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