CHEM 1A03 Lecture Notes - Lecture 8: Buffer Solution, Ammonia

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

Document Summary

A mixture of a conjugate acid-base pair that maintains a nearly constant ph when diluted with a strong acid or base. A buffered solution is one that resists a change in its ph when either a hydroxide or protons are added. One important natural buffer is blood which can absorb the acids and bases produced by biological reactions without changing the ph (contains hco3 and h2co3). It can contain a weak acid and its salts ( hf and naf) or a weak base and its salt (nh3 and nh4cl) How does a buffered solution resist changes in ph when an acid or a base is added. (aq) + h+ (aq) hc2h3o2 (aq). Use bronsted -lowry equation for acid base reaction. Example: addition of naoh to a buffer of acetic acid-acetate ion buffer would have the following equation. Hc2h3o2 (aq) + oh- (aq) c2h3o2 - (aq) + h2o (l)