Why must some solid remain in contact with a solution of a sparingly soluble salt in order to ensure equilibri [Solved]

Equilibrium is a dynamic process. Removing some solid would cause the equilibrium of the solution to shift to the left and produce more solid from the dissolved solution to reestablish equilibrium.

Equilibrium is a dynamic process. Removing some solid would cause the equilibrium of the solution to shift to the left and produce more solid from the dissolved solution to reestablish equilibrium.

The equilibrium we are talking about is AgCl(s) <---> Ag (aq) Cl-(aq)
At equilibria these will be at a certain balance, controlled by the equilibrium constant Kc

But what would happen if you removed the solid AgCl The condition for Kc would not longer be true and silver ions and chloride ions would have to react to form AgCl solid. This is why solid must be present.

Source(s): retired chemistry examiner

Source(s): retired chemistry examiner

The equilibrium we are talking about is AgCl(s) <---> Ag (aq) Cl-(aq)
At equilibria these will be at a certain balance, controlled by the equilibrium constant Kc

This post is last updated on hrtanswers.com at Date : 1st of September – 2022

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