Answer:
The statement is FALSE.
Explanation:
It is known as the ion effect common to the displacement of an ionic equilibrium when the concentration of one of the ions that are involved in said equilibrium changes, due to the presence in the dissolution of a salt that is dissolved in it.
Given the reaction of the dissociation reaction of a weak electrolyte:
AB (s) ⇔ A⁺(aq) + B⁻ (aq)
The equilibrium constant of the reaction is:
[tex]K_{ps}=\frac{[A^+][B^-]}{[AB]}[/tex]
Given the reaction of the dissociation reaction of a stong electrolyte:
CB (s) ⇒ C⁺(aq) + B⁻ (aq)
If the electrolyte CB is added to the medium in which electrolyte AB is found, the medium will have a common ion B⁻:
AB (s) ⇔ A⁺(aq) + B⁻ (aq)
CB (s) ⇒ C⁺(aq) + B⁻ (aq)
By the Le Chatelier's principle, having more concentration of products, the balance will shift to the right.
Hence, the extent of ionization of a weak electrolyte is decreased by adding to the solution a strong electrolyte that has an ion in common with the weak electrolyte.
