Visible-Light Driven Photocatalytic Degradation of Pirimicarb by Pt-Doped AgInS 2 Nanoparticles

: This study describes the synthesis and characterization of Pt-doped AgInS 2 nanoparticles and reports their prospective application as visible-light catalysts for photodegradation of frequently used pirimicarb insecticides, which pose serious health and environmental concerns. The nanomaterials were characterized by XRD, SEM, TEM, XPS, photoluminescence (PL), and UV–vis di ﬀ use reﬂectance spectra (DRS). The presented photocatalytic method for water treatment from pirimicarb has the advantages of using visible light source without any costly additive such as H 2 O 2 needed in other employed methods. The Pt-doped AgInS 2 exhibited higher photocatalytic activities for pirimicarb degradation than undoped AgInS 2 . The 1.0 wt% Pt / AgInS 2 photocatalyst exhibited the highest photodegradation rate, showing enhancement of 56% in comparison to the pure AgInS 2 photocatalyst. The photodegradation rate was found to increase with increasing the catalyst dosage until reaching the optimal dosage of 1.0 g L − 1 . The pirimicarb degradation was signiﬁcantly more e ﬃ cient under acidic conditions, and the rates drastically dropped upon increasing the pH. The photocatalytic mechanism of Pt / AgInS 2 composites and the main active species involved in the process were investigated. The mechanism of pirimicarb degradation was proposed via two di ﬀ erent pathways, N-dealkylation and decarbamoylation. Lastly, the photocatalysts demonstrated remarkable stability and were reusable in three successive catalytic tests without compromising catalytic activities. The Pt / AgInS 2 photocatalyst also exhibited e ﬃ ciency and feasibility in pirimicarb removal from environmental lake and river water samples. were using a with a microwave bridge frequency, GHz; microwave 22.8 amplitude, G; modulation kHz).

The synthesis and application of ternary semiconductor nanomaterials with a general formula of XY m Z n (X = Ag, Cu, Cd, Zn; Y = In, Ga; Z = S, Se, Te; m, n = integer) has gained more attention in recent years [21,22]. These semiconductors have been found to exhibit excellent optical and electrical characteristics, which led to their diverse efficient applications in optoelectronic devices, linear and nonlinear optical instruments, photovoltaic solar cells, and photocatalysis [23]. Silver indium sulfide (AgInS 2 ) is highly stable and non-toxic material with remarkable photocatalytic activity towards degradation of organic pollutants, so it is one of the most prospective materials of ternary chalcogenides for these applications [24]. Depending on the crystal structure of AgInS 2 , the theoretical band gap of these materials varies between 1.7 and 2.0 eV. Such a band gap is smaller than that of common photocatalysts, such as TiO 2 (3.2 eV), ZnO (3.4 eV), and ZnS (3.6 eV), and is convenient for absorption of visible solar light [25,26]. Li et al. reported the synthesis of AgInS 2 nanoparticles using the microwave hydrothermal method and the photocatalytic efficiency of the prepared materials in dye degradation [27]. However, the photocatalytic activity of a single semiconductor can be limited by the fast recombination of its photogenerated electrons and holes [28]. Noble metal doping is used as an effective modification method to further improve the activity of semiconductor photocatalysts. Noble metal nanoparticle dopants on oxide materials can act as a sink for electrons and can promote interfacial electron transfer due to the high Schottky barriers at the metal-Semiconductor interface [29]. The group of Aazam has investigated Pt-doped AgInS 2 nanoparticles in the photooxidation of cyanide using visible light [30]. The Pt dopant was found to enhance the photocatalytic activity of AgInS 2 significantly. Nevertheless, there has been no detailed study on the photocatalytic mechanism of Pt/AgInS 2 composites and the main active species involved in the process. Furthermore, to the best of our knowledge, the visible-light driven degradation of the commonly used carbamate insecticides in water using Pt/AgInS 2 has not been explored yet.
The present work firstly reports efficient visible-light driven photocatalytic degradation of pirimicarb using Pt-doped AgInS 2 and the systematic studies of optimization of the process via different operational variables (e.g., Pt content, catalytic dosage, and initial pH value). Next, this paper addresses various scavenger investigations and ESR measurements that reveal mechanistic insights of the photocatalytic process underlying high performance of these doped materials and the contribution of major reactive species ( • O 2 − , • OH, h + ) in this mechanism. The last section of the report examines the efficiency, stability, and recyclability of the Pt/AgInS 2 photocatalyst in practical treatment of environmental water.  2 2) planes of orthorhombic-type structure of AgInS 2 , respectively [31]. The same structural characteristics were observed for Pt/AgInS 2 , i.e., orthorhombic AgInS 2 phase as in the pure material, suggesting that platinum doping did not alter the structure of AgInS 2 . No additional diffraction peaks were observed that can be attributed to the presence of the metallic Pt in the Pt/AgInS 2 samples, which is most likely due to the low Pt doping content [30].  3 2 2) planes of orthorhombictype structure of AgInS2, respectively [31]. The same structural characteristics were observed for Pt/AgInS2, i.e., orthorhombic AgInS2 phase as in the pure material, suggesting that platinum doping did not alter the structure of AgInS2. No additional diffraction peaks were observed that can be attributed to the presence of the metallic Pt in the Pt/AgInS2 samples, which is most likely due to the low Pt doping content [30]. Next, the samples were characterized using scanning electron microscopy (SEM); a representative micrograph of 1.0 wt% Pt/AgInS2 sample is displayed in Figure 2a. The SEM micrograph infers that the as-prepared Pt/AgInS2 product is mainly composed of agglomerated nanoparticles with diameters in the 20-80 nm range. The presence of Pt in these composite materials was confirmed by high-resolution transmission electron microscopy (HRTEM). The HRTEM image of 1.0 wt% Pt/AgInS2 is presented in Figure 2b. We can observe the AgInS2 phase with d spacing of 0.31 nm due to (1 2 1) and the Pt phase with d spacing of 0.22 nm due to (1 1 1) are in close contact with each other [31,32].  Figure 3 displays the UV-vis diffuse reflectance spectra of the AgInS2 and Pt/AgInS2 samples. A strong absorption in the visible region was observed for all samples, showing a steep absorption edge around 600-700 nm. This shape inferred that the visible-light absorption band was due to the band gap transition and not due to the transition from impurity levels [27]. In order to estimate the band Next, the samples were characterized using scanning electron microscopy (SEM); a representative micrograph of 1.0 wt% Pt/AgInS 2 sample is displayed in Figure 2a. The SEM micrograph infers that the as-prepared Pt/AgInS 2 product is mainly composed of agglomerated nanoparticles with diameters in the 20-80 nm range. The presence of Pt in these composite materials was confirmed by high-resolution transmission electron microscopy (HRTEM). The HRTEM image of 1.0 wt% Pt/AgInS 2 is presented in Figure 2b. We can observe the AgInS 2 phase with d spacing of 0.31 nm due to (1 2 1) and the Pt phase with d spacing of 0.22 nm due to (1 1 1) are in close contact with each other [31,32].  3 2 2) planes of orthorhombictype structure of AgInS2, respectively [31]. The same structural characteristics were observed for Pt/AgInS2, i.e., orthorhombic AgInS2 phase as in the pure material, suggesting that platinum doping did not alter the structure of AgInS2. No additional diffraction peaks were observed that can be attributed to the presence of the metallic Pt in the Pt/AgInS2 samples, which is most likely due to the low Pt doping content [30]. Next, the samples were characterized using scanning electron microscopy (SEM); a representative micrograph of 1.0 wt% Pt/AgInS2 sample is displayed in Figure 2a. The SEM micrograph infers that the as-prepared Pt/AgInS2 product is mainly composed of agglomerated nanoparticles with diameters in the 20-80 nm range. The presence of Pt in these composite materials was confirmed by high-resolution transmission electron microscopy (HRTEM). The HRTEM image of 1.0 wt% Pt/AgInS2 is presented in Figure 2b. We can observe the AgInS2 phase with d spacing of 0.31 nm due to (1 2 1) and the Pt phase with d spacing of 0.22 nm due to (1 1 1) are in close contact with each other [31,32].  Figure 3 displays the UV-vis diffuse reflectance spectra of the AgInS2 and Pt/AgInS2 samples. A strong absorption in the visible region was observed for all samples, showing a steep absorption edge around 600-700 nm. This shape inferred that the visible-light absorption band was due to the band gap transition and not due to the transition from impurity levels [27]. In order to estimate the band  Figure 3 displays the UV-vis diffuse reflectance spectra of the AgInS 2 and Pt/AgInS 2 samples. A strong absorption in the visible region was observed for all samples, showing a steep absorption edge around 600-700 nm. This shape inferred that the visible-light absorption band was due to the band gap transition and not due to the transition from impurity levels [27]. In order to estimate the band gap energies, the following equation is used: (αhν) n = k(hν − Eg), where α is the absorption coefficient, hν is the photonic energy, k is a constant, Eg is the absorption band gap energy, and lastly n Catalysts 2020, 10, 857 5 of 20 is 1 2 and 2 for an indirect and direct band gaps, respectively [33]. The band gap values were found to be around 1.70~1.72 eV, with insignificant difference among the various prepared samples.

