![]() We can compare numerical values of Q with K sp to predict whether precipitation will occur, as shows. If the concentrations are such that Q is less than K sp, then the solution is not saturated and no precipitate will form. A saturated solution in equilibrium with the undissolved solid will result. The reaction shifts to the left and the concentrations of the ions are reduced by formation of the solid until the value of Q equals K sp. We want the calcium carbonate in a chewable antacid to dissolve because the \(\) ions are such that Q is greater than K sp for the mixture. On the other hand, sometimes we want a substance to dissolve. Preventing the dissolution prevents the decay. The dissolution process is aided when bacteria in our mouths feast on the sugars in our diets to produce lactic acid, which reacts with the hydroxide ions in the calcium hydroxylapatite. Tooth decay, for example, occurs when the calcium hydroxylapatite, which has the formula Ca 5(PO 4) 3(OH), in our teeth dissolves. The preservation of medical laboratory blood samples, mining of sea water for magnesium, formulation of over-the-counter medicines such as Milk of Magnesia and antacids, and treating the presence of hard water in your home’s water supply are just a few of the many tasks that involve controlling the equilibrium between a slightly soluble ionic solid and an aqueous solution of its ions.ĭissolution from occurring. ![]() Carry out equilibrium computations involving solubility, equilibrium expressions, and solute concentrations.Write chemical equations and equilibrium expressions representing solubility equilibria.By the end of this section, you will be able to:
0 Comments
Leave a Reply. |
AuthorWrite something about yourself. No need to be fancy, just an overview. ArchivesCategories |