Multiple Choice
According to general solubility rules, which of the following compounds is most likely to be soluble in water at room temperature?
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6. Chemical Quantities & Aqueous Reactions
Solubility Rules
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According to solubility rules and the solubility product constant (K_sp) for Fe(OH)_2, above what Fe^{2+} concentration will Fe(OH)_2 begin to precipitate in a solution with [OH^-] = 1.0 imes 10^{-4} M? (K_{sp} = 8.0 imes 10^{-16})
A
8.0 imes 10^{-8} M
B
8.0 imes 10^{-4} M
C
8.0 imes 10^{-8} M
D
8.0 imes 10^{-8} M
Verified step by step guidance1
Write the dissociation equation for Fe(OH)\_2: $\mathrm{Fe(OH)_2 (s) \rightleftharpoons Fe^{2+} (aq) + 2 OH^- (aq)}$.
Express the solubility product constant $K_{sp}$ in terms of ion concentrations: $K_{sp} = [Fe^{2+}][OH^-]^2$.
Rearrange the $K_{sp}$ expression to solve for the concentration of $Fe^{2+}$: $[Fe^{2+}] = \frac{K_{sp}}{[OH^-]^2}$.
Substitute the given values into the equation: $K_{sp} = 8.0 \times 10^{-16}$ and $[OH^-] = 1.0 \times 10^{-4} \; M$.
Calculate $[Fe^{2+}]$ using the substituted values to find the concentration above which $Fe(OH)_2$ will begin to precipitate.
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