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On adding 0.1 M solution each of [Ag^(+)], [Ba^(2+)], [Ca^(2+)] in a Na_(2)SO_(4) solution, species first precipitated is [K_(sp) BaSO_(4) = 10^(-11), K_(sp)CaSO_(4) = 10^(-6), K_(sp)Ag_(2)SO_(4) = 10^(-5)] Least solubility is of BaSO_(4), hence it will precipitate first. |
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Answer» `Ag_(2)SO_(4)` `= 3.16 xx 10^(-6)` mol/L. Solubility of `CaSO_(4)(x) = sqrt(K_(sp)) = sqrt(10^(-6))` `= 1.0 xx 10^(-3)` mol/L. Solubility of `Ag_(2)SO_(4) = 3sqrt((K_(sp))/(4))` (`because` for `Ag_(2)SO_(4), 4x^(3) = K_(sp)`) `= 3sqrt((10^(-5))/(4)) = 1 xx 10^(-2)` mol/L |
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