We will refer to the solubility rules in order to determine if the product form would be 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+)
A) Pb(NO3)2(aq) + KCl(aq)
• Pb(NO3)2(aq) → aqueous → will break up into its ions
▪ Pb2+ → metal
▪ NO3- → polyatomic anion
Complete and balance each of the following equations. Remember to put states of matter.
Pb(NO3)2(aq) + KCl(aq)
NaCl(aq) + Mg(C2H3O2)2(aq)
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