LSCI 211 Lecture Notes - Lecture 3: Equilibrium Constant, Conjugate Acid, Ph
28 Aug 2016
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Document Summary
Ionization of water at equilibrium is described by the equilibrium constant. Hydrogen ion concentration ph = -log[h+] ph and poh always adds to 14. The acid dissociation constant: ka = [h+][base] / [acid] We can rearrange and solve for [h+] to determine ph. Ka = [h+][a-]/[ha] pka = -logka ph= pka log [ha]/[a-] Biological systems: ph affects biological activity and molecules. Co2 emissions are decreasing ph in the environment. Increase in ocean acidity is bleaching coral reefs. Buffer system consists of a weak acid and its conjugate base. The ph at which there is an equal concentration of acid and base. Buffers are functional 1 unit above or below their pka. The isoelectric point (pi) is in the middle of 2 pkas. Diprotic acids can give and take up to 2 protons.
