CHM 2354 Lecture Notes - Lecture 7: Acid Dissociation Constant, Equilibrium Constant, Rice Chart
Document Summary
Weak acids and bases do not completely dissociate. Ka, the dissociation for the acid ha is. Kb, the dissociation for the acid ha is pk is the negative logarithm of the equilibrium. The higher the pka, the lower the ka, but pk are simpler to write. Conjugate acid-base pairs are related by the gain or loss of a proton. A weak" makes a weak" and a strong" makes a very weak because it dissociates completely. Any effect that increases the stability of the product drives the reaction forward. A lower pka means it is more stable (higher ka). A higher pka means it is less stable (lower ka). Unlike with concentrated strong acid we need to account for water ionization. Find the ph for a solution of a general weak acid ha is below 1. 0 x 10-8 constant. (ka. The [h+] represents the protons from both sources: f is the total ph (dissociated + non dissociated)