Based on the solubility product constant (Ksp) values, and the molar solubility values and concentration of the ions, the precipitate formed is Fe(OH)3.
The solubility product constant, Ksp, is the equilibrium constant for the dissolution of a solid into an aqueous solution.
The value of Ksp predicts the extent to which a compound can dissociate in water.
The higher the Ksp, the more soluble the compound is and vice versa.
The Ksp of the Fe(OH)2 and Fe(OH)3 are given as:
Also, the higher the molar solubility (x), the more soluble the solution.
The molar solubility depends on the Ksp and the number of ions produced.
The dissociation of Fe(OH)2 = Fe2+ + 2 OH-
Number of ions produced by Fe(OH)2 = 3
x * (2x)^2 = 4.87 x 10^-17
5x^2 = 4.87 x 10^-17
molar solubility, x = 3.12 × 10^-9
The dissociation of Fe(OH)3 = Fe3+ + 3 OH-
Number of ions produced by Fe(OH)3 = 4
x * (3x)^3 = 2.79 x 10^-39
27x^4 = 2.79 x 10^-39
molar solubility, x = 1.01 × 10^-10
Comparing the Ksp values of the two solutions shows that Fe(OH)2 has a higher Ksp value than Fe(OH)3.
Since, the concentration of the ions are the same, and the molar solubility values of Fe(OH)2 is greater than that of Fe(OH)3, the precipitate formed is Fe(OH)3.
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