renal physiology part 2 - acid base balance Flashcards
what is the pH of arterial blood
7.45
what is the pH of venous blood
7.35
what is the average pH of blood
7.4
why is venous blood more acidic than arterial blood
due to presence of CO2
what is considered acidotic
below 7.35
what is considered alkalotic
above 7.45
what is the equation for pH using log and [H+]
log(1/[H+])
an increase in [H+] does what to the pH
lowers the pH
small change in pH reflect ____ changes in [H+]
large
acidosis can lead to ____ of the CNS
depression
alkalosis can lead to ____ of the peripheral and later the central nervous system
overexcitability
what are some examples of changes in the nervous system due to alkalosis
pins and needles (sensory) muscle spasms (motor) - fatal if respiratory
change of pH of bodily fluids will alter the ______ of proteins causing a knock on effect on ____
secondary structure
enzymes
increased plasma [H+] ______ K+ secretion in renal tubules
decreases
what are the 3 ways in which H+ is added to the bodily fluids
carbonic acid formation
inorganic acids produced during breakdown of nutrients
organic acids resulting from metabolism e.g. lactic acid
what is a strong acid
dissociates completely in solution
what is a weak acid
partially dissociates in solution
what is the first line defence to any change in pH
buffer systems
what does a buffer system consist of
one substance can yield a H+ ion if [H+] decreases
one substance can bind to H+ if [H+] increases
what is the equation of a buffer solution
HA H+ + A-
what is the base in the buffer solution
A-
what is the undissociated acid in the buffer solution
HA
what is the proton in the buffer solution
H+
if H+ is added to a buffer system equilibrium shifts to the ….
why?
left
H+ is mopped up by A- leading to formation of more HA
[HA] rises, [A-] falls