One-step synthesis of magnetic-TiO2-nanocomposites with high iron oxide-composing ratio for photocatalysis of rhodamine 6G

In the study, a facile one-step method for synthesizing magnetic-TiO2-nanophotocatalysts was developed. With the same composing ratio of 0.5 and 0.35 (Fe:Ti, mole:mole), we prepared two types of magnetic-TiO2-nanocomposites as one-step synthesized FexOy-composed TiO2 (FexOy/TiO2-0.5 and FexOy/TiO2-0.35) and two-step synthesized core-shell FexOy@TiO2 (FexOy@TiO2-0.5 and FexOy@TiO2-0.35), and tested their performance in rhodamine 6G (R6G) photodegradation. X-ray diffraction (XRD) analysis showed that FexOy@TiO2-0.5 has the smallest crystallite size (16.8 nm), followed by FexOy@TiO2-0.5 (18.4 nm), FexOy/TiO2-0.35 (21.0 nm) and FexOy/TiO2-0.5 (19.0 nm), and X-ray photoelectron spectroscopy (XPS) suggested the decreasing percentage of Fe3O4 from 52.1% to 36.7%-47.2% after Ti-deposition treatment. The saturated magnetisms followed the order: FexOy@TiO2-0.5 > FexOy@TiO2-0.35 > FexOy/TiO2-0.5 > FexOy/TiO2-0.35. R6G photodegradation followed the first order kinetics and was slightly influenced by pH but significantly affected by initial photocatalyst concentration. FexOy/TiO2-0.35 achieved the highest removal efficiency for R6G (92.5%), followed by FexOy@TiO2-0.35 (88.97%), FexOy@TiO2-0.5 (60.49%) and FexOy/TiO2-0.5 (48.06%). Additionally, all these magnetic-TiO2-nanocomposites had satisfied magnetic recoverability and exhibited laudable reusability after 5-times reuse, even achieving higher R6G removal efficiencies from 97.30% to 98.47%. Our one-step method took only 75 min for nanocomposite synthesis, 90 min less than conventional two-step method, showing its feasibility as a practical method for magnetic-TiO2-nanocomposite synthesis in industrial application.


Introduction
Photocatalysis is one of most popular advanced oxidation processes (AOPs) in water treatment owning to its promising features of environment-friendly, generally non-selectivity and less secondary pollution [1]. In photocatalysis process, photocatalyst is the crucial component producing reactive oxygen species (ROS), e.g., OH radicals [2], during the reaction by stopping recombination of photo excited electron hole pair on the surface of the photocatalysts [3]. Among them, titanium dioxide (TiO 2 ) is recognized as one of the best photocatalysts for its redox ability, high chemical and biological stability (particularly to photocorrosion), cost effectiveness and minor toxicity [3,4,5]. Bare TiO 2 photocatalysts have some inherent shortages. As working within a narrow ultraviolet wavelength [6], TiO 2 photocatalysts normally have a relatively low quantum efficiency and the most applied approach is minimizing the particulate size of TiO 2 to achieve a large specific surface area [7]. Accordingly, most TiO 2 catalysts are used in nano-scale [8,9], challenging the separation and recovery of these ultrafine particles after photocatalytic reaction. Considering their risks to the environment [10], recovering and reusing these TiO 2 nano-photocatalysts is of great urgency. To solve this problem, some approaches are developed to support TiO 2 nano-particulates with different anchors, e.g., glass and ceramic [11]. Nevertheless, the photoactivities of these fixed-bed systems suffer from the low ratio of mass transfer, comparing to the suspension systems [4]. Recent studies therefore propose the introduction of iron elements in TiO 2 nano-photocatalysts as a promising method to achieve magnetic separation and harvesting [12]. Magnetic separation is more selective, efficient, and often much faster than centrifugation or filtration [13,14]. The key in magnetic separation is to generate strong magnetic forces on the target particles to overcome opposing forces, e.g. viscous drag, Brownian motion and sedimentation. Particulate size influences the magnetic forces [15], and decreasing the crystallite size from micrometers to nanometers significantly increases the magnetism by 100 to 1,000 times [16]. Thus, magnetic nanoparticulates (MNPs) have gained increasing attentions recently [17,18,19,20].
