Question

solution of silver chloride at constant temperature: AgCl(s) ↔ Ag+(aq) + Cl-(aq) As NaCl(s) is dissolved in the solution, the concentration of the Ag+ ions in the solution 1. decreases, and the concentration of Cl- ions increases 2. decreases, and the concentration of Cl- ions remains the same 3. increases, and the concentration of Cl- ions increases 4. increases, and the concentration of Cl- ions remains the same

Answer 1

As a matter of fact, NaCl(s), when dissolves in water, dissociates into ion Na+ and Cl-.

There is water in the silver chloride solution. Therefore, when being added to the solution, NaCl dissociates into Na+ and Cl-, which makes the concentration of Cl- in the solution increase.

According to Le Chatelier's Principle, when [Cl-] increases, the chemical equation seems to shift in a way that could make more AgCl. Therefore, Ag+ has to react with Cl-, which makes [Ag+] decrease.

The correct answer is (1).

Hope this helps~