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The solubility product of Fe(OH)3 is 1xx...

The solubility product of `Fe(OH)_3` is `1xx10^(-36)` What is the minimum concentration of `OH^-` ions required to precipitate `Fe(OH)_3` from a 0.001 M solution of `FeCl_3` ?

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To solve the problem of finding the minimum concentration of \( OH^- \) ions required to precipitate \( Fe(OH)_3 \) from a 0.001 M solution of \( FeCl_3 \), we can follow these steps: ### Step 1: Write the expression for the solubility product (Ksp) of \( Fe(OH)_3 \) The solubility product \( K_{sp} \) for \( Fe(OH)_3 \) can be expressed as: \[ K_{sp} = [Fe^{3+}][OH^-]^3 \] ...
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