A state of dynamic equilibrium exists in the silver (I) carbonate solution. A) w
ID: 854057 • Letter: A
Question
A state of dynamic equilibrium exists in the silver (I) carbonate solution. A) will the equilibrium shift toward s products or reactants when AgCO3 is added to the solution? B) where will the equilibrium shift when AgCO3 is added to the solution? C) how will the equilibrium be affected when HCl is added to the solution? A state of dynamic equilibrium exists in the silver (I) carbonate solution. A) will the equilibrium shift toward s products or reactants when AgCO3 is added to the solution? B) where will the equilibrium shift when AgCO3 is added to the solution? C) how will the equilibrium be affected when HCl is added to the solution?Explanation / Answer
a)
Your chemical equations are now unbalanced. You have too much Ag2CO3 in the system thus you must add more Ag and CO3 to match and create equilibrium once more.
This will favor the forward reaction because you are making products!
Nothing will happen to your Ag and CO3 when you add more of Ag2CO3. You must add more of Ag and CO3 to acheive the same rate of change again.
b)
With HCl, it's a different way because of the Cl- ion.
Ag+ + Cl- ==> AgCl, as a precipiate.
So with HCl you would be having both the acid reactionr AND the AgCl formation. This means you would be removing both Ag+ ions and CO3(2-) ions from solution. Still, though, it would result in a SHIFT to the RIGHT.As the acid reaction is dominant.
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