Blood Gases and Acid-Base Balance Flashcards
substances that donates H+ when dissolved in H2O
acid
substances that accepts H+ when dissolved in H2O
base
the negative logarithm (-log) of H+ concentration
pH
a system that RESIST CHANGES IN pH upon addition of acids and bases
buffer
buffer contains?
weak acid (H2CO3) and salt of conjugate base (HCO3-)
H + OH = H2O is what theory?
Bronsted-Lowry theory
hydrogen ion concentration
36-44 nmol/L
the strength of H+ present a substance
pH
what should be the blood pH considered as alkalemia
> 7.45
what should be the blood pH considered as acidemia
<7.35
what is the normal blood pH
7.35-7.45
in chemistry, blood pH is slightly alkaline but physiologically, a blood pH of 7.35-7.45 is considered neutral
true
human body naturally produce H+ ion approximately ______.
150g H+/day
34-44 nmol/L of H+ conc. is equivalent to normal blood pH
true
process that causes acidemia
acidosis
process that causes alkalemia
alkalosis
what are the control centers of acid-base balance
buffer, lungs, and kidneys
controls CO2
lungs
controls HCO3-
kidneys
acidic component of blood
CO2
alkaline component of blood
HCO3-
acid or basic: high conc. of CO2
acidic
acid or basic: low conc. of CO2
basic
acid or basic: high conc. of HCO3-
basic
acid or basic: low conc. of HCO3-
acidic
at blood pH of 7.40, the HCO3- to H2CO3 ratio is?
20:1
most important blood buffer system
bicarbonate-carbonic acid buffer system
utilized HCO3- (conjugate base) and H2CO3 (conjugate acid) to minimize pH changes
bicarbonate-carbonic acid buffer system
uses PLASMA PROTEINS to minimize pH changes
protein buffer system
primary buffer in urine
phosphate buffer system
utilizes HPO4- and H2PO4
phosphate buffer system
plays a role in buffering CO2 during transport to the lungs
hemoglobin buffer system
enumerate the 4 buffer systems
(1) bicarbonate-carbonic acid buffer system
(2) protein buffer system
(3) phosphate buffer system
(4) hemoglobin buffer system
