BCHM 102 Lecture Notes - Lecture 3: Isoelectric Point, Sodium Hydroxide, Alanine
2 Dec 2016
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Define acid, base, ph and pka and how they apply to biochemical molecules. Explain the behaviour of weak acids and bases in solution using the henderson-hasselbalch equation and titration curves. Describe buffers, such as amino acids, and their importance to biological systems. In aqueous solution (water: acids are proton (h+) donors - they give up protons easily, bases are proton (h+) acceptors - takes protons from wherever it can get them. Strong acids dissociate completely into a proton and a weak conjugate base. Hcl --> h+ + oh- (dissociates into proton and ion) Strong bases ionize to release a powerful proton acceptor. Naoh --> na+ + oh- (dissociates into proton and ion) ph ph = -log [h+] The higher the [h+] the lower the ph. Low ph means acidic (high protons), high ph means basic (low protons) Most physiological reactions occur between 6. 5 and 8. Exist in equilibrium between weak acid (ha), dissociate proton (h+), and conjugate base (a-)
