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vera_ewing
 one year ago
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
vera_ewing
 one year ago
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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Photon336
 one year ago
Best ResponseYou've already chosen the best response.0definitely not 8.6.. would be <8.6 for sure.

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0I will said between 3.2 and 8.6

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0@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

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0I am trying to figure out

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0pH = pKA so at that point half the acid is gone.

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0we 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

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0what is your logical thinking about the problem?

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0did you read the book?

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0why do you think is B?

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0I'm curious to know how to get the answer for this

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0@vera_ewing did you find the correct answer yet?
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