The kinetics of S(IV) oxidation by ozone in aqueous solution have been studied at 10¿C and 25¿C in the pH range 3.0 to 6.2 by using stopped-flow spectrophotometry. The rate data are empirically correlated by r=(k1+k2 10pH)3> with k1=4.39¿1011 e-4131/r (¿3¿104) M-1s-1, and k2=2.56¿103 e966/r (¿15) s-1, at an ionic strength of 0.01 M. Reaction rate is unaffected by incident strong UV radiation, or the presence of MN(II) or Fe(III), but is weakly dependent on ionic strength. The present results, in comparison with reported rates of oxidation of S(IV) by hydrogen peroxide, indicate that at typical pH levels encountered in nonurban tropospheric cloud water and at representative concentrations of 03 and H2O2 in the troposphere, oxidation by O3 can be competitive with that by H2O3, or possibly even dominate. The reaction appears to proceed by other than a free-radical process, and a reaction scheme involving direct ozone attack catalyzed by hydroxide ion is proposed. A rate expressions consistent with this scheme is r=(ke+kb ->)>HSO3-><)3> where ka=3.8¿105 M-1s-1 and kb=1.05¿1016 M-2s-1 at 25¿C. This expression correlates the present data with literature data over the pH rane 1.0 to 6.2.