A solution contains ${\text{Ag}}^{+}$ and ${\text{Pb}}^{2+}$ at $0.10\text{M}$. Aqueous $\text{HCl}$ is added until $[{\text{Cl}}^{-}]=0.10\text{M}$. What are the concentrations of ${\text{Ag}}^{+}$ and ${\text{Pb}}^{2+}$ at equilibrium? ($K_{sp}$ for $\text{AgCl}=1.8\times 10^{-10}$, $K_{sp}$ for ${\text{PbCl}}_2=1.7\times 10^{-5}$)

1. A
   $[{\text{Ag}}^{+}]=1.8\times 10^{-9}\text{M},[{\text{Pb}}^{2+}]=1.7\times 10^{-3}\text{M}$
2. B
   $[{\text{Ag}}^{+}]=1.8\times 10^{-11}\text{M},[{\text{Pb}}^{2+}]=1.7\times 10^{-4}\text{M}$
3. C
   $[{\text{Ag}}^{+}]=1.8\times 10^{-7}\text{M},[{\text{Pb}}^{2+}]=1.7\times 10^{-6}\text{M}$
4. D
   $[{\text{Ag}}^{+}]=1.8\times 10^{-11}\text{M},[{\text{Pb}}^{2+}]=8.5\times 10^{-5}\text{M}$