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Perovskite-like oxides SrCo1−xTixO3−δ (SCTx, x=0.1, 0.2, 0.4, 0.6) were used as heterogeneous catalysts to activate peroxymonosulfate (PMS) for phenol degradation under a wide pH range, exhibiting more rapid phenol oxidation than Co3O4 and TiO2. The SCT0.4/PMS system produced a high activity at increased initial pH, achieving optimized performance at pH≥7 in terms of total organic carbon removal, the minimum Co leaching and good catalytic stability. Kinetic studies showed that the phenol oxidation kinetics on SCT0.4/PMS system followed the pseudo-zero order kinetics and the rate on SCT0.4/PMS system decreased with increasing initial phenol concentration, decreased PMS amount, catalyst loading and solution temperature. Quenching tests using ethanol and tert-butyl alcohol demonstrated sulfate and hydroxyl radicals for phenol oxidation. This investigation suggested promising heterogeneous catalysts for organic oxidation with PMS, showing a breakthrough in the barriers of metal leaching, acidic pH, and low efficiency of heterogeneous catalysis.
Organic compounds containing wastewaters that are discharged from households and industries may produce hazardous impacts on human health and the environment. In recent years, this concern together with the limited clean water resources have led to the development of efficient remediation techniques for removal of the organic contaminants from wastewaters1. Currently, the removal of organic contaminants via advanced oxidation processes (AOPs) relies upon the generation of highly reactive species with high redox potentials2,3. Hydroxyl radical (·OH, E0=1.8–2.7V) is the most commonly used species in the Fenton reaction which demonstrates a high efficiency to oxidize organic compounds4. Nonetheless, some AOPs to generate hydroxyl radicals, such as Fenton reaction, ozonation and UV radiation, give rise to several drawbacks. Fenton reaction needs to be at acidic condition (pH of 3–4), production of large amount of sludge and leaching of metal ions5,6 while ozonation and UV radiation require high energy inputs7,8. Sulfate radicals (SO4·−, E0=2.5–3.1V) represent another active species that shows higher oxidation potential and longer half-life than hydroxyl radicals and they have been used to oxidize organic compounds such as phenol and its derivatives due to no limitation of reaction condition, faster reaction rate and lower energy requirements9,10,11,12.
The generation of sulfate radicals can be initiated via the activation of peroxymonosulfate (PMS) by photocatalysis13, transition metal catalysis14, and electrochemistry15. In particular, tradition metal activation, which involves homogeneous and heterogeneous catalysis, has been considered as the most effective process16,17. The associated metal ion leaching problems, however, limit the applicability of tradition metal catalysts, because of the hazardous risk of the metal ions to human health and the environment. The Fenton-like heterogeneous catalyst systems are more practical for phenol oxidation involving PMS activation. Co/PMS process has been reported to be highly effective for organic compound degradation despite the drawbacks of utilizing Co ions (for their subsequent pollution risk to the environment)18,19,20,21. Accordingly, several Co-based heterogeneous catalysts, e.g., Co oxides22, supported Co23,24, Co exchanged zeolites25,26, and bimetallic Co-based oxides27,28, have been studied for PMS activation, while the issue has not been fully resolved.
A perovskite oxide has a chemical formula of ABO3 in which alkaline earth metals or rare-earth metals can be incorporated into the A-site while transition metals can be incorporated into the B-site. The presence of oxygen vacancies from oxygen non-stoichiometry in concomitant with the redox couple from the transition metals endow such perovskite oxides mixed (oxygen) ionic-electronic conductivity and reduction-oxidation (redox) properties29, which are beneficial for applications in solid oxide fuel cells, oxygen permeation membranes, metal-air batteries, and electrochemical water splitting30,31,32,33. Taran et al. reported the catalytic activity of LaCuO3 for wet peroxide oxidation of phenol, which indicates the potential applicability of perovskite oxides for catalytic oxidation34. Nevertheless, perovskite oxides have been barely used in AOPs for PMS activation35.
