chemistry - exam practice help!!
posted by Anya on .
i'm not exactly sure how to do this question :/
i don't even know where to start.
"Determine the equilibrium [F-] of the following solution with initial concentrations od [HF]= 1.296 M and [NaF] = 1,045 M (ka for HF is 6.6 * 10 ^ -4)
d) 8.2 * 10^-4
all i know is that HF is a weak acid
that HF dissociates into H+ and F-
any help at all is appreciated!!
I assume the (NaF) = 1.045M and not 1,045M.
..........HF ==> H^+ + F^-
.........NaF ==> Na^+ + F^-
Ka for HF = (H^+)(F^-)/(HF)
(H^+) = x
(F^-) = x + 1.045
(HF) = 1.296-x
The easy of solving this is to substitute concns I've listed above, assume x + 1.045 = 1.045 and 1.296-x = 1.296; then solve for x in the Ka expression. When you obtain that, then total (F^-) = 1.045+x. If you want to do it up brown, set up the Ka expression and solve the quadratic equation.
thank you! and yes the 1,045 was a typo ,
but how did you know that the change row in the ice table for NaF under Na+ and F- were gonna be 1.045 ? wouldn't they be x as well ? that's just the only part that messes me up. :S
NaF is a salt, it is completely soluble in water, it is an ionic compound, and it is 100% ionized in aqueous solution. There is no unionized NaF left over as there is in HF, a weak acid and weak electrolyte.
wow, i don't know how i missed that connection before. of course, its simple. i must be getting too nervous for my test lol. Thank you so much for clearing that up for me!
It's ok to get nervous; just don't thing crooked, think straight.
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