Consideration of Photoactivity of TiO2 Pigments via the Photodegration of Methyl Orange under UV Irradiation

Developing a rapid and reliable method for measuring the photoreactivity of TiO2 pigments is of great importance for industrial application. The photoactivity of industrial TiO2 pigments were evaluated via the photodegradation of a model azo dye, methyl orange (MO), in the present work. The TiO2 pigments were characterized by Fourier-transform infrared spectroscopy (FTIR), ultraviolet–visible (UV–vis) spectroscopy, scanning electron microscopy (SEM), and photoluminescence (PL) spectroscopy. The photoactivity test results showed that the anatase TiO2 pigment was responsible for accelerating MO degradation, while the rutile pigment acted as a stabilizer, and effective UV absorber retarded the photodegradation of MO. It was found that the photodegradation of MO was driven mainly by photoholes (h+) and hydroxyl radicals (•OH), in the presence of TiO2 pigment with high photoactivity. With the help of the degradation intermediates during the photodegradation process and the calculated data, the preliminary degradation mechanism including azo bond cleaving, h+ oxidation, and hydroxylated products’ generation for MO was also elucidated. The photoactivity of TiO2 pigments can be rapidly evaluated in this work, which would be an efficient approach for assessing the product quality control and the end-use performance of TiO2 pigments.


Introduction
Titanium dioxide (TiO 2 ) is an important chemical material that is extensively utilized in coatings, rubber, plastics, and paper due to its excellent properties of higher whiteness, gloss, and refractive index, which better cover power and UV absorption performance [1,2]. The global production of TiO 2 reached almost 8.0 million tons in 2021 [3], and it is projected to reach 8.8 million tons by 2025 [4]. The biggest consumer of TiO 2 is the pigment industry, which is ca. 95% of the world's consumption of titanium dioxide [5].
It is well-known that TiO 2 can generate electron-hole pairs when irradiated with photons, with energy that is equal to or greater than its band gap energy [6,7]. The generated reactive species, such as holes (h + ), hydroxyl radicals (•OH), and superoxide radicals (O 2 •− ), are commonly believed to be highly reactive radicals for the decomposition of organic molecules [8][9][10][11]. If bare TiO 2 is directly used in outdoor application, the photocatalyzed behavior of TiO 2 will lead, either directly or indirectly, to the organic materials' discoloration or even total destruction [12,13]. The applications of pure TiO 2 particles with a high level of photocatalytic activity were severely limited in the paint, coating, and plastic [14]. In order to suppress the photoactivity of titanium dioxide, while maintaining its UV-shielding performance, inert oxides such as SiO 2 [15,16], Al 2 O 3 [17,18], ZrO 2 [19], and CeO 2 [20] and organic treatments have usually been applied to coat the titanium dioxide surface. Several recent studies, however, have demonstrated that the photoreactivity of titanium dioxide pigment remains one of the most important influential factors for coatings degradation [13,21,22].
Previous studies have focused on various physical changes such as weight loss, discoloration, and gloss retention in a coating film, through an artificial accelerated aging test or outdoor exposure test to evaluate the photoactivity performance of industrial TiO 2 pigments [23][24][25]. These physical changes, however, often take hundreds or thousands of hours to appear. Besides, the analysis of intermediate products about such a solid sample is difficult. In recent years, the formation of CO 2 (ca. 2360 cm −1 ) that is caused by the photocatalytic oxidation in a polymer film can be monitored by FTIR spectroscopy [26]. Other methods, such as time-resolved photoluminescence spectroscopy measurement [27], electron paramagnetic resonance (EPR) analysis [28], and the photoelectrochemical approach [29] have also been proposed. However, the above-mentioned studies required tedious operation, a long amount of time, or expensive equipment. In addition, the test method, which used Rhodamine-B or Acid Blue 9 degradation to evaluate the photostability of TiO 2 particles, uncoated or coated by metal oxides, also required a very long measurement time [30,31]. It is worth noting that some characteristic results of the photoactivities of various commercial TiO 2 pigments are usually ambiguous [32]. Thus, it seems pretty difficult to assess and select the appropriate TiO 2 pigments because little information about the photoactivity of TiO 2 pigments was provided from the perspective of the degradation mechanism [33]. Therefore, developing a rapid and reliable method for measuring the photoreactivity of TiO 2 pigment would be desirable.
In the present work, commercial TiO 2 pigments were used and characterized by ultraviolet-visible (UV-vis), Fourier-transform infrared (FTIR), scanning electron microscopy (SEM), and photoluminescence (PL) spectroscopy. The apparent photoactivities of TiO 2 pigments were evaluated utilizing methyl orange (MO), which acted as a model molecule under ultraviolet irradiation in an aqueous solution. During the photodegradation process, the contributions of reactive species, e.g., holes and hydroxyl radicals, were further investigated. The preliminary degradation mechanism of MO was also elucidated via the identified intermediates by gas chromatography-mass spectrometry (GC-MS) and theoretical calculation by Gaussian. This is expected to identify the various TiO 2 pigments and provide the referential information for the application of TiO 2 pigments.

