Kinetics and mechanism of the reaction between chlorite ion and hypochlorous acid

G. Peintler, I. Nagypál, Irving R. Epstein

Research output: Contribution to journalArticle

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Abstract

The reaction between ClO2•- and HOCl has been studied by spectrophotometrically monitoring the production of ClO2 at pH 5-6. In excess ClO2-, the reaction is first order in ClO2-, HOCl, and H+, and the stoichiometry is given by HOCl + 2ClO2- + H+ → 2ClO2 + Cl- + H2O. In excess HOCl and at higher pH's, ClO3- is produced, and the order of the reaction is between 1 and 2 for HOCl and between 0 and 1 for H+. By combining computer simulation and least-squares analysis, we obtain a mechanism in which the reaction 2HOCl + ClO2- → ClO3- + Cl2 + H2O (k = (2.1 ± 0.1) × 10-3 M-2 s-1) plays a key role in explaining the behavior at high [HOCl]/[ClO2-].

Original languageEnglish
Pages (from-to)2954-2958
Number of pages5
JournalJournal of Physical Chemistry
Volume94
Issue number7
Publication statusPublished - 1990

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Hypochlorous Acid
Stoichiometry
Ions
acids
Kinetics
Acids
Monitoring
Computer simulation
kinetics
ions
stoichiometry
computerized simulation
chlorite

ASJC Scopus subject areas

  • Physical and Theoretical Chemistry

Cite this

Kinetics and mechanism of the reaction between chlorite ion and hypochlorous acid. / Peintler, G.; Nagypál, I.; Epstein, Irving R.

In: Journal of Physical Chemistry, Vol. 94, No. 7, 1990, p. 2954-2958.

Research output: Contribution to journalArticle

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abstract = "The reaction between ClO2•- and HOCl has been studied by spectrophotometrically monitoring the production of ClO2 at pH 5-6. In excess ClO2-, the reaction is first order in ClO2-, HOCl, and H+, and the stoichiometry is given by HOCl + 2ClO2- + H+ → 2ClO2 + Cl- + H2O. In excess HOCl and at higher pH's, ClO3- is produced, and the order of the reaction is between 1 and 2 for HOCl and between 0 and 1 for H+. By combining computer simulation and least-squares analysis, we obtain a mechanism in which the reaction 2HOCl + ClO2- → ClO3- + Cl2 + H2O (k = (2.1 ± 0.1) × 10-3 M-2 s-1) plays a key role in explaining the behavior at high [HOCl]/[ClO2-].",
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N2 - The reaction between ClO2•- and HOCl has been studied by spectrophotometrically monitoring the production of ClO2 at pH 5-6. In excess ClO2-, the reaction is first order in ClO2-, HOCl, and H+, and the stoichiometry is given by HOCl + 2ClO2- + H+ → 2ClO2 + Cl- + H2O. In excess HOCl and at higher pH's, ClO3- is produced, and the order of the reaction is between 1 and 2 for HOCl and between 0 and 1 for H+. By combining computer simulation and least-squares analysis, we obtain a mechanism in which the reaction 2HOCl + ClO2- → ClO3- + Cl2 + H2O (k = (2.1 ± 0.1) × 10-3 M-2 s-1) plays a key role in explaining the behavior at high [HOCl]/[ClO2-].

AB - The reaction between ClO2•- and HOCl has been studied by spectrophotometrically monitoring the production of ClO2 at pH 5-6. In excess ClO2-, the reaction is first order in ClO2-, HOCl, and H+, and the stoichiometry is given by HOCl + 2ClO2- + H+ → 2ClO2 + Cl- + H2O. In excess HOCl and at higher pH's, ClO3- is produced, and the order of the reaction is between 1 and 2 for HOCl and between 0 and 1 for H+. By combining computer simulation and least-squares analysis, we obtain a mechanism in which the reaction 2HOCl + ClO2- → ClO3- + Cl2 + H2O (k = (2.1 ± 0.1) × 10-3 M-2 s-1) plays a key role in explaining the behavior at high [HOCl]/[ClO2-].

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