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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

Comparing Ksp value to Q value determines if a precipitate is likely to form.

Concept #1: Solution Saturation

Relative values of Ksp vs Q determine the degree of solution saturation.

Example #1: Will BaSO4 precipitate out when 8.2 x 10-7 M BaCO3 is mixed with 5.7 x 10-6 M SrSO4? Ksp of BaSO4 is 1.1 x 10-10.

Practice: Two mixtures are added into one flask at 25 °C, one mixture contains 0.55 mL of 0.75 M BaF2 and another 0.25 mL of 1.3 M Mg(OH)2. Ksp of Magnesium Fluoride, MgF2, is 7.4 x 109. Identify the correct option.

a) MgF2 solid will form

b) MgF2 solid forms, along with Mg+2 and F ions

c) solution is unsaturated, precipitate does not form

d) solution is saturated, precipitate forms