50 ml of a solution containing 10−3mol of Ag+ is mixed with 50 ml of a 0.1 M HCl solution. How much Ag+ remains in solution? (Ksp of AgCl=1.0×10−10)
A
2.5×10−9
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B
2.5×10−7
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C
2.5×10−8
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D
2.5×10−10
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Solution
The correct option is C2.5×10−8 Ag+↓1×10−3mol+Cl−↓5×10−3mol→AgCl(s) [HCl]=50ml×0.1M =5.0mmol=5.0×10−3mol [H+]=[Cl−]=5×10−3mol All of the silver reacts with the chloride ions and then starts to dissociate to form silver ions again. [Cl−]=4×10−3 mol after the reaction. [Ag+]=1.0×10−104.0×10−3=2.5×10−8 mol