In this work, we reported that Ti-doped SrCoO3−δ (SCO) perovskites can effectively activate PMS for generation of sulfate radicals. The synthesized SrCo1−xTixO3−δ (SCTx, x=0, 0.1, 0.2, 0.4, and 0.6), in fact, demonstrated a higher catalytic activity with respect to Co3O4. In terms of the minimum Co ion leaching, SCT0.4 is viewed as the best catalyst which also showed a high catalytic activity for phenol oxidation. The effects of initial phenol concentration, PMS amount, catalyst loading, and solution temperatures on SCT0.4/PMS system for phenol degradation were evaluated. Furthermore, in figuring out the most plausible mechanism of activation, we also evaluated the effect of solution pH and studied the oxidation kinetics in the presence of ethanol and tert-butyl alcohol that react distinctly to sulfate and hydroxyl radicals. It was found that SCT0.4/PMS presented higher efficiencies in organic degradation at high pH, which can overcome the common problems of Fenton reaction and provide a promising application for real wastewater treatments under alkaline conditions.
A combined ethylenediaminetetraacetic acid-citric acid (EDTA-CA) complexing sol-gel route36 was used to synthesize the perovskite oxide catalysts, SrCo1−xTixO3−δ (SCTx, x=0.1, 0.2, 0.4, and 0.6). Detailed information is presented in supplementary data.
The properties of catalysts were investigated by various techniques, which are detailed in supplementary data.
Batch oxidation tests of phenol degradation were carried out in a 1L glass vessel containing 500mL of phenol solution (with a concentration of 20 ppm), SrCo0.6Ti0.4O3−δ (SCT0.4, 0.1gL−1) and peroxymonosulphate (PMS, 2gL−1) under continuous stirring (250rpm) in a temperature-controlled water bath at 25°C. Detailed information is presented in supplementary data.
The phase structure of the SCTx (x=0.1, 0.2, 0.4, and 0.6) catalysts calcined at 1000°C for 6h was obtained by powder X-ray diffraction (XRD) and their patterns are shown in Fig. 1(a). The characteristic peaks of all samples can be indexed according to the primitive cubic perovskite lattice with a space group Pmm (#221)30. In Fig. 1(a), SCTx have stronger intensity of diffraction peaks of perovskites than SCO, which presented higher stability of perovskite-type structure. Compared with the XRD patterns of SCO and TiO2 (see Fig. 1(a)), SCTx (x=0.1, 0.2, 0.4, 0.6), which exhibited the single phase, at varying ratio of Ti addition will not change the perovskite-type structure. The characteristic peaks of all perovskites overlap each other, suggesting almost identical lattice parameters for all the perovskites. With increasing Ti content, the most intense characteristic peak at around 2θ of 33° appears to shift slightly toward the lower angles. This indicates an expansion of SCTx lattice, due to the partial substitution of Co by Ti (Note that Co3+(VI) HS (high spin) has an ionic radius of 0.61Å while Ti4+(VI) has an ionic radius of 0.75Å)37.
The particulate morphology of SCTx (x=0.1, 0.2, 0.4, and 0.6) was then carried out by SEM and the typical images are shown in Fig. 1(b). Ti-doped SrCoO3−δ samples clearly experienced significant agglomeration during calcination at 1000°C for 6h, which had a large size of 1–5 μm. An increase in Ti content (or equivalently, the increase in x) somewhat led to the loosening of grain agglomeration (Fig. 1(b)). Relatively identical nano-sized grains of 10–20nm are nonetheless observed for all four samples (See Fig. 1(b)). Nitrogen sorption furthermore reveals an increasing Brunauer-Emmett-Teller specific surface area (SBET) with increasing Ti content, i.e., the surface area increased from 0.4m2g−1 for x=0 to 1.2m2g−1 for x=0.6 (Supplementary Table S1) that supports the SEM observation.
