Low Temperature Synthesis of Photocatalytic Mesoporous TiO 2 Nanomaterials

: We report the synthesis of mesoporous TiO 2 nanostructures based on the decomposition of TiOSO 4 in aqueous alkaline solution at room temperature, followed by mild thermal treatment (110 ◦ C) in an oven and suitable to yield up to 40 g of product per batch. The duration of the thermal treatment was found to be crucial to control crystalline phase composition, speciﬁc surface area, surface chemistry and, accordingly, the photocatalytic properties of the obtained TiO 2 nanocrystals. The thorough investigation of the prepared samples allowed us to explain the relationship between the structure of the obtained nanoparticles and their photocatalytic behavior, that was tested in a model reaction. In addition, the advantage of the mild treatment against a harsher calcination at 450 ◦ C was illustrated. The proposed approach represents a facile and sustainable route to promptly access an e ﬀ ective photocatalyst, thus holding a signiﬁcant promise for the development of solutions suitable to real technological application in environmental depollution.


Introduction
In recent years, an enormous research effort of scientific community has been focusing towards novel technologies for environmental remediation. Among the most critical environmental issues, the exponential increase in pollutants in wastewater has urged particular attention, as several studies have confirmed the presence in water bodies of emerging pollutants [1], that are a class of compounds, including pharmaceutical and personal care products or pollutants coming from civil, industrial and agricultural waste sewage, and have a tremendous environmental impact, and thus represent a

Results and Discussion
The synthesis of TiO 2 nanoparticles (NPs) involves TiOSO 4 as cost effective Ti 4+ precursor, and exploits a precipitation method in alkaline solution by dropwise addition of the TiOSO 4 solution to NH 4 HCO 3 ( Figure 1A) under constant magnetic stirring. Upon mixing, TiOSO 4 suddenly reacts, promoting the formation and precipitation of Ti-hydroxide species, resulting in a coalescence of the reaction mixture that turns into a milky slurry at the end of the reaction. The obtained nanocrystals were collected by centrifugation at 3000 rpm and the precipitate was repeatedly washed by subsequent cycles of dispersion in water and centrifugation. At this stage, the obtained white precipitate was thermally treated in an oven at 110 • C for 2, 8, 16 and 24 h, respectively. The obtained samples were comprehensively investigated by integrating a number of complementary techniques, namely DRS (Diffuse Reflectance Spectroscopy), TGA/DTA (Thermogravimetric Analysis/Differential Thermal Analysis), N 2 adsorption-desorption isotherms, HRTEM (high-resolution transmission electron microscopy), STEM/EDS (scanning transmission electron microscopy/energy dispersive spectroscopy), SEM (scanning electron microscopy), XRD (X-ray diffraction) and finally, their photocatalytic activity was evaluated spectrophotometrically, by monitoring photocatalyst-assisted decoloration of a dye molecule, methylene blue, selected as a model compound.
All the investigated TiO 2 samples show the typical absorbance onset at 345 nm, irrespective of the duration of the thermal treatment, corresponding to a band gap of 3.65 eV, calculated according to the Tauc plot [24]. The DR spectrum of a representative sample (TiO 2 _16 h) is reported in Figure 1B.
Catalysts 2020, 10, x FOR PEER REVIEW 3 of 19 methylene blue (MB), showing a progressive increase (up to 1.5 times) for the photocatalyst obtained after prolonged thermal treatment. The overall results indicate that the proposed synthesis represent a viable, easily up-scalable and sustainable approach to achieve a photocatalytically active mesoporous TiO2, characterized by a relevant technological potential that holds a great promise for real application in the field of environmental depollution.

Results and Discussion
The synthesis of TiO2 nanoparticles (NPs) involves TiOSO4 as cost effective Ti 4+ precursor, and exploits a precipitation method in alkaline solution by dropwise addition of the TiOSO4 solution to NH4HCO3 ( Figure 1A) under constant magnetic stirring. Upon mixing, TiOSO4 suddenly reacts, promoting the formation and precipitation of Ti-hydroxide species, resulting in a coalescence of the reaction mixture that turns into a milky slurry at the end of the reaction. The obtained nanocrystals were collected by centrifugation at 3000 rpm and the precipitate was repeatedly washed by subsequent cycles of dispersion in water and centrifugation. At this stage, the obtained white precipitate was thermally treated in an oven at 110 °C for 2, 8, 16 and 24 h, respectively. The obtained samples were comprehensively investigated by integrating a number of complementary techniques, namely DRS (Diffuse Reflectance Spectroscopy), TGA/DTA (Thermogravimetric Analysis/Differential Thermal Analysis), N2 adsorption-desorption isotherms, HRTEM (highresolution transmission electron microscopy), STEM/EDS (scanning transmission electron microscopy/energy dispersive spectroscopy), SEM (scanning electron microscopy), XRD (X-ray diffraction) and finally, their photocatalytic activity was evaluated spectrophotometrically, by monitoring photocatalyst-assisted decoloration of a dye molecule, methylene blue, selected as a model compound.
All the investigated TiO2 samples show the typical absorbance onset at 345 nm, irrespective of the duration of the thermal treatment, corresponding to a band gap of 3.65 eV, calculated according to the Tauc plot [24]. The DR spectrum of a representative sample (TiO2_16 h) is reported in Figure  1B.  Table 1 and Figures 2 and S1 report the main results of the structural characterization performed by means of XRD analysis on TiO2 NPs samples as a function of the thermal treatment duration at 110 °C. Surprisingly, after the purification step, the TiO2 sample (TiO2_0) shows an initial crystalline structure characterized by a dominant presence of brookite (85%) and a reduced amount of anatase (15%). After 2 h of thermal treatment, the two polymorphs occur almost in the same percentage (53% anatase and 47% brookite). For a longer treatment time, the phase composition of the samples changes significantly, with anatase becoming the prevalent phase. Indeed, between 8 and 16 h of treatment, the TiO2 sample is shown to be composed of 75% anatase phase, and 25% brookite phase. Finally, after 24 h of thermal treatment, anatase and brookite appear in the percentages of 81% and 19%,  Table 1 and Figure 2 and Figure S1 report the main results of the structural characterization performed by means of XRD analysis on TiO 2 NPs samples as a function of the thermal treatment duration at 110 • C. Surprisingly, after the purification step, the TiO 2 sample (TiO 2 _0 h) shows an initial crystalline structure characterized by a dominant presence of brookite (85%) and a reduced amount of anatase (15%). After 2 h of thermal treatment, the two polymorphs occur almost in the same percentage (53% anatase and 47% brookite). For a longer treatment time, the phase composition of the samples changes significantly, with anatase becoming the prevalent phase. Indeed, between 8 and 16 h of treatment, the TiO 2 sample is shown to be composed of 75% anatase phase, and 25% brookite phase. Finally, after 24 h of thermal treatment, anatase and brookite appear in the percentages of 81% and 19%, respectively. In summary, immediately after the precipitation reaction, the dominant crystallographic Catalysts 2020, 10, 893 4 of 18 phase in the TiO 2 NPs is brookite, and as thermal treatment proceeds, the brookite phase progressively converts into the anatase phase, as depicted in Figure 3. Table 1. Crystallographic composition of the TiO 2 NPs as a function of the duration of the thermal treatment.

