Kinetics of hydrogen peroxide quenching following UV/H2O2 advanced oxidation by thiosulfate, bisulfite, and chlorine in drinking water treatment

Tianyi Chen, Lizbeth Taylor-Edmonds, Susan Andrews, Ron Hofmann

PDF(1383 KB)
PDF(1383 KB)
Front. Environ. Sci. Eng. ›› 2023, Vol. 17 ›› Issue (12) : 147. DOI: 10.1007/s11783-023-1747-4
RESEARCH ARTICLE

Kinetics of hydrogen peroxide quenching following UV/H2O2 advanced oxidation by thiosulfate, bisulfite, and chlorine in drinking water treatment

Author information +
History +

Highlights

● H2O2 quenching rates by Cl/S-based chemicals were measured

● Chlorine takes seconds-to-minutes to quench H2O2 at common water pH

● The form of chlorine (gas vs . hypochlorite) affects the H2O2 quenching rate

● H2O2 quenching rates by chlorine in different conditions were predicted

Abstract

Residual H2O2 from UV/H2O2 treatment can be quenched by thiosulfate, bisulfite, and chlorine, but the kinetics of these reactions have not been reported under the full range of practical conditions. In this study, the rates of H2O2 quenching by these compounds were compared in different water matrices, temperatures, pH, and when using different forms of bisulfite and chlorine. In general, it was confirmed that thiosulfate would be too slow to serve as a quenching agent in most practical scenarios. At pH 7–8.5, chlorine tends to quench H2O2 more than 20 times faster than bisulfite in the various conditions tested. An important observation was that in lightly-buffered water (e.g., alkalinity of 20 mg/L as CaCO3), the form of chlorine can have a large impact on quenching rate, with gaseous chlorine slowing the reaction due to its lowering of the pH, and hypochlorite having the opposite effect. These impacts will become less significant when water buffer capacity (i.e., alkalinity) increases (e.g., to 80 mg/L as CaCO3). In addition, water temperature should be considered as the time required to quench H2O2 by chlorine at 4 °C is up to 3 times longer than at 20 °C.

Graphical abstract

Keywords

UV/H2O2 / H2O2 quenching / Chlorine type / Water alkalinity / Temperature

Cite this article

Download citation ▾
Tianyi Chen, Lizbeth Taylor-Edmonds, Susan Andrews, Ron Hofmann. Kinetics of hydrogen peroxide quenching following UV/H2O2 advanced oxidation by thiosulfate, bisulfite, and chlorine in drinking water treatment. Front. Environ. Sci. Eng., 2023, 17(12): 147 https://doi.org/10.1007/s11783-023-1747-4

