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At a certain temperature K = 1.10×103 for the reaction:   Fe3+(aq) + SCN-(aq) FeSCN2+(aq) 1.80×10-1 mol of Fe(NO3)3 is added to 1.32 L of 2.27×10-2 M KSCN. Neglecting any volume change and assuming that all species remain in solution--: 1a) Calculate the equilibrium concentration of Fe3+ (in mol/L). 1b) Calculate the equilibrium concentration of SCN- (in mol/L). 1c) Calculate the equilibrium concentration of FeSCN2+ (in mol/L)

At a certain temperature K = 1.10×103 for the reaction:   Fe3+(aq) + SCN-(aq) FeSCN2+(aq) 1.80×10-1 mol of Fe(NO3)3 is added to 1.32 L of 2.27×10-2 M KSCN. Neglecting any volume change and assuming that all species remain in solution--: 1a) Calculate the equilibrium concentration of Fe3+ (in mol/L). 1b) Calculate the equilibrium concentration of SCN- (in mol/L). 1c) Calculate the equilibrium concentration of FeSCN2+ (in mol/L)

Chemistry for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 12.40PAE: Because carbonic acid undergoes a second ionization, the student in Exercise 12.39 is concerned that...
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Hi i need help with this! Handwritten solutions are prefered rather than typed solutions because they are easier to understand 

At a certain temperature K = 1.10×103 for the reaction:

 

Fe3+(aq) + SCN-(aq) FeSCN2+(aq)

1.80×10-1 mol of Fe(NO3)3 is added to 1.32 L of 2.27×10-2 M KSCN.

Neglecting any volume change and assuming that all species remain in solution--:

1a) Calculate the equilibrium concentration of Fe3+ (in mol/L).

1b) Calculate the equilibrium concentration of SCN- (in mol/L).

1c) Calculate the equilibrium concentration of FeSCN2+ (in mol/L).

 

 

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