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Calculate ion concentrations involving chemical equilibrium. The common-ion effect is used to describe the effect on an equilibrium when one or more species in the reaction is shared with another reaction. This results in a shifitng of the equilibrium properties.
In chemistry, the common-ion effect refers to the decrease in solubility of an ionic precipitate by the addition to the solution of a soluble compound with an ion in common with the precipitate. [1] This behaviour is a consequence of Le Chatelier's principle for the equilibrium reaction of the ionic association / dissociation.
The common ion effect is an effect that suppresses the ionization of an electrolyte when another electrolyte (which contains an ion which is also present in the first electrolyte, i.e. a common ion) is added. It is considered to be a consequence of Le Chatlier’s principle (or the Equilibrium Law).
The common ion effect is a decrease in the solubility of an ionic compound as a result of the addition of a common ion. Adding calcium ion to the saturated solution of calcium sulfate causes additional \(\ce{CaSO_4}\) to precipitate from the solution, lowering its solubility.
The solubility of an ionic compound is decreased by the presence of a common ion (an ion that is also present in the compound); this is known as the common-ion effect.
Keep going! Check out the next lesson and practice what you’re learning:https://www.khanacademy.org/science/ap-chemistry-beta/x2eef969c74e0d802:equilibrium/x...
We call this the common ion effect. Example #1: AgCl will be dissolved into a solution which is ALREADY 0.0100 M in chloride ion. What is the solubility of AgCl?