Answer:
Option A is correct.
The two Brönsted Lowry bases are NH₃ and HS⁻.
Explanation:
In any neutralization reaction or any reaction that seems like a neutralization reaction, the Bronsted Lowry Acid is the specie that donates a proton in reaction, the base is the specie that accepts the donated proton in the reaction.
The acid, after donating the proton becomes the conjugate base, and the base after receiving the proton becomes a specie known as the conjugate acid.
In this reaction, H₂S (acid) loses a proton to NH₃ (base) to form a HS⁻ (conjugate base) and NH₄⁺ (conjugate acid).
In a backward reaction, the conjugate acid and conjugate base form the acid and base pair respectively as required.
Hence, the two two Brönsted-Lowry bases are NH₃ and HS⁻.
Hope this Helps!!!
Answer:
A) NH3 and HS-
Explanation:
A Bronsted-Lowry base is a substance that accepts protons.
The ammonia is a Bronsted-Lowry base because can accept a proton from the hydrogen of H2S to become NH4+.
The HS⁻ is the Brønsted-Lowry base too because it has one more H atom. It has accepted a proton (H⁺), so it is a Brønsted-Lowry base.
