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0.10 mol sample of AgNO3 is dissolved in one litre of 2.00 M NH3. Is it possible AgCl(s) form the solution by adding 0.010 mol of NaCl ? ( Ksp(AgCl) = 1.8 × 10–10, Kf[Ag(NH3)2+] = 1.6 × 107)

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It is assumed that all Ag+ ions have been complex and only x amount is left

 x = 1.93 × 10–9 M = [Ag+] undisolved 

[Cl] = 1.0 × 10–2

∴ [Ag+] [Cl] = 1.93 × 10–9 × 1.0 × 10–2 = 1.93 × 10–11 < 1.8 × 10–10 [Ksp(AgCl)

Hence, AgCl (s) will not precipitate.

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