The solubility product

A solution containing the chloride ion is added dropwise to a solution containing the $Ag^+$ ion. As long as the product $ [Ag^+] [Cl^-] $ has a value less than the solubility product, there is no .......... that is formed. However, once the product $[Ag^+][Cl^-]$ has reached the value of the solubility product, any attempt to increase the concentration of the $Cl^-$ or $Ag^+$ ions will lead to precipitation of a greater amount of $ AgCl $. When $Cl^-$ or $Ag^+$ is added, the product $[Ag^+][Cl^-]$ remains .........., but the amount of $AgCl(s)$ ........... Let $x$ be the maximum molarity of $NaCl$ in a $10^{-4}$ M solution in Ag⁺. Given that the solubility product of $ AgCl $ is equal to $K_s$ $ = $ $1.6 \cdot 10^{-10} $, calculate $x$.

Calcul: ....... We have $x = [Cl^-] $    , because the chloride ions come only from $NaCl$ ....... In the saturated solution we have: $K_s$ $=$ $[Ag^+][Cl^-]$ $1,6\cdot 10^{-10}$ $=$ $10^{-4}x$ ....... Maximum molarity of $NaCl\;$ $=$ $\frac{1.6\cdot 10^{-10}}{10^{-4}}$ $=$ $1.6\cdot 10^{-6}\frac{mol}{L}$