Sample
Anatase Phase Brookite Phase Catalysts 2020, 10, x FOR PEER REVIEW  4 of 19 respectively. In summary, immediately after the precipitation reaction, the dominant crystallographic phase in the TiO2 NPs is brookite, and as thermal treatment proceeds, the brookite phase progressively converts into the anatase phase, as depicted in Figure 3.  The XRD patterns were also analyzed by a whole-profile Rietveld-based fitting program according to a procedure fully described elsewhere [25]: the fitting procedure carried out the XRD patterns including only the TiO2 anatase phase, which allows us to evaluate the coherent crystal apparent domain size which remains substantially constant (around 3.3 nm ± 0.5) all along the thermal treatment duration. The XRD patterns were also analyzed by a whole-profile Rietveld-based fitting program according to a procedure fully described elsewhere [25]: the fitting procedure carried out the XRD patterns including only the TiO 2 anatase phase, which allows us to evaluate the coherent crystal apparent domain size which remains substantially constant (around 3.3 nm ± 0.5) all along the thermal treatment duration. The bright field TEM (BF-TEM) micrographs of TiO2 NCs before and after thermal treatment at 110 °C in an oven are reported in Figure 4. The variation of NP morphology and size can be put in correlation with thermal treatment duration. Indeed, the as prepared TiO2 NPs are very small (approximately 1 nm in diameter) with irregular shape. The thermal treatment promotes an increase in NP size (Table 2) and a reshaping towards spherical-like NPs. In fact, the samples TiO2_2 h and TiO2_8 h ( Figure 4B,C, respectively) are characterized by slightly larger particles (4 ± 1 and 13 ± 8 nm, respectively). After 16 h of thermal treatment ( Figure 4D), even larger particles are visible, and spherical in shape (diameter 23 ± 6 nm; Table 2). A prolonged thermal treatment, up to 24 h ( Figure  4E), does not results in any substantial modification of the NP morphology (still spherical particles are observed) and size (diameter 22 ± 7 nm). A representative SEM micrograph of the TiO2_16 h sample ( Figure 4F) shows that the sample is composed of micrometric aggregates of NPs irrespective of thermal treatment duration (data not reported). The bright field TEM (BF-TEM) micrographs of TiO 2 NCs before and after thermal treatment at 110 • C in an oven are reported in Figure 4. The variation of NP morphology and size can be put in correlation with thermal treatment duration. Indeed, the as prepared TiO 2 NPs are very small (approximately 1 nm in diameter) with irregular shape. The thermal treatment promotes an increase in NP size (Table 2) and a reshaping towards spherical-like NPs. In fact, the samples TiO 2 _2 h and TiO 2 _8 h ( Figure 4B,C, respectively) are characterized by slightly larger particles (4 ± 1 and 13 ± 8 nm, respectively). After 16 h of thermal treatment ( Figure 4D), even larger particles are visible, and spherical in shape (diameter 23 ± 6 nm; Table 2). A prolonged thermal treatment, up to 24 h ( Figure 4E), does not results in any substantial modification of the NP morphology (still spherical particles are observed) and size (diameter 22 ± 7 nm). A representative SEM micrograph of the TiO 2 _16 h sample ( Figure 4F) shows that the sample is composed of micrometric aggregates of NPs irrespective of thermal treatment duration (data not reported). The bright field TEM (BF-TEM) micrographs of TiO2 NCs before and after thermal treatment at 110 °C in an oven are reported in Figure 4. The variation of NP morphology and size can be put in correlation with thermal treatment duration. Indeed, the as prepared TiO2 NPs are very small (approximately 1 nm in diameter) with irregular shape. The thermal treatment promotes an increase in NP size (Table 2) and a reshaping towards spherical-like NPs. In fact, the samples TiO2_2 h and TiO2_8 h ( Figure 4B,C, respectively) are characterized by slightly larger particles (4 ± 1 and 13 ± 8 nm, respectively). After 16 h of thermal treatment ( Figure 4D), even larger particles are visible, and spherical in shape (diameter 23 ± 6 nm; Table 2). A prolonged thermal treatment, up to 24 h ( Figure  4E), does not results in any substantial modification of the NP morphology (still spherical particles are observed) and size (diameter 22 ± 7 nm). A representative SEM micrograph of the TiO2_16 h sample ( Figure 4F) shows that the sample is composed of micrometric aggregates of NPs irrespective of thermal treatment duration (data not reported).  HRTEM analyses do not allow to us distinguish between the anatase and brookite phases, due to both the inherent accuracy of magnification calibration in HRTEM, not higher than 5% [26], and the similarity of the two polymorphs of TiO 2 , that share the octahedral coordination of Ti atoms but slightly differ in the way the TiO 6 octahedra are linked [27]. For this reason, the indexing of the fast Fourier transforms (FFTs) of HRTEM images in Figure 5 is done based on both phases.   HRTEM analyses do not allow to us distinguish between the anatase and brookite phases, due to both the inherent accuracy of magnification calibration in HRTEM, not higher than 5% [26], and the similarity of the two polymorphs of TiO2, that share the octahedral coordination of Ti atoms but slightly differ in the way the TiO6 octahedra are linked [27]. For this reason, the indexing of the fast Fourier transforms (FFTs) of HRTEM images in Figure 5 is done based on both phases. The occurrence of brookite as the prevalent phase immediately after the purification step can be ascribed to a high stochiometric excess of bicarbonate and carbonate anions present in the reaction medium with respect to the TiO2 precursor (approximately 5:1 according to the investigated experimental condition). Under these conditions, bicarbonate and carbonated anions, similarly to The occurrence of brookite as the prevalent phase immediately after the purification step can be ascribed to a high stochiometric excess of bicarbonate and carbonate anions present in the reaction medium with respect to the TiO 2 precursor (approximately 5:1 according to the investigated experimental condition). Under these conditions, bicarbonate and carbonated anions, similarly to oxalate anions, can act as rigid bidentate ligands [26,27], able to bridge two Ti centers, thus leading to a chelate complex that promotes the stabilization of the oxide, namely the metastable brookite phase, as previously reported [28]. Several reports, indeed, indicated that brookite generation takes place through the formation of water-soluble titanium complexes including oxalates [28], citrates [29] and lactates [30]. The small fraction of anatase phase present in the investigated as-prepared sample can be associated to the presence of sulphate anions. The dropwise addition of the acidic TiOSO 4 solution to the NH 4 HCO 3 solution determines a progressive decrease in the pH of the resulting mixed solution and a concomitant generation of the zero-charge complex [Ti(OH) 4 (H 2 O) 2 ] 0 . The complexes can condense due to olation and oxolation reactions, thus resulting in the formation of crystallization nuclei and their subsequent growth. Remarkably, in the presence of sulphate anions, the condensation reaction promotes the generation of anatase structure, since sulphate anions, entering in the coordination sphere of Ti, behave as structure directing agents, as previously demonstrated [28]. Under the investigated experimental conditions, the conversion of the chelate complex of Ti with carbonate/bicarbonate species in brookite, along with the concomitant generation of anatase phase through the condensation reaction of Ti complexes, can be further promoted by mild heating, in agreement with previous reports [31][32][33][34]. Indeed, a progressive conversion of brookite into anatase as a function of thermal treatment duration can be observed in Figure 3. Such evidence seems rather surprising, as brookite is generally recognized as more thermodynamically stable than anatase [35,36]. However, the thermodynamic stability, and, accordingly, the phase conversion process may be affected by the initial size of the nanocrystals. In fact, for nanocrystals up to 11 nm in size, anatase is reported to be the most stable phase, while brookite becomes the most stable phase for size between 11 and 35 nm [37]. In our experiments, the initial crystallite size is below 11 nm, therefore, as calculated by Zhang and Banfiel [38], the formation enthalpy of brookite is higher than that of anatase. Accordingly, it can be reasonably thought that, during the thermal treatment, the less stable brookite particles are progressively converted in the more stable anatase NPs, with the brookite to anatase transformation being energetically downhill.
