Answer
Balanced equation:
$ 1Ag_2Cr{O_4}(s) \lt -- \gt 2 Ag^{+}(aq) + 1Cr{O_4}^{2-}(aq)$
$K_{sp} = [Ag^{+}]^2 \times [Cr{O_4}^{2-}]$
Work Step by Step
1. Identify the ions in the compound:
$Ag^{+}$ and $Cr{O_4}^{2-}$
2. Write the dissociation equation, where the solid ionic compound produces its ions in the water:
$ Ag_2Cr{O_4}(s) \lt -- \gt Ag^{+}(aq) + Cr{O_4}^{2-}(aq)$
Balance the equation:
$ 1Ag_2Cr{O_4}(s) \lt -- \gt 2 Ag^{+}(aq) + 1Cr{O_4}^{2-}(aq)$
3. To get the $K_{sp}$ expression, multiply the ions concentrations, where their balancing coefficients are the exponents of the molarities.
$K_{sp} = [Ag^{+}]^2 \times [Cr{O_4}^{2-}]^1$
$K_{sp} = [Ag^{+}]^2 \times [Cr{O_4}^{2-}]$