Characterization of the As-Prepared Undoped and Pt-Doped AgInS 2 Samples
Catalysts 2020, 10, x FOR PEER REVIEW 5 of 20 gap energies, the following equation is used: (αhν) n = k(hν − Eg), where α is the absorption coefficient, hν is the photonic energy, k is a constant, Eg is the absorption band gap energy, and lastly n is ½ and 2 for an indirect and direct band gaps, respectively [33]. The band gap values were found to be around 1.70~1.72 eV, with insignificant difference among the various prepared samples. XPS analyses were performed to verify the surface chemical composition and the valence state of elements of the Pt/AgInS2 powder ( Figure 4). The spectra of the Ag species ( Figure 4a) manifested two symmetric peaks at binding energies of 367.4 and 373.4 eV with a separation of 6 eV, conforming to Ag + ion. They are attributed to the spin-orbit splitting characteristic of Ag 3d5/2 and Ag 3d3/2, respectively. The peaks in Figure 4b were observed at about 444.4 and 452.0 eV which are the characteristic of In 3d5/2 and In 3d3/2, respectively, corresponding to the presence of indium as In 3+ [34]. The S 2p spectrum in Figure 4c displayed a strong XPS peak at 161.4 eV, indicating the presence of S 2− species in the AgInS2. The XPS analyses corroborate the XRD results and affirm the composition of the AgInS2 material. Considering the presence of the Pt dopant in the synthesized materials, Figure  4d shows the XPS for Pt 4f with peaks located at 70.8 and 74.0 eV, corresponding to the binding energies of Pt 4f7/2 and Pt 4f5/2 [35]. It has been reported that Pt 0 exhibits Pt 4f7/2 and Pt 4f5/2 bands in the ranges of 70.2-71.0 and 73.6-74.0 eV, respectively [36]. The   XPS analyses were performed to verify the surface chemical composition and the valence state of elements of the Pt/AgInS 2 powder ( Figure 4). The spectra of the Ag species (Figure 4a) manifested two symmetric peaks at binding energies of 367.4 and 373.4 eV with a separation of 6 eV, conforming to Ag + ion. They are attributed to the spin-orbit splitting characteristic of Ag 3d 5/2 and Ag 3d 3/2 , respectively. The peaks in Figure 4b were observed at about 444.4 and 452.0 eV which are the characteristic of In 3d 5/2 and In 3d 3/2 , respectively, corresponding to the presence of indium as In 3+ [34]. The S 2p spectrum in Figure 4c displayed a strong XPS peak at 161.4 eV, indicating the presence of S 2− species in the AgInS 2 . The XPS analyses corroborate the XRD results and affirm the composition of the AgInS 2 material. Considering the presence of the Pt dopant in the synthesized materials, Figure 4d shows the XPS for Pt 4f with peaks located at 70.8 and 74.0 eV, corresponding to the binding energies of Pt 4f 7/2 and Pt 4f 5/2 [35]. It has been reported that Pt 0 exhibits Pt 4f 7/2 and Pt 4f 5/2 bands in the ranges of 70.2-71.0 and 73.6-74.0 eV, respectively [36]. The XPS result indicated that the oxidation state of Pt on Pt/AgInS 2 is Pt 0 .
Catalysts 2020, 10, x FOR PEER REVIEW 5 of 20 gap energies, the following equation is used: (αhν) n = k(hν − Eg), where α is the absorption coefficient, hν is the photonic energy, k is a constant, Eg is the absorption band gap energy, and lastly n is ½ and 2 for an indirect and direct band gaps, respectively [33]. The band gap values were found to be around 1.70~1.72 eV, with insignificant difference among the various prepared samples. XPS analyses were performed to verify the surface chemical composition and the valence state of elements of the Pt/AgInS2 powder ( Figure 4). The spectra of the Ag species ( Figure 4a) manifested two symmetric peaks at binding energies of 367.4 and 373.4 eV with a separation of 6 eV, conforming to Ag + ion. They are attributed to the spin-orbit splitting characteristic of Ag 3d5/2 and Ag 3d3/2, respectively. The peaks in Figure 4b were observed at about 444.4 and 452.0 eV which are the characteristic of In 3d5/2 and In 3d3/2, respectively, corresponding to the presence of indium as In 3+ [34]. The S 2p spectrum in Figure 4c displayed a strong XPS peak at 161.4 eV, indicating the presence of S 2− species in the AgInS2. The XPS analyses corroborate the XRD results and affirm the composition of the AgInS2 material. Considering the presence of the Pt dopant in the synthesized materials, Figure  4d shows the XPS for Pt 4f with peaks located at 70.8 and 74.0 eV, corresponding to the binding energies of Pt 4f7/2 and Pt 4f5/2 [35]. It has been reported that Pt 0 exhibits Pt 4f7/2 and Pt 4f5/2 bands in the ranges of 70.2-71.0 and 73.6-74.0 eV, respectively [36]. The XPS result indicated that the oxidation state of Pt on Pt/AgInS2 is Pt 0 .   Since photoluminescence (PL) emission arises from the recombination of the photogenerated free carriers, PL emission spectroscopy is commonly employed in the investigations of the transfer, separation, and recombination patterns of photogenerated electrons and holes [37]. Figure 5 shows the PL spectra of the pure AgInS2 and Pt-doped AgInS2 samples. The PL spectra of Pt-doped AgInS2 samples showed a significant decrease in intensity in comparison to that of pure AgInS2. This weaker   Since photoluminescence (PL) emission arises from the recombination of the photogenerated free carriers, PL emission spectroscopy is commonly employed in the investigations of the transfer, separation, and recombination patterns of photogenerated electrons and holes [37]. Figure 5 shows the PL spectra of the pure AgInS 2 and Pt-doped AgInS 2 samples. The PL spectra of Pt-doped AgInS 2 samples showed a significant decrease in intensity in comparison to that of pure AgInS 2 . This weaker intensity indicates a lower recombination probability of free charge carriers. Thus, PL data infer that the Pt doping can effectively inhibit the recombination of photogenerated charge carriers, which helps in separating photogenerated electron-hole pairs in AgInS 2 . However, it can be observed that at higher Pt content, the peak intensity of 1.5 wt% Pt/AgInS 2 is higher than that of 1.0 wt% Pt/AgInS 2 . This might be due to the behavior of the Pt dopant as a recombination center conversely when its percentage is high [29].
(c) (d) Since photoluminescence (PL) emission arises from the recombination of the photogenerated free carriers, PL emission spectroscopy is commonly employed in the investigations of the transfer, separation, and recombination patterns of photogenerated electrons and holes [37]. Figure 5 shows the PL spectra of the pure AgInS2 and Pt-doped AgInS2 samples. The PL spectra of Pt-doped AgInS2 samples showed a significant decrease in intensity in comparison to that of pure AgInS2. This weaker intensity indicates a lower recombination probability of free charge carriers. Thus, PL data infer that the Pt doping can effectively inhibit the recombination of photogenerated charge carriers, which helps in separating photogenerated electron-hole pairs in AgInS2. However, it can be observed that at higher Pt content, the peak intensity of 1.5 wt% Pt/AgInS2 is higher than that of 1.0 wt% Pt/AgInS2. This might be due to the behavior of the Pt dopant as a recombination center conversely when its percentage is high [29].