In Figure 6A, the TGA curves registered as a function of time and temperature for the sample TiO 2 _0 h treated at 110 • C under air flow for 2 and 8 h, respectively, are reported. This conversion from brookite to the anatase phase starts to appear already after 2 h treatment, getting to completion after 8 h. The corresponding DTA profiles as a function of time are shown in Figure 6B. TGA/DSC experiments were carried out to elucidate the effect of the thermal treatment performed on the TiO 2 samples, in order to investigate the weight loss and the enthalpic balance of the processes that take place during the thermal cycle. When the temperature is increased from 25 to 110 • C, a rapid weight loss, from 100% to 87%, is observed in the first 0.1 h at 107 • C and subsequently to 85% after 0.2 h, when a temperature of 110 • C is reached (see Figure 6A,C where the modifications occurring during the first 0.5 h are displayed). Afterwards only a slight decrease in weight is detected, to 83.2 and to 82.45 wt%, after 2 and 8 h of treatment at 110 • C, respectively. Interestingly, the observed weight losses are concomitant with the changes observed in the crystalline phase composition of the sample, that, starting from an initial composition characterized by a prevalence of brookite (85%) in the as prepared sample, ends up with a dominant anatase phase (75%) after 8 h of thermal treatment ( Table 1).
The DTA curves ( Figure 6B,D) show an endothermic peak, likely due to water loss, appearing during the first 0.1-0.15 h, then, no other significant heat changes are detected, until the end of the experiment.   Figure 7A displays the N2 adsorption/desorption isotherms that are of type IV for all TiO2 NP samples. A very reduced hysteresis loop (H3 or H4 type) is just visible between 0.4 and 0.6 p/p 0 only for TiO2 0 and TiO2 2 h and then at relatively high pressure, ~0.9-1.0 p/p 0 , for all samples. According to the relevant literature [39], such types of hysteresis are usually found in solids forming a slitshaped porous network with non-uniform (H3 type) or uniform (H4 type) size. By increasing the temperature and duration time of the treatment, the isotherm curves, as well the hysteresis loop, become gradually flatter according to a decrease in specific surface area (SSA) and porosity, as a consequence of the particle growth and the inter-particles void drop. The textural parameters derived from N2 physisorption experiments are listed in Tables 3 and 4. The average pore distribution is centered between 3 and 4 nm when the Barrett-Joyner-Halenda (BJH) model is applied and comparable values for the pore diameters were obtained from both adsorption and desorption branches, suggesting the presence of cylindrical pores and/or of interparticles voids with uniform size. In Figure 7B, the pore size distribution as dV/dW (cm 3 /g*nm) vs. pore width (nm) calculated by the Barrett-Joyner-Halenda (BJH) model applied to the desorption curve is shown.
In Figure 8, the cumulative pore volume (cm 3 /g) vs. the pore width (nm) is displayed and the slope of the curves confirms how the duration of the treatment affects the properties of the TiO2 samples.  Figure 7A displays the N 2 adsorption/desorption isotherms that are of type IV for all TiO 2 NP samples. A very reduced hysteresis loop (H3 or H4 type) is just visible between 0.4 and 0.6 p/p 0 only for TiO 2 0 and TiO 2 2 h and then at relatively high pressure,~0.9-1.0 p/p 0 , for all samples. According to the relevant literature [39], such types of hysteresis are usually found in solids forming a slit-shaped porous network with non-uniform (H3 type) or uniform (H4 type) size. By increasing the temperature and duration time of the treatment, the isotherm curves, as well the hysteresis loop, become gradually flatter according to a decrease in specific surface area (SSA) and porosity, as a consequence of the particle growth and the inter-particles void drop. The textural parameters derived from N 2 physisorption experiments are listed in Tables 3 and 4. The average pore distribution is centered between 3 and 4 nm when the Barrett-Joyner-Halenda (BJH) model is applied and comparable values for the pore diameters were obtained from both adsorption and desorption branches, suggesting the presence of cylindrical pores and/or of interparticles voids with uniform size. In Figure 7B, the pore size distribution as dV/dW (cm 3 /g*nm) vs. pore width (nm) calculated by the Barrett-Joyner-Halenda (BJH) model applied to the desorption curve is shown.
In Figure 8, the cumulative pore volume (cm 3 /g) vs. the pore width (nm) is displayed and the slope of the curves confirms how the duration of the treatment affects the properties of the TiO 2 samples. branches, suggesting the presence of cylindrical pores and/or of interparticles voids with uniform size. In Figure 7B, the pore size distribution as dV/dW (cm 3 /g*nm) vs. pore width (nm) calculated by the Barrett-Joyner-Halenda (BJH) model applied to the desorption curve is shown.
In Figure 8, the cumulative pore volume (cm 3 /g) vs. the pore width (nm) is displayed and the slope of the curves confirms how the duration of the treatment affects the properties of the TiO2 samples.   Furthermore, as listed in Table 3, the average sizes of TiO2 particles or agglomerates of crystallites were calculated by means of BET analysis (dBET) using the following equation: dBET = n/ρ × SSA, where ρ is the theoretical density of anatase (3.90 g/cm 3 ), SSA is the specific surface area (m 2 /g) of the TiO2 samples determined by BET measurement and n is the shape factor of the particle, being equal to 6 for a sphere. Such an equation is based on a simplified model, i.e., the surface area of a sample is the sum of the surface of each particle in the sample. Since dBET values agree well with the crystallite size calculated by XRD, it can be inferred that each crystallite in the sample, though assembling in a larger structure and getting in contact with each other, preserve its own individuality, as also confirmed by TEM analysis. The empty space between the aggregate of nearly spherical NPs gives rise to a porous structure due to the occurrence of interparticle voids and the evolution of the resulting texture is clearly pointed out by the results of the BET analysis of the samples. This assumption is consistent with the formation of a mesoporous material [8,40,41], occurring here without any porogenic compound-surfactant molecule-that behave as soft templating agent, able to induce pore formation, that would have, in fact, required a high temperature thermal treatment or, as an alternative, a series of washing steps with strong acid solution. Indeed, the proposed mild thermal treatment, while promoting the anatase phase formation, is suited to prevent the nanocrystals from turning into a more compact material, which is, instead, typical of the much harsher calcination procedure. Furthermore, as listed in Table 3, the average sizes of TiO 2 particles or agglomerates of crystallites were calculated by means of BET analysis (d BET ) using the following equation: d BET = n/ρ × SSA, where ρ is the theoretical density of anatase (3.90 g/cm 3 ), SSA is the specific surface area (m 2 /g) of the TiO 2 samples determined by BET measurement and n is the shape factor of the particle, being equal to 6 for a sphere. Such an equation is based on a simplified model, i.e., the surface area of a sample is the sum of the surface of each particle in the sample. Since d BET values agree well with the crystallite size calculated by XRD, it can be inferred that each crystallite in the sample, though assembling in a larger structure and getting in contact with each other, preserve its own individuality, as also confirmed by TEM analysis. The empty space between the aggregate of nearly spherical NPs gives rise to a porous structure due to the occurrence of interparticle voids and the evolution of the resulting texture is clearly pointed out by the results of the BET analysis of the samples. This assumption is consistent with the formation of a mesoporous material [8,40,41], occurring here without any porogenic compound-surfactant molecule-that behave as soft templating agent, able to induce pore formation, that would have, in fact, required a high temperature