1
$\begingroup$

So I have a liter of buffer consisting of .1 M $\ce{HF}$ and 0.05 M $\ce{NaF}$. I'm given three solutions to determine what would essentially destroy the buffer:

(a) 0.050 mol of $\ce{HCl}$
(b) 0.050 mol of $\ce{NaF}$
(c) 0.05 mol $\ce{NaOH}$

Do I assume the aqueous solution of the buffer specifically contain 0.05 M $\ce{F-}$ from the dissociation of the salt. How do I account for the changes in concentration ?

$\endgroup$
1
$\begingroup$

$\ce{HCl}$ would react with nothing but use up some of $\ce{HF}$'s protons, since they have difference in acidities. $\ce{NaF}$ will increase already present concentration. $\ce{NaOH}$ would react with acid $\ce{HF}$. Now a buffer needs to have reasonable amount of both $\ce{HF}$ and $\ce{NaF}$ in almost equal proportions (up to a factor of ten is reasonable). See which is now destroyed.

$\endgroup$

Your Answer

By clicking “Post Your Answer”, you agree to our terms of service, privacy policy and cookie policy

Not the answer you're looking for? Browse other questions tagged or ask your own question.