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: Which of the following compounds precipitates from a solution that has the concentrations indicated? (See Appendix J for Ksp values.)(a) KClO4: [K+] = 0.01 M, [ClO4−] = 0.01 M(b) K2PtCl6: [K+] = 0.01

Problem

Which of the following compounds precipitates from a solution that has the concentrations indicated? (See Appendix J for Ksp values.)

(a) KClO4: [K+] = 0.01 M, [ClO4] = 0.01 M
(b) K2PtCl6: [K+] = 0.01 M, [PtCl62−] = 0.01 M
(c) PbI2: [Pb2+] = 0.003 M, [I] = 1.3 x 10–3 M
(d) Ag2S: [Ag+] = 1 x 10–10 M, [S2–] = 1 x 10–13 M