Chapter 4: Problem 123
Hydrochloric acid is not an oxidizing agent in the sense that sulfuric acid and nitric acid are. Explain why the chloride ion is not a strong oxidizing agent like \(\mathrm{SO}_{4}^{2-}\) and \(\mathrm{NO}_{3}^{-}\).
Short Answer
Step by step solution
Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Chloride Ion
- It cannot easily accept electrons from other species.
- Its electron-rich state keeps it stable, reducing its reactivity as an oxidizer.
Sulfate Ion
- Presence in a higher oxidation state.
- Potential to accept electrons and reduce to lower oxidation states.
Nitrate Ion
- It is capable of moving from a higher to lower oxidation state.
- This transition involves accepting electrons, which facilitates oxidation reactions.
Chemical Reactions
- Electron transfer, where oxidizing agents gain electrons.
- Balancing of reactants and products, calculated by assessing oxidation state changes.
Oxidation States
- Chlorine in \(\mathrm{Cl}^{-}\) is in a low oxidation state, making it unreceptive to further electron gain.
- Sulfur in \(\mathrm{SO}_{4}^{2-}\) and nitrogen in \(\mathrm{NO}_{3}^{-}\) have higher oxidation states, conducive to electron acceptance.