Write the ionic equation for the dissolution and the Ksp expression for each of the following sl

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Write the ionic equation for the dissolution and the Ksp...

Write the ionic equation for the dissolution and the $K_{\mathrm{sp}}$ expression for each of the following slightly soluble ionic compounds:
(a) $\mathrm{LaF}_{3}$
(b) $\mathrm{CaCO}_{3}$
(c) $\mathrm{Ag}_{2} \mathrm{SO}_{4}$
(d) $\mathrm{Pb}(\mathrm{OH})_{2}$

Key Concepts

Ionic Dissolution Reactions

This concept involves writing balanced chemical equations that depict how a solid ionic compound dissociates into its constituent ions when it dissolves in water. In these reactions, the solid (often a sparingly soluble salt) is represented on the left, and its ionic components in solution are shown on the right, with stoichiometric coefficients reflecting the compound’s formula.

Solubility Product (Ksp)

The solubility product is the equilibrium constant for the dissolution process of a sparingly soluble ionic compound. It is defined as the product of the molar concentrations of the dissolved ions, each raised to the power of its coefficient in the balanced dissolution equation. This expression helps predict whether a precipitate will form under given conditions.

Chemical Equilibrium in Dissolution

The dissolution of a sparingly soluble salt reaches a dynamic equilibrium where the rate of dissolution equals the rate of precipitation. Understanding this equilibrium is essential for setting up the Ksp expression and for comprehending how changes in conditions can affect solubility.

Stoichiometry in Ionic Reactions

Stoichiometry ensures that the number of atoms and charges is balanced in the dissolution process. The proper use of stoichiometric coefficients is crucial when writing both the ionic dissolution equations and the corresponding Ksp expressions, as it directly affects the numerical exponents in the solubility product.

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