To explore the capability of perovskite oxides for removing phenol, the toxic organic with stable structure, adsorption and/or oxidation of phenol in the presence or absence of different oxide catalysts, with or without PMS were tested, as shown in Fig. 1(c). To provide baselines for the catalytic performance comparison, oxide catalyst self-adsorption and PMS self-oxidation were firstly checked. PMS clearly could not induce any noticeable phenol degradation in the absence of catalysts. In this case, less than 5% of phenol was removed during 90min. Adsorption of phenol on Co3O4, TiO2, or SCT0.1 was the only possible mechanism in the absence of PMS. Such adsorption may not translate to effective phenol removal given the low surface areas of these oxides. Accordingly, less than 5% of phenol was removed during the 90 min-period which implies negligible phenol adsorption on these oxides.
Oxidations occurred when both oxide catalysts (i.e., Co3O4, TiO2, or SCT0.1) and PMS were present, in which phenol degradations become more pronounced. These oxidations are related to the activation of PMS to generate sulfate and hydroxyl radicals that can degrade phenol. SCT0.1/PMS system showed the largest catalytic activity, degrading the phenol in 15min. For Co3O4 and TiO2, however, only ~60% and ~10% of the phenol were degraded in 90min, respectively. The catalytic performance thus increased in an order of TiO2<Co3O4<SCT0.1 (see Fig. 1(c)). Moreover, the total organic carbon (TOC) analysis showed that about 78% of phenol could be mineralized to CO2 after 2 h-oxidation using SCT0.1/PMS system. And compared with Co3O4 (14.4 m2g−1) and TiO2 (9.5 m2g−1), SCT0.1 (0.4 m2g−1) has the lowest specific surface area (Supplementary Table S1), which all investigated that SCT0.1 has the excellent catalytic performance for phenol oxidation with PMS activation.
The catalytic performances of SCTx (x=0.1, 0.2, 0.4, and 0.6) was also investigated in the PMS activation for the oxidative degradation of phenol (Fig. 1(d)). SCT0.2 showed the highest catalytic degradation efficiency. Increasing surface area for the perovskite with increasing Ti content did not appear to well correlate with the catalytic improvement for phenol oxidation (Supplementary Table S1). The general trend (Fig. 1(d)) indicates a decreasing rate of phenol oxidation with increasing titanium (Ti) content on the perovskite although SCT0.6 can still be considered as a highly active catalyst given its capability to completely oxidize phenol within 45min in the presence of PMS. The leaching of metal ions from the perovskite matrix to the solution was evaluated using ICP-AES. Co concentration in the filtrate varies from 3.1 to 5.4mgL−1 (at pH of 3–4) which implies substantial leaching out of Co from SCTx in acidic condition. Co concentration appears to decrease with increasing Ti content in the perovskite. On the other hand, Ti leaching is not as obvious as Co considering its relatively lower concentration, i.e. below 1.0mgL−1 in all perovskite cases. Therefore, it is a trade-off to obtain both maximized catalytic activity and minimized Co leaching. SCT0.4 showed a similar Co concentration of 3.1mgL−1 to SCT0.6, indicating either SCT0.4 or SCT0.6 could be chosen. The TOC analysis for SCTx (x=0.1, 0.2, 0.4, and 0.6) showed the maximum TOC reduction on SCT0.2 (82% TOC reduction) after 5h phenol oxidation (Inset of Fig. 1(d)). SCT0.4 could reduce about 77% of TOC over this duration. So given their identical Co leaching level and higher catalytic activity of SCT0.4, more tests were then focused on SCT0.4.
