McGraw-Hill Education SAT Subject Test Chemistry 4th Ed. by Thomas A. Evangelist

Author:Thomas A. Evangelist
Language: eng
Format: epub
Publisher: McGraw Hill LLC
Published: 2016-01-15T00:00:00+00:00

COMMON ION EFFECT

Consider the chemical equation for AgCl dissolved in water to make a saturated solution: AgCl(s) ←→ Ag1+(aq) + Cl1−(aq). At 298 K the solubility product constant is 1.8 × 10−10, which indicates that is a slightly soluble salt. There is a way of making AgCl even less soluble, via the common ion effect. Consider the following, when an ion that is already present is added to the solution, the equilibrium will shift to consume the increase in concentration of the ion.

If NaCl(aq) were added to a solution of silver chloride, the NaCl would introduce more Cl1− ions and shift the equilibrium to the left. This would favor the production of more AgCl(s). Adding the common ion, Cl1−, actually decreases the solubility of AgCl by forming more of its solid.

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