The solubility product of \( \text{Ag}_2 \text{CrO}_4 \) is \( 3.2 \times 10^{-12} \). What is the concentration of \( \text{CrO}_4^{2-} \) ions in that solution?
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The solubility product can be used to determine the concentration of ions in a saturated solution.
The solubility product \( K_{sp} \) for \( \text{Ag}_2 \text{CrO}_4 \) is given as:
\[
K_{sp} = [\text{Ag}^+]^2 [\text{CrO}_4^{2-}]
\]
By using stoichiometry, we can solve for the concentration of \( \text{CrO}_4^{2-} \) ions.