---
title: "A student constructs a galvanic cell using a zinc electrode immersed in a \\(1.0 \\text{ M ZnSO}_4\\text{(aq)}\\) solution and a copper electrode immersed in a \\(1.0 \\text{ M CuSO}_4\\text{(aq)}\\) solution. The two half-cells are separated by a porous glass frit that permits ion movement between the solutions, as shown in the diagram. As the reaction \\(\\text{Zn(s)} + \\text{Cu}^{2+}\\text{(aq)} \\rightarrow \\text{Zn}^{2+}\\text{(aq)} + \\text{Cu(s)}\\) proceeds, which of the following correctly describes the migration of ions through the porous glass frit and provides the correct justification?"
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url: "https://nerd-notes.com/ubq/119371/"
date_modified: "2026-08-19T12:40:03+00:00"
---

# A student constructs a galvanic cell using a zinc electrode immersed in a \(1.0 \text{ M ZnSO}_4\text{(aq)}\) solution and a copper electrode immersed in a \(1.0 \text{ M CuSO}_4\text{(aq)}\) solution. The two half-cells are separated by a porous glass frit that permits ion movement between the solutions, as shown in the diagram. As the reaction \(\text{Zn(s)} + \text{Cu}^{2+}\text{(aq)} \rightarrow \text{Zn}^{2+}\text{(aq)} + \text{Cu(s)}\) proceeds, which of the following correctly describes the migration of ions through the porous glass frit and provides the correct justification?

A student constructs a galvanic cell using a zinc electrode immersed in a \(1.0 \text{ M ZnSO}_4\text{(aq)}\) solution and a copper electrode immersed in a \(1.0 \text{ M CuSO}_4\text{(aq)}\) solution. The two half-cells are separated by a porous glass frit that permits ion movement between the solutions, as shown in the diagram. As the reaction \(\text{Zn(s)} + \text{Cu}^{2+}\text{(aq)} \rightarrow \text{Zn}^{2+}\text{(aq)} + \text{Cu(s)}\) proceeds, which of the following correctly describes the migration of ions through the porous glass frit and provides the correct justification?

![A schematic diagram of a galvanic cell consisting of two glass beakers separated by a vertical wall containing a porous glass frit in the center. The left beaker contains a zinc strip labeled Zn(s) immersed in a 1.0 M ZnSO4 solution containing Zn2+ and SO42- ions. The right beaker contains a copper strip labeled Cu(s) immersed in a 1.0 M CuSO4 solution containing Cu2+ and SO42- ions. A metallic wire connects the top of the Zn(s) electrode to the top of the Cu(s) electrode through a voltmeter labeled V. An arrow above the wire points from left to right, indicating the direction of electron flow from the Zn(s) electrode to the Cu(s) electrode. The Zn(s) electrode is labeled Anode (-), and the Cu(s) electrode is labeled Cathode (+). No other text, labels, or annotations appear.](https://nerd-notes.com/wp-content/uploads/ubq-frq-generated/stem-diagram-1-1787143203-mCHpsI.jpg)

- **A.** \(\text{SO}_4^{2-}\text{(aq)}\) ions migrate toward the cathode to neutralize the buildup of positive charge at the cathode.
- **B.** \(\text{Zn}^{2+}\text{(aq)}\) ions migrate toward the anode to balance the loss of positive charge as zinc metal is oxidized.
- **C.** \(\text{SO}_4^{2-}\text{(aq)}\) ions migrate toward the anode to neutralize the buildup of positive charge from \(\text{Zn}^{2+}\text{(aq)}\) ions generated during oxidation.
- **D.** \(\text{Cu}^{2+}\text{(aq)}\) ions migrate toward the anode to prevent the deposition of copper metal on the surface of the anode.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119371/*