Calculate the molar solubility of Ni(OH)2 (Ksp = 6x10-16) in(1) pure water(2) pH = 2.00 buffer(3) pH = 10.00 buffer%3!Assuming the buffer solutions do not contain any species that react directly with Ni(OH)2.

#1. Pure water: The equation for the dissociation of Ni(OH)2 is: Ni(OH)2(s) ⇌ Ni2+(aq) + 2OH-(aq)

Calculate the molar solubility of Ni(OH)2 (Ksp = 6x10-16) in !3! (1) pure water (2) pH = 2.00 buffer %3D (3) pH = 10.00 buffer Assuming the buffer solutions do not contain any species that react directly with Ni(OH)2.

Calculate the molar solubility of Ni(OH)2 (Ksp = 6x10-16) in !3! (1) pure water (2) pH = 2.00 buffer %3D (3) pH = 10.00 buffer Assuming the buffer solutions do not contain any species that react directly with Ni(OH)2.

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter6: The Systematic Approach To Equilibria: Solving Many Equations

Section: Chapter Questions

Problem 11P

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Question

Calculate the molar solubility of Ni(OH)2 (Ksp = 6x10-16) in
(1) pure water
(2) pH = 2.00 buffer
(3) pH = 10.00 buffer
%3!
Assuming the buffer solutions do not contain any species that react directly with Ni(OH)2.

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