Materials
The industrial TiO 2 pigments were purchased from Hunan Zhuzhou Chemical Group Co., Ltd. (Zhuzhou, China) and labeled as P1, P2, and P3 in this work, with their corresponding information listed in Table 1. Methyl orange (C 14 H 14 N 3 SO 3 Na, purity > 99%) was obtained from Tianjin Damao Chemical Reagent Co. Inc. Other chemicals such as silver nitrate (AgNO 3 ), potassium iodide (KI), methanol (MeOH), and isopropanol (IPA) were of analytical grade and were used as received without further purification. Water was prepared by a Millipore Milli-Q ultrapure water-purification system.

TiO 2 Pigment Characterization
The FTIR spectra of the samples were collected by the KBr pellet technique on a Nicolet 370 Fourier-transform infrared spectrophotometer in the range of 500-4000 cm −1 . The morphologies of the samples were tested by scanning electron microscopy on a MIRA3 TESCAN using an accelerating voltage of 20 kV. The UV-vis transmittance spectra of TiO 2 pigments were obtained on a Hitachi U-3010 spectrophotometer with an integrating sphere. PL spectra were obtained on a Hitachi F-4500 fluorometer with the excitation at 300 nm, slit width of 5.0 nm, multiplier voltage of 700 V, and scanning region of 300-550 nm.

Photoactivity Tests
The photoactivity tests were carried out in a quartz reactor (total volume ca. 70 mL). The light source was a 300 W medium-pressure mercury lamp (λ max = 365 nm, Philips, Saarbrücken, Germany) with a double-walled cooling-water jacket housed in one side of the reactor to provide the irradiation. The experimental device is schematically shown in Figure 1.
MIRA3 TESCAN using an accelerating voltage of 20 kV. The UV-vis transmittance spectra of TiO2 pigments were obtained on a Hitachi U-3010 spectrophotometer with an integrating sphere. PL spectra were obtained on a Hitachi F-4500 fluorometer with the excitation at 300 nm, slit width of 5.0 nm, multiplier voltage of 700 V, and scanning region of 300-550 nm.

Photoactivity Tests
The photoactivity tests were carried out in a quartz reactor (total volume ca. 70 mL). The light source was a 300 W medium-pressure mercury lamp (λmax = 365 nm, Philips, Saarbrücken, Germany) with a double-walled cooling-water jacket housed in one side of the reactor to provide the irradiation. The experimental device is schematically shown in Figure 1. A volume of 35 mL of solution containing 30 μmol/L of MO was added to the quartz reactor with 35 mg of TiO2 pigment powder. Before exposure to UV radiation, the suspension was magnetically stirred in the dark for 30 min. During the photodegradation process, about 2 mL of the reaction solutions was obtained at regular intervals and centrifuged to remove TiO2 pigment. The concentration of MO was analyzed using UV-vis spectrophotometer and calculated from the standard calibration for the characteristic λmax of MO. The degradation efficiency was calculated according to the equation: X (%) = (C0 − Ct)/C0 × 100%, where C0 is the initial concentration of MO, and Ct is the concentration of MO after photoirradiation for t minutes. All the MO degradation experiments were performed at least in triplicate, and average data are presented.
The degradation intermediates in the photodegradation process were identified by gas chromatography-mass spectrometry (GC-MS) method. Shimadzu GC system equipped with a capillary (30 m length, 0.32 mm internal diameter, 0.25 μm film thickness) was used. Helium was used as a carrier gas at a flow rate of 1 mL/min. The oven temperature program was as follows: 3 min isothermal at 100 °C, ramped from 100 to 260 °C at a rate of 10 °C/min, and held at 300 °C for 10 min. The NIST05S.LIB library was used for the mass spectrum analysis.

