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Did the precipitated agcl dissolve explain

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– AgCl(s) is sparingly soluble.
Its dissolution is governed by the solubility product Ksp for the equilibrium AgCl(s) ⇌ Ag+(aq) + Cl−(aq), with Ksp ≈ 1.8 × 10−10 at 25 °C.
A very small amount dissolves; adding ligands or light can change this.

Example:

– In pure water at 25 °C, let [Ag+] = [Cl−] = s.

Then s^2 = Ksp, so s ≈ sqrt(1.8×10−10) ≈
1.3×10−5 M.
– This corresponds to about
1.9 mg of AgCl dissolved per liter of water.
Practically, most of the precipitate remains solid.
Brief explanation: – The small Ksp means only a tiny amount dissolves in water; dissolution can be increased by removing Ag+ or Cl− via complexation (e.g., with NH3 to form [Ag(NH3)2]+) or other ligands, which shift the equilibrium to dissolve more AgCl.

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