A) both form precipitate with \[BaC{{l}_{2}},SO_{3}^{2-}\]dissolves in HCI but \[SO_{4}^{2-}\]does not
B) \[SO_{3}^{2-}\]forms precipitate with \[BaC{{l}_{2}},SO_{4}^{2-}\]does not
C) \[SO_{4}^{2-}\]forms precipitate with \[BaC{{l}_{2}},SO_{3}^{2-}\]does not
D) both form precipitate with \[BaC{{l}_{2}},SO_{4}^{2-}\]dissolves in \[HCl\] but \[SO_{3}^{2-}\]does not
Correct Answer: A
Solution :
\[\text{SO}_{3}^{2-}\]and \[\text{SO}_{4}^{2-}\]when treated with \[\text{BaC}{{\text{l}}_{\text{2}}}\]give white ppt of \[\text{BaS}{{\text{O}}_{3}}\]and\[\text{BaS}{{\text{O}}_{4}}\] respectively. \[BaC{{l}_{2}}+SO_{3}^{2-}\xrightarrow{{}}\underset{\begin{smallmatrix} \text{Barium} \\ \text{sulphide} \end{smallmatrix}}{\mathop{BaS{{O}_{3}}}}\,+2C{{l}^{-}}\] \[BaC{{l}_{2}}+SO_{4}^{2-}\xrightarrow{{}}\underset{\begin{smallmatrix} \text{Barium} \\ \text{sulphide} \end{smallmatrix}}{\mathop{BaS{{O}_{4}}+2C{{l}^{-}}}}\,\] Out of these two. \[SO_{3}^{2-}\]is soluble in HCl but \[SO_{4}^{2-}\]does not.
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