Final answer:
To calculate the solubility of silver sulfate (Ag₂SO₄) in different solutions, use the Ksp value and the concentrations of ions present. In water, use the Ksp value to calculate the concentration of Ag⁺ ions. In 0.01 M AgNO₃ solution, use the Ag⁺ concentration. In 0.20 M K₂SO₄ solution, calculate the concentration of SO₄²⁻ ions.
Step-by-step explanation:
To calculate the solubility of silver sulfate (Ag₂SO₄) in different solutions, we need to consider the solubility product constant (Ksp) and the concentrations of the ions present in the solution.
a) In water, since Ag₂SO₄ dissociates into Ag⁺ and SO₄²⁻ ions, we can use the Ksp value to calculate the concentration of Ag⁺ ions, which is equal to the solubility. Solubility (g/L) = [Ag⁺] = sqrt(Ksp) = sqrt(1.2 × 10⁻⁵).
b) In 0.01 M AgNO₃ solution, we can use the Ag⁺ concentration from the solution as the value for [Ag⁺].
c) In 0.20 M K₂SO₄ solution, we need to calculate the concentration of SO₄²⁻ ions from the solution and then use it as the value for [SO₄²⁻] in the Ksp expression.