Does adding different solid affect the quilibrium?

[Nope]

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

Homework Equations

The Attempt at a Solution

 

[chemisttree]

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?

 

[Blueshift5]

I would like to clarify that adding different solids can indeed affect the equilibrium of a chemical reaction. In this reaction, the addition of silver nitrate can shift the equilibrium to the left, favoring the reactants, as silver nitrate can react with the chloride ions (Cl-) to form a precipitate of silver chloride (AgCl). This reaction consumes chloride ions, reducing the concentration of Cl- in the solution, which can shift the equilibrium to the left to maintain a constant concentration of CoCl4 2-.

In general, adding a solid to a reaction mixture can affect the equilibrium by changing the concentrations of the reactants and products. This is because the solid does not contribute to the equilibrium constant (K), but it can change the activities of the species in solution, which can affect the equilibrium position.

As for your second question, the addition of aqueous or gaseous species to a reaction can also affect the equilibrium. The direction of the shift will depend on the specific reaction and the concentrations of the added species. In general, adding a reactant will shift the equilibrium to the right, while adding a product will shift it to the left. However, this is not always the case and can vary depending on the reaction conditions.

In conclusion, adding different solids can indeed affect the equilibrium of a chemical reaction, and the direction of the shift will depend on the specific reaction and the concentrations of the added species. It is important to carefully consider the effect of adding any species to a reaction mixture in order to accurately predict the equilibrium position.