Effect of Pt Content
Four sets of experiments (adsorptions, photolysis, and photocatalysis) were carried out to verify the role of Pt/AgInS2 in the reported reaction. The experiments and relevant results are summarized in Table 2 and Figure 6. In summary, both adsorption experiments (dark conditions, no visible light Wavelength (nm) Intensity (a.u.)

Effect of Pt Content
Four sets of experiments (adsorptions, photolysis, and photocatalysis) were carried out to verify the role of Pt/AgInS 2 in the reported reaction. The experiments and relevant results are summarized in Table 2 and Figure 6. In summary, both adsorption experiments (dark conditions, no visible light source) showed an insignificant decrease of pirimicarb (less than 15%), implying that the hydrolysis and adsorption of pirimicarb on AgInS 2 and Pt-doped AgInS 2 was insignificant. Likewise, photolysis showed negligible pirimicarb degradation. On the other hand, the photocatalytic experiments exhibited efficient pirimicarb degradation in aqueous Pt/AgInS 2 dispersions by visible-light irradiation. ca. 85% of pirimicarb was degraded after irradiation for 24 h.

Experiment Conditions Results (After 24 h)
Less than 15% of pirimicarb adsorption Less than 15% of pirimicarb adsorption Ⅲ-Photolysis 85% pirimicarb degradation  Figure 7 presents the influence of the Pt content on the photodegradation rate of pirimicarb under visible-light irradiation. As can be seen, the photocatalytic activity of the Pt-doped AgInS2 material was significantly higher than that of the undoped AgInS2. When subjected to visible-light irradiation for 28 h, 93% of pirimicarb degraded in the presence of 1.0 wt% Pt-doped AgInS2, whereas only 37% of pirimicarb degraded in the presence of undoped AgInS2. In addition, the degradation rate enhanced from 73% to 93% with increasing the Pt doping content from 0.25 to 1.0 w%, respectively. The enhanced photocatalytic activities can be rationalized by the improvement of charge separation as a result of the Pt doping. However, the further increase of Pt content (above 1.0 wt%) resulted in a decrease of the photocatalytic activity of the Pt-doped AgInS2. This result might be explained by the higher recombination of charge carriers as higher Pt doping conversely behave as recombinant centers [29]. These results are in line with the previously discussed effect of Pt doping on the separation of photoinduced electrons and holes in AgInS2 photocatalysts observed in the PL spectra ( Figure 5). In addition, a higher content of Pt might act as a shield that prevents the incident  Figure 7 presents the influence of the Pt content on the photodegradation rate of pirimicarb under visible-light irradiation. As can be seen, the photocatalytic activity of the Pt-doped AgInS 2 material was significantly higher than that of the undoped AgInS 2 . When subjected to visible-light irradiation for 28 h, 93% of pirimicarb degraded in the presence of 1.0 wt% Pt-doped AgInS 2 , whereas only 37% of pirimicarb degraded in the presence of undoped AgInS 2 . In addition, the degradation rate enhanced from 73% to 93% with increasing the Pt doping content from 0.25 to 1.0 wt%, respectively. The enhanced photocatalytic activities can be rationalized by the improvement of charge separation as a result of the Pt doping. However, the further increase of Pt content (above 1.0 wt%) resulted in a decrease of the photocatalytic activity of the Pt-doped AgInS 2 . This result might be explained by the higher recombination of charge carriers as higher Pt doping conversely behave as recombinant centers [29]. These results are in line with the previously discussed effect of Pt doping on the separation of photoinduced electrons and holes in AgInS 2 photocatalysts observed in the PL spectra ( Figure 5). In addition, a higher content of Pt might act as a shield that prevents the incident photons from reaching the surface of the catalyst, thereby reducing the photocatalytic activity of the semiconductors [38].  Further analysis of the photocatalytic performance of the different materials was performed using regression analysis based on first-order reaction kinetics for the pirimicarb degradation. Degradation rate constants (kapp) were calculated from the slope of ln C0/C = kappt plots. The kapp values as well as the linear regression coefficients for the different studied materials are listed in Table 3. The appropriate first-order relationship shows to fit well, according the obtained values. As shown in Table 3, 1.0 wt% Pt-doping produces the most effective photocatalytic activity for all the AgInS2 samples. Therefore, the 1.0 wt% Pt-doping samples were chosen as the research object for the subsequent investigations. The amount of the photocatalyst (catalyst dosage) is a parameter that has important effects on photodegradation rates of organic compounds [39,40]. This parameter was examined by using different concentrations of 1.0 wt% Pt/AgInS2 (0.1 to 1.5 g L −1 ) in the pirimicarb degradation. The results are shown in Figure 8. In the absence of the catalyst, the degradation of pirimicarb was negligible up to 24 h under visible-light irradiation. The result highlighted the important role of the Pt/AgInS2 in this application. Figure 8 further displays that the increase in Pt/AgInS2 concentration