Photodegradation of haloacetic acids in water

Lifongo, Lydia L.; Bowden, Derek; Brimblecombe, Peter

doi:10.1016/j.chemosphere.2003.11.006

Cited by 80 publications

(47 citation statements)

References 43 publications

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“…Chloroacetic acids (CAAs) are formed upon the reaction of the added chlorine to water with the organic impurities for disinfection purposes [1] and through the use of chlorocarbon and chlorofluorocarbon replacement compounds in various industrial applications [2]. CAAs tend to accumulate in surface waters and pose threats to humans and the ecosystem due to their toxicity and high stability.…”

Section: Introductionmentioning

confidence: 99%

Electrocatalytic dechlorination of chloroacetic acids by silver nanoparticles modified glassy carbon electrode

Liu

Deng

et al. 2011

J Solid State Electrochem

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A simple potentiostatic method was employed to prepare silver nanoparticles deposited on glassy carbon electrode. The silver nanoparticles exhibit extraordinary electrocatalytic activities toward the reduction process of chloroacetic acids. The electrochemical behavior of trichloroacetic acid, dichloroacetic acid, and monochloroacetic acid has been investigated by cyclic voltammetry at the silver nanoparticles-modified glassy carbon electrode in 0.1 M LiClO 4 solution; each compound exhibits a series of reduction peaks which represent sequential dechlorination steps up to acetic acid. The electrocatalytic dechlorination mechanism for chloroacetic acids was also discussed in this work.

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Section: Introductionmentioning

confidence: 99%

Electrocatalytic dechlorination of chloroacetic acids by silver nanoparticles modified glassy carbon electrode

Liu

Deng

et al. 2011

J Solid State Electrochem

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“…When UV light illuminates at energy higher that the band gap of TiO 2 it generates conduction band electrons and valence band holes. The valence band hole can either be trapped at the surface of the TiO 2 or react with surface hydroxyl ions in water to from hydroxyl radical which oxidize phenol in both cases according (Lifongo, Bowden, & Brimblecombe, 2004): …”

Section: Resultsmentioning

confidence: 99%

Photocatalytic Degradation of Phenol using Fe-TiO2 by Different Illumination Sources

Shawabkeh¹,

Khashman²,

Bisharat³

2010

IJC

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A Fe-doped titanium dioxide (Fe-TiO 2 ) was prepared using hydrothermal method and used for degradation of phenol from aqueous solution. The samples were characterized by X-ray diffraction (XRD) and showed a presence of both TiO 2 and Fe 2 O 3 peaks. The photocatalytic activity of Fe-TiO 2 catalyst was evaluated for oxidation of phenol in aqueous solution using different illumination sources. Visible light irradiation from sun, UV light sources with 190 and 390 nm, fluorescence and dark environment were used and found that the degradation of phenol was in the order of 7.8%, 12%, 7.5%, 6.8% and 5% obtained after 24 h, respectively. It was found that the increase in exposure time to UV, the increase in solution temperature and pH have increased the rate of phenol degradation in solution. This rate was best fitted using first order kinetic model with reaction constant of 3 10 268 . 6 − × .

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“…Numerous studies have demonstrated that monochloroacetate is toxic to aquatic life, in particular to algae (Ku¨hn & Pattard 1990); MCA was recognized as the most toxic of all haloacetates toward several aquatic macrophytes, although toxicity was observed for concentrations higher than currently met in the environment (Hanson & Solomon 2004). Chloroacetic acid has relatively long lifetime in natural environment (Ellis et al 2001) which may result from its resistance to photodegradation (Lifongo et al 2004). On the other hand, spontaneous microbial dehalogenation of MCA in surface waters has been reported (Hashimoto et al 1998;Ellis et al 2001).…”

Section: Introductionmentioning

confidence: 97%

Biodegradation of monochloroacetic acid used as a sole carbon and energy source by Xanthobacter autotrophicus GJ10 strain in batch and continuous culture

Torz

Beschkov

2005

Biodegradation

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Batch and continuous mode degradation of monochloroacetic acid used as a sole carbon and energy source in the concentration range of 0.9-48.4 mM by pure culture of Xanthobacter autotrophicus GJ10 was investigated. The substrate was completely degraded in each flask in batch system. Partial substrate inhibition occurred at the concentrations exceeding 25.4 mM. Temporary accumulation of glycolic acid in the medium indicated that dehalogenation was undergoing faster than further utilization of glycolate. Three different carbon substrates were used for inoculum preparation--1,2-dichloroethane, tri-sodium citrate and a nutrient broth. The fastest growth on monochloroacetate occurred for 1,2-dichloroethane-grown inoculum. The assays of haloacid dehalogenase in crude extract indicated that the bacteria grown on 1,2-dichloroethane possessed higher level of the enzyme. The response of the GJ10 culture towards spikes of 20 mM monochloroacetate was tested in 2.5-1 continuously stirred tank fermentor. The substrate was readily utilized within 7-8 h. Continuous degradation of monochloroacetate in the fermentor was demonstrated for monochloroacetate concentration of 20 mM and dilution rate 0.016 h(-1). Quantitative agreement between the amount of monochloroacetate introduced and chloride released was found. The results demonstrated that the strain X. autotrophicus GJ10 might be suitable for biodegradation of monochloroacetate contaminated media.

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Photodegradation of haloacetic acids in water

Cited by 80 publications

References 43 publications

Electrocatalytic dechlorination of chloroacetic acids by silver nanoparticles modified glassy carbon electrode

Electrocatalytic dechlorination of chloroacetic acids by silver nanoparticles modified glassy carbon electrode

Photocatalytic Degradation of Phenol using Fe-TiO2 by Different Illumination Sources

Biodegradation of monochloroacetic acid used as a sole carbon and energy source by Xanthobacter autotrophicus GJ10 strain in batch and continuous culture

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