A) \[108\times {{10}^{-3}}\]
B) \[1.0\times {{10}^{-14}}\]
C) \[2\times {{10}^{-16}}\]
D) \[1.035\times {{10}^{-5}}\]
Correct Answer: B
Solution :
Key Idea: Write the reaction for dissociation of\[AgCl\]. Find the relationship between solubility product and solubility and solve the problem. \[AgClA{{g}^{+}}+C{{l}^{-}}\] concentration \[x\] \[x\] \[\therefore \] \[{{K}_{sp}}=[A{{g}^{+}}[\,[C{{l}^{-}}]\] \[{{K}_{sp}}=(x)\times (x)\] or \[{{K}_{sp}}={{x}^{2}}\] Given, \[x=1.435\,\times {{10}^{-5}}g/L\] \[=1.435\,\times {{10}^{-5}}/143\,mol/L\] \[\therefore \] \[{{K}_{sp}}={{(1\times {{10}^{-7}})}^{2}}\] \[=1\times {{10}^{-14}}\]
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