Coupling TiO 2 photocatalysts with MNPs provides a group of novel nanophotocatalysts integrating the superior photodegradation performance of TiO 2 and simple recovery by external magnetic fields. It has the potential to overcome the troubles in recovering and harvesting nanophotocatalysts after reuse. Generally, magnetic-TiO 2 -nanophotocatalysts are manufactured by functionalizing the surface of MNPs with one thin layer of TiO 2 photocatalysts. Zhang et al. prepared magnetic-TiO 2 -nanophotocatalysts via wrapping TiO 2 on montmorillonite and Fe 3 O 4 , achieving satisfied photodegradation rates and reusability for methylene blue [21]. Chen et al. synthesized three types of magnetic-TiO 2 -nanophotocatalysts, showing that Fe 2 O 3 @TiO 2 had the highest adsorption efficiency (99%, 10 min) and Fe/TiO 2 achieved the highest photodegradation efficiency (94%, 150 min) for methylene blue [22]. Magnetic-TiO 2 -nanophotocatalysts with different silver composing ratios could degrade 83.9% of methylene blue within 6 hours and the degradation efficiency remained 79% after 5-cycle reuse [23]. Although these magnetic-TiO 2 -nanophotocatalysts achieved satisfied photodegradation efficiencies and magnetic recoveries, they all require a complicated multiple-step synthesis and time-consuming pre-synthesis of MNPs or TiO 2 precursor [5]. Alternatively, iron-composing is also used in TiO 2 nanophotocatalysts to modify the bandgap energy of TiO 2 and obtain a better photoactivity or extend the absorption spectrum [24,25]. The composing ratio of iron is normally less than 1% (mass ratio) owing to the declined photoactivity by excessive composing, and their magnetic recovery performance is not satisfied [26,27,28,29].
To the best of our knowledge, no previous research has reported simple or one-step synthesis processes to obtain iron-composed magnetic TiO 2 nanophotocatalysts with high Fe atomic percentage (>20%) via coprecipitation method. In this study, we developed a facile approach to synthesize magnetic-TiO 2 -nanocomposites via one-step coprecipitation from iron and titanium salts. The synthesized magnetic-TiO 2 -nanocomposites achieved comparable photocatalytic degradation performance of rhodamine 6G (R6G) and had good durability after recovery and reuse. The main advantages of this method are: 1) simplified synthesis procedure without the need of pre-synthesizing MNPs or TiO 2 precursor; 2) 55% less synthesis time comparing to two-step method; 3) cost-saving for fewer reagents in synthesis process.

Magnetic TiO 2 synthesis
All the chemicals used in this study were of analytical grade and purchased from Sigma Aldrich (UK). One-step synthesis of TiO 2 -composing MNPs followed the previously reported coprecipitation method with modifications [30,31]. Briefly, 2 mL FeCl 3 (1.0 M) and 1 mL FeCl 2 (2.0 M) were gently mixed and added with 20 mL titanium isopropoxide (TTIP, 97%) and isopropanol (IPA, �99.7%). The mixture was kept shaking, to avoid agglomeration, with drop-by-drop addition of 45 mL NaOH (1.0 M) to control the crystallization rate, and continuously homologized for 30 min by ultrasound (60 kHz, LNGF175, Langford Electronics Ltd., UK). The synthesized brown-dark nanoparticles were harvested by a permanent magnet and rinsed with ultrapure water until the supernatant reached neutral pH (7.0 Table. In comparison, two TiO 2 -coating magnetic nanophotocatalysts (core-shell), Fe x O y @TiO 2 -0.5 (Fe:Ti = 0.5, mole:mole) and Fe x O y @TiO 2 -0.35 (Fe:Ti = 0.35, mole:mole), were prepared using the conventional two-step synthesis method. Firstly, MNPs synthesis followed the reported protocol [32], except for Fe 2+ /Fe 3+ ratio (1:1, mole:mole). The synthetized MNPs were washed with ultrapure water several times until pH was 7.0, and resuspended in 25 mL ultrapure water. Subsequently, 10 mL of MNPs suspensions were rinsed with 25 mL IPA three times for dehydration. Then, 25 mL IPA and 0.2 mL HCl (2.0 M) were added, gently mixed at 60 rpm, followed by rapidly adding TTIP of different volume (0.95 mL for Fe x O y @TiO 2 -0.5 and 1.35 mL for Fe x O y @TiO 2 -0.35) and keep shaking with drop-by-drop addition of 45 mL1.0 M NaOH (at least 45 minutes). After ultrasonic treatment for 30 min, another 1 mL NaOH (1.0 M) was added with an extra one-hour ultrasonic treatment.
