a. Show that the solubility of Al(OH)3, as a function of [H+ ], obeys the equationS = [H+]3Ksp /Kw3 + KKw/ [H+]S = solubility = [Al3+] + [Al(OH)4-] andK is the equilibrium constant forAl(OH)3 (s) + OH- (aq) < ======= Al(OH)4- (aq)b.) The value of K is 40.0 and Ksp for Al(OH)3 is 2 x 10 -32. Plot the log solubility of Al(OH)3 in the pH range 4–12. 9.) a. Show that the solubility of Al(OH)3, as a function of [H* ], obeys the equationS = [H*]°Ksp /Kw³ + KKW/ [H*]S = solubility = [A3+] + [Al(OH)4] andK is the equilibrium constant forAI(OH); (s) + OH (aq) < =======> Al(OH)4 (aq)b.) The value of K is 40.0 and Ksp for Al(OH); is 2 x 10 -32. Plot the log solubility of Al(OH)3in the pH range 4F12.pH (x -axis)Log S (y-axis)4

a. Show that the solubility of Al(OH)3, as a function of [H+ ], obeys the equation S = [H+]3Ksp /Kw3 + KKw/ [H+] S = solubility = [Al3+] + [Al(OH)4-] and K is the equilibrium constant for Al(OH)3 (s) + OH- (aq) < ======= Al(OH)4- (aq) b.) The value of K is 40.0 and Ksp for Al(OH)3 is 2 x 10 -32. Plot the log solubility of Al(OH)3 in the pH range 4–12.

a. Show that the solubility of Al(OH)3, as a function of [H+ ], obeys the equation S = [H+]3Ksp /Kw3 + KKw/ [H+] S = solubility = [Al3+] + [Al(OH)4-] and K is the equilibrium constant for Al(OH)3 (s) + OH- (aq) < ======= Al(OH)4- (aq) b.) The value of K is 40.0 and Ksp for Al(OH)3 is 2 x 10 -32. Plot the log solubility of Al(OH)3 in the pH range 4–12.

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 12.71PAE: Acrylic acid is used in the polymer industry in the production of acrylates. Its K, is 5.6 X 10“’....

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Question

a. Show that the solubility of Al(OH)3, as a function of [H+ ], obeys the equation

S = [H+]3Ksp /Kw3 + KKw/ [H+]

S = solubility = [Al3+] + [Al(OH)4-] and

K is the equilibrium constant for

Al(OH)3 (s) + OH- (aq) < ======= Al(OH)4- (aq)

b.) The value of K is 40.0 and Ksp for Al(OH)3 is 2 x 10 -32. Plot the log solubility of Al(OH)3 in the pH range 4–12.

9.) a. Show that the solubility of Al(OH)3, as a function of [H* ], obeys the equation
S = [H*]°Ksp /Kw³ + KKW/ [H*]
S = solubility = [A3+] + [Al(OH)4] and
K is the equilibrium constant for
AI(OH); (s) + OH (aq) < =======> Al(OH)4 (aq)
b.) The value of K is 40.0 and Ksp for Al(OH); is 2 x 10 -32. Plot the log solubility of Al(OH)3
in the pH range 4F12.
pH (x -axis)
Log S (y-axis)
4

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