The concentration of chromate ions ($CrO_4^{2-}$) at $15^oC$ in a saturated solution of pure strontium chromate is equal to $0.006\frac{mol}{L}$.
The equation of dissolution of pure strontium chromate
$SrCrO_4(s)$ 
$Sr^{2+}(aq)$ $+$ $CrO_4^{2-}(aq)$
shows that in that case the concentration of $Sr^{2+}$ is equal to .......... $\frac{mol}{L}$
The solubility product at $15^oC$ of $SrCrO_4$ is therefore equal to
$K_s$ $=$ $[Sr^{2+}][CrO_4^{2-}]$ = .......... $\frac{mol^2}{L^2} $
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