Answer:
a. H₂O (conjugate acid) ; b. OH⁻ (conjugate base), H₃O⁺ (conjugate acid) ; c. H₂CO₃ (conjugate acid), CO₃⁻² (conjugate base) ; d. NH₄⁺ (conjugate strong acid) e. H₂SO₄ (conjugate acid), SO₄⁻² (conjugate base) ; f. No conjugate acid either base; g. H₂S (conjugate acid), S⁻² (conjugate base);
h. H₄N₂ (conjugate base)
Explanation:
a. OH⁻ + H⁺ ⇄ H₂O
The hydroxide acts like a Bronsted Lory base, so it can catch a proton. Water will be the conjugate acid.
b. H₂O, is an amphoterus compound. It can act as an acid or a base. If it is a base, the conjugate acid is the H₃O⁺. If it is an acid, the conjugate base is the OH⁻.
c. HCO₃⁻ + H⁺ ⇄ H₂CO₃
HCO₃⁻ + H₂O ⇄ CO₃⁻² + H₃O⁺
The bicarbonate is also amphoteric. When it catches the proton, the carbonic acid is the conjugate acid, cause it works as a base.
When the HCO₃⁻ (acid) release the proton, the conjugate base is the carbonate.
d. Ammonia is a weak base, so the conjugate strong acid is the ammonium.
NH₃ + H₂O ⇄ NH₄⁺ + OH⁻
e. Another amphoteric compound. The acid sulfate acts an acid and a base.
(like bicarbonate). When it is a base, the conjugate acid is the sulfuric acid, when it is an acid, the conjugate base is the sulfate.
HSO₄⁻ + H₂O ⇄ SO₄⁻² + H₃O⁺
HSO₄⁻ + H⁺ ⇄ H₂SO₄
f. H₂O₂ does not recieve H⁺ or OH⁻, and it does not release H⁺. It is a neutral compound and it doesn't act as a base or acid.
g. HS⁻ is amphoterous.
HS⁻ + H⁺ ⇄ H₂S
HS⁻ + H₂O ⇄ S⁻² + H₃O⁺
Same case as bicarbonate or acid sulfate.
h. H₅N₂⁺ + H₂O ⇄ H₄N₂ + H₃O⁺
Hidrazinium acts an acid, so, the conjugate base will be the hidrazine.