Theoretical Calculations
Theoretical calculations were carried out by density functional theory (DFT) method (B3LYP) with the 6-31G (d,p) basis set using the Gaussian 09 program (Gaussian, Inc., Wallingford, CT, USA). The point charges (PC) of MO were calculated to predict the chemisorption position of MO onto the surface of TiO2 pigment.  A volume of 35 mL of solution containing 30 µmol/L of MO was added to the quartz reactor with 35 mg of TiO 2 pigment powder. Before exposure to UV radiation, the suspension was magnetically stirred in the dark for 30 min. During the photodegradation process, about 2 mL of the reaction solutions was obtained at regular intervals and centrifuged to remove TiO 2 pigment. The concentration of MO was analyzed using UV-vis spectrophotometer and calculated from the standard calibration for the characteristic λ max of MO. The degradation efficiency was calculated according to the equation: X (%) = (C 0 − C t )/C 0 × 100%, where C 0 is the initial concentration of MO, and C t is the concentration of MO after photoirradiation for t minutes. All the MO degradation experiments were performed at least in triplicate, and average data are presented.
The degradation intermediates in the photodegradation process were identified by gas chromatography-mass spectrometry (GC-MS) method. Shimadzu GC system equipped with a capillary (30 m length, 0.32 mm internal diameter, 0.25 µm film thickness) was used. Helium was used as a carrier gas at a flow rate of 1 mL/min. The oven temperature program was as follows: 3 min isothermal at 100 • C, ramped from 100 to 260 • C at a rate of 10 • C/min, and held at 300 • C for 10 min. The NIST05S.LIB library was used for the mass spectrum analysis.

Theoretical Calculations
Theoretical calculations were carried out by density functional theory (DFT) method (B3LYP) with the 6-31G (d,p) basis set using the Gaussian 09 program (Gaussian, Inc., Wallingford, CT, USA). The point charges (PC) of MO were calculated to predict the chemisorption position of MO onto the surface of TiO 2 pigment.

