Calculate the equilibrium concentration of $Pb^{2+}$ ions in a solution of $PbS$ containing $1 \times 10^{-11} \ mol \ dm^{-3}$ of sulphide ions. (Given $K_{sp}$ for $PbS = 8.0 \times 10^{-28}$)
- A$8 \times 10^{-17} \ mol \ dm^{-3}$
- B$4 \times 10^{-17} \ mol \ dm^{-3}$
- C$8 \times 10^{-18} \ mol \ dm^{-3}$
- D$8 \times 10^{-11} \ mol \ dm^{-3}$
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