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

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