posted by Katie on .
I'm doing a chemistry lab called colorimetric equilibrium study of a complex ion. But I just have one question which is how to obtain CS which is the total stoichiometric molarity of thiocynate ion and CF which is iron (III) iron.
Fe+3 + SCN --> Fe(NCS)^+2
Fe(NCS)^+2 + SCN ---> Fe(NCS) (SQUARED ON THE BOTTOM OF (NCS)
Fe(NCS)^-2 (SQUARED ON THE BOTTOM OF (NCS) BUT BY A FACTOR OF 5
+ SCN ---> Fe(NCS)^-3 (SQUARED ON THE BOTTOM OF (NCS) BUT BY A FACTOR OF 6
This lab is stating CS AND CF can be expressed as the sum of the equilibrium concentrations of the various species.
CS = [SCN] + [Fe(NCS)]
CF = [Fe] + [Fe(NCS)]
[KSCN]= 0.002 M
[HNO3] = 0.5 M
[FeNO3] = 0.1 M
Would I need the absorbance and volume to calculate CF and CS? If so, how do I calculate CF and CS? I was wondering the concentrations would equal to [SCN] and etc but I believe I'm wrong since the absorbance has to be used in order to calculate CF and CS.
thank you very much for any help