As phenol was efficiently degraded by SCT0.4-activated PMS, we investigated SCT0.4/PMS system for phenol under different operating conditions, such as initial phenol concentration, PMS amount, catalyst loading and reaction temperature. Figure 2(a) displays the kinetic dependence of phenol oxidation on initial phenol concentration (C0). The inset of Fig. 2(a) further shows the dependence of the reaction rate constant (k) for phenol oxidation on the initial phenol concentration (C0). Phenol oxidation at 100% is attained within 30min when the initial phenol concentration is less than 40mgL−1, while the oxidations at only 71% and 64% are attained for the initial phenol concentrations of 60mgL−1 and 80mgL−1, respectively. Considering a fixed amount of catalyst, Fernandez et al.21. and Shulkla et al.38. provided a pseudo-zero-order kinetics of phenol removal, which is presented by the following equation:
where kCo is the apparent zero order constant, Cph is the phenol concentration at any instant time (t), V is the volume of reactor, and W is the mass of catalyst. Therefore, the mathematical model of the degradation profile in Fig. 2(a,b,c,d) is induced by the integration of the above Equation (1). Shukla et al. also studied the kinetics of phenol oxidation by heterogeneous activation of PMS with different Co catalysts and reported that zero-order or first-order kinetics may occur depending on the catalysts used24,25,38,39. Table 1 shows the rate constants and the regression coefficients followed the pseudo-zero-order kinetics at four different initial phenol concentrations. The reaction rate decreased with the increasing initial phenol concentration. The reasonably good fittings are indicated by the high values of regression coefficients (R2>0.97).
The PMS amount also shows a significantly effect on kinetic phenol oxidation in Fig. 2(b). Higher amount of PMS led to a higher oxidation rate which translates to reduced time for complete oxidation of PMS. For example, when double amount of PMS was added, i.e., 1.5g of PMS relative to 0.75g of PMS, phenol oxidation could be completed within 10min instead of 20min.
Besides, the phenol oxidation kinetic dependence on the catalyst loading was probed as displayed in Fig. 2(c). Likewise, an increase in catalyst loading also correlates with the increase in the reaction rate. This is consistent with the expected increase of the active sites (Co) for phenol oxidation that enhances the generation of sulfate and hydroxyl radicals24.
Phenol degradation by SCT0.4-activated PMS was conducted at different reaction temperatures to further study the catalytic activity of SCT0.4 for the activation of PMS. Figure 2(d) shows phenol oxidations at three different solution temperatures, 15, 25, and 35 °C while complete phenol oxidations were attained within 50, 20, and 10min, respectively. Such an increase in reaction rate with increasing solution temperature highlights the endothermic nature of the phenol oxidation on SCT0.4/PMS system. The inset of Fig. 2(d) displays the thermal-dependent Arrhenius representation of the pseudo-zero order reaction rate constant (k) for phenol oxidation. By using the pseudo-zero order kinetic equation and the Arrhenius equation, the activation energy (Ea) for the oxidation process was obtained as 77.5kJmol−1 (see Table 2). The absence of perovskite data for PMS activation means that the activation energies for phenol oxidation on SCT0.4/PMS system should be compared to phenol oxidations on the other more widely studied catalyst systems (Table 2). As we all know, one of critical factors influencing on the reaction activation energy is catalysts. Therefore, Table 2 showed that the phenol oxidation with different catalysts have different activation energies. Co-SiO2 and Co-ZSM-5, in particular, showed the closest activation energies to SCT0.4/PMS system. Co/AC and Co/Fly-ash exhibited the lower activation energy.
As a heterogeneous catalyst, the recyclability of SCT0.4 is critical for practical implication. Figure 2(e) depicts the performance of the recycled SCT0.4 catalyst for phenol degradation. The catalyst was recovered using filtration followed by mild washing with de-ionized water while the filtrate was stored for further analysis. The reused SCT0.4 catalyst can still catalyze complete phenol oxidation within 60min after three subsequent recycles. It showed more pronounced decrease in the activity after the first recycle followed by less decrease in activities in the subsequent recycles. TOC analysis showed that the TOCs were reduced by 76.2% and 75.3% during the first 2h period of phenol oxidations in the first and second runs, respectively (see Supplementary Table S3). Increasing the reaction time up to 6h can improve the TOC reduction to above 80% even after the second recycle (see Supplementary Table S3).
