Question

Determine the concentration of Ag⁺ required to initiate precipitation of Ag₂CO₃ in a solution that is 2.50 × 10⁻⁶ M in CO₃²⁻.

a) 1.25 × 10⁻⁶ M
b) 5.00 × 10⁻⁶ M
c) 1.00 × 10⁻⁶ M
d) 2.50 × 10⁻⁶ M

Answer 1

To initiate precipitation of Ag₂CO₃ in a solution that is 2.50 × 10⁻⁶ M in CO₃²⁻, the concentration of Ag⁺ required is approximately 8.05 × 10⁻⁶ M.

Step-by-step explanation:

To determine the concentration of Ag⁺ required to initiate precipitation of Ag₂CO₃, we need to consider the solubility product constant (Ksp) of Ag₂CO₃. The Ksp is a measure of the equilibrium concentrations of the ions in a saturated solution. In this case, the concentration of CO₃²⁻ is given as 2.50 × 10⁻⁶ M.

We can set up the Ksp expression: Ksp = [Ag⁺]² [CO₃²⁻]. Substituting the given values, we have 8.1 × 10⁻¹² = [Ag⁺]² (2.50 × 10⁻⁶). Solving for [Ag⁺], we find that the concentration required to initiate precipitation is approximately 8.05 × 10⁻⁶ M.