3 research outputs found
Detailed Kinetics and Mechanism of the Oxidation of Thiocyanate Ion (SCN<sup>–</sup>) by Peroxomonosulfate Ion (HSO<sub>5</sub><sup>–</sup>). Formation and Subsequent Oxidation of Hypothiocyanite Ion (OSCN<sup>–</sup>)
The haloperoxidase-catalyzed in vivo oxidation of thiocyanate
ion (SCN<sup>–</sup>) by H<sub>2</sub>O<sub>2</sub> is important
for generation of the antimicrobial hypothiocyanite ion (OSCN<sup>–</sup>), which is also susceptible to oxidation by strong
in vivo oxidizing agents (i.e., H<sub>2</sub>O<sub>2</sub>, OCl<sup>–</sup>, OBr<sup>–</sup>). We report a detailed mechanistic
investigation on the multistep oxidation of excess SCN<sup>–</sup> with peroxomonosulfate ion (HSO<sub>5</sub><sup>–</sup> in
the form of Oxone) in the range from pH 6.5 to 13.5. OSCN<sup>–</sup> was detected to be the intermediate of this reaction under the above
conditions, and a kinetic model is proposed. Furthermore, by kinetic
separation of the consecutive reaction steps, the rate constant of
the direct oxidation of OSCN<sup>–</sup> by HSO<sub>5</sub><sup>–</sup> was determined: <i>k</i><sub>2</sub> = (1.6 ± 0.1) × 10<sup>2</sup> M<sup>–1</sup> s<sup>–1</sup> at pH 13.5 and <i>k</i><sub>2</sub><sup>H</sup> = (3.3 ± 0.1) × 10<sup>3</sup> M<sup>–1</sup> s<sup>–1</sup> at pH 6.89. A critical evaluation of the estimated
activation parameters of the elementary steps revealed that the oxidations
of SCN<sup>–</sup> as well as the consecutive OSCN<sup>–</sup> by HSO<sub>5</sub><sup>–</sup> are more likely to proceed
via 2e<sup>–</sup>-transfer steps rather than 1e<sup>–</sup> transfer
Mechanism of Decomposition of the Human Defense Factor Hypothiocyanite Near Physiological pH
Relatively little is known about the reaction chemistry of the human defense factor hypothiocyanite (OSCN<sup>–</sup>) and its conjugate acid hypothiocyanous acid (HOSCN), in part because of their instability in aqueous solutions. Herein we report that HOSCN/OSCN<sup>–</sup> can engage in a cascade of pH- and concentration-dependent comproportionation, disproportionation, and hydrolysis reactions that control its stability in water. On the basis of reaction kinetic, spectroscopic, and chromatographic methods, a detailed mechanism is proposed for the decomposition of HOSCN/OSCN<sup>–</sup> in the range of pH 4–7 to eventually give simple inorganic anions including CN<sup>–</sup>, OCN<sup>–</sup>, SCN<sup>–</sup>, SO<sub>3</sub><sup>2–</sup>, and SO<sub>4</sub><sup>2–</sup>. Thiocyanogen ((SCN)<sub>2</sub>) is proposed to be a key intermediate in the hydrolysis; and the facile reaction of (SCN)<sub>2</sub> with OSCN<sup>–</sup> to give NCS(O)SCN, a previously unknown reactive sulfur species, has been independently investigated. The mechanism of the aqueous decomposition of (SCN)<sub>2</sub> around pH 4 is also reported. The resulting mechanistic models for the decomposition of HOSCN and (SCN)<sub>2</sub> address previous empirical observations, including the facts that the presence of SCN<sup>–</sup> and/or (SCN)<sub>2</sub> decreases the stability of HOSCN/OSCN<sup>–</sup>, that radioisotopic labeling provided evidence that under physiological conditions decomposing OSCN<sup>–</sup> is not in equilibrium with (SCN)<sub>2</sub> and SCN<sup>–</sup>, and that the hydrolysis of (SCN)<sub>2</sub> near neutral pH does not produce OSCN<sup>–</sup>. Accordingly, we demonstrate that, during the human peroxidase-catalyzed oxidation of SCN<sup>–</sup>, (SCN)<sub>2</sub> cannot be the precursor of the OSCN<sup>–</sup> that is produced
Kinetics of Formation of the Host–Guest Complex of a Viologen with Cucurbit[7]uril
Host–guest complexation between the dicationic viologen 1-tri(ethylene glycol)-1′-methyl-<i>m</i>-xylyl-4,4′-bipyridinium and cucurbit[7]uril (<b>CB7</b>) was studied at pH = 4.5 in water. The stability constants of the mono- and bis-<b>CB7</b> adducts were determined at 25 °C by UV–vis spectroscopy. Stopped-flow kinetic experiments were performed to measure the formation and dissociation rate constants of the monoadduct: <i>k</i><sub>1</sub> = (6.01 ± 0.03) × 10<sup>6</sup> M<sup>–1 </sup>s<sup>–1</sup> and <i>k</i><sub>–1</sub> = 52.7 ± 0.4 s<sup>–1</sup>, respectively. Possible mechanisms of complexation are discussed in view of the kinetic results