CHEM 1A03 Lecture Notes - Lecture 6: Hypobromous Acid, Svante Arrhenius, Lone Pair

• School: McMaster University
• Department: Chemistry
• Course: CHEM 1A03
• Professor: David Brock

Document Summary

Acid-base chemistry: water shows amphoteric properties b/c it acts as an acid and base, kw= [h3o+][oh-]=1 10-14 at 25 c. Svante arrhenius: acid: ionizes/dissociates in water to produce h+ ions. Hcl(aq) h+(aq) + cl-(aq: base: ionizes in water to produce oh- ions. Naoh(aq) na+(aq) +oh-(aq: acid-base reaction: neutralization of an aq proton with a hydroxide ion. *only includes protic acids and metal hydroxides not bf3 or nh3. Bronsted-lowry: acid: proton donor, base: proton acceptor. Lewis theory: acid: electron pair acceptor, base: electron pair donor. *encompasses all theories and describes acids and bases in aq and non-aq solvents as well as unusual non-protic acid systems. Strong acids and bases: strong acid reacts with strong base and reaction moves to weaker side, the stronger the acid the weaker the conjugate base, sa+sb have a high k value b/c completely dissociate and reaction favours products. Strong acids (cooh groups: hcl, hi, hbr, h2so4, hclo4, hno3.