Respuesta :
Answer:
Explanation has been given below.
Explanation:
Let's consider solubility equilibrium of an ionic insoluble compound e.g. [tex]BaSO_{4}[/tex]
[tex]BaSO_{4}\rightleftharpoons Ba^{2+}+SO_{4}^{2-}[/tex]
Equilibrium constant of this solubility equilibrium is represented in terms of solubility product ([tex]K_{sp}[/tex]) which is expressed as-
[tex]K_{sp}=[Ba^{2+}][SO_{4}^{2-}][/tex]
Now, if we add an ionic salt e.g. [tex]Na_{2}SO_{4}[/tex] with a common ion [tex]SO_{4}^{2-}[/tex] then concentration of [tex]SO_{4}^{2-}[/tex] increases.
But, at a constant temperature, [tex]K_{sp}[/tex] is constant.
Therefore, to keep [tex]K_{sp}[/tex] constant, excess amount of [tex]SO_{4}^{2-}[/tex] will combine with free [tex]Ba^{2+}[/tex] ion in solution and produce [tex]BaSO_{4}[/tex].
Hence, as a whole, solubility of [tex]BaSO_{4}[/tex] decreases.