TiO 2 Pigment Characterization
The FTIR spectra of TiO 2 samples are displayed in Figure 2. The broader peak at 3460 cm −1 was attributed to the stretching vibration and bending vibration of hydroxyl groups [34]. The other peak at 1630 cm −1 was attributed to the bending vibration of H-O-H. In addition, a peak in the range of 500-800 cm −1 is generally related to the stretching vibration modes of Ti-O-Ti bands [35]. In the FTIR spectra, both P1 and P3 showed new peaks at 1080 cm −1 and 1600 cm −1 , which are characteristic of SiO 2 and Al 2 O 3 [36]. However, the photoholes (h + ) induced by UV light would oxidize surface hydroxyl groups onto the TiO 2 surface to generate •OH radicals, if the TiO 2 surface was not coated completely. In that case, the TiO 2 pigments are likely to participate in organic substrate degradation under UV irradiation.
groups [34]. The other peak at 1630 cm −1 was attributed to the bending vibration of H-O-H. In addition, a peak in the range of 500-800 cm −1 is generally related to the stretching vibration modes of Ti-O-Ti bands [35]. In the FTIR spectra, both P1 and P3 showed new peaks at 1080 cm −1 and 1600 cm −1 , which are characteristic of SiO2 and Al2O3 [36]. However, the photoholes (h + ) induced by UV light would oxidize surface hydroxyl groups onto the TiO2 surface to generate •OH radicals, if the TiO2 surface was not coated completely. In that case, the TiO2 pigments are likely to participate in organic substrate degradation under UV irradiation.  Figure 3b clearly demonstrates that the size range of P2 was widely from several micrometers to tens of micrometers, and P2 has a relatively smooth surface. As indicated by the arrow in Figure 3c, the surface of TiO2 was coated by amorphous silica and alumina coating layers, which was consistent with the FTIR analysis. Transmittance (a.u.) SEM images of TiO 2 pigments are shown in Figure 3. The shape of P1 was spherical, and the size of P1 was approximately 200 nm ( Figure 3a). Figure 3b clearly demonstrates that the size range of P2 was widely from several micrometers to tens of micrometers, and P2 has a relatively smooth surface. As indicated by the arrow in Figure 3c, the surface of TiO 2 was coated by amorphous silica and alumina coating layers, which was consistent with the FTIR analysis. UV-vis spectra of TiO2 pigments are shown in Figure 4. The increase in transmittance in the UV region (280-400 nm) suggests the decrease in UV-shielding ability. The UV-shielding ability of P3 decreased slightly compared to the original P2. This may be because the point defects in both amorphous Al2O3 and SiO2 on the surface of the TiO2 particles can absorbe UV light in this region [37,38]. The UV-shielding ability of the rutile TiO2 pigment P3 was better than that of the anatase TiO2 pigment P1, because the former could absorb UV light up to 400 nm, while the latter only showed UV-vis spectra of TiO 2 pigments are shown in Figure 4. The increase in transmittance in the UV region (280-400 nm) suggests the decrease in UV-shielding ability. The UVshielding ability of P3 decreased slightly compared to the original P2. This may be because the point defects in both amorphous Al 2 O 3 and SiO 2 on the surface of the TiO 2 particles can absorbe UV light in this region [37,38]. The UV-shielding ability of the rutile TiO 2 pigment P3 was better than that of the anatase TiO 2 pigment P1, because the former could absorb UV light up to 400 nm, while the latter only showed significant absorption up to 380 nm. Importantly, the rutile phase was likely to be much lower apparent photoreactivity than the anatase phase under UV irradiation [13]. Thus, the rutile-based pigment with UV absorption performance and lower photoreactivity can act as an effective UV absorber in the polymer coatings. UV-vis spectra of TiO2 pigments are shown in Figure 4. The increase in transmittance in the UV region (280-400 nm) suggests the decrease in UV-shielding ability. The UV-shielding ability of P3 decreased slightly compared to the original P2. This may be because the point defects in both amorphous Al2O3 and SiO2 on the surface of the TiO2 particles can absorbe UV light in this region [37,38]. The UV-shielding ability of the rutile TiO2 pigment P3 was better than that of the anatase TiO2 pigment P1, because the former could absorb UV light up to 400 nm, while the latter only showed significant absorption up to 380 nm. Importantly, the rutile phase was likely to be much lower apparent photoreactivity than the anatase phase under UV irradiation [13]. Thus, the rutile-based pigment with UV absorption performance and lower photoreactivity can act as an effective UV absorber in the polymer coatings.   Figure 5 displays the PL spectra of TiO 2 pigments. It is known that the PL signals of semiconductor particles mainly result from the recombination of photoinduced charge carriers. Commonly, lower PL intensity indicates a lower recombination rate of photoinduced electron-hole pairs and, thus, higher photocatalytic activity [39][40][41]. The anatase-based pigment P1 gave a strong emission band with a wavelength maximum at 390 nm, whereas the rutile-based pigment for both P2 and P3 gave strong emission bands with a wavelength at ca. 415 and ca. 470 nm, respectively. These differences may be attributed to the different crystalline structure of TiO 2 particles. It can be seen that the SiO 2 /Al 2 O 3 coating layer did not influence the PL spectra of TiO 2 pigment. Several excitonic PL peaks illustrated that the surface states or defects of the TiO 2 pigment were abundant [27].
Materials 2022, 14, x FOR PEER REVIEW 6 of 12 Figure 5 displays the PL spectra of TiO2 pigments. It is known that the PL signals of semiconductor particles mainly result from the recombination of photoinduced charge carriers. Commonly, lower PL intensity indicates a lower recombination rate of photoinduced electron-hole pairs and, thus, higher photocatalytic activity [39][40][41]. The anatase-based pigment P1 gave a strong emission band with a wavelength maximum at 390 nm, whereas the rutile-based pigment for both P2 and P3 gave strong emission bands with a wavelength at ca. 415 and ca. 470 nm, respectively. These differences may be attributed to the different crystalline structure of TiO2 particles. It can be seen that the SiO2/Al2O3 coating layer did not influence the PL spectra of TiO2 pigment. Several excitonic PL peaks illustrated that the surface states or defects of the TiO2 pigment were abundant [27].

Photoactivity Tests
The maximum absorption at 464 nm is a characteristic peak of the π-π* transition of azo bonds (-N=N-). The peak at 280 nm corresponds to the π-π* transition of the benzyl ring. As shown in Figure 6a, the peak at 464 nm shifted towards the low absorbance values with the increase in illumination time for P1. As described above, the loss in the spectral features of the MO reveals the start of decomposition. However, a blank experiment was performed under UV irradiation in the absence of TiO2 pigments, and

