In the reversible reaction in water solution nh3 + h2o ⇀↽ nh + 4 + oh -, what acts as a bronsted-lowry acid and what acts as a bronsted-lowry base? 1. oh-; h2o 2. h2o; oh - 3. h2o; nh + 4 4. oh-; nh + 4 5. nh3; h2o

The equation is:

NH₃ + H₂O ↔ NH₄⁺ + OH⁻

base acid conj. acid conj. base

NH₃ is the proton acceptor so it considered as Bronsted-Lowry base and H₂O is proton donor so it considered as Bronsted-Lowry acid

NH₃ when accepted H⁺ it converted into NH₄⁺ (conjugate acid) and H₂O when losing H⁺ it converted into OH⁻ (conjugate base)

The question asks for acid and base

1) OH⁻ base, H₂O acid

2) H₂O acid, OH⁻ base

3) H₂O acid, NH₄⁺ acid

4) OH⁻ base, NH₄⁺ acid

5) NH₃ base, H₂O acid

so the correct answer is 2) because it is the only one containing acid then base