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Use the mean value of 535 for K to calculate the SCN concentration in a solution whose initial Fe concentration was 4.50x10 02 M and initial SCN concentration was 1 50x10-00 M Fe+ + SCN-- FENCS+

Use the mean value of 535 for K to calculate the SCN concentration in a solution whose initial Fe concentration was 4.50x10 02 M and initial SCN concentration was 1 50x10-00 M Fe+ + SCN-- FENCS+

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Use the mean value of 535 for K to calculate the SCN concentration in a solution whose initial Fe concentration was 4.50x10 02 M and initial SCN concentration was 1 50x10-00 M Fe+ + SCN-- FENCS+
Transcribed Image Text:Use the mean value of 535 for K to calculate the SCN concentration in a solution whose initial Fe concentration was 4.50x10 02 M and initial SCN concentration was 1 50x10-00 M Fe+ + SCN-- FENCS+
Expert Solution
Step 1

The equilibrium reaction taking place is given as,

=> Fe3+ (aq) + SCN- (aq) ------> FeSCN2+ (aq)                                     Keq = 535

Given : Initial concentration of Fe3+ = 4.50 X 10-2 M

And initial concentration of SCN- = 1.50 X 10-3 M

 

Step 2

Assuming y concentration of Fe3+ ions reacts to reach equilibrium.

Hence as per the above balanced reaction, the concentration of SCN- ions reacting = y

And the concentration of FeSCN2+ ions formed at equilibrium, [FeSCN2+ ] = y

Hence the equilibrium concentration of reactants are,

=> [SCN- ] = Initial - reacted = 1.50 X 10-3 - y 

And [Fe3+ ] = Initial - reacted = 4.50 X 10-2 - y

 

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