Find the concentration of Ag+ in a saturated solution of AgBrO3 that also contains 0.02M LiNO3, 0.02M KClO4 and 0.01M NaF.
3 answers
I have looked at this for some time and I don't see anything difficult about the problem except it is tedious to solve. I wonder if this is work with the Debye-Huckel theory. If so you calculate the ionic strength of LiNO3, KClO4 and NaF and use that to find the (Ag^+). I can help you through this if I'm on the right track.
for LiNO3 i found the ionic strength to be .02M
for KClO4 i found the ionic strength to be .05M
for NaF i found the ionic strength to be .01M
i'm stuck on what else to do from here.
for KClO4 i found the ionic strength to be .05M
for NaF i found the ionic strength to be .01M
i'm stuck on what else to do from here.
I don't know that I agree with the ionic strength values. Check them out.
[Ag^+]*^+ x [BrO3^-]*fBro3^- = Ksp
so [Ag^+][BrO3^-] = [Ksp/(^+*fBrO3^-) K'sp which is the concentration constant for Ksp in this solution.
where ^+ and fBrO3^-. You obtain these activity coefficients from the Debye-Huckel equation or some texts have a table that can be used.
The rest of the problem is worked as a regular Ksp problem is approached.
[Ag^+]*^+ x [BrO3^-]*fBro3^- = Ksp
so [Ag^+][BrO3^-] = [Ksp/(^+*fBrO3^-) K'sp which is the concentration constant for Ksp in this solution.
where ^+ and fBrO3^-. You obtain these activity coefficients from the Debye-Huckel equation or some texts have a table that can be used.
The rest of the problem is worked as a regular Ksp problem is approached.