Final answer:
The solubility product constant (Ksp) of Ag3PO4 at 25 °C is calculated using the concentrations of the ions produced upon dissolution and is found to be 7.2 × 10^-12.
Step-by-step explanation:
To find the solubility product constant (Ksp) of Ag3PO4, we need to consider the dissociation of Ag3PO4 in water:
Ag3PO4 (s) ⇌ 3 Ag+ (aq) + PO43- (aq)
The given solubility (S) of Ag3PO4 is 4.3 × 10-5 M. This means that when Ag3PO4 dissolves, it forms 4.3 × 10-5 M of PO43- ions and 3 times that amount in Ag+ ions, which is 3 × 4.3 × 10-5 M or 1.29 × 10-4 M. The Ksp can thus be calculated using the formula:
Ksp = [Ag+]3[PO43-]
By plugging in the concentrations, we get:
Ksp = (1.29 × 10-4 M)3 × (4.3 × 10-5 M)
Ksp = 7.2 × 10-12