At 25 â°c only 0.0690 mol of the generic salt ab3 is soluble in 1.00 l of water. what is the ksp of the salt at 25 â°c?

We can write the equation for the solubility of the salt AB3 in water as
     AB3(s) ⇌ A3+ + 3B- 
Since 0.0690 mol AB3 dissolves in 1.00 L of water, the concentration of the ions in moles per liter is calculated as
     0.0690 mol / 1.00 L water = 0.0690 M
We now substitute this value to the solubility product Ksp expression
     Ksp = [A3+] [B-]^3
            = (0.0690 M) (3 * 0.0690 M)^3 
            = 0.000612
Therefore, the Ksp of the salt is 6.12 x 10^-4.

The answer is !