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At \( 25^{\circ} \mathrm{C} \), a galvanic cell was set up having the following
P half-reactions:
\[
\begin{array}{ll}
\mathrm{Fe}^{2+}(\mathrm{aq})+2 e^{-} \rightleftharpoons \mathrm{Fe}(\mathrm{s}) ; & E_{\mathrm{Fe}^{2 *}}^{\circ}=-0.447 \mathrm{~V} \\
\mathrm{Cu}^{2+}(\mathrm{aq})+2 e^{-} \rightleftharpoons \mathrm{Cu}(\mathrm{s}) ; & E_{\mathrm{Cu}^{2 *}}^{0}=+0.3419 \mathrm{~V}
\end{array}
\]
W
The copper half-cell contained \( 100 \mathrm{~mL} \) of \( 1.00 \mathrm{M} \mathrm{CuSO}_{4} \). The iron half-cell contained \( 50.0 \mathrm{~mL} \) of \( 0.100 \mathrm{M} \mathrm{FeSO}_{4} \). To the iron half-cell was added \( 50.0 \mathrm{~mL} \) of \( 0.500 \mathrm{M} \mathrm{NaOH} \) solution. The mixture was stirred and the cell potential was measured to be \( 1.175 \mathrm{~V} \). Calculate the value of \( K_{\text {ip }} \) for \( \mathrm{Fe}(\mathrm{OH})_{2} \).
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