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Question

# 50 ml of a solution containing 10−3 mol of Ag+ is mixed with 50 ml of a 0.1 M HCl solution. How much Ag+ concentration remains in solution? (Ksp of AgCl=1.0×10−10)

A
2.5×109
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B
2.5×107
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C
2.5×108
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D
2.5×1010
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Solution

## The correct option is C 2.5×10−8Ag+↓1×10−3 mol+Cl−↓5×10−3 mol→AgCl(s) Millimoles of HCl=50 ml×0.1 M =5.0 mmol=5.0×10−3 mol [H+]=[Cl−]=5×10−3 mol 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=2.5×10−8mol

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