Chemistry

Chemistry

Problem

An aqueous mixture contains 0.0010 M0.0010\,\mathrm{M} each of Zn2+^{2+}, Fe2+^{2+}, and Mn2+^{2+}. The pH is adjusted to 8.8 with a buffer. Solubility product constants at 25\,°C are Ksp(Zn(OH)2)=3.0×10−17K_{sp}(\mathrm{Zn(OH)_2}) = 3.0 \times 10^{-17} Ksp(Fe(OH)2)=4.9×10−17K_{sp}(\mathrm{Fe(OH)_2}) = 4.9 \times 10^{-17} Ksp(Mn(OH)2)=2.0×10−13K_{sp}(\mathrm{Mn(OH)_2}) = 2.0 \times 10^{-13} At this pH, which metal hydroxide(s) will precipitate? a) Only Zn(OH)2\mathrm{Zn(OH)_2} b) Fe(OH)2\mathrm{Fe(OH)_2} and Mn(OH)2\mathrm{Mn(OH)_2} only c) Zn(OH)2\mathrm{Zn(OH)_2} and Fe(OH)2\mathrm{Fe(OH)_2} only d) All three hydroxides precipitate

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