Final answer:
To calculate the solubility product constant (Ksp) for Ag2C2O4, use the provided concentration of Ag+ ions in a saturated solution and apply the stoichiometric relationship of the dissolution reaction. The calculated Ksp for silver oxalate is 5.3 × 10−11.
Step-by-step explanation:
The question pertains to the calculation of the solubility product constant (Ksp) of silver oxalate (Ag2C2O4). To find the solubility product constant, we need to understand the dissolution of Ag2C2O4 in water, which can be represented by the equation:
Ag2C2O4 (s) ⇌ 2 Ag+ (aq) + C2O42- (aq)
Given that the concentration of Ag+ ions in a saturated solution is 2.2 × 10−4 mol L−1, and following the stoichiometry of the dissolution, the concentration of C2O42- will be half of the concentration of Ag+, so [C2O42-] = 1.1 × 10−4 mol L−1.
Then, we can calculate the solubility product constant as:
Ksp = [Ag+]2 × [C2O42-] = (2.2 × 10−4)2 × (1.1 × 10−4) = 5.3 × 10−11
Thus, the solubility product of Ag2C2O4 is 5.3 × 10−11.