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Suheily218
13.06.2020 •
Chemistry
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?
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Ответ:
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.
Ответ:
An area of rectangle: a · b
a = 0.4 km
b = 0.07 km
a · b = 0.4 km · 0.07 km = 0.028 km²