Question

Which of the following species will be oxidized by \(1 \mathrm{M} \mathrm{HCl} ?\) (a) \(\mathrm{Au}\) (b) \(\mathrm{Mg}\) (c) \(\mathrm{Cu}\) (d) \(\mathrm{F}^{-}\)

Short answer

Answer: (b) Mg

Step-by-step solution

Find the Standard Reduction Potentials for each species

Refer to the Standard Reduction Potential table to find the reduction potentials for Au, Mg, Cu, and F-. Also, find the reduction potential for H+ in HCl. The reduction potentials are as follows: - Au: +1.50 V - Mg: -2.37 V - Cu: +0.34 V - F-: +2.87 V - H+: 0 V (as a reference)

Compare the Reduction Potentials

To find out which species will be oxidized by 1 M HCl, we need to compare the reduction potentials of the given species to that of H+. A species will be oxidized when its reduction potential is lower than that of another reacting species. Comparing the values, we can see that the Reduction Potential of: - Au (+1.50 V) > H+ (0 V), so Au will not be oxidized. - Mg (-2.37 V) < H+ (0 V), so Mg will be oxidized. - Cu (+0.34 V) > H+ (0 V), so Cu will not be oxidized. - F- (+2.87 V) > H+ (0 V), so F- will not be oxidized.

Choose the Species that will be Oxidized

Based on the comparison of reduction potentials in Step 2, the species that will be oxidized by 1 M HCl is Mg (b).