The leaching of Co2+ from perovskite matrix was inevitable given the necessary long term contact and constant mixing between the perovskite catalysts and the aqueous phase. We also tested phenol oxidation using Co2+/PMS system in an analogous mole amount to SCT0.4 as well as phenol oxidation using the filtrate from the previous SCT0.4/PMS system of the first run. The phenol oxidation on Co2+/PMS system was more rapid than the phenol oxidation on filtrate/PMS. This suggests that cobalt leaching did occur but it was at a much lower rate reflected by its low reaction rate.
We also did some characterizations of the reused SCT0.4 to study its stability. Figure 2(f) shows the powder XRD patterns of the catalysts before and after the phenol oxidation for 2h to check the possible changes in the phase compositions. The main perovskite phase of SCT0.4 was retained although unknown phase(s) appeared afterwards, which are likely due to decomposition of the perovskite phase caused by metal leaching40 and carbonate adsorption on the solid surface34.
The changes in the surface composition of the fresh and used SCT0.4 catalysts were further evaluated using X-ray photoelectron spectroscopy (XPS). Figure 3(a) displays the survey scan on SCT0.4 surface, evidencing the presence of Sr, Co, Ti, and O elements. The high resolution Sr 3d XPS spectra for the fresh and used SCT0.4 catalysts (Fig. 3(b)) further reveal the formation of four peaks at 134.9eV, 133.8eV, 133.0eV, and 131.8eV. Sr 3d3/2 components are located at higher binding energy (BE) while 3d5/2 components are located at lower BE41. Accordingly, Sr 3d5/2 peak at 131.8eV and Sr 3d3/2 peak at 133.0eV correspond to Sr in the perovskite phase42. Sr 3d peak at approximately 133.8eV, on the other hand, is likely related to the strontium carbonate on the surface34,43,44.
Figure 3(c) further shows the high resolution Co 2p XPS spectra for the fresh and used SCT0.4 catalysts. The Co 2p spectra contain 2p1/2 and 2p3/2 components. The peaks at 786.4eV and 802.9eV were the additional satellite peaks for Co 2p1/2 and Co 2p3/2, respectively. The peak located at BE of 781.2eV (Co 2p3/2) represents Co3+ while the peak located at BE of 780.1eV (Co 2p3/2) represents Co2+, consistent with the literature27,43,44. The peaks corresponding to Co3+ and Co2+ can be deconvoluted to determine their peak areas. Accordingly, Co3+ to Co2+ ratio increased from 1.93 to 2.93 after the phenol oxidation for 2h. This may indicate the activity of Co2+/Co3+ redox couple (SCT0.4-Co(II)/SCT0.4-Co(III)) in catalyzing the phenol oxidation in the presence of PMS. However, the average cobalt oxidation states were calculated approximately to be 2.71 and 2.73 in the fresh and used SCT0.4, respectively. The results suggest that the cobalt oxidation states in the phase of perovskite were almost unchanged, which indicates the stability of SCT0.4 in the catalytic process of phenol oxidation, and the metal leaching is likely to be mainly caused by the perovskite oxides dissolved in the acidic solution.
The high resolution Ti 2p XPS spectra for the fresh and used SCT0.4 catalysts are depicted in Fig. 3(d) which features two peaks for 2p3/2 and 2p1/2 components at 457.5eV and 463.2eV, respectively; both of which can be assigned to Ti4+. Despite the slight shift in the binding energy, Ti ions in perovskite existed as Ti4+ after the phenol oxidation for 2h.
