CHE 2B Lecture Notes - Lecture 10: Conjugate Acid, Amphoterism, Acid Strength

• School: UC-Davis
• Department: Chemistry
• Course: CHE 2B
• Professor: undefined

Document Summary

Acids and bases: the concept of equilibrium applies also to an h+ and an. Oh- in a solution: in an aqueous solution h+ is not free but it forms a hydronium ion h3o+ Arrhenius definition of acid and base: an acid is capable to yield an h+ in a water solution, a base is able to yield an oh- in a water solution, but what about nh3. Br nsted-lowry acid: an acid is a proton h+ donor, gas phase reaction in vacuum, aqueous environment include h2o. Hcl(g) h+(g) + cl-(g: strong acid <= large kc, weak acid <= small kc, a base is a proton h+ acceptor, strong acid <= large kc. O2-(aq) +h2o(l) 2oh-(aq: weak acid <= small kc. Water is amphiprotic: water performs autoprotolysis, 2h2o h3o+ + oh, equilibrium constant is: Examples: what are the concentrations of h3o+ and oh- in a 1. 3x10- = 7. 692x10-12: what are the concentrations of h3o+ and oh- in a 4. 5x10-