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Sulfuric acid is a strong acid so it should fully dissociate into h+ ions and HSO4- ions leaving behind no H2SO4 molecules. But some chemistry mechanisms actually show an entire h2so4 molecule reacting. is that correct
Accepted Answer
In aqueous solutions, sulfuric acid (H2SO4) undergoes a stepwise dissociation process rather than fully dissociating into H+ and HSO4- ions. While it is a strong acid and predominantly dissociates, a small equilibrium concentration of undissociated H2SO4 molecules remains in solution. This is because the second dissociation step, where HSO4- dissociates further to form H+ and SO42-, is not complete. Therefore, it is possible for entire H2SO4 molecules to participate in certain chemical reactions, especially in non-aqueous solvents or under specific experimental conditions where the equilibrium is shifted towards the undissociated form.
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