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In one liter saturated solution of AgCl [Ksp = 1.6 x 10-10], 0.1 mol of CuCl [Ksp = 1.0 x 10-10 ] is added. Find out the resultant concentration of Ag+ in the solution.

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Let the concentration of AgCl is x mol/L and concentration of CuCl is mol/L

Ksp of AgCl= [Ag+][Cl]

= x (x + y)  ...........(i)

Ksp of CuCl = [Cu+][Cl]

= y ( x + y)  .........(ii)

On solving equation (i) and (ii), we get

\(\frac{K_{sp}\,of\,AgCl}{K_{sp}\,of\,CuCl}\) = \(\frac{X}{y}\)

\(\frac{1.6\times10^{-10}}{1.0\times10^{-6}}\) = \(\frac{X}{0.1}\)

or x = \(\frac{1.6\times10^{-10}\times0.1}{1.0\times10^{-6}}\)

= 1.6 x 10-5 mol/L

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