Solubility Equilibrium-Common ion effect
Department of Pure and Applied Chemistry
College of Arts and Sciences
Visayas State University
Name: Almera P. Padolina Course & Year: BS Chem 2
Date Performed: July 24, 2012 Date Submitted: August 6, 2012
Experiment No. 4
Solubility Equilibrium- Common Ion Effect
INTRODUCTION:
The common ion effect is another example of Le Châtelier 's Principle in action.The common ion effect tells us that the solubility of an ionic compound is decreased by the addition to the solution of another ionic compound that contains one of the ions involved in the solution It is also responsible for the reduction in solubility of an ionic precipitate when a soluble compound combining one of the ions of the precipitate is added to the solution in equilibrium with the precipitate. It may be confusing, but an example should help clarify.If we have a barium sulfate solution, the solid salt is in equilibrium with its ions:
If we then add solid barium chloride to this solution, which dissolves to produce Ba2+ and Cl- ions, we are increasing the concentration of Ba2+ ions in our solution. (The new Cl- ions will remain in solution as spectator ions). Ba2+ is the ion common to both solutions. Le Châtelier 's Principle tells us that if the concentration of one of the reaction participants is increased, then equilibrium will shift to use up the additional substance. So adding more Ba2+ will force the equilibrium to shift to the left (the reverse direction) in order to use up the added Ba2+ ions, producing more solid BaSO4. The concentration of SO42- will decrease, indicating that solubility has decreased. In this experiment, the groups will learn the equilibria which concerns more on a saturated solutions of ammonium chloride, which exists in equilibrium with ammonia, consequently ammonium ion is a weak acid and ammonia is a weak base.
OBJECTIVE: To know the effects of adding solutions of strong acid,
College of Arts and Sciences
Visayas State University
Name: Almera P. Padolina Course & Year: BS Chem 2
Date Performed: July 24, 2012 Date Submitted: August 6, 2012
Experiment No. 4
Solubility Equilibrium- Common Ion Effect
INTRODUCTION:
The common ion effect is another example of Le Châtelier 's Principle in action.The common ion effect tells us that the solubility of an ionic compound is decreased by the addition to the solution of another ionic compound that contains one of the ions involved in the solution It is also responsible for the reduction in solubility of an ionic precipitate when a soluble compound combining one of the ions of the precipitate is added to the solution in equilibrium with the precipitate. It may be confusing, but an example should help clarify.If we have a barium sulfate solution, the solid salt is in equilibrium with its ions:
If we then add solid barium chloride to this solution, which dissolves to produce Ba2+ and Cl- ions, we are increasing the concentration of Ba2+ ions in our solution. (The new Cl- ions will remain in solution as spectator ions). Ba2+ is the ion common to both solutions. Le Châtelier 's Principle tells us that if the concentration of one of the reaction participants is increased, then equilibrium will shift to use up the additional substance. So adding more Ba2+ will force the equilibrium to shift to the left (the reverse direction) in order to use up the added Ba2+ ions, producing more solid BaSO4. The concentration of SO42- will decrease, indicating that solubility has decreased. In this experiment, the groups will learn the equilibria which concerns more on a saturated solutions of ammonium chloride, which exists in equilibrium with ammonia, consequently ammonium ion is a weak acid and ammonia is a weak base.
OBJECTIVE: To know the effects of adding solutions of strong acid,
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