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IB Chemistry SL 3.2.6 Primary Voltaic Cells Questions

Use real SL exam questions to draw voltaic cells, trace electrons and explain how salt bridges complete the circuit.

Syllabus
First assessment 2025
Course
Chemistry SL
Level
SL

Exam points

  • Draw or interpret a voltaic cell with two metal/metal-ion half-cells, electrodes, electrolytes, salt bridge and an external circuit.
  • Identify the spontaneous redox reaction and electron flow from the anode to the cathode through the external circuit.
  • Explain salt-bridge ion movement and electrical neutrality, and choose or label the cell arrangement that supports the stated voltaic reaction.

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Study 3.2.6—Primary (voltaic) cells conceptsOpen the corresponding Concept lesson for explanations, examples and exam connections.

IB Chemistry SL 3.2.6 Primary Voltaic Cells Questions question 1

[Maximum number: 1]

Iron rusts in the presence of oxygen and water. Rusting is a redox process involving several steps that produces hydrated iron(III) oxide, Fe2O3∙nH2O\mathrm{Fe}_{2} \mathrm{O}_{3} \bullet \mathrm{nH}_{2} \mathrm{O}, as the final product. The half-equations involved for the first step of rusting are given below.

Half-equation 1: Fe(s)→Fe2+(aq)+2e−\quad \mathrm{Fe}(\mathrm{s}) \rightarrow \mathrm{Fe}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-}

Half-equation 2: O2(aq)+4e−+2H2O(l)→4OH−(aq)\quad \mathrm{O}_{2}(\mathrm{aq})+4 \mathrm{e}^{-}+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \rightarrow 4 \mathrm{OH}^{-}(\mathrm{aq})

A voltaic cell is made from a half-cell containing a magnesium electrode in a solution of magnesium nitrate and a half-cell containing a silver electrode in a solution of silver(I) nitrate.

Figure for Question IB Chemistry SL 3.2.6 Primary Voltaic Cells Questions question 1 — IB Chemistry SL

Negative electrode (anode):

Positive electrode (cathode):
(ii) Outline one function of the salt bridge.

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