At the new equilibrium, is less and is greater than in the solution of Ca(OH)2 in pure water. 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. 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 this experiment, The common ion affects the solubility of the compound in a solution. This behaviour is a consequence of Le Chatelier’s principle for the equilibrium reaction of the ionic association/dissociation. 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.
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