Question

10. 217 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. 0 .000056 X mol (b) How will the solubility calculated in part (a) be affected by the Ky 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), will be less than we would expect just on the basis of ks: The solubility of Mg(OH), will be greater than we would expect just on the basis of Ksp Supporting Materials Periodic Table Physical Constants I Supplemental Materials Additional Materials Section 6.7 Submit Answer

Answer 1

NgroH) car Mgr (aq) + 28ncaq) At to s At Eqm o S as S = solubility of my only Ksp = [m2 27 [on]² = (S) (25)? Ksp = Sx48² Ksp 2 453 S = (Ksp) . logis = log (Ksp) logs = log kep] = 3 [ logksp - logy] logs = I [-11.15-0.60205] 3 I M=n V=Sooml m = 1.21x10m V logs: 31917 S: 10-3917 n= MX V 2 1.2x16' SOO 1 ooo -9 S = 1.2) X10 M -4 my moles. n= 0.6810