Login or Sign Up
  1. Login
  2. Search
Ask a New Question

This is for a lab about determining the equilibrium constant.

Given: 5.00mL of .203M Fe(NO3)3 mixed with 100mL of .00205M KSCN in a .5M HNO3 solvent for both solutions. Resulting absorbance for solution is .315.

How can i find the total Fe, [Fe*] and SCN, [SCN*] in the system without determining equilibrium values of [FeSCN+2], [Fe+3], and [SCN-].

What i know so far is that:
Fe+3 + SCN- makes FeSCN+2
[Fe*] = [Fe+3] + [FeSCN+2]
[SCN*] = [SCN-] + [FeSCN+2]

Question ID
524793

Created
April 3, 2011 8:51pm UTC

Rating
0

URL
https://questions.llc/questions/524793

Answers
1

Views
759

1 answer

  1. Make an ICE chart.
    Total Fe = moles Fe(NO3) = 5.00 mL x 0.203 M = ??millimoles Fe.
    Total SCN = mL x M = 100 x 0.00205 = ??millimoles SCN
    ...............Fe^+3 + SCN^- ==> FeSCN^+2
    initial......
    change.......
    equil........

    One caution here. The ICE chart prepared as above is done with millimoles. Before you can use this to determine a Keq value, millimoles must be changed to M which = millimoles/TOTAL mL.
    Total mL in this case is 105 mL.

    Answer ID
    524806

    Created
    April 3, 2011 9:10pm UTC

    Rating
    0

    URL

Answer this Question