Using the dissociation constant, Kd = 3.4x10 15, calculate the equilibrium concentrations of OH in a 0.0465-M solution of Zn(OH)42O a. 1.8x10-5 MO b.9.1x10-4 MO c. 3.8x10-4 MO d. 6.0x10-7 M Using the dissociation constant, Kd 1x1044, calculate the equilibrium concentrations of CN in a 0.333 M solution of Fe(CN)6-.О а. 1.8х10-5 мO b. 3.8x10-4 MO c. 6.0x10-7MO d. 9.1x10-4 M

Given, The dissociation constant of this complex is = 3.4× 10^-15 M. Concentration of solution is =…

Answered: Using the dissociation constant, Kd =…

Using the dissociation constant, Kd = 3.4x1015 calculate the equilibrium concentrations of OH in a 0.0465-M solution of Zn(OH)4-2 O a. 1.8x10-5 M O b.9.1x10-4 M Oc 3.8x10-4 M O d.6.0x10-7 M

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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Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

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Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

Using the dissociation constant, Kd = 3.4x10 15, calculate the equilibrium concentrations of OH in a 0.0465-M solution of Zn(OH)42
O a. 1.8x10-5 M
O b.9.1x10-4 M
O c. 3.8x10-4 M
O d. 6.0x10-7 M

Using the dissociation constant, Kd 1x1044, calculate the equilibrium concentrations of CN in a 0.333 M solution of Fe(CN)6-.
О а. 1.8х10-5 м
O b. 3.8x10-4 M
O c. 6.0x10-7
M
O d. 9.1x10-4 M

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