Solubility product, calculation

Given gas partial pressures (Fig. 3.10), a model to calculate solubility product (Eq. 3.36) can be calculated for gas hydrates (Fig. 3.11). The actual solubility product calculations are made at the experimental gas partial pressures, which vary widely (Fig. 3.10). Equation 2.29 was used to adjust all these pressure-dependent estimates (Kp) to a hypothetical 1.0 atm total pressure (iTP0), which is what is presented in Fig. 3.11. [Pg.44]

In pure water the usual solubility product calculation applies ... [Pg.689]

The following example illustrates how solubility-product calculations are used to determine the feasibility of separations based on solubility differences. [Pg.300]

Solubility product calculations are actually based on heterogeneous equilibria. Why are pure soUds and liquids exempted from these calculations ... [Pg.845]

Slavtscheva, Popova, and Gospodinov [84SLA/POP] prepared Ge(Se03)2(cr) and measured its solubility in dilute mineral acids. The solubility product calculated from these measurements is not accepted, see Appendix A. [Pg.213]

Popova, Slavtscheva, and Gospodinov [86POP/SLA] determined the solubility of aluminium selenite in dilute nitric acid. The preparation and composition of the selenite is not discussed. It is assumed to have the formula Al2(Se03)3-6H20(cr) by the review. The solubility product calculated in the paper, see Appendix A, for Reaction (V.65),... [Pg.231]

The solubility product calculated from the Gibbs energy of formation of a-HgSe is log = - (60.35 + 0.70) and overlaps with the values from the experimental measurements. [Pg.282]

When carrying out solubility and/or solubility product calculations, keep in mind the following important points ... [Pg.669]

For all the metal cations studied, the potentiometric titration curves at different temperatures show no essential distinctions, and resemble the corresponding dependences for the KCl-NaCl melt. The solubility product calculations demonstrate that an increase in the melt temperature causes the increase in the oxide solubility (pTWo) by 0.3-0.4. The obtained data show... [Pg.293]

The solubility of Ni(OH)2 in pure water was measured from 298.15 to 313.15K. Only the solubility products calculated by the assumption 2[Ni(II)] = [OH ] have been given (at 25°C log 5K°D= - 11.82). Thus, the conclusion has been confirmed that by direct reaction of Ni(OH)2(cr) with water no reliable solubility data can be obtained [18ALM], [67BLA]. Thus, these results were not included in either Table V-6 or Figure V-11. [Pg.389]

It is reasonable to assume that the solubility product values for these solid phases determined at 16°C and 30°C apply to 25°C because 1) the experimental temperatures (ranging from 16 to 30°C) differ only slightly from 25°C, 2) the equilibrium constants for the formation of ThSO and Th(S04)2(aq) reported at 10°C, 25°C, and 30°C differ insignificantly from each other, and 3) the solubility products calculated for Th(S04)2-9H20(cr) at 16°C and 25°C are essentially identical as listed in this table. [Pg.299]

TABLE 14.10 Solubility products, calculated formation constants, and calculated and experimental E° values (V vs NHE) for the silver halides at 298 K. [Pg.467]

B. (a) Using activity coefficients with the solubility product, calculate the solubility of HgBr2 in water. By solubility, we mean the concentration of dissolved Hg ". The solubility is so small that the ionic strength is approximately 0 and the activity coefficients are approximately 1. [Pg.265]

This differs considerably from the solubility product calculated with the activity coefficient and saturation molality. Rearranging equation (6.3) using this value for the solubility product and the saturation molality of 31.7, the activity coefficient needed for use with the Kgp can be calculated ... [Pg.404]

The solubility product calculated by the product of the activities would be for this reaction ... [Pg.405]

This Is about half the value of the solubility product calculated using the NBS data that assumes complete dissociation. Since the amount of calcium and sulfate ions in solution are so low and the association of the two to form an aqueous molecule would have little effect on the ionic strength, it may be decided to disregard the interaction. The large difference in the solubility products points out that care must be taken in matching the thermodynamic data to the modeling method chosen. [Pg.435]

Solubility from solubility product Calculate the concentration of CrO " in a solution saturated with BaCr04 and containing (a) no other solute (b) 0.20 mole BaClg/liter,... [Pg.293]

Calculating solubility from solubility product Calculate the solubility of copper(ll) sulfide in mol dm-3. [Pg.327]

Equilibrium aspects of acid-base reactions, including calculations and discussion of changes in pH during acid-base titrations. Examples of solubility product calculations. [Pg.596]

Big Chemical Encyclopedia

Chemical substances, components, reactions, process design ...