thermal treatment or, as an alternative, a series of washing steps with strong acid solution. Indeed, the proposed mild thermal treatment, while promoting the anatase phase formation, is suited to prevent the nanocrystals from turning into a more compact material, which is, instead, typical of the much harsher calcination procedure. In order to get a more comprehensive description of the pore size distribution and shape, pore width values were also calculated by the Gurvitsch method, according to the equation (4V/A), where V is the total pore volume at p/p0 0.98 and A is the BET surface area (see Table 4). According to the relevant literature [42], the BJH method, usually valid for calculating the pore width of cylinders, slits and voids between solid spherical NPs, however, may underestimate in some cases (e.g., gel materials) the size of pores, because it neglects the effect of the curvature of the pore walls on the thickness of the adsorbed gas layer. On the other hand, the Gurvitsch method (4V/A) works well for determining the pore sizes of mesoporous materials with cylindrical pores that have a narrow size distribution [42]. In order to compare the pore-or the intraparticle void-size in the TiO 2 samples, values derived from the BJH and Gurvitsch methods were compared (see Tables 3 and 4).
It is shown that Gurvitsch pore size values are higher than the BJH values found for TiO 2 samples treated for 0.2 and 8 h, respectively, while comparable values were obtained from the two methods for longer thermal treatments, 16 and 24 h. T.
Such a result is consistent with the formation, upon thermal treatment of a stable porous structure where the effect of the curvature of the pore walls upon the thickness of the adsorbed gas layer becomes negligible. Finally, the contribution of micropores to the texture of the TiO 2 samples was evaluated by applying the Horvath-Kavazoe method [43]. On the basis of values listed in Tables 3 and 4, irrespective of the applied model, all the results point to a decrease in surface area and porosity (in terms of interparticle pores or voids, micropores and related pores volume) by increasing the temperature and the duration of treatment. In particular, the main changes in the morphological properties occur at first by increasing the drying temperature from 50 to 110 • C, namely by comparing TiO 2 _0 h and TiO 2 _2 h (TiO 2 _2 h behaves similarly to TiO 2 _8 h), and then increasing the duration of 110 • C treatment from 8 to 16 h. In fact, TiO 2 _16 h TiO 2 _24 h.
In Figure 9, the results of photocatalytic experiments are reported. Since, to best of our knowledge, a standard method for the characterization of photocatalytic efficiency of TiO 2 nanocatalysts in the form of a powder sample is not available, a test was set up on the basis of the conditions reported for the ISO standard 10678 (2010), that has been established for the determination of photocatalytic activity of surfaces in an aqueous medium by degradation of MB. Indeed, the photocatalytic performance of the prepared TiO 2 NP samples was tested by using a light flux of 0.2 mW/cm, a 10 −5 M MB aqueous solution, at pH 6, just in agreement with the ISO standard conditions. In addition, the photocatalytic experiment was performed by using an irradiation source at 254 nm, keeping the solution under constant magnetic stirring, which has been identified as more suited to the peculiar characteristics of the catalysts under investigation, presenting an absorption onset at 345 nm and precipitating from the water dispersion if not properly stirred. Moreover, a standard conditioning time of 30 min in the dark was applied for all samples to achieve a reliable adsorption-desorption equilibrium of MB at the surface of the catalysts.
Catalysts 2020, 10, x FOR PEER REVIEW 11 of 19 nm and precipitating from the water dispersion if not properly stirred. Moreover, a standard conditioning time of 30 min in the dark was applied for all samples to achieve a reliable adsorptiondesorption equilibrium of MB at the surface of the catalysts. In Figure 9, the time course evolution of the MB decoloration assisted by the TiO2 NP samples obtained for increasing thermal treatment duration (panel A) is reported, while in panel B, the histogram showing the percentage of MB decoloration after 120 min of UV irradiation as a function of thermal treatment time is displayed. Negligible degradation is observed in the absence of a catalyst. For all samples, the adsorption of MB was also investigated, and the adsorption measured for all the investigated samples is of ca. (17 ± 5)% after 120 min. The reported data clearly highlight that the prepared TiO2 NPs are photoactive already before any thermal treatment, although with a not exceedingly high decoloration value, (29 ± 5)%. The photocatalytic performance does not significantly improve for the sample thermally treated for 2 h (TiO2_2 h) (28 ± 4)%. The TiO2_8 h sample shows an enhancement of the photocatalytic performance, with (52 ± 3)% of decoloration. A further increase in the duration of the thermal treatment systematically results in an increase in the photocatalytically assisted decoloration, up to (72 ± 4)% for the TiO2_16 h sample. Finally, for the TiO2_24 h sample, no significant difference in the extent of the decoloration ((68 ± 5)%) is observed, being, in fact the difference within the experimental error.
The obtained results point out that the presence of a sufficiently high fraction of anatase phase in the catalyst sample is necessary to have a significant increase in the photocatalytic activity. In fact, the samples TiO2_0 and TiO2_2 h, having a phase composition of 15% anatase-85% brookite and 53% anatase-47% brookite, respectively, present a low photocatalytic activity, in spite of a very high SSA (503 and 354 m 2 /g, respectively). Surprisingly, the TiO2_8 h sample shows a much lower photocatalytic activity (52%) than the TiO2_16 h (72%) and TiO2_24 h (68%) in spite of its higher SSA (350.0 vs. 336.5 and 255.7 m 2 /g, respectively). This evidence can be explained considering that, once the conversion to the anatase phase takes place, there are different properties of the TiO2 samples that may play a role on their photocatalytic activity. A comparison of the characteristics and the photocatalytic efficiency of the TiO2_8 h and TiO2_16 h samples allows us to safely infer that the SSA is not essential in improving the catalytic activity, at least in a certain range. Indeed, SSA decreases as duration of the thermal treatment increases, while the efficiency of the photocatalytic degradation of MB increases with the duration of the thermal treatment of the nanostructured catalyst assisting the decolouration process. It can be noticed that, concomitantly, pore width and volume remain In Figure 9, the time course evolution of the MB decoloration assisted by the TiO 2 NP samples obtained for increasing thermal treatment duration (panel A) is reported, while in panel B, the histogram showing the percentage of MB decoloration after 120 min of UV irradiation as a function of thermal treatment time is displayed. Negligible degradation is observed in the absence of a catalyst. For all samples, the adsorption of MB was also investigated, and the adsorption measured for all the investigated samples is of ca. (17 ± 5)% after 120 min. The reported data clearly highlight that the prepared TiO 2 NPs are photoactive already before any thermal treatment, although with a not exceedingly high decoloration value, (29 ± 5)%. The photocatalytic performance does not significantly improve for the sample thermally treated for 2 h (TiO 2 _2 h) (28 ± 4)%. The TiO 2 _8 h sample shows an enhancement of the photocatalytic performance, with (52 ± 3)% of decoloration. A further increase in the duration of the thermal treatment systematically results in an increase in the photocatalytically assisted decoloration, up to (72 ± 4)% for the TiO 2 _16 h sample. Finally, for the TiO 2 _24 h sample, no significant difference in the extent of the decoloration ((68 ± 5)%) is observed, being, in fact the difference within the experimental error.
