Common ion effect on solubility

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. 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 statement correctly explain common ion effect against solubility? and how to explain well?