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. 2023 Jan 20;13(5):3193-3203.
doi: 10.1039/d2ra07640c. eCollection 2023 Jan 18.

La2CoO4+ δ perovskite-mediated peroxymonosulfate activation for the efficient degradation of bisphenol A

Xin Zhong  1   2 , Wenting Wu  2 , Haonan Jie  2 , Fubin Jiang  1
Affiliations

La2CoO4+ δ perovskite-mediated peroxymonosulfate activation for the efficient degradation of bisphenol A

Xin Zhong et al. RSC Adv. .

Abstract

Sulfate radical-based technology has been considered as an efficient technology to remove pharmaceuticals and personal care products (PPCPs) with heterogeneous metal-mediated catalysts for the activation of peroxymonosulfate (PMS). In this study, La2CoO4+δ perovskite with Ruddlesden-Popper type structure was synthesised by the sol-gel method, which was employed in PMS activation. Different characteriazation technologies were applied for the characterization of La2CoO4+δ , such as SEM-EDX, XRD, and XPS technologies. A common organic compound, bisphenol A (BPA), is used as a target contaminant, and the effect impactors were fully investigated and explained. The results showed that when the dosage of La2CoO4+δ was 0.5 g L-1 and the concentration of PMS was 1.0 mM in neutral pH solution, about 91.1% degradation efficiency was achieved within 25 minutes. Quenching experiments were introduced in the system to verify the catalytic mechanism of PMS for the BPA degradation, proving the existence of superoxide, hydroxyl radicals and sulfate radicals, which are responsible for the catalytic degradation of BPA. Moreover, the reusability and stability of the catalyst were also conducted which showed good stability during the reaction. This work would improve the applications of A2BO4-type perovskites for activating PMS to degrade BPA.

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Conflict of interest statement

There are no conflicts to declare.

Figures

Fig. 1
Fig. 1. (a) XRD patterns of fresh and used LCO catalyst; (b) isotherm image of LCO catalyst.
Fig. 2
Fig. 2. (a and b) SEM images of LCO catalyst; (c) EDX spectra of LCO catalyst; (d–f) mapping images of LCO catalyst.
Fig. 3
Fig. 3. XPS spectra of LCO (a) survey spectra; (b) La 3d; (c) Co 2p; (d) O 1s.
Fig. 4
Fig. 4. FTIR spectra of fresh and used LCO catalyst.
Fig. 5
Fig. 5. BPA degradation in different reaction systems. Reaction conditions: [BPA] = 0.05 mM, [PMS] = 1.0 mM, [LCO] = 0.5 g L−1, initial PH = 6.8.
Fig. 6
Fig. 6. Effect of catalyst dosage on BPA degradation. Reaction conditions: [BPA] = 0.05 mM, [PMS] = 1.0 mM, [LCO] = 0.1–1.0 g L−1, initial PH = 6.8.
Fig. 7
Fig. 7. Effect of PMS concentration on BPA degradation. Reaction conditions: [BPA] = 0.05 mM, [PMS] = 0.1–1.0 mM, [LCO] = 0.5 g L−1, initial PH = 6.8.
Fig. 8
Fig. 8. Effect of initial pH on BPA degradation. Reaction conditions: [BPA] = 0.05 mM, [PMS] = 1.0 mM, [LCO] = 0.5 g L−1, initial PH = 3.1–9.1.
Fig. 9
Fig. 9. Effect of co-existing ions (a) Cl−; (b) HCO3− and (c) natural organic matter on BPA degradation. Reaction conditions: [BPA] = 0.05 mM, [PMS] = 1.0 mM, [LCO] = 0.5 g L−1, initial PH = 6.8.
Fig. 10
Fig. 10. Effect of radical scavengers on BPA degradation. Reaction conditions: [BPA] = 0.05 mM, [PMS] = 1.0 mM, [LCO] = 0.5 g L−1, initial PH = 6.8, [scavengers] = 0.2 M.
Fig. 11
Fig. 11. (a) Reusability of LCO on BPA degradation, (b) effect of water matrix on BPA degradation, (c) different contaminants in the LCO/PMS systems. Reaction conditions: [BPA] = 0.05 mM, [PMS] = 1.0 mM, [LCO] = 0.5 g L−1, initial PH = 6.8.
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