Figure 3(e) shows the high resolution O 1s XPS spectra for the fresh and used SCT0.4 catalysts. The oxygen O 1s peak can be deconvoluted into four sub-peaks. The peak at BE of approximately 528.4eV represents the lattice oxygen within the perovskite oxides4. The other two peaks at BE of approximately 529.7eV and 531.2eV can be ascribed to the chemisorbed oxygen which co-existed in the form of O22− and O− at the surface. The peak at the highest BE of around 532.6eV, on the other hand, can be assigned to OH from the hydroxyl groups or carbonates27,42,44. Carbonates may be generated during the complex adsorption process of organic compounds or during the oxidation reactions that involves the formation of carbon-based intermediates34, likely corresponding to the unknown phase(s) in the XRD of Fig. 2(f). Therefore, the carbonate adsorption on the surface of SCT0.4 after reaction may cause the deactivation of SCT0.4 during the subsequent reuses.
For the aqueous reaction of PMS activation, initial pH of reaction solution is an important factor to influence the interfacial interactions between PMS, organics and catalysts45 and was further investigated. Figure 4(a) presents the phenol oxidation on SCT0.4/PMS system at different initial solution pH. The pH of the original phenol solution is around 6. We used 0.1M H2SO4 or 0.1M KOH to adjust the initial solution pH. Relative to the neutral condition (pH of 7), higher acidity lowers the oxidation rate while higher alkalinity is in the opposite way. The effect of pH on the phenol degradation rate was attributed to the concentration change of the active radicals in the solution. When the pH is below 7, OH− ions react with H+ ions in neutralization reaction to generate water. This essentially inhibits the two primary reactions that generate hydroxyl radicals (·OH, See Equations (5) and (6) which will be discussed below). Likewise, increasing the amount of OH− served to shift these reaction equilibria to the products, thus favoring the generation of hydroxyl radicals.
It is interesting that the TOC reduction (after 2h) trend did not exactly follow the phenol oxidation rate trend. Maximum TOC reduction was observed at the neutral condition (pH of 7) (See inset of Fig. 4(a)). The fact that the TOC reduction for the initial pH=9 was actually lower than that at the initial pH=7 can be rationalized in terms of the derived phenoate (that was formed in an alkaline condition) which may slow down the reactivity of phenol and reaction intermediates in oxidation processes46.
The initial solution pH also showed a significant effect on metal ion leaching. The concentration of metal ions in the solution sharply decreased by increasing initial solution pH. Taking Co leaching as an example, with respect to the initial pH=6 where no H2SO4 or KOH was added, the initial pH=6 resulted in the lower concentration of cobalt ions in the solution (CCo=3.1mgL−1). Increasing the pH further as represented by the initial pH=9 led to an even lower concentration of cobalt ions in the solution (CCo=2.2mgL−1).
Maintaining the solution pH neutral (pH of 7) by constant pH monitoring and periodic addition of KOH) throughout the oxidation process minimized the Co leaching problem. Compared to the initial pH=6, much lower concentration of cobalt ions in the solution was obtained (CCo=1.3mgL−1). This additionally resulted in a more rapid phenol oxidation than the initial pH=9 (Compare Fig. 4(a) with Fig. 4(d) and note the different y-axis representations). By keeping the solution pH at 7 throughout the oxidation process, complete phenol oxidation can be achieved within 10min as opposed to 20min required for the initial pH=9. The preservation of neutral pH during the oxidation course clearly optimized the phenol oxidation performance on SCT0.4/PMS system.
