What concentration of Fe₂(SO₄)₃(aq)is required for the solution to have [Fe³⁺(aq)] = 0.32 M? A)0.16 M B)0.32 M C)0.64 M D)0.080 M E)0.12 M

Question

Quizplus · Accepted Answer

The given compound can be represented as FeSO4(SO4)2. We can write the balanced chemical equation of its dissociation as:
FeSO4(SO4)2 ⇌ Fe2+ + SO4^2- + 2SO4^2-

Let the concentration of FeSO4(SO4)2 be x M, then the concentration of Fe2+ ions would also be x M (1:1 stoichiometry). Now, the concentration of SO4²⁻ ions would be 2x M (2:1 stoichiometry). We can use the given equilibrium constant expression to relate these concentrations:

Ksp = [Fe2+][SO4^2-]²
Ksp = x(2x)² = 4x³
x = (Ksp/4)^(1/3) = (8.7×10⁻¹³/4)^(1/3) ≈ 0.16 M

Therefore, the required concentration of FeSO4(SO4)2 is 0.16 M to have [Fe²⁺] = 0.32 M.

What Concentration of Fe2(SO4)3(aq)is Required for the Solution to Have

What Concentration of Fe₂(SO₄)₃(aq)is Required for the Solution to Have