A student determines that an aqueous solution that contains 0.155 M potassium acetate and 0.344 M acetic acid, also has a H3O* concentration of 5.67×105 M. Based on these data, calculate the value of the equilibrium constant K for the equilibrium: CH3COOH(aq) +H2O=H30*(aq) + CH3COO"(aq) (1) as is usually done, without the inclusion of water in the expression for K: K= (2) for comparison, with the inclusion of water in the expression for K: K=

A student determines that an aqueous solution that contains 0.155 M potassium acetate and 0.344 M acetic acid, also has a H3O* concentration of 5.67×105 M. Based on these data, calculate the value of the equilibrium constant K for the equilibrium: CH3COOH(aq) +H2O=H30*(aq) + CH3COO"(aq) (1) as is usually done, without the inclusion of water in the expression for K: K= (2) for comparison, with the inclusion of water in the expression for K: K=

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 12.41PAE: Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go...

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Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go a step further and examine the equilibrium between carbonate ion and CaCOj. The reaction is Ca2+(aq) + COj2_(aq) ** CaCO,(s) The equilibrium constant for this reaction is 2.1 X 10*. If the initial calcium ion concentration is 0.02 AI and the carbonate concentration is 0.03 AI, what are the equilibrium concentrations of the ions? A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H2COj(aq) H+(aq) + HCO}‘(aq) K = 4.4 X 10"7 She starts with 0.1000 AI carbonic acid. What are the concentrations of all species at equilibrium?
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When 1.00x10-3 mol PCl5 is introduced into a 250.0 mL flask and equilibrium is established at 284oC, the following reaction takes place: PCl5 (g)  PCl3 (g) + Cl2 (g). The quantity of Cl2 (g) present at equilibrium is found to be 9.65x10-4 mol. What is the value of Kc for the dissociationreaction at 284oC? What would the equilibrium constant be for the reverse reaction?