Photoactivity Tests
The maximum absorption at 464 nm is a characteristic peak of the π-π* transition of azo bonds (-N=N-). The peak at 280 nm corresponds to the π-π* transition of the benzyl ring. As shown in Figure 6a, the peak at 464 nm shifted towards the low absorbance values with the increase in illumination time for P1. As described above, the loss in the spectral features of the MO reveals the start of decomposition. However, a blank experiment was performed under UV irradiation in the absence of TiO 2 pigments, and the degradation rate was 7.0% in 50 min. The photodegradation efficiency of MO over various TiO 2 pigments was compared, and the results re shown in Figure 6b. Both P2 and P3 exhibit the negligible activity for photodegradation of MO. Moreover, P3 showed a more significant inhibitory effect for the degradation of MO than that of P2, suggesting that the coated rutile pigments with suppression of photoactivity can act as a stabilizer and effective UV absorber [42]. On the contrary, the TiO 2 pigment P1, the form of anatase, has a significant photoreactivity under UV irradiation, in spite of its surface being coated by SiO 2 /Al 2 O 3 , showing 95.0% photocatalytic degradation for MO after 50 min of irradiation. The abovementioned results suggest that the photoactivity of the commercial TiO 2 pigments can be rapidly evaluated and decrease in the order P1 > P2 > P3. These experimental results were consistent with our previously reported findings [43].

Photodegradation Mechanism
The scavengers for holes and hydroxyl radical were further employed to investigate the photoactivity of TiO2 pigments. When KI, which was often used as a hole-capturer [44], was added to the reaction system, the degradation efficiency of MO was suppressed and reduced to 74.4%. As a well-known hydroxyl radical scavenger, the addition of IPA decreased the degradation efficiency to 79.8%. MeOH was reported to serve as an

