Ksp for AgCl=[Ag+][Cl−] ∴[Ag+]Ksp for PbCl2∴[Pb2+]=10−11.8×10−10=1.8×10−9M.=[Pb2+][Cl−]2=10−1×10−11.7×10−5=1.7×10−3M
In qualitative analysis, the metals of group I can be separated from other ions by precipitating them as chloride salts. A solution initially contains Ag+and Pb2+ at a concentration of 0.10M. Aqueous HCl is added to this solution until the Cl−concentration is 0.10M. What will be the concentration of Ag+and Pb2+ be at equilibrium? ( Ksp for AgCl=1.8×10−10,Ksp for PbCl2=1.7×10−5 )
Held on 30 Apr 2011 · Verified 9 Jul 2026.
[Ag+]=1.8×10−7M;[Pb2+]=1.7×10−6M
[Ag+]=1.8×10−11M;[Pb2+]=8.5×10−5M
[Ag+]=1.8×10−9M;[Pb2+]=1.7×10−3M
[Ag+]=1.8×10−11M;[Pb2+]=8.5×10−4M
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