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: Three cations, Ni2+, Cu2+, and Ag+, are separated using two different precipitating agentsBased on Figure 17.22 in the textbook, what two precipitating agents could be used?

Solution: Three cations, Ni2+, Cu2+, and Ag+, are separated using two different precipitating agentsBased on Figure 17.22 in the textbook, what two precipitating agents could be used?

Problem

Three cations, Ni2+, Cu2+, and Ag+, are separated using two different precipitating agents

1. Mixture of cations A, B, and C in test tube. 2. Add first precipitating agent.  Cation A is removed as precipitate, B and C remain in solution 3. Decant liquid.  Only cations B and C remain. 4. Add second precipitating agent.  Cation B is removed as precipitate, cation C remains in solution. 5. Decant liquid.  Only cation C remains.

Based on Figure 17.22 in the textbook, what two precipitating agents could be used?

Solution

Establish the solubility rules and determine which ion can be used to separate NI2+, Cu2+ and Ag+

Recall that the Solubility Rules are:

Soluble Ionic Compounds:

Group 1A ions (Li+, Na+, K+, etc.) and Ammoniumion (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+

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