Data tables solubility product constants

The solubility of sparingly soluble compounds that do not appear in this table may be calculated from the data in the table Solubility Product Constants . Solubility of inorganic gases may be found in the table Solubility of Selected Gases in Water Compounds are listed alphabetically by chemical formula in the most commonly used form (e.g., NaCl, NH NO, etc.). 

As an alternative to laboratory solubility measurements, solubility product constants (KSp), which are derived from thermodynamic data, can be used to calculate the solubility of solids in water (Table 2.9). Each solubility product constant describes a disassociation of a solid in water and calculates the activities or concentrations of the dissolution products in the saturated solution. The solubility product constant or another equilibrium constant of a reaction may be derived from the Gibbs free energy of the reaction (AG"K) as shown in the following equation ... 

In Table 22-1 there are given values of the solubility-product constants at room temperature for many substances. More complete tables of values of these constants may be found in the handbooks and reference books mentioned at the end of Chapter 1. An extensive table App. Ill) and a discussion of the experimental data on which the values depend are given by W. M. Latimer,. T/ie Oxidation States of the Elements and Their Potentials in Aqueous Solution, Prentice-Hall, Inc., New York, 1938. 

You can now use the data in the table to make a trial to see if the concentrations of Fe " and Fe(CN)6" in the mixed solution exceed the value of K p when substituted into the solubility product constant expression. 

Interpret Data What compound would precipitate first if a 0.500M sodium fluoride solution were added gradually to a solution already containing 0.500M concentrations of both barium ions and magnesium ions Use the data in Table 17.6. Write the solubility equilibrium equations and solubility product constant expressions for both compounds. Explain your answer. 

Table 6. Free calcium concentrations in equilibrium with common complexing agents. A low free calcium concentration implies effective complexation, whether the complex formed is soluble or insoluble. The data were derived from either stability constants (soluble complexes) or solubility products (insoluble complexes).

Appendix 1 presents numerous reference tables containing most important data on the solubility of inorganic compounds in water, the density, dissociation constants, solubility products, ionization potentials of various atoms, etc., as well as thermochemical constants because many laws of inorganic chemistry cannot be explained without these quantities. 

The study of the variation of the solubility with the selenite concentration is stated to have been carried at the constant ionic strengths 0.01 and 0.3 M. How this was accomplished was not clear from the information in the paper. The data in the tables rather seem to indicate that the ionic strength varied and reached 0.03 and 0.5 M, respectively, in the solution with the highest selenite concentrations. The analysis of the data was made with an equilibrium model that comprised the solubility equilibrium and the formation of the complex 0(8003)2 T us the formation of CoSe03(aq) was not included in the model. The analysis led to values of the solubility product at the two ionic strengths that appear to be inconsistent with the value obtained from the solubility in water. This result together with the improbable model made the review reject the outcome of the equilibrium analysis. 

As is seen from Fig. 3.7.1 the pO values at the excess of the studied cation are sufficiently low, and owing to the enhanced acidic properties of the KCl-LiCl melt, the increase in the melt acidity results in a considerable increase in the oxide solubility, so that CoO, which is practically insoluble in the molten KCl-NaCl equimolar mixture, becomes appreciably soluble with a sharp pronounced section of the unsaturated solution (see Fig. 3.7.1, curve 3). The existence of the said section allows us to calculate the dissociation constant of CoO in the molten KCl-LiCl eutectic at 700 °C using the potentiometric data for three initial points of the calibration curve (the corresponding treatment results are collected in Table 3.7.2), and its average value is presented in Table 3.7.3. The fourth point of the titration curve is the boundary one between the saturated and unsaturated solution, and therefore, it is available for calculations of the values of both the dissociation constant and the solubility product. 

An example of the SAM data treatment for zinc oxide is presented in Table 3.7.6. The quantities of ZnO corresponding to points 1-6 do not result in the formation of a saturated solution the e.m.f. (pO) data make it possible to estimate the dissociation constant of ZnO in the KCl-NaCl melt as pKZnQ = 6.37 0.08. Point 7 corresponds to the weight of ZnO which provides saturation of the melt by zinc oxide, thereat the added powder of oxide is dissolved in the melt only partially. Subsequent additions of ZnO to the saturated melt result in an appreciable reduction in the saturated solution s concentration (decrease in the solubility product of ZnO) owing to the reduction in the averaged molar surface area of the deposit and, in turn, the oxide solubility. This reduction ends after the true plateau is achieved, when the changes of molar surface-area are negligible. 

Everett and Rasmussen studied cell (Va) with acetone and found = —0.53 V at 25°C assuming the dissociation constant of HCl to be 10" . They also calculated E (Ag+ Ag) assuming ATso(AgCl) = 4.10" (no reference was given for J so) More recent work yields = 10" -. Other e.m.f. measurements on this cell have employed acetone/HaO mixtures and the results have been tabulated elsewhere. - An Agl cell similar, to (VII) was studied by Mackor in several water/acetone mixtures. Mackor s data for the solubility product of Agl are summarised in Table 2.7.12 (25 C). 

This woik was prepared under the sponsorship of the Commission on Electrochemical Data of the Section of Analytical Chemistry of the International Union of Pure and Applied Chemistry. It is included in a general program of the Section of Analytical Chemistry. The Commission on Equilibrium Data, for example publishes elsewhere solubility products and stability constants of metal-ion complexes. From these constants and from the values reported here, the values of the potentials of many redox systems not reported in the present Tables can be computed. 

This handbook contains extensive tables of data for the more common Inorganic and organic aqueous electrolyte solutions. Properties covered include dielectric constants, activity coefficients, relative partial molar enthalpies, equilibrium constants, solubility products, conductivities, electrochemical potentials, Gibbs energies and enthalpies of formation, entropies, heat capacities, viscosities, and diffusion coefficients. Unfortunately, only a few of the tables contain references to the sources of the data. 

The data collected in this table show that the order of arrangement of oxides according to increase of their solubility corresponds to the similar dependences in the KCl-NaCl and CsCl-KCl-NaCl melts at 600 and 700°C. The performed study makes it possible to estimate the dissociation constants of PbO and CdO, which are close, therefore, it can assumed that the dissociation constants of oxides, having close solubility product values, are practically the same. The solubility parameters are close to those in the KCl-NaCl melt at 700°C. The dependences of the oxide solubility on the polarizing action of cation by Goldschmidt can be approximated by the following equation ... 

The experimental data were interpreted by using mononuclear hydrolysis constants only. The total Zr concentration could not be used as a variable to distinguish between mononuclear or polynuclear hydrolysis products because the concentration was fixed by the solubility of Zr(OH)4(s). The stability constants listed in Table A-5 were obtained. These constants were converted, with error propagation, to hydrolysis constants, logio Pq x, as given in Table A-6. 

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