Original scientific paper
Influence of pH, Temperature and Common Ion on Magnesium Hydrogenurate Octahydrate Solubility
Vesna Babić-Ivančić
; Department of Materials Chemistry, »Ruđer Bošković« Institute, Zagreb, Croatia
Martina Jendrić
; Department of Materials Chemistry, »Ruđer Bošković« Institute, Zagreb, Croatia
Nives Šoštarić
; Department of Materials Chemistry, »Ruđer Bošković« Institute, Zagreb, Croatia
Teuta Opačak-Bernardi
; Department of Mineral Metabolism, School of Medicine, University »Josip Juraj Strossmayer«, Osijek, Croatia
Sandra Tucak Zorić
; Department of Environmental Protection, City of Zagreb, Zagreb, Croatia
Maja Dutour Sikirić
; Department of Physical Chemistry, »Ruđer Bošković« Institute, Zagreb, Croatia
Abstract
Physico-chemical investigation of urolithiasis today is mostly focused on applying physico-chemical description of precipitation processes to the stone formation with the aim to distinguish between stone formers and nonstone formers. This is done by calculating supersaturation for different solid phases which can be formed in urine using data obtained by urine analysis and existing solubility product, dissociation and complexation constants. In order for this approach to succeed it is of utmost importance that system is described as detailed as possible, i.e. that all species that can be formed are taken into account. Magnesium hydrogenurate octahydrate, Mg(C5H3N4O3)2·8H2O (Mg(HU)2·8H2O), is among species which can precipitate in the urine and for which solubility data doesn’t exist. In order to fill this void crystals of Mg(C5H3N4O3)2·8H2O phase I and phase II have been prepared and characterized. Solubility product constant of Mg(C5H3N4O3)2·8H2O phase I in water at 37 °C and phase II at different temperatures, pH and in different solvents have been determined by measuring total concentration of uric acid and magnesium ions in solutions at different time periods. Results show that in water at 37 °C thermodynamically less stable phase I is more soluble (Ksp=(5.64±0.20).10–9 mol3 dm–9) than phase II (Ksp=(1.66±0.13).10–9 mol3dm–9). Solubility of Mg(HU)2·8H2O phase II increases with temperature. At equilibrium the solubility of phase II is the lowest in the presence of excess of magnesium ions, while solubility in the presence of uric acid is comparable with the one obtained in water.
Keywords
magnesium hydrogenurate octahydrate; solubility; preparation; characterisation
Hrčak ID:
51775
URI
Publication date:
25.3.2010.
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