Equilibrium sign

[Riya Sood 4G]

Do we add the equilibrium sign if we are writing the dissociation of a strong acid/strong base ?

[Sarah Nichols 4C]

No, because for strong acids and bases we assume 100% dissociation, so after the reaction there will be no reactants in solution, only products

[Jacob Motawakel]

No, since strong acids and bases are completely dissociated, it is only a one way reaction. Weak acids and bases use the equilibrium sign because the weak acid/base is not completely dissociated, so there are still H+ or OH- ions on the reactant side, as well as some on the products side.

[Rishika Yadav 3D]

No because reactions with strong acids and bases only go in one direction, while reactions with weak acids and bases reach equilibrium and then occur at a constant rate.

[Gerald Bernal1I]

Equilibrium sign is added only for weak acids and bases since they do not dissociate or ionize fully.

[Dominic Benna 2E]

No because there will be theoretically a 100% dissociation of the acid or base.

[Kristina Krivenko 3I]

No, we don't write the equilibrium sign when writing reactions for the dissociation of a strong acid/strong base because the assume that they dissociate completely.

[IanWheeler3F]

The Ka values of strong acids and bases are so large that it can be assumed that there is no back and forth between which species are present, there are just protons and anions.

[Ava Nickman]

No the dissociation is complete and the equilibrium sign does not apply

[Ximeng Guo 2K]

No because we assume that strong acids/bases are completely ionized in water