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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
Intro to Buffers
Henderson-Hasselbalch Equation
Intro to Acid-Base Titration Curves
Strong Titrate-Strong Titrant Curves
Weak Titrate-Strong Titrant Curves
Acid-Base Indicators
Titrations: Weak Acid-Strong Base
Titrations: Weak Base-Strong Acid
Titrations: Strong Acid-Strong Base
Titrations: Diprotic & Polyprotic Buffers
Solubility Product Constant: Ksp
Ksp: Common Ion Effect
Precipitation: Ksp vs Q
Selective Precipitation
Complex Ions: Formation Constant

Complex Ion is a structure containing a metal cation that acts as a Lewis Acid.

Concept #1: Complex Ion and Ligand

Formation Constant (Kf): a ratio of product to reactant concentrations.

Example #1: The formation of the complex ion created from the combining of silver ion and cyanide ion is given below: 

                                     Ag+ (aq) + 2 CN (aq) ⇌ Ag(CN)2 (aq)  Kf = 1.0 x 1021

If 100.0 mL of 0.0120 M AgClO4 is mixed with 220.0 mL of 0.25 M CN, what is the [Ag+] once equilibrium has been reached? 

Practice: If your equilibrium constant K is equal to the product of Ksp and Kf, find the solubility of AgCl in 2.0 M NH3. Ksp of AgCl = 1.77 × 1010; Kf of Ag(NH3)2+ = 1.7 × 107.

Practice: A solution is composed of 3.20 × 104 M Co(NO3)3 mixed with 0.200 M NH3. Determine the [Co3+] that remains once the solution reaches equilibrium in the formation of Co(NH3)63+.