Solid `AgNO_3` is added to a solution which is 0.1M in `Cl^-` and 0.1 M in `CrO_4^(2-)`. If `K_(sp)` values for AgCl and `Ag_2CrO_4` are `1.7 xx 10^(-10) and 1.9 xx 10^(-12)` respectively, which one will precipitate first? Find the concentration of `Cl^(-)` wher `Ag_2CrO_4` starts precipitating.

Explanation

To solve the problem, we need to determine which silver salt (AgCl or Ag2CrO4) will precipitate first when solid AgNO3 is added to a solution containing 0.1 M Cl⁻ and 0.1 M CrO4²⁻ ions. We will also find the concentration of Cl⁻ when Ag2CrO4 starts to precipitate.

### Step 1: Write the dissociation equations and Ksp expressions

1. **For AgCl:**
\[ \text{AgCl (s)} \rightleftharpoons \text{Ag}^+ (aq) + \text{Cl}^- (aq) \]
...