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