CHEM102 Lecture Notes - Acid Dissociation Constant, Conjugate Acid, Acid Strength

• School: University of Alberta
• Department: Chemistry
• Course: CHEM102
• Professor: Sai Yiu

Document Summary

Br nsted-lowry definitions: an acid-base reaction is a proton transfer process. Acid: proton (h+, h3o+) donor during acid-base reaction. An acid must therefore contain h in its formula. Hence, a base must contain lone pair of electrons in formula so to form a bond with the hydrogen ion. + (aq) + oh- (aq) (cid:1) nh3 (aq) + h2o (l) nh4. +, the product from nh3 becomes an acid and oh-, the product from h2o. Hcl (aq) + h2o (l) (cid:1) h3o+ (aq) + cl- (aq) Acid h = conjugate base (increase one negative charge) Base + h = conjugate acid (less one negative charge) Therefore, every acid has a conjugate base and every base has a conjugate acid. Give the conjugate acid for the following base: Give the conjugate base for the following acid: Every acid-base reaction has two conjugate acid-base pairs. For example: nh3 (aq) + h2o (l) (cid:1) nh4 stronger base stronger acid weaker acid weaker base.