Since everyone knows an acid would dissociate(partially or fully) in its aqueous solution and liberate $\ce{H+}$. We also calculate the $\pu{pH}$ of the solution using $[\ce{H+}]$ and this$(\ce{H+})$ is what gives the solution acidity. Now consider we have just got a strong acid i.e pure acid without having any water in it, for example, $\ce{H2SO4}$ and no water in it, would the sulphuric acid dissociate in this case i.e without the aid of water? If it does not dissociate would this substance be acidic, since there would be no $\ce{H+}$ in that case?

• Depends on the definition of acid that you use - en.wikipedia.org/wiki/Acid#Definitions_and_concepts Undissociated H2SO4 isn't an Arrhenius acid (unless you count the tiny amount of self-ionisation), but it is still a Bronsted acid Jul 15 '17 at 10:53
• I think if we had FAQ section or sth like that, this topic would be there. Jul 15 '17 at 14:10
• @Mithoron Excuse me, my question is different. Jul 15 '17 at 14:47
• chemistry.stackexchange.com/questions/53580/… Jul 15 '17 at 14:49

Not really. Like lots of things with polar bonds, sulfuric acid can undergo ion transfer reactions in the liquid and make ionic species in solution. And it is indeed protons that get transferred just like water. But as with water, at least under ordinary conditions, these ionic species are only a minor portion of the liquid which is mostly $\ce{H2SO4}$ molecules.
First of all, sulfuric acid is just hydrated sulfur trioxide ($\ce{SO3}$). Sulfur trioxide is obviously not an Arrhenius acid, but it is Lewis acidic.