Question

How are Bronsted lowry acid and bases defined?

Answer 1

A Brønsted-Lowry acid is any substance (molecule or ion) that can donate a hydrogen ion (`H^(+)`).

A Brønsted-Lowry base is any species that can accept a hydrogen ion (`H^(+)`).

Explanation:

In short, acids have the ability to donate protons and bases have the ability to accept protons.

Take the following reaction for example:

`H_2SO_4 + NH_3 rightleftharpoons NH_4^(+) + HSO_4^(-)`

Sulfuric acid (`H_2SO_4`) is the Brønsted-Lowry acid because it donates a hydrogen ion. Ammonia (`NH_3`) is the Brønsted-Lowry base because it accepts the hydrogen ion.

The Brønsted-Lowry theory also introduces the concept of conjugate acid-base pairs. A conjugate acid-base pair are two species that differ by a (`H^(+)`) ion.

Based on the reaction above, the ammonium ion
(`NH_4^(+)`) is the conjugate acid of the base ammonia and the hydrogen sulfate ion (`HSO_4^(-)`) is the conjugate base of sulfuric acid.

Here's a tip to let you know which substance is the conjugate acid and which substance is the conjugate base:

A conjugate base has one less (`H^(+)`) proton than the acid you started with.

A conjugate acid has one more (`H^(+)`) proton than the base you started with.

Here's general depiction of conjugate acid-base pairs:

`HA` represents an acid

`B` represents a base

`A^(-)` represents the conjugate base since this substance has one less proton than the acid, HA.

`HB^(+)` represents the conjugate acid since this substance has one more proton than the base, B.

I really hope this makes sense!