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Secondaire 5 • December 6, 2025

Hello! I do not get Bronsted Lowry theory well. I just get that an acid is H+ donor while a base is a H+ acceptor. My teacher wrote the following on the board but I do not get, are both equation the same? Why is one an equilibirum while the other isnt. I thought its the same . A base accepts H+ in water NH3(base) + H+ -> NH4+ NH3 + H2O <-> NH4+ + OH-

Explanation (1)

Student Explanation

December 6, 2025

Hello there, learning supernova! 😁 We're delighted that you're using Alloprof! You already understand the basic Bronsted–Lowry idea : Acid = H⁺ donor Base = H⁺ acceptor. In the first equation, NH₃ (ammonia) is acting as a base and accepts H⁺. H⁺ is just “given” to NH₃. It's a complete reaction. In the second equation, at equilibrium, NH₃ is still the base. But H⁺ doesn’t exist freely in water. Instead, water donates H⁺ (acting as an acid) and becomes OH⁻. This reaction doesn’t go 100% to products because NH₃ is a weak base. Most ammonia molecules stay as NH₃ in water. That’s why it’s an equilibrium. I suggest this worksheet for your revision.

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