---
title: "A student constructs the galvanic cell shown in the diagram, operating at \\(298\\text{ K}\\) under standard conditions according to the following balanced equation:  \\[ \\text{Ni}(s) + 2\\,\\text{Ag}^+(aq) \\rightarrow \\text{Ni}^{2+}(aq) + 2\\,\\text{Ag}(s) \\quad E^\\circ_{\\text{cell}} = +1.06\\text{ V} \\]  The student then adds a few drops of concentrated \\(\\text{NaCl}(aq)\\) to the cathode compartment, causing the immediate formation of a white precipitate of \\(\\text{AgCl}(s)\\) while the total solution volume remains virtually unchanged. Which of the following best predicts and explains the effect of this addition on the cell potential, \\(E_{\\text{cell}}\\)?"
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url: "https://nerd-notes.com/ubq/123941/"
date_modified: "2026-09-28T12:32:23+00:00"
---

# A student constructs the galvanic cell shown in the diagram, operating at \(298\text{ K}\) under standard conditions according to the following balanced equation:

\[ \text{Ni}(s) + 2\,\text{Ag}^+(aq) \rightarrow \text{Ni}^{2+}(aq) + 2\,\text{Ag}(s) \quad E^\circ_{\text{cell}} = +1.06\text{ V} \]

The student then adds a few drops of concentrated \(\text{NaCl}(aq)\) to the cathode compartment, causing the immediate formation of a white precipitate of \(\text{AgCl}(s)\) while the total solution volume remains virtually unchanged. Which of the following best predicts and explains the effect of this addition on the cell potential, \(E_{\text{cell}}\)?

A student constructs the galvanic cell shown in the diagram, operating at \(298\text{ K}\) under standard conditions according to the following balanced equation:

\[ \text{Ni}(s) + 2\,\text{Ag}^+(aq) \rightarrow \text{Ni}^{2+}(aq) + 2\,\text{Ag}(s) \quad E^\circ_{\text{cell}} = +1.06\text{ V} \]

The student then adds a few drops of concentrated \(\text{NaCl}(aq)\) to the cathode compartment, causing the immediate formation of a white precipitate of \(\text{AgCl}(s)\) while the total solution volume remains virtually unchanged. Which of the following best predicts and explains the effect of this addition on the cell potential, \(E_{\text{cell}}\)?

![A grayscale line drawing of a galvanic cell consisting of two open beakers connected by an inverted U-tube salt bridge and an external wire with a circle labeled V representing a voltmeter. The left beaker contains a gray rectangular electrode labeled \(\text{Ni}(s)\) submerged in a solution labeled \(1.0\text{ M }\text{Ni}^{2+}(aq)\). The right beaker contains a gray rectangular electrode labeled \(\text{Ag}(s)\) submerged in a solution labeled \(1.0\text{ M }\text{Ag}^+(aq)\). The inverted U-tube spans between the two beakers with its ends immersed in each solution, labeled salt bridge. An external wire connects the top of the \(\text{Ni}\) electrode to the left terminal of the voltmeter and the right terminal of the voltmeter to the top of the \(\text{Ag}\) electrode. No other particles, labels, text, or annotations appear.](https://nerd-notes.com/wp-content/uploads/ubq-frq-generated/stem-fig-1-1790598742-wfrPwN.jpg)

- **A.** \(E_{\text{cell}}\) decreases because \([\text{Ag}^+]\) decreases, which increases the value of \(Q\) and makes the forward reaction less thermodynamically favorable.
- **B.** \(E_{\text{cell}}\) decreases because \([\text{Ag}^+]\) decreases, which decreases the standard cell potential, \(E^\circ_{\text{cell}}\).
- **C.** \(E_{\text{cell}}\) increases because precipitation removes reactant ions, which decreases the value of \(Q\) and drives the forward reaction.
- **D.** \(E_{\text{cell}}\) remains unchanged because \(\text{AgCl}(s)\) is an insoluble precipitate, and pure solids do not alter the reaction quotient, \(Q\).

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/123941/*