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Hydrolysis of 2‐aminoethanethiolsulfate ions
Author(s) -
Zheng Z. B.,
Littlejohn D.,
Chang S. G.,
Zhuang Y. H.
Publication year - 1994
Publication title -
international journal of chemical kinetics
Language(s) - English
Resource type - Journals
SCImago Journal Rank - 0.341
H-Index - 68
eISSN - 1097-4601
pISSN - 0538-8066
DOI - 10.1002/kin.550260507
Subject(s) - chemistry , hydrolysis , catalysis , reaction rate constant , kinetics , ion , hydrolysis constant , rate equation , work (physics) , medicinal chemistry , inorganic chemistry , thermodynamics , organic chemistry , physics , quantum mechanics
The kinetics of the acid catalyzed hydrolysis of 2‐aminoethanethiolsulfate (AETS) ions were investigated. The dependence of the hydrolysis rate constant on acidity and temperature was determined. The hydrolysis rate equation can be expressed as\documentclass{article}\pagestyle{empty}\begin{document}$$ d{{\left[{{\rm AETS}} \right]} \mathord{\left/ {\vphantom {{\left[{{\rm AETS}} \right]} {dt}}} \right. \kern-\nulldelimiterspace} {dt}} = - k{\rm H}_{\rm o} \left[{{\rm AETS}} \right] $$\end{document}where H o is the Hammett acidity function. The rate constant, k , can be expressed asThe p K a 's for the compound were measured and literature value of p K a was found to be in error. The values determined in this study are p K a1 < −0.5 and p K a2 = 9.1 ± 0.1. General acid catalysis of the hydrolysis reaction was found not to proceed to a significant degree. © 1994 John Wiley & Sons, Inc. This article is a US Government work and, as such, is in the public domain in the United States of America.