DETAILED ANSWERS|LATEST
pH - ANSWER how we measure acid base environment in the body
Blood pH range - ANSWER 7.35-7.45
When a solution is too basic it: - ANSWER donates H+
when a solution is to acidic it: - ANSWER absorbs H+
3 buffer systems - ANSWER proteins, phosphates, and carbonic acid bicarbonate
volatile acid - ANSWER - CO2 combines with water forming the volatile acid, carbonic
acid (H2CO3)
§ Enzyme: carbonic anhydrase in RBCS
- H2CO3 dissociates into CO2 and water
- CO2 exhaled by the lungs
Non-volatile (fixed) acids - ANSWER - Not converted to CO2
- Ketones, lactic acid, etc.
Lower pH value - ANSWER more acidic
Higher pH value - ANSWER more basic
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, metabolic acids - ANSWER - CO2 (volatile)
- Ketones
- Lactic acid
hydrogen ion - ANSWER very strong acid but has a low concentration in body fluids
and because the concentration is small it's expressed as pH> negative logarithm of hydrogen
ion concentration
why do we have buffer systems? - ANSWER If our pH deviation is out of normal you
can have cellular dysfunction > so the buffer system are there to prevent the swing in blood
pH by either absorbing or donating hydrogen ions
protein - ANSWER Largest buffering system in the body
Hemoglobin is one of the primary proteins
Phosphate - ANSWER Regulate intracellular pH
They can take on acidic or basic form
carbonic acid-bicarbonate buffering - ANSWER Involves carbon dioxide, carbonic acid,
hydrogen ions, bicarbonate
- Lungs and kidneys utilize this system to help maintain blood pH
When does the equation move to the RIGHT? - ANSWER when CO2 is elevated
- more HCO3 + H+ are formed
When does the equation move to the LEFT? - ANSWER when H+ ions are elevated
- H+ ions are converted to CO2
ABGs - ANSWER how we measure arterial CO2 & bicarbonate levels in the blood
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pH - ANSWER how we measure acid base environment in the body
Blood pH range - ANSWER 7.35-7.45
When a solution is too basic it: - ANSWER donates H+
when a solution is to acidic it: - ANSWER absorbs H+
3 buffer systems - ANSWER proteins, phosphates, and carbonic acid bicarbonate
volatile acid - ANSWER - CO2 combines with water forming the volatile acid, carbonic
acid (H2CO3)
§ Enzyme: carbonic anhydrase in RBCS
- H2CO3 dissociates into CO2 and water
- CO2 exhaled by the lungs
Non-volatile (fixed) acids - ANSWER - Not converted to CO2
- Ketones, lactic acid, etc.
Lower pH value - ANSWER more acidic
Higher pH value - ANSWER more basic
1
, metabolic acids - ANSWER - CO2 (volatile)
- Ketones
- Lactic acid
hydrogen ion - ANSWER very strong acid but has a low concentration in body fluids
and because the concentration is small it's expressed as pH> negative logarithm of hydrogen
ion concentration
why do we have buffer systems? - ANSWER If our pH deviation is out of normal you
can have cellular dysfunction > so the buffer system are there to prevent the swing in blood
pH by either absorbing or donating hydrogen ions
protein - ANSWER Largest buffering system in the body
Hemoglobin is one of the primary proteins
Phosphate - ANSWER Regulate intracellular pH
They can take on acidic or basic form
carbonic acid-bicarbonate buffering - ANSWER Involves carbon dioxide, carbonic acid,
hydrogen ions, bicarbonate
- Lungs and kidneys utilize this system to help maintain blood pH
When does the equation move to the RIGHT? - ANSWER when CO2 is elevated
- more HCO3 + H+ are formed
When does the equation move to the LEFT? - ANSWER when H+ ions are elevated
- H+ ions are converted to CO2
ABGs - ANSWER how we measure arterial CO2 & bicarbonate levels in the blood
2
