Question

If solubility product of $ HgS{{O}_{4}} $ is $ 6.4\times {{10}^{-5}} $ , then its solubility is

• 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 $

Answer 1

Answer: (A)

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 $