Chemistry

Problem

A solution is 0.010 M in both

Pb^{2+}

and

Ag^{+}

. Chloride ion is added dropwise while the solution is stirred. Given

K_{sp}(PbCl_2)=1.7\times10^{-5}

and

K_{sp}(AgCl)=1.8\times10^{-10}

, which compound will precipitate first as the concentration of

Cl^-

increases? a) Both compounds precipitate at the same

[Cl^-]

because their cation concentrations are equal. b)

AgCl

PbCl_2

d) Neither compound precipitates until

[Cl^-]

exceeds

1.7\times10^{-3}\,\text{M}