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 0.10 M. Aqueous HCl is added to this solution until the Cl- concentration is 0.10 M. What will the concentration of Ag+ and Pb2 + be at equilibrium? ( Ks p for AgCl =1.8× 10- 10,Ks p for PbCl2=1.7× 10- 5 )

Question

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 0.10 M. Aqueous HCl is added to this solution until the Cl- concentration is 0.10 M. What will the concentration of Ag+ and Pb2 + be at equilibrium? ( Ks p for AgCl =1.8× 10- 10,Ks p for PbCl2=1.7× 10- 5 ) (A) [.Ag+].=1.8× 10- 7M,[.Pb2 +].=1.7× 10- 6M (B) [.Ag+].=1.8× 10- 11M,[.Pb2 +].=8.5× 10- 5M (C) [.Ag+].=1.8× 10- 9M,[.Pb2 +].=1.7× 10- 3M (D) [.Ag+].=1.8× 10- 11M,[.Pb2 +].=1.7× 10- 4M

Tardigrade Admin · Accepted Answer

Ks p[.AgCl].=[.Ag+].[.Cl-]. [.Ag+].=(1.8 × 1 0- 10/1 0- 1)=1.8× 10- 9M textK textsp [ textPbCl2 ]=[ textPb2 +] [ textCl-]2 [.Pb2 +].=(1.7 × 1 0- 5/1 0- 1 × 1 0- 1)=1.7× 10- 3M

$[A g^{+}] = 1.8 \times 1 0^{- 7} M, [P b^{2 +}] = 1.7 \times 1 0^{- 6} M$

$[A g^{+}] = 1.8 \times 1 0^{- 11} M, [P b^{2 +}] = 8.5 \times 1 0^{- 5} M$

$[A g^{+}] = 1.8 \times 1 0^{- 9} M, [P b^{2 +}] = 1.7 \times 1 0^{- 3} M$

$[A g^{+}] = 1.8 \times 1 0^{- 11} M, [P b^{2 +}] = 1.7 \times 1 0^{- 4} M$

$K_{s p} [A g Cl] = [A g^{+}] [C l^{-}]$
$[A g^{+}] = \frac{1.8 \times 1 0 ^{- 10}}{1 0 ^{- 1}} = 1.8 \times 1 0^{- 9} M$
$K_{sp} [PbCl_{2}] = [Pb^{2 +}] [Cl^{-}]^{2}$
$[P b^{2 +}] = \frac{1.7 \times 1 0 ^{- 5}}{1 0 ^{- 1} \times 1 0 ^{- 1}} = 1.7 \times 1 0^{- 3} M$

[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+]=1.7×10−4M

Ksp​[AgCl]=[Ag+][Cl−] [Ag+]=10−11.8×10−10​=1.8×10−9M Ksp​[PbCl2​]=[Pb2+][Cl−]2 [Pb2+]=10−1×10−11.7×10−5​=1.7×10−3M

$[A g^{+}] = 1.8 \times 1 0^{- 7} M, [P b^{2 +}] = 1.7 \times 1 0^{- 6} M$

$[A g^{+}] = 1.8 \times 1 0^{- 11} M, [P b^{2 +}] = 8.5 \times 1 0^{- 5} M$

$[A g^{+}] = 1.8 \times 1 0^{- 9} M, [P b^{2 +}] = 1.7 \times 1 0^{- 3} M$

$[A g^{+}] = 1.8 \times 1 0^{- 11} M, [P b^{2 +}] = 1.7 \times 1 0^{- 4} M$

$K_{s p} [A g Cl] = [A g^{+}] [C l^{-}]$
$[A g^{+}] = \frac{1.8 \times 1 0 ^{- 10}}{1 0 ^{- 1}} = 1.8 \times 1 0^{- 9} M$
$K_{sp} [PbCl_{2}] = [Pb^{2 +}] [Cl^{-}]^{2}$
$[P b^{2 +}] = \frac{1.7 \times 1 0 ^{- 5}}{1 0 ^{- 1} \times 1 0 ^{- 1}} = 1.7 \times 1 0^{- 3} M$