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In 1L saturated solution of $AgCl[K_{sp} AgCl=1.6 \times 10^{-10}]$ 0.1 mole of $CuCl[K_{sp}[CuCl]=1.0 \times 10^{-6}]$ is added . The resulatnt conenetration  of $Ag^{+}$ in the solution is $1.6 \times 10^{-x}$ .The value of x is 

Answer:

Explanation:

It is a case of simultaneous solubility of salts with a common ion. Here solubility product of
CuCl is much greater than that of AgCl, it can be assumed that Cl^- in solution comes mainly from CuCl

$\Rightarrow$   $|Cl^{-}|=\sqrt{K_{sp}(CuCl)}=10^{-3} M$

Now for $AgCl:K_{sp}=1.6 \times 10^{-10}= [Ag^{+}][Cl^{-}]=[Ag^{+}] \times 10^{-3}$

$ \Rightarrow [Ag^{+}]=1.6 \times 10^{-7}$