Metal complexes formation constants, table

The table summarizes the data up to the end of 1972. For each extractant and Its extractable metal complexes, distribution equilibrium constants, as well as appropriate extraction constants, are recorded. In addition, the homogeneous equilibria involving the acid dissociation of the extractant in the aqueous phase and adduct or mixed ligand complex formation in the organic phase are characterized. Aqueous phase metal complex formation constants however, are not included inasmuch as these are already covered in Stability Constants. 

This 228 page volume summarizes equilibrium constants for liquid-liquid distribution equilibrium constants up to the end of 1972. Each table includes the extractant and its extractable metal complexes, and.the distribution equilibrium constants and extraction constants. The aqueous phase metal complex formation constants are not included and the reader is referred to items and in this bibliography for sources of this type of data. References to the primary literature are included. 

Similar curves were obtained for racemic and L-polypropyleneglycine, PICEI and PEA. At high ligand concentration n approaches the limiting value of 2. Taking account of the presence of two coordinating atoms in each monomer unit, the coordination number four is thus found from the experimental data. Table IV summarizes the metal complex formation constants for the different poly ampholytes. The displacement constant B2 is defined by the equation... 

In common with other hydroxy organic acids, tartaric acid complexes many metal ions. Formation constants for tartaric acid chelates with various metal ions are as follows Ca, 2.9 Cu, 3.2 Mg, 1.4 and Zn, 2.7 (68). In aqueous solution, tartaric acid can be mildly corrosive toward carbon steels, but under normal conditions it is noncorrosive to stainless steels (Table 9) (27). 

Based upon analogies between surface and molecular coordination chemistry outlined in Table 1, we have recently set forth to investigate the interaction of surface-active and reversibly electroactive moieties with the noble-metal electrocatalysts Ru, Rh, Pd, Ir, Pt and Au. Our interest in this class of compounds is based on the fact that chemisorption-induced changes in their redox properties yield important information concerning the coordination/organometallic chemistry of the electrode surface. For example, alteration of the reversible redox potential brought about by the chemisorption process is a measure of the surface-complex formation constant of the oxidized state relative to the reduced form such behavior is expected to be dependent upon the electrode material. In this paper, we describe results obtained when iodide, hydroquinone (HQ), 2,5-dihydroxythiophenol (DHT), and 3,6-dihydroxypyridazine (DHPz), all reversibly electroactive... 

The following Table (Table 1) shows the values of the stability constants of some purines and pyrimidines with a number of transition metal ions (7, 2, 36, 69). Procedures for the synthesis of Cu, Co and Ni complexes with pyrimidines have been reported (65, 92, 93). The preparation of purine-metal compounds are described elsewhere (94, 95). There seem to be great difficulties in the quantitative study of metal complex formation, especially with the free purines, since the resulting metal chelates are almost insoluble in aqueous solution. Therefore, dioxane-water mixtures have been employed in a number of experiments. 

The larger the value of the constant is, the more stable the complex (Table 12.11). The metal-ammine formation constants Ksl and Kst are known as stepwise formation constants. Stepwise formation constants1 could be used to estimate overall formation constants. For example,... 

Example 3.1 Estimate the omplex for the system with Fe2+/3+ as the metal ions and EDTA4- as the ligand. Take the approximate log values of the complex formation constants as 14 and 25 for the EDTA4- complexes of Fe2+ and Fe3+, respectively. The E q can be found in any table of standard potentials. 

These parameters, intrinsic bond stability c and ligand sensitivity x referring to some certain hapticity, can now be applied for calculating and thus predicting complex formation constants for all the metal ions, complex fragments and organometal species in Table 2.3... 

Formation Constants of Metal Complexes (Section 1, Table 1-17)... 

Table 1 Complex formation constants for reactions of metal ions with multidentate ligands and their unidentate analogs. ...

Table 3. Work of adsorption limiting adsorption (/ ax) and logarithm of the complex-formation constant (IgK) of DBK-metal salt complexes at the interface of aqueous solutions of inorganic salts and benzene solutions of DBK...

C6, the most widely used complexing agent is ethylenediaminetetracetic acid or EDTA, and Table 1 gives a selection of metal EDTA formation constants. 

Within the limits of experimental error PPG-L presents practically the same complex formation constants as the racemic PPG. From the table it can be seen that log 2 > equal to log p2 log/ i, is usually much smaller than logA i it very likely results from chain conformation restrictions and steric effects, as well as from variation of the electrostatic potential due to the binding of the metal ion on the neighboring unit. 

Table 8.12 Cumulative Formation Constants for Metal Complexes with...

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