Question

Given a chemical equation, showing the dissociation of an acid in solution, be able to identify the "acid", the "base", the "conjugate acid", and the "conjugate base"

Answer 1

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

`HA+H_2O\rightarrow A^-+H_3O^+`

Suppose acid Ha is getting dissociated in its solution and after dissociation it donates its proton to water molecule and forms conjugate base. Where as water (acting as a base) accepts protons and forms conjugate acid.

HA = Acid

`H_2O` = Base

`A^-` = Conjugate base

`H_3O^+` = Conjugate acid

For example:

`H_2SO_4+2H_2O\rightarrow SO_4^(2-)+2H_3O^+`

Sulfuric acid dissociating in its solution to form conjugate base and conjugate acid.

Sulfuric acid = Acid

`H_2O` = Base

`SO_^(2-)` = Conjugate base

`H_3O^+` = Conjugate acid