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Predict if there will be any precipitate by mixing \( 50 \mathrm{mL} \) of \( 0.01 \mathrm{M} \) NaCl and 50 mL of \( 0.01 \mathrm{M} A g N O_{3} \) solution. The solubility product of \( A g C l \) is \( 1.5 \times \) \( 10^{-10} \)

1. since ionic product is greater than solubility product no precipitate will be formed
2. since ionic product is lesser than solubility product. precipitation will occur
3. since ionic product is greater than solubility product. precipitation will occur.
4. since ionic product and solubility product are same, precipitation will not occur

Correct answer: since ionic product is greater than solubility product. precipitation will occur.

Solution

The ionic product of AgCl is calculated by multiplying the concentrations of Ag+ and Cl- ions, and if it is greater than the solubility product, precipitation will occur. [AI-generated key — verify before high-stakes use]

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