The obtained results point out that the presence of a sufficiently high fraction of anatase phase in the catalyst sample is necessary to have a significant increase in the photocatalytic activity. In fact, the samples TiO 2 _0 h and TiO 2 _2 h, having a phase composition of 15% anatase-85% brookite and 53% anatase-47% brookite, respectively, present a low photocatalytic activity, in spite of a very high SSA (503 and 354 m 2 /g, respectively). Surprisingly, the TiO 2 _8 h sample shows a much lower photocatalytic activity (52%) than the TiO 2 _16 h (72%) and TiO 2 _24 h (68%) in spite of its higher SSA (350.0 vs. 336.5 and 255.7 m 2 /g, respectively). This evidence can be explained considering that, once the conversion to the anatase phase takes place, there are different properties of the TiO 2 samples that may play a role on their photocatalytic activity. A comparison of the characteristics and the photocatalytic efficiency of the TiO 2 _8 h and TiO 2 _16 h samples allows us to safely infer that the SSA is not essential in improving the catalytic activity, at least in a certain range. Indeed, SSA decreases as duration of the thermal treatment increases, while the efficiency of the photocatalytic degradation of MB increases with the duration of the thermal treatment of the nanostructured catalyst assisting the decolouration process. It can be noticed that, concomitantly, pore width and volume remain almost unchanged, also upon prolonged thermal treatment. To further elucidate the photocatalytic behaviour of the material, FTIR spectroscopic investigation was carried out on the TiO 2 NP samples throughout the thermal treatment duration. Interestingly, for the three investigated TiO 2 samples (TiO 2 _8 h, TiO 2 _16 h and TiO 2 _24 h; Figure S2), the intensity of the band associated with O-H stretching decreases for prolonged thermal treatment. Such evidence could be consistent with the fact that the amount of OH groups, that are at the surface of the TiO 2 NPs, and that basically derive from the synthetic conditions, being therefore randomly distributed inside and outside TiO 2 NP aggregates, decreases. Such OH groups can be thought to effectively react with the photogenerated holes in the nanocatalyst, thus leading to OH radicals. However, taking into account the size of the aggregates, the surface particles represent a fraction of the total; therefore, it is reasonable to assume that a large fraction of such OH groups is located inside the aggregate, and, thus, have a much lower probability to come in contact with MB and assist its degradation. Conversely, the OH groups located on the inner, less accessible surface of the photocatalyst, may serve rather as hole scavenger than to promote the photocatalytic process. Such an effect becomes evident once the evolution of the crystalline phase composition reached a plateau and the SSA decrease is not dramatic. Prolonging the thermal treatment, i.e., sample TiO 2 _24 h, the intensity of the OH group band in FTIR spectra, and hence their overall amount in the whole sample, further decreases, while an increase in the anatase fraction occurs (81%), thus leading us to assume an overall increase in photocatalytic activity. On the contrary, MB photodegradation occurred to a lower, or at least comparable-considering the experimental error-extent (68 ± 5% vs. 72 ± 4% for TiO 2 _16 h). Such results could be accounted for by the strong decrease in SSA that drops to 255.7 m 2 /g, with a loss in SSA of 81 m 2 /g with respect to TiO 2 _16 h. It can be proposed that such a loss may counterbalance the increase in photocatalytic performances expected from the decrease in OH groups on the inner surface of the aggregate, thus finally resulting in a comparable photocatalytic activity.
Finally, a comparison of the photocatalytic performance of the TiO 2 _16 h, thermally treated at 110 • with that recorded for a sample prepared using the same preparative conditions, but introducing a calcination step at 450 • C for 2 h [22] (referred to as TiO 2 _450 • C in the following), shows that the former performs much better than the sample calcinated at 450 • C, with a 1.5% increase in the photodegradation percentage ( Figure 10).
Catalysts 2020, 10, x FOR PEER REVIEW  12 of 19 almost unchanged, also upon prolonged thermal treatment. To further elucidate the photocatalytic behaviour of the material, FTIR spectroscopic investigation was carried out on the TiO2 NP samples throughout the thermal treatment duration. Interestingly, for the three investigated TiO2 samples (TiO2_8 h, TiO2_16 h and TiO2_24 h; Figure S2), the intensity of the band associated with O-H stretching decreases for prolonged thermal treatment. Such evidence could be consistent with the fact that the amount of OH groups, that are at the surface of the TiO2 NPs, and that basically derive from the synthetic conditions, being therefore randomly distributed inside and outside TiO2 NP aggregates, decreases. Such OH groups can be thought to effectively react with the photogenerated holes in the nanocatalyst, thus leading to OH radicals. However, taking into account the size of the aggregates, the surface particles represent a fraction of the total; therefore, it is reasonable to assume that a large fraction of such OH groups is located inside the aggregate, and, thus, have a much lower probability to come in contact with MB and assist its degradation. Conversely, the OH groups located on the inner, less accessible surface of the photocatalyst, may serve rather as hole scavenger than to promote the photocatalytic process. Such an effect becomes evident once the evolution of the crystalline phase composition reached a plateau and the SSA decrease is not dramatic. Prolonging the thermal treatment, i.e., sample TiO2_24 h, the intensity of the OH group band in FTIR spectra, and hence their overall amount in the whole sample, further decreases, while an increase in the anatase fraction occurs (81%), thus leading us to assume an overall increase in photocatalytic activity. On the contrary, MB photodegradation occurred to a lower, or at least comparable-considering the experimental error-extent (68 ± 5% vs. 72 ± 4% for TiO2_16 h). Such results could be accounted for by the strong decrease in SSA that drops to 255.7 m 2 /g, with a loss in SSA of 81 m 2 /g with respect to TiO2_16 h. It can be proposed that such a loss may counterbalance the increase in photocatalytic performances expected from the decrease in OH groups on the inner surface of the aggregate, thus finally resulting in a comparable photocatalytic activity. Finally, a comparison of the photocatalytic performance of the TiO2_16 h, thermally treated at 110° with that recorded for a sample prepared using the same preparative conditions, but introducing a calcination step at 450 °C for 2 h [22] (referred to as TiO2_450 °C in the following), shows that the former performs much better than the sample calcinated at 450 °C, with a 1.5% increase in the photodegradation percentage ( Figure 10). Such behaviour is particularly interesting when considering the crystal phase of the samples. Indeed, it looks like that the sample calcined at 450 °C, and due to the preparative conditions, it is entirely anatase in phase with a SSA of 69.1 m 2 /g [22], while the sample obtained after a lowtemperature treatment presents a small fraction of brookite and a much higher SSA (336.5 m 2 /g). Such behaviour is particularly interesting when considering the crystal phase of the samples. Indeed, it looks like that the sample calcined at 450 • C, and due to the preparative conditions, it is entirely anatase in phase with a SSA of 69.1 m 2 /g [22], while the sample obtained after a low-temperature treatment presents a small fraction of brookite and a much higher SSA (336.5 m 2 /g). Therefore, the prevalence of the anatase phase does not appear to be a sufficiently decisive factor to explain alone the photocatalytic activity of the photocatalyst, but it is rather a specific combination of different structural, chemical and morphological characteristics that contribute to defining the photocatalytic behaviour [44,45]. Remarkably, this comparison highlights how a low-temperature procedure may be much more effective than a process carried out at high temperature, with an evident technological advantage in terms of requirements for the materials manufacturing. Finally, we performed additional experiments to compare the photocatalytic performance of our samples with that of TiO 2 P25, tested as a commercial benchmark. The results of the comparison, reported in the Supporting Information ( Figures S3 and S4), point out that the decoloration extent for the reaction assisted by TiO 2 P25 (83 ± 5%) is slightly higher than that obtained when the TiO 2 _16 h sample is used (72 ± 4%). However, a decisive assessment could not be safely performed, considering the different characteristics of the investigated photocatalyst with respect to the commercially available counterpart.

