Asked by blair
Calculate the pH when 75.20 mL of 0.114 M HCl is titrated with 0 ml of 0.108 M NaOH
Answers
Answered by
DrBob222
The pH at what point?
Answered by
blair
it doesn't say. That's all that is asked.
Answered by
DrBob222
Frankly I don't know what it's asking unless by titration they mean the HCl has been exactly neutralized. If that is the case, then the pH will be 7.0 because the salt produced is NaCl and neither the cation nor the anion is hydrolyzed.
The other interpretation is that the zero mL means they want the pH of the HCl at the beginning of the titration. If that is the case you want the pH of the 0.114 M HCl. H^+ = 0.114 and pH = -log(H^+)
The other interpretation is that the zero mL means they want the pH of the HCl at the beginning of the titration. If that is the case you want the pH of the 0.114 M HCl. H^+ = 0.114 and pH = -log(H^+)
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.