Hydrolysis constant for, III

Table III. Acid Hydrolysis Constants for Various Cellulosic Materials...

The first hydrolysis constant for plutonium(III), that is, the equilibrium constant for the reaction... 

Liu and Millero (1999) have determined the solubility of Fe(lll) in NaCl solutions as a function of pH, temperature, and ionic strength. These results clearly show that the solubility in NaCl (10 pM) near pH = 8 is much higher than in seawater (200-600 pM) at the same temperature and ionic strength. These results have been used to determine the hydrolysis constants for the formation of Fe(III) complexes with hydroxide (Figure 8) as a function of temperature and ionic strength. The cumulative stoichiometric hydrolysis constants (3 for reactions are given by... 

Cm(iii) is a class A or hard metal ion and thus complexes far more strongly to oxygen and fluoride donors than to more polarizable donors such as chloride or sulfur. Solution reactions of Cm resemble those of the trivalent lanthanides and actinides. The fluoride, oxalate, phosphate, iodate, and hydroxide are essentially water-insoluble and the chloride, iodide, perchlorate, nitrate, and sulfate are water-soluble. The first hydrolysis constant for Cm ", i.e. for the reaction ... 

Preparation and chemistry of chromium compounds can be found ia several standard reference books and advanced texts (7,11,12,14). Standard reduction potentials for select chromium species are given ia Table 2 whereas Table 3 is a summary of hydrolysis, complex formation, or other equilibrium constants for oxidation states II, III, and VI. 

The variation of the concentration of the free (non-hydrolyzed) cations with pH is shown for the oxidation states of III to VI in Figure 3. These curves are based on estimated values of the hydrolysis constants but are of sufficient accuracy to indicate the pH values at which hydrolysis becomes significant (e.g.,... 

Rate Constants for Aquation and for Base Hydrolysis of Selected penta-ammine-Cobalt(III) Complexes a... 

Calculate the hydrolysis constant Kh for the ammonium chloride solution from Part III. Assume that [NH4+] is the same as the initial concentration of ammonium chloride. 

Metastability of Hydrolyzed Iron (III) Solutions The low solubility of ferric hydroxide has been alluded to in the Introduction. Feitknecht and Michaelis (29) have observed that aU ferric perchlorate solutions to which base has been added are unstable with respect to eventual precipitation of various forms of hydrated ferric oxides. In 3 M NaC104 at 25° C the two phase system reaches an apparent equilibrium after 200 hours, according to Biedermann and Schindler (6), who obtained a reproducible solubility product constant for ferric hydroxide at varying degrees of hydrolysis. It appears that many of the solutions used in the equilibrium studies of Hedstrom (9) and Biedermann (22) were metastable, and should eventually have produced precipitates. Nevertheless, since the measured potentials were reversible, the conclusions reached about the species present in solution remain valid. 

The kinetic effects of C02 in the base catalyzed hydrolysis of some carboxylato amine cobalt(III) complexes have been reported (80-82). In the base catalyzed hydrolysis of oxalatopentaammine-cobalt(III) (80), C02 retarded the reaction due to the formation of a virtually unreactive ion-pair, f (N H .) r, 2 2 COi ]. The equilibrium constant for formation of carbonate ion-pairs with (glycinato-O) (tetraethylene-pentamine)cobalt(III), (81) and (o-methoxybenzoato) (tetraethylenepentamine)cobalt(III) (82) were, however, much smaller than for the oxalatopentamminecobat(III) and a very weak rate retardation and virtually no effect was observed in the base catalyzed hydrolysis of the latter two complexes. 

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