Limitations of Common Ion Effect
Common ion effect is useful in understanding equilibrium in solutions but its affects can depend on various factors like temperature and other external factors. Some of the limitations of Common ion effect are listed below,
- Common ion effect only works with strong electrolytes(where complete dissociation occurs) When weak electrolytes, affects are negligible.
- Common ion effect needs relatively high concentration of ions, as a result in dilute solutions, the changes are negligible.
- Sometimes, In Precipitation reactions, if the ratio of common ion and solution is not appropriate, precipitation will occur without common ion effect.
- Changes in temperature affect ionization and solubility equilibrium.
Common Ion Effect – Definition, Explanation, Examples
Common ion effect is a phenomenon in chemistry that describes the decrease in solubility of a compound when it is dissolved in a solution that already contains one of its constituent ions. This effect occurs due to the principle of chemical equilibrium and Le Chatelier’s principle.
In this article, we will learn in detail about the common ion effect, its impact on solubility, and its validity in the case of acids, bases, and salts. We will also learn its limitations and FAQs based on the common ion effect.