(Solved): a Calculate the molar solubility of silver thiocyanate, AgSCN, in pure water (Ksp=1.01012). ...

a Calculate the molar solubility of silver thiocyanate, $\mathrm{AgSCN}$, in pure water $\left(K_{\mathrm{sp}}=1.0\times 10^{?12}\right)$. Solubility $=$ M Correct The general equilibrium constant expression, $K_{\mathrm{sp}}$ (solubility constant), for dissolving a poorly soluble salt ${\mathrm{A}}_x{\mathrm{B}}_y$ is: $\begin{array}{l}{\mathrm{A}}_x{\mathrm{B}}_y(\mathrm{s})?x{\mathrm{A}}^{y+}(\mathrm{aq})+y{\mathrm{B}}^{x?}(\mathrm{aq})\\ K_{\mathrm{sp}}={\left[{\mathrm{A}}^{y+}\right]}^x{\left[{\mathrm{B}}^{x?}\right]}^y\\ K_{\mathrm{sp}}=\left[{\mathrm{Ag}}^{+}\right]\left[{\mathrm{SCN}}^{?}\right]=(x)(x)=x^2=1.0\times 10^{?12}\\ x=\text{ solubility of AgSCN in water }=1.0\times 10^{?6}\mathrm{mol}/\mathrm{L}\end{array}$ b Calculate the molar solubility of silver thiocyanate, $\mathrm{AgSCN}\left(K_{\mathrm{sp}}=1.0\times 10^{?12}\right)$, in water containing $0.017\mathrm{M}\mathrm{NaSCN}$. Solubility $=$ M