BIOL-242 Lecture Notes - Lecture 38: Peripheral Chemoreceptors, Buffer Solution, Sodium Bicarbonate
9 Jun 2020
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Chapter 26 part 2 | acids and bases. Chemical buffer: system of one or more compounds that act to resist ph changes when strong acid or base is added. Bind h+ if ph drops; release h+ if ph rises: bicarbonate buffer system, phosphate buffer system, protein buffer system. Mixture of h2co3 (weak acid) and salts of hco3 (e. g. , nahco3, a weak base) Co2 + h2o h2co3 h+ + hco3 . During co2 unloading reaction shifts to left (and h+ incorporated into h2o) During co2 loading reaction shifts to right (and h+ buffered by proteins) More co2 is removed from the blood. Effective buffer in urine and icf, where phosphate concentrations are high. Intracellular proteins are most plentiful and powerful buffers; plasma proteins also important. Protein molecules are amphoteric (can function as both weak acid and weak base) When ph rises, organic acid or carboxyl (cooh) groups release h+ When ph falls, nh2 groups bind h+ hemoglobin functions as intracellular buffer.
