A student determines that an aqueous solution that contains 0.474 M potassium hypochlorite and 0.180 M hypochlorous acid, also has an H30* concentration of1.89x10-8 M. Based on these data, calculate the value of the equilibrium constant K for the equilibrium:HCIO(aq) + H2O =H30*(aq) + ClO(aq)Calculate K as is usually done, omitting the solvent, water, from the expression for K: K

KClO = 0.474M HClO = 0.180M H3O+ = 1.89 x 10-8M

A student determines that an aqueous solution that contains 0.474 M potassium hypochlorite and 0.180 M hypochlorous acid, also has an H3O* concentration of 1.89×10-8 M. Based on these data, calculate the value of the equilibrium constant K for the equilibrium: HCIO(aq) + H2O =H3o*(aq) + Cl0(aq) Calculate K as is usually done, omitting the solvent, water, from the expression for K: K=

A student determines that an aqueous solution that contains 0.474 M potassium hypochlorite and 0.180 M hypochlorous acid, also has an H3O* concentration of 1.89×10-8 M. Based on these data, calculate the value of the equilibrium constant K for the equilibrium: HCIO(aq) + H2O =H3o*(aq) + Cl0(aq) Calculate K as is usually done, omitting the solvent, water, from the expression for K: K=

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 38A

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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?
Calculate the value of the equilibrium constant for the reaction N2(g)+2O2(g)2NO2(g) if the concentrations of the species at equilibrium are [N2] = 0.0013, [O2] = 0.0024, and [NO2] = 0.00065.
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