Answer to Question #207528 in General Chemistry for ACYY

Question

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.. In this experiment, The common ion affects the solubility of the compound in a solution. For example, Ca(OH)2 dissociate into Ca2+ and OH− ions as follows; If Ca(OH)2 is added to a saturated solution of CaCl2 , the reaction shifts to the left to relieve the stress produced by the additional Ca2+ ion, in accordance with Le Châtelier’s principle. In quantitative terms, the added Ca2+ causes the reaction quotient to be larger than the solubility product (Q > Ksp), and Ca(OH)2 forms until the reaction quotient again equals Ksp. At the new equilibrium, [OH–] is less and [Ca2+] is greater than in the solution of Ca(OH)2 in pure water.

It this correctly explain about common ion effect on solubility?

Answer 1

Answer:-

We know that the, If we have the solution , the solute at the equilibrium position and adding a common ion , that decreases the solubility of the solute , As this happens because Le Chatelier's principle states the reaction will shift toward the left that is toward the reactants to relieve the stress on the excess product side .