Abstract: Under the condition of constant acidity, it has been shown that the hydrolysis of aconitine is a consecutive first-order reaction containing two successive steps. The rate constants of both steps increase with decrease of acidity. The pH dependence of rate constant is ploted as a parabolic curve. The reaction is catalyzed by the OH^-ion. In basic solution, the rate constants of both steps gradually decrease with increase of ionic strength, and under this condition the reaction appears greater kinetic salt effect. However, in neutral and acidic solution, the kinetic salt effect becomes very weak. The energy of activation of these two reaction steps at pH 5.21, 6.95, and 8.01 is 104.0±2.2, 94. 1±0.8 and 73.9±0.6 kJ/mol, respectively, for the first step, and 104.9±1.3, 83.85±0.6 and 57.3±0.4 kJ/mol, respectively, for the second step.