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: Trimethylamine, N(CH3)3, is the molecule that is responsible for the “fishy smell” of seafood. It has a Kb of 6.3 x 10 -5, making it a moderately-strong weak base.   A. Write a balanced chemical equation showing how N(CH 3)3 acts as a weak base in water.   B. Now consider the ionic compound HN(CH 3)3Cl, formed by reacting N(CH3)3 with HCl. In water, HN(CH3)3Cl separates into HN(CH3)3+(aq) and one of our favorite spectator ions, Cl -(aq). Calculate the pH of 0.18 M HN(CH 3)3Cl.     1. Write a balanced chemical equation for the acid-base reaction your calculation is based on. You do not need to include Cl‒(aq) because it is a spectator.         2. Determine the pH of this solution.         3. Is the pH you calculated consistent with the chemical equation you wrote for Part B.1?

Problem

Trimethylamine, N(CH3)3, is the molecule that is responsible for the “fishy smell” of seafood. It has a Kb of 6.3 x 10 -5, making it a moderately-strong weak base.

 

A. Write a balanced chemical equation showing how N(CH 3)3 acts as a weak base in water.

 

B. Now consider the ionic compound HN(CH 3)3Cl, formed by reacting N(CH3)3 with HCl. In water, HN(CH3)3Cl separates into HN(CH3)3+(aq) and one of our favorite spectator ions, Cl -(aq). Calculate the pH of 0.18 M HN(CH 3)3Cl.

 

 

1. Write a balanced chemical equation for the acid-base reaction your calculation is based on. You do not need to include Cl(aq) because it is a spectator.

 

 

 

 

2. Determine the pH of this solution.

 

 

 

 

3. Is the pH you calculated consistent with the chemical equation you wrote for Part B.1?