Agcl(s) < > ag+(aq) + cl–(aq) what will happen to the chemical equilibrium if agno3 is added?

Chemical equilibrium will shift towards the left.

Explanation:

If we look at the equation AgCl(s) <---> Ag+(aq) + Cl– (aq)

We can see that the equation is balanced and the reaction has reached the state of chemical equilibrium where amount of reactants is same as the amount of products.

If we will add AgNO3 in this solution, that will disturb the chemical equilibrium of this reaction and cause the formation of more number of silver ions.

Then the system will try to counter the problem of excessive production of Ag+ ions and the production of silver ions will become less by the precipitation of great amount of AgCl (silver chloride). This is in accordance with Le Chatelier's principle, because Ag+ that is increasing due to addition of AgNo3 should decrease in order to maintain equilibrium.

                            Ag+(aq) + Cl– (aq)            --->       AgCl(s)

When Ag becomes greater than Cl, this decreases the solubility of AgCl and it starts to precipitate out. This phenomenon is also commonly referred to be as common ion effect between AgNO3 and AgCl.

Hope it help!

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