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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

Respuesta :

Billymkhoi
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~

If in the silver chloride solution we add NaCl then concentration of silver ions decreases, and the concentration of Chloride ions increases.

What is equilibrium law?

According to this law, when any external stress is applied in the equilibrium state then the reaction will shift on those side where the stress will reduces.

If in the silver chloride solutions then in the solution silver and chloride ions are present, and then when we add sodium chloride to that solution then it also dissociates into sodium and chloride ions. Then as a result of which concentration of chloride ions increases and to maintain the change equilibrium will shift towards the reactant side as a result of which concentration of silver ion decreases.

Hence, concentration of silver ions decreases, and the concentration of Chloride ions increases.

To know more about equilibrium law, visit the below link:
https://brainly.com/question/2943338

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