Solubility of AgCl is `10^(-5)` mol `litre^(-1)` . A solution contains 1 mg AgCl in 900 mL water . What amount of AgCl should be more added to make it saturated ?

Explanation

To solve the problem of how much more AgCl should be added to make the solution saturated, we can follow these steps:

### Step 1: Calculate the solubility product (Ksp) of AgCl
The solubility of AgCl is given as \(10^{-5}\) mol/L. The dissociation of AgCl in water can be represented as:
\[ \text{AgCl} \rightleftharpoons \text{Ag}^+ + \text{Cl}^- \]
If the solubility (S) of AgCl is \(10^{-5}\) mol/L, then at saturation:
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