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    12.11.26: Congratulations to Yagmur Aydogan-Sun and collaborators

    "Electrolyte Effects on the Elementary Steps of ESPT in Photobases–An Investigation of Dissociation and Quenching Rates in Aqueous Solutions" in The Journal of Physical Chemistry A

    Excited-state proton transfer (ESPT) in photoacids or photobases depends on several factors, such as the solvent’s pKa, temperature, or the concentration of electrolytes in solution. The latter is especially relevant for biological applications but has, to date, been explored almost exclusively for photoacids. In this contribution, we study the effect of sodium halides (NaF, NaCl, and NaI) on the ESPT reaction of 5- and 6-methoxyquinoline (5-MeOQ and 6-MeOQ). We interpret our results in the light of anion effects, i.e., quenching and enhanced recombination, competing with the effects of cations, i.e., screened recombination and an increased acidity of the solvent. Whereas for NaI, and in most solutions of NaCl, quenching effects seem to be the dominant factor, other effects are more pronounced in aqueous NaF solutions. We associate this with a charge-transfer quenching mechanism that primarily affects the (positively charged) protonated form and that is most prominent for the weak photobase 6-MeOQ and the strong quencher I–. When quenching is negligible, though, our steady-state emission experiments show an increased emission from the unprotonated form of 6-MeOQ, which we associate with an increased recombination rate. For 5-MeOQ, however, we argue that the observed results are largely attributable to Na+ effects. While these are thought to compete with quenching, UV/vis fs-TA experiments suggest an increasing contribution from the fully separated ion pair (FSIP), i.e., the product of the dissociation process in a two-step Eigen–Weller model. Lastly, we show that the dissociation rate also depends on the temperature of the solvent. We associate the observed increase in this rate with the increasing temperature of the solvents’ changed viscosity and thus a higher mobility of the OH– ions.