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Exercise and and Your pH

Reasons to Exercise

  • Health
  • Enjoyment (i.e. Sports)
  • De-stress
  • Help to sleep better
  • And many more!

Why should we care?

Change in blood pH

  • If pH gets too low (below 7.4) acidosis may occur
  • If the pH drops below 6.8 or rises above 7.8, death may occur

(Niedziocah, August 2013)

**Acidosis is when the lungs and kidneys cannot keep your body's pH level balanced

(Allen & Boskey, 2012, July 16)

The following steps outline the processes that affect the buffers in the blood during exercise.

  • Hemoglobin carries O2 from the lungs to the muscles through the blood.
  • The muscles need more O2 than normal, because their metabolic activity is increased during exercise.
  • The amount of oxygen in the muscle is therefore depleted in the muscles,.
  • Oxygen diffuses from the blood to the muscles,.The muscles produce CO2 and H+ as a result of increased metabolism,.
  • The CO2 and H+ flow from the muscles to the blood, The buffering action of hemoglobin picks up the extra H+ and CO2. If the amounts of H+ and CO2 exceed the capacity of hemoglobin, they affect the carbonic acid equilibrium (Equation 10), as predicted by Le Châtelier's Principle or the quantitative treatment in terms of equilibrium constants. As a result, the pH of the blood is lowered, causing acidosis. The lungs and kidneys respond to pH changes by removing CO2, HCO3-, and H+ from the blood.

Exercise

The basic explanation:

During aerobic metabolism (a pathway of energy that uses oxygen), your muscle cells release carbon dioxide into your blood. When blood travels into the working muscles, oxygen is exchanged for carbon dioxide and hydrogen. The cells take in oxygen from the blood and the blood takes away carbon dioxide and hydrogen. The combination of carbon dioxide and hydrogen creates a reaction that decreases the pH of your blood.

An activity requiring physical effort, carried out especially to sustain or improve physical health

(Blessing, 2013)

The Effects

Carbonic-Acid-Bicarbonate Buffer

The Body's Buffers

This is the equilibrium reaction meaning that if one side of the reaction becomes greater than the other, the body will fight to balance them again

(Casiday & Frey, n.d.)

Some of the equations behind the buffer...

Note that as acid is added, the pH decreases and the buffer shifts toward greater H2CO3 and CO2 concentration. As base is added, the pH increases and the buffer shifts toward greater HCO3 concentration

This equation helps to determine the pH of the buffer reaction

(Casiday & Frey, n.d.)

Where K is the equillibrium constant of the buffer. In the carbonic-acid-bicarbonate buffer, pK=6.1 at normal body temperature

(Casiday & Frey, n.d.)

The body has many different "safety nets" to ensure that the pH does not rise or drop past a safe level.

Sources

Acid-Base Physiology. (n.d.). Retrieved June 5, 2015.

Allen, S., & Boskey, E. (2012, July 16). Acidosis. Retrieved June 4, 2015.

Blessing, J. (2013, October 21). The Chemical Reaction That Takes Place in the Body After Exercise. Retrieved June 5, 2015.

Casiday, R., & Frey, R. (n.d.). Blood, Sweat, and Buffers: PH Regulation During Exercise. Retrieved June 5, 2015.

Niedziocah, L. (2013, August 16). Decrease in pH of Blood Caused by Exercise. Retrieved June 5, 2015.

Some other buffers

And also the plasma protein buffer, and phosphate buffer, but they have minimal impact

(Casiday & Frey, n.d.)

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