The Ksp for the following dissociation is
1.6 × 10–5
$PbC{l_{2(s)}} \leftrightharpoons Pb_{(aq)}^{2 + } + 2Cl_{(aq)}^ -$
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 ?
Solution
[Pb<sup>2+</sup>] = ${{300 \times 0.134} \over {400}}$
<br><br> = 1.005 × 10<sup>–1</sup> M
<br><br>[Cl<sup>-</sup>] = ${{100 \times 0.4} \over {400}}$
<br><br>= 10<sup>–1</sup> M
<br><br>$PbC{l_{2(s)}} \leftrightharpoons Pb_{(aq)}^{2 + } + 2Cl_{(aq)}^ -$
<br><br>Q = [Pb<sup>2+</sup>] × [Cl<sup>–</sup>]<sup>2</sup>
<br><br>= 0.1005 × (0.1)<sup>2</sup>
<br><br>= 1.005 × 10<sup>–3</sup>
<br><br>Given K<sub>sp</sub>
= 1.6 × 10<sup>–5</sup>
<br><br>$\therefore$ Q > K<sub>sp</sub>
About this question
Subject: Chemistry · Chapter: Equilibrium · Topic: Chemical Equilibrium and Kc, Kp
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