Acid-base balance. Buffering of hydrogen ions in body fluids – buffer systems.

Question 2

acid-base balance - definition

Answer 2

pH remains in range of 7.36-7.44 for stable internal environment for homeostasis to prevent acidosis/ alkolosis

Question 3

acids

Answer 3

release H+ into solution
for example - carbonic acid dissociates into h+ and bicarbonate ions

Question 4

bases

Answer 4

release OH- into solutions

Question 5

pH

Answer 5

measures concentration of H+ in solution
pH neutral = 7
pH = -log(H+)

Question 6

buffers - definition

Answer 6

substances that help maintain a stable pH
accepting/ releasing H+ in response to changes in pH
needed to regulate pH in blood

Question 7

buffers - example 1

Answer 7

bicarbonate buffer system
= primary buffer system in ECF

when blood pH is too low
- H++HCO3- to form H2CO3 to be converted in CO2 to be exhaled into lungs

when blood pH is too high
-H2​CO3​⇌H++HCO3− so H+ increases acidity

regulated by lungs/ kidney

Question 8

buffers - example 2

Answer 8

PHOSPHATE BUFFER = needed for pH regulation inside cells/ kidneys

H2​PO4−​⇌H++HPO42−​
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Question 9

buffers - example 3

Answer 9

PROTEIN BUFFER SYSTEM

proteins contain -COOH group and release H+
proteins contain -NH3 group to accept H+