Question

The Bronsted-Lowry definition of acids and bases refers to the transfer of a "proton" from the acid to the base; however, the symbol for a proton (p+) is not generally used in this context. What is the chemical symbol that is commonly used to represent a "proton" in the context of Bronsted-Lowry acids and bases?

Answer 1

Answer:
`H^+`

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 thus forming conjugate base and a base is defined as a substance which accepts protons and thus forming conjugate acid.

Example: For the given chemical equation:

`H_3BO_3(aq.)+HS^-(aq.)\rightarrow H_2BO_3^-(aq.)+H_2S(aq.)`

Here,
`H_3BO_3` is loosing a proton, thus it is considered as an acid and after losing a proton, it forms
`H_2BO_3^-` which is a conjugate base.

And,
`HS^-` is gaining a proton, thus it is considered as a base and after gaining a proton, it forms
`H_2S` which is a conjugate acid.

Thus the chemical symbol that is commonly used to represent a "proton" in the context of Bronsted-Lowry acids and bases is
`H^+`