Con. and dil. HCl,HNO3,H2SO4 's chemical properties

Let's separately look at each acid first:
1) Hydrochloric acid (HCl)
Looking at the anion Cl-, this is rather a stable ion that it won't discharge under usual conditions. So to speak, the property exhibited by HCl is mainly the acidity and also it is not a strong oxidizing agent at all concentrations since H+ is not a strong oxidizing agent.
So conclusively, HCl can only react with those metals below H in the E.C.S. (ElectroChemical Series).
2) Nitric acid (HNO3)
Looking at the anion NO3-, it is a quite strong oxidizing agent according to its position in the E.C.S.
Therefore, HNO3 also shows an oxidizing property unless at a very low concentration (0.1M). In other words, very dilute HNO3 is an acid but not a strong oxidizing agent.
At usual low concentration, say 1M, HNO3 can react with metal lower than H in the E.C.S. (e.g. Cu) since in this case, oxidizing property predominates over the acidic property and the copper metal is being corroded as a result of redox reaction but not reaction of acids:
3Cu(s) + 8HNO3(aq) → 3Cu(NO3)2(aq) + 2NO(g) + 4H2O(l)
The nitrogen monoxide gas formed (NO, colourless) readily combines with oxygen in the atmosphere to give brown fumes nitrogen dioxide (NO2):
2NO(g) + O2(g) → NO2(g)
Also dil. HNO3 can react with non-metals like carbon by its oxidizing property:
3C(s) + 4HNO3(aq) → 3CO2(aq) + 4NO(g) + 2H2O(l)
At high concentration (≧2M), HNO3 is even a stronger oxidizing agent that upon reacting with metals, brown NO2 fumes are evolved directly:
Cu(s) + 4HNO3(aq) → Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l)
Similarly it can also react with carbon:
C(s) + 4HNO3(aq) → CO2(aq) + 4NO2(g) + 2H2O(l)
3) Sulphuric acid (H2SO4)
Looking at the anion SO42-, it is a strong oxidizing agent when in high concentrations (98% by mass, which makes up to about 18M)
Therefore, H2SO4 shows an oxidizing property at high concentrations. For low concentrations of it (≦1M, say), it is an ordinary acid and does not have other properties of concentrated one like oxdizing, dehydrating and involatility.
Similar to conc. HNO3, conc. H2SO4 can also react with metal lower than H in the E.C.S. (e.g. Cu), giving off a choking, colourless and pungent smell sulphur dioxide gas (SO2):
Cu(s) + 2H2SO4(aq) → Cu(SO4)(aq) + SO2(g) + 2H2O(l)
And with carbon/sulphur:
C(s) + 2H2SO4(aq) → CO2(g) + 2SO2(g) + 2H2O(l)
S(s) + 2H2SO4(aq) → 3SO2(g) + 3H2O(l)
In addition to oxidizing property, conc. H2SO4 also has the following properties:
(a) Dehydrating
Those compounds with H and O in a ratio of 2:1 in their molecules are readily extracted by H2SO4. Examples include glucose (C6H12O6), ethanol (C2H5OH) and hydrated copper(II) sulphate (CuSO4.5H2O):
C6H12O6(s) → C(s) + 6H2O(l)
C2H5OH(l) → C2H4(g) + H2O(l)
CuSO4.5H2O(s) → CuSO4(s) + 5H2O(l)
(b) Involatility
Meaning that it can displace the anion of other acid to form a sulphate salt and the acid of the displaced ion, say displacing nitrate to give nitric acid:
H2SO4(aq) + 2NaNO3(aq) → Na2SO4(aq) + 2HNO3(aq)