 8 min could be chosen for further uses. 2018, 23,xFOR PEER 7 of 10 converted to a negatively-charged carboxylate ion. Therefore, quaternary ammonium alkaloids were significantly adsorbed onto the carboxylic acid-rich surface, possibly due to electrostatic interactions. The results from this study seem to fit well with a previous report on the study of the charge interaction of alkaloids and polyelectrolyte films. From Table S2, as for Berberine, the most adsorption could be obtained at 8 min. While the most adsorption could be obtained at 10 min for Palmatine. Considering the effect of adsorption time on liquid phase system, the adsorption conditions of 8 min has been chosen. The adsorption percentage of Palmatine was 8.67%, and the adsorption percentage of Berberine was 7.25%.
The effect of pH was greater than that of adsorption time. Considering the above conditions, pH 8 and the adsorption time of 8 min could be chosen for further uses.

Conclusions
In conclusion, magnetite (Fe3O4) could be prepared by FeCl2 and FeCl3, which is a ferromagnetic black color iron oxide of both Fe(II) and Fe(III). XRD was used for the determination of

Conclusions
In conclusion, magnetite (Fe 3 O 4 ) could be prepared by FeCl 2 and FeCl 3 , which is a ferromagnetic black color iron oxide of both Fe(II) and Fe(III). XRD was used for the determination of be used for modification at the subsequent trials. Fe 3 O 4 @SiO 2 nanoparticles were successfully obtained by TEOS. Fe 3 O 4 @SiO 2 -NH 2 nanoparticles were prepared by APTMS, while Fe 3 O 4 @SiO 2 -NH 2 -AA nanoparticles were obtained by activated AA via amidation reaction. IR, XPS and SEM analysis were used for the characterizations of Fe 3 O 4 @SiO 2 -NH 2 and Fe 3 O 4 @SiO 2 -NH 2 -AA nanoparticles. Alkaloid adsorption experiments implied that Fe 3 O 4 @SiO 2 -NH 2 -AA nanoparticles as a absorbent could be used for the adsorption of the alkaloids. At pH 8, the carboxylic acid of Fe 3 O 4 @SiO 2 -NH 2 -AA nanoparticleswas converted to a negatively-charged carboxylate ion. Therefore, quaternary ammonium alkaloids were significantly adsorbed onto the carboxylic acid-rich surface, possibly due to electrostatic interactions. As for Palmatine and Berberine, the most adsorption could be obtained at pH 8 when the adsorption time was 6 min. The adsorption percentage of Palmatine was 22.2%, while the adsorption percentage of Berberine was 23.6% at pH 8. As for the effect of adsorption time on liquid phase system, the adsorption conditions of 8 min has been chosen when pH 7 was used. Considering the above conditions, pH 8 and the adsorption time of 8 min could be chosen for further uses. This work demonstrates the potential of AA modification in a Fe 3 O 4 -based alkaloid adsorption study. In further experiments, when the amidation reaction is performed, residual carboxyl groups from AA on the modified Fe 3 O 4 @SiO 2 -NH 2 -AA nanoparticles may be used for bio-molecule immobilization.
Supplementary Materials: The supplementary materials are available online.