The degradation kinetics of chiorimuron-ethyl during chlorination was analyzed, and the effects of the influencing factors of pH, bromide and ammonium concentrations and reaction temperature on degradation kinetics were evaluated. Regarding degradation kinetics, the chlorination of chlorimuron-ethyl followed second-order kinetics, first-order kinetics when the chlorine concentration was changed, and first-order kinetics when the chlorimuron-ethyl concentration was changed. The apparent second-order rate constant was calculated, which significantly decreased increasing pH. The rate constant of the reaction between chlorimuron-ethyl(-) and HOCl was calculated as 3.25 (+/- 1.14) x 10(3) M-1 min(-1), and under the acid-catalyzed condition, the rate constant significantly increased to 6.41 (+/- 1.62) x 10(7) M-1 min( -1). The degradation rate of chlorimuron-ethyl decreased with increasing bromide (at pH 5.5-7.0) and ammonium concentrations (<= 6 mu M). Chlorimuron-ethyl chlorination is an endothermic reaction, with an activation energy estimated as 22.46 kJ mol(-1) using the Arrhenius equation. During chlorimuron-ethyl chlorination, chloroform was the major volatile degradation product during chlorimuron-ethyl chlorination, and its concentration increased with the increasing reaction time and pH level. The distribution of disinfection by-products (DBPs) formed at different solution pH levels was quite distinct. In the presence of bromide, the concentration and species of brominated DBPs increased with the increasing bromide concentration. Notably, carcinogenicity and mutagenicity of brominated DBPs were higher than their chlorinate analogs.