Thermodynamic study on the formation of the cupric ion hydrolytic species

Copper(II) complexes with an avian prion N-terminal region and their potential SOD-like activity

“…All data, including the computed distribution diagrams, were handled using the HYPERQUAD program, which minimizes the error-square sum of the differences between measured and calculated electrode potentials [53]. In order to get a better description, copper(II) hydrolytic species were taken into account [54]. In this paper, errors in stability constants are reported as three times standard deviations.…”

Chemical speciation of environmentally significant metals with inorganic ligands Part 2: The Cu2+-OH-, Cl-, CO32-, SO42-, and PO43- systems (IUPAC Technical Report)

“…Its existence has also been postulated by others [72OKa,82BBb,97RSb]. In addition to these dimeric species, a trinuclear complex Cu 3 (OH) 4 2+ has been suggested [60PEc,76ACb,79SDb]. This appears to form in measurable amounts only in solutions supersaturated with respect to CuO(s) and Cu(OH) 2 (s).…”

“…They found it impossible to determine the corresponding value for the formation of CuOH + . However, from calorimetric measurements in 0.1 mol dm -3 NaClO 4 at 25 °C, Arena et al [76ACb] reported ∆ r H m (*K 1 ) = 35.6 ± 2.9 kJ mol -1 for the formation of CuOH + (reaction 5), ∆ r H m (*β 2,2 ) = 77.0 ± 1.7 kJ mol -1 for Cu 2 (OH) 2 2+ (reaction 15) and ∆ r H m (*β 3,4 ) = 109 ± 4 kJ mol -1 for Cu 3 (OH) 4 2+ (reaction 16). Using K(T) data based upon potentiometric titrations within the temperature interval 10-45 °C (0.10 mol dm -3 NaClO 4 ) [97RSb] reported: ∆ r H m (*β 2,1 ) = 46.1 ± 2.9 kJ mol -1 and ∆ r H m (*β 2,2 ) = 68.1 ± 1.7 kJ mol -1 .…”

Thermodynamics of copper(II) dicarboxylate coordination in aqueous solution

“…The potentiometric data were treated by the computer programs ACBA (6°) and SCOGSB (7) and the calorimetric data by the program DOEC (61), as reported previously (59 …”

“…The calorimetric measurements were performed as reported previously (59). The heats of protonation were determined both by titrating the acids (50-60 mmol dm -3) with 0.1 mol dm -3 NaOH and by titrating HCIO4 (10-20 mmol dm -3 ) with the correspondent buffers.…”