Thermodynamic quantities of single ions, such as the proton activity (i.e. pH values) or single ion Gibbs solvation energies (i.e. redox potential values), are widely used in chemistry and related sciences.[1] Thus, methods for the experimental determination of these values are of great interest. Our work focuses on the experimental determination of Gibbs transfer energies Δtrans G(i, S1 → S2) of the ion i, between the different solvents S1 and S2, as the central values for the solvent independent, unified acidity scale pHabs H2O and redox scale E abs H2O, and their two-dimensional combination, the Protoelectric Potential Map (PPM).[2] We established an 'ideal' ionic liquid salt bridge (ILSB) setup, using potential measurements between two electrochemical half cells (Fig. 1).[3] In this setup, the electroactive species is dissolved in different solvents, like water or acetonitrile, and the half-cells are connected by an ILSB. 'Ideal' regarding identical diffusion coefficients for both cation and anion of the ionic liquid to minimize liquid junction potentials at the phase boundaries.Up to now, our research focused on solvents with high permittivity, like water or acetonitrile, utilizing the redox systems Ag+/Ag and Cl2/Cl−.[4] Within this contribution, we present the E abs H2O-scale extended by measured transfer energies in low permittivity solvents, like dichloromethane or fluorobenzene, which are not compatible with the previous setup due to the low solubility of the redox systems used. For this application the redox systems Ag+/Ag and Ferrocenium/Ferrocene (Fc+/Fc) were used. In this way, we can include several values measured by cyclic voltammetry.[5] The E abs H2O-scale gives the experimental chemist the possibility of a more straightforward synthesis design and the theoretical chemist values to benchmark his calculations. REFERENCES P. Hünenberger, M. Reif, Single-ion solvation. Experimental and theoretical approaches to elusive thermodynamic quantities, Royal Society of Chemistry, Cambridge, 2011.V. Radtke, D. Himmel, K. Pütz, S. K. Goll, I. Krossing, Chem-Eur. J. 2014, 20, 4194.a) V. Radtke, A. Ermantraut, D. Himmel, T. Koslowski, I. Leito, I. Krossing, Chem. Int. Ed. 2018, 130, 2368; b) A. Ermantraut, V. Radtke, N. Gebel, D. Himmel, T. Koslowski, I. Leito, I. Krossing, Angew. Chem. Int. Ed. 2018, 130, 2372.a) V. Radtke, N. Gebel, D. Priester, A. Ermantraut, M. Bäuerle, D. Himmel, R. Stroh, T. Koslowski, I. Leito, I. Krossing, Eur. J. 2022, 28, e202200509.; b) V. Radtke, D. Priester, A. Heering, C. Müller, T. Koslowski, I. Leito, I. Krossing, Chem. Eur. J. 2023, 29, e202300609.I. Krossing, C. Armbruster, M. Sellin, M. Seiler, T. Würz, F. Oesten, M. Schmucker, T. Sterbak, J. Fischer, V. Radtke et al., e-preprint DOI: 10.21203/rs.3.rs-3921217/v1. Figure 1
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