On the Solubility Product of Precipitated Iron(III) Hydroxide.

Solubility constants of metal oxides, metal hydroxides and metal hydroxide salts in aqueous solution

“…For oxides and hydroxides oftri-and multivalent metals the calculation of Ks 0 often yields doubtful results, since the corresponding ions form stable complexes with numerous ligands. For instance, pH-measurements of partly precipitated T1Cl 3 solutions gave 13 a value of log Ks 0 = -34·2. This high value can be ascribed to the fact that the dissolved TJIII must have been present mainly in the form of chloro complexes.…”

Formation, stability, and solubility of metal oxide nanoparticles: Surface entropy, enthalpy, and free energy of ferrihydrite

“…The ultimate goal is relating the obtained thermodynamic properties of the mineral core and surface to experimental data sets on the solubility (Biedermann and Schindler, 1957;Fox, 1988;Hiemstra and van Riemsdijk, 2006;Liu and Millero, 1999;Schindler et al, 1963;Stefansson, 2007), mineral stability of Fh (Michel et al, 2010), as well as its formation by nucleation. Crucial is a well-founded thermodynamic analysis (Enüstün and Turkevich, 1960;Godec et al, 2009;Kaptay, 2012;Nancollas and Wu, 2009;Wu and Nancollas, 1999).…”

Siderophore electrochemistry: relation to intracellular iron release mechanism.

“…Aerobic microorganisms have a particularly severe problem acquiring iron, because in oxidizing environments iron is available only as ferric ion, for which a saturated solution is about 10(18 molar at physiological pH (Ksp = [Fe3+][OH-]3 -10-39) (6). This problem has been circumvented in many prokaryotes by the evolution of ferrichrome and other siderophores, ligands that bind ferric ion with extreme avidity and selectivity, thereby solubilizing it for metabolic incorporation (7).…”