✔ 最佳答案
1) Normally, if metal is added to a dilute acid (eg HCl or H2SO4), the reaction is:
M + H+ → M+ + H2
However, the case is different in HNO3.
For very dilute HNO3 (0.1 M), the equation is the same as above.
For bench dilute HNO3 (2 M), though, the reaction becomes:
M + HNO3 → M+ + NO + H2O
As you see, HNO3 has become an oxidising agent.
2) We study acids first by learning the most general properties of them.
Since bench dilute HNO3 does not show the usual property the other acids does towards metals (see above), HNO3 is often discussed separately.
3) Some acids, when in a high concentration, tend to attract electrons readily. This way they have become oxidising agents. You may find that some acids actually appear in the Electrochemical Series. As this differs from the usual acid properties, this is not discussed.
Also, carrying out this reaction can be extremely dangerous, as concentrated acids are corrosive.
4) M + conc. H2SO4 → M+ + SO2 + H2O
M + conc. HNO3 → M+ + NO2 + H2O
Conc. HCl, being non-oxidising, behaves the same as dilute HCl.
Hope these help you.
參考: I recalled these from my F5 Chemistry book. Hope there aren't any mistakes.