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title: "A student prepares a galvanic cell at \\(298\\text{ K}\\) based on the following standard reaction: \\[ \\text{Zn}(s) + 2\\,\\text{Ag}^+(aq) \\rightleftharpoons \\text{Zn}^{2+}(aq) + 2\\,\\text{Ag}(s) \\quad E^\\circ_{\\text{cell}} = +1.56\\text{ V} \\] The student uses a beaker containing a zinc strip in \\(1.0\\text{ M Zn(NO}_3)_2(aq)\\) as the anode half-cell and a beaker containing a silver strip in \\(1.0\\text{ M AgNO}_3(aq)\\) as the cathode half-cell. Instead of using a salt bridge saturated with \\(\\text{KNO}_3(aq)\\), the student mistakenly uses a salt bridge saturated with \\(\\text{KCl}(aq)\\). Upon inserting the bridge, a white precipitate forms immediately around the tip in the cathode compartment, and the initial measured cell potential is noticeably lower than \\(+1.56\\text{ V}\\). Which of the following best explains why the cell potential is lower than \\(E^\\circ_{\\text{cell}}\\)?"
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url: "https://nerd-notes.com/ubq/123916/"
date_modified: "2026-09-28T12:32:10+00:00"
---

# A student prepares a galvanic cell at \(298\text{ K}\) based on the following standard reaction:
\[ \text{Zn}(s) + 2\,\text{Ag}^+(aq) \rightleftharpoons \text{Zn}^{2+}(aq) + 2\,\text{Ag}(s) \quad E^\circ_{\text{cell}} = +1.56\text{ V} \]
The student uses a beaker containing a zinc strip in \(1.0\text{ M Zn(NO}_3)_2(aq)\) as the anode half-cell and a beaker containing a silver strip in \(1.0\text{ M AgNO}_3(aq)\) as the cathode half-cell. Instead of using a salt bridge saturated with \(\text{KNO}_3(aq)\), the student mistakenly uses a salt bridge saturated with \(\text{KCl}(aq)\). Upon inserting the bridge, a white precipitate forms immediately around the tip in the cathode compartment, and the initial measured cell potential is noticeably lower than \(+1.56\text{ V}\). Which of the following best explains why the cell potential is lower than \(E^\circ_{\text{cell}}\)?

A student prepares a galvanic cell at \(298\text{ K}\) based on the following standard reaction:
\[ \text{Zn}(s) + 2\,\text{Ag}^+(aq) \rightleftharpoons \text{Zn}^{2+}(aq) + 2\,\text{Ag}(s) \quad E^\circ_{\text{cell}} = +1.56\text{ V} \]
The student uses a beaker containing a zinc strip in \(1.0\text{ M Zn(NO}_3)_2(aq)\) as the anode half-cell and a beaker containing a silver strip in \(1.0\text{ M AgNO}_3(aq)\) as the cathode half-cell. Instead of using a salt bridge saturated with \(\text{KNO}_3(aq)\), the student mistakenly uses a salt bridge saturated with \(\text{KCl}(aq)\). Upon inserting the bridge, a white precipitate forms immediately around the tip in the cathode compartment, and the initial measured cell potential is noticeably lower than \(+1.56\text{ V}\). Which of the following best explains why the cell potential is lower than \(E^\circ_{\text{cell}}\)?

- **A.** Precipitation of \(\text{AgCl}(s)\) decreases \([\text{Ag}^+]\), making \(Q > 1\), which decreases \(E_{\text{cell}}\) according to the Nernst equation.
- **B.** Precipitation of \(\text{AgCl}(s)\) decreases \([\text{Ag}^+]\), making \(Q < 1\), which decreases \(E_{\text{cell}}\) according to the Nernst equation.
- **C.** Precipitation of \(\text{ZnCl}_2(s)\) decreases \([\text{Zn}^{2+}]\), making \(Q > 1\), which decreases \(E_{\text{cell}}\) according to the Nernst equation.
- **D.** Migration of \(\text{K}^+\) into the cathode compartment reduces the standard reduction potential \(E^\circ\) of the silver half-cell.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/123916/*