What experimental procedure could you use to confirm that aqueous sulfuric acid consists of ions, not uncharge

Question

(continue from the question) not uncharged molecules, as a result of the reaction between the acid molecules and water molecules?

Answer 1

One experiment you can conduct is to get some pH paper and measure the pH of water before and after adding sulfuric acid.

Since the pH of the solution will be lower than seven this will actually mean that there is a higher concentration of hydronium ion (a charged molecule) because of the acid dissociation, you can deduce that there are charges involved because if there is a positive charge somewhere in your system then there has to be a negative charge to balance it.

This is how it works..
Initially water will have an equal concentration of hydronium and hydroxide ions which can be seen with the auto dissociation of water:
2H2O ---> H3O(+) + OH(-)
Thus, the number of moles of H3O(+) equals the number of moles of OH-. (This is why water has a pH of 7)

However, when you add sulfuric acid to water you will have:
H2SO4 + 2H2O ---> 2H3O(+) + SO4(2-) (a higher concentration of hydronium ions will bring the pH below 7)

Ultimately, you can see there are two moles of positively charged hydronium ions produced in this reaction. Once again, you can immediately confirm that aqueous sulfuric acid consists of ions and not uncharged particles. Once again if you think about charge balance there has to be a negatively charged ion which in fact is the sulphate ion (2-).

Answer 2

you could measure the conductivity of the solution i suppose, before and after adding sulfuric acid to water.