All the synthesized magnetic-TiO 2 -nanocomposites were washed by ultrapure water until neutral pH. They were finally separated by magnet bar and dried overnight in a 60˚C vacuum oven. After ground into powder, the granules were crystallized in a muffle furnace at 500˚C for 4 hours.

Adsorption and photocatalysis experiment
Adsorption experiments were carried out in the dark to investigate R6G adsorption on magnetic-TiO 2 -nanocomposites. R6G was dissolved in ultrapure water to make series concentrations from 1 to 25 mg/L. The synthesized magnetic-TiO 2 -nanocomposites were added and the concentration was fixed as 0.4 g/L. The reaction system was kept continuous shaking (150 rpm) for 360 min and the water samples were collected at 1, 2, 3, 4, 5 and 6 hours. At each time point, the magnetic-TiO 2 -nanocomposites were removed by external magnetic field and the supernatant was collected for R6G analysis. To test the effects of pH on R6G adsorption, R6G solution was adjusted to pH�3, 7 and 10 by adding HCl (1.0 M) or NaOH (1.0 M), respectively.
R6G photodegradation was carried out in 6-well plates (Costar, UK), with a 20-watt UV lamp (253 nm) as the irradiation source. Initial R6G concentration was 10 mg/L, and the concentration of magnetic-TiO 2 -nanocomposites was 0.4 g/L. During the 6-hour degradation experiment, the mixture was kept shaking at 150 rpm, and 250 μL of samples were collected at, 1, 2, 3, 4, 5 and 6 hours. After centrifugation at 10,000 rpm for 1 min, the supernatant was collected for R6G analysis. To test the effect of light wavelength on the photocatalytic degradation of R6G, 460-nm and 540-nm light was also used, following the same procedure described above. For the effects of pH and nanocomposite concentration on photocatalytic efficiency, the pH of the reaction system was adjusted to 3.0, 7.0 and 10.0 by adding HCl (1.0 M) or NaOH (1.0 M), and the concentrations of magnetic-TiO 2 -nanocomposites were set as 0.2, 0.4 and 0.8 g/L. For each experiment, a blank control without UV light was set up and all the adsorption and photodegradation experiments were carried out in triplicates.
To test the durability of the synthesized magnetic-TiO 2 -nanocomposites, they were recovered by a magnetic bar after 4-hour photodegradation of R6G, washed by ultrapure water for three times, dried at room temperature for 10 min, and finally added into fresh R6G for reuse, following the same procedure as described above. All the magnetic-TiO 2 -nanocomposites were recovered and reused at least five times.

