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   <subfield code="a">Temperature and ionic strength influence on U(VI/V) and U(IV/III) redox potentials in aqueous acidic and carbonate solutions</subfield>
   <subfield code="h">[Elektronische Daten]</subfield>
   <subfield code="c">[H. Capdevila, P. Vitorge]</subfield>
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   <subfield code="a">Redox potentials: E(UO 2 2+ /UO 2 + )=60±4 mV/NHE, E(U4+/U3+)=−630±4mV/NHE measured at 25°C in acidic medium (HClO4 1M) using cyclic voltametry are in accordance with the published data. From 5°C to 55°C the variations of the potentials of these systems (measured against Ag/AgCl electrode) are linear. The entropies are then constant: [ΔS(UO 2 2+ /UO 2 + )−ΔS(Ag/AgCl)]/F=0±0.3 mV/°C, [ΔS(U4+/U3+)−ΔS(Ag/AgCl)]/F=1.5±0.3 mV/°C. From 5°C to 55°C, in carbonate medium (Na2CO3=0.2M), the Specific Ionic Interaction Theory can model the experimental results up to I=2M (Na+, ClO 4 − , CO 3 2− ): E(UO2(CO3) 3 4− /UO2(CO3) 3 5− )=−778±5 mv/NHE (I=0, T=25°C, Δ∈(25°C)=∈(UO2(CO3) 3 4− , Na+)−∈(UO2(CO3) 3 5− , Na+)=0.92 kg/mole, ΔS(UO2(CO3) 3 4− /UO2(CO3) 3 5− =−1.8±0.5 mV/°C (I=0), Δ∈=∈(Cl−, Na+)=(1.14−0.007T) kg/mole. The U(VI/V) potential shift, between carbonate and acidic media, is used to calculate (at I=0,25°C): $$\log \frac{{\beta _3 U(V)}}{{\beta _3 U(VI)}} = - 14.7 \pm 0.5$$ and then $$\log \beta _3 U(V) = 6.6 \pm 0.3.$$</subfield>
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