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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+] remains in the solution? (Given: Ksp of AgCl=10–10)

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

## The correct option is A 2.5×10−9M[Ag+]initial just after mixing=10−350+50×1000=0.01 M [Cl−]initialjust after mixing=0.1×5050+50=0.05 M I.P.=[Ag+][Cl−]=5×10−4 (where I.P. = ionic product) ∵I.P.>Ksp Ag+(aq)+Cl−(aq)→AgCl(s)0.01 M0.05Initial conc.X0.04 Mconc. after precipitation Ksp=[Ag+][Cl−] 10−10=[Ag+](0.04) ∴[Ag+]=2.5×10−9M

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