A weak acid with an initial pH of 3.2 was titrated with a strong base. 15 mL of 0.1 M NaOH was added to the acid to reach the equivalence point at a pH of 8.6. What would you expect the approximate pH of the analyte to be after the first 5 mL of 0.1 M NaOH was added? A. 5.1 B. 7.2 C. 3.4 D. 8.6

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A weak acid with an initial pH of 3.2 was titrated with a strong base. 15 mL of 0.1 M NaOH was added to the acid to reach the equivalence point at a pH of 8.6. What would you expect the approximate pH of the analyte to be after the first 5 mL of 0.1 M NaOH was added? A. 5.1 B. 7.2 C. 3.4 D. 8.6

Chemistry
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definitely not 8.6.. would be <8.6 for sure.
I will said between 3.2 and 8.6
@cuanchi is there a formula for this, because we don't know anything about the pKa. i would guess it's either 5.1 or 7.2

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Other answers:

I am trying to figure out
pH = pKA so at that point half the acid is gone.
we can not calculate the Ka because we don't have the initial volume of the acid, neither the final volume after the titration. We can calculate the moles but not the concentrations
what is your logical thinking about the problem?
did you read the book?
why do you think is B?
I'm curious to know how to get the answer for this
@vera_ewing did you find the correct answer yet?

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