The volume (in `mL`) of `0.1M Ag NO_(3)` required for complete precipitation of chloride ions present in `30 mL` of `0.01M` solution of `[Cr(H_(2)O)_(5)Cl]Cl_(2)`, as silver chloride is close to:

Explanation

To solve the problem, we need to find the volume of `0.1 M AgNO3` required to completely precipitate the chloride ions from the given complex `[Cr(H2O)5Cl]Cl2`. Here are the steps to arrive at the solution:

### Step 1: Determine the number of moles of chloride ions in the complex
The complex `[Cr(H2O)5Cl]Cl2` contains two types of chloride ions:
- One chloride ion is part of the coordination sphere (non-ionizable).
- The other two chloride ions are outside the coordination sphere (ionizable).

Since only the ionizable chloride ions will react with `AgNO3`, we focus on those.
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