Final answer:
Sulfuric acid, H2SO4, dissolves in water and produces ions due to its ability to undergo ionization; it effectively releases protons forming hydronium and sulfate ions, which interact with water molecules. This process enables electrical conductivity in the solution, distinguishing sulfuric acid from covalent compounds that do not ionize in water.
Step-by-step explanation:
Sulfuric acid, H2SO4, is a diprotic acid that dissolves in water, despite being a covalent molecule because it can undergo ionization. When H2SO4 dissolves in water, it releases two protons (H+ ions) successively. The first proton is released easily because H2SO4 is a strong acid in this respect, forming the hydronium ion (H3O+) and the hydrogen sulfate ion (HSO4−).
The second proton can be released forming sulfate ion (SO4²−), though to a lesser degree, as sulfuric acid is a weak acid when donating the second proton. Moreover, the solvation process when sulfuric acid dissolves in water involves the attraction between these ions and the polar water molecules, which facilitates the dissociation into ions.
Such ionization is crucial for electrical conductivity in aqueous solutions. While sulfuric acid is an example of a strong acid that ionizes completely at the first stage, not all acids behave the same way. For instance, acetic acid (CH3CO2H) largely remains as neutral molecules in solution, with less than 1% dissociating into ions.
It is also important to note that sulfuric acid's ability to ionize makes it distinct among other covalent substances that do not produce ions in solution. This ability to form ions in water is why a solution of sulfuric acid can conduct electricity, contrasting with non-ionizing covalent compounds.