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Thermodynamic properties of the protonation of  D -gluconic acid (HGH 4 (aq)) and its complexation with Np(V) have been studied in acidic to nearly neutral solutions at  t  =25 °C and  I =1 M NaClO 4  by potentiometry, spectrophotometry and calorimetry. The protonation constant (log K  H ) and enthalpy (Δ H  H ) of the carboxylate group are determined to be (3.30±0.10) and −(4.03±0.07) kJ mol -1 , respectively. Gluconate forms two Np(V) complexes in nearly neutral solutions. The formation constants and enthalpies of complexation are: log β 1  = (1.48±0.03) and Δ H  1  = −(7.42±0.13) kJ mol -1  for NpO 2 (GH 4 )(aq), log β 2 =(2.14±0.09) and Δ H  2 = −(12.08±0.45) kJ mol -1  for NpO 2 (GH 4 ) 2  - . The thermodynamic parameters indicate that gluconic acid, like isosaccharinic acid and other α-hydroxycarboxylic acids, is a slightly stronger acid and forms stronger complexes with Np(V) than simple monocarboxylic acids.

Protonation of D -gluconate and its complexation with Np(V) in acidic to nearly neutral solutions