from 0.1 to 1.0 g L −1 led to a substantial enhancement of the photodegradation efficiency from 27%-98% under visible-light irradiation for 24 h. The optimal catalyst dosage was found to be 1.0 g L −1 , after which the degradation rate begins to be in equilibrium. The enhanced photodegradation rates with the increase of the Pt/AgInS2 dosage can be attributed to the increase in the total surface area (accessible active sites) available for the photocatalytic reaction [41]. Upon catalyst overdose, scattering of incident light and less penetration might occur, causing a loading of 1.5 g/L to have similar degradation rate of pirimicarb as 1.0 g/L. Further analysis of the photocatalytic performance of the different materials was performed using regression analysis based on first-order reaction kinetics for the pirimicarb degradation. Degradation rate constants (k app ) were calculated from the slope of ln C 0 /C = k app t plots. The k app values as well as the linear regression coefficients for the different studied materials are listed in Table 3. The appropriate first-order relationship shows to fit well, according the obtained values. As shown in Table 3, 1.0 wt% Pt-doping produces the most effective photocatalytic activity for all the AgInS 2 samples. Therefore, the 1.0 wt% Pt-doping samples were chosen as the research object for the subsequent investigations. The amount of the photocatalyst (catalyst dosage) is a parameter that has important effects on photodegradation rates of organic compounds [39,40]. This parameter was examined by using different concentrations of 1.0 wt% Pt/AgInS 2 (0.1 to 1.5 g L −1 ) in the pirimicarb degradation. The results are shown in Figure 8. In the absence of the catalyst, the degradation of pirimicarb was negligible up to 24 h under visible-light irradiation. The result highlighted the important role of the Pt/AgInS 2 in this application. Figure 8 further displays that the increase in Pt/AgInS 2 concentration from 0.1 to 1.0 g L −1 led to a substantial enhancement of the photodegradation efficiency from 27-98% under visible-light irradiation for 24 h. The optimal catalyst dosage was found to be 1.0 g L −1 , after which the degradation rate begins to be in equilibrium. The enhanced photodegradation rates with the increase of the Pt/AgInS 2 dosage can be attributed to the increase in the total surface area (accessible active sites) available for the photocatalytic reaction [41]. Upon catalyst overdose, scattering of incident light and less penetration might occur, causing a loading of 1.5 g/L to have similar degradation rate of pirimicarb as 1.0 g/L.

Effect of Initial Ph Value
The initial pH value of the reaction mixture has been revealed in previous research as an important process parameter with prominent impact on photocatalytic performance [42]. Figure 9 displays the pH effect on pirimicarb photodegradation. The degradation process proceeded significantly faster under an acidic pH, and the degradation rate decreased with the increase of the initial pH. As the pH was increased from 3 to 9, the degradation rate of pirimicarb within 24 h significantly decreased from 98% to 49%. The lower degradation rate at higher pH could be due to a Nernstian shift of the band edges to more negative values, which led to reduction in the oxidation potential of the positive holes [39]. Higher pH and the presence of increased number of hydroxyl groups on the surface might also decrease the conduction band electrons due to electron-hole recombination at active sites [43], which might be another plausible explanation for this observation. In line, Cunningham et al. postulated a model for faster hole-electron recombination at a pH of 9.5, compared to that at lower pH, based on the larger surface concentration of hydroxyls at pH 9.5 [44].

Identification of Active Species (Quenching and ESR Studies)
The role of potential active species in this photocatalytic process was investigated by adding different scavengers, particularly isopropanol (IPA) for • OH, ethylenediaminetetraacetic acid (EDTA) for h + , and benzoquinone (BQ) for • O2 − [45].

Effect of Initial Ph Value
The initial pH value of the reaction mixture has been revealed in previous research as an important process parameter with prominent impact on photocatalytic performance [42]. Figure 9 displays the pH effect on pirimicarb photodegradation. The degradation process proceeded significantly faster under an acidic pH, and the degradation rate decreased with the increase of the initial pH. As the pH was increased from 3 to 9, the degradation rate of pirimicarb within 24 h significantly decreased from 98% to 49%. The lower degradation rate at higher pH could be due to a Nernstian shift of the band edges to more negative values, which led to reduction in the oxidation potential of the positive holes [39]. Higher pH and the presence of increased number of hydroxyl groups on the surface might also decrease the conduction band electrons due to electron-hole recombination at active sites [43], which might be another plausible explanation for this observation. In line, Cunningham et al. postulated a model for faster hole-electron recombination at a pH of 9.5, compared to that at lower pH, based on the larger surface concentration of hydroxyls at pH 9.5 [44].

