Question

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?

• A. \( 2 \times 10^{-4} \, \text{M} \)
• B. \( 16 \times 10^{-4} \, \text{M} \)
• C. \( 8 \times 10^{-4} \, \text{M} \)
• D. \( 10 \times 10^{-4} \, \text{M} \)

Hint:

The solubility product can be used to determine the concentration of ions in a saturated solution.

Answer 1

The Correct Option is A

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.