Problem: Calculate the molar solubility of Ni(OH)2 when buffered at pH = 10.3.Express your answer using one significant figure.

FREE Expert Solution

Ni(OH)2(s)  Ni2+(aq) + 2 OH(aq)



Calculate the OH concentration in the solution:


pH+pOH=1410.3+pOH=14pOH=14-10.3

pOH = 3.7


[OH-]=10-pOH[OH-]=10-3.7

[OH] = 1.995x10–4 M



Notice that there is a common ion present, OH


We can construct an ICE table for the dissociation of Ni(OH)2



The Ksp expression for Ni(OH)2 is:


Ksp=productsreactants=[Ni2+][OH-]2



We can now plug in the equilibrium concentrations and solve for x, which is the molar solubility of Ni(OH)2 in M or mol/L


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Problem Details

Calculate the molar solubility of Ni(OH)2 when buffered at pH = 10.3.

Express your answer using one significant figure.

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