Asked by Grant
A student mixes 5 mL of 2.00 x 10^-3 M Fe(NO3)3 with 5 mL 2.00 x 10 ^-3 M KSCN. They find that in the equilibrium mixture concentration of FeSCN^2+ is 1.40 x 10^-4 M.
Find each of the following: the initial concentration in solution for Fe^3+ and SCN, the equilibrium constant for the reaction, and explain what happened to the K and the NO3 ions in the solution.
Find each of the following: the initial concentration in solution for Fe^3+ and SCN, the equilibrium constant for the reaction, and explain what happened to the K and the NO3 ions in the solution.
Answers
Answered by
DrBob222
initial concn Fe(NO3)3 = 2.00E-3 x (5/10) = ?
initial concn KSCN = 2.00E-3 x (5/10) = ?
.........SCN^- + Fe^3+ ==> Fe(SCN)^2+
I.......1E-3....1E-3..........0
C.........-x.....-x...........x
E.......1E-3-x.,.1E-3-x.......x
The problem tells you that x = 1.4E-4M
Evaluate 1E-3 -x, substitute into the Kc expression, and solve for Kc.
Where do NO3^- and K^+ go. They become spectator ions in the solution; ie., one associated with KNO3 and the other two with FeSCN(NO3)2
initial concn KSCN = 2.00E-3 x (5/10) = ?
.........SCN^- + Fe^3+ ==> Fe(SCN)^2+
I.......1E-3....1E-3..........0
C.........-x.....-x...........x
E.......1E-3-x.,.1E-3-x.......x
The problem tells you that x = 1.4E-4M
Evaluate 1E-3 -x, substitute into the Kc expression, and solve for Kc.
Where do NO3^- and K^+ go. They become spectator ions in the solution; ie., one associated with KNO3 and the other two with FeSCN(NO3)2
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.