How many moles of Fe(OH)2 will dissolve in 1.0 liter of water buffered at ph= 10

Question

Explanation / Answer

Fe(OH)2 --> Fe++ (aq) + 2 OH- (aq) By definition, the equilibrium equation is: Ksp = [Fe++] [OH-]² From the equation, if x moles of Fe(OH)2 dissolve in 1 L of buffer solution, then the concentration of ferrous ion is x and the concentration of hydroxide ion is 2x. Substitute this and Ksp into the equilibrium equation: 1.8 x 10^-15 = x (2x)², or 1.8 x 10^-15 = 4x³. Solving for x, the solubility, x = ((1.8 x 10^-15)/4)^(1/3) = 7.7x10^-6 M.

Related Questions

Navigate

• Browse (All)
• Browse H
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.