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

Solution: Consider the following four titrations (i–iv):i. 150 mL of 0.2 M NH 3 (Kb = 1.8 x 10 -5) by 0.2 M HClii. 150 mL of 0.2 M HCl by 0.2 M NaOHiii. 150 mL of 0.2 M HOCl (K a = 3.5 x 10 -8) by 0.2 M NaOHiv.

Problem

Consider the following four titrations (i–iv):

i. 150 mL of 0.2 M NH 3 (Kb = 1.8 x 10 -5) by 0.2 M HCl
ii. 150 mL of 0.2 M HCl by 0.2 M NaOH
iii. 150 mL of 0.2 M HOCl (K a = 3.5 x 10 -8) by 0.2 M NaOH
iv. 150 mL of 0.2 M HF (K a = 7.2 x 10 -4) by 0.2 M NaOH

a. Rank the four titrations in order of increasing pH at the halfway point to equivalence (lowest to highest pH).