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pH regulation
Blood pH
• pH = measure of hydrogen ion concentration
• pH = -log [H+]
• Blood pH = 7.35-7.45
• pH imbalances are quickly lethal body needs to compensate
• H+ intake:
- food
- drink
- metabolism (carbohydrate, protein, lipid)
- breathing
• H+ output
- urine
Figure 19.23
pH regulation
• Three lines of defense:- Buffers- Respiration- Kidneys
• Buffer reactions are nearly instantaneous. However, they are limited to the amount of buffer available in the blood
• Respiration helps buffer the blood by shifting H+ into HCO3-. However, it can be limiting and take several minutes
• Kidneys are the only organ which can get rid of H+. However, they can take several hours (time enough to be dead!!- therefore, the presence of the other 2 lines of defense)
pH regulation
• Three lines of defense:
- Buffers
- Respiration
- Kidneys
First line of defense: Buffers
• Buffers:
- protein buffer
- bicarbonate buffer
- phosphate buffer
Only free H+ contributes to pH
H+ can be shifted from a strong acid to a weaker one.
• Strong acid complete dissociation
• (100) HCl (100)H+ + (100) Cl-
• Weak acid • (100) H2CO3 (80) H2CO3 +
(20) H+ + (20) HCO3-
pH regulation
• If strong acid intake:
• H+ + Cl- + ( blood Na+ HCO3-)
Na+ Cl- + H+ + HCO3-
• Less H+ is circulating into the blood - smaller shift toward acidosis
• If strong base intake:
• Na+ OH- + (blood H2 CO3) H2O
+ Na+ HCO3-
• Less OH- is circulating in the blood smaller shift toward alkalosis
Second line of defense: breathing
• Three lines of defense:
- Buffers
- Respiration
- Kidneys
CO2 + H2O H2CO3 H+ + HCO3-
• CO2 retention: ↑ blood H+ ↓ pH acidosis
• CO2 loss:• ↓ blood H+ pH ↑ alkalosis
Figure 17.22
Figure 19.24
Third line of defense: kidneys
• Three lines of defense:
- Buffers
- Respiration
- Kidneys
• Kidneys are the only organs able to eliminate H+ from the body slow process
• H+ can be bound to HCO3-
for transport to the bladder and eliminated
• H+ can be added to NH3 to make ammonia (NH4
+) and eliminated
• H+ can be eliminated directly by exchange with Na+
• Urine is usually slightly acid. It’s pH varies with food and drink intakes
Clinical applications:
• Acidosis: Blood pH<7.35
Figure 19.28