---
title: "A student constructs a galvanic cell at \\(298 \\text{ K}\\) based on the balanced reaction below:  \\[\\text{Ni}(s) + 2\\text{Ag}^+(aq) \\rightarrow \\text{Ni}^{2+}(aq) + 2\\text{Ag}(s)\\]  Initially, the cell operates under standard conditions with \\([\\text{Ag}^+] = 1.0 \\text{ M}\\) and \\([\\text{Ni}^{2+}] = 1.0 \\text{ M}\\), giving a standard cell potential \\(E^\\circ_{\\text{cell}} = +1.06 \\text{ V}\\). Distilled water is added to the \\(\\text{Ag}^+(aq)\\) half-cell, lowering \\([\\text{Ag}^+]\\) to \\(0.10 \\text{ M}\\) while \\([\\text{Ni}^{2+}]\\) remains \\(1.0 \\text{ M}\\). Which of the following predicts the effect of this modification on the cell potential, \\(E_{\\text{cell}}\\), and provides the correct reasoning?"
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url: "https://nerd-notes.com/ubq/119281/"
date_modified: "2026-08-19T12:39:38+00:00"
---

# A student constructs a galvanic cell at \(298 \text{ K}\) based on the balanced reaction below:

\[\text{Ni}(s) + 2\text{Ag}^+(aq) \rightarrow \text{Ni}^{2+}(aq) + 2\text{Ag}(s)\]

Initially, the cell operates under standard conditions with \([\text{Ag}^+] = 1.0 \text{ M}\) and \([\text{Ni}^{2+}] = 1.0 \text{ M}\), giving a standard cell potential \(E^\circ_{\text{cell}} = +1.06 \text{ V}\). Distilled water is added to the \(\text{Ag}^+(aq)\) half-cell, lowering \([\text{Ag}^+]\) to \(0.10 \text{ M}\) while \([\text{Ni}^{2+}]\) remains \(1.0 \text{ M}\). Which of the following predicts the effect of this modification on the cell potential, \(E_{\text{cell}}\), and provides the correct reasoning?

A student constructs a galvanic cell at \(298 \text{ K}\) based on the balanced reaction below:

\[\text{Ni}(s) + 2\text{Ag}^+(aq) \rightarrow \text{Ni}^{2+}(aq) + 2\text{Ag}(s)\]

Initially, the cell operates under standard conditions with \([\text{Ag}^+] = 1.0 \text{ M}\) and \([\text{Ni}^{2+}] = 1.0 \text{ M}\), giving a standard cell potential \(E^\circ_{\text{cell}} = +1.06 \text{ V}\). Distilled water is added to the \(\text{Ag}^+(aq)\) half-cell, lowering \([\text{Ag}^+]\) to \(0.10 \text{ M}\) while \([\text{Ni}^{2+}]\) remains \(1.0 \text{ M}\). Which of the following predicts the effect of this modification on the cell potential, \(E_{\text{cell}}\), and provides the correct reasoning?

- **A.** \(E_{\text{cell}}\) will be less than \(+1.06 \text{ V}\) because decreasing \([\text{Ag}^+]\) increases the reaction quotient \(Q\) above \(1\), which decreases the thermodynamic driving force for the forward reaction.
- **B.** \(E_{\text{cell}}\) will be greater than \(+1.06 \text{ V}\) because decreasing \([\text{Ag}^+]\) causes the system to shift toward the products to replace the lost reactant ions.
- **C.** \(E_{\text{cell}}\) will be less than \(+1.06 \text{ V}\) because decreasing \([\text{Ag}^+]\) lowers the standard cell potential \(E^\circ_{\text{cell}}\).
- **D.** \(E_{\text{cell}}\) will remain equal to \(+1.06 \text{ V}\) because cell potential depends only on the identity of the electrodes and temperature, not on ion concentrations.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119281/*