1. D. C. Mikulecky

2.  CHEMICAL COMPOUNDS CAN BE PROTON DONORS OR ACCEPTORS  PROTON DONORS ARE ACIDS  PROTON ACCEPTORS ARE BASES  ACIDS AND BASES REACT TO NEUTRALIZE EACH OTHER FORMING SALTS

3. HCl + NaOH NaCl + H 2 O ACID + BASE SALT + WATER

4. AcidicAlkaline (Basic) [OH - ] [H + ] Neutral pH 014 7 AcidosisAlkalosis Normal 7.35-7.45 Venous Blood Arterial Blood 6.8 8.0 7.4

5. H 2 CO 3 HCO 3 - H + Na + Cl - Add HCl Na + Cl - H + Cl - Unbuffered Salt Solution All protons are free H 2 CO 3 : HCO 3 - Buffer Add HCl H 2 CO 3 HCO 3 - + H + Protons taken up as Carbonic Acid

6.  Weak acid/salt systems act as a “sponge” for protons  As acidity tends to increase they take protons up  As acidity tends to decrease they release protons

7.  Carbonic acid/Bicarbonate: Primary buffer against non-carbonic acid changes  Proteins: Primary ICF buffer, also ECF  Hemoglobin: Primary buffer against carbonic acid changes  Phosphate: Urinary buffer, also ICF

8.  Alterations in ventilation alter the rate of excretion of carbon dioxide  Alterations in the rate of carbon dioxide excretion cause alterations in pH through carbonic acid  This way the respiratory system can help control non-respiratory acidosis and alkalosis

9.  Metabolic: Severe diarrhea, Diabetes mellitus, strenuous exercise, uremia  Respiratory: hypoventilation

10.  Metabolic: Vomiting, ingestion of alkaline drugs  Respiratory: hyperventilation

11.  Proton excretion  Bicarbonate excretion  Ammonia secretion