A method for the calculation of the enthalpies of crystal lattices and standard enthalpies of formation of anhydrous metal nitrates and carboxylates is presented. The estimation of ~l-Ilat is based on interpolation of the linear plots of this value vs. the Edwards parameter, which, in turn, is a linear function of the logarithm of the acid dissociation constant. Linearity of the above dependence was previously found experimentally for the corresponding uranyl salts. Previously unknown lattice enthalpies and standard enthalpies of formation of a large set of anhydrous metal nitrates and carboxylates are calculated.Various aspects of the effect of the anionic characteristics, particularly electrondonor power, on the properties of salts both in crystalline state and solution were extensively studied. Anionic effects also contributes significantly to extraction processes. It was demonstrated with the example of haloacetate complexes that optimization of electron-donor characteristics of the anion in attraction to neutral extractants by solvation and hydration-solvation mechanisms allows an enhancement of the distribution coefficients, and in certain cases, of the cation partition coefficients [1][2][3][4].In Markus's classic work [5], devoted to determination of the enthalpies of crystal lattice (AHlat) of uranyl fluoride and standard formation enthalpy (AH0f, 298) of gaseous UO22 § and also in other works, it was demonstrated that thermodynamic calculations of extraction equilibria, prediction of the distribution coefficients, and, correspondingly, of element separation require information on the termodynamic characteristics of various salts.This study is devoted to the calculation of the lattice enthalpies and standard enthalpies of formation of metal nitrates, acetates, and haloacetates. It should be noted that the above thermodynamic functions are fundamental, and their importance is not restricted to problems of extraction [3,5].In [6], a thermochemical cycle was proposed for calculation of lattice enthalpies of uranyl haloacetates and dissociation enthalpies of the corresponding acids in the gaseous state. The lattice enthalpies ofuranyl salts were calculated from experimental calorimetric data [7] using the standard enthalpy of formation of gaseous uranyl ion calculated in [5]. It was shown in [6] that in the series of nitrate, trifluoroacetate, trichloroacetate, monochloroacetate, and acetate ions, in which the electron-donor power of the anion increases, the lattice enthalpies of the anhydrous uranyl salts and the dissociation enthalpies of the corresponding acids in the gaseous state under normal conditions linearly correlate with the Edwards parameter within experimental error. In turn, this parameter is linearly related to the logarithm of the acid dissociation constant in aqueous solution [8], if the corrected Edwards parameter is used for nitric acid [6].