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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 :

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.

[tex]HA+H_2O\rightarrow A^-+H_3O^+[/tex]

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

[tex]H_2O[/tex] = Base

[tex]A^-[/tex] = Conjugate base

[tex]H_3O^+[/tex] = Conjugate acid

For example:

[tex]H_2SO_4+2H_2O\rightarrow SO_4^{2-}+2H_3O^+[/tex]

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

Sulfuric acid  = Acid

[tex]H_2O[/tex] = Base

[tex]SO_^{2-}[/tex] = Conjugate base

[tex]H_3O^+[/tex] = Conjugate acid

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