Chemical analysis
Fe and Ti oxidation phases of the synthesized magnetic-TiO 2 -nanocomposites were analysed by X-ray photoelectron spectroscopy (XPS) via an ESCALAB 250Xi (Thermo Fisher, UK), using AlKα X-ray radiation (hv = 1486.6 eV, 1500 W) for excitation. X-ray diffraction (XRD) analysis was performed on an X' Pert PRO MPD diffractometer (PANalytical, Netherlands) equipped with Cu-Kα radiation at 40 kV and 40 mA. Surface morphologies were analysed using transmission electron microscopy (TEM, Tecnai G2 F20, USA). A vibrating sample magnetometer (VSM, Lake Shore 7410, USA) was used to measure the magnetism of the synthesized magnetic-TiO 2 -nanocomposites. Energy dispersive spectroscopy (EDS) analysis was conducted by a field emission scanning electron microscope (Quanta 450F, FEI, USA) with a voltage of 30 V. The Brunauer-Emmett-Teller (BET) surface area was measured by N 2 physisorption on an Autosorb iQ-C (Quantachrome Instruments, USA). The concentrations of MNPs and magnetic-TiO 2 -nanocomposites were determined by gravimetric method. R6G concentration was determined by at 540 nm (excitation at 350 nm) by a multimode plate reader (FLUOstar Omega, Germany).

Data analysis
All the data were presented in terms of mean ± standard deviation. The removal efficiency (%) of R6G was calculated by the equation (C 0 -C t )/C 0 , where C 0 is the initial concentration of R6G in the solution (mg/L) and C t is the R6G concentration at time t (mg/L). Data of XPS and XRD were analysed by XPSpeak41 and Jade 6.5, respectively. The analysis of variance (ANOVA) was carried out via SPSS 20.0 for windows, and the significant level is p<0.05.
R6G degradation or removal efficiency was calculated as the ratio of residual R6G to initial R6G in each treatment. The R6G degradation kinetics was calculated according to the firstorder reaction, ln(C t /C 0 ) = -k obs t. Here, k obs is the photodegradation rate constant (h -1 ). Both Langmuir and Freundlich isotherm models were used to assess the adsorption capacity of the synthesized magnetic-TiO 2 -nanocomposites, as expressed in the following equations: Here, Q is the amount of R6G adsorbed on magnetic-TiO 2 -nanocomposites (mg/g), and C is the equilibrium concentration of R6G in aqueous phase (mg/L). For Langmuir isotherm, Q max is the theoretical maximum adsorption capacity (mg/g) and K L is the adsorption equilibrium constant. K F and n are the constants of Freundlich model.
To distinguish the different pathway of R6G loss by different magnetic-TiO 2 -nanocomposites via adsorption, photolysis and photocatalysis, the changes of R6G concentrations in different treatments were calculated by Eqs (3) to (8).
Here, "0.2", "0.4" and "0.8" indicates different treatments with initial magnetic-TiO 2 -nanocomposites concentration of 0.2, 0.4 and 0.8 mg/L, respectively. AD is the R6G loss in treatments with magnetic-TiO 2 -nanocomposites but no UV-irradiation. PL is the R6G loss in treatments with UV-irradiation but no magnetic-TiO 2 -nanocomposites. Total is the R6G loss in treatments with both magnetic-TiO 2 -nanocomposites and UV-irradiation. PC refers to the contribution of photocatalysis to R6G loss as calculated in Eqs (3)- (5). PAD, PRL and PRC refers to the average percentage of adsorption, photolysis and photocatalysis in R6G loss, respectively.

