ChemInform Abstract: STABILITAET VON MONOFORMIATO‐, ‐ACETATO‐, ‐PROPIONATO‐, ‐BUTYCATO‐, ‐GLYKOLATO‐ UND ‐CHLORACETATOKOBALT(II), ‐NICKEL(II), ‐KUPFER(II), ‐ZINK(II), ‐CADMIUM(II) UND ‐BLEI(II)

Filipović, Ivana; Matusinović, Tomislav; Mayer, Bernd; Piljac, I.; Bach‐Dragutinovic, B.; Bujak, A.

doi:10.1002/chin.197118037

Cited by 2 publications

(3 citation statements)

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“…Glycolate occasionally forms a chelate with metal ions without deprotonation of the α-OH group. This is the case for nickel(II) glycolate. − Accordingly, the stability constant of the nickel(II) glycolate complex is considerably larger than that of nickel(II) acetate. In contrast, the stability constant for palladium(II) glycolate is significantly smaller than that for palladium(II) acetate, which further supports the assumption of formation of a monodentate complex, as discussed above in connection with the absorption spectra.…”

Section: Discussionmentioning

confidence: 98%

Equilibrium and High-Pressure Kinetic Study of Formation and Proton-Assisted Aquation of Monodentate Acetate, Propionate, and Glycolate Complexes of Palladium(II) in Aqueous Solution

Shi

Elding

1996

Inorg. Chem.

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Kinetics and equilibria for reversible formation of 1:1 monodentate complexes between Pd(H2O)4 2+ and acetic, propionic, and glycolic acid (RCOOH) according to the equation Pd(H2O)4 2+ + RCOOH ⇌ Pd(H2O)3OOCR+ + H3O+ (k 1, k - 1) have been studied as a function of temperature and pressure in an aqueous medium with 0.60 ≤ [H+] ≤ 1.00 M, [RCOOH]/[H+] ≤ 1.0, and ionic strength 1.00 M. Stability constants β1 for the formation of acetate, propionate, and glycolate complexes are (2.19 ± 0.09) × 104, (2.10 ± 0.24) × 104, and (6.4 ± 0.1) × 103 M-1, repectively, at 25 °C and for a 1.00 M perchlorate medium. The rate expression, k obsd = k 1[RCOOH] + k - 1[H+], indicates that reaction between palladium and carboxylate anions is negligible under the experimental conditions used. Values for k 1/M-1 s-1, k - 1/M-1 s-1, ΔH 1 ⧧/kJ mol-1, ΔH - 1 ⧧/kJ mol-1, ΔS 1 ⧧/J K-1 mol-1, ΔS - 1 ⧧/J K-1 mol-1, ΔV 1 ⧧/cm3 mol-1, and ΔV - 1 ⧧/cm3 mol-1 at 25.0 °C are 19.3 ± 0.6, 32.8 ± 0.2, 52.5 ± 0.4, 57.5 ± 0.4, −44 ± 1, −23 ± 1, −8.1 ± 0.3, and −1.7 ± 0.2 for acetic acid; 12.0 ± 1.1, 26.4 ± 0.3, 55.3 ± 0.6, 56.8 ± 0.3, −32 ± 2, −34 ± 1, −8.9 ± 0.8, and −1.7 ± 0.2 for propionic acid; and 21.1 ± 0.3, 13.7 ± 0.1, 53.6 ± 0.4, 59.2 ± 0.6, −40 ± 1, −25 ± 2, −3.4 ± 0.2, and −2.3 ± 0.2 for glycolic acid. There is no relation between formation rate constants and pK a for these carboxylic acids. The nucleophilic properties of the carboxylic acids toward palladium(II) are similar to those of water molecules. A trigonal bipyramidal transition state stabilized by hydrogen bonding between the entering carboxylic acid and the leaving aqua ligand or (equivalent) between the entering oxonium ion and the leaving carboxylate ligand is suggested. Negative entropies, volumes of activation, and volume profiles support a strong contribution from bond making in the activation process.

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Section: Discussionmentioning

confidence: 98%

Equilibrium and High-Pressure Kinetic Study of Formation and Proton-Assisted Aquation of Monodentate Acetate, Propionate, and Glycolate Complexes of Palladium(II) in Aqueous Solution

Shi

Elding

1996

Inorg. Chem.

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“…The stability constant of 80PS appears to be too low compared with the values reported by other authors and is rejected. The last two values at 2.0 mol dm -3 ionic strength are from the same group and are rejected, the potentiometric one [70FM] because, as the authors admit, an interaction occurs between quinhydrone and the metal…”

Section: Formation Constants Of Complexes Of 2-hydroxyacetic Acid (Glmentioning

confidence: 99%

“…The polarographic value of 70FB must be rejected for the same reasons mentioned above for the zinc(II) complexes. The remaining values are reliable and, therefore, provisional [54EM,70FM,69W].…”

confidence: 99%

Critical evaluation of stability constants for alpha-hydroxycarboxylic acid complexes with protons and metal ions and the accompanying enthalpy changes. Part II. Aliphatic 2-hydroxycarboxylic acids (IUPAC Technical Report)

Portanova

Lajunen

Tolazzi

et al. 2003

Pure and Applied Chemistry

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ChemInform Abstract: STABILITAET VON MONOFORMIATO‐, ‐ACETATO‐, ‐PROPIONATO‐, ‐BUTYCATO‐, ‐GLYKOLATO‐ UND ‐CHLORACETATOKOBALT(II), ‐NICKEL(II), ‐KUPFER(II), ‐ZINK(II), ‐CADMIUM(II) UND ‐BLEI(II)

Cited by 2 publications

References 0 publications

Equilibrium and High-Pressure Kinetic Study of Formation and Proton-Assisted Aquation of Monodentate Acetate, Propionate, and Glycolate Complexes of Palladium(II) in Aqueous Solution

Equilibrium and High-Pressure Kinetic Study of Formation and Proton-Assisted Aquation of Monodentate Acetate, Propionate, and Glycolate Complexes of Palladium(II) in Aqueous Solution

Critical evaluation of stability constants for alpha-hydroxycarboxylic acid complexes with protons and metal ions and the accompanying enthalpy changes. Part II. Aliphatic 2-hydroxycarboxylic acids (IUPAC Technical Report)

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