Lecture 6
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Buffers
solutions that resist pH changes Act by neutralizing added acid or base Made by preparing a solution of a weak acid/base and the salt of its conjugate acid/base
Henderson-Hasselbalch Equation
Used to calculate pH of buffer solution
In the Henderson-Hasselbalch Equation, if A and B are equal…
pH=pKa This is a buffer equally prepared to neutralize acids and bases
H+/OH- catalyze what?
hydrolysis/condensation reactions
pH affects?
the charge on an enzyme its shape ability to function
Forms of dissolved CO2 steps
• dissolved CO2 forms carbonic acid H2CO3 • Carbonic acid then forms the bicarbonate ion HCO3- • Bicarbonate can go on to form carbonate ion CO32-
Removal of CO2 by the lungs does what?
shifts this reaction to the left (by Le Chateliers Principle) reducing carbonic acid and raising pH
Respiratory Acidosis/ Alkalosis
Acidosis /alkalosis due to breathing problems (removal of CO2)
Metabolic Acidosis or Alkalosis
Acidosis or alkalosis due to metabolic problems (diarrhea/vomiting, ketoacidosis, or kidneys problems)
pH Compensation
If one of the two modes of pH regulation fails, the other will try to Compensate
Partial compensation
pH is not returned to the reference range: 7.35-7.45
What is the normal body pH range?
7.35-7.45
Full compensation
pH is returned to the reference range: 7.35-7.45
Vomiting
Vomiting removes stomach acid Raises pH, metabolic alkalosis
Diarrhea
causes loss of bicarbonate Lowers ph, metabolic acidosis
Respiratory acidosis
Reduced CO2elimination
Respiratory alkalosis
increase CO2 elimination