Question

Consider the reaction below.

Answer 1

Answer: $HI$ and $I^-$

Explanation:

According to the Bronsted-Lowry conjugate acid-base theory, an acid is defined as a substance which looses donates protons and thus forming conjugate base and a base is defined as a substance which accepts protons and thus forming conjugate acid.

For the given chemical equation:

$HI+H_2O\rightarrow H_3O^++I^-$

Here, $HI$ is loosing a proton, thus it is considered as an acid and after losing a proton, it forms $I^-$ which is a conjugate base.

And, $H_2O$ is gaining a proton, thus it is considered as a base and after gaining a proton, it forms $H_3O^+$ which is a conjugate acid.

Hence, the correct answer is D.