Ch.14 - Chemical EquilibriumWorksheetSee 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: When excess PbCl2 is dissolved in 1.00 L of water, 0.032 mol of Cl − forms at equilibrium. What is the Kc of the reaction: PbCl2 (s) ⇌ Pb2+ (aq) + 2 Cl − (aq) Kc = ? A. 1.0x10−3 B. 1.3x10−4 C. 3.3

Problem

When excess PbCl2 is dissolved in 1.00 L of water, 0.032 mol of Cl  forms at equilibrium. What is the Kc of the reaction:

PbCl2 (s) ⇌ Pb2+ (aq) + 2 Cl  (aq) Kc = ?

A. 1.0x10−3

B. 1.3x10−4

C. 3.3x10−5

D. 1.6x10−5