In acid catalysis, an acid accelerates a chemical reaction and is regenerated by the complete catalytic cycle. Protonating a substrate can create a better electrophile or leaving group, opening a lower-barrier pathway.
For example, acid-catalyzed ester hydrolysis begins by increasing the reactivity of a carbonyl group toward water. A catalyst changes the rates of forward and reverse reactions without changing their equilibrium constant. Specific acid catalysis depends on the solvent's protonated species, while general acid catalysis can involve other proton donors directly in the rate-controlling process.
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Acid catalysis refers to a process in which an acid is used to speed up a chemical reaction. In this context, acids act as catalysts by donating protons (H⁺ ions) to reactants, which can stabilize transition states or alter the reactivity of the substrates involved in the reaction. This can lead to a lower activation energy barrier, making it easier for the reaction to occur.