Calculate the solubility of silver chloride in a solution that is 0.110 M in NH3. Express your answer using two significant figures.
AgCl(s) <======> Ag+(aq) + Cl-(aq)
Ag+(aq) + 2NH3(aq) <=====> Ag(NH3)2+(aq)
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AgCl(s) + 2NH3(aq) <======> [Ag(NH3)2]+(aq) + Cl-
I ---- 0.110 M 0 0 Using ICE table
C ----- -2x +x +x let us suppose 'x' moles [Ag(NH3)2]+ formed
E ---- 0.110 - 2x +x +x from x moles AgCl. Since AgCl is a solid we neglect moles of AgCl.
Concentration of Ag(NH3)2+ formed =x= 0.0054 M = Concentration of AgCl soluble = x = 5.4x10-3 M
Calculate the solubility of silver chloride in a solution that is 0.110 M in NH3. Express...
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