The acid dissociation constant and hydrolysis rate of hydroxysulfamic acid (HSA) in acid aqueous solutions have been studied. The acid dissociation constant was determined to be K = 1.5 ± 0.5 M at 298 K. The hydrolysis rate, R, was found to be R = k[H+][HSA], where k = 6.2 × 1012 exp (−26 300/RT) M−1 s−1 at (μ = 1.0 M and [HSA] is the concentration of all forms of hydroxysulfamic acid. Keywords: hydroxysulfamic acid, hydrolysis, acid dissociation.
029ChemInform Abstract The kinetics of reaction A has been studied over the temp. range 283-333 K at solution pHs ranging from 4.1-6.7, and at ionic strengths of 0.03-0.5 M. The hydrolysis reaction has first-order dependence on the N(SO3)33-concentration. The first-order dependence on (H+) indicates that the reaction is acid-catalyzed. The uncatalyzed reaction (pH 8-10) is found to be insignificant. An Arrhenius expression for the rate constant is given.
The kinetics of the acid-catalyzed hydrolysis of nitridotrisulfate ion in aqueous solution were studied over a pH range of 4.1 to 6.7 and a temperature range of 283 K to 333 K. The build-up of the reaction products was observed by ion chromatography. The reaction has first order dependence on both hydrogen ion and nitridotrisulfate ion. When the rate constant is expressed ask = A exp (-EajRT), values of A = 1.5 ± 0.7 x 10 13 I mor 1 sec-l and E = 16.5 ± 0.3 kcal mor l are obtained at an ionic strength of 0.05. a. The ionic strength dependence was also studied.
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