The solubility of iron(III)hydroxide is 4.39E-10M. What is the Ksp for this compound? I don't know how I would go about this problem.
...........Fe(OH)3 ==> Fe^3+ + 3OH^-
I...........solid......0........0
C......x dissolves.....x........3x
E...........solid......x........3x
The problem tells you that x = 4.39E-10M = (Fe^3+).
Therefore, 3x = 3*4.39E-10M = (OH^-)
Then Ksp = (Fe^3+)(OH^-)^3 = substitute and solve for Ksp.
1.52x10^64
To find the Ksp (solubility product constant) for iron(III) hydroxide, you need to understand the relationship between the equilibrium equation and the solubility of a compound.
The solubility product constant (Ksp) is a measure of the maximum amount of a compound that can dissolve in a solution at equilibrium. It is determined by the stoichiometry of the balanced equation for the dissociation of the compound.
The solubility equilibrium for iron(III) hydroxide can be represented by the balanced equation:
Fe(OH)3(s) ⇌ Fe3+(aq) + 3OH-(aq)
The Ksp expression for this equilibrium is:
Ksp = [Fe3+][OH-]^3
Where [Fe3+] represents the concentration of Fe3+ ions and [OH-] represents the concentration of OH- ions at equilibrium.
Given that the solubility of iron(III) hydroxide is 4.39E-10 M, we can assume that the concentration of Fe3+ ions is also 4.39E-10 M at equilibrium, since they have a 1:1 stoichiometric ratio.
Substituting the known values into the Ksp expression:
Ksp = (4.39E-10)^1 * (4.39E-10)^3
= 8.805E-40
Therefore, the Ksp for iron(III) hydroxide is 8.805E-40.