What is the molar solubility of Fe(OH)3 in water?
Can you write the ICE chart and Ksp equation? Show what you can do and explain where you have problems.
To determine the molar solubility of Fe(OH)3 in water, we need to consider the solubility product constant (Ksp) of Fe(OH)3. The Ksp represents the equilibrium constant for the dissolution of a solid compound.
The balanced equation for the dissolution of Fe(OH)3 in water is:
Fe(OH)3 (s) ⇌ Fe3+ (aq) + 3OH- (aq)
The Ksp expression for this equilibrium is:
Ksp = [Fe3+] * [OH-]^3
From the equation, we can see that one mole of Fe(OH)3 produces one mole of Fe3+ ions and three moles of OH- ions.
To calculate the molar solubility, we assume that x is the molar solubility of Fe(OH)3 in water. Therefore, the concentration of Fe3+ ions would be x M, and the concentration of OH- ions would be 3x M.
Plugging these values into the Ksp expression:
Ksp = (x) * (3x)^3
Simplifying the expression:
Ksp = 27x^4
Now, we need the value of the Ksp for Fe(OH)3. According to literature data, the Ksp value for Fe(OH)3 is 1.1 x 10^-38.
Setting up the equation:
1.1 x 10^-38 = 27x^4
Rearranging and solving for x:
x^4 = (1.1 x 10^-38) / 27
x ≈ (1.1 x 10^-38 / 27)^(1/4)
Using a calculator, we can evaluate this expression to find the molar solubility of Fe(OH)3 in water.