29 October 2017 to 3 November 2017
Australia/Sydney timezone

Solubility of the rhabdophane, LnPO4.0.667 H2O (Ln = La to Dy): implications for the long-term stability of monazite matrices.

1 Nov 2017, 10:45
Oral Presentation National and international collaborative waste management programs Ceramic and Glass-Ceramic Wasteforms


Dr Stéphanie Szenknect (ICSM)


Minerals belonging to the monazite family, REEPO4 (REE: Y, Sc, La to Dy) could incorporate in their structure substantial amounts of Th and U [1]. Moreover, monazites maintain their crystallinity even after geological times of exposure to self-irradiation. Therefore, this phase appears as a promising candidate for the specific conditioning of transuranic elements (AnIV,AnIII). Already, many thermodynamic properties of monazite are reported in the litterature [2]. However, its hydrated form namely, rhabdophane, REEPO4.0.667 H2O could be stabilized at low temperatures, and thus control the concentrations of actinides in solution after the leaching of the monazite matrices [3, 4]. For the first time, a systematic study of the solubility of the rhabdophane, LnPO4.0.667 H2O (Ln = La to Dy) was performed using over-saturated and under-saturated experiments at different temperatures (298 to 363 K) to demonstrate the reversibility of the solubility equilibrium [5]. The structure of the neoformed phases was carefully controlled in the entire range of temperatures in order to attribute unambiguously the solubility products and the derived thermodynamic data associated to the rhabdophane phases. The obtained results indicate that the stability domain of the rhabdophane phase is limited in temperature and depends on the ionic radius of the lanthanide. The values of the solubility constant depend also slightly on the lanthanide with log KS,0° (298 K) ranging from -25.6 ± 0.8 (Pr) to -24.9 ± 1.7 (Eu) with minimum values for Pr to Sm. The values of the standard free enery of formation at 298 K varied between -1984 ± 2 and -2004 ± 2 kJ.mol-1 whatever the lanthanide element considered, except for Eu-rhabdophane that presented the highest value for the Gibbs energy of formation (-1896 ± 2 kJ.mol-1). From the solubility data obtained at various temperatures, the values of enthalpy of formation of the rhabdophanes were found between -2151 ± 13 and -2130 ± 12 kJ. mol-1 excepted for Eu for which it reached -2057 ± 9 kJ.mol-1. It is worth noting that the data reported by Ushakov et al. [6] for monazites LnPO4 (Ln = La to Gd) determined by oxide melt calorimetry and recalculated by taking into account the contribution of the water molecules are in very good agreement with the data obtained for rhabdophane in this work. This result indicates that the enthalpy of formation of the rhabdophane can be simply deduced from the enthalpy of formation of the monazite by adding the contribution of 0.667 molecule of structural water. These results could be used to estimate the thermodynamic properties of AnIIIPO4 .0.667 H2O (with AnIII =Am, Pu or Cm) by analogy with the lanthanides of close ionic radii. The rhabdophane structure can also incorporate AnIV by coupled substitution of LnIII by MII and AnIV. In this field, Nd0.8Ca0.1Th0.1PO4 .n H2O were prepared by wet chemistry route and preliminary solubility data were determined, which showed that this phase is metastable in solution at 298 K, Th and Nd being released leading to the formation of Th2(PO4)2(HPO4). H2O (TPHPH) [7] and NdPO4.0.667 H2O, respectively. References: [1] N. Clavier, R. Podor, N. Dacheux, (2011). Journal of the European Ceramic Society 31: 941-976. [2] F. Poitrasson, E. Oelkers, J. Schott, J.-M. Montel, (2004).Geochimica et Cosmochimica Acta 68: 2207-2221. [3] E. Du Fou de Kerdaniel, N. Clavier, N. Dacheux, O. Terra, R. Podor, (2007). Journal of Nuclear Materials 362: 451-458. [4] N. Dacheux, N. Clavier, R. Podor, (2013). American Mineralogist 98: 833-847. [5] C. Gausse, S. Szenknect, D.W. Qin, A. Mesbah, N. Clavier, S. Neumeier, D. Bosbach, N. Dacheux, (2016). European Journal of Inorganic Chemistry 2016: 4615-4630. [6] S.V. Ushakov, K.B. Helean, A. Navrotsky, L.A. Boatner, (2001). Journal of Materials Research 16: 2623-2633. [7] D. Qin, C. Gausse, S. Szenknect, A. Mesbah, N. Clavier, N. Dacheux, (2017). The Journal of Chemical Thermodynamics, dx.doi.org/10.1016/j.jct.2017.01.003

Primary author


Dr Clémence Gausse (ICSM) Dr Nicolas Clavier (ICSM) Prof. Nicolas Dacheux (ICSM) Dr Stefan NEUMEIER (IEK-6 FZ Jülich) Dr adel mesbah (ICSM Marcoule, France)

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