Molecular views of the reactant solutions for a precipitation reaction are shown below
(with ions represented as spheres and water molecules omitted):
(a) Which compound is dissolved in beaker A: Li2CO3, NH4Cl, Ag2SO4, or FeS?
(b) Which compound is dissolved in beaker B: Ni(OH)2, AgNO3, CaCl2, or BaSO4?
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Answer:
(a) Li2CO3 is dissolved in A
(b)CaCl2 is dissolved in B
Explanation:
in beaker A , Ag2SO4 is a white precipitate sobit cannot be dissolved , FeS is a black precipitate so it cannot be dissolved , NH4+ has a 1+ charge while in image it is shown a 2+ charge so NH4Cl cannot be dissolved while it still is soluble
in beaker B , Ni(OH)2 is a white precipitate so it cannot be dissolved , AgNO3 is soluble but Ag1+ has 1+ charge while in image it is shown a 2+ charge , BaSO4 is soluble but SO42- has 2- charge while in image it is shown a -1 charge
Upon mixing Li2CO3 and CaCl2 a white precipitate of CaCO3 is formed
Li2CO3 + CaCl2 - CaCO3 + LiCl hence the spectator ions would be Li+ and Cl-
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