# What is the ionic concentrations of Ag+ and CrO4^-2 in a saturated solution of Ag2CrO4 at 25C? Ksp of Ag2CrO4 is 1.9x10^-12 mole^3/dm^9?

May 7, 2017

We interrogate the solubility equilibrium:

$A {g}_{2} C r {O}_{4} \left(s\right) r i g h t \le f t h a r p \infty n s 2 A {g}^{+} + C r {O}_{4}^{2 -}$

#### Explanation:

Now we have ${K}_{\text{sp}} = {\left[A {g}^{+}\right]}^{2} \left[C r {O}_{4}^{2 -}\right]$, and if we call the solubility of $\text{silver chromate}$ under the given conditions $S$, then, by the given stoichiometry, we write..........

${K}_{\text{sp}} = {\left(2 S\right)}^{2} \times S = 4 {S}^{3}$

And thus S=""^3sqrt((1.9xx10^-12)/(4))=7.80xx10^-5*mol*L^-1.

And thus ${S}_{A {g}^{+}} = 15.6 \times {10}^{-} 5 \cdot m o l \cdot {L}^{-} 1$;

${S}_{C r {O}_{4}^{2 -}} = 7.80 \times {10}^{-} 5 \cdot m o l \cdot {L}^{-} 1$.