AP Chemistry
4.9 Oxidation-Reduction (Redox) Reactions
4.8 Introduction to Acid-Base Reactions
4.7 Types of Chemical Reactions
A student investigates three chemical processes used to treat different laboratory wastewater samples. The balanced chemical equations for the reactions are shown in the table below.
Which species acts as the reducing agent in the oxidation-reduction reaction?
| Process | Balanced chemical equation |
|---|---|
| 1 | \(\text{Pb(NO}_3\text{)}_2\text{(aq)} + 2\,\text{KI(aq)} \rightarrow \text{PbI}_2\text{(s)} + 2\,\text{KNO}_3\text{(aq)}\) |
| 2 | \(\text{HNO}_3\text{(aq)} + \text{KOH(aq)} \rightarrow \text{KNO}_3\text{(aq)} + \text{H}_2\text{O(l)}\) |
| 3 | \(\text{Zn(s)} + 2\,\text{HCl(aq)} \rightarrow \text{ZnCl}_2\text{(aq)} + \text{H}_2\text{(g)}\) |
Which species acts as the reducing agent in the oxidation-reduction reaction?
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