The dissociation or ionization of a weak electrolyte is suppressed by the addition of strong electrolyte containing one of the same ions of weak electrolyte is called as
The correct answer and explanation is:
The phenomenon described is known as the common ion effect.
When a weak electrolyte is dissolved in water, it only partially dissociates into ions. The dissociation equilibrium for a weak electrolyte can be represented as follows: HA (aq)⇌H+(aq)+A−(aq)\text{HA (aq)} \rightleftharpoons \text{H}^+ (\text{aq}) + \text{A}^- (\text{aq})
Where HA is the weak electrolyte, and H⁺ and A⁻ are the ions it dissociates into. The dissociation of weak electrolytes is governed by an equilibrium constant known as the ionization constant (Kₐ). When a strong electrolyte, such as NaA, which provides the common ion A⁻, is added to the solution, the concentration of the ion A⁻ increases significantly.
According to Le Chatelier’s principle, the system will try to counteract this disturbance by shifting the equilibrium to the left, decreasing the dissociation of the weak electrolyte HA. As a result, fewer H⁺ and A⁻ ions are produced from the weak electrolyte, and the degree of dissociation is reduced.
This suppression of ionization is due to the presence of a large concentration of one of the ions from the weak electrolyte, thus reducing its tendency to dissociate further. The common ion effect is particularly important in buffer solutions, where the concentration of a weak acid and its conjugate base (or weak base and its conjugate acid) is deliberately controlled to maintain a stable pH.
The practical implications of the common ion effect can be observed in various chemical processes, such as in the solubility of salts, acid-base equilibria, and even in biological systems, where ion concentration needs to be finely tuned for proper function.