Synthesis of TiO 2 Nanoparticles
The synthesis of TiO 2 nanoparticles (NPs) used of TiOSO 4 as TiO 2 precursor, that was selected due to its cost effectiveness, and exploited a simple precipitation method in alkaline aqueous solution. Briefly, 50 mL of 0.64 M TiOSO 4 solution were added dropwise in 76 mL of 2.00 M NH 4 HCO 3 solution. After the complete mixing, the pH of the solution was adjusted to pH 8 by adding a proper amount of 2.00 M NH 4 HCO 3 . The obtained precipitate was repeatedly washed by subsequent cycles of dispersion in water and centrifugation at 3000 rpm. Afterwards, the product was thermally treated in oven at 110 • C to promote crystallization and to enhance the photocatalytic properties. A systematic study of the effect of the thermal treatment time was performed in the time range 2-24 h. The samples treated for 2-8-16-24 h were characterized by SEM, TEM, XRD, BET and photocatalytic experiments.

UV-Vis Absorbance Spectroscopy and Diffuse Reflectance Spectroscopy
UV-Vis absorption spectra and diffuse reflectance (DR) spectra were recorded with a UV-Vis-NIR Cary 5 (Agilent Technologies, Inc., Santa Clara, CA, USA) spectrophotometer. DR spectra were plotted in Kubelka-Munk (KM) arbitrary unit vs. wavelength. Band gap energy (Eg) was calculated by graphical extrapolation. Plotting a modified Kubelka-Munk function as a function of energy, the Eg was measured from the value of the intercept between the tangent of the curve and the axis on which the energies are reported [24].

