We are being asked to identify the precipitate. We will refer to the solubility rules in order to determine if it is an insoluble salt (precipitate) or not.
•Soluble Ionic Compounds:
▪ Group 1A ions (Li+, Na+, K+, etc.) and Ammonium ion (NH4+) are soluble
▪ Nitrates (NO3-), Acetates (CH3COO- or C2H3O2-), and most Perchlorates (ClO4-) are soluble
▪ Cl-, Br-, and I- are soluble except when paired with Ag+, Pb2+, Cu+, Hg22+
▪ Sulfates (SO42-) are soluble except those of Ca2+, Sr2+, Ba2+, Ag+, and Pb2+
•Insoluble Ionic Compounds:
▪ Hydroxides (OH-) and Sulfides (S2-) are insoluble except when with Group 1A ions (Li+, Na+, K+, etc.) and ammonium ion (NH4+) and Ca2+, Sr2+, Ba2+
▪ Carbonates (CO32-) and Phosphates (PO43-) are insoluble except when with Group 1A ions (Li+, Na+, K+, etc.) and ammonium ion (NH4+)
For each reaction, identify the precipitate or lack thereof
CaCl2 (aq) + K2CO3 (aq) → CaCO3 + 2 KCl
c. no precipitate
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