Final answer:
To find the Ksp for silver carbonate (Ag₂CO₃), the dissociation equation Ag₂CO₃(s) → 2Ag+(aq) + CO₃²−(aq) is used, and the Ksp expression is Ksp = [Ag+]2[CO₃2−]. The specific silver ion concentration must be known to calculate the exact Ksp value. For silver carbonate, the Ksp value at 25°C is 8.46 × 10⁻⁹.
Step-by-step explanation:
The solubility product constant, Ksp, is a special type of equilibrium constant that measures the solubility of a sparingly soluble ionic compound. For a compound like silver carbonate, Ag₂CO₃, the dissociation in water is represented by the chemical equation:
Ag₂CO₃(s) → 2Ag+(aq) + CO₃²−(aq
The Ksp expression for this reaction is
Ksp = [Ag+]2[CO₃2−
If the silver ion concentration at saturation is given, let's denote it as [Ag+] = x. Since the stoichiometry of Ag₂CO₃ dictates that for every mole of Ag₂CO₃ that dissolves, two moles of Ag+ are produced, the carbonate ion concentration will be [CO₃2−] = x/2 due to the 1:1 ratio in the formula.
Thus, substituting the ion concentrations into the Ksp expression, we will have
Ksp = x2(x/2
However, to provide an accurate Ksp value, the specific silver ion concentration must be known. The exercise provided mentions a value of Ksp for silver carbonate of 8.46 × 10⁻⁹° at 25°C. Therefore, by applying stoichiometry and this Ksp value, one can calculate the molarity and the mass of Ag₂CO₃ that will dissolve in a given volume of water.