3) Buffer C: 100.0 mL at pH = 12.000, [conj. base]: = 0.500 M %3D a) What conjugate pair should be chosen? Conjugate acid: Conjugate base: b) Calculate the molarity of the conjugate acid necessary to obtain the desired pH using the Henderson-Hasselbalch equation. Show the variable equation with specific species and Ka values.
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Part A B and C
![3) Buffer C: 100.0 mL at pH = 12.000, [conj. base] = 0.500 M
%3D
a) What conjugate pair should be chosen?
Conjugate acid:
Conjugate base:
b) Calculate the molarity of the conjugate acid necessary to obtain the desired pH using the
Henderson-Hasselbalch equation. Show the variable equation with specific species and Ka
values.
Answer:
c) The source of the conjugate acid is a solid. Calculate the mass (in g) of solid necessary (include
the identify the solid as part of your answer).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F70932241-1ad7-48fc-b0c5-52d574ff0aa2%2F019f5372-7963-4ebb-b383-3a266a9e1386%2Fx20fjye_processed.jpeg&w=3840&q=75)
We need to an acid whose pKa is close to 12. then we make a solution of the acid and its conjugate base.
The acid pKa colse to 12 are H3PO4 and ascorbic acid (H2C2H6O2)
pKa3 of H3PO4 = 12.32
pKa2 of H2C2H6O2 = 11.79
The solution of Na2HPO4 and NaOH can be used make buffer solution:
let the Buffer solution Na3PO4(PO4-3) and Na2HPO4(HPO4-2).
molar mass of Na3PO4 = 163.94 g/mol
molar mass of Na2HPO4 = 141.96 g/mol
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