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AP Chemistry
9.10 Cell Potential Under Nonstandard Conditions
9.8 Galvanic (Voltaic) and Electrolytic Cells
IntermediateMCQConceptual21.1k
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.
Schematic diagram of the galvanic cell under standard conditions at \(298\text{ K}\).
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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