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title: "A student constructs a galvanic cell under standard conditions. One beaker contains a \\(\\text{Zn(s)}\\) electrode immersed in \\(1.0\\text{ M }\\text{Zn(NO}_3)_2\\text{(aq)}\\), and the second beaker contains a \\(\\text{Cu(s)}\\) electrode immersed in \\(1.0\\text{ M }\\text{Cu(NO}_3)_2\\text{(aq)}\\). The two half-cells are connected by an external wire with a voltmeter and a salt bridge filled with \\(\\text{KNO}_3\\text{(aq)}\\). The balanced equation for the spontaneous reaction is \\[\\text{Zn}(s) + \\text{Cu}^{2+}(aq) \\rightarrow \\text{Zn}^{2+}(aq) + \\text{Cu}(s)\\] Which of the following correctly identifies the direction of \\(\\text{NO}_3^-\\text{(aq)}\\) ion migration from the salt bridge and provides the correct justification?"
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url: "https://nerd-notes.com/ubq/120007/"
date_modified: "2026-08-21T08:31:50+00:00"
---

# A student constructs a galvanic cell under standard conditions. One beaker contains a \(\text{Zn(s)}\) electrode immersed in \(1.0\text{ M }\text{Zn(NO}_3)_2\text{(aq)}\), and the second beaker contains a \(\text{Cu(s)}\) electrode immersed in \(1.0\text{ M }\text{Cu(NO}_3)_2\text{(aq)}\). The two half-cells are connected by an external wire with a voltmeter and a salt bridge filled with \(\text{KNO}_3\text{(aq)}\). The balanced equation for the spontaneous reaction is
\[\text{Zn}(s) + \text{Cu}^{2+}(aq) \rightarrow \text{Zn}^{2+}(aq) + \text{Cu}(s)\]
Which of the following correctly identifies the direction of \(\text{NO}_3^-\text{(aq)}\) ion migration from the salt bridge and provides the correct justification?

A student constructs a galvanic cell under standard conditions. One beaker contains a \(\text{Zn(s)}\) electrode immersed in \(1.0\text{ M }\text{Zn(NO}_3)_2\text{(aq)}\), and the second beaker contains a \(\text{Cu(s)}\) electrode immersed in \(1.0\text{ M }\text{Cu(NO}_3)_2\text{(aq)}\). The two half-cells are connected by an external wire with a voltmeter and a salt bridge filled with \(\text{KNO}_3\text{(aq)}\). The balanced equation for the spontaneous reaction is
\[\text{Zn}(s) + \text{Cu}^{2+}(aq) \rightarrow \text{Zn}^{2+}(aq) + \text{Cu}(s)\]
Which of the following correctly identifies the direction of \(\text{NO}_3^-\text{(aq)}\) ion migration from the salt bridge and provides the correct justification?

- **A.** \(\text{NO}_3^-\text{(aq)}\) ions migrate into the \(\text{Cu(s)}\) half-cell because negative ions must balance the excess positive charge produced as \(\text{Cu}^{2+}\text{(aq)}\) is reduced.
- **B.** \(\text{NO}_3^-\text{(aq)}\) ions migrate into the \(\text{Cu(s)}\) half-cell because anions follow the path of electrons flowing through the salt bridge.
- **C.** \(\text{NO}_3^-\text{(aq)}\) ions migrate into the \(\text{Zn(s)}\) half-cell because negative ions must balance the accumulation of positive charge as \(\text{Zn(s)}\) is oxidized to \(\text{Zn}^{2+}\text{(aq)}\).
- **D.** \(\text{NO}_3^-\text{(aq)}\) ions migrate into the \(\text{Zn(s)}\) half-cell because anions transfer electrons directly through the solution to the anode.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/120007/*