Characteristics of magnetic-TiO 2 -nanocomposites
After crystallization, all the four types of magnetic-TiO 2 -nanocomposites had a red-brown colour (S1 Fig). TEM images (S2 Fig) illustrated that all the magnetic-TiO 2 -nanocomposites had a typical solid particle structure, irregular ball or rod. Their crystallite size ranged from 10-100 nm, fitting well with the critical size suggested for effective magnetic separation (~50 nm) [16]. The morphologies of these particles were similar to that of Fe(III)-composed TiO 2 particles synthesized by previous work [33]. It is worth mentioning that the one-step synthesis of Fe x O y /TiO 2 nanocomposites took only 75 min, 55% less than that of Fe x O y @TiO 2 nanocomposites synthesized by conventional two-step method (165 min). EDS results (S3  Facile magnetic-TiO 2 -nanocomposites for rhodamine 6G photocatalysis The elemental composition of the synthesized MNPs and magnetic-TiO 2 -nanocomposites was analysed by XPS (Fig 2A). All the materials had iron and oxygen as core elements, owing to the main peaks of Fe 2p (710.3 to 710.7 eV) and O 1s (529.3 to 529.9 eV). One additional Ti 2p peak (457.8 to 457.9 eV) appeared in the XPS spectra of magnetic-TiO 2 -nanocomposites. Fig 2B to 2F further show the Fe 2p bands in the binding energy region of 705-730 eV. MNPs showed the strongest intensity, followed by Fe x O y @TiO 2 nanocomposites. All the spectra of magnetic-TiO 2 -nanocomposites could fit into two Fe 2p3/2 peaks (around 710 eV and 723 eV) and two Fe 2p1/2 peaks (around 711 eV and 725 eV) [35,36], suggesting the presence of both Fe 3 O 4 and Fe 2 O 3 [37]. Furthermore, the satellite peak at 719 eV is the main identity of Fe 2 O 3 or FeO [38]. Accordingly, Fe 3 O 4 accounted for 52.1% of the total iron oxides in MNPs, decreasing to 36.7%-47.2% in magnetic-TiO 2 -nanocomposites. In addition, nanocomposites with higher Ti-deposition ratio had relatively higher proportion of  Fig 2G. The coercivity (H c ) and remanence magnetization (M r ) of all the magnetic-TiO 2 -nanocomposites were zero, indicating that the hysteresis loops were coincident completely and these nanocomposites dispersed well in the absence of external magnetic field. Generally, the saturation magnetisms of Fe x O y @TiO 2 nanocomposites were higher than Fe x O y /TiO 2 ones, explained by the incomplete coordination of iron atoms in the Fe x O y /TiO 2 nanocomposites [5]. Additionally, the saturation magnetism increased with the Fe/Ti ratio, owing to the strong link between M s and the percentage of Fe 3 O 4 [39]. The saturation magnetisms of our synthesized magnetic-TiO 2nanocomposites fell in the range of previously studied magnetic nanophotocatalysts (0.54-42.2 emu/g, Table 1), indicating their comparable magnetic recovery or separation efficiency.

R6G adsorption isotherm
The adsorption of organic molecules on catalysts is an important process during photocatalysis [46], which is related to the R6G photocatalytic degradation efficiency by magnetic-  (Table 2), Langmuir adsorption described the adsorption mechanisms better except for Fe x O y /TiO 2 -0.5 according to R 2 of each nanocomposite. Accordingly, Fe x O y @TiO 2 nanocomposites presented a better adsorption performance than Fe/Ti ones. Previous studies [47,48,49] suggested that the molecular adsorption on catalysts is involved in the surface complexation and ion exchange between the catalyst surface and the adsorbates. The functional groups located on the surface of TiO 2 include TiOH 2 + , TiOH and TiO − [50], which are more abundant than those on the surface of iron oxides [51]. The adsorption of R6G on nanocomposites is therefore dependent on the proportion of TiO 2 on the surface, which is higher in Fe x O y @TiO 2 nanocomposites.
In the present study, pH change from 3 to 10 did not significantly affect the R6G adsorption on magnetic-TiO 2 -nanocomposites (S5 Fig, p>0.05). pH has been considered as one of the most important operational parameters in many photocatalytic systems, significantly affecting the photocatalytic efficiency via changing the structure and adsorption-desorption process of adsorbates. As the point of zero charge (PZC) for TiO 2 is 6.25 [5], the changes in surface charge of TiO 2 at various pH values are expressed in Eqs (9) and (10) [50]. At pH lower than PZC, the increasing proportion of TiOH 2 + led to the positively charged TiO 2 surface, whereas the negatively charged TiOoccurs at pH>PZC. Meanwhile, R6G has a logarithmic acid dissociation constant (pKa) of 6.13, similar as the PZC for TiO 2 . At pH>6.13, R6G is primarily in molecular state as the free electron pair on the primary amine group transfer to the aromatic rings and behave hydrophobic, but change to hydrophilic at lower pH when the protonation of nitrogen carries on in the secondary amine group of the xanthene ring [52]. Accordingly, the electrostatic force interactions between TiO 2 surface and R6G were reported to be weak repulsion or attraction in a broad range of pH [53], showing similar adsorption performance.

