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Solved: A galvanic cell is constructed by immersing a
Chapter 18, Problem 18.135(choose chapter or problem)
A galvanic cell is constructed by immersing a piece of copper wire in 25.0 mL of a 0.20 \(M \ CuSO_{4}\) solution and a zinc strip in 25.0 mL of a 0.20 \(M \ ZnSO_{4}\) solution.
(a) Calculate the emf of the cell at \(25^{\circ}C\) and predict what would happen if a small amount of concentrated \(NH_3\) solution were added to (i) the \(CuSO_{4}\) solution and (ii) the \(ZnSO_{4}\) solution. Assume that the volume in each compartment remains constant at 25.0 mL.
(b) In a separate experiment, 25.0 mL of 3.00 \(M\) \(NH_3\) are added to the \(CuSO_{4}\) solution. If the emf of the cell is 0.68 V, calculate the formation constant (\(Kf\)) of \(Cu(NH_{3})^{2+}_4\).
Questions & Answers
QUESTION:
A galvanic cell is constructed by immersing a piece of copper wire in 25.0 mL of a 0.20 \(M \ CuSO_{4}\) solution and a zinc strip in 25.0 mL of a 0.20 \(M \ ZnSO_{4}\) solution.
(a) Calculate the emf of the cell at \(25^{\circ}C\) and predict what would happen if a small amount of concentrated \(NH_3\) solution were added to (i) the \(CuSO_{4}\) solution and (ii) the \(ZnSO_{4}\) solution. Assume that the volume in each compartment remains constant at 25.0 mL.
(b) In a separate experiment, 25.0 mL of 3.00 \(M\) \(NH_3\) are added to the \(CuSO_{4}\) solution. If the emf of the cell is 0.68 V, calculate the formation constant (\(Kf\)) of \(Cu(NH_{3})^{2+}_4\).
ANSWER:Step 1 of 6
Given
\(\begin{array}{l}
V\left(\mathrm{CuSO}_{4}\right)=25.0 \mathrm{ml} \\
C\left(\mathrm{CuSO}_{4}\right)=0.20 \mathrm{M} \\
V\left(\mathrm{ZnSO}_{4}\right)=25.0 \mathrm{ml} \\
C\left(\mathrm{ZnSO}_{4}\right)=0.20 \mathrm{M} \\
V \rightarrow \text { volume } \\
C \rightarrow \text { concentration }
\end{array}\)
Standard reduction potential at \(25^{\circ} \mathrm{C}\) for pair \(\mathrm{Cu}^{2+} / \mathrm{Cu} \text { is } 0.34 \mathrm{~V}\).
Standard reduction potential at \(25^{\circ} \mathrm{C}\) for pair \(\mathrm{Zn}^{2+} / \mathrm{Zn} \text { is }-0.76 \mathrm{~V}\).
The more positive \(E^{\circ}\) value is, the greater the tendency for the substance to be reduced.
By the standard reduction potential at \(25^{\circ} \mathrm{C}\)
Hence we can say copper is the cathode and zinc is the anode.