Final answer:
Ionic equations illustrate the dissociation of slightly soluble ionic compounds in water into constituent ions, with Ksp expressions representing their solubility products. For CuS, Zn(OH)2, SrF2, and Fe2O3, the respective ionic equations and Ksp expressions have been provided, demonstrating the equilibrium concentrations of the dissolved ions.
Step-by-step explanation:
The dissolution of a slightly soluble ionic compound in water can be illustrated using an ionic equation that shows how the compound dissociates into its constituent ions. The solubility product constant (Ksp) is an expression that quantifies the solubility of the compound under equilibrium conditions.
- CuS dissociates into Cu2+ and S2- ions:
CuS(s) ⇌ Cu2+(aq) + S2-(aq)
The Ksp expression is Ksp = [Cu2+][S2-] - Zn(OH)2 dissociates into Zn2+ and 2OH- ions:
Zn(OH)2(s) ⇌ Zn2+(aq) + 2 OH-(aq)
The Ksp expression is Ksp = [Zn2+][OH-]^2 - SrF2 dissociates into Sr2+ and 2F- ions:
SrF2(s) ⇌ Sr2+(aq) + 2 F-(aq)
The Ksp expression is Ksp = [Sr2+][F-]^2 - Fe2O3 dissociates into 2Fe3+ and 3O2- ions (note that O2- doesn't exist freely in solution and typically water molecules would be involved in the actual solubility equilibrium, but for simplicity it's shown here):
Fe2O3(s) ⇌ 2Fe3+(aq) + 3O2-(aq)
The Ksp expression is Ksp = [Fe3+]^2[O2-]^3