Final answer:
The molar solubility of CdCO₃, given the Ksp of 5.2 × 10⁻¹², is calculated to be 2.28 × 10⁻¶ mol/L, using the solubility product relationship.
Step-by-step explanation:
To calculate the molar solubility of CdCO₃, we must first write out the dissociation equation and then establish the relationship between the concentrations of the ions produced and the solubility product constant (Ksp).
CdCO₃(s) → Cd²⁺(aq) + CO₃²⁺(aq)
Let's assume that the solubility of CdCO₃ is 's' mol/L. This would yield 's' mol/L of Cd²⁺ and 's' mol/L of CO₃²⁺. Plugging these values into the Ksp expression:
Ksp = [Cd²⁺][CO₃²⁺] = (s)(s) = s²
We are given Ksp for CdCO₃ as 5.2 × 10⁻¹². Therefore:
5.2 × 10⁻¹² = s²
To find the value of 's', we take the square root of both sides:
s = √(5.2 × 10⁻¹²) = 2.28 × 10⁻¶ mol/L
Therefore, the molar solubility of CdCO₃ is 2.28 × 10⁻¶ mol/L.