“…From the electrode potentials obtained above pH = 6 for the [Eu II (DTPA)(H 2 O)] 3- /[Eu III (DTPA)(H 2 O)] 2- system, E 1/2 , one can calculate the stability constant of the [Eu II (DTPA)(H 2 O)] 3- complex by using the known stability constant of [Eu III (DTPA)(H 2 O)] 2- (log K III = 22.39) 19 and the potential of the Eu 2+ (aq) /Eu 3+ (aq) redox couple, E ‘ 1/2 , and considering eqs 1−6 The Nernst equations for the redox couple Eu 2+ (aq) /Eu 3+ (aq) and [Eu II (DTPA)(H 2 O)] 3- /[Eu III (DTPA)(H 2 O)] 2- are given in eqs 1 and 2, respectively:
The stability constants of the two complexes are expressed by eqs 3 and 4:
Insertion of eqs 3 and 4 into eq 2 yields
After making the general assumption of E ‘ 0 1/2 = E 0 1/2 , , we obtain
The stability constant obtained in this way is log K II = 9.94 (25 °C; I = 0.5 M), which corresponds well to the value previously determined by pH potentiometry, log K II = 10.08 (25 °C; I = 1 M KCl) . The electrochemical data also confirm that at higher pH only the nonprotonated species is present in solution, which is in accordance with the p K a = 5.45 value published in the literature (see Figure S2, Supporting Information) …”