A) \[AgCl\]
B) \[AgBr\]
C) \[A{{g}_{2}}Cr{{O}_{4}}\]
D) Any of these
Correct Answer: C
Solution :
For binary salts (like \[AgCl,AgBr\]), \[s=\sqrt{{{K}_{sp}}}\] \[\therefore \] solubility of \[AgCl\] \[=\sqrt{1.8\times {{10}^{-10}}}=1.35\times {{10}^{-5}}\] mole/litre solubility of \[AgBr=\sqrt{5.0\times {{10}^{-13}}}\] \[=7.1\times {{10}^{-7}}\] mole/litre For, \[A{{g}_{2}}Cr{{O}_{4}},\] \[{{K}_{sp}}=4{{s}^{3}}\] \[\therefore \] solubility of \[A{{g}_{2}}Cr{{O}_{4}}\] \[=\frac{\sqrt[3]{{{K}_{sp}}}}{4}=\frac{\sqrt[3]{2.4\times {{10}^{-12}}}}{4}\] \[\sqrt[3]{600\times {{10}^{-15}}}\] \[=8.44\times {{10}^{-5}}\] mole/litre As \[A{{g}_{2}}Cr{{O}_{4}}\] has maximum solubility, if will give maximum \[A{{g}^{+}}\] ions in solution. Hence it will be used.You need to login to perform this action.
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