We’re being asked to determine which of the given reactions are the precipitation and non-precipitation reactions. Recall that in a precipitation reaction, a solid is formed as a product (precipitate).
For this problem, we need the solubility rules:
• 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
• Halides (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.), ammonium ion (NH4+), Ca2+, Sr2+, and Ba2+
• Carbonates (CO32–) and Phosphates (PO43–) are insoluble except when with Group 1A ions (Li+, Na+, K+, etc.) and ammonium ion (NH4+)
Identify the precipitation and non-precipitation reactions
a. 4P + 5O2 → 2P2O5
b. H2O2 + NaIO → NaI + H 2O + O2
c. Ba(NO3)2 + MgSO4 → BaSO4 + Mg(NO3)2
d. Hg2(C2H3O2)2 + 2NaBr → Hg 2Br2 + 2NaC2H3O2
e. 2KI + Pb(NO3)2 → PbI2 + 2KNO3
f. HCI + NaOH → NaCI + H 2O
g. HBr + NaOH → NaBr + H 2O
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