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Additional solid silver sulfate, a slightly soluble solid, is added to a solution of silver ion and sulfate ion atequilibrium with solid silver sulfate.$2 \mathrm{Ag}^{+}(a q)+\mathrm{SO}_{4}^{2-}(a q) \rightleftharpoons \mathrm{Ag}_{2} \mathrm{SO}_{4}(s)$Which of the following will occur?(a) $\mathrm{Ag}^{+}$ or $\mathrm{SO}_{4}^{2-}$ concentrations will not change.(b) The added silver sulfate will dissolve.(c) Additional silver sulfate will form and precipitate from solution as Ag' ions and $\mathrm{SO}_{4}^{2-}$ ions combine.(d) The Ag' ion concentration will increase and the $\mathrm{SO}_{4}^{2-}$ ion concentration will decrease.
a
Chemistry 102
Chapter 13
Fundamental Equilibrium Concepts
Chemical Equilibrium
Aqueous Equilibria
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So here we have the equilibrium between silver ions and solve it ions in a solution as it pertains to the insoluble soul silver sulfate. So what we should think about for this reaction is what it means for tohave an insoluble salt and what that means in terms of the equilibrium expression. So here, your equilibrium expression, we don't have any products and our equation that are gonna be included because the only thing that we have is thesis Ah, lid, silver Sophie. Which means that our equilibrium expression is just going to be one over the concentrations of our reactions because of this silver sulfate is not going to be considered in this reaction equation. So if we add silver sulfate to our solution, this is going to have no change in the concentrations of our dissolve species because silver sulfate does not contribute to this equilibrium expression, so there will be no change and the dissolve species
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