01:160:162 Lecture Notes - Lecture 12: Equilibrium Constant, Chief Operating Officer, Molar Mass
Document Summary
A buffer contains both an acid together with its conjugate base, both present in appreciable. Compare three related, but different solutions, and calculate ph of each solution. = 1. 8 x 10-5 ph = - log (0. 0030) = 2. 52. Solving: x = [h3o+] = [ch3coo-] = 0. 0030 m. There is a small amount (0. 0030 m) acetate ion present with the 0. 50 m acetic acid. The ratio of acetic acid/acetate ion is very far from 1:1, and the acetate ion concentration is very small. The acetate ion is the conjugate base of acetic acid. = kb = 5. 6 x 10-10 x = [oh-] = [ch3cooh] = 1. 3 x 10-5 poh = -log (1. 3 x 10-5) = 4. 89 ph = 14. 00 - 4. 89 = 9. 11. There is a small amount (1. 3 x 10-5 m) acetic acid present with the 0. 30 m acetate ion. The ratio of acetic acid/acetate ion is very far from 1:1, and the acetic acid concentration is very small.
