Ch.15 - Acid and Base EquilibriumWorksheetSee 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: Calculate the pH of a 0.10 M solution of barium hydroxide, Ba(OH)2.

Solution: Calculate the pH of a 0.10 M solution of barium hydroxide, Ba(OH)2.

Problem

Calculate the pH of a 0.10 M solution of barium hydroxide, Ba(OH)2.

Solution

Barium hydroxide, $BaOH_2$, is a strong base. Remember that when we have a strong acid or strong base, we do not need an ICE chart to find the pH. All that needs to be done is take the –log to find either pH or pOH. Because we are dealing with a strong base, we will find pOH first.

One tricky thing about strong bases is that we need to find the correct concentration. We must count the number of moles of $OH^-$ to make sure we find the correct pH in the end. Notice the dissociation:

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