What is the solubility, in moles per liter, of Fe(OH)₂ (K_sp = 7.9 × 10^-¹⁶), in 0.0500 molar NaOH solution?^{Hint: Be sure to account for the presence of a common ion. You should also be able to simplify the math because the solubility is very low.}

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The solubility of Fe(OH)₂ in the presence of a common ion (OH⁻ from NaOH) is calculated using the Ksp expression: Ksp = [Fe²⁺][OH⁻]². With [OH⁻] = 0.0500 M from NaOH, the solubility (s) of Fe(OH)₂ is s = Ksp / (0.0500)² = 7.9 × 10⁻¹⁶ / 0.0025 = 3.16 × 10⁻¹³ M.

What Is the Solubility, in Moles Per Liter, of Fe(OH)2

What Is the Solubility, in Moles Per Liter, of Fe(OH)₂