Solubility constant/product values listed

Examples of solubility products are listed in Table 1.9. Similarly to the dissociation constants, the solubility products are also dimensionless quantities. However, because of the choice of the standard state, their values numerically correspond to units of moles per cubic decimetre. 

The solubility product constant values listed in Appendix H were determined at 25°C. How would those values change, if at all, with a change in temperature ... 

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. 

Solubility equilibrium constants, such as (20) and (22), are given a special name—the solubility product. It is symbolized K,p. A low value of K,p means the concentrations of ions are low at equilibrium. Hence the solubility must be low. Table 10-11 lists solubility products for some common compounds. 

It is very important to distinguish between the solubility of a given solid and its solubility product. The solubility product is an equilibrium constant and thus has only one value for a given solid at a given temperature. Solubility, on the other hand, is an equilibrium position and has an infinite number of possible values at a given temperature, depending on the other conditions (such as the presence of a common ion). The Ksp values at 25°C for many common ionic solids are listed in Table 8.5. The units are customarily omitted. 

To what reaction does the solubility product constant, refer Table 16.1 lists sp values for several ionic solids. For any of these ionic compounds, you should be able to calculate the solubility. What is the solubility of a salt, and what procedures do you follow to calculate the solubility of a salt How would you calculate the value for a salt given the solubility ... 

If the solubility product characterizes only the level at which the solution is saturated, the solubility is the equivalent amoimt of the mineral in the solution under the same conditions. The values of the solubility product do not depend on the water composition whereas the solubility does. That is why the latter are not constants and are practically not used in thermodynamic evaluations. Moreover, it is necessary to distinguish between the mineral solubility in pure water, which is usually listed in reference books, and solubility of minerals in the real natural water, which is called effective solubility. 

Solubility product constants are important fiar a wide variety of applications, and have been determined for many sparingly soluble salts. Table 12.4 lists some common salts and their values. A more extensive table is included in Appendix H. 

The solid is omitted from the equilibrium constant because the solid is in its standard state. Values of sp re listed in Appendix A. We will use the solubility product to discuss precipitation titrations in Section 6-5. 

Even very small solubility products can be measured electrically, and these values are listed in chemical tables. As the above exercise illustrates, the solubility of a substance can be derived from its solubility product. Solubility products are generally listed only for slightly or sparingly soluble substances. If is very small, the substance is often termed insoluble (in water). In the case of moderately and highly soluble substances (such as NaCl or NaOH), the use of solubility products is not very useful. This is because instead of defining an equilibrium constant in terms of concentrations we would have to... 

Because each AgCl unit contains only one Ag and one CF ion, its solubility product expression is particularly simple to write. Many ionic compounds dissociate into more than two ions. Table 17.4 lists a number of slightly soluble ionic compounds along with equations representing their dissolution equilibria and their solubility product constants. (Compounds deemed soluble by the solubility rules in Chapter 4 are not listed for the same reason we did not list values for the strong acids in Table 16.6.) In general, the magnitude of indicates the solubility of an ionic compound—the smaller the value, the less soluble the compound. To make a direct... 

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