In the quantitative estimation of `Ag^(o+)` ions as `AgCl`, solution of `NaCl` is used as the precipitating reagent. Why a large excess of `NaCl` should be avoided?

Explanation

To answer the question regarding why a large excess of NaCl should be avoided in the quantitative estimation of Ag⁺ ions as AgCl, we can break down the explanation into clear steps:

### Step-by-Step Solution:

1. **Understanding the Reaction**:
- When NaCl is added to a solution containing Ag⁺ ions, the chloride ions (Cl⁻) from NaCl react with Ag⁺ to form a precipitate of silver chloride (AgCl).
- The reaction can be represented as:
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