Analogy Salt Soluble ! Sand:
Answers
Answer:
insoluble
Explanation:
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Answer:
When a slightly soluble ionic compound is added to water, some of it dissolves to form a solution, establishing an equilibrium between the pure solid and a solution of its ions. For the dissolution of calcium phosphate, one of the two main components of kidney stones, the equilibrium can be written as follows, with the solid salt on the left:
Ca3(PO4)2(s)⇌3Ca2+(aq)+2PO3−4(aq)(17.1.1)
As you will discover in Section 17.4 and in more advanced chemistry courses, basic anions, such as S2−, PO43−, and CO32−, react with water to produce OH− and the corresponding protonated anion. Consequently, their calculated molarities, assuming no protonation in aqueous solution, are only approximate.
The equilibrium constant for the dissolution of a sparingly soluble salt is the solubility product (Ksp) of the salt. Because the concentration of a pure solid such as Ca3(PO4)2 is a constant, it does not appear explicitly in the equilibrium constant expression. The equilibrium constant expression for the dissolution of calcium phosphate is therefore
K=[Ca2+]3[PO3−4]2[Ca3(PO4)2](17.1.2)
[Ca3(PO4)2]K=Ksp=[Ca2+]3[PO3−4]2(17.1.3)
At 25°C and pH 7.00, Ksp for calcium phosphate is 2.07 × 10−33, indicating that the concentrations of Ca2+ and PO43− ions in solution that are in equilibrium with solid calcium phosphate are very low. The values of Ksp for some common salts are listed in Table 17.1.1 , which shows that the magnitude of Ksp varies dramatically for different compounds. Although Ksp is not a function of pH in Equations 17.1.2 and 17.1.3 , changes in pH can affect the solubility of a compound as discussed later.