Ch.4 - Chemical Quantities & Aqueous ReactionsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: Identify the precipitation and non-precipitation reactionsa. 4P + 5O2 → 2P2O5b. H2O2 + NaIO → NaI + H 2O + O2c. Ba(NO3)2 + MgSO4 → BaSO4 + Mg(NO3)2d. Hg2(C2H3O2)2 + 2NaBr → Hg 2Br2 + 2NaC2H3O2e. 2KI +

Solution: Identify the precipitation and non-precipitation reactionsa. 4P + 5O2 → 2P2O5b. H2O2 + NaIO → NaI + H 2O + O2c. Ba(NO3)2 + MgSO4 → BaSO4 + Mg(NO3)2d. Hg2(C2H3O2)2 + 2NaBr → Hg 2Br2 + 2NaC2H3O2e. 2KI +

Problem

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

Solution

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+)


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