FTIR Spectroscopy
Fourier transform infrared (FTIR) spectra of TiO 2 samples were recorded using a Perkin-Elmer Spectrum One spectrometer (Waltham, MA, USA) equipped with a deuterated tryglicine sulfate (DTGS) detector. Spectra were collected with a resolution of 4 cm −1 operating in Attenuated Total Reflection (ATR) mode, using a three-bounce 4 mm-diameter diamond microprism as internal reflection element (SensIR technologies). Powders were cast directly onto the internal reflection element, carefully covering the upper face of the diamond crystal. The spectra for all experiments were collected with a resolution of 4 cm −1 in the range 2300-4000 cm −1 .

Thermogravimetry
TGA experiments were carried out with a TGA/DSC1 STAR system (Mettler Toledo, Bristol, UK). The sample TiO 2 0 h T.T (10 mg) was fast heated from room temperature up to 110 • C (heating ramp of 90 • C/min) under air flow (30 mL/min), then was treated under the same air flow at 110 • C for 2 and 8 h, respectively, in order to monitor the weight loss and heat-flow occurring under the oven drying conditions used for the treatment of the TiO 2 samples.

Specific Surface Area and Pore Size Distribution
Specific surface area (SSA) and pore size distribution of the samples were determined by N 2 adsorption-desorption isotherms at −196 • C using ASAP 2020 Plus Micromeritics (Norcross, GA, USA). All the samples were pre-treated under vacuum at 80 • C for 2 h prior to the measurements, except the sample labelled as TiO 2 0 h T.T, which was pre-treated under vacuum at 25 • C for 2 h. The specific surface area was calculated using the Brunauer-Emmett-Teller (BET) method applied to the adsorption branch in the range 0.05-0.30 p/p0 [46]. The pore size distribution and cumulative pore volume vs. pore size were determined by comparing different methods, the Barrett-Joyner-Halenda (BJH) [47], the Gurvitsch [42] and the Horvath-Kavazoe methods [43]. The total pore volume of pores with sizes less than 50 nm was also estimated from single point desorption at p/p0 equal to 0.98. The obtained textural parameters were quoted with a precision of ±10%.

