`1.0L` of solution which was in equilibrium with solid mixture of `AgC1` and `AgC1` and `Ag_(2)CrO_(4)` was found to contain `1xx 10^(-4) mol of Ag^(o+)` ions, `1.0 xx 10^(-6) mol` of `C1^(Θ)` ions and `8.0 xx 10^(-4)` moles of `CrO_(4)^(2-)` ions. `Ag^(o+)` ions added slowely to the above mixture (keeping volume constant) till `8.0 xx 10^(-7)` mol of `AgC1` got precipitated. How many moles of `Ag_(2)CrO_(4)` were also precipitated?

Explanation

To solve the problem step by step, we will follow the reasoning laid out in the transcript while providing a clear mathematical approach.

### Step 1: Understand the Initial Conditions
We have a 1.0 L solution in equilibrium with solid AgCl and Ag2CrO4. The concentrations of ions in the solution are:
- \( [Ag^+] = 1 \times 10^{-4} \, \text{mol} \)
- \( [Cl^-] = 1 \times 10^{-6} \, \text{mol} \)
- \( [CrO_4^{2-}] = 8.0 \times 10^{-4} \, \text{mol} \)

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