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Question

# 50 mL of a solution containing 10−3 moles 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
2.5×109
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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 A 2.5×10−9Concentration of [Ag+]=10−350+50×1000=0.01 M Concentration of [Cl−]=0.1×5050+50=0.05 M So, the reaction quotient is Q=[Ag+][Cl−]=5×10−4 M ∵Q>Ksp, so precipitate forms Ag+(aq.)+Cl−(aq.)⇌AgCl(s)At given condition0.010.05After precipitationx≈0.04 Ksp=[Ag+][Cl−]⇒10−10=x×0.04 ⇒x=[Ag+]=2.5×10−9

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