The Ksp of FeCO3 is 3.13*10-11, the Ksp of Fe (OH) 2 is 4.87*10-17, and the Ksp of FeF2 is 2.36*10-6. If a solution contained CO2-3, OH-, and F - ions, each at a concentration of 0.1 M, and the Fe2 + ion concentration is slowly increased from a trace amount, which of the salts would precipitate first?

Fe (OH) ₂ will precipitate first

Explanation:

Ksp formulas for FeCO₃, Fe (OH) ₂ and FeF₂ are:

FeCO₃:

FeCO₃ (s) ⇄ Fe²⁺ + CO₃²⁻

Ksp = [Fe²⁺] [CO₃²⁻]. Replacing with the Ksp and CO₃²⁻ concentration values: 3.13x10⁻¹¹ = [Fe²⁺] [0.1M]

3.13x10⁻¹⁰ = [Fe²⁺]

That means, the system reaches the equilibrium when [Fe²⁺] = 3.13x10⁻¹⁰, for higher concentrations the FeCO₃ begins precipitation.

For the other salts:

Fe (OH) ₂:

Fe (OH) ₂ (s) ⇄ Fe²⁺ + 2OH⁻

Ksp = [Fe²⁺] [OH⁻]². Replacing with the Ksp and OH⁻ concentration values: 4.87x10⁻¹⁷ = [Fe²⁺] [0.1M]²

4.87x10⁻¹⁵ = [Fe²⁺]

FeF₂:

FeF₂ (s) ⇄ Fe²⁺ + 2F⁻

Ksp = [Fe²⁺] [F⁻]². Replacing with the Ksp and F⁻ concentration values: 2.36x10⁻⁶ = [Fe²⁺] [0.1M]²

2.36x10⁻⁴ = [Fe²⁺]

As you can see, the Fe (OH) ₂ begins the precipitation with the lower Fe²⁺ concentration, thus, Fe (OH) ₂ will precipitate first.