Question

HX(aq) + H2O(l) → H3O+(aq) + X−(aq)

Based on the equation, HX would be classified as A) an acid, because it accepts a proton
B) a base, because it accepts a proton. C) a base, because it donates a proton D) an acid, because it donates a proton

Answer 1

The correct answer is option D.

Step-by-step explanation:

According to the Bronsted-Lowry conjugate acid-base theory:

• An acid is defined as a substance which looses donates protons and changes to its conjugate base.
• A base is defined as a substance which accepts protons and changes to its conjugate acid.

For the given chemical equation:

`HX(aq) + H_2O(l) \rightarrow H_3O^+(aq) + X^-(aq)`

In the above reaction ,
`HX` is loosing a proton, thus it is considered as an acid and after losing a proton, it forms
`X^-` 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 option D.