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Q.

The $K_{sp}$ for the following dissociation is $1.6 \times 10^{- 5}$ ${PbCl}_{2 (s)} ⇌ {Pb}_{(aq)}^{2 +} + 2 {Cl}_{(aq)}^{-}$
Which of the following choices is correct for a mixture of $300 mL 0.314 MPb {({NO}_{3})}_{2}$ and $100 mL 0.4 MNaCl$ ?

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a

$Q < K_{sp}$

b

Not enough data provided

c

$Q > K_{sp}$

d

$Q = K_{sp}$

answer is C.

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Detailed Solution

Reaction quotient, $Q = [{Pb}^{2 +}] {[{Cl}^{-}]}^{2}$

= $\frac{300 \times 0.134}{400} \times [\frac{100 \times 0.4}{400}]$

= $\frac{3 \times 0.134}{4} \times (0.1)^{2}$

=0.105 $\times 10^{- 2}$

=1.05 $\times 10^{- 3}$

$Q > K_{sp}$

Hence the correct option is (C) $Q > K_{sp}$ .

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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 mL0.314MPbNO32 and 100 mL0.4MNaCl ?