# Chapter 15 - Additional Aqueous Equilibria - Questions for Review and Thought - Topical Questions - Page 693b: 50b

$1 Ag_2SO_4(s) \lt -- \gt 2Ag^+ + 1S{O_4}^{2-}$ $K_{sp} (Ag_2SO_4) = [Ag^+]^2 [S{O_4}^{2-}]^1$

#### Work Step by Step

- Silver $(Ag^+)$ sulfate $(S{O_4}^{2-})$: $Ag_2SO_4$ 1. Write the dissociation equation for this salt: - Identify the ions of the salt: $Ag^+$ and $S{O_4}^{2-}$, these are the products, and the reactant is the solid salt. $Ag_2SO_4(s) \lt -- \gt Ag^+ + S{O_4}^{2-}$ - Balance the equation: $1 Ag_2SO_4(s) \lt -- \gt 2Ag^+ + 1S{O_4}^{2-}$ 2. Now, write the $K_{sp}$ expression. - Multiply the concentrations of the ions; - The equilibrium coefficients represent the exponent of these concentrations: $K_{sp} (Ag_2SO_4) = [Ag^+]^2 \times [S{O_4}^{2-}]^1$

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