Acid-Base - Pt 1 Intro Flashcards
Bicarbonate levels in the blood are [].
24 mEg/L
PaCo2 in arterial blood is []
40 mmHg
[H+] in blood is []?
40 nEq/L
Only the [] [] concentration contributes to pH. That which is bound to any [], chemical (proteins etc) oranything has [] contribution to the pH
Only the Free H+ concentration contributes to pH. That which is bound to any buffer, chemical (proteins etc) or anything has zero contribution to the pH
A hydrogen ion (H+) is a single [] [] released from a hydrogen atom
free proton
Easy definitions:
- Acid = proton []
- [] [] is more likely to give up a proton. [] is a good example.
- [] [] is less likely to give up a proton. [] [] is a good example
- Acid = proton donor
- Strong acid is more likely to give up a proton. HCl is a good example.
- Weak acid is less likely to give up a proton. Carbonic acid is a good example
Extreme conditions of [H+]:
- 10 nEq/L….pH ~ []
- 160 nEq/L…pH ~[]
- 10 nEq/L….pH ~ 8
- 160 nEq/L…pH ~6.8
pH is [] related to the [H+].
inversely
- Normal pH of blood is [] +/- .02
- Acidosis occurs at a pH less than []
- Alkalosis occurs at a pH greater than []
- Normal pH of blood is 7.4 +/- .02
- Acidosis occurs at a pH less than 7.38
- Alkalosis occurs at a pH greater than 7.42
- Volatile acids are defined as [] that may be eliminated by the [].
- Example: []
- Volatile acids are defined as gases that may be eliminated by the lungs.
- Example: CO2
Fixed Acids:
- Acids which result from [] of sulfur or phosphate containg amino acids, phospholipids, nucleic acids, phosphoporteins and phosphoglycerides
- Primarily [] (H2SO4) and [] acid (H3PO4).
- Acids which result from metabolism of sulfur or phosphate containg amino acids, phospholipids, nucleic acids, phosphoporteins and phosphoglycerides
- Primarily sulfuric (H2SO4) and phosphoric acid (H3PO4).
Organic Acids:
- Comes from ordinary [] such as lactic, pyruvic, ketones during oxygen [], shock, and []
Comes from ordinary production such as lactic, pyruvic, ketones during oxygen debt, shock, and exercise
- There are 3 regulatory systems that interact to control body pH
- [] buffering system
- [] Responses
- [] [] Responses
- There are 3 regulatory systems that interact to control body pH
- Chemical buffering system
- Respiratory Responses
- Renal System Responses
What are the 4 major physicoChemical Buffers?
Bicarbonate
Phosphate
Ammonia
Proteins
The respiratory response will attempt to move pH back toward []but will always remain [], due to feedback [] and receptor [] and functionality.
The respiratory response will attempt to move pH back toward normal but will always remain incomplete, due to feedback inhibition and receptor sensitivity and functionality.
Kidneys respond to pH via several mechanisms
- Increased [] of H+/HCO3- into the urine
- Increased [] of H+/HCO3- into the blood
- [] [] H+ cellular secretory transport mechanisms
- [] [] HCO3- cellular secretory transport mechanism
- Make New []
- Increased secretion of H+/HCO3- into the urine
- Increased reabsorption of H+/HCO3- into the blood
- Up/Down regulate H+ cellular secretory transport mechanisms
- Up/Down regulate HCO3- cellular secretory transport mechanism
- Make New HCO3-
Normally, it doesn’t matter where the H+ comes from, it’ll always bind to [] if available.
bicarbonate
- pH and bicarbonate have a [] relationship. When [Bicarbonate] increases, pH []
- pH and CO2 have an [] relationship. When [CO2 increases, pH []
- pH and bicarbonate have a direct relationship. When [Bicarbonate] increases, pH increases
- pH and CO2 have an indirect relationship. When [bicarbonate] increases, pH decreases
The optimum effect of a buffer occurs at the [] point of a titration curve. This is also the [] of the buffer - or its dissociation constant.
The optimum effect of a buffer occurs at the inflection point of a titration curve. This is also the pK of the buffer - or its dissociation constant.
- Bicarbonate’s optimum pK is [] +/- 1 unit at a normal pH of 7.4
- However, this optimum pK falls under our normal body’s pH of 7.4, which is why bircarb is not the most [] buffer in our body.
- Bicarbonate’s optimum pK is 6.1 +/- 1 unit at a normal pH of 7.4
- However, this optimum pK falls under our normal body’s pH of 7.4, which is why bircarb is not the most powerful buffer in our body.
Buffering Power is based on 2 things:
- Buffering of a solution is [] when the pH of the solutin is at or near the [] of the buffer
- Or +/- one pH unit from the pK
- [] of the buffering sibstances…The more buffer, the better
- Buffering of a solution is greatest when the pH of the solution is at or near the pK of the buffer
- Or +/- one pH unit from the pK
- Concentration of the buffering sibstances…The more buffer, the better
- The most important buffering system in the body is the [] [] []
- This is becuase both elements are []systems.
- The lungs can [] CO2
- The kidneys can [] Bicarb/H+
- The most important buffering system in the body is the Bicarbonate Buffer System
- This is becuase both elements are open systems.
- The lungs can expire CO2
- The kidneys can micturate/save Bicarb/H+
In normal body conditions, the bicarbonate buffering system cannot be [] to one extreme of the system or the other.
pushed
The HCO3- buffering system links together [] buffering, the [] system and the [] system in the regulation of body pH
The HCO3- buffering system links together chemical buffering, the respiratory system and the renal system in the regulation of body pH