Symmetrical weak electrolyte, conductivity

Molar Conductivity and Association Constants of Symmetrical Weak Electrolytes... 

Following the concept underlying the MSA-MAL conductivity equation [3, 32, 33] and by taking into account that the total concentration of electrically conducting particles is molar conductivity in the AMSA for symmetrical electrolytes [13]. The possibility of such modification of the AMSA theory is quite promising for the description and interpretation of thermodynamic and transport properties of electrolyte solutions in a weakly polar solvent. 

Liquid ammonia appears to be an exception to this rule. The conductivities of solutions of acids and bases are high, but so are the conductivities of other electrolyte solutions in this solvent. An explaination has been advanced from a structural point of view all units involved in frequent proton transfer reactions are not fully coordinated and polar such as H3O+, H2O and OH in water or H2F+, HF and F in liquid hydrogen fluoride. In contrast the NH4+ ion produced in liquid ammonia is symmetrical and non-polar and release of a proton is not easily possible (the NH4+-ion is a very weak Bronsted acid, while the HaO -ion is the strongest Bronsted acid in water). 

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