A novel method to determine redox potentials without electrolyte is presented. The method is based on a new ability to determine the dissociation constant, K degrees(d), for ion pairs formed between any radical anion and any inert electrolyte counterion. These dissociation constants can be used to determine relative shifts of redox potential as a function of electrolyte concentration, connecting referenced potentials determined with electrochemistry (with 0.1 M electrolyte) to electrolyte-free values. Pulse radiolysis created radical anions enabling determination of equilibrium constants for electron transfer between anions of donor and acceptor molecules as a function of electrolyte concentration in THF. The measurements determined "composite equilibrium constants", K-eqC, which contain information about the dissociation constant for the electrolyte cations, X+, with the radical anions of both the donor, K degrees(d)(D-center dot,X+) and the acceptor, K degrees(d)(A(-center dot),X+). Dissociation constants were obtained for a selection of radical anions with tetrabutylammonium (TBA(+)). The electrolyte was found to shift the reduction potentials of small molecules 1-methylpyrene and trans-stilbene by close to +130 mV whereas oligo-fluorenes and polyfluorenes experienced shifts of only (+25 +/- 6) mV due to charge delocalization weakening the ion pair. These shifts for reduction of aromatic hydrocarbon molecules are smaller than shifts of +232 and +451 mV seen previously for benzophenone radical anion with TBA(+) and Na+ respectively where the charge on the radical anion is localized largely on one C=O bond, thus forming a more tightly bound ion pair.