Final answer:
To calculate the Ksp for the generic salt AB with a molarity of 8.8 × 10^-5 M at 25°C, square the molarity to get Ksp = 7.744 × 10^-9.
Step-by-step explanation:
The question asks for the calculation of the solubility product constant (Ksp) for a generic salt AB, given its solubility at 25°C. The solubility has been converted to molarity as 8.8 × 10-5 M, implying that when AB dissolves, it produces a molar concentration of A+ and B- ions each equal to the molarity of the dissolved salt.
The equation for the dissolution of AB in water is:
AB(s) ⇌ A+(aq) + B-(aq)
If we let the molar solubility of AB be represented as 's', then the molarity of A+ ions and B- ions in solution at equilibrium will both be 's'. The expression for Ksp is:
Ksp = [A+][B-] = s2
Substituting the given molar solubility into the expression:
Ksp = (8.8 × 10-5)2
Ksp = 7.744 × 10-9