Does adding different solid affect the quilibrium?

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Adding silver nitrate, which dissociates in solution, can affect the equilibrium of the reaction involving CoCl4 2- and Co(H2O)62+, as the Ag+ ion may interact with Cl- ions, potentially shifting the equilibrium. The initial assumption that adding a solid has no effect on equilibrium is correct, but the context changes with the introduction of ions in solution. Regarding the addition of gases or aqueous solutions, if the added species do not appear in the equilibrium expression, they typically do not alter the equilibrium position. However, if the added species do affect the concentrations of reactants or products in the equilibrium expression, they can shift the equilibrium. Understanding the specific interactions and concentrations is crucial for predicting the effects on equilibrium.
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Homework Statement


CoCl4 2-+6H2O --> Co(H2O)62++4Cl-+energy
If I add silver nitrate, which direction does it shift?
I think it is no effect, because adding solid does not affect the equilibrium?... Am i right?

Btw, what happen if i add aqueous to X gas --> Z gas + Y gas, vise verse...
or gas to x(aq)--->Z aq + Y aq
Thanks

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Silver nitrate is not being added as a solid. Assume that it is being added as a dissociated species in solution. What effect would the Ag+ ion have on the equilibrium?

I can't tell what you are asking about your gases but I assume that you are adding water vapor to a mixture of interconverting gases at equilibrium, yes? If the partial pressure of water vapor doesn't appear in the equilibrium expression, will it change the equilibrium?
 
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