1. How would you prepare a liter of "carbonate buffer" at a pH of 10.07? You are provided with carbonic acid (H2CO3), sodium hydrogen carbonate (NaHCO3), and sodium carbonate (Na2CO3).
Please give an explanation.
2. Provide the mole ratio to support your answer. (Give your answer in the form base : acid.)
ph = 10.07
This is a buffer so:
pH = pKa2 + log(A-2/HA-)
Ka2 = 4.7 × 10−11
pKa = -log(Ka2) =-log(4.7 × 10−11)= 10.33
substitute
pH = pKa2 + log(A-2/HA-) = 10.33 + log(A-2/HA-) = 10.07
Solve for ratio
log(A-2/HA-) = 10.07-10.33 = -0.26
CO3-2 / HCO3 -=0.5495
CO3-2 = 0.5495*HCO3
If you need V = 1L then
[Na2CO3] = 1M
[NaHCO3] = 0.5495 M
2)
mole ratio
bse: acid must be... 1 : 0.5495
1. How would you prepare a liter of "carbonate buffer" at a pH of 10.07? You...
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