BogMonkey said:Sulphuric acid is a diprotic acid that dissociates completely when dissolved in water.
How does a monoprotic acid like trifluoromethanesulfonic acid produce a greater pH change than H2SO4?
A strong acid is defined as an acid that completely dissociates in water, meaning that all of the acid molecules break apart into ions. This results in a high concentration of H+ ions in the solution, making it a powerful proton donor.
The strength of a strong acid is measured by its acid dissociation constant (Ka) or its pH level. A low Ka or a high pH indicates a strong acid, while a high Ka or a low pH indicates a weak acid.
Some common examples of strong acids include hydrochloric acid (HCl), sulfuric acid (H2SO4), and nitric acid (HNO3).
Strong acids have several distinct properties, including high reactivity, the ability to corrode metals, and the ability to conduct electricity in solution. They also have a sour taste and can cause burns on skin and tissue.
Strong acids differ from weak acids in their ability to dissociate completely in water. Weak acids only partially dissociate, resulting in a lower concentration of H+ ions in solution. This means that strong acids have a higher acidity and are more reactive than weak acids.