Since saturated solutions are equilibriums....

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In saturated solutions, the equilibrium between dissolved salt and undissolved salt means that adding more salt does not increase the amount of dissolved salt. According to Le Chatelier's principle, any change in a system at equilibrium will shift the equilibrium to counteract that change. However, the activity of a solid is defined as 1, regardless of the amount present, which means that adding more solid does not affect the equilibrium concentration of the dissolved ions. Therefore, the saturation point is reached when the solution can no longer dissolve additional salt, and the equilibrium remains unchanged despite the presence of excess solid.
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Since saturated solutions are equilibriums, why does adding more salt into the solution not increase the amount of dissolved salt? Le Chatelier's principle state that if there is a change in a equilibrium, the equilibrium moves to counteract the change. I know my statement is wrong but I don't know why because it fits with the principle fine (I think).
 
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Activity of the solid is always 1, it doesn't depend on the solid amount.
 
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