- #1
lkh1986
- 96
- 0
When a metal displaces hydrogen from a non-oxidizing strong acid, which substance is the oxidizing agent? Thanks 
Oxidizing Agent in Metal-Hydrogen Acid Reactions
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Discussion Overview
The discussion revolves around identifying the oxidizing agent in metal-hydrogen acid reactions, particularly when a metal displaces hydrogen from a non-oxidizing strong acid. Participants explore examples, definitions, and the underlying principles of oxidation and reduction.
Discussion Character
- Exploratory
- Technical explanation
- Conceptual clarification
- Debate/contested
Main Points Raised
- Some participants suggest that to determine the oxidizing agent, one should consider specific examples, such as copper and sulfuric acid.
- It is noted that copper does not react with sulfuric acid at room temperature, and only reacts under certain conditions, which complicates its role as an oxidizing agent.
- Another example provided is zinc reacting with hydrochloric acid, where zinc is oxidized and hydrogen is reduced, leading to the conclusion that hydrogen acts as the oxidizing agent in this case.
- Some participants express uncertainty about the definitions of oxidation, reduction, oxidizing agents, and reducing agents, indicating a need for clarification on these concepts.
- There is mention of the activity series, with a distinction made between non-oxidizing and oxidizing acids, particularly regarding their reactions with different metals.
Areas of Agreement / Disagreement
Participants do not reach a consensus on the identity of the oxidizing agent, as different examples and interpretations are presented, leading to multiple competing views on the topic.
Contextual Notes
Some limitations include varying definitions of oxidizing and reducing agents, the conditions under which metals react with acids, and the dependence on the activity series of metals.
- #2
User Name
- 19
- 0
lkh1986 said:When a metal displaces hydrogen from a non-oxidizing strong acid, which substance is the oxidizing agent? Thanks
To first solve this problem, you should try and come up with an example equation.
For example: Copper and Sulfuric Acid.
So when the ions "split apart", you have hydrogen ions and copper metal, so there's only one way each of those elements could be oxidized/reduced.
And remember, an oxidizing agent is personally being reduced.
(Technically, copper sucks as an example since there's two ways it can be changed... but I hope I got my point across)
- #3
Cesium
- 273
- 0
User Name said:
Copper does not react with sulfuric acid at room temperature. Only in the hot concentrated acid does it react and under these conditions sulfuric acid is a sufficient oxidizing agent.
lkh1986 said:
Take the example of Zn and HCl.
Zn + HCl --> ZnCl2 + H2
Zn has an oxidation number of 0 in Zn and oxidation number of +2 in ZnCl2. Because it is moving to a more positive state, it is being oxidized. Therefore zinc is the reducing agent. H has an oxidization number of +1 in HCl and an oxidation number of 0 in H2. Because it is moving to a more negative state, it is being reduced. Therefore, it is the oxidizing agent.
If are you uncertain as to how to calculate oxidation numbers, your textbook is sure to explain it.
Hydrochloric acid may be labeled as a "non-oxidizing acid" but this is just in regards to the more noble metals that are below hydrogen in the activity series like copper. When it reacts with a more active metal, it is indeed the oxidizing agent. Nitric acid is considered an "oxidizing acid" because it has the peculiar ability to react with some metals that are below hydrogen in the activity series.
- #4
sdekivit
- 91
- 0
lkh1986 said:When a metal displaces hydrogen from a non-oxidizing strong acid, which substance is the oxidizing agent? Thanks
i think the problem here is: what means oxidation and reduction and what does an oxidizing agent and a reducing agent.
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