Answer:
9.28 × 10⁻¹¹ mol/L
Explanation:
Let's consider the solution of iron(III) hydroxide.
Fe(OH)₃(s) ⇄ Fe³⁺(aq) + 3 OH⁻(aq)
We can relate the solubility (S) of the hydroxide with the solubility product (Ksp) using an ICE chart.
Fe(OH)₃(s) ⇄ Fe³⁺(aq) + 3 OH⁻(aq)
I 0 0
C +S +3S
E S 3S
The solubility product is:
Ksp = [Fe³⁺] × [OH⁻]³ = S × (3S)³ = 27 S⁴
[tex]S=\sqrt[4]{\frac{Ksp}{27} } = \sqrt[4]{\frac{2.0 \times 10^{-39} }{27} } = 9.28 \times 10^{-11} mol/L[/tex]
Answer:
S = 9.28 E-11 M
Explanation:
S S 3S
∴ Ksp Fe(OH)3 = 2.0 E-39
⇒ Ksp = [Fe3+]*[OH-]³ = (S)*(3S)³ = 27(S)∧4
⇒ 27(S)∧4 = 2.0 E-39
⇒ (S)∧4 = 7.407 E-41
⇒ S = (7.407 E-41)∧(1/4)
⇒ S = 9.28 E-11 M
