The Ksp for the following dissociation is 1.6 × 10-5 PbCl2(s) leftharpoons Pb2+(aq) + 2Cl-(aq) Which of the following choices is correct for a mixture of 300 mL 0.134 M Pb(NO3)2 and 100 mL 0.4 M NaCl ?

Question

The Ksp for the following dissociation is 1.6 × 10-5 PbCl2(s) leftharpoons Pb2+(aq) + 2Cl-(aq) Which of the following choices is correct for a mixture of 300 mL 0.134 M Pb(NO3)2 and 100 mL 0.4 M NaCl ? (A) Q < Ksp (B) Q > Ksp (C) Q = Ksp (D) Not enough data provided

Tardigrade Admin · Accepted Answer

[Pb2+]=(300×0.134/400) =1.005×10-1M [Cl-]=(100×0.4/400)=10-1M Pbcl2(s) leftharpoons pb(a q.)+2+2Cl(a q.)- Q=[Pb2+]×[Cl-]2 =1.005×10-3 > ks p

Q. The $K_{s p}$ for the following dissociation is $1.6 \times 1 0^{- 5}$
$P b C l_{2 (s)} ⇌ P b_{(a q)}^{2 +} + 2 C l_{(a q)}^{-}$
Which of the following choices is correct for a mixture of 300 mL 0.134 M Pb $(N O_{3})_{2}$ and 100 mL 0.4 M NaCl ?

$Q < K_{s p}$

$Q > K_{s p}$

$Q = K_{s p}$

Not enough data provided

$[P b^{2 +}] = \frac{300 \times 0.134}{400}$
$= 1.005 \times 1 0^{- 1} M$
$[C l^{-}] = \frac{100 \times 0.4}{400} = 1 0^{- 1} M$
$P b c l_{2 (s)} ⇌ p b_{(a q .)}^{+ 2} + 2 C l_{(a q .)}^{-}$
$Q = [P b^{2 +}] \times [C l^{-}]^{2}$
$= 1.005 \times 1 0^{- 3} > k_{s p}$

Q. The Ksp​ for the following dissociation is 1.6×10−5 PbCl2(s)​⇌Pb(aq)2+​+2Cl(aq)−​ Which of the following choices is correct for a mixture of 300 mL 0.134 M Pb(NO3​)2​ and 100 mL 0.4 M NaCl ?

Q<Ksp​

Q>Ksp​

Q=Ksp​