chater 26 acid-base balance

Question 1

what is the normal homeostatic pH range for arterial blood

Answer 1

7.35 - 7.45

Question 2

Define chemical buffer systems

Answer 2

try to resist changes in pH, If pH drops buffers bind H+, if pH rises buffers release H+

Question 3

Describe bicarbonate buffer systems

Answer 3

• If acid is added, the system is driving to the right, bicarbonate ions will “mop” up excess H+ ions and forms more carbonic acid, HCl is converted to a weak acid so pH doesn’t change much HCl+NaHCO3 -> H2CO3 + NaCl.
• If strong base is added, NaOH + H2CO3 -> NaHCO3 + H2O, we effectively diet the solution by making H2O. Replace strong base with a weak one so pH does not change much

Question 4

Describe phosphate buffer system:

Answer 4

The phosphate buffer system operates in the internal fluid of all cells. This buffer system consists of dihydrogen phosphate ions (NaH2PO4) as hydrogen-ion donor (acid) and hydrogen phosphate ions (Na2HPO4) as hydrogen-ion acceptor (base). HCl+Na2HPO4 -> NaH2PO4 + NaCl
important buffer in urine and intracellular fluid

Question 5

what are some phosphate containing molecules

Answer 5

DNA, RNA, ATP ect

Question 6

Describe protein buffer systems

Answer 6

Includes plasma proteins and intracellular proteins
when pH becomes alkaline: R-COOH –> R-COO +H
when pH becomes acidic: R-NH2 + H –> R-NH3
*powerful buffering system 3/4 of all buffering in cells, therefore, functions as acid or base (amphoteric) ex: Hb, histone proteins, nucleic acids.

Question 7

what does hypoventilation lead to

Answer 7

CO2 build up, = respiratory acidosis pH

Question 8

what does hyperventilation lead to

Answer 8

CO2 purge = respiratory alkalosis pH>7.45