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: Copper (I) ions in aqueous solution react with 0.56 M NH 3 (aq) according toCu+ (aq) + 2 NH3 (aq) → Cu(NH3)2+ (aq)      Calculate the solubility in g. Note: Kf = 6.3 x 10 10 and Copper (I) ions come f

Problem

Copper (I) ions in aqueous solution react with 0.56 M NH (aq) according to

Cu(aq) + 2 NH(aq) → Cu(NH3)2(aq)      

Calculate the solubility in g. Note: Kf = 6.3 x 10 10 and Copper (I) ions come from Copper (I) bromide.

Solution

The solubility of CuBr is:

$CuBr (s) \rightleftharpoons Cu+ (aq) + Br – (aq)$

The solubility product $Ksp = 6.3 \times 10^{-9}$

The expression would then be:

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