Asked by bekah
It is possible to manipulate the solubility of some compounds through pH adjustments. What is the appropriate pH that will yield a Molar solubility for Mg(OH)2 of 2.51 x 10-8? The Ksp for Mg(OH)2 is 1.2 x 10-11. (Hint: you may assume the concentration of hydroxide is constant as the solute dissolves, since so little dissolves. Also, it is required to solve for pOH in this problem and then convert to pH.)
Answers
Answered by
DrBob222
.......Mg(OH)2 ==> Mg^2+ + 2OH^-
I......solid........0........0
C......solid........x........2x
E......solid........x........2x
So Ksp = 1.2E-10
You want solubility Mg(OH)2 to be 2.51E-8M = (Mg^2+) = x in the above equation.
Plug those values into Ksp expression and solve for OH^-, then convert to pH.
I......solid........0........0
C......solid........x........2x
E......solid........x........2x
So Ksp = 1.2E-10
You want solubility Mg(OH)2 to be 2.51E-8M = (Mg^2+) = x in the above equation.
Plug those values into Ksp expression and solve for OH^-, then convert to pH.
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