Monochloramine Formation and Decay in the Presence of after Advanced Oxidation
Publication: Journal of Environmental Engineering
Volume 146, Issue 6
Abstract
When treating drinking water using advanced oxidation, the residual is usually quenched to allow for downstream chlorine stability. In some utilities, monochloramine () is used for secondary disinfection, and may not need to be quenched because and can coexist for some time. However, when ammonia and chlorine are applied to form in the -containing water, will compete with ammonia to react with the applied chlorine, compromising the formation efficiency. This research combined theory and experiments to evaluate formation efficiency in the presence of in Lake Ontario water and, after formation, its subsequent decay at different temperatures and pH. The results demonstrated that at many typical temperatures and pH, the presence of does not significantly impair the formation of . Furthermore, while accelerates decay, the results suggest that under specific conditions, such as short to medium residence times (e.g., less than 48 h), it may be possible for to coexist with as much as without compromising secondary disinfection.
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Data Availability Statement
All data, models, and code generated or used during the study appear in the published article.
Acknowledgments
This work was funded by the Natural Sciences and Engineering Research Council of Canada through the Industrial Research Chair program (Project No. IRCPJ 428979-16).
References
Collins, J., and J. R. Bolton. 2016. Advanced oxidation handbook. Denver: American Water Works Association.
Davies, G., and K. Kustin. 1973. “Hydrogen peroxide-chlorine reaction and its catalysis by manganese(III)-manganese(II).” Inorg. Chem. 12 (4): 961–962. https://doi.org/10.1021/ic50122a059.
Duirk, S. E., B. Gombert, J.-P. Croué, and R. L. Valentine. 2005. “Modeling monochloramine loss in the presence of natural organic matter.” Water Res. 39 (14): 3418–3431. https://doi.org/10.1016/j.watres.2005.06.003.
Duirk, S. E., and R. L. Valentine. 2006. “Modeling dichloroacetic acid formation from the reaction of monochloramine with natural organic matter.” Water Res. 40 (14): 2667–2674. https://doi.org/10.1016/j.watres.2006.05.010.
Held, A. M., D. J. Halko, and J. K. Hurst. 1978. “Mechanisms of chlorine oxidation of hydrogen peroxide.” J. Am. Chem. Soc. 100 (18): 5732–5740. https://doi.org/10.1021/ja00486a025.
Hoffmann, M. R., and J. O. Edwards. 1975. “Kinetics of the oxidation of sulfite by hydrogen peroxide in acidic solution.” J. Phys. Chem. 79 (20): 2096–2098. https://doi.org/10.1021/j100587a005.
Huang, Y., Z. Nie, C. Wang, Y. Li, M. Xu, and R. Hofmann. 2018. “Quenching residuals after oxidation using GAC in drinking water treatment.” Environ. Sci.: Water Res. Technol. 4 (10): 1662–1670. https://doi.org/10.1039/C8EW00407B.
Kim, H.-Y. 2013. “Statistical notes for clinical researchers: Assessing normal distribution (2) using skewness and kurtosis.” Restor. Dent. Endodontics 38 (1): 52–54. https://doi.org/10.5395/rde.2013.38.1.52.
Kruithof, J. C., P. C. Kamp, and B. J. Martijn. 2007. “ treatment: A practical solution for organic contaminant control and primary disinfection.” Ozone: Sci. Eng. 29 (4): 273–280. https://doi.org/10.1080/01919510701459311.
Li, J., A. Zamyadi, and R. Hofmann. 2016. “Effect of granular activated carbon type and age on quenching residuals after drinking water treatment.” J. Water Supply: Res. Technol.-Aqua 65 (1): 28–36. https://doi.org/10.2166/aqua.2015.134.
Makower, B., and W. C. Bray. 1933. “The rate of oxidation of hydrogen peroxide by chlorine in the presence of hydrochloric acid.” J. Am. Chem. Soc. 55 (12): 4765–4776. https://doi.org/10.1021/ja01339a006.
McKay, G., B. Sjelin, M. Chagnon, K. P. Ishida, and S. P. Mezyk. 2013. “Kinetic study of the reactions between chloramine disinfectants and hydrogen peroxide: Temperature dependence and reaction mechanism.” Chemosphere 92 (11): 1417–1422. https://doi.org/10.1016/j.chemosphere.2013.03.045.
Qiang, Z., and C. D. Adams. 2004. “Determination of monochloramine formation rate constants with sopped-flow spectrophotometry.” Environ. Sci. Technol. 38 (5): 1435–1444. https://doi.org/10.1021/es0347484.
Stefan, M. I. 2018. Advanced oxidation processes for water treatment: Fundamentals and applications, 710. Edited by M. I. Stefan. London: International Water Association Publishing.
Vikesland, P. J., K. Ozekin, and R. L. Valentine. 2001. “Monochloramine decay in model and distribution system waters.” Water Res. 35 (7): 1766–1776. https://doi.org/10.1016/S0043-1354(00)00406-1.
Wang, C., M. Hofmann, A. Safari, I. Viole, S. Andrews, and R. Hofmann. 2019. “Chlorine is preferred over bisulfite for quenching following UV-AOP drinking water treatment.” Water Res. 165 (Nov): 115000. https://doi.org/10.1016/j.watres.2019.115000.
Yokosuka, F., T. Kurai, A. Okuwaki, and T. Okabe. 1975. “Oxidation of sodium thiosulfate with hydrogen peroxide and sodium hypochlorite.” Nippon Kagaku Kaishi 1975 (11): 1901–1909. https://doi.org/10.1246/nikkashi.1975.1901.
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©2020 American Society of Civil Engineers.
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Received: Aug 21, 2019
Accepted: Nov 19, 2019
Published online: Mar 27, 2020
Published in print: Jun 1, 2020
Discussion open until: Aug 27, 2020
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