Contribution of adsorption, photolysis and photocatalysis to R6G degradation
Under all pH conditions, R6G exhibited limited removal without light (approximately 14.1%, S6 Fig) which was significantly lower than those with 253-nm UV-irradiation (averagely 73.58%, p<0.01, Fig 4). In addition, the R6G degradation efficiency with 460-nm or 540-nm irradiation (S7 Fig) was similar as that without light. It proved the significant contribution of photocatalysis to R6G degradation comparing to adsorption, and UV irradiation wavelength is a critical factor triggering R6G photodegradation with the aid of magnetic-TiO 2 -nanocomposites. It is worth mentioning that there was neglectable R6G degradation in treatments with bare MNPs (data not shown), proving that neither Fe 3 O 4 nor Fe 2 O 3 contributed to R6G photocatalysis.  However, the loss of R6G might be explained by either adsorption, photolysis or photocatalysis as previously reported [46], which needs to be distinguished to evaluate the actual R6G photocatalysis performance.   [23]. These results indicated that the photocatalytic performance of the synthesised magnetic-TiO 2 -nanocomposites increased with the Ti/Fe ratio. Since the photocatalytic active sites are mainly located on TiO 2 instead of iron oxides [43], higher percentage of TiO 2 in magnetic-TiO 2nanocomposites increases the photocatalysis capability. Iron-composing benefits the photocatalytic performance of TiO 2 because transition metal ions can act as shallow charge traps in the crystal structure, inhibiting the recombination of electron-hole pairs and prolonging their lifetime [54]. Although the impacts of transition metals on TiO 2 catalytic performance strongly depend on the composing ratio and are reported to peak at low level, all the previous studies focused on the low Fe-composing ratio, normally less than 10 at.% [33,55]. Our synthesized magnetic-TiO 2 -nanocomposites had the high Fe:Ti ratio (Fe-atomic percentage ranging from 25.4-35.5%). For the first time, our results suggested magnetic-TiO 2 -nanocomposites with high Fe-composing ratio still have satisfied photocatalysis capability.  Facile magnetic-TiO 2 -nanocomposites for rhodamine 6G photocatalysis Our results showed slightly higher R6G photodegradation efficiencies under neutral pH conditions than acidic and basic treatments. It might be explained by the higher R6G adsorption on magnetic-TiO 2 -nanocomposites as mentioned above. As adsorption is a key step for photocatalysis [46], more R6G absorbed on magnetic-TiO 2 -nanocomposites under neutral pH therefore contribute to higher R6G removal. A similar result was also reported that the highest efficiency was obtained at the neutral condition (pH = 7.4) during the phenol photodegradation process with TiO 2 as photocatalyst [50].

R6G photodegradation kinetics
The photocatalysis kinetics of R6G by different magnetic-TiO 2 -nanocomposites are illustrated in Fig 5. R6G degradation followed the first-order kinetics (correlation coefficient above 0.9), consistent with previous study [52]. For two-step synthesized magnetic-TiO 2 -nanocomposites, R6G photodegradation rate constant (k obs ) ranged from 0.0816 to 0. Among them, Fe x O y @TiO 2 -0. 35 and Fe x O y /TiO 2 -0.35 nanocomposites showed higher photocatalytic activities than previously reported methylene blue degradation by magneticnanophotocatalyst Ni-Cu-Zn ferrite@SiO 2 @TiO 2 @Ag [23] (k obs from 0.1326 to 0.2544 h -1 ). It is worth noting that the dosage of magnetic-TiO 2 -nanocomposites did not significantly change the k obs , possibly attributing to the decrease of surface active sites as nanophotocatalysts aggregate at elevated concentration, or the declined light utilization efficiency caused by the increasing opacity level and scattering of light at high nanocomposite concentration [56].

