An analytical chemist is titrating 120.0mL of a 0.5200 M solution of diethylamine ((C2H5)2NH) with a...
An analytical chemist is titrating 120.0mL of a 0.5200 M solution of diethylamine ((C2H5)2NH) with a 0.07300 M solution of HNO3. The pKb of diethylamine is 2.89. Calculate the pH of the base solution after the chemist has added 395.6mL of HNO3 solution to it.
Homework Answers
![Ansues:- SzHEANH] = 0.5200M, 120.0m FHNO3) = 0.07300M 398-6 oko 2.89 -pka = 14-pko: 14-2-89 _ =11.11 (SzHs), MH + HO-945), Ny](http://img.homeworklib.com/questions/c5c4a800-d694-11eb-8305-e739109923dd.png?x-oss-process=image/resize,w_560)
Answer:-
This question is solved by using the simple concept of calculation of pH of buffer solution using Henderson Hasselbach equation.
The answer is given in the image,
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An analytical chemist is titrating 120.0mL of a 0.5200 M
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