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Question
The Ksp of salt AgCl at 25oC is 2.56×10−10. The how much volume of H2O is required to dissolve 0.01 mole of salt.
The Ksp of salt AgCl at 25oC is 2.56×10−10. The how much volume of H2O is required to dissolve 0.01 mole of salt.
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Solution
The correct option is B 625 L
AgCl(s)⇌Ag++Cl−⇒Ksp=[Ag+][Cl−]=2.56×10−10If S is the solubility then,S2=2.56×10−10⇒S=1.6×10−5molL−1S in gL−1=1.6×10−5×143.32 =229.3×10−5=2.3×10−3gL−1For a solution of 0.01 mole=1.43g2.3×10−3gL=621.73≃625L
AgCl(s)⇌Ag++Cl−
⇒Ksp=[Ag+][Cl−]=2.56×10−10
If S is the solubility then,
S2=2.56×10−10
⇒S=1.6×10−5molL−1
S in gL−1=1.6×10−5×143.32
=229.3×10−5=2.3×10−3gL−1
For a solution of 0.01 mole
=1.43g2.3×10−3gL=621.73≃625L
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