Ch.16 - Aqueous Equilibrium WorksheetSee 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: Consider the solubility of lead (II) chloride, The equilibrium constant, Ksp, is 1.2 × 10−5. If 100 mL each of 0.02 M KCl and 0.02 M Pb(NO3)2, both strong electrolytes, are mixed together, what will take place? 1. A precipitate of PbCl2 would form. 2. No precipitate would form. 3. There is not enough information. 4. A precipitate of KNO3 would form.

Problem

Consider the solubility of lead (II) chloride,

The equilibrium constant, Ksp, is 1.2 × 10−5. If 100 mL each of 0.02 M KCl and 0.02 M Pb(NO3)2, both strong electrolytes, are mixed together, what will take place?

1. A precipitate of PbCl2 would form.

2. No precipitate would form.

3. There is not enough information.

4. A precipitate of KNO3 would form.