This redox equation is given: $\text{SnCl}_2(aq) + 2\text{HgCl}_2(aq) \rightarrow \text{SnCl}_4(aq) + \text{Hg}_2\text{Cl}_2(s)$. Which species undergoes oxidation in this reaction?
- A$\text{Sn}^{2+}$
- B$\text{Cl}^-$
- C$\text{Hg}^+$
- D$\text{Hg}^{2+}$
Chemistry 9701 · AS & A Level · Electrochemistry