Question

10. 2/7 points | Previous Answers (a) Using only Ksp from the equilibria of alkaline earth metal hydroxides table, calculate how many moles of Mg(OH)2 will dissolve in 500 mL of water. 2000083 (b) How will the solubility calculated in part (a) be affected by the Ki reaction in this table? (Select all that apply.) The dissolution reaction will be drawn to the right. The dissolution reaction will be drawn to the left. The solubility of Mg(OH)2 will be less than we would expect just on the basis of Kap The solubility of Mg(OH)2 will be greater than we would expect just on the basis of K Supporting Materials Periodic Table Physical Constants Supplemental Materials Additional Materials Section 6.7 Submit Answer

Answer 1

I don't know what the K_{​​​​​​sp} value is given in your Table,that isn't given in your question. I'm assuming the K_{​​​​​​sp} value of Mg(OH)₂ to be 5.61 x 10^-12.

Let, the Solubility of Mg(OH) is S moles/L.

:: 45* = Ksp=561410142 1.5=t0l19x10n4 modes 2

Thus, in 500mL of Water, the no. Of moles of Mg(OH)₂ will be (1.119 x 10^-4)/2 = 0.000056 moles.