Abstract
Abstract The sulfuric acid-catalyzed reversible formation of peracetic acid from acetic acid and hydrogen peroxide in aqueous acetic acid has been studied kinetically. The rate of peracid formation is proportional to the product of the concentrations of acetic acid and of hydrogen peroxide, increasing with an increase in the concentration of sulfuric acid. The plot of the logarithm of the rate constant vs. −H0 gives a straight line, with a slope of 0.82 and 1.10. The mechanism has been discussed in connection with the analogous acid-catalyzed esterification. The equilibrium constants for the present reaction also increase with an increase in the acidity, and the similar plot of logK1 vs. −H gives a straight line with a slope of 0.22. These facts are explicable by considering the protonation of water.
Sign-in/Register to access full text options 
Free) 
Talk to us
Join us for a 30 min session where you can share your feedback and ask us any queries you have
Schedule a call
