BIO 12 Acid base Reactions Summary

4/21/2020




Acid-Base Balance
for Allied Health Majors
Using the Henderson-Hasselbach Equation
Chapter 30 (12th ed.), Chapter 31 (13th ed.)




HCO3 - α =0.03
pH = pK + log
pCO 2 (α)



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Outline
I. Acids and bases

II. Buffering systems

III. Compensation for deviation

IV. Practice problems

V. Anion gap

VI. Clinical correlation: Abuse of diuretics or Conn’s
disease

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I. Acids and Bases
ACID: a substance that will disassociate a H+ and become
more negatively charged (electron acceptor).
•When hydrogen ions accumulate in a solution, it becomes more
acidic ([H+] increases = more acidity).




HCl

2 7
H+ Cl-
H+ Cl-
pH
H+ Cl-
H+ Cl-
H+ Cl-
Hydronium ions in solution
Concentration of hydrogen ions
increases, pH drops



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, 4/21/2020




I. Acids and Bases
BASE: a chemical that will remove hydrogen ions from the
solution
•The base has a negative charge (or extra electrons) to donate
to hydrogen ions and thus create a bond with hydrogen




2 7
NaOH Na+ OH-
H+ Cl-
H+ Cl-
Na+ OH- pH
H+ Cl-
Acids and basis
H+ Cl- Na+ OH-
neutralize eachother
H+ Cl-
Na+ OH-




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A change of 1 pH unit corresponds to
a 10-fold change in hydrogen ion
concentration




2 7


Na+ Cl-
Na+ Cl- pH


H+ OH- H2O


Na+ Cl-
Na+ Cl-




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Acids are being created constantly
through metabolism
• Inorganic phosphates (mostly from ATP,
etc.)
• Anaerobic respiration of glucose produces
lactic acid
• Fat metabolism yields organic acids and
ketone bodies
• Carbon dioxide ultimately causes H+ to be
released from carbonic acid (see slide 8)




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