Kinetic studies on the oxidation of iodide by peroxyacetic acid

Awad, Mohamed I.; Oritani, Tadato; Ohsaka, Takeo

doi:10.1016/s0020-1693(02)01337-3

Cited by 21 publications

(14 citation statements)

References 12 publications

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“…In the absence of Mo(VI), the rate of the reaction of PAA and Iis 5 orders of magnitude higher than that of H 2 O 2 and I -, but in its presence, the rate of the former reaction is only 2 orders of magnitude higher than that of the latter one. 17 Thus, the effect of the addition of Mo(VI) catalyst on the potential-time curve was examined. The results are given in Figure 4.…”

Section: Resultsmentioning

confidence: 99%

“…[6][7][8][9][10][11][12][13][14][15][16] For instance, the uncatalyzed reaction rate of PAA and Iis by 5 orders of magnitude larger than that of H 2 O 2 with I -. 17 Several techniques for detection of PAA are based on this concept. For instance, titration 18 and spectrophotometric 19 methods were suggested for the monitoring of the two species.…”

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confidence: 99%

“…Because of the similarities of the behavior of both species, the simultaneous analysis of both species is a challenging problem. The concept for the simultaneous analysis of the two species is based on the difference in their oxidizing power. − For instance, the uncatalyzed reaction rate of PAA and I - is by 5 orders of magnitude larger than that of H 2 O 2 with I - . Several techniques for detection of PAA are based on this concept.…”

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confidence: 99%

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Simultaneous Potentiometric Determination of Peracetic Acid and Hydrogen Peroxide

2003

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A rapid and highly selective potentiometric method for the simultaneous analysis of peracetic acid (PAA) and hydrogen peroxide (H2O2) has been proposed, for the first time, using glassy carbon (GC) as an indicator electrode and I2/I- potential buffer. On the basis of the large difference in the reaction rates of PAA and H2O2 with I-, which was confirmed using stopped-flow spectrophotometry, a transient potential response corresponding to the reactions of the two species with I- was observed. The response times were typically a few seconds and several minutes for PAA and H2O2, respectively. The effects of the concentrations of molybdate catalyst, H+, I2, and I- in the potential buffer on the selectivity as well as the sensitivity were examined. The potential response obtained using the GC indicator electrode was found to be Nernstian over a wide range of their concentrations (typically from micromolar to millimolar) with slopes of 30.5 and 29.5 mV for PAA and H2O2, respectively (in close agreement with the theoretical value, that is, 29.6 mV). O2 was found to have no substantial effect on the potential change at the GC electrode in the present potential buffer.

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Section: Resultsmentioning

confidence: 99%

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Simultaneous Potentiometric Determination of Peracetic Acid and Hydrogen Peroxide

2003

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“…Highly selective analytical methods for the PAA determination are required because PAA typically coexists with H 2 O 2 . Several PAA concentration determination methods using chromatographic, titrimetric, colorimetric, and potentiometric techniques have been reported. − These methods can measure the respective concentrations of PAA and H 2 O 2 based on the difference in their oxidation ability.…”

Section: Background Of Paamentioning

confidence: 99%

Reactivity of Peracetic Acid with Organic Compounds: A Critical Review

2020

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As an emerging oxidant and disinfectant, peracetic acid (PAA) has increasingly been used in wastewater treatment and the food and medical industries and has attracted greater research interest. To better understand reactions initiated by PAA, this paper is among the first to comprehensively review the reactivity of PAA with respect to organic compounds of various structures. The reactivities of PAA with respect to 123 organic compounds are compiled from the literature and new experiments, and possible reaction pathways and products are discussed. Overall, PAA is an electrophile with high selectivity in reaction. The second-order rate constants of PAA oxidation of organic compounds vary by nearly 10 orders of magnitude, from 3.2 × 10 −6 to >1.0 × 10 5 M −1 s −1 , which are much larger than those of H 2 O 2 coexisting in PAA solutions. Electron-donating groups of compounds increase the reactivity with respect to PAA, evidenced by the strong negative correlations between rate constants and substituent constants [Hammett (σ) or Taft (σ*)] of compounds. Sulfur moieties show exceptionally high reactivity with respect to PAA. Limited studies have shown that generally oxygen-added reaction products are formed from PAA oxidation. This critical review provides a useful foundation for advancing our understanding of the fate of organic compounds in wastewater treatment including PAA and identifies further research needs to evaluate a broader range of compounds and their oxidation products and toxicity.

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“…HOI oxidation, disproportionation, and/or its reaction with organic compounds all contribute to the consumption of HOI . Oxidation kinetics of HOI with various oxidants have been systematically studied under relevant water treatment conditions. ,− The oxidation of HOI to iodate by ozone is fast with a high second-order rate constant k O3+HOI = 3.6 × 10 4 M –1 s –1 . Chlorination leads to iodate formation; however, this process is much slower due to the relatively low second-order rate constants ( k HOCl+HOI = 8.2 M –1 s –1 ; k OCl − +HOI = 52 M –1 s –1 ) .…”

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confidence: 99%

Kinetic and Mechanistic Aspects of the Reactions of Iodide and Hypoiodous Acid with Permanganate: Oxidation and Disproportionation

Zhao

Salhi

Liu

et al. 2016

Environ. Sci. Technol.

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Oxidation kinetics of iodide and HOI/OI(-) by permanganate were studied in the pH range of 5.0-10.0. Iodide oxidation and iodate formation were faster at lower pH. The apparent second-order rate constants (k(obs)) for iodide oxidation by permanganate decrease with increasing pH from 29 M(-1) s(-1) at pH 5.0 and 6.9 M(-1) s(-1) at pH 7.0 to 2.7 M(-1) s(-1) at pH 10.0. k(obs) for HOI abatement are 56 M(-1) s(-1) at pH 5.0, 2.5 M(-1) s(-1) at pH 7.0, and 173 M(-1) s(-1) at pH 10.0. Iodate yields over HOI abatement decrease from 98% at pH 6.0 to 33% for pH ≥ 9.5, demonstrating that HOI disproportionation dominates HOI transformation by permanganate at pH ≥ 8.0. MnO2 formed as a product from permanganate reduction, oxidizes HOI to iodate for pH < 8.0, and promotes HOI disproportionation for pH ≥ 8.0. The rate of HOI oxidation or disproportionation induced by MnO2 is much lower than for permanganate. During treatment of iodide-containing waters, the potential for iodinated disinfection byproducts (I-DBPs) formation is highest at pH 7.0-8.0 due to the long lifetime of HOI. For pH < 6.0, HOI/I2 is quickly oxidized by permanganate to iodate, whereas for pH ≥ 8.0, HOI/OI(-) undergoes a fast permanganate-mediated disproportionation.

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Kinetic studies on the oxidation of iodide by peroxyacetic acid

Cited by 21 publications

References 12 publications

Simultaneous Potentiometric Determination of Peracetic Acid and Hydrogen Peroxide

Simultaneous Potentiometric Determination of Peracetic Acid and Hydrogen Peroxide

Reactivity of Peracetic Acid with Organic Compounds: A Critical Review

Kinetic and Mechanistic Aspects of the Reactions of Iodide and Hypoiodous Acid with Permanganate: Oxidation and Disproportionation

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