Give the conjugate base of h2s
The Correct Answer and Explanation is:
Correct Answer: The conjugate base of H₂S is HS⁻ (hydrosulfide ion).
Explanation:
A conjugate base is the species that remains after an acid has donated a proton (H⁺). In this case, hydrogen sulfide (H₂S) is a diprotic acid, meaning it can donate two protons. When it donates one proton, it forms its conjugate base, which is the HS⁻ ion.
To understand how this works, we look at the dissociation reaction of H₂S in water:
H₂S ⇌ H⁺ + HS⁻
In this reaction, H₂S loses one hydrogen ion (proton), resulting in the formation of the hydrosulfide ion (HS⁻). This means HS⁻ is the conjugate base of H₂S, since it is what remains after H₂S gives up a proton.
This process is part of Brønsted–Lowry acid–base theory, where acids are defined as proton donors and bases are proton acceptors. According to this theory, once H₂S donates a proton, it becomes capable of accepting a proton again, so HS⁻ is a base — specifically, a conjugate base.
HS⁻ itself can also act as a weak acid, since it can donate a second proton to form the S²⁻ (sulfide) ion:
HS⁻ ⇌ H⁺ + S²⁻
But in the context of the first proton donation, HS⁻ is the conjugate base of H₂S.
In summary, when H₂S loses one hydrogen ion, it becomes HS⁻, which is its conjugate base. This concept is essential in acid–base chemistry, especially when understanding acid strength, pH, buffer systems, and equilibrium in aqueous solutions.
