Asked by frank
Write the overall net-ionic reaction that occurs when iron (ii) hydroxide (Fe(OH)2, Ksp = 7.9 x 10^-15) is dissolved in a 0.500 M sodium cyanide solution forming a complex ion. (Fe(CN)6^4-, Kf = 7.7 x 10^36)
Determine the value of the equilibrium constant for the overall net-ionic reaction.
Which chemical is the ligand in the complex ion?
Determine the value of the equilibrium constant for the overall net-ionic reaction.
Which chemical is the ligand in the complex ion?
Answers
Answered by
DrBob222
Fe(OH)2 ==> Fe^2+ + 2OH^- Ksp = ?
Fe^2+ + 6CN^- ==> [Fe(CN6]^4 Kf = ?
--------------------------
Fe(OH)2+ 6CN^- => Fe^2+ +2OH^- +[Fe(CN)6]^4-
CN^- is the ligand
Keq for the rxn as shown is Kf*Ksp = ?
Fe^2+ + 6CN^- ==> [Fe(CN6]^4 Kf = ?
--------------------------
Fe(OH)2+ 6CN^- => Fe^2+ +2OH^- +[Fe(CN)6]^4-
CN^- is the ligand
Keq for the rxn as shown is Kf*Ksp = ?
Answered by
frank
do I have to find Ksp using the .5M?
Answered by
DrBob222
No. K is K. It changes ONLY with temperature. Ksp is given Kf is given. If you wonder how I know Keq is Kf*Ksp, here is what you do.
Write the Ksp expression and multiply that by the Kf
Write the Ksp expression and multiply that by the Kf
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.