Several studies have reported that PMS activation using metal-based catalysts involve of two key active radicals, i.e., sulfate radicals (SO4·−) and hydroxyl radicals (·OH)10,47,48,49. To reveal the phenol degradation mechanism in SCT0.4/PMS system, different radical inhibitors, ethanol (EtOH) and tert-butyl alcohol (TBA), were employed to evaluate the reaction. It is worth noting that EtOH (with α-H) readily reacts with both SO4·− and ·OH whereas TBA (without α-H) reacts mainly with ·OH and is inert to SO440,50,51. Figure 4(b,c,d) confirms that the phenol degradation rate was reduced with the presence of these radical inhibitors and their increasing concentrations. The presence of 0.2M EtOH led to k of 0.012mgL−1 min−1, lower than k of 0.016mgL−1 min−1 obtained in the presence of 0.2M TBA in the system. This suggests that both SO4·− and ·OH were generated in the PMS activation process using SCT0.4, where normally more SO4·− than ·OH formed, as reported in several previous works27,52,53. Moreover, Fig. 4(d) reveals that upon maintaining neutral condition (pH=7) throughout the oxidation course, more rapid phenol oxidation was obtained than that in the original oxidation case where the pH was not controlled. Relative to the original case, the phenol oxidation rate at the neutral condition increased by 1.95 times and 5.84 times for the tests with 0.2M EtOH and 0.2M TBA, respectively. This is likely due to the increased active radical species at such neutral condition. In the insert of Fig. 4(c,d), the presence of 0.2M TBA at the neutral condition k shows more higher value than that without pH control, whereas the presence of 0.2M EtOH keeps the similar phenol oxidation rate, which could be explained by more SO4·− generated than ·OH with pH control at 7, for that TBA reacts mainly with ·OH, but EtOH readily reacts with both them.
Our aforementioned characterization results and literature survey led us to propose the most plausible Fenton-like mechanism of phenol oxidation on SCT0.4/PMS system as follows:
SO4·− and ·OH are initially generated simultaneously by the activation of PMS on SCT0.4 (Equations (2) and (3)). Then a majority of the produced SO4·− radicals react with phenol rapidly, due to their higher potential (E0=2.5–3.1V)9. Moreover, some ·OH radicals also participate in the oxidation at a slower rate, leaving ·OH radicals as the only active species after all SO4·− has been consumed (Equation (7)). The Co2+/Co3+ redox couple on SCT0.4 (SCT0.4-Co(II)/SCT0.4-Co(III)) reacts in cycles with PMS to generate the reactive oxygen species (Equations (2), (3), and (4)). Moreover, the generated SO5·− radicals (Equation (4)), which have relatively low potential (E0=1.1V)54, react with OH− ions to produce ·OH radicals that completely oxidize (mineralize) phenol (Equation (7)).
We have demonstrated that SrCo1−xTixO3−δ (x=0.1, 0.2, 0.4, and 0.6) perovskite oxides exhibit a fast catalytic activity for phenol oxidation in the presence of PMS in a wide pH range. Powder XRD patterns showed cubic perovskite lattice and its stable structure in aqueous reaction. The catalytic performance for phenol oxidation presented an order of SCT0.6<SCT0.4<SCT0.1<SCT0.2. The operating conditions can be adjusted to increase the phenol oxidation rate by increasing PMS amount, catalyst loading, and initial pH. Under neutral and alkaline conditions, SrCo1−xTixO3−δ/PMS presented effective degradation efficiency of aqueous contaminants with less metal leaching and higher TOC reduction rate, which is better than Fenton-like systems and provides promising application for organic oxidation with sulfate radicals.
How to cite this article: Miao, J. et al. SrCo1−xTixO3−δ perovskites as excellent catalysts for fast degradation of water contaminants in neutral and alkaline solutions. Sci. Rep. 7, 44215; doi: 10.1038/srep44215 (2017).
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This work was financially supported by the National Nature Science Foundation of China (No. 21576135), the Priority Academic Program Development of Jiangsu Higher Education Institutions (PAPD), the Major Project of Educational Commission of Jiangsu Province of China (No. 13KJA430004), the Program for Jiangsu Specially-Appointed Professors, and the Youth Fund in Jiangsu Province (No. BK20150945).
The authors declare no competing financial interests.
Author Contributions W.Z., J.M., and C.S. conceived and designed the research; J.M. and C.S. carried out the experiments; J.M., C.S., W.Z., S.B.W. and Z.P.S. analyzed data and interpreted results; J.M. prepared figures and wrote the manuscript; J.S. W.Z. and S.B.W. edited and revised the manuscript; all authors reviewed and approved the manuscript.