Effect of Initial Ph Value
The initial pH value of the reaction mixture has been revealed in previous research as an important process parameter with prominent impact on photocatalytic performance [42]. Figure 9 displays the pH effect on pirimicarb photodegradation. The degradation process proceeded significantly faster under an acidic pH, and the degradation rate decreased with the increase of the initial pH. As the pH was increased from 3 to 9, the degradation rate of pirimicarb within 24 h significantly decreased from 98% to 49%. The lower degradation rate at higher pH could be due to a Nernstian shift of the band edges to more negative values, which led to reduction in the oxidation potential of the positive holes [39]. Higher pH and the presence of increased number of hydroxyl groups on the surface might also decrease the conduction band electrons due to electron-hole recombination at active sites [43], which might be another plausible explanation for this observation. In line, Cunningham et al. postulated a model for faster hole-electron recombination at a pH of 9.5, compared to that at lower pH, based on the larger surface concentration of hydroxyls at pH 9.5 [44].

Identification of Active Species (Quenching and ESR Studies)
The role of potential active species in this photocatalytic process was investigated by adding different scavengers, particularly isopropanol (IPA) for • OH, ethylenediaminetetraacetic acid (EDTA) for h + , and benzoquinone (BQ) for • O2 − [45]. Figure 10

Identification of Active Species (Quenching and ESR Studies)
The role of potential active species in this photocatalytic process was investigated by adding different scavengers, particularly isopropanol (IPA) for • OH, ethylenediaminetetraacetic acid (EDTA) for h + , and benzoquinone (BQ) for • O 2 − [45]. Figure 10 summarizes the photocatalytic degradation of pirimicarb with 1.0 wt% Pt/AgInS 2 catalyst under visible-light irradiation in the absence and presence of each scavenger. In the absence of any scavenger, the photodegradation of pirimicarb was 98% after 24 h of treatment. A dominant inhibition effect on the photodegradation rate (98% to 16%) was observed upon adding IPA (1 mM) to the reaction mixture, evidencing the important role of the • OH in this reaction. Similar inhibition effect from 98% to 27% was observed upon adding BQ (1 mM), which infers that • O 2 − also played a role in the photodegradation. In contrast, the addition of EDTA (1 mM) slightly reduced the degradation rate indicating that photogenerated holes played an assistant role in this catalytic degradation of pirimicarb. Electron spin resonance (ESR) spin-trap technique (with 5,5-dimethylpyridine-N-oxide (DMPO)) was employed to further assess and detect the reactive radical species involved in the reactions. absence and presence of each scavenger. In the absence of any scavenger, the photodegradation of pirimicarb was 98% after 24 h of treatment. A dominant inhibition effect on the photodegradation rate (98% to 16%) was observed upon adding IPA (1 mM) to the reaction mixture, evidencing the important role of the • OH in this reaction. Similar inhibition effect from 98% to 27% was observed upon adding BQ (1 mM), which infers that • O2 − also played a role in the photodegradation. In contrast, the addition of EDTA (1 mM) slightly reduced the degradation rate indicating that photogenerated holes played an assistant role in this catalytic degradation of pirimicarb. Electron spin resonance (ESR) spin-trap technique (with 5,5-dimethylpyridine-N-oxide (DMPO)) was employed to further assess and detect the reactive radical species involved in the reactions. Figure 11 displays the results of these experiments. In the absence of light, no ESR signal was observed. Under visible-light irradiation, the characteristic signals for DMPO-• O2 − (intensity ratios of 1:1:1:1) and DMPO-• OH (intensity ratios of 1:2:2:1) spin adducts were observed, indicating the activation of the photocatalysts upon exposure to visible light and the generation of reactive oxygen species such as hydroxyl radical and superoxide anion radical. These results are in line with the generation of • OH and • O2 − radicals under these photocatalytic conditions concluded from the radical scavenger experiments. absence and presence of each scavenger. In the absence of any scavenger, the photodegradation of pirimicarb was 98% after 24 h of treatment. A dominant inhibition effect on the photodegradation rate (98% to 16%) was observed upon adding IPA (1 mM) to the reaction mixture, evidencing the important role of the • OH in this reaction. Similar inhibition effect from 98% to 27% was observed upon adding BQ (1 mM), which infers that • O2 − also played a role in the photodegradation. In contrast, the addition of EDTA (1 mM) slightly reduced the degradation rate indicating that photogenerated holes played an assistant role in this catalytic degradation of pirimicarb. Electron spin resonance (ESR) spin-trap technique (with 5,5-dimethylpyridine-N-oxide (DMPO)) was employed to further assess and detect the reactive radical species involved in the reactions. Figure 11 displays the results of these experiments. In the absence of light, no ESR signal was observed. Under visible-light irradiation, the characteristic signals for DMPO-• O2 − (intensity ratios of 1:1:1:1) and DMPO-• OH (intensity ratios of 1:2:2:1) spin adducts were observed, indicating the activation of the photocatalysts upon exposure to visible light and the generation of reactive oxygen species such as hydroxyl radical and superoxide anion radical. These results are in line with the generation of • OH and • O2 − radicals under these photocatalytic conditions concluded from the radical scavenger experiments. The photocatalytic mechanism of the Pt/AgInS 2 catalysts may be summarized as such: electrons (e − ) in the valence band (VB) of AgInS 2 are excited to its conduction band (CB) upon irradiation with visible light creating the same number of holes (h + ) in the VB. In pure AgInS 2 , the excited charge carriers (electron and hole) rapidly recombine at and/or within the surface of AgInS 2 particles, thereby resulting in reduced photocatalytic activity. In contrast, the Pt doped on AgInS 2 is believed to serve as an electron sink (Schottky barrier electron trapping) and thus to retard fast charge-pair recombination [46]. In essence, the photoexcited electrons would migrate from the low work function AgInS 2 (−4.72 eV) to the high work function noble metal Pt (−5.65 eV) [47,48]. Thus, the incorporated Pt nanoparticles would effectively withdraw electrons from the AgInS 2 , behaving as efficient electron sinks. Afterwards, Pt can release the accumulated electrons in the presence of efficient acceptors as O 2 forming • O 2 − active radical species which can subsequently form the • OH species [49]. The generated active oxygen species or the oxidative holes in turn attack the organic contaminants and gradually degrade them. Figure 12 summarizes the schematic representation of pirimicarb photodegradation mechanism at the surface of Pt/AgInS 2 catalysts under visible-light irradiation.
Catalysts 2020, 10, x FOR PEER REVIEW 11 of 20 The photocatalytic mechanism of the Pt/AgInS2 catalysts may be summarized as such: electrons (e − ) in the valence band (VB) of AgInS2 are excited to its conduction band (CB) upon irradiation with visible light creating the same number of holes (h + ) in the VB. In pure AgInS2, the excited charge carriers (electron and hole) rapidly recombine at and/or within the surface of AgInS2 particles, thereby resulting in reduced photocatalytic activity. In contrast, the Pt doped on AgInS2 is believed to serve as an electron sink (Schottky barrier electron trapping) and thus to retard fast charge-pair recombination [46]. In essence, the photoexcited electrons would migrate from the low work function AgInS2 (−4.72 eV) to the high work function noble metal Pt (−5.65 eV) [47,48]. Thus, the incorporated Pt nanoparticles would effectively withdraw electrons from the AgInS2, behaving as efficient electron sinks. Afterwards, Pt can release the accumulated electrons in the presence of efficient acceptors as O2 forming • O2 − active radical species which can subsequently form the • OH species [49]. The generated active oxygen species or the oxidative holes in turn attack the organic contaminants and gradually degrade them. Figure 12 summarizes the schematic representation of pirimicarb photodegradation mechanism at the surface of Pt/AgInS2 catalysts under visible-light irradiation.

