---
title: "A student constructs the galvanic cell shown in the diagram, consisting of a $\\text{Zn(s)}$ electrode immersed in $1.0\\text{ M }\\text{Zn(NO}_3)_2\\text{(aq)}$ and a $\\text{Cu(s)}$ electrode immersed in $1.0\\text{ M }\\text{Cu(NO}_3)_2\\text{(aq)}$. A salt bridge filled with $\\text{KNO}_3\\text{(aq)}$ connects the two solutions, and the initial cell potential is measured as $+1.10\\text{ V}$. During the trial, the student lifts the salt bridge completely out of the solutions. Which of the following best predicts and explains the effect of removing the salt bridge on the measured cell potential?"
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url: "https://nerd-notes.com/ubq/120350/"
date_modified: "2026-08-23T04:23:19+00:00"
---

# A student constructs the galvanic cell shown in the diagram, consisting of a $\text{Zn(s)}$ electrode immersed in $1.0\text{ M }\text{Zn(NO}_3)_2\text{(aq)}$ and a $\text{Cu(s)}$ electrode immersed in $1.0\text{ M }\text{Cu(NO}_3)_2\text{(aq)}$. A salt bridge filled with $\text{KNO}_3\text{(aq)}$ connects the two solutions, and the initial cell potential is measured as $+1.10\text{ V}$. During the trial, the student lifts the salt bridge completely out of the solutions. Which of the following best predicts and explains the effect of removing the salt bridge on the measured cell potential?

A student constructs the galvanic cell shown in the diagram, consisting of a $\text{Zn(s)}$ electrode immersed in $1.0\text{ M }\text{Zn(NO}_3)_2\text{(aq)}$ and a $\text{Cu(s)}$ electrode immersed in $1.0\text{ M }\text{Cu(NO}_3)_2\text{(aq)}$. A salt bridge filled with $\text{KNO}_3\text{(aq)}$ connects the two solutions, and the initial cell potential is measured as $+1.10\text{ V}$. During the trial, the student lifts the salt bridge completely out of the solutions. Which of the following best predicts and explains the effect of removing the salt bridge on the measured cell potential?

![A line drawing in grayscale depicting a galvanic cell apparatus. On the left, a glass beaker contains a liquid solution labeled $1.0\text{ M }\text{Zn(NO}_3)_2\text{(aq)}$, with a solid rectangular electrode shaded light gray labeled $\text{Zn(s)}$ immersed in it. On the right, a second glass beaker contains a liquid solution labeled $1.0\text{ M }\text{Cu(NO}_3)_2\text{(aq)}$, with a solid rectangular electrode shaded dark gray labeled $\text{Cu(s)}$ immersed in it. A wire connects the $\text{Zn(s)}$ electrode to a circular voltmeter labeled $\text{V}$, which connects via wire to the $\text{Cu(s)}$ electrode. An inverted U-tube salt bridge labeled $\text{KNO}_3\text{(aq)}$ bridges the two beakers with its open ends submerged in each solution. No other particles, labels, text, or annotations appear.](https://nerd-notes.com/wp-content/uploads/ubq-frq-generated/stem-fig-1-1787458999-o0WIHg.jpg)

- **A.** The measured potential remains $+1.10\text{ V}$ because the cell potential is determined solely by the standard reduction potentials of $\text{Zn}^{2+}\text{(aq)}$ and $\text{Cu}^{2+}\text{(aq)}$.
- **B.** The measured potential increases above $+1.10\text{ V}$ because removing the salt bridge prevents $\text{NO}_3^-\text{(aq)}$ from migrating into the anode half-cell, driving zinc oxidation forward.
- **C.** The measured potential immediately drops to $0.00\text{ V}$ because ions can no longer migrate between half-cells to maintain electrical neutrality, rapidly halting electron flow through the external circuit.
- **D.** The measured potential immediately drops to $0.00\text{ V}$ because electrons are prevented from traveling through the salt bridge from the cathode half-cell back to the anode half-cell.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/120350/*