In addition, as summarized in Fig. , our statistical perspective allows to collapse the effect of the complex structural heterogeneity found in experimental data Figure : Our simplifying statistical approach efficiently describes the thermodynamic properties of complex electrolyte solutions: A: Weakly interacting ions or dilute solutions (e.g. CsBr, see Fig. ) show a more homogeneous charge distribution (anions in red, cations in blue). Top: illustration of typical instantaneous charge distributions within the observation droplet. Center: Qualitative probability distribution of the instantaneous droplet net charge. Regardless of the distribution the average droplet charge is zero by construction. Bottom: Illustration of instantaneous ion distributions inside and outside a selection of observation droplets (yellow spheres). The dipole term in our model is sufficient to describe the thermodynamics of these cases. B: Same set of illustrations for complex electrolytes at high concentrations where ion clustering starts to become important (e.g. LiCl. ZnCl 2 , see Fig. ). Even for these cases the effect of the increasing structural heterogeneity on the thermodynamics is fully captured by the quadrupole and octupole terms in our model. and simulations, for strongly interacting ions and concentrated solutions, into the quadrupolar and octupolar terms of our thermodynamic functions. For example, recent studies suggest that a Kirkwood transition, i.e. the concentration where the Debye-length is no longer the characteristic length scale in an electrolyte solution, happens at lower concentrations for strongly interacting electrolytes due to ion clustering. This is in qualitative agreement with our findings in Fig. , where the transition from dipole-dipole to more complex interactions happens at lower concentrations for strongly interacting electrolytes.