A) \[8\times {{10}^{-3}}mol/L\]
B) \[6.4\times {{10}^{-5}}mol/L\]
C) \[6.4\times {{10}^{-3}}mol/L\]
D) \[2.8\times {{10}^{-6}}mol/L\]
Correct Answer: A
Solution :
Key Idea: First find the relationship between solubility and solubility product of \[HgS{{O}_{4}}\] then substitute the values and calculate to find the value of solubility of \[HgS{{O}_{4}}\]. Let the solubility of \[HgS{{O}_{4}}\] be s mol/L \[HgS{{O}_{4}}H{{g}^{2+}}+SO_{4}^{2-}\] \[{{K}_{sp}}=[H{{g}^{2+]}}[SO_{4}^{2-}]\] \[=S\times S\] \[={{S}^{2}}\] or \[S=\sqrt{{{K}_{sp}}}\] \[=\sqrt{6.4\times {{10}^{-5}}}\] \[=8\times {{10}^{-3}}mol/L\]
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