The discussion revolves around the identification of an unknown buffer solution through titration with NaOH and HCl in a laboratory setting. Participants explore the methodology used to determine the pKa value and the implications of their findings, as well as the interpretation of the lab instructions regarding the neutralization process.
Participants express uncertainty regarding the identification of the buffer and the interpretation of the lab instructions. There is no consensus on the terminology used to describe the titration process, and multiple interpretations of "neutralization" are present.
Limitations include potential misunderstandings of the lab instructions and the lack of a definitive list of buffers, which may affect the identification process. The calculations and assumptions made during the titration are also not fully resolved.
This discussion may be useful for students and educators involved in laboratory work related to buffer solutions, titration techniques, and the interpretation of lab instructions in a chemistry context.
kooombaya said:I required 19.92 mL of NaOH to neutralize a 10 mL portion of my buffer. I did the same thing using another 10 mL portion of the buffer but this time with HCl and it took me 17 mL.
Borek said:What do you mean by "neutralize the buffer"?
kooombaya said:This was how the question was stated in the lab book.
Borek said:Can you explain what they meant? I have never seen something like that, even if it is wrong, I have nothing against knowing.
Yup exactly. Thanks again.Borek said:So it was just shifting pH of the buffer by addition of strong acid or base. There was an acid base reaction involved (which can be technically called neutralization), but it didn't end with neutral solution.
Not the best wording if you ask me.