Transmission Electron Microscopy Investigation
Transmission electron microscopy (TEM) analysis was performed by means of a JEOL JEM-1011 (JEOL, Akishima, Tokyo, Japan) microscope operating at 100 kV. The TEM samples were prepared by casting a drop of TiO 2 methanol solution onto a carbon hollowed TEM grid. High-resolution transmission electron microscopy (HRTEM) imaging and STEM/EDS analyses (scanning transmission electron microscopy/energy dispersive spectroscopy) was carried out on a JEOL JEM-2200FS TEM (Schottky emitter), equipped with a CEOS C S corrector for the objective lens, and an in-column image filter (Ω-type), operated at 200 kV.

Scanning Electron Microscopy Investigation
Field emission scanning electron microscopy (FE-SEM) was performed by using a Zeiss Sigma microscope (Carl Zeiss Co., Oberkochen, Germany) operating in the range 0.5-20 kV and equipped with an in-lens secondary electron detector and an INCA Energy Dispersive Spectroscopy (EDS) detector. FE-SEM samples were prepared by casting a few drops of nanoparticle suspension in ethanol onto a silicon slide. Samples were mounted onto stainless-steel sample holders by using double-sided carbon tape and grounded by silver paste.

XRD Characterization
XRD patterns were recorded with a D8-Discover Bruker diffractometer (Bruker AXS GmbH, Karlsruhe, Germany) equipped with a Cu source (operated at 40/40 mA/kV), a Goebel mirror, an Eulerian cradle goniometer, and a scintillator detector. The samples were prepared by depositing the sample from a concentrated colloidal dispersion onto a silicon substrate, and then allowing the solvent to evaporate. XRD patterns were collected, in 2θ scan mode with a fixed incident angle of 5 • , moving the detector over the 2θ range 10 • -120 • with a step size of 0.05 • .
The XRD patterns were analyzed by a whole-profile Rietveld based fitting program (FULLPROF) [48] to evaluate the crystalline domain apparent size at different heating time as reported in Table 2.
A quantitative phase analysis was also carried out to obtain the structural models of mixed compounds, by Rietveld method by using Quanto [49], a Rietveld program specialized for quantitative phase analysis (QPA) of polycrystalline mixtures.

Photocatalytic Experiments
The photocatalytic activity of the prepared TiO 2 samples was evaluated in an aqueous water suspension under UV light irradiation. (λ = 254 nm; light flux 0.2 mW/cm 2 determined by radiometer (Delta Ohm Data Logger) 9721), using an organic dye, methylene blue (MB) as a model target compound. The TiO 2 powder was suspended in a glass beaker containing a 10 −5 M MB solution in milliQ water at pH 6. The pH value was carefully adjusted by the addition of HCl 0.1M and NaOH 0.1M. The MB-TiO 2 dispersion was left to stir in the dark for 30min to reach the adsorption-desorption equilibrium. Afterward, the suspension was irradiated under continuous stirring by a UV fluorescent lamp located at a distance of 6 cm over the beaker surface. At scheduled time intervals, aliquots were collected, purified by centrifugation, and the MB concentration was estimated by absorption spectroscopy as a function of reaction time. The percentage of decoloration as a function of reaction time was calculated using the following equation: As control experiments, the MB adsorption in the dark and the direct photolysis of MB, respectively, were investigated.

Conclusions
The decomposition of a cost effective precursor, TiOSO 4 in aqueous alkaline solution, at room temperature, followed just by a mild thermal treatment in oven (110 • C) has been established as a valuable synthetic approach able to supply mesoporous TiO 2 NPs in the gram-scale, without adding any templating, porogen agent. Optical (DRS), morphologic (TEM, SEM), physical chemical (TGA, DSC, BET) and structural (XRD, HRTEM) investigations demonstrated the possibility to tune the properties of the catalyst as a function of thermal treatment duration. The prepared nanostructured material was shown to be an effective photocatalyst able to assist in the UV-induced degradation of MB, the model compound selected for the photocatalytic test. The investigation has highlighted the strong interplay of the different characteristics, namely surface area, crystalline phase, and surface chemistry, of the prepared nanomaterials in defining their photocatalytic properties. Moreover, the comparison of photocatalytic behavior of two samples, prepared by using the same procedure, but then thermally treated in an oven at 110 • C and calcined at 450 • C, respectively, show the advantage of the mild treatment against the harsher calcination step. Overall, the presented results demonstrate that the proposed approach offers a facile and sustainable route to promptly access a photocatalyst, that may be used in technologically viable systems for the photocatalytic degradation of organic compounds, thus definitely representing a step forward toward the real application of TiO 2 -based photocatalysis in the field of environmental depollution. Funding: This work was partially supported by the Italian Apulia Region funded "FontanApulia" (WOBV6K5) and by the Italian PON MIUR "Energy for TARANTO" (Proposal Code ARS01_00637) projects.