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The question was:
What is the pka for a conjugate acid of the solute in solution X?
a. 1
b. 2
c. 3
d. 9
Now the passage stated that the pH of Solution X is 10.7 and the titration graph reflects this (monoprotic solution).
The explanation in the back of the book gave a long drawn out solution stating that we need to change the pH to pOH to find the pkb to get the pka. But I want to know is if we already know that pH of the solution and pH=pka at the half mark to the equivalence point, do we really need to be going from pH→pOH→pkb→pka?
What is the pka for a conjugate acid of the solute in solution X?
a. 1
b. 2
c. 3
d. 9
Now the passage stated that the pH of Solution X is 10.7 and the titration graph reflects this (monoprotic solution).
The explanation in the back of the book gave a long drawn out solution stating that we need to change the pH to pOH to find the pkb to get the pka. But I want to know is if we already know that pH of the solution and pH=pka at the half mark to the equivalence point, do we really need to be going from pH→pOH→pkb→pka?