References

[1]
Breytenbach L, van Pareen W, Pienaar J J, van Eldik R. (1994). The influence of organic acids and metal ions on the kinetics of the oxidation of sulfur(IV) by hydrogen peroxide. Atmospheric Environment, 28(15): 2451–2459
CrossRef Google scholar
[2]
Dotson A D, Keen V S, Metz D, Linden K G. (2010). UV/H2O2 treatment of drinking water increases post-chlorination DBP formation. Water Research, 44(12): 3703–3713
CrossRef Google scholar
[3]
Held A M, Halko D J, Hurst J K. (1978). Mechanisms of chlorine oxidation of hydrogen peroxide. Journal of the American Chemical Society, 100(18): 5732–5740
CrossRef Google scholar
[4]
Hoffmann M R, Edwards J O. (1975). Kinetics of the oxidation of sulfite by hydrogen peroxide in acidic solution. Journal of Physical Chemistry, 79(20): 2096–2098
CrossRef Google scholar
[5]
Huang Y, Nie Z, Wang C, Li Y, Xu M, Hofmann R. (2018). Quenching H2O2 residuals after UV/H2O2 oxidation using GAC in drinking water treatment. Environmental Science. Water Research & Technology, 4(10): 1662–1670
CrossRef Google scholar
[6]
Kan E, Koh C I, Lee K, Kang J. (2015). Decomposition of aqueous chlorinated contaminants by UV irradiation with H2O2. Frontiers of Environmental Science & Engineering, 9(3): 429–435
CrossRef Google scholar
[7]
Kerker M. (1957). The ionization of sulfuric acid. Journal of the American Chemical Society, 79(14): 3664–3667
CrossRef Google scholar
[8]
Kruithof J C, Kamp P C, Martijn B J. (2007). UV/H2O2 treatment: a practical solution for organic contaminant control and primary disinfection. Ozone Science and Engineering, 29(4): 273–280
CrossRef Google scholar
[9]
Lagrange J, Pallares C, Wenger G, Lagrange P. (1993). Electrolyte effects on aqueous atmospheric oxidation of sulphur dioxide by hydrogen peroxide. Atmospheric Environment. Part A, General Topics, 27(2): 129–137
CrossRef Google scholar
[10]
Lister M W. (1952). The decomposition of hypochlorous acid. Canadian Journal of Chemistry, 30(11): 879–889
CrossRef Google scholar
[11]
Liu W, Andrews S A, Stefan M I, Bolton J R. (2003). Optimal methods for quenching H2O2 residuals prior to UFC testing. Water Research, 37(15): 3697–3703
CrossRef Google scholar
[12]
Lu S, Wang N, Wang C. (2018). Oxidation and biotoxicity assessment of microcystin-LR using different AOPs based on UV, O3 and H2O2. Frontiers of Environmental Science & Engineering, 12(3): 12
CrossRef Google scholar
[13]
Lu Y, Gao Q, Xu L, Zhao Y, Epstein I R. (2010). Oxygen-sulfur species distribution and kinetic analysis in the hydrogen peroxide-thiosulfate system. Inorganic Chemistry, 49(13): 6026–6034
CrossRef Google scholar
[14]
Maaß F, Elias H, Wannowius K J. (1999). Kinetics of the oxidation of hydrogen sulfite by hydrogen peroxide in aqueous solution. Atmospheric Environment, 33(27): 4413–4419
CrossRef Google scholar
[15]
Mader P M. (1958). Kinetics of the hydrogen peroxide-sulfite reaction in alkaline solution. Journal of the American Chemical Society, 80(11): 2634–2639
CrossRef Google scholar
[16]
Sharma V K, Yu X, McDonald T J, Jinadatha C, Dionysiou D D, Feng M. (2019). Elimination of antibiotic resistance genes and control of horizontal transfer risk by UV-based treatment of drinking water: a mini review. Frontiers of Environmental Science & Engineering, 13(3): 37
CrossRef Google scholar
[17]
StefanM I (2017). Chapter 2: UV/Hydrogen Peroxide Process. Advanced Oxidation Processes for Water Treatment: Fundamentals and Application, 7–123
[18]
Wang C, Hofmann M, Safari A, Viole I, Andrews S, Hofmann R. (2019). Chlorine is preferred over bisulfite for H2O2 quenching following UV-AOP drinking water treatment. Water Research, 165(15): 115000
CrossRef Google scholar
[19]
Wang T X, Margerum D W. (1994). Kinetics of reversible chlorine hydrolysis: temperature dependence and general-acid/base-assisted mechanisms. Inorganic Chemistry, 33(6): 1050–1055
CrossRef Google scholar
[20]
van Klassen N, Marchington D, McGowan H C E. (1994). H2O2 Determination by the I3 method and by KMnO4 Titration. Analytical Chemistry, 66(18): 2921–2925
CrossRef Google scholar
[21]
van McArdle J, Hoffmann M R. (1983). Kinetics and mechanism of the oxidation of aquated sulfur dioxide by hydrogen peroxide at low pH. Journal of Physical Chemistry, 87: 5425–5429
CrossRef Google scholar

Acknowledgements

We acknowledge AECOM and the City of Toronto for their support and collaboration. This work was supported through the Natural Sciences and Engineering Grant CRDPJ-542302-2019, by AECOM and by the City of Toronto.

Conflict of Interest

The authors declare that the research was conducted in the absence of any commercial or financial relationships that could be construed as a potential conflict of interest.

Electronic Supplementary Material

Supplementary material is available in the online version of this article at https://doi.org/10.1007/s11783-023-1747-4 and is accessible for authorized users.

RIGHTS & PERMISSIONS

2023 Higher Education Press
AI Summary AI Mindmap
PDF(1383 KB)

Accesses

Citations

Detail

Sections
Recommended

/