Nucleophilic/Oxidizing Degradation of Paraoxon and Thioanisole Using NH3 Modified Aqueous H2O2 Solution

San Ping Zhao; Hai Ling Xi; Qi Wang; Yan Jun Zuo

doi:10.4028/www.scientific.net/AMM.675-677.75

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HomeApplied Mechanics and MaterialsApplied Mechanics and Materials Vols. 675-677Nucleophilic/Oxidizing Degradation of Paraoxon and...

Nucleophilic/Oxidizing Degradation of Paraoxon and Thioanisole Using NH₃ Modified Aqueous H₂O₂ Solution

Abstract:

Degradation of paraoxon and thioanisole (PhSMe) were studied using NH₃ modified H₂O₂ solution as decontaminant. Degradation rates of paraoxon depend exponentially on pH of the modified solution. Nucleophilic substitution mediated by HOO^- is the major degradation mechanism and at least two orders of magnitude faster than hydrolysis. Proton catalytic oxidation and solvent-aided oxidation contribute differently to the primary oxidation of PhSMe (PhSMe→PhS(O)Me), and the apparent kinetic constants (k_ap) of the primary oxidation show a three-stage profile with pH of the NH₃-modified H₂O₂ solution. Secondary oxidation of PhSMe (PhS(O) Me→PhS(O)₂Me) is much slower than the primary oxidation in the modified H₂O₂ solution, and the yield of PhS(O)₂Me depended exponentially on pH too. The best pH range for the NH₃ modified H₂O₂ solution as a broad-spectrum decontaminant is at 9.5-10.0 since a balance of nucleophilic/oxidizing decontamination reactivity could be achieved.

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Periodical:

Applied Mechanics and Materials (Volumes 675-677)

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75-81

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https://doi.org/10.4028/www.scientific.net/AMM.675-677.75

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Online since:

October 2014

Authors:

San Ping Zhao, Hai Ling Xi*, Qi Wang, Yan Jun Zuo

Keywords:

Degradation, Hydrogen Peroxide, Paraoxon, Thioanisole

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References

[1] G.W. Wagner, Main Group Chemistry. 28 (2010) 257-263.

Google Scholar

[2] H. Xi, S. Zhao, W. Zhou, Environmental Science. 34 (2013) 1-8.

Google Scholar

[3] G.W. Wagner, D.C. Sorrick, L.R. Procell, Z.A. Hess, M.D. Brickhouse, I.F. McVey, L.I. Schwartz, U.S. Army Edgewood Chemical Biological Center, Aberdeen Proving Ground, (2003).

Google Scholar

[4] G.W. Wagner, D.C. Sorrick, L.R. Procell, M.D. Brickhouse, I.F. Mcvey, L.I. Schwartz, Langmuir. 23 (2007) 1178-1186.

DOI: 10.1021/la062708i

Google Scholar

[5] M.D. Brickhouse, A. Turetsky, B.K. Maclver, J.W. Pfarr, T.A. Lalain, L. McVey, W. Alter, J. Lloyd, Jr. M.A. Fonti, U.S. Army Research Development and Engineering Command, (2007).

Google Scholar

[6] L.N. Vakhitova, K.V. Matvienko, N.A. Taran, N.V. Lakhtarenko, A.F. Popov, Russian Journal of Organic Chemistry. 47 (2011) 965-973.

DOI: 10.1134/s1070428011070013

Google Scholar

[7] H. Fakhraian, F. Valizadeh, Journal of Molecular Catalysis A: Chemical. 333 (2010) 69-72.

Google Scholar

[8] I. Um, Y. Shin, S. Lee, K. Yang, E. Buncel, Journal of Organic Chemistry. 73 (2008) 923-930.

Google Scholar

[9] G.W. Wagner, Y. Yang, Industrial & Engineering Chemistry Research. 41 (2002) 1925-(1928).

Google Scholar

[10] L.N. Vakhitova, K.V. Matvienko, A.V. Skrypka, N.V. Lakhtarenko, N.A. Taran, V.V. Rybak, A.F. Popov, Theoretical and Experimental Chemistry. 46 (2010) 1-7.

DOI: 10.1007/s11237-010-9159-5

Google Scholar

[11] A.P. Burke, University of Florida, (2005).

Google Scholar

[12] L.N. Vakhitova, A.V. Skrypka, V.A. Savelova, A.F. Popov, B.V. Panchenko, Theoretical and Experimental Chemistry. 41 (2005) 98-104.

DOI: 10.1007/s11237-005-0027-7

Google Scholar

[13] D.A. Bennett, H. Yao, D.E. Richardson, Inorganic Chemistry. 40 (2001) 2996-3001.

Google Scholar

[14] Z. Rappoport, in: Z. Rappoport (Ed. ), The chemistry of peroxides, John Wiley & Sons Ltd, 2006, pp.1-92.

Google Scholar