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
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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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).
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