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(A) $SO_{3}^{2-}$ and $SO_{4}^{2-}$ ions react with $BaCl_{2}$ to form white precipitates of $BaSO_{3}$ and $BaSO_{4}$ respectively.$Ba^{2+} + SO_{3}^

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Both form precipitate with $BaCl_{2}$, $SO_{3}^{2-}$ dissolves in $HCl$ but $SO_{4}^{2-}$ does not.

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(A) $SO_{3}^{2-}$ and $SO_{4}^{2-}$ ions react with $BaCl_{2}$ to form white precipitates of $BaSO_{3}$ and $BaSO_{4}$ respectively.$Ba^{2+} + SO_{3}^{2-} \longrightarrow BaSO_{3} (s)$ (White precipitate)$Ba^{2+} + SO_{4}^{2-} \longrightarrow BaSO_{4} (s)$ (White precipitate)$BaSO_{3}$ is a salt of a weak acid $(H_{2}SO_{3})$, so it dissolves in dilute $HCl$ due to the formation of $SO_{2}$ gas.$BaSO_{3} + 2HCl \longrightarrow BaCl_{2} + H_{2}O + SO_{2} \uparrow$$BaSO_{4}$ is a salt of a strong acid $(H_{2}SO_{4})$ and is insoluble in dilute $HCl$.

Among the following observations, the correct one that differentiates between $SO_{3}^{2-}$ and $SO_{4}^{2-}$ is:

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