The mechanisms of S N 1 reactions were one of the most intensively studied topics in organic chemistry during the middle of the 20th century.[1] These reactions typically proceed with slow formation of the carbocations followed by fast subsequent reactions with the solvent (Scheme 1).Detailed mechanistic studies by Winstein et al. [2] showed that intermediate carbocations can recombine with the leaving group at the ion-pair or free-ion stage before being trapped by the solvent. Since methods for studying fast reaction kinetics were not available at that time, most information on the relative rates of ionization, ion recombination, and reaction of the intermediate carbocation with the solvent was derived indirectly from measurement of the overall solvolysis rates.Recently we have shown that the ionization rates of covalent benzhydryl esters can be observed photometrically if the resulting carbocations are highly stabilized and do not undergo subsequent reactions with the solvent.[3] We have also reported that the trifluoroethanolysis of chlorobis(pmethoxyphenyl)methane proceeds with instantaneous formation of the carbocation, and its subsequent combination with trifluoroethanol could be followed photometrically with a stopped-flow instrument.[4] Based on these results it was predicted that it should be possible to design systems where both the ionization and the following reaction can be measured. We have now realized such systems and report on the first solvolysis reactions in which the formation of carbocations and their subsequent disappearance in aqueous acetone and acetonitrile can be measured directly and fitted by the kinetic model depicted in Scheme 2.When water was added to the colorless solution of 4,4'-bis(morpholino)benzhydryl acetate (1-OAc) in acetonitrile, the solution rapidly turned blue, then faded again within a couple of minutes. A video demonstrating such "carbocation watching" is provided in the Supporting Information (see also Experimental Section).Photometric monitoring of this process showed that the maximum of the carbocation concentration was reached after 7 s in 80 % aqueous acetonitrile. From the absorbance one could derive that at this point, the concentration of the carbocation corresponded to approximately 3 % of the initial substrate concentration. The fact that the blue color appears much faster than it disappears indicates that the small maximum concentration of the carbocation must result from the fast recombination of the carbocations with the acetate anions. Owing to the involvement of several rate and equilibrium constants (partial dissociation of acetic acid) we were not able to find a kinetic model that fits the resulting plot of the carbocation concentration versus time (see Figure S6 in the Supporting Information). However, the corresponding reaction in the presence of diisopropyl-methylamine ((iPr) 2 NMe), which shows a similar absorbance-time correlation (Figure 1), could be fitted to the kinetic model shown in Scheme 1. The resulting rate constants and the Gepasi [5] fi...