CHE 8A Lecture Notes - Lecture 3: Acid Strength, Lone Pair, Conjugate Acid
Document Summary
Relative acid strengths - pka + strengths. Acids = donate h+ in h20; have h+ in formula. Bases = donate oh- in h2o; have oh- in formula. Naoh, koh, ca(oh)2, nh4oh* (*doesn"t actually have oh) Organics don"t like h2o and some things don"t fit. And other stuff outside of water reactions. And anything that has extra e- (anything with a lone pair) Acids = accept electron pair into empty orbital. Bases = donate lone pair into empty orbital. Small # = donates lots of h+ (good acid) Large # = keeps h+ (bad acid) Neutralization conjugate pairs play pass the proton . Hcl + h2o cl- + h3o+ Acid + base base + acid. Stronger acid forces weaker acid to take the h+ (proton) Organics will look at strength not dissociation. Measure acid strength by how well it donates h+: Ka = [h3o+][a-] / [ha] = acid dissociation constant. Ha + h2o a- + h3o+
