50mL of a solution containing 10−3 mole of Ag+ is mixed with 50mL of a 0.1MHCl solution how much Ag+ remains in solution? (KspofAgCl=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 A2.5×10−9 [Ag+]=10−350+50×1000=0.01[Cl−]=0.1×5050+50=0.05Q=[Ag+][Cl−]=5×10−4∵Q>KspAg+(aq.)+Cl−(aq.)→AgCl(s) at given condition0.010.05after precipitationx≈0.04 Ksp=[Ag+][Cl−]10−10≈x×0.04x=[Ag+]=2.5×10−9