1. Tardigrade
  2. Question
  3. Chemistry
  4. 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 Error Report

Thank you for reporting, we will resolve it shortly

Back to Question

Q. The $K_{sp}$ for the following dissociation is $1.6 \times 10^{-5}$
$PbCl_{2\left(s\right)} {\rightleftharpoons} Pb^{2+}_{\left(aq\right)} + 2Cl^{-}_{\left(aq\right)}$
Which of the following choices is correct for a mixture of 300 mL 0.134 M Pb$(NO_3)_2$ and 100 mL 0.4 M NaCl ?

JEE MainJEE Main 2020Equilibrium

Solution:

$\left[Pb^{2+}\right]=\frac{300\times0.134}{400}$
$=1.005\times10^{-1}M$
$\left[Cl^{-}\right]=\frac{100\times0.4}{400}=10^{-1}M$
$Pbcl_{2\left(s\right)} {\rightleftharpoons} \, pb_{\left(a q.\right)}^{+2}+2Cl_{\left(a q.\right)}^{-}$
$Q=\left[Pb^{2+}\right]\times\left[Cl^{-}\right]^{2}$
$=1.005\times10^{-3} >\, k_{s p}$