CHEM102 Lecture Notes - Lecture 14: Buffer Solution, Conjugate Acid, Weak Base

• School: University of Alberta
• Department: Chemistry
• Course: CHEM102
• Professor: Camille Bowen-Forbes

Document Summary

Common ion effect and buffer solutions: buffer systems: Chemical reactions sensitive to ph: common ion effect: Presence of common ion causes a substance to ionise less than it normally would. A given ion is added to an equilibrium that already contains the ion and the position of equilibrium shifts away from forming it. Percent dissociation of acid and base decreases: acid-base buffers: Lessens the impact of ph from addition of acid or base. Solution of weak acid and conjugate base. Solution of a weak base and its conjugate acid. Effect up to +/- 1 ph unit of buffer ph. Buffer components can consume small amount of acid or base by a shift in equilibrium position. Equal amounts of acid and conjugate base give the optimum buffer. Optimum buffer: greatest resistance to ph change: buffer capacity: Measure of the strength of the buffer. Ability to maintain ph followed by the addition of string acid or base.