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 \[HgS{{O}_{4}}\underset{s}{\mathop{H{{g}^{2+}}}}\,+\underset{s}{\mathop{SO_{4}^{2-}}}\,\] \[{{K}_{sp}}=[H{{g}^{2+}}][SO_{4}^{2-}]\] \[=s\times s\] \[={{s}^{2}}\] Or \[s=\sqrt{{{K}_{sp}}}\] \[=\sqrt{6.4\times {{10}^{-5}}}\] \[=8\times {{10}^{-3}}mol/L\]
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