#23
At 25 °C only 0.0800 mol of the generic salt AB3 is soluble in 1.00 L of water. What is the Ksp of the salt at 25 °C?
.........AB3 --> A + 3B
I.......solid....0....0
C.......solid..0.08..3*0.08
E.......solid..0.08..0.24
Ksp = (A)(B)^3 = ?
Substitute from the ice chart and solve for Ksp.
To find the Ksp of the salt AB3 at 25 °C, we need to use the given solubility information. The solubility of AB3 is given as 0.0800 mol/L at 25 °C.
The solubility product constant, Ksp, is an equilibrium constant for the dissolution of a solid salt into its constituent ions in a saturated solution. For the generic salt AB3, it can be represented by the equation:
AB3 (s) ↔ A+ (aq) + 3B- (aq)
In this equation, A+ and B- represent the cations and anions, respectively, that make up the salt AB3.
The equilibrium expression for the solubility product is:
Ksp = [A+] * [B-]^3
In this case, the concentration of A+ is the same as the concentration of AB3, which is 0.0800 mol/L.
Therefore, we can substitute the given values into the equilibrium expression:
Ksp = (0.0800) * (0.0800)^3
Simplifying the expression:
Ksp = 0.0800 * 0.0800 * 0.0800 * 0.0800
Calculating:
Ksp = 4.096 x 10^(-6)
Therefore, the Ksp of the generic salt AB3 at 25 °C is 4.096 x 10^(-6).