A) \[6.0\times {{10}^{-10}}M\]
B) \[0.2M\]
C) \[1.2\times {{10}^{-10}}M\]
D) \[0.2\times {{10}^{-10}}M\]
Correct Answer: A
Solution :
Given, concentration of\[NaCl=0.2\,\,M\] \[{{K}_{sp}}(AgCl)=1.20\times {{10}^{-10}}\] Let the solubility of\[AgCl\]in\[NaCl=x\] \[AgCl\xrightarrow{{}}A{{g}^{+}}+C{{l}^{-}}\] Solubility\[\underset{0.2}{\overset{x}{\mathop{NaCl}}}\,\xrightarrow{{}}\underset{0.2}{\overset{x}{\mathop{Na}}}\,+\underset{0.2}{\overset{x}{\mathop{Cl-}}}\,\] \[\therefore \] \[[A{{g}^{+}}]=x\]and\[[C{{l}^{-}}]=(x+0.2)\] \[\therefore \] \[{{K}_{sp}}(AgCl)=[A{{g}^{+}}][C{{l}^{-}}]\] \[=x(x+0.2)\] \[={{x}^{2}}+0.2x\] \[\therefore \] \[{{K}_{sp}}=0.2x({{x}^{2}}<<1)\] or \[1.2\times {{10}^{-10}}=0.2x\] \[\therefore \] \[x=6\times {{10}^{-10}}\]
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