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  • The  for the following dissociation is <img alt="1.6\times 10^{-5}" src="http://entrancecorner.onc

The K_{sp} for the following dissociation is 1.6\times 10^{-5}.

PbCl_{2}(s)=Pb^{2+}(aq)+2Cl^{-}(aq)

Which of the following choices is correct for a mixture of 300mL, 0.134 M Pb(NO_{3})_{2} and 100 mL 0.4 M NaCl?

Option: 1

Q<K_{sp}


Option: 2

Q>K_{sp}


Option: 3

Q=K_{sp}


Option: 4

Not enough data is provided


Answers (1)

best_answer

The K_{sp} for the following dissociation is 1.6\times 10^{-5}.

PbCl_{2}(s)=Pb^{2+}(aq)+2Cl^{-}(aq)

So,

\\Q=\left[\mathrm{Pb}^{2+}\right]\left[\mathrm{Cl}^{2}\right]^{2} \\Q= \frac{300 \times 0.134}{400} \times\left[\frac{100 \times 0.4}{400}\right]^{2} \\ \\Q= \frac{3 \times 0.134}{4} \times(0.1)^{2} \\Q= 0.105 \times 10^{-2} \\Q= 1.005 \times 10^{-3}

So, Q > Ksp

Hence, the option number (2) is correct.

Posted by

Rishabh

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