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: Butyric acid is responsible for the foul smell of rancid butter. The pKa of butyric acid is 4.84.Calculate the pH of a 5.0×10−2 M solution of sodium butyrate.

Solution: Butyric acid is responsible for the foul smell of rancid butter. The pKa of butyric acid is 4.84.Calculate the pH of a 5.0×10−2 M solution of sodium butyrate.

Problem

Butyric acid is responsible for the foul smell of rancid butter. The pKa of butyric acid is 4.84.

Calculate the pH of a 5.0×10−2 M solution of sodium butyrate.

Solution

We’re being asked to calculate the pOH of a 5.0×10−2 M sodium butyrate solution.


Since we don't really need to know the composition of butyric acid, we'll assign it as just HA. 

So sodium butyrate is NaA which is just the salt form of the conjugate base.

The salt dissociates in solution as:

 NaA → Na+(aq) + A-(aq)

So we effectively have a weak base in the solution.


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