Photodegradation Mechanism
The scavengers for holes and hydroxyl radical were further employed to investigate the photoactivity of TiO 2 pigments. When KI, which was often used as a hole-capturer [44], was added to the reaction system, the degradation efficiency of MO was suppressed and reduced to 74.4%. As a well-known hydroxyl radical scavenger, the addition of IPA decreased the degradation efficiency to 79.8%. MeOH was reported to serve as an alternative hole and hydroxyl radical scavenger [45]. The degradation rate of MO, however, was significantly improved when 1.0 mol/L methanol was added, which seems to be in contradiction to the expected result. This observation can be explained on the basis that a large excess of methanol reacts rapidly with both h + and •OH, generating •OCH 3 radicals that can be trapped by O 2 . As a result, HO 2 • radicals were generated, which are of an important intermediate active species in the solution. The photodegradation of MO was further investigated in the presence of an electron scavenger (Ag + ions). Figure 7 depicts that the addition of Ag + ions can greatly promote the degradation of MO. In total, 96.1% of MO was degraded after irradiation for only 20 min. This is because the silver ion is a strong electron acceptor [E 0 (Ag + /Ag) = 0.80 V NHE ] that increases the lifetime of holes and electrons [46], resulting in improving the oxidation rate of MO. The above-mentioned results indicate that the degradation of MO was driven by h + and •OH radicals.  After the exploration of active species during the MO photodegradation process, we also tried to elucidate the photodegradation mechanism of MO in the presence of a highly photoactive pigment. The experiments were conducted using 30 μmol/L solutions of MO in the presence of P1 under UV irradiation, and the main degradation intermediates were identified by GC-MS. The GC-MS chromatogram is given in Figure  S1. The m/z peak at 304 can be attributed to the ionization of the dye molecule. Two degradation intermediates with m/z peaks at 166 (denoted as compound I) and 172 (denoted as compound II) may be attributed to the substituted aromatic amines. The theoretical atomic point charges of MO were computed to predict initial attack site, and the corresponding data are listed in Table 2. It can be seen from the table that the most negative point charges were located at C2 (−0.886), C13 (−0.776), while a more positive charges was found for N7. The azo group (-N=N-), therefore, was apt to be absorbed on the surface of TiO2 pigments, attacked by photoholes, and decomposed. Additionally, the electrophilic nature of •OH radicals was also apt to attack the azo group, which has the higher electron density [47]. So, the characteristic peak at 464 nm (in Figure 6a), shifting toward the low absorbance values, increased in the duration time of illumination. The cleavage of the -N=N-double bond was consistent with the previous results [45,48]. Besides, MO can be adsorbed on the TiO2 pigment's surface via the sulfonate group, due to the negative point charges located on the oxygen atoms of O19, O20, and O21 [49]. The photodegradation pathways for MO are shown in Figure 8 After the exploration of active species during the MO photodegradation process, we also tried to elucidate the photodegradation mechanism of MO in the presence of a highly photoactive pigment. The experiments were conducted using 30 µmol/L solutions of MO in the presence of P1 under UV irradiation, and the main degradation intermediates were identified by GC-MS. The GC-MS chromatogram is given in Figure S1. The m/z peak at 304 can be attributed to the ionization of the dye molecule. Two degradation intermediates with m/z peaks at 166 (denoted as compound I) and 172 (denoted as compound II) may be attributed to the substituted aromatic amines. The theoretical atomic point charges of MO were computed to predict initial attack site, and the corresponding data are listed in Table 2. It can be seen from the table that the most negative point charges were located at C2 (−0.886), C13 (−0.776), while a more positive charges was found for N7. The azo group (-N=N-), therefore, was apt to be absorbed on the surface of TiO 2 pigments, attacked by photoholes, and decomposed. Additionally, the electrophilic nature of •OH radicals was also apt to attack the azo group, which has the higher electron density [47]. So, the characteristic peak at 464 nm (in Figure 6a), shifting toward the low absorbance values, increased in the duration time of illumination. The cleavage of the -N=N-double bond was consistent with the previous results [45,48]. Besides, MO can be adsorbed on the TiO 2 pigment's surface via the sulfonate group, due to the negative point charges located on the oxygen atoms of O19, O20, and O21 [49]. The photodegradation pathways for MO are shown in Figure 8. •OH radicals (oxidation potential: 2.8 V) are stronger oxidants that can oxidize organics by the abstraction of protons generating organic radicals (R•), which can be further oxidized [48]. Moreover, the S15-C10 bond (1.8431 Å), N16-C17 bond (1.4735 Å), and N16-C18 bond (1.4737 Å) are longer than the other C-C bonds (ca. 1.44 Å), which indicated that the corresponding groups were more easily removed than the C-C groups. The degradation intermediate with m/z = 197 (denoted as compound III) may be attributed to the loss of the sulfonic group and methyl group during the photodegradation process. The degradation intermediate with m/z = 156 (denoted as compound IV) may be generated from (II) by further loss of -NH 2 . Eventually, the mineralization of MO by stepwise advance oxidation leads to the production of small molecules and ions such as CO 2 , H 2 O, SO 4 2− , NO 3 − , NH 4 + , etc. [50]. These results indicated that •OH radicals and photoholes exhibited the major contributions to the degradation of MO, which provides powerful evidence for the photocatalytic performance of TiO 2 pigment. This is mainly due to the fact that the SiO 2 /Al 2 O 3 coating layers did not completely cover all the TiO 2 surface in the industrial production process. The roles of TiO 2 pigments relating to the paint film would also be predicted in actual usage using this method. It is, therefore, believed that a TiO 2 pigment with high photoactivity could accelerate the degradation of organic substrates in polymer film [51], which will possess a series of unfavorable properties, such as surface gloss loss, color change, chalking, and cracking.

C17
−0.285 N16-C17 1.4 C18 −0.276 N16-C18 1.4 O19 −0.467 S15-O19 1.4 O20 −0.465 S15-O20 1.4 O21 −0.320 S15-O21 1.6 These results indicated that •OH radicals and photoholes exhibit contributions to the degradation of MO, which provides powerful evi photocatalytic performance of TiO2 pigment. This is mainly due to the SiO2/Al2O3 coating layers did not completely cover all the TiO2 surface in production process. The roles of TiO2 pigments relating to the paint film w predicted in actual usage using this method. It is, therefore, believed that a with high photoactivity could accelerate the degradation of organic substrat film [51], which will possess a series of unfavorable properties, such as surf color change, chalking, and cracking.

Conclusions
In summary, the photoactivity of commercial TiO 2 pigments was quickly evaluated via the photodegradation of MO. The photodegradation results showed that rutile TiO 2 pigment, along with high UV opacity and photostability, retards the photodegradation of MO, whereas the anatase TiO 2 pigment operates primarily as an effective photoactivity for accelerating the rate of photodegradation. h + and ·OH radicals are the major reactive species in the photodegradation of MO over anatase TiO 2 pigment. We also reveal the photodegradation mechanism for MO, which is supported by GC-MS and theoretical calculation. This work provides a useful strategy toward evaluating the photoactivities of various TiO 2 pigments and assessing the potential effects of TiO 2 pigments on coatings stabilization or degradation. At the same time, this method may be very useful in preparing multi-purpose TiO 2 pigments.