Ch.16 - Aqueous Equilibrium See 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: The question below pertains to a titration where 0.30 M HNO 3 (in a buret) is added to 60.0mL of 0.40 M trimethylamine, (CH 3)3N (in the flask). How is the solution in the flask best characterized after 50. mL of the HNO 3 solution has been added? This is before equivalence point of the titration. (a) the solution is now a weak base (b) the solution is now a weak acid (c) the solution is now a strong base (d) the solution is now a strong acid (e) it is now a neutral solution (f) it is now a buffer solution

Problem

The question below pertains to a titration where 0.30 M HNO 3 (in a buret) is added to 60.0mL of 0.40 M trimethylamine, (CH 3)3N (in the flask).

How is the solution in the flask best characterized after 50. mL of the HNO 3 solution has been added? This is before equivalence point of the titration.

(a) the solution is now a weak base

(b) the solution is now a weak acid

(c) the solution is now a strong base

(d) the solution is now a strong acid

(e) it is now a neutral solution

(f) it is now a buffer solution