The minimum concentration of Ag+ ions required in order to initiate the precipitation of AgCl from a solution containing 0.004 mol L–1 of Cl– ion will be [Ksp of AgCl = 1.8 × 10–10]
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Answer:
2.5 ×10−8 ⋅mol⋅L−1
Explanation:
The chemical reaction under equilibrium would be:
Ag+ + Cl−→AgCL(s)
As per question statement we are given that thermodynamic equilibrium constant for the reaction, i.e.:
Ksp=[Ag+][Cl−]=1×10−10.
Ksp is also known as the solubility product. Now we are given the concentration of Cl- ions which is 0.004 or 4 x 10−3
Putting this in formula
[Ag+]=Ksp / [Cl-]= 1×10−10 / 4×10−3
=2.5 ×10−8 ⋅mol⋅L−1
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