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In 1L saturated solution of AgCl[K(SP)(A...

In 1L saturated solution of `AgCl[K_(SP)(AgCl)= 1.6xx10^(-10)], 0.1` mole of CuCI `[K_(SP)(CuCl)=1.0xx10^(-6)]` is added. The resulrant concentration of `Ag^(+)` in the solution is `1.6xx10^(-x)`. The value of `"x"` is:

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To solve the problem step by step, we will analyze the situation involving the solubility product constants (Ksp) of AgCl and CuCl, and how the addition of CuCl affects the concentration of Ag⁺ ions in the saturated solution of AgCl. ### Step 1: Understand the initial conditions We have a saturated solution of AgCl with a Ksp of \(1.6 \times 10^{-10}\). This means that at equilibrium, the concentration of Ag⁺ and Cl⁻ ions in the solution can be expressed as: \[ K_{sp} = [Ag^+][Cl^-] = 1.6 \times 10^{-10} \] ...
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