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: a. Use the molar solubility 1.08 x 10 -5 in pure water to calculate Ksp for BaCrO4. b. Use the molar solubility 1.55 x 10 -5 in pure water to calculate Ksp for Ag2SO3. c. Use the molar solubility 2.22 x 10 -8 in pure water to calculate Ksp for Pd(SCN)2.

Problem

a. Use the molar solubility 1.08 x 10 -5 in pure water to calculate Ksp for BaCrO4.

b. Use the molar solubility 1.55 x 10 -5 in pure water to calculate Ksp for Ag2SO3.

c. Use the molar solubility 2.22 x 10 -8 in pure water to calculate Ksp for Pd(SCN)2.