Question

The aqueous solubility product of nickel hydroxide, Ni(OH)2 is Ksp = 2.0 x 10-15.What is the...

The aqueous solubility product of nickel hydroxide, Ni(OH)2 is Ksp = 2.0 x 10-15.What is the solubility in a solution with pH = 12.2 in grams per Liter of solution?

Homework Answers

Answer #1

Ni(OH)2(s) --------------> Ni2+ + 2OH-

With a pH = 12.2 let's calculate the concentration of [OH]:

pOH = 14 - 12.2 = 1.8

[OH-] = 10-1.8 = 0.0158 M

With this we can calculate the solubility:

Ni(OH)2(s) --------------> Ni2+ + 2OH-

i. s 0 0.0158

e. 0 s 0.0158

We can assume that this solution is buffered with that pH therefore, there's no change in the concentration of OH, now let's solve for s:

Ksp = s [OH-]2

s = Ksp / [OH-]2

s = 2x10-15 / (0.0158)2

s = 1.26x10-13 mol/L

The molar mass of Ni(OH)2 is: (58.69) + (2*16) + (2*1) = 92.69 g/mol

s = 1.26x10-13 mol/L * 92.69 g/mol = 1.17x10-11 g/L

Hope this helps

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