What is the solubility in moles/liter for iron(III) hydroxide at 25 oC given a Ksp value of 2.0 x 10-39. Write using scientific notation and use 1 or 2 decimal places (even though this is strictly incorrect!)
2 answers:
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
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
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