Problem 16 - Chemistry A Guided Inquiry

Question

Which is the stronger oxidizing agent, \(\mathrm{Cu}^{2+}(\mathrm{aq})\) or \(\mathrm{H}^{+}(\mathrm{aq})\) ?

Step-by-Step Solution

Answer

The stronger oxidizing agent is determined by comparing the standard reduction potentials of \(\mathrm{Cu}^{2+}(\mathrm{aq})\) and \(\mathrm{H}^{+}(\mathrm{aq})\). Without the specific values from a standard electrode potential table, a definitive answer can't be given in this context. However, once the numbers are available, the ion with the higher reduction potential will be the stronger oxidizing agent.

Step 1: Refer to Standard Electrode Potential Table

Refer to a Standard Electrode Potential Table which will have reduction potentials listed for various half-reactions. The reduction potential values for \(\mathrm{H}^{+} \rightarrow \mathrm{H_{2}} (g)\) and \(\mathrm{Cu}^{2+} \rightarrow \mathrm{Cu} (s)\) are required.

Step 2: Compare the Standard Reduction Potentials

Compare the standard reduction potentials. Use the values obtained from the standard electrode potential table. The species with the higher standard reduction potential will be the stronger oxidizing agent.

Step 3: Draw a conclusion

The species with the higher standard reduction potential is the stronger oxidizing agent, because it is more prone to be reduced (gain electrons).