Week 11 - Acid Base Balance Introduction Flashcards
Why are hydrogen ions important? (2)
- vital to life and circulate in our bodies
- expressed as pH
The normal range for pH is 7.35-7.45. What happens if pH is:
a) below 7.35
b) above 7.45
a) acidotic state
b) alkalotic state
What is an acid? (3)
- substance that release hydrogen ions when dissolved in water or body fluids
- increases the amount of free hydrogen ions in that solution
- are produced as end products of metabolism
What is a base?
- substance that binds free hydrogen ions in solution and lower the amount of free hydrogen ions in solution
Our body has to maintain acid-base balance. This occurs in 3 mechanisms. Name them all in order. (4)
- Chemical - protein buffers, chemical buffers
- Respiratory
- Kidney
(4) K+ exchange
Give 3 examples of protein buffers
- albumin
- globulins
- hemoglobin
quick to react in acidic environments
Give 2 examples of chemical buffers.
- bicarbonate
- phosphate
What is bicarbonate also known as?
- carbonic acid bicarbonate system
Where is phosphate present in the body? (2)
- cells and body fluids
- especially active in the kidneys
What does phosphate act as?
- acts like bicarbonate and neutralizes excess hydrogen ions
What is the primary buffer system in our body?
carbonic acid-bicarbonate system
What is the pH and ratio of bicarbonate to carbonic acid in the carbonic acid-bicarbonate system? (3)
- 7.4
- 20 parts bicarbonate (HCO3-) to 1 part carbonic acid (H2CO3)
- this ratio determines H+ concentration of body fluid
What is carbonic acid (H2CO3) concentration controlled by? (2)
- excretion of CO2 in the lungs
- rate and depth of respiration change in response to the change in CO2
Carbonic acid it is highly regulated by respiration
- no carbon dioxide means you’ll slow down breathing to build H2CO3
What is bicarbonate concentration controlled by? (2)
- the kidneys
- They selectively retain or excrete bicarbonate in response to bodily needs
What would it look like for carbonic acid excess/deficit? how about Bicarbonate?
