The addition of NaCI to AgCI decreases the solubility of AgCl
Correct answer: C. due to the common ion effect of Cl-
- A. as solubility product decreases
- B. as solubility becomes unsaturated
- C. due to the common ion effect of Cl-
- D. as solution becomes supersaturated
Explanation
In the case of the common ion effect, the presence of a common ion (Cl-) in the solution decreases the solubility or ionization of the compound (AgCl) by shifting the equilibrium toward the formation of the undissociated or unionized form. This occurs because the common ion is already present in the solution and its addition (by adding compound NaCl) reduces the need for the compound to dissociate or dissolve further.
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About Chemical Equilibrium
Reversible reactions reach dynamic equilibrium when forward and reverse rates become equal, and Le Chatelier's principle predicts the effect of changing concentration, pressure or temperature. The chapter also covers solubility product, the common ion effect, buffer action and the conditions used in Haber's process, with equilibrium shifts distinguished from changes in the equilibrium constant.
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