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: What is the solubility of M(OH) 2 in a 0.202 M solution of M(NO 3)2? Ksp = 9.05 x 10 -18

Solution: What is the solubility of M(OH) 2 in a 0.202 M solution of M(NO 3)2? Ksp = 9.05 x 10 -18

Problem

What is the solubility of M(OH) 2 in a 0.202 M solution of M(NO 3)2? Ksp = 9.05 x 10 -18

Solution

 M(OH) has a Ksp, which stands for the solubility product constant. That means that  M(OH) 2 is a solid and it will dissociate as follows

 M(OH)2(s)  M2+ + 2OH– {aq}

Anytime we deal with Ksp, we are dealing with an ICE chart. Remember, in ICE charts we ignore anything that is a solid or a liquid, meaning we will ignore M(OH) 2.

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