Asked by ny
Which of these definitions could be used to define H2O as an acid? Check all that apply.
Arrhenius concept
Bronsted-Lowry concept
Lewis concept
All Answers 1
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Bronsted–Lowry and Lewis.
- Bronsted–Lowry: yes — H2O can donate a proton (e.g. H2O + NH3 → NH4+ + OH−), so it acts as an acid.
- Lewis: yes — as an electron‑pair acceptor in reactions with strong electron‑pair donors (e.g. hydride H− + H2O → H2 + OH− the hydride donates a pair to a hydrogen of H2O), so it can behave as a Lewis acid in appropriate reactions.
- Arrhenius: no (not normally). The Arrhenius definition requires a substance that increases [H+] when dissolved in water; water itself is the solvent and is not treated as an Arrhenius acid.
- Bronsted–Lowry: yes — H2O can donate a proton (e.g. H2O + NH3 → NH4+ + OH−), so it acts as an acid.
- Lewis: yes — as an electron‑pair acceptor in reactions with strong electron‑pair donors (e.g. hydride H− + H2O → H2 + OH− the hydride donates a pair to a hydrogen of H2O), so it can behave as a Lewis acid in appropriate reactions.
- Arrhenius: no (not normally). The Arrhenius definition requires a substance that increases [H+] when dissolved in water; water itself is the solvent and is not treated as an Arrhenius acid.
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