Reusability of magnetic-TiO 2 -nanophotocatalysts for R6G photodegradation
Reusability is a critical factor for evaluating the practical feasibility of nanophotocatalysts in industrial applications. After recycling the synthesized magnetic-TiO 2 -nanocomposites and reusing them for R6G photocatalytic degradation five times, our results proved their satisfactory stability in photocatalysis, as illustrated in Fig 6. The photocatalytic activities of all the magnetic-TiO 2 -nanocomposites remained unchanged or even increased in all the cycles. After 5 cycles, the R6G removal efficiency was up to 97.30% to 98.47%, and there was no significant difference between the four magnetic-TiO 2 -nanocomposites. Additionally, R6G degradation still followed the first-order kinetics and the photodegradation rate constant k obs was 0.1434-1. decreasing k obs during reuse was also reported by some previous studied and might be explained by the activation of photocatalytic active sites [57,58,59].
Numerous studies have attempted to synthesize and reuse different types of magnetic nanophotocatalysts in removing dyes, as listed in Table 3. For industrial application, both photocatalytic capability and recovery ratio are important to achieve cost-effectiveness. Nevertheless, none of the studies mentioned above have provided data support. Here, we evaluated the recovery ratio for all the synthesized magnetic-TiO 2 -nanocomposites, which were acceptable after 5-time reuse and achieved 68.83% for Fe x O y /TiO 2 -0.5, 65.38% for Fe x O y /TiO 2 -0.35, 80.32% for Fe x O y @TiO 2 -0.5 and 77.84% for Fe x O y @TiO 2 -0.35. Our result indicated long lifecycles of these synthesized magnetic-TiO 2 -nanocomposites, and the recovery ratio might be further improved by increasing M s to enhance magnetic separation efficiency and prolong their life-time.
Of all the concerns to apply nanophotocatalysts for industrial applications, including the extension of excitation wavelength, viability of magnetic separation, photocatalytic activity and cost-effectiveness in nanocomposite synthesis, our study attempted to reduce the synthesis Facile magnetic-TiO 2 -nanocomposites for rhodamine 6G photocatalysis  Facile magnetic-TiO 2 -nanocomposites for rhodamine 6G photocatalysis time and chemical consumption by one-step facile synthesis. More studies can be introduced from this basis to target other objectives. For instance, iron-composing was reported to extend the excitation wavelength of TiO 2 nanophotocatalysts [60] or improve their photocatalytic efficiency [61], and the magnetism of iron-composing TiO 2 nanophotocatalysts can be altered by synthesis modification. Accordingly, our one-step facile synthesis of magnetic-TiO 2 -nanophotocatalysts with high iron-composing ratio provides opportunities for synthesizing similar magnetic-TiO 2 -nanocomposites with new features for further industrial applications.

Conclusion
In the present study, magnetic-TiO 2 -nanocomposites with high iron-composing g ratio were prepared by a one-step coprecipitation method without any pre-synthesized precursor. Comparing to conventional two-step synthesized TiO 2 -coating magnetic-nanocomposites with MNPs as precursor, we successfully decreased the synthesis time from 165 minutes to 75 minutes. Our results also proved that one-step synthesised magnetic-TiO 2 -nanocomposites had satisfied R6G adsorption capability, photodegradation efficiency and photodegradation rate constant. The photocatalytic performance was dependent on Fe/Ti atomic ratio, and Fe x O y / TiO 2 -0.35 was the most feasible nanophotocatalysts for industrial application. With facile synthesis process, comparable photocatalytic capability, acceptable viability of magnetic separation and satisfactory reusability, this synthesis method provides an alternative approach to prepare magnetic-TiO 2 -nanophotocatalysts feasible for industrial practices.
Supporting information S1