I know for a fact that dilute $\ce{H2SO4}$ is a non-oxidizing acid which makes it a reducing agent. I also know for a fact that $\ce{PbO2}$ is a strong oxidizing agent. So, I thought Redox reaction should have occurred between them, but my teacher says that no reaction occurs between the said reactants because $\ce{PbO2}$ does not react with low concentration of acid. If it were so, why does $\ce{PbO2}$ react with dilute $\ce{HCl}$. Since, both dilute $\ce{HCl}$ and dilute H2SO4 are reducing acids of low concentrations, both should be eligible for the Redox reaction.

I have tried this on the internet but all I get are reaction balancing links .JD Lee's Concise Inorganic Chemistry has nothing about this also.


YOur logic is wrong.

I know for a fact that dilute $\ce{H2SO4}$ is a non-oxidizing acid...

sort of, but so far so good.

...which makes it a reducing agent.

This is where you are wrong, just because it is non-oxidizing does not make it reducing. Concentrated $\ce{H2SO4}$ is an oxidizer, diluting it does not make it less of an oxidizer, but limits the strength/mechanism.

A similar example is mixing nitroglycerin and diatomaceous earth doesn't make nitroglycerin less explosive, it just makes it harder for it to explode (dynamite).

  • $\begingroup$ So, what you mean is dilute sulfuric acid is still an oxidizing acid but its capacity has been diluted to the point that it cannot oxidize appreciably anymore. $\endgroup$ – Lucifer - Nov 14 '18 at 5:42
  • $\begingroup$ @Lucifer - Yes. $\endgroup$ – A.K. Nov 14 '18 at 14:07

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