When excess Ag metal is added to 0.190 L of 1.230 M Fe3+ (aq) at 298K, the following equilibrium is established: Ag+ (aq) + Fe2+ (aq) Ag(s) + Fe³+ (aq) (1) If the equilibrium concentration of Ag+ is 0.499 M, what is the value of K? K = (2) Using the value of K from part (1), calculate the new equilibrium concentrations of the three species in solution, if the volume of the solution is increased to 0.714 L by the addition of pure water? [Ag+]= [Fe2+] [Fe³+] = H =

When excess Ag metal is added to 0.190 L of 1.230 M Fe3+ (aq) at 298K, the following equilibrium is established: Ag+ (aq) + Fe2+ (aq) Ag(s) + Fe³+ (aq) (1) If the equilibrium concentration of Ag+ is 0.499 M, what is the value of K? K = (2) Using the value of K from part (1), calculate the new equilibrium concentrations of the three species in solution, if the volume of the solution is increased to 0.714 L by the addition of pure water? [Ag+]= [Fe2+] [Fe³+] = H =

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 14.70QE

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Question

Q 05.

When excess Ag metal is added to 0.190 L of 1.230 M Fe³+ (aq) at 298K, the following equilibrium is
established:
Ag+ (aq) + Fe²+ (aq) Ag(s) + Fe³+ (aq)
(1) If the equilibrium concentration of Ag+ is 0.499 M, what is the value of K?
K =
(2) Using the value of K from part (1), calculate the new equilibrium concentrations of the three
species in solution, if the volume of the solution is increased to 0.714 L by the addition of pure water?
[Ag+] =
[Fe2+] =
=
[Fe3+]:
Submit Answer
=
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