5.00 mL of 0.0200 M Fe(NO3)3 was mixed with 5.00 mL of 0.00200 M KSCN to form the FeSCN²+ complex. The equilibrium molar concentration of the FeSCN²+ complex was determined to be 1.00 X 104 M Moles of Fe³+, initial Moles of SCN, initial Moles of FeSCN²+ a) b) c)
5.00 mL of 0.0200 M Fe(NO3)3 was mixed with 5.00 mL of 0.00200 M KSCN to form the FeSCN²+ complex. The equilibrium molar concentration of the FeSCN²+ complex was determined to be 1.00 X 104 M Moles of Fe³+, initial Moles of SCN, initial Moles of FeSCN²+ a) b) c)
Chemical Principles in the Laboratory
11th Edition
ISBN:9781305264434
Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi
Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi
Chapter27: Relative Stabilities Of Complex Ions And Precipitates Prepared From Solutions Of Copper(ii)
Section: Chapter Questions
Problem 1ASA
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![1)
5.00 mL of 0.0200 M Fe(NO3)3 was mixed with 5.00 mL of 0.00200 M KSCN to form the
FeSCN²+ complex. The equilibrium molar concentration of the FeSCN²+ complex was
determined to be 1.00 X 104 M
Moles of Fe³+, initial
Moles of SCN, initial
Moles of FeSCN²+
a)
b)
c)
d)
e)
f)
h)
i)
j)
Moles of Fe³+ used
Moles of SCN used
Moles of Fe³+ left
Moles of SCN left
[Fe³+] at equilibrium
[SCN] at equilibrium
Kc
(a - d)
(b-e)
Show calculations for (a), (c), (e), (h), (j) above.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa7634a6a-5ecc-40e2-9892-46ba7a4cefd4%2Ff95ce5a3-1711-42f5-a7fa-cf7a9127b38f%2Fq1jw8sp_processed.jpeg&w=3840&q=75)
Transcribed Image Text:1)
5.00 mL of 0.0200 M Fe(NO3)3 was mixed with 5.00 mL of 0.00200 M KSCN to form the
FeSCN²+ complex. The equilibrium molar concentration of the FeSCN²+ complex was
determined to be 1.00 X 104 M
Moles of Fe³+, initial
Moles of SCN, initial
Moles of FeSCN²+
a)
b)
c)
d)
e)
f)
h)
i)
j)
Moles of Fe³+ used
Moles of SCN used
Moles of Fe³+ left
Moles of SCN left
[Fe³+] at equilibrium
[SCN] at equilibrium
Kc
(a - d)
(b-e)
Show calculations for (a), (c), (e), (h), (j) above.
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