Final answer:
To calculate the concentrations of ions in saturated solutions of BaF2, ZnS, Mg(OH)2, and SrSO4, we can use their respective solubility products. The molar solubility of each compound is equal to the concentrations of its ions in the saturated solution.
Step-by-step explanation:
(a) BaF2
To calculate the concentrations of ions in a saturated solution of BaF2, we need to determine the molar solubility of BaF2 using its solubility product. The solubility product (Ksp) of a compound is equal to the product of the concentrations of its ions raised to the power of their stoichiometric coefficients. For BaF2, the dissolution equation is:
BaF2(s) → Ba^2+(aq) + 2F^-(aq)
The Ksp expression is:
Ksp = [Ba^2+][F^-]^2
Since BaF2 is a strong electrolyte when it dissolves, we can assume that its molar solubility is equal to the concentrations of its ions in the saturated solution. Therefore, the concentration of Ba^2+ is equal to the molar solubility of BaF2, and the concentration of F^- is twice the molar solubility of BaF2.
(b) ZnS
The dissolution equation for ZnS is:
ZnS(s) → Zn^2+(aq) + S^2-(aq)
The Ksp expression is:
Ksp = [Zn^2+][S^2-]
Again, the molar solubility of ZnS is equal to the concentrations of its ions in the saturated solution.
(c) Mg(OH)2
The dissolution equation for Mg(OH)2 is:
Mg(OH)2(s) → Mg^2+(aq) + 2OH^-(aq)
The Ksp expression is:
Ksp = [Mg^2+][OH^-]^2
Once again, the molar solubility of Mg(OH)2 is equal to the concentrations of its ions in the saturated solution.
(d) SrSO4
The dissolution equation for SrSO4 is:
SrSO4(s) → Sr^2+(aq) + SO4^2-(aq)
The Ksp expression is:
Ksp = [Sr^2+][SO4^2-]
Similarly, the molar solubility of SrSO4 is equal to the concentrations of its ions in the saturated solution.