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A solution contains a mixture of Ag^(+)(...

A solution contains a mixture of `Ag^(+)(0.10M)` and `Hg_(2)^(2+)(0.10M)` which are to be separated by selective precipitation. Calculate the maximum concentration of iodide ion at which one of them gets precipitated almost completely. `(K_(SP)of AgI=8.5xx10^(-17)` and `K_(SP)` of `Hg_(2)I_(2)=2.5xx10^(-26))`

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To solve the problem of separating Ag⁺ and Hg₂²⁺ ions by selective precipitation using iodide ions (I⁻), we need to calculate the maximum concentration of I⁻ that can be added to the solution before one of the ions precipitates completely. We will do this by using the solubility product constants (Ksp) for AgI and Hg₂I₂. ### Step 1: Calculate the concentration of iodide ion for AgI precipitation. The solubility product expression for AgI is given by: \[ K_{sp} = [Ag^+][I^-] \] ...
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