CHEM 1A03 Lecture Notes - Lecture 7: Lone Pair, Carboxylic Acid, Conjugate Acid

• School: McMaster University
• Department: Chemistry
• Course: CHEM 1A03
• Professor: Lydia Chen

Document Summary

Equilibrium between water and the hydronium & hydroxide ions; water is amphoteric (behaving as both acid and base) Kw = [h3o+][oh-] = 1. 0 10-14 at 25 c. Pkw = ph + poh = 14. Acids: ionize in water to generate proton (h+) Bases: ionize in water to produce hydroxide ions (oh-) Acid-base reaction: neutralization of an aqueous proton. Only applicable to protic acids and metal hydroxides in water. Excludes species e. g. bf3 or nh3. Every a-b reaction has an a + b as reactants, and conjugate a + b as products. Difference between a and conjugate b is loss of one proton/h+ Reactions proceed away from stronger a + b toward weaker conjugate a + b. Stronger acid, weaker conjugate base relative to one another. Describes a + b in aqueous and non-aqueous solvents. Distinguish between systems that form true equilibria vs those that proceed almost entirely toward product. Strength = measure of how much species ionizes.