The solubility product of Fe(OH)3 is 8.0x10^-40. Calculate its solubility at 35 degrees Celsius in a saturated solution.
IF Ksp is 8.0E-40 @ 35C, then, let S = solubility.
............Fe(OH)3 ==> Fe^+3 + 3OH^-
..............S.........S........3S
Ksp = (Fe^+3)(OH^-)^3
Ksp = (S)(3S)^3
Solve for S.
To calculate the solubility of Fe(OH)3 at 35 degrees Celsius in a saturated solution, we need to make use of the solubility product constant (Ksp) and the equation representing the dissolution of Fe(OH)3.
The solubility product constant (Ksp) is the equilibrium constant for the dissociation of a sparingly soluble compound into its constituent ions. For Fe(OH)3, the equation representing its dissolution is:
Fe(OH)3(s) ⇌ Fe3+(aq) + 3OH-(aq)
Given that the solubility product constant (Ksp) for Fe(OH)3 is 8.0x10^-40, we can set up an equation using the stoichiometry of the reaction:
Ksp = [Fe3+] * [OH-]^3
Let's assume that x represents the molar solubility of Fe(OH)3. At equilibrium, the concentration of Fe3+ ions is equal to the molar solubility (x), and the concentration of OH- ions is 3x (based on the stoichiometry of the reaction).
Substituting these values into the Ksp expression, we have:
Ksp = (x) * (3x)^3
Simplifying this equation, we get:
8.0x10^-40 = 27x^4
To solve for x, we can take the fourth root and calculate:
x = (8.0x10^-40)^(1/4)
x = 1.00x10^-10
So, the solubility of Fe(OH)3 at 35 degrees Celsius in a saturated solution is 1.00x10^-10 mol/L.