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| - Temperature Dependence of the Acid Dissociation Constant of the Hydroxyl Radical
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| - The acid dissociation constant of the hydroxyl radical in aqueous solution was determined by pulse radiolysisfrom the [OH-] dependence of the rate constant for reaction of the •OH/O•- radical with benzoate ions. Therate constant and the pKa(•OH) values were determined over the temperature range 284−343 K. At 298 K,pKa 298(•OH) = 11.54 ± 0.04 and ΔionG°298(•OH) = (65.9 ± 0.3) kJ mol-1. From the temperature dependenceof Ka(•OH), we calculate ΔionH°298(•OH) = (24.85 ± 0.5) kJ mol-1 and ΔionS°298(•OH) = (−139 ± 2) J mol-1K-1. The activation energy for the reaction of •OH with C6H5CO2- was found to be (8.8 ± 0.6) kJ mol-1 andthe Arrhenius preexponential factor (2.4 ± 0.6) × 1011 L mol-1 s-1.
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