3) One of the main buffer systems found in living organisms is the phosphate buffer system, often used in biological research to mimic cellular conditions. The phosphate equilibrium reactions and their corresponding pKa's are as follows: H3PO4 = H* + H2PO, H2PO, = H* + HPO?- HPO- = H* + PO- pKai pKa2 pKa3 = 2.12 7.21 = 12.44 (a) Given the above chemical reaction, write out the expression for K, of the buffer system which would predominate at neutral pH conditions. Justify your choice. (b) The human body, and many other lifeforms, prefer an internal pH of 7.2 to maintain homeostasis. However, some more acid-tolerant or basic-tolerant organisms can survive (and sometimes thrive) within different ranges of pH. Calculate the mass and moles of the correct acid and corresponding conjugate base solid (assume you have sodium salts of each base: NaH,PO4, Na,HPO,, and Na,PO,) which are needed to make 500 mL of a 0.5 M buffer solution (0.5 M total, including the concentration of acid and base combined) at pH of 6.0 for an acid-tolerant organism. (Hint: Use the Henderson-Hasselbach equation and a system of equations to find the moles of acid and base.)
3) One of the main buffer systems found in living organisms is the phosphate buffer system, often used in biological research to mimic cellular conditions. The phosphate equilibrium reactions and their corresponding pKa's are as follows: H3PO4 = H* + H2PO, H2PO, = H* + HPO?- HPO- = H* + PO- pKai pKa2 pKa3 = 2.12 7.21 = 12.44 (a) Given the above chemical reaction, write out the expression for K, of the buffer system which would predominate at neutral pH conditions. Justify your choice. (b) The human body, and many other lifeforms, prefer an internal pH of 7.2 to maintain homeostasis. However, some more acid-tolerant or basic-tolerant organisms can survive (and sometimes thrive) within different ranges of pH. Calculate the mass and moles of the correct acid and corresponding conjugate base solid (assume you have sodium salts of each base: NaH,PO4, Na,HPO,, and Na,PO,) which are needed to make 500 mL of a 0.5 M buffer solution (0.5 M total, including the concentration of acid and base combined) at pH of 6.0 for an acid-tolerant organism. (Hint: Use the Henderson-Hasselbach equation and a system of equations to find the moles of acid and base.)
General Chemistry - Standalone book (MindTap Course List)
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ISBN:9781305580343
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Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter21: Chemistry Of The Main-group Elements
Section: Chapter Questions
Problem 21.196QP
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Transcribed Image Text:3) One of the main buffer systems found in living organisms is the phosphate buffer
system, often used in biological research to mimic cellular conditions. The
phosphate equilibrium reactions and their corresponding pKa's are as follows:
H3PO4 = H* + H2PO,
H2PO, = H+ + HPO?-
HPO- = H+ + PO;-
pKa1
pКаz —D 7.21
= 12.44
= 2.12
pKa3
(a) Given the above chemical reaction, write out the expression for K, of the buffer
system which would predominate at neutral pH conditions. Justify your choice.
(b) The human body, and many other lifeforms, prefer an internal pH of 7.2 to
maintain homeostasis. However, some more acid-tolerant or basic-tolerant
organisms can survive (and sometimes thrive) within different ranges of pH.
Calculate the mass and moles of the correct acid and corresponding conjugate base
solid (assume you have sodium salts of each base: NaH,PO4, Na,HPO4, and
Na PO,) which are needed to make 500 mL of a 0.5 M buffer solution (0.5 M total,
including the concentration of acid and base combined) at pH of 6.0
for an acid-tolerant organism. (Hint: Use the Henderson-Hasselbach equation and a
system of equations to find the moles of acid and base.)
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