Reaction Pathway of Pirimicarb Degradation
The analysis of intermediate products was carried out in order to further understand the photodegradation pathway of pirimicarb using Pt/AgInS2. The chromatogram of the pirimicarb solution after treatment with Pt/AgInS2 under visible-light irradiation for 16 h is shown in Figure 13. The last peak at 34.11 min represents the pirimicarb (PMC) reactant. Peaks A-G label the main intermediates in the photodegradation process since their intensities increase then subsequently decrease ( Figure S1). The summary of the detected chemical entities in this process, their characteristic ions of mass spectra, as well as retention times is depicted in Table 4. The presence of many pirimicarb degradation products can be attributed to the lack of selectivity of the active radical species ( • OH and • O2 − ) that may attack pirimicarb or the subsequent intermediates at different reactive sites.

Reaction Pathway of Pirimicarb Degradation
The analysis of intermediate products was carried out in order to further understand the photodegradation pathway of pirimicarb using Pt/AgInS 2 . The chromatogram of the pirimicarb solution after treatment with Pt/AgInS 2 under visible-light irradiation for 16 h is shown in Figure 13. The last peak at 34.11 min represents the pirimicarb (PMC) reactant. Peaks A-G label the main intermediates in the photodegradation process since their intensities increase then subsequently decrease ( Figure S1). The summary of the detected chemical entities in this process, their characteristic ions of mass spectra, as well as retention times is depicted in Table 4. The presence of many pirimicarb degradation products can be attributed to the lack of selectivity of the active radical species ( • OH and • O 2 − ) that may attack pirimicarb or the subsequent intermediates at different reactive sites.
Catalysts 2020, 10, x FOR PEER REVIEW 11 of 20 The photocatalytic mechanism of the Pt/AgInS2 catalysts may be summarized as such: electrons (e − ) in the valence band (VB) of AgInS2 are excited to its conduction band (CB) upon irradiation with visible light creating the same number of holes (h + ) in the VB. In pure AgInS2, the excited charge carriers (electron and hole) rapidly recombine at and/or within the surface of AgInS2 particles, thereby resulting in reduced photocatalytic activity. In contrast, the Pt doped on AgInS2 is believed to serve as an electron sink (Schottky barrier electron trapping) and thus to retard fast charge-pair recombination [46]. In essence, the photoexcited electrons would migrate from the low work function AgInS2 (−4.72 eV) to the high work function noble metal Pt (−5.65 eV) [47,48]. Thus, the incorporated Pt nanoparticles would effectively withdraw electrons from the AgInS2, behaving as efficient electron sinks. Afterwards, Pt can release the accumulated electrons in the presence of efficient acceptors as O2 forming • O2 − active radical species which can subsequently form the • OH species [49]. The generated active oxygen species or the oxidative holes in turn attack the organic contaminants and gradually degrade them. Figure 12 summarizes the schematic representation of pirimicarb photodegradation mechanism at the surface of Pt/AgInS2 catalysts under visible-light irradiation.

Reaction Pathway of Pirimicarb Degradation
The analysis of intermediate products was carried out in order to further understand the photodegradation pathway of pirimicarb using Pt/AgInS2. The chromatogram of the pirimicarb solution after treatment with Pt/AgInS2 under visible-light irradiation for 16 h is shown in Figure 13. The last peak at 34.11 min represents the pirimicarb (PMC) reactant. Peaks A-G label the main intermediates in the photodegradation process since their intensities increase then subsequently decrease ( Figure S1). The summary of the detected chemical entities in this process, their characteristic ions of mass spectra, as well as retention times is depicted in Table 4. The presence of many pirimicarb degradation products can be attributed to the lack of selectivity of the active radical species ( • OH and • O2 − ) that may attack pirimicarb or the subsequent intermediates at different reactive sites. The tentative degradation pathway of pirimicarb with two possible routes (I and II) is suggested in Figure 14 based on our results. Route I involves the formation of carbamate intermediates A-D via subsequent N-dealkylations of the 2-dimethylamine group. The • OH radicals act on the adjacent C-H bonds to nitrogen, with pronounced stereoelectronic effect that improves the rate of abstraction of H atoms, forming carbon-centered radicals. Furthermore, • OH radicals can react with the lone-pair electron of the N atom leading to cationic radicals that transform to these carbon-centered radicals [50]. Peroxyl radicals are then formed by oxygen addition to the generated radicals, which in turn decompose to different intermediates (A and B). The results and proposed pathways using this Pt/AgInS 2 catalytic system are similar to pirimicarb photodegradation routes using BiVO 4 that we have reported previously [16]. Table 4. Identification of the intermediates from the photodegradation of pirimicarb by LC/MS.

Structure t R (min) Characteristic Ions (m/z)
Catalysts 2020, 10, x FOR PEER REVIEW 12 of 20                 The results and proposed pathways using this Pt/AgInS2 catalytic system are similar to pirimicarb photodegradation routes using BiVO4 that we have reported previously [16].

Efficiency of Recycled Catalyst
Practical application of catalysis strongly depends on the reusability and stability of the catalyst materials. For this purpose, the performance of Pt/AgInS2 materials was studied in three consecutive runs of photodegradation of pirimicarb under visible-light irradiation. The Pt/AgInS2 catalyst was collected after each run, dried, and reused under the same experimental conditions. As shown in Figure 15a, the photocatalytic activity of Pt/AgInS2 was consistent after three successive catalytic tests with 98%, 96%, and 92% degradation of pirimicarb, respectively. In addition, Figure 15b displays that the XRD patterns of the used Pt/AgInS2 powder after the reaction match closely the patterns of the fresh powder before usage, with minor differences in the relative intensities only [31]. The

Efficiency of Recycled Catalyst
Practical application of catalysis strongly depends on the reusability and stability of the catalyst materials. For this purpose, the performance of Pt/AgInS 2 materials was studied in three consecutive runs of photodegradation of pirimicarb under visible-light irradiation. The Pt/AgInS 2 catalyst was collected after each run, dried, and reused under the same experimental conditions. As shown in Figure 15a, the photocatalytic activity of Pt/AgInS 2 was consistent after three successive catalytic tests with 98%, 96%, and 92% degradation of pirimicarb, respectively. In addition, Figure 15b displays that the XRD patterns of the used Pt/AgInS 2 powder after the reaction match closely the patterns of the fresh powder before usage, with minor differences in the relative intensities only [31]. The experiments show that the Pt/AgInS 2 system is significantly stable and reusable for long-term practical photocatalytic processes without photocorrosion risk.
Catalysts 2020, 10, x FOR PEER REVIEW 14 of 20 experiments show that the Pt/AgInS2 system is significantly stable and reusable for long-term practical photocatalytic processes without photocorrosion risk.

Photocatalytic Treatment of Natural Water Samples
The visible-light driven Pt/AgInS2 photocatalysis was applied to study the degradation of pirimicarb in the natural water as a reaction medium. The results are summarized in Figure 16 which shows the photodegradation rates of pirimicarb in deionized water and natural water. In the presence of Pt/AgInS2 photocatalyst, pirimicarb concentration in the natural water samples was found to

Photocatalytic Treatment of Natural Water Samples
The visible-light driven Pt/AgInS 2 photocatalysis was applied to study the degradation of pirimicarb in the natural water as a reaction medium. The results are summarized in Figure 16 which shows the photodegradation rates of pirimicarb in deionized water and natural water. In the presence of Pt/AgInS 2 photocatalyst, pirimicarb concentration in the natural water samples was found to decrease upon irradiation time. The degradation rate of pirimicarb in natural water samples was slightly reduced in comparison to that in deionized water. This can be due to the presence of organic matter and anions in environmental water (Table 5), which can slightly deactivate the catalyst or compete with the target pirimicarb for the active sites [51]. Despite this slight decrease in rates, the photocatalytic activity of Pt/AgInS 2 in the degradation of pirimicarb is still noticeable even in natural water scenarios, demonstrating the efficiency and prospect of the prepared catalytic system for practical environmental and waste water treatment.

Photocatalytic Treatment of Natural Water Samples
The visible-light driven Pt/AgInS2 photocatalysis was applied to study the degradation of pirimicarb in the natural water as a reaction medium. The results are summarized in Figure 16 which shows the photodegradation rates of pirimicarb in deionized water and natural water. In the presence of Pt/AgInS2 photocatalyst, pirimicarb concentration in the natural water samples was found to decrease upon irradiation time. The degradation rate of pirimicarb in natural water samples was slightly reduced in comparison to that in deionized water. This can be due to the presence of organic matter and anions in environmental water (Table 5), which can slightly deactivate the catalyst or compete with the target pirimicarb for the active sites [51]. Despite this slight decrease in rates, the photocatalytic activity of Pt/AgInS2 in the degradation of pirimicarb is still noticeable even in natural water scenarios, demonstrating the efficiency and prospect of the prepared catalytic system for practical environmental and waste water treatment.

Materials
Pirimicarb (99.2%) was purchased from ChemService (West Chester, PA, USA) and employed without any further purification. A stock solution comprising 10 mg L −1 of pirimicarb in water was prepared, protected from light, and stored at 4 • C. The presence of pirimicarb as a pure organic compound was confirmed by HPLC analysis. Silver nitrate AgNO 3 (Aldrich, St. Louis, MO, USA, 99%), indium (III) chloride tetrahydrate (Aldrich, 97%), and L-cysteine (Alfa Aesar, Haverhill, MA, USA 98%) were used as the precursors of silver indium sulfide. Hydrogen hexachloroplatinate (IV) hydrate (Alfa Aesar, 99.9%) was used as source of the Pt dopant. HPLC-grade methanol, nitric acid, sodium hydroxide, and reagent-grade ammonium acetate were obtained from Merck. 5,5-Dimethyl-1-pyrroline-N-oxide (DMPO) was purchased from Sigma-Aldrich. Deionized water was used throughout this study. The water was purified with a Milli-Q water ion-exchange system (Millipore Co. Burlington, MA, USA) for a resistivity of 1.8 × 10 7 Ω-cm.

Preparation and Characterization Of Pt/Agins 2
For the synthesis of AgInS 2 catalyst, 4 mmol of AgNO 3 and 4 mmol of InCl 3 ·4H 2 O were separately dissolved in 20 mL of deionized water each. The AgNO 3 solution was then mixed with the InCl 3 ·4H 2 O solution. A 20 mL of 8 mmol L-cysteine was slowly added to the mixture. The final pH value of the solution was adjusted to 7 using ammonia solution. After stirring for 30 min, the obtained slurry was then transferred into Teflon-lined stainless steel autoclave and heated to 160 • C. After 24 h, the heating was stopped allowing the sample to naturally cool down to room temperature. The obtained precipitate was collected by filtration, washed with absolute ethanol and deionized water several times prior to drying at 60 • C for 12 h. The Pt-doped AgInS 2 catalysts were prepared by the impregnation method using AgInS 2 and hydrogen hexachloroplatinate (IV) hydrate. The as-prepared AgInS 2 powder (0.2 g) was added to 5 mL deionized water containing an appropriate amount of H 2 PtCl 6 in a ceramic dish. The suspension was stirred using a glass rod during evaporation of water on the Corning stirrer/plate (Corning, New York, NY, USA). The resulting powder was collected and calcined in an oven at 400 • C for 0.5 h. The content of doping species was calculated according to the mass percentage of Pt. The value for the actual Pt loading of the synthesized catalysts was obtained by using inductively coupled plasma atomic emission spectroscopy (ICP-AES, Optima 2000DV, Wellesley, MA, USA), which is summarized in Table 6. The phase and composition of the as-prepared Pt/AgInS 2 powders were measured using an X-ray diffractometer (PHILIPS X'PERT Pro MPD, Almelo, Netherlands). The morphology of Pt/AgInS 2 powders were analyzed using a field-emission scanning electron microscope (FE-SEM, HITACHI S-4800, Tokyo, Japan). The sample morphology was also observed by a transmission electron microscope (TEM, JEOL JEM-F200, Tokyo, Japan) operated at accelerating voltage of 200 kV. The UV-vis diffuse reflectance spectra of the Pt/AgInS 2 powders were measured using a UV-vis spectrophotometer equipped with an integration sphere (Perkin Elmer Lambda 35, Wellesley, MA, USA). The photoluminescence (PL) emission spectra of Pt/AgInS 2 were obtained using a fluorescence spectrometer (SpectraMax M5, San Jose, CA, USA). The binding energy of Ag, In, S, and Pt was measured at ambient temperature using an X-ray photoelectron spectroscope (XPS, VG Scientific ESCALAB 250, Waltham, MA, USA). The peak position of each element was corrected by C1s (284.6 eV).

Apparatus and Instruments
The apparatus utilized in the photocatalytic degradation studies of pirimicarb is described elsewhere [52]. The C-75 Chromato-Vue UVP cabinet provided a wide area of illumination from 4 W visible-light tubes positioned on two sides of the cabinet interior. A Waters ZQ LC/MS system, equipped with a binary pump, a photodiode array detector, an autosampler, and a micromass detector, was used for separation and identification. The electron spin resonance (ESR) signals of • OH and • O 2 − radicals, trapped using 5,5-dimethyl-1-pyrroline-N-oxide (DMPO), were recorded using a Bruker EMX A300-10/12 with a microwave bridge (microwave frequency, 9.85 GHz; microwave power, 22.8 mW; modulation amplitude, 1 G; modulation frequency, 100 kHz).

Procedures and Analyses
Photocatalytic tests were performed on 100 mL of aqueous solutions containing 10 mg L −1 pirimicarb and five different amounts of Pt/AgInS 2 (0.1, 0.25, 0.5, 1.0, and 1.5 g L −1 ) at different pH values. The initial pH of the suspension in the different tests was adjusted by adding either HNO 3 or NaOH solution. Prior to irradiation, the suspension was magnetically stirred in the dark for ca. 30 min to ensure the establishment of an adsorption/desorption equilibrium. Irradiation was carried out using two fluorescent lamps (F4T5/CW, Philips Lighting Co., Taipei, Taiwan). The lamp mainly provides visible light in the range of 400-700 nm. The average light intensity striking the surface of the reaction solution was about 1420 lux, as measured by a digital luxmeter (XRP-3000 AccuMAX™, Westbury, USA). At any given irradiation time interval, the suspension was sampled (5 mL) and centrifuged (30 min at 3000 rpm) to separate the Pt/AgInS 2 powders. The residual amount of pirimicarb was determined by HPLC after each irradiation cycle. The analysis of organic intermediates was accomplished by high-performance liquid chromatography-electrospray ionization mass spectrometry (HPLC-ESI-MS) after readjusting the chromatographic conditions to make the mobile phase compatible with the working conditions of the mass spectrometer. A 25 mM aqueous ammonium acetate buffer (pH 6.9) was used as solvent A and methanol was used as solvent B. LC was carried out on an Atlantis TM dC 18 column (250 mm × 4.6 mm i.d., dp =5 µm, Milford, USA). The flow rate of the mobile phase was set at 1 mL/min. A linear gradient was run as follows, t = 0, A = 95, B = 5; t = 20, A = 50, B = 50; t = 35-40, A = 10, B = 90; and t = 45, A = 95, B = 5. The elution was monitored at 245 nm. The column effluent was introduced into the ESI source of the mass spectrometer. The quadruple mass spectrometer, equipped with an ESI interface with a heated nebulizer probe at 350 • C, was used with an ion source temperature of 80 • C. ESI was carried out with the vaporizer at 350 • C, and nitrogen was used as sheath (80 psi) and auxiliary (20 psi) gas to assist with the preliminary nebulization and to initiate the ionization process. A discharge current of 5 µA was applied. The tube lens and capillary voltages were optimized for maximum response during the perfusion of the pirimicarb standard.

Procedure for Degradation of Pirimicarb in Natural Water Samples
The efficiency of the Pt/AgInS 2 photocatalytic system was investigated in natural water samples by collecting river water from the Han River in Taichung City and lake water from the lake in Taichung Park. The suspended solids were removed from all samples by filtration through a 0.45 µm membrane, after which the samples were stored in the dark at 4 • C until analysis. Finally, the natural water samples were spiked with the target compound (at 10 mg L −1 ) just prior to photocatalytic experiments. Degradations were performed on 100 mL of the natural water samples containing 1.0 wt% Pt/AgInS 2 (1.0 g L −1 ) without pH adjustment. The photocatalytic activity is expressed by C/C 0 versus t (time), where C is the concentration at a given time and C 0 is the initial concentration of pirimicarb.

Conclusions
This work reported that the photocatalytic efficiency of AgInS 2 nanoparticles for pirimicarb degradation could be enhanced considerably upon introducing Pt species. The photocatalytic activity of the Pt/AgInS 2 composite samples improved with increasing Pt content until an optimal loading of 1.0 wt% Pt/AgInS 2 , exhibiting the best activity of 98% reduction in pirimicarb concentration after 24 h of visible-light irradiation. The optimal catalytic dosage for this process was found to be 1.0 g L −1 . The photodegradation favored under acidic conditions, and the rates decreased with the increase of pH. The main active species in pirimicarb photodegradation were found to be • OH and • O 2 − radicals based on scavenger and ESR experiments, while h + showed to play a secondary role in the reaction. Possible routes of the pirimicarb photodegradation were proposed involving dealkylation and decarbamoylation pathways. The Pt/AgInS 2 catalytic system demonstrated chemical stability and durable photocatalytic activity in different recycling experiments. The Pt/AgInS 2 photocatalyst was tested in actual scenarios for pirimicarb degradation in lake and river water samples, revealing its practicality for water treatment